11th Standard Chemistry Study material & Free Online Practice Tests - View and download Sample Question Papers with Solutions for Class 11 Session 2019 - 2020 TN Stateboard

Chemistry Question Papers & Study Material

11th Chemistry Thermodynamics Model Question Paper - by Uma - Nagapattinam - View & Download

  • 1)

    All the naturally occurring processes proceed spontaneously in a direction which leads to

  • 2)

    Heat of combustion is always

  • 3)

    Change in internal energy, when 4 kJ of work is done on the system and 1 kJ of heat is given out by the system is

  • 4)

    The bond dissociation energy of methane and ethane are 360 kJ mol-1 and 620 kJ mol-1 respectively. Then, the bond dissociation energy of C-C bond is

  • 5)

    Which among the following is not an extensive property?

11th Chemistry Unit 6 Alkali and Alkaline Earth Metals Model Question Paper - by Uma - Nagapattinam - View & Download

  • 1)

    Which of the following compounds will not evolve H2 gas on reaction with alkali metals?

  • 2)

    Lithium shows diagonal relationship with

  • 3)

    Which is the correct sequence of solubility of  carbonates of alkaline earth metals?

  • 4)

    The hydration enthalpies of alkali metal ions decreases in ______ order.

  • 5)

    The reducing power of a metal depends on various factors. Suggest the factor. which makes Li, the strongest reducing agent in aqueous solution

11th Chemistry Unit 6 Gaseous State Model Question Paper - by Uma - Nagapattinam - View & Download

  • 1)

    Rate of diffusion of a gas is

  • 2)

    The value of universal gas constant depends upon

  • 3)

    Compressibility factor for CO2 at 400 K and 71.0 bar is 0.8697. The molar volume of CO2 under these conditions is

  • 4)

    Pressure is _____________

  • 5)

    The hydrogen balloon was invented by ______________

11th Chemistry First Mid Term Model Question Paper - by Uma - Nagapattinam - View & Download

  • 1)

    40 ml of methane is completely burnt using 80 ml of oxygen at room temperature The volume of gas left. after cooling to room temperature is

  • 2)

    Hot concentrated sulphuric acid is a moderately strong oxidizing agent. Which of the following reactions does not show oxidising behaviour?

  • 3)

    Which of the following compound(s) has /have a percentage of carbon same as that in ethylene (C2H4)

  • 4)

    Molecular mass =

  • 5)

    Assertion: Helium has the highest value of ionization energy among all the elements known
    Reason: Helium has the highest value of electron affinity among all the elements known

11th Chemistry Chapter 4 Hydrogen Model Question Paper - by Uma - Nagapattinam - View & Download

  • 1)

    Which of the following statements about hydrogen is incorrect?

  • 2)

    Non-stoichiometric hydrides are formed by

  • 3)

    If a body of a fish contains 1.2 g hydrogen in its total body mass, if all the hydrogen is replaced with deuterium then the increase in body weight of the fish will be

  • 4)

    The number of neutrons in  hydrogen atom is ___________.

  • 5)

    _____________ is known as heavy hydrogen.

11th Standard Chemistry Chapter 3 Periodic Classification Of Elements Important Question Paper - by Uma - Nagapattinam - View & Download

  • 1)

    What would be the IUPAC name for an element with atomic number 222?

  • 2)

    The electronic configuration of the elements A and Bare 1s2, 2s 2,2p6,3s2 and 1s2, 2s2,2p5 respectively. The formula of the ionic compound that can be formed between these elements is

  • 3)

    The first list of 23 chemical elements was published by _____ in the year 1789.

  • 4)

    Which of the following is Dobereiner's triad?

  • 5)

    What would be the formula of the compound formed by A and B, where A has the valence 3 and B has the valence 3?

Plus 1 Chemistry Chapter 2 Quantum Mechanical Model of Atom Important Question Paper - by Uma - Nagapattinam - View & Download

  • 1)

    The energy of light of wavelength 45 nm is

  • 2)

    The energies E1and E2 of two radiations are 25 eV and 50 eV respectively. The relation between their wavelengths ie \(\lambda \)1 and\(\lambda \)2 will be

  • 3)

    Splitting of spectral lines in an electric field is called

  • 4)

    The electronic configuration of Eu (Atomic no. 63) Gd (Atomic no. 64) and Tb (Atomic no. 65) are

  • 5)

    Which of the following pairs of d-orbitals will have electron density along the axes ?

11th Chemistry - Unit 1 Question Paper - by Uma - Nagapattinam - View & Download

  • 1)

    40 ml of methane is completely burnt using 80 ml of oxygen at room temperature The volume of gas left. after cooling to room temperature is

  • 2)

    An element X has the following isotopic Composition 200X = 90%, 199X = 8% and 202X = 2% The Weighted average atomic mass of the element X is closet to  

  • 3)

    Assertion: Two mole of glucose contains 12.044 x 1023 molecules of glucose
    Reason: Total number of entities present in one mole of any substance is equal to 6.02 x 1022

  • 4)

    The oxidation number of hydrogen in LiH is _____________

  • 5)

    The oxidation number of Cr in Cr2O72- __________ is

creative one mark questions for english medium in eleventh standard chemistry - by Karthi - View & Download

  • 1)

    Match the List-I and List-II using the correct code given below the list.

    List-I List-II
    A. Hydrogenation of unsaturated vegetable oils 1. Rocket fuel
    B. Calcium hydride 2. Welding of metals
    C. Liquid hydrogen 3. Desiccant
    D. Atomic hydrogen 4. Margarine
  • 2)

    Which of the following causes temporary hardness of water?

  • 3)

    Which of the following can oxidise Hydrogen peroxide?

  • 4)

    Which of the following process is important in food industry?

  • 5)

    Which of the following is used as desiccants to remove moisture from organic solvents?

Important one marks questions in plus one english medium chemistry chapter one Hydrogen - by Karthi - View & Download

  • 1)

    HF has ______ hydrogen bond.

  • 2)

    Acetic acid exist as a __________

  • 3)

    What is the dihedral angle of H2O2 in gas and solid phase?

  • 4)

    H2O2 acts as

  • 5)

    The reaction H2O2 ➝ H2O+O2 represents,

eleventh standard chemistry chapter one Hydrogen one mark questions english medium - by Karthi - View & Download

  • 1)

    The most abundant element in the universe is _________.

  • 2)

    The number of neutrons in  hydrogen atom is ___________.

  • 3)

    _____________ is known as heavy hydrogen.

  • 4)

    Deuterium consist of _____________

  • 5)

    The radioactive isotope of hydrogen is __________

Eleventh standard Model question paper for chapters 1, 2 & 3 English medium - by Karthi - View & Download

  • 1)

    40 ml of methane is completely burnt using 80 ml of oxygen at room temperature The volume of gas left. after cooling to room temperature is

  • 2)

    Fe2 + \(\longrightarrow\) Fe3+ + e- is a ________ reaction.

  • 3)

    Which one of the following represents 180g of water?

  • 4)

    Among the three metals, zinc, copper and silver, the electron releasing tendency decreases in the following order.

  • 5)

    Which of the following statement(s) is/are not true about the following decomposition reaction.
    2KClO3 \(\longrightarrow\) 2KCl + 3O2
    (i) Potassium is undergoing oxidation
    (ii) Chlorine is undergoing oxidation
    (iii) Oxygen is reduced
    (iv) None of the species are undergoing oxidation and reduction.

Chapter - 3 Periodic Classification Of Elements most expected five mark questions English medium eleventh standard - by Karthi - View & Download

  • 1)

    Using Slater's rule calculate the effective nuclear charge on a 3p electron in aluminium and chlorine. Explain how these results relate to the atomic radii of the two atoms.

  • 2)

    (a) State Mendeleev's periodic law.
    (b) Describe about the merits of Mendeleev's periodic table.

  • 3)

    Explain about the anomalies of Mendeleev's periodic table.

  • 4)

    Explain about the structural features of Moseley's long form of periodic table.

  • 5)

    Explain the merits of Moseley's long form of periodic table.

Eleventh standard Public exam five mark questions Periodic Classification Of Elements chapter - 3 - by Karthi - View & Download

  • 1)

    Give the structural features of modern periodic law.

  • 2)

    Mention Anomalies of Mendeleev's periodic table.

  • 3)

    How do you classify of elements into blocks? Give their electronic configuration.

  • 4)

    Give the characteristics of p-block elements.

  • 5)

    Give any five characteristic properties of inner transition elements.

Eleventh standard English medium Important three mark questions Periodic Classification Of Elements - II - by Karthi - View & Download

  • 1)

    Explain how electronegativity values are used to predict the nature of the bond between two atoms between A and B

  • 2)

    Which of the following species will have the largest and smallest size?

