Question Set A

CBSE 11th Chemistry Structure of Atom Model Questions Papers Study Material - QB365

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Questions:

Multiple Choice Question

90 x 1 = 90

Anything that influences the valence electrons will affect the chemistry of the element. Which one of the following factors does not affect the valence shell?

(a)

Valence principal quantum number (n)

(b)

Nuclear charge (Z)

(c)

Nuclear mass

(d)

Number of core electrons

Which of the following electrodes will act as anodes, when connected to Standard Hydrogen Electrode?

(a)

\(\mathrm{Al} / \mathrm{Al}^{3+} \ \ \mathrm{E}^{\ominus}=-1.66 \)

(b)

\(\mathrm{Fe} / \mathrm{Fe}^{2+} \ \mathrm{E}^{\ominus}=-0.44\)

(c)

\(\mathrm{Cu} / \mathrm{Cu}^{2+} \ \mathrm{E}^{\Theta}=+0.34 \)

(d)

\( \mathrm{F}_{2}(\mathrm{~g}) / 2 \mathrm{~F}^{-}(a q) \ \mathrm{E}^{\Theta}=+2.87\)

Identify the correct statements with reference to the given reaction
\(\mathrm{P}_{4}+3 \mathrm{OH}^{-}+3 \mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{PH}_{3}+3 \mathrm{H}_{2} \mathrm{PO}_{2}^{-}\)

(a)

Phosphorus is undergoing reduction only.

(b)

Phosphorus is undergoing oxidation only

(c)

Phosphorus is undergoing oxidation as well as reduction.

(d)

Hydrogen is undergoing neither oxidation nor reduction.

The more positive the value of EO, the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
E^o values:
\( \mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}=+0.77 ; \mathrm{I}_{2}(\mathrm{~s}) / \mathrm{I}=+0.54 \)
\(\mathrm{Cu}^{2+} / \mathrm{Cu}=+0.34 ; \mathrm{Ag}^{+} / \mathrm{Ag}=+0.80 \mathrm{~V} \)

(a)

\( \mathrm{Fe}^{3+} \)

(b)

\(\mathrm{I}_{2}(\mathrm{~s}) \)

(c)

\(\mathrm{Cu}^{2+} \)

(d)

\(\mathrm{Ag}^{+} \)

Which of the following is not a redox reaction?

(a)

\( \mathrm{CaCO}_{3} \longrightarrow \mathrm{CaO}+\mathrm{CO}_{2} \)

(b)

\(2 \mathrm{H}_{2}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O} \)

(c)

\(2 \mathrm{Na}+2 \mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{NaOH}+\mathrm{H}_{2} \)

(d)

\(\mathrm{MnCl}_{3} \longrightarrow \mathrm{MnCl}_{2}+\frac{1}{2} \mathrm{Cl}_{2} \)

Which of the following metal displacement reaction will not take place and why?

(a)

\(\mathbf{C u}+\mathbf{M g}^{2+} \longrightarrow \)

(b)

\( \mathrm{Mg}+\mathrm{Cu}^{2+} \longrightarrow \)

(c)

\(\mathbf{P b}+\mathbf{A g}^{+} \longrightarrow \)

(d)

\( \mathrm{Zn}+\mathrm{Cu}^{2+} \longrightarrow\)

Standard reduction frotential of X, Y, Z are -1.2 v, + 0.5 v, -3.0 v respectively, the reducing power of the metals will be ______.

(a)

Y > Z > X

(b)

Y > X > Z

(c)

Z > X > Y

(d)

X > Y > Z

The oxidation state of Cr in CrO₅ is ______.

(a)

+10

(b)

(c)

(d)

Which of the following solution is strongest oxidising agent?

(a)

\(\mathbf{M n O}_{4}^{-} \text {in acidic medium }\)

(b)

\(\mathbf{M n} \mathbf{O}_{4}^{-} \text {in basic medium }\)

(c)

MnO₂ in basic medium

(d)

\(\mathrm{CrO}_{4}^{2-} \text { in basic medium }\)

10.

The statement that is not correct for periodic classification of elements is:

(a)

The properties of elements are periodic function of their atomic numbers.

(b)

Non metallic elements are less in number than metallic elements.

(c)

For transition elements, the 3d-orbitals are filled with electrons after 3p-orbitals and before 4s-orbitals.

(d)

The first ionisation enthalpies of elements generally increase with increase in atomic number as we go along a period.

11.

Which of the following statements are correct?

(a)

Helium has the highest first ionisation enthalpy in the periodic table.

(b)

Chlorine has less negative electron gain enthalpy than fluorine.

(c)

Mercury and bromine are liquids at room temperature.

(d)

In any period, atomic radius of alkali metal is the highest.

12.

The electronegativities of C, N, Si and P are in order of ______.

(a)

Si < P < C < N

(b)

Si < P < N < C

(c)

P < Si < N < C

(d)

P < Si < C < N

13.

Which elements is expected to have lowest ionisation enthalpy?

(a)

(b)

(c)

(d)

14.

In the p^3-, S^2- and CI- ions, the increasing order of size is ______.

(a)

CI^-, S^2-, P^3-

(b)

P^3-, S^2-, CI^-

(c)

S^2-, CI^-, P^3-

(d)

S^2-, P^3-, CI^-

15.

Which of the following sets of quantum numbers are correct?

(a)

n = 1
l = 1
m_l= +2

(b)

n = 2
l = 1
m_l= +1

(c)

n = 3
l = 2
m_l= -2

(d)

n = 3
l = 4
m_l= -2

16.

Out of the following pairs of electrons, identify the pairs of electrons present in degenerate orbitals: _______.

(a)

\((i) n=3, l=2, m_{l}=-2, m_{s}=-\frac{1}{2} \)
\((ii) n=3, l=2, m_{l}=-1, m_{s}=-\frac{1}{2}\)

(b)

\((i) n=3, l=1, m_{l}=1, m_{s}=+\frac{1}{2} \)
\((ii) n=3, l=2, m_{l}=1, m_{s}=+\frac{1}{2}\)

(c)

\((i) n=4, l=1, m_{l}=1, m_{s}=+\frac{1}{2} \)
\((ii) n=3, l=2, m_{l} \doteq 1, m_{s}=+\frac{1}{2}\)

(d)

\((i) n=3, l=2, m_{l}=+2, m_{s}=-\frac{1}{2} \)
\((ii) n=3, l=2, m