  • 3)

    Given the formula of the species that will be isoelectronic with the following atoms or ions
    (i) Ar (ii) F- (iii) K+ (iv) S-2

  • 4)

    Which of the following pairs of elements would you expect to have higher ionisation energy?(i) CI or F, (ii) S or CI, (iii) Na or Ne, (iv)Ar or Kr.
     

  • 5)

    (i) Why has chlorine higher electron affinity than fluorine?
    (ii) Why has nitrogen has higher 1st ionisation potential than oxygen atom?
    (iii) Why has magnesium higher I.E. than aluminium atom?

Periodic Classification Of Elements chapter - 3 creative three mark questions English medium for +1 - by Karthi - View & Download

  • 1)

    Write the name and deduce the atomic number of the following element
    i. The second alkali metal
    ii. The fourth noble gas
    iii. The third halogen
    iv. The first transition element

  • 2)

    Name the third chalcogen and fifth noble gas

  • 3)

    Lanthanoids and actinoids are placed in separate rows at the bottom of the periodic table. Explain.

  • 4)

    Helium has a electronic configuration of 1s2 but placed in p block in group 18. Justify.

  • 5)

    Describe in brief Lothar Meyer's classification of elements.

Board exam two mark questions in Periodic Classification Of Elements eleventh standard English medium - by Karthi - View & Download

  • 1)

    The ionisation energy is directly related to metallic character. Explain the variation of metallic character along the period and in the group.

  • 2)

    Explain the nature of oxides formed by metals and non metals.

  • 3)

    How does the basic and acidic nature of oxides vary along a period and in group?.

  • 4)

    How is ionisation energy related to the metallic character? How does the basic nature of hydroxides of alkaline earth metals very down the group?

  • 5)

    Account for the difference in size of Na +(95 pm) and Mg+2(65pm) both of which have the same noble gas configuration

Mostly asked +1 chapter - 3 Periodic Classification Of Elements two mark questions - by Karthi - View & Download

  • 1)

    How does atomic and ionic radii vary across the group and period.

  • 2)

    Mandeleev predicted that elements with atomic weights 72.68 and 70 in group IV and their properties. Name the elements that were discovered later and have properties predicted by Mandeleev.

  • 3)

    Give Mosley's relationship.

  • 4)

    Briefly outline anomalies of Mandeleev's periodic table

  • 5)

    Explain how will you find the atomic number of an element from the frequency of X-rays emitted by an element.

English medium Periodic Classification Of Elements frequently asked one mark questions eleventh standard - by Karthi - View & Download

  • 1)

    The first ionisation potential ofNa is 5.1 eY. The value of electron gain enthalpy is

  • 2)

    Electronegativity of the following elements increases in the order

  • 3)

    Consider the following elements: B, AI, Mg and K.

  • 4)

    Ionic radii vary in:
    (1) inverse proportion to the effective nuclear charge
    (2) inverse proportion to the square of the effective nuclear charge.
    (3) direct proportion to the screening effect.
    (4) direct proportion to the square of screening effect

  • 5)

    The chemical symbol of carbon and cobalt are______

Eleventh standard Public one mark questions Periodic Classification Of Elements English medium - by Karthi - View & Download

  • 1)

    Match the list I with List II and select the correct answer using. the code given below the lists.

    List I List II
    A A halogen 1 Cesium
    B An alkali metal 2 Germanium
    C A chalcogen 3 Iodine
    D A metalloid 4 Selenium
  • 2)

    Period of an element is represented by _____ quantum number

  • 3)

    The first list of 23 chemical elements was published by _____ in the year 1789.

  • 4)

    Match the list I with List II and select the correct answer using. the code given below the lists.

    List I List II
    A Chancourtois 1 Addition of synthetic elements
    B Rang 2 Families and periods Long form
    C Glenn Seaborg 3 Modem periodic law
    D Moseley 4 First periodic law
  • 5)

    Which of the following statement (s) about the Modern Periodic Table is are incorrect
    i. The elements in the Modern Periodic Table are arranged on the basis of their decreasing atomic number.
    ii. The elements in the Modern Periodic Table are arranged on the basis of their increasing atomic masses.
    iii. Isotopes are placed in adjoining group (s) in the Periodic Table.
    iv. The elements in the Modern Periodic Table are arranged on the basis of their increasing atomic number.

Chapter - 2 Quantum Mechanical Model of Atom important five mark questions English medium eleventh standard - by Karthi - View & Download

  • 1)

    If an electron is moving with a velocity 600 ms-1 which is accurate upto 0.005%, then calculate the uncertainty in its position. (h = 6.63 x 10-34 Js. mass of electron = 9.1 x 10-31 kg)

  • 2)

    Light of wavelength 12818 \(\overset { o }{ A } \) is emitted when the electron of a hydrogen atom drops from 5th to 3rd orbit. Find the wavelength of a photon emitted when the electron falls from 3rd to 2nd orbit.

  • 3)

    Calculate the de Broglie wavelength of an electron that has been accelerated from rest through a potential difference of 1 keV.

  • 4)

    Calculate the uncertainty in the position of an electron, if the uncertainty in its velocity is 5.7 x 105 ms-1.

  • 5)

    Calculate the total number of angular nodes and radial nodes present in 3d and 4f orbitals.

Eleventh standard Centum five mark questions Quantum Mechanical Model of Atom English medium - by Karthi - View & Download

  • 1)

    Enlist the postulates of Bohr's atom model.

  • 2)

    By applying Bohr's postulates, arrive at the radius of nth orbit for hydrogen like atom

  • 3)

    Write a note on limitations of Bohr's atom model.

  • 4)

    Derive an equation for the wavelength of a matter wave.

  • 5)

    List out the important features of quantum mechanical model of atom

English medium chapter - 2 Quantum Mechanical Model of Atom frequently asked three mark questions - III - by Karthi - View & Download

  • 1)

    Which has the stable electronic configuration? Ni2+ or Fe3+.

  • 2)

    How many electrons in an atom may have the following quantum numbers? 
    (a) n = 4; ms = -1\2 (b) n = 3, 1=0.

  • 3)

    Show that the circumference of the Bohr orbit for the hydrogen atom is an integral multiple of the de Broglie wavelength associated with the electron revolving around the orbit.

  • 4)

    An ion with mass number 56 contains 3 units of positive charge and 30.4% more neutrons than electrons. Assign symbol to the ion.

  • 5)

    The uncertainty in the position of a moving bullet of mass 10 g is 10-5 m. Calculate the uncertainty in its velocity?

Chapter - 2 Creative three mark questions Quantum Mechanical Model of Atom - II for english medium - by Karthi - View & Download

  • 1)

    Explain the shapes of p orbitals

  • 2)

    Discuss the shapes of d orbitals.

  • 3)

    Write a note on the shape of f orbitals

  • 4)

    (i) What is common between dxy and dx2-y2 orbitals?
    (ii) What is the difference between them?
    (iii) What is the angle between the lobes of the above two orbitals?

  • 5)

    If the K.E of electron is 2.5 \(\times\)10-24 J, then calculate its de-Broglie wavelength.

English medium Most asked three mark questions Quantum Mechanical Model of Atom chapter - 2 - by Karthi - View & Download

  • 1)

    An electron a proton which one will have a higher velocity to produce matter waves of the same wavelength? Explain it

  • 2)

    Explain why the uncertainty principle is significant only for the motion of sub-atomic particles but is negligible for the macroscopic objects?

  • 3)

    What are quantum numbers?

  • 4)

    What is the maximum number of electrons that can be accommodated in a shell?

  • 5)

    What is meant by nodal surface or node?

Chapter - 2 Quantum Mechanical Model of Atom english medium Public two mark questions - II - by Karthi - View & Download

  • 1)

    How many unpaired electrons are present in the ground state of
    (i) Cr3+ (Z = 24) (ii) Ne (Z = 10)

  • 2)

    What is meant by electronic configuration? Write the electronic configuration of N (Z = 7).

  • 3)

    Which is the actual configuration of Cr ( Z = 24). Why?

  • 4)

    What is the actual configuration of copper (Z = 29)? Explain about its stability.

  • 5)

    Write a note about J.J. Thomson's atomic model.

English medium Most important two mark questions in chapter - 2 Quantum Mechanical Model of Atom - by Karthi - View & Download

  • 1)

    Write a note on Thomson's plum pudding model of an atom.

  • 2)

    What did Rutherford's alpha ray scattering experiment prove

  • 3)

    What are the defects of Rutherford's model?

  • 4)

    What is the charge and mass of an electron?

  • 5)

    What is the difference between atomic mass and mass number?

Chapter - 2 Quantum Mechanical Model of Atom English medium Public one mark questions - III - by Karthi - View & Download

  • 1)

    The Bohr's radius of Li2+ of 2nd orbit is ________________

  • 2)

    The formula used to calculate the Bohr's radius is_________________

  • 3)

    Who proposed the dual nature of light to all forms of matter?

  • 4)

    de Broglie equation is________________

  • 5)

    The crystal used in Davison and Germer experiment is____________________

English medium Quantum Mechanical Model of Atom Creative one mark questions with answer key - II - by Karthi - View & Download

  • 1)

    Schrodinger wave equation is applied to determine______.

  • 2)

    Bohr's equation for energy of an election in a hydrogen atom is given as______

  • 3)

    The effect which represents the splitting of spectral lines by external electric field is______

  • 4)

    According to Bohr's theory angular momentum of an electron in 6th orbit is

  • 5)

    When an electron jumps from lower orbit to higher orbit

Important one mark questions Quantum Mechanical Model of Atom English medium - by Karthi - View & Download

  • 1)

    The oxidation state of a element in its uncombined state is

  • 2)

    Fe2 + \(\longrightarrow\) Fe3+ + e- is a ________ reaction.

  • 3)

    Assertion: Fluorine has an oxidation state of - 1in all its compounds.
    Reason: Fluorine is the most electronegative element of the periodic table.

  • 4)

    The oxidation number of oxygen in O2 is _______________

  • 5)

    The oxidation number of hydrogen in LiH is _____________

Frequently asked five mark questions Basic Concepts of Chemistry and Chemical Calculations - by Karthi - View & Download

  • 1)

    Balance the following equation by ion-electron method In acidic medium.
    \(Mn{O}_4^-+I^-\rightarrow MnO_2+I_2\)

  • 2)

    Balance the following equation by ion-electron method In acidic medium.
    \(Mn{O}_4^-+Fe^{2+}\rightarrow Mn^{2+}+Fe^{3+}\)

  • 3)

    Balance the following equation by ion-electron method In acidic medium.
    \(Cr{(OH)}_4^-+H_2O_2\rightarrow Cr{O}_4^{2-}\)

  • 4)

    (a) Define equivalent mass of an oxidising agent.
    (b) How would you calculate the equivalent mass of potassium permanganate?

  • 5)

    (a) Define equivalent mass of an reducing agent.
    (b) How would you determine the equivalent mass of Ferrous sulphate?

English medium Model question paper for chapter - 1 Basic Concepts of Chemistry and Chemical Calculations - by Karthi - View & Download

  • 1)

    Rusting of iron articles is an example of ___________ reaction

  • 2)

    Identify the correct statement(s) with respect to the following reaction :
    Zn + 2HCl \(\longrightarrow\) ZnCl2 + H2
    (i) Zinc is acting as an oxidant
    (ii) Chlorine is acting as a reductant
    (iii) Hydrogen is not acting as an oxidant
    (iv) Zn is acting as a reductant

  • 3)

    Match the list-I with list-II and select the correct answer using the code given below the lists.

    List-I List-II
    A Cr2O72- 1 +5
    B MnO4- 2 +6
    C VO3- 3 +3
    D FeF63+ 4 +7
  • 4)

    Match the items in column list-I with relevant items in list-II.

    List-I List-II
    A Ions having positive charge 1 anion
    B Ions having negative charge 2 -1
    C Oxidation number of fluorine in NaF 3 0
    D The sum of oxidation number of all atoms in a neutral molecule 4 cation
  • 5)

    Assertion (A): Among halogens fluorine is the best oxidant. Reason
    (R): Fluorine is the most electronegative atom.

Most expected three mark questions in Basic Concepts of Chemistry and Chemical Calculations - IV English medium - by Karthi - View & Download

  • 1)

    Balance the following reaction:
    Sb3++ Mn\({ O }_{ 4 }^{ - }\)\(\rightarrow \) Sb5++ Mn2+

  • 2)

    Define the following: (i) Element, (ii) Compound.

  • 3)

    Give two examples of elementary molecules which are (i) Monoatomic (ii) Diatomic and (iii) Polyatomic.

  • 4)

    Define a.m.u or unified atomic mass.

  • 5)

    Calculate the mass of the following atoms in a.m.u (unified atomic mass).

English medium Most expected three mark questions in Basic Concepts of Chemistry and Chemical Calculations - III - by Karthi - View & Download

  • 1)

    Calculate the number of atoms/molecules present in the following 1Kg of acetic acid

  • 2)

    The approximate production of Na2C03 per month is 424 x 106gwhile that of methyl alcohol is 320 x 106g. Which is produced more in terms of moles?

  • 3)

    Calculate number of moles of carbon atoms in three .moles of ethane.

  • 4)

    Find the molecular mass of FeSO47H2O.

  • 5)

    Calculate the number of moles present in the following 50g of calcium chloride

English medium Most expected three mark questions in Basic Concepts of Chemistry and Chemical Calculations - II - by Karthi - View & Download

  • 1)

    (i) If an acid is mono basic, how will you relate their equivalent mass and molecular mass.
    (ii) What is the basicity of H4 P2 O7 ?
    (iii) Give any two examples for dibasic acids.

  • 2)

    Why are the atomic mass of most of the elements fractional?

  • 3)

    Write down the formulae for calculating the equivalent mass of an acid, base and oxidizing agent.

  • 4)

    1.05g of a metal gives on oxidation 1.5g of its oxide. Calculate its equivalent mass.

  • 5)

    Calculate Equivalent mass of the Hydrochloric acid

Public exam five mark questions in Basic Concepts of Chemistry and Chemical Calculations English medium - by Karthi - View & Download

  • 1)

    Write note on combination reaction.

  • 2)

    Write note on decomposition reaction

  • 3)

    Explain displacement reaction.

  • 4)

    What are disproportionation reaction?

  • 5)

    Arrange the elements silver, Zinc and copper in the order of their decreasing electron releasing tendency and justify your arrangement with an appropriate experiment.

Most expected three mark questions in Basic Concepts of Chemistry and Chemical Calculations chapter - 1 ENglish medium - by Karthi - View & Download

  • 1)

    Classify the following species into acids and bases according to Lewis concept.
    S2-, H+, OH-, BF3' Ni2+, F-

  • 2)

    MnO42- undergoes disproportionation reaction in acidic medium but MnO4- does not. Give reason.

  • 3)

    Categorise the redox reactions that occur in our daily life

  • 4)

    2Cu2S + 3O2 \(\longrightarrow\) 2Cu2O + 2SO2
    (i) In this reaction which substance is getting oxidised and which substance is getting reduced?
    (ii) Name the oxidising and reducing agents.

  • 5)

    How would you know whether a redox reaction is taking place in an acidic, alkaline or neutral medium?

Creative two mark questions Basic Concepts of Chemistry and Chemical Calculations English medium - II - by Karthi - View & Download

  • 1)

    Calculate the equivalent mass of the following - Aluminium hydroxide

  • 2)

    Calculate the equivalent mass of the following - Sodium Hydroxide

  • 3)

    Calculate the equivalent mass of the following - Potassium Sulphate

  • 4)

    Explain the term limiting reagent.

  • 5)

    3 grams of hydrogen reacts with 29 g of O, to yield H2O. Which is the limiting reagent?

Creative two mark questions Basic Concepts of Chemistry and Chemical Calculations English medium - by Karthi - View & Download

  • 1)

    Calculate the molar mass of the following compounds. - acetone [CH3 COCH3]

  • 2)

    Calculate the molar mass of the following compounds. -boric Acid [H3BO3]

  • 3)

    Calculate the molar mass of the following compounds. -Sulphurci  Acid [H2SO4]

  • 4)

    Balance the following equations by ion electron method - \({ C }_{ 2 }{ O }_{ 4 }^{ 2- }+{ Cr }_{ 2 }{ O }_{ 7 }^{ 2- }\longrightarrow { Cr }^{ 3+ }+{ CO }_{ 2 }\) (in acid medium)

  • 5)

    Balance the following equations by ion electron method \({ Na }_{ 2 }{ S }_{ 2 }{ O }_{ 3 }+{ I }_{ 2 }\longrightarrow { Na }_{ 2 }{ S }_{ 4 }{ O }_{ 6 }+NaI\)

Basic Concepts of Chemistry and Chemical Calculations important one mark questions English medium - by Karthi - View & Download

  • 1)

    The oxidation state of a element in its uncombined state is

  • 2)

    Fe2 + \(\longrightarrow\) Fe3+ + e- is a ________ reaction.

  • 3)

    Assertion: Fluorine has an oxidation state of - 1in all its compounds.
    Reason: Fluorine is the most electronegative element of the periodic table.

  • 4)

    The oxidation number of oxygen in O2 is _______________

  • 5)

    The oxidation number of hydrogen in LiH is _____________

11th Standard Chemistry Public Exam March 2019 Important Creative 3 Mark Questions and Answers - by Karthi - View & Download

  • 1)

    Calculate the oxidation number of underlined atoms of the following:
    K2CrO4

  • 2)

    Calculate the equivalent mass of potassium dichromate in acid medium
    [K2Cr2O7 + 4H2SO4 )\(\rightarrow\)K2SO4 + Cr2(SO4)3 +4H2O + 3(O) 3 x 16 = 48 294 g]

  • 3)

    Calculate the oxidation number of underlined atoms\({ C }_{ \underline { 6 } }{ H }_{ 12 }{ O }_{ 6 }\)

  • 4)

    Calculate the number of moles present in the following 19.5g of potassium

  • 5)

    Calculate the equivalent mass of barium hydroxide

11th Standard Chemistry Public Exam March 2019 Important Creative One Mark Test 1 - by Karthi - View & Download

  • 1)

    The oxidation state of a element in its uncombined state is

  • 2)

    Fe2 + \(\longrightarrow\) Fe3+ + e- is a ________ reaction.

  • 3)

    The oxidation number of hydrogen in LiH is _____________

  • 4)

    The oxidation number of Cr in Cr2O72- __________ is

  • 5)

    Maximum oxidation state is present in the central metal atom of which compound

11th Standard Chemistry Public Exam March 2019 Important One Marks Questions - by Karthi - View & Download

  • 1)

    Assertion: Two mole of glucose contains 12.044 x 1023 molecules of glucose
    Reason: Total number of entities present in one mole of any substance is equal to 6.02 x 1022

  • 2)

    When 22.4 litres of H2(g) is mixed with 11.2 litres of Cl2(g), each at 273 K at 1 atm the moles of HCl (g), formed is equal to

  • 3)

    7.5 g of a gas occupies a volume of 5.6 litres at 0° C and 1 atm pressure. The gas is

  • 4)

    The equivalent mass of ferrous oxalate is __________.

  • 5)

    Two 22.4 litre containers A and B contains 8 g of O2 and 8 g of SO2 respectively at 273 K and 1 atm pressure, then

11th Standard Chemistry Public Exam March 2019 Important Creative Questions and Answers - by Karthi - View & Download

  • 1)

    Define relative atomic mass.

  • 2)

    What do you understand by the term oxidation number?

  • 3)

    Balance the following equations by ion electron method - \({ C }_{ 2 }{ O }_{ 4 }^{ 2- }+{ Cr }_{ 2 }{ O }_{ 7 }^{ 2- }\longrightarrow { Cr }^{ 3+ }+{ CO }_{ 2 }\) (in acid medium)

  • 4)

    Balance the following equations by oxidation number method - \({ KMn }O_{ 4 }+{ H }_{ 2 }{ C }_{ 2 }{ O }_{ 4 }+{ H }_{ 2 }{ SO }_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ MnSO }_{ 4 }+{ CO }_{ 2 }+{ H }_{ 2 }O\)

  • 5)

    Give examples for the following redox reaction "Metal displacement reaction".

Plus One Chemistry Public Exam March 2019 One Mark Question Paper - by Karthi - View & Download

  • 1)

    An element X has the following isotopic Composition 200X = 90%, 199X = 8% and 202X = 2% The Weighted average atomic mass of the element X is closet to  

  • 2)

    The equivalent mass of a trivalent metal element is 9 g eq-1 the molar mass of its anhydrous oxide is

  • 3)

    Total number of electrons present in 1.7 g of ammonia is

  • 4)

    Identify disproportionation reaction

  • 5)

    Which of the following statement(s) is/are not true about the following decomposition reaction.
    2KClO3 \(\longrightarrow\) 2KCl + 3O2
    (i) Potassium is undergoing oxidation
    (ii) Chlorine is undergoing oxidation
    (iii) Oxygen is reduced
    (iv) None of the species are undergoing oxidation and reduction.

11th Standard Chemistry Public Exam March 2019 Important 5 Marks Questions - by Karthi - View & Download

  • 1)

    Calculate the molar mass of the following compounds. -
    i) urea [CO(NH2)2]
    ii) acetone [CH3 COCH3]
    iii) boric Acid [H3BO3]
    iv) Sulphurci  Acid [H2SO4]

  • 2)

    The reaction between aluminum and ferric oxide can generate temperatures up to 3273 K and is used in welding metals. (Atomic mass of AC = 27 u atomic mass of O = 16 u )
    2Al + Fe2O3 \(\longrightarrow \) Al2O3 + 2Fe;  If in this process, 324 g of aluminum is allowed to react with 1.12 kg of ferric oxide
    i) Calculate the mass of Al2O3 formed
    ii) How much of the excess reagent is left at the end of the reaction?

  • 3)

    Write note on decomposition reaction

  • 4)

    Balance the following equations by oxidation number method
    i) \({ K }_{ 2 }{ Cr }_{ 2 }{ O }_{ 7 }+KI+{ H }_{ 2 }SO_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ Cr }_{ 2 }({ SO }_{ 4 })+{ I }_{ 2 }+{ H }_{ 2 }O\)
    ii) \({ K }Mno_{ 4 }+{ Na }_{ 2 }{ So }_{ 3 }\longrightarrow { MnO }_{ 2 }+{ Na }_{ 2 }{ So }_{ 4 }+KOH\)
    iii) \(Cu+{ HNO }_{ 3 }\longrightarrow Cu\left( { No }_{ 3 } \right) _{ 2 }+{ No }_{ 2 }+{ H }_{ 2 }O\)
    iv) \({ KMn }O_{ 4 }+{ H }_{ 2 }{ C }_{ 2 }{ O }_{ 4 }+{ H }_{ 2 }{ SO }_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+{ MnSO }_{ 4 }+{ CO }_{ 2 }+{ H }_{ 2 }O\)

  • 5)

    Explain the term competitive electron transfer reaction with an example.

internal - by Demo Chemistry New - View & Download

  • 1)

    Assertion: Fluorine has an oxidation state of - 1in all its compounds.
    Reason: Fluorine is the most electronegative element of the periodic table.

  • 2)

    The oxidation number of oxygen in O2 is _______________

  • 3)

    Rusting of iron articles is an example of ___________ reaction

  • 4)

    Distinguish between oxidation and reduction.

  • 5)

    The density of carbon dioxide is equal to 1.965 kgm-3 at 273 K and 1 atm pressure. calculate the molar mass of CO2

11th Standard Chemistry Public Exam March 2019 Model Question Paper - by Karthi - View & Download

  • 1)

    22 g of CO2 contains ____________ molecules of CO2.

  • 2)

    For d-electron, the orbital angular momentum is

  • 3)

    Ionic radii vary in:
    (1) inverse proportion to the effective nuclear charge
    (2) inverse proportion to the square of the effective nuclear charge.
    (3) direct proportion to the screening effect.
    (4) direct proportion to the square of screening effect

  • 4)

    Tritium nucleus contains

  • 5)

    sodium is stored in

Plus One Chemistry Official Public Exam Question Paper 2019 - by Karthi - View & Download

  • 1)

    The change in the oxidation number of S in H2S and SO2,in the following industrial reaction:
    2H2S(g) + SO2(g) \(\longrightarrow\) 3S(s) + H2O(g)

  • 2)

    Time independent Schnodinger wave equation is

  • 3)

    Match the list I with list II and select the correct answer using the code given below the list.

    List I List II
    A Ionisation energy 1 ionic compound
    B electro negativity 2 alloys
    C s-block elements 3 KJ mol-1
    D d-block elements 4 No unit
  • 4)

    The reaction H3PO2 + D2O ➝ H2DPO2 + HDO indicates that hypo-phosphorus acid is

  • 5)

    A colourless solid substance (A) on heating evolved CO2 and also gave a white residue, soluble in water. Residue also gave CO2 when treated with dilute HCI

11th Standard Chemistry Basic Concepts of Chemistry and Chemical Calculations Important Questions - by Karthi - View & Download

  • 1)

    An element X has the following isotopic Composition 200X = 90%, 199X = 8% and 202X = 2% The Weighted average atomic mass of the element X is closet to  

  • 2)

    When 6.3g of sodium bicarbonate is added to 30g of the acetic acid solution, the residual solution is found to weigh 33g. The number of moles of carbon dioxide released in the reaction is

  • 3)

    The oxidation number of oxygen in O2 is _______________

  • 4)

    Which of the following is/are true with respect to carbon -12

  • 5)

    The change in the oxidation number of S in H2S and SO2,in the following industrial reaction:
    2H2S(g) + SO2(g) \(\longrightarrow\) 3S(s) + H2O(g)

11th Standard Chemistry 3rd Revision Test Question and Answer 2019 - by Karthi - View & Download

  • 1)

    Assertion: The number of oxygen atoms in 16g of oxygen and 16g of ozone is same 
    Reason Each of the species represent 1g atom of oxygen

  • 2)

    The total number of orbitals associated with the principal quantum number n = 3 is

  • 3)

    Which of the following statement is incorrect?

  • 4)

    Zeolite used to soften hardness of water is hydrated

  • 5)

    The suspension of slaked lime in water is known as

11th Standard Chemistry Public Exam March 2019 Model Question Paper - by Karthi - View & Download

  • 1)

    The number of molecules in 40 g of sodium hydroxide is _______________

  • 2)

    Two electrons occupying the same orbital are distinguished by

  • 3)

    The oxidation state of alkali metal is _______

  • 4)

    Ionic hydrides are formed by

  • 5)

    Which is the correct sequence of solubility of  carbonates of alkaline earth metals?

11th Standard Chemistry Revision Test Model Question Paper 2019 - by Karthi - View & Download

  • 1)

    In the reaction 2AuCl3 + 3SnCl2 \(\rightarrow\) 2Au + 3SnCl4 which is an oxidising agent?

  • 2)

    What is the maximum numbers of electrons that can be associated with the following set of quantum numbers? n = 3, I = 1 and m =-1

  • 3)

    In the modern periodic table, the period indicates the value of____

  • 4)

    Zeolite used to soften hardness of water is hydrated

  • 5)

    The name 'Blue John' is given to which of the following compounds?

11th Stateboard Chemistry Periodic Classification Of Elements Important Questions - by Karthi - View & Download

  • 1)

    The electronic configuration of the elements A and Bare 1s2, 2s 2,2p6,3s2 and 1s2, 2s2,2p5 respectively. The formula of the ionic compound that can be formed between these elements is

  • 2)

    Period of an element is represented by _____ quantum number

  • 3)

    Which of the following statement (s) about the Modern Periodic Table is are incorrect
    i. The elements in the Modern Periodic Table are arranged on the basis of their decreasing atomic number.
    ii. The elements in the Modern Periodic Table are arranged on the basis of their increasing atomic masses.
    iii. Isotopes are placed in adjoining group (s) in the Periodic Table.
    iv. The elements in the Modern Periodic Table are arranged on the basis of their increasing atomic number.

  • 4)

    The atomic weight of Au is ______

  • 5)

    The vertical columns in the periodic table are called as

11th Standard Chemistry Model Question Paper 2019 - by K Sudhakar - View & Download

  • 1)

    7.5 g of a gas occupies a volume of 5.6 litres at 0° C and 1 atm pressure. The gas is

  • 2)

    Which of the following provides the experimental justification of magnetic quantum number?

  • 3)

    Which one of the following is true about metallic character when we move from left to right in a period and top to bottom in a group?

  • 4)

    Which pair are not hydrogen isotopes?

  • 5)

    Which of the following has the highest tendency to give the reaction \(M_{g}^{+}\xrightarrow[Medium]{Aqueous}M_{aq}^{+}\)

+1 Chemistry First Revision Test Model question paper and answer - by Karthi - View & Download

  • 1)

    One 'U' stands for the mass of

  • 2)

    How many electrons in an atom with atomic number 105 can have (n + I) = 8 ? 

  • 3)

    Which of the following N3-, O2-, F- is largest in size?

  • 4)

    A commercial sample of hydrogen peroxide marked as 100 volume H2O2, it means that

  • 5)

    Which of the following statements is in correct?

11th Chemistry Half Yearly Important Questions paper - by Karthi - View & Download

  • 1)

    Identify the correct statement(s) with respect to the following reaction :
    Zn + 2HCl \(\longrightarrow\) ZnCl2 + H2
    (i) Zinc is acting as an oxidant
    (ii) Chlorine is acting as a reductant
    (iii) Hydrogen is not acting as an oxidant
    (iv) Zn is acting as a reductant

  • 2)

    What is the maximum numbers of electrons that can be associated with the following set of quantum numbers? n = 3, I = 1 and m =-1

  • 3)

    Match the list-I and list-II using the code given below the list

    List-I List-II
    A.Law of triads 1.Chancourtois
    B.Law of octaves 2.Henry Moseley
    C.First periodic law 3.Newland
    D.Modem periodic law 4.Johann Dobereiner
  • 4)

    Which of the following statements about hydrogen is incorrect?

  • 5)

    Assertion : BeSO4 is soluble in water while BaSO4 is not
    Reason : Hydration energy decreases down the group from Be to Ba and lattice energy remains almost constant.

Haloalkanes and Haloarenes Important Questions - by Karthi - View & Download

  • 1)

    Of the following compounds, which has the highest boiling point?

  • 2)

    In the reaction  X is ________.

  • 3)

    The name of C2F4Cl2 is ___________

  • 4)

    Freon-12 is manufactured from tetrachloro methane by

  • 5)

    Silverpropionate when refluxed with Bromine in carbontetrachloride gives

Environmental Chemistry Important Questions from 11th Chemistry - by Karthi - View & Download

  • 1)

    Which sequence for green house gases is based on GWP?

  • 2)

    Biochemical oxygen Demand value less than 5 ppm indicates a water sample to be

  • 3)

    Assertion (A): If BOD level of water in a reservoir is more than 5 ppm it is highly polluted
    Reason(R) : High biological oxygen demand means high activity of bacteria in water

  • 4)

    High concentration of lead in human blood damages

  • 5)

    Green house gases cause

11th Standard Chemistry Half Yearly Model Question Paper 1 - by Karthi - View & Download

  • 1)

    Hot concentrated sulphuric acid is a moderately strong oxidizing agent. Which of the following reactions does not show oxidising behaviour?

  • 2)

    Which of the following pairs of d-orbitals will have electron density along the axes ?

  • 3)

    The value of Bohr radius for hydrogen atom is

  • 4)

    In which of the following options the order of arrangement does not agree with the variation of property indicated against it?

  • 5)

    The highest ionization energy is exhibited by_________

11th Standard Chemistry Unit Test Important Questions - by K RAJA - View & Download

  • 1)

    If Kb and Kf for a reversible reactions are 0.8 ×10–5 and 1.6 × 10–4 respectively, the value of the equilibrium constant is,

  • 2)

    At a given temperature and pressure, the equilibrium constant values for the equilibria
    \({ 3A }_{ 2 }+{ B }_{ 2 }+2C\overset { { K }_{ 1 } }{ \rightleftharpoons } { 2A }_{ 3 }BC\) and
    \({ A }_{ 3 }BC\overset { { K }_{ 2 } }{ \rightleftharpoons } 3/2\left[ { A }_{ 2 } \right] +\frac { 1 }{ 2 } { B }_{ 2 }+C\)
    The relation between K1 and K2 is

  • 3)

    The equilibrium constant for a reaction at room temperature is K1 and that at 700 K is K2. If K1 > K2, then

  • 4)

    The formation of ammonia from N2(g) and H2(g) is a reversible reaction
    N2(g) + 3H2(g) ⇌ 2NH3(g) + Heat
    What is the effect of increase of temperature on this equilibrium reaction

  • 5)

    Solubility of carbon dioxide gas in cold water can be increased by

11th Standard Chemistry Unit Test Question Paper - by K RAJA - View & Download

  • 1)

    The molality of a solution containing 1.8g of glucose dissolved in 250g of water is

  • 2)

    Which of the following concentration terms is/are independent of temperature

  • 3)

    Stomach acid, a dilute solution of HCl can be neutralised by reaction with Aluminium hydroxide
    Al (OH)3 + 3HCl (aq) → AlCl3 + 3 H2O
    How many millilitres of 0.1 M Al(OH)3 solution are needed to neutralise 21 mL of 0.1 M HCl?

  • 4)

    The partial pressure of nitrogen in air is 0.76 atm and its Henry's law constant is 7.6 × 104 atm at 300K. What is the mole fraction of nitrogen gas in the solution obtained when air is bubbled through water at 300K?

  • 5)

    The Henry's law constant for the solubility of Nitrogen gas in water at 350 K is 8 × 104 atm. The mole fraction of nitrogen in air is 0.5. The number of moles of Nitrogen from air dissolved in 10 moles of water at 350K and 4 atm pressure is

11th Standard Chemistry Model question Paper - by K RAJA - View & Download

11th Standard Chemistry Monthly Test Model Questions - by K RAJA - View & Download

  • 1)

    For alkali metals, which one of the following trends is incorrect?

  • 2)

    Which of the following statements is in correct?

  • 3)

    Which of the following compounds will not evolve H2 gas on reaction with alkali metals?

  • 4)

    Which of the following has the highest tendency to give the reaction \(M_{g}^{+}\xrightarrow[Medium]{Aqueous}M_{aq}^{+}\)

  • 5)

    sodium is stored in

Important 5mark -chapter 9,10 - by Karthi - View & Download

  • 1)

    Calculate the proportion of O2 and N2 dissolved in water at 298 K. When air containing 20% O2 and 80% N2 by volume is in equilibrium with it at 1 atm pressure. Henry’s law constants for two gases are KH(O2) = 4.6 x 104 atm and KH (N2) = 8.5 x 104 atm.

  • 2)

    Calculate the mole fractions of benzene and naphthalene in the vapour phase when an ideal liquid solution is formed by mixing 128 g of naphthalene with 39 g of benzene. It is given that the vapour pressure of pure benzene is 50.71 mmHg and the vapour pressure of pure naphthalene is 32.06 mmHg at 300 K.

  • 3)

    An aqueous solution of 2% nonvolatile solute exerts a pressure of 1.004 bar at the boiling point of the solvent. What is the molar mass of the solute when PA is 1.013 bar?

  • 4)

    2.56 g of Sulphur is dissolved in 100g of carbon disulphide. The solution boils at 319. 692 K. What is the molecular formula of Sulphur in solution The boiling point of CS2 is 319. 450K. Given that Kb for CS2 = 2.42 K Kg mol-1.

  • 5)

    Ethylene glycol (C2H6O2) can be at used as an antifreeze in the radiator of a car. Calculate the temperature when ice will begin to separate from a mixture with 20 mass percent of glycol in water used in the car radiator. Kf for water = 1.86 K Kg mol-1 and molar mass of ethylene glycol is 62 g mol-1.

Important 3mark -chapter 9,10 - by Karthi - View & Download

  • 1)

    If 5.6 g of KOH is present in (a) 500 mL and (b) 1 litre of solution, calculate the molarity of each of these solutions.

  • 2)

    2.82 g of glucose is dissolved in 30 g of water. Calculate the mole fraction of glucose and water.

  • 3)

    What volume of 4M HCl and 2M HCl should be mixed to get 500 mL of 2.5 M HCl?

  • 4)

    How much volume of 6 M solution of NaOH is required to prepare 500 mL of 0.250 M NaOH solution.

  • 5)

    0.24 g of a gas dissolves in 1 L of water at 1.5 atm pressure. Calculate the amount of dissolved gas when the pressure is raised to 6.0 atm at constant temperature.

Important 2mark -chapter 9,10 - by Karthi - View & Download

  • 1)

    The antiseptic solution of iodopovidone for the use of external application contains 10 % w/v of iodopovidone. Calculate the amount of iodopovidone present in a typical dose of 1.5 mL.

  • 2)

    A litre of sea water weighing about 1.05 kg contains 5 mg of dissolved oxygen (O2). Express the concentration of dissolved oxygen in ppm.

  • 3)

    Explain why the aquatic species are more comfortable in cold water during winter season rather than warm water during the summer.

  • 4)

    At 400 K 1.5 g of an unknown substance is dissolved in solvent and the solution is made to 1.5 L. Its osmotic pressure is found to be 0.3 bar. Calculate the molar mass of the unknown substance.

  • 5)

    Define (i) molality (ii) Normality.

Important 1mark -chapter 9,10 - by Karthi - View & Download

  • 1)

    Stomach acid, a dilute solution of HCl can be neutralised by reaction with Aluminium hydroxide
    Al (OH)3 + 3HCl (aq) → AlCl3 + 3 H2O
    How many millilitres of 0.1 M Al(OH)3 solution are needed to neutralise 21 mL of 0.1 M HCl?

  • 2)

    The partial pressure of nitrogen in air is 0.76 atm and its Henry's law constant is 7.6 × 104 atm at 300K. What is the mole fraction of nitrogen gas in the solution obtained when air is bubbled through water at 300K?

  • 3)

    Which one of the following is incorrect for ideal solution?

  • 4)

    Which one of the following gases has the lowest value of Henry's law constant?

  • 5)

    P1 and P2 are the vapour pressures of pure liquid components, 1 and 2 respectively of an ideal binary solution if x1 represents the mole fraction of component 1, the total pressure of the solution formed by 1 and 2 will be

11th State Board Chemistry Equilibrium and Redox Reactions Important Questions - by Karthi - View & Download

  • 1)

    Which among the following is an intensive property?

  • 2)

    Match the list I with list II and select the correct answer using the code given below the list.

    List-I List-II
    A ΔS<0 1 I2(s)⟶I2(g)
    B ΔG<0 2 \(Ice\overset { 273\quad K }{ \rightleftharpoons } Water\)
    C ΔG=0 3 2O3(g)⟶3O2(g)
    D ΔS>0 4 \(H_{ 2 }O_{ (I) }\overset { 270K }{ \longrightarrow } { H }_{ 2 }O_{ (s) }\)
  • 3)

    In general, for an exothermic reaction to be spontaneous:

  • 4)

    In the equilibrium,
    2A(g) ⇌ 2B(g) + C2(g)
    the equilibrium concentrations of A, B and C2 at 400 K are 1 × 10–4 M, 2.0 × 10–3 M, 1.5 × 10–4 M respectively. The value of KC for the equilibrium at 400 K is

  • 5)

    In a chemical equilibrium, the rate constant for the forward reaction is 2.5 × 102 and the equilibrium constant is 50. The rate constant for the reverse reaction is,

11th Standard Chemistry Thermodynamics and Gaseous State Important 5 Mark Questions - by Karthi - View & Download

  • 1)

    Calculate the standard heat of formation of propane, if its heat of combustion is -2220.2 kJ mol-1. the heats of formation of CO2(g) and H2O(l) are -393.5 and -285.8 kJ mol-1 respectively

  • 2)

    If an automobile engine burns petrol at a temperature of 816° C and if the surrounding temperature is 21° C, calculate its maximum possible efficiency

  • 3)

    The heat of combustion of solid naphthalene (C10H10) at constant volume was -4984 kJ mol-1 at 298 K. Calculate the value of enthalpy change.
    Given: 
    C10H8(s)+12O2(g) ➝ 10CO2(g)+4H2O(l)
    \(\Delta U\)=-4984 kJ mol-1
    \(\Delta U\)=-4984 kJ mol-1,R=8.314 JK-1 mol-1
    T=298 K

  • 4)

    The standard heat of formation of H2O(l) from its elements and O2 is -290.83 kJ mol-1 and the standard entropy change for the same reaction is -330 JK-I at 25°C. Will the reaction be spontaneous at 25°C.
    Given: \(\Delta{H^{o}}\)= -290.83 kJ mol-1
    = -290830 J mol-1
    \(\Delta{S^{o}}\) = -330 JK-1
    T = 25°C = 298 K

  • 5)

    Calculate the entropy change when 1 mole of ethanol is evaporated at 351 K The molar heat of vaporisation of ethanol is 39.84 kJ mol-1.

Important 2mark -chapter 7,8 - by Karthi - View & Download

  • 1)

    State the first law of thermodynamics.

  • 2)

    Define Hess's law of constant heat summation.

  • 3)

    Explain intensive properties with two examples

  • 4)

    What is the usual definition of entropy? What is the unit of entropy?

  • 5)

    Predict the feasibility of a reaction when
    (i) both ΔH and ΔS positive
    (ii) both ΔH and ΔS negative
    (iii) ΔH decreases but ΔS increases

11th Standard Chemistry Thermodynamics and Gaseous State Important 3 Mark Questions - by Karthi - View & Download

  • 1)

    Define the following terms
    (a) isothermal process (b) adiabatic process
    (c) isobaric process (d) isochoric process

  • 2)

    What are state and path functions? Give two examples

  • 3)

    The equilibrium constant of a reaction is 10, what will be the sign of ΔG? Will this reaction be spontaneous?

  • 4)

    Define the following terms.

  • 5)

    Predict the change in internal energy for an isolated system at constant volume.

Important 1mark -chapter 7,8 - by Karthi - View & Download

  • 1)

    In a reversible process, the change in entropy of the universe is

  • 2)

    The intensive property among the quantities below is

  • 3)

    The enthalpies of formation of Al2O3 and Cr2Oare -1596 kJ and -1134 kJ, respectively. ΔH for the reaction 2AI + Cr2O3 ⟶ 2Cr + Al2O3 is

  • 4)

    The value of ΔH for cooling 2 moles of an ideal monatomic gas from 125° C to 25° C at constant pressure will be [given Cp=\(\frac{5}{2}\)R]

  • 5)

    When 15.68 litres of a gas mixture of methane and propane are fully combusted at 0° C and 1 atmosphere, 32 litres of oxygen at the same temperature and pressure are consumed. The amount of heat of released from this combustion in KJ is (ΔHc (CH4) = - 890 KJ mol-1 and ΔHc (C3H8 = - 2220 KJ mol-1)

Alkali And Alkaline Earth Metals & Gaseous State Important Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Which of the following compounds will not evolve H2 gas on reaction with alkali metals?

  • 2)

    A colourless solid substance (A) on heating evolved CO2 and also gave a white residue, soluble in water. Residue also gave CO2 when treated with dilute HCI

  • 3)

    The general electronic configuration of alkali metals is ____________

  • 4)

    When an ideal gas undergoes unrestrained expansion, no cooling occurs because the molecules

  • 5)

    Equal moles of hydrogen and oxygen gases are placed in a container, with a pin-hole through which both can escape what fraction of oxygen escapes in the time required for one-half of the hydrogen to escape.

Alkali And Alkaline Earth Metals & Gaseous State Important Five Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Discuss briefly the similarities between beryllium and aluminium.

  • 2)

    Alkaline earth metal (A), belongs to 3rd period reacts with oxygen and nitrogen to form compound (B) and (C) respectively. It undergo metal displacement reaction with AgNO3 solution to form compound (D).

  • 3)

    Explain the important common features of Group 2 elements.

  • 4)

    Describe briefly the biological Importance of Calcium and magnesium

  • 5)

    Bring out the simularities between lithium and magnesium.

Alkali And Alkaline Earth Metals & Gaseous State Important Three Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Why sodium hydroxide is much more water soluble than chloride?

  • 2)

    Write the chemical equations for the reactions involved in solvay process of preparation of sodium carbonate.

  • 3)

    An alkali metal (x) forms a hydrated sulphate, X2SO4•10H2O. Is the metal more likely to be sodium (or) potassium.

  • 4)

    Why alkaline earth metals are harder than alkali metals.

  • 5)

    Which would you expect to have a higher melting point magnesium oxide or magnesium fluoride? Explain your reasoning.

Alkali And Alkaline Earth Metals & Gaseous State Important Two Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Explain what is meant by efflerescence.

  • 2)

    Give the systematic names for the following
    (i) milk of magnesia
    (ii) lye
    (iii) lime
    (iv) Caustic potash
    (v) washing soda
    (vi) soda ash
    (vii) trona

  • 3)

    Mention the uses of plaster of paris

  • 4)

    Beryllium halides are Covalent whereas magnesium halides are ionic why?

  • 5)

    How is plaster of paris prepared?

Alkali And Alkaline Earth Metals & Gaseous State Important One Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Which of the following statements is in correct?

  • 2)

    Which of the following has the highest tendency to give the reaction \(M_{g}^{+}\xrightarrow[Medium]{Aqueous}M_{aq}^{+}\)

  • 3)

    sodium is stored in

  • 4)

    RbO2 is

  • 5)

    Lithium shows diagonal relationship with

Periodic Classification Of Elements & Hydrogen Important Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    The electronic configuration of the elements A and Bare 1s2, 2s 2,2p6,3s2 and 1s2, 2s2,2p5 respectively. The formula of the ionic compound that can be formed between these elements is

  • 2)

    Which of the following elements will have the highest electro negativity

  • 3)

    Various successive ionisation enthalpies (in kJ mol-1) of an element are given below.

    IE1 IE2 IE3 IE4 IE5
    577.5 1,810 2,750 11,580 14,820

    The element is

  • 4)

    The correct order of decreasing electronegativity values among the elements X, Y, Z and A with atomic numbers 4, 8,7 and 12 respectively

  • 5)

    How does electron affinity change when we move from left to right in a period in the periodic table?

Periodic Classification Of Elements & Hydrogen Important Five Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Explain the periodic trend of ionisation potential.

  • 2)

    Explain the diagonal relationship.

  • 3)

    By using paulings method calculate the ionic radii of K+ and CI- ions in the potassium chloride crystal. Given that dk+-cl-=3.14 Å. 

  • 4)

    Explain the following, give appropriate reasons.
    (i) Ionisation potential of N is greater than that of O.
    (ii) First ionisation potential of C-atom is greater than that of B atom, where as the reverse is true is for second ionisation potential.
    (iii) The electron affinity values of Be, Mg and noble gases are zero and those of N (0.02 eV) and P (0.80 eV) are very low.
    (iv) The formation of F-(g) from F(g) is exothermic while that of O2-(g) from O (g) is endothermic.

  • 5)

    Calculate the effective nuclear charge experienced by the 4s electron in potassium atom.

Periodic Classification Of Elements & Hydrogen Important Three Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Energy of an electron in the ground state of the hydrogen atom is -2.8 x 10-18 J. Calculate the ionisation enthalpy of atomic hydrogen in terms of kJ mol-1.

  • 2)

    The electronic configuration of atom is one of the important factor which affects the value of ionisation potential and electron gain enthalpy. Explain.

  • 3)

    In what period and group will an element with Z = 118 will be present?

  • 4)

    Mention any two anomalous properties of second period elements.

  • 5)

    What are metalloids? Give example.

Periodic Classification Of Elements & Hydrogen Important Two Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Define modern periodic law.

  • 2)

    Define electro negativity.

  • 3)

    How would you explain the fact that the second ionisation potential is always higher than first ionisation potential?

  • 4)

    Give the general electronic configuration of lanthanides and actinides.

  • 5)

    How does atomic and ionic radii vary across the group and period.

Periodic Classification Of Elements & Hydrogen Important One Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    The electronic configuration of the elements A and Bare 1s2, 2s 2,2p6,3s2 and 1s2, 2s2,2p5 respectively. The formula of the ionic compound that can be formed between these elements is

  • 2)

    Various successive ionisation enthalpies (in kJ mol-1) of an element are given below.

    IE1 IE2 IE3 IE4 IE5
    577.5 1,810 2,750 11,580 14,820

    The element is

  • 3)

    In the third period the first ionization potential is of the order

  • 4)

    Identify the wrong statement.

  • 5)

    Which one of the following arrangements represent the correct order of least negative to most negative electron gain enthalpy

Basic Concepts Of Chemistry And Chemical Calculations & Quantum Mechanical Model Of Atom Important Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Assertion (A): Among halogens fluorine is the best oxidant. Reason
    (R): Fluorine is the most electronegative atom.

  • 2)

    The oxidation number of fluorine in all its compounds is equal to

  • 3)

    The empirical formula of glucose is _______________

  • 4)

    The maximum number of electrons in a sub shell is given by the expression

  • 5)

    What will be the wavelength of a ball of mass 0.1 kg moving with a velocity of 10ms-1?

Basic Concepts Of Chemistry And Chemical Calculations & Quantum Mechanical Model Of Atom Important Five Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Balance the following equation by oxidation number method:
    Zn + HNO3 \(\rightarrow\)Zn(NO3)2 + NH4NO3 + H2O

  • 2)

    Balance the following equation by ion-electron method In acidic medium.
    \(S_2O_3^{2-}+I_2\rightarrow S_2O_4^{2-}+SO_2+I^-\)

  • 3)

    Balance the following equation by ion-electron method In acidic medium.
    \(Cr{(OH)}_4^-+H_2O_2\rightarrow Cr{O}_4^{2-}\)

  • 4)

    An insecticide has the following percentage composition by mass: 47.5% C, 2.54% H, and 50.0% Cl. Determine its empirical formula and molecular formulae. Molar mass of the substance is 354.5g mol-1

  • 5)

    The Mn3+ ion is unstable in solution and undergoes disproportionation to give Mn2+, MnO2 and H+ ion. Write a balanced ionic equation for the reaction.

Basic Concepts Of Chemistry And Chemical Calculations & Quantum Mechanical Model Of Atom Important Three Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    How much mass (in gram units) is represented by the following?
    0.2 mol of NH3

  • 2)

    Calculate the Formula Weights of the following compounds.C6H12O6 - Glucose

  • 3)

    Calculate the Formula Weights of the following compounds.NaOH

  • 4)

    Calculate Equivalent mass of the Phosphorous acid

  • 5)

    Calculate the molar volume of the following 460g of formic acid

Basic Concepts Of Chemistry And Chemical Calculations & Quantum Mechanical Model Of Atom Important Two Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Define equivalent mass

  • 2)

    Distinguish between oxidation and reduction.

  • 3)

    Calculate the molar mass of the following compounds. -
    i) urea [CO(NH2)2]
    ii) acetone [CH3 COCH3]
    iii) boric Acid [H3BO3]
    iv) Sulphurci  Acid [H2SO4]

  • 4)

    Calculate the molar mass of the following compounds. -boric Acid [H3BO3]

  • 5)

    Calculate the average atomic mass of naturally occurring magnesium using the following data

    Isotope Istopic atomic mass Abundance(%)
    Mg24 23.99 78.99
    Mg26 24.99 10.00
    Mg25 25.98 11.01

Basic Concepts Of Chemistry And Chemical Calculations & Quantum Mechanical Model Of Atom Important One Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Assertion: Two mole of glucose contains 12.044 x 1023 molecules of glucose
    Reason: Total number of entities present in one mole of any substance is equal to 6.02 x 1022

  • 2)

    1 g of an impure sample of magnesium carbonate (containing no thermally decomposable impurities) on complete thermal decomposition gave 0.44 g of carbon dioxide gas. The percentage of impurity in the sample is ______________

  • 3)

    When 22.4 litres of H2(g) is mixed with 11.2 litres of Cl2(g), each at 273 K at 1 atm the moles of HCl (g), formed is equal to

  • 4)

    Hot concentrated sulphuric acid is a moderately strong oxidizing agent. Which of the following reactions does not show oxidising behaviour?

  • 5)

    Fe2 + \(\longrightarrow\) Fe3+ + e- is a ________ reaction.

11th Chemistry Important Question Paper 4 - by Karthi - View & Download

  • 1)

    The electronic configuration of the elements A and Bare 1s2, 2s 2,2p6,3s2 and 1s2, 2s2,2p5 respectively. The formula of the ionic compound that can be formed between these elements is

  • 2)

    The group of elements in which the differentiating electron enters the anti penultimate shell of atoms are called

  • 3)

    How does electron affinity change when we move from left to right in a period in the periodic table?

  • 4)

    Which of the following pairs of elements exhibit diagonal relationship?

  • 5)

    Period of an element is represented by _____ quantum number

11th Chemistry Term 2 Question Paper - by Karthi - View & Download

  • 1)

    In which of the following Compounds does the central atom obey the octet rule?

  • 2)

    In the molecule O= C = OB, the formal charge on OA, C and OB are respectively.

  • 3)

    Which of the following is electron deficient?

  • 4)

    Which of the following molecule contain no л bond?

  • 5)

    Of the following molecules, which have shape similar to carbondixide?

11th Chemistry Important Question Paper 2 - by Karthi - View & Download

  • 1)

    The number of water molecules in a drop of water weighing 0.018 g is

  • 2)

    1 g of an impure sample of magnesium carbonate (containing no thermally decomposable impurities) on complete thermal decomposition gave 0.44 g of carbon dioxide gas. The percentage of impurity in the sample is ______________

  • 3)

    When 6.3g of sodium bicarbonate is added to 30g of the acetic acid solution, the residual solution is found to weigh 33g. The number of moles of carbon dioxide released in the reaction is

  • 4)

    When 22.4 litres of H2(g) is mixed with 11.2 litres of Cl2(g), each at 273 K at 1 atm the moles of HCl (g), formed is equal to

  • 5)

    The oxidation number of oxygen in O2 is _______________

11th Chemistry Model Paper 2 - by Karthi - View & Download

  • 1)

    Which of the following statements about hydrogen is incorrect?

  • 2)

    Water gas is

  • 3)

    The cause of permanent hardness of water is due to

  • 4)

    Zeolite used to soften hardness of water is hydrated

  • 5)

    A commercial sample of hydrogen peroxide marked as 100 volume H2O2, it means that

11th Chemistry Model Question Paper 1 - by Karthi - View & Download

  • 1)

    Which of the following statements about hydrogen is incorrect?

  • 2)

    Water gas is

  • 3)

    The hardness of water can be determined by volumetrically using the reagent

  • 4)

    The cause of permanent hardness of water is due to

  • 5)

    Zeolite used to soften hardness of water is hydrated

11th Chemistry Important One Mark Question Paper 1 - by K RAJA - View & Download

  • 1)

    40 ml of methane is completely burnt using 80 ml of oxygen at room temperature The volume of gas left. after cooling to room temperature is

  • 2)

    An element X has the following isotopic Composition 200X = 90%, 199X = 8% and 202X = 2% The Weighted average atomic mass of the element X is closet to  

  • 3)

    Assertion: Two mole of glucose contains 12.044 x 1023 molecules of glucose
    Reason: Total number of entities present in one mole of any substance is equal to 6.02 x 1022

  • 4)

    Carbon forms two oxides, namely carbon monoxide and carbon dioxide. The equivalent mass of which element remains constant?

  • 5)

    The equivalent mass of a trivalent metal element is 9 g eq-1 the molar mass of its anhydrous oxide is

11th chemistry p - Block Elements important question paper - by K RAJA - View & Download

  • 1)

    The electronic configuration of the elements A and Bare 1s2, 2s 2,2p6,3s2 and 1s2, 2s2,2p5 respectively. The formula of the ionic compound that can be formed between these elements is

  • 2)

    The group of elements in which the differentiating electron enters the anti penultimate shell of atoms are called

  • 3)

    In which of the following options the order of arrangement does not agree with the variation of property indicated against it?

  • 4)

    Which of the following elements will have the highest electro negativity

  • 5)

    Various successive ionisation enthalpies (in kJ mol-1) of an element are given below.

    IE1 IE2 IE3 IE4 IE5
    577.5 1,810 2,750 11,580 14,820

    The element is

11th standard Coordination Compounds and Bio-Coordination Compounds - by K RAJA - View & Download

  • 1)

    Gases deviate from ideal behavior at high pressure. Which of the following statement(s) is correct for non-ideality?

  • 2)

    Rate of diffusion of a gas is

  • 3)

    Which of the following is the correct expression for the equation of state of van der Waals gas?

  • 4)

    When an ideal gas undergoes unrestrained expansion, no cooling occurs because the molecules

  • 5)

    Equal weights of methane and oxygen are mixed in an empty container at 298 K. The fraction of total pressure exerted by oxygen is

Quantum Mechanical Model Of Atom Important Question Paper - by MUTHUSAMY K - View & Download

  • 1)

    How many orbitals are possible for n =4?

  • 2)

    How many radial nodes for 2s, 4p, 5d and 4f orbitals exhibit? How many angular nodes

  • 3)

    Which quantum number reveal information about the shape, energy, orientation and size of orbitals?

  • 4)

    What are the defects of Rutherford's model?

  • 5)

    What is the charge and mass of an electron?

Important One Mark Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    Carbon forms two oxides, namely carbon monoxide and carbon dioxide. The equivalent mass of which element remains constant?

  • 2)

    The oxidation number of oxygen in O2 is _______________

  • 3)

    7.5 g of a gas occupies a volume of 5.6 litres at 0° C and 1 atm pressure. The gas is

  • 4)

    Give an example of molecule in which the ratio of the molecular formula is six times the empirical formula.

  • 5)

    The compound in which mass percentage of carbon is 75% and that of hydrogen is 25% is

11th Chemistry Term I Model Question Paper - by Karthi - View & Download

  • 1)

    40 ml of methane is completely burnt using 80 ml of oxygen at room temperature The volume of gas left. after cooling to room temperature is

  • 2)

    An element X has the following isotopic Composition 200X = 90%, 199X = 8% and 202X = 2% The Weighted average atomic mass of the element X is closet to  

  • 3)

    The number of water molecules in a drop of water weighing 0.018 g is

  • 4)

    Which one of the following represents 180g of water?

  • 5)

    The oxidation number of Cr in Cr2O72- __________ is

Thermodynamics Important Question Paper In 11th Chemistry - by Karthi - View & Download

  • 1)

    The enthalpies of formation of Al2O3 and Cr2Oare -1596 kJ and -1134 kJ, respectively. ΔH for the reaction 2AI + Cr2O3 ⟶ 2Cr + Al2O3 is

  • 2)

    Which of the following is not a thermodynamic function?

  • 3)

    The value of ΔH for cooling 2 moles of an ideal monatomic gas from 125° C to 25° C at constant pressure will be [given Cp=\(\frac{5}{2}\)R]

  • 4)

    Given that C(g)+ O2(g) ⟶ CO2(g)ΔHo =-akJ;2CO(g)+O2(g) ⟶ 2CO2(g)ΔHo=-bkJ; Calculate the AHo for the reaction C(g)+ 1/2O2(g) ⟶ CO(g)

  • 5)

    When 15.68 litres of a gas mixture of methane and propane are fully combusted at 0° C and 1 atmosphere, 32 litres of oxygen at the same temperature and pressure are consumed. The amount of heat of released from this combustion in KJ is (ΔHc (CH4) = - 890 KJ mol-1 and ΔHc (C3H8 = - 2220 KJ mol-1)

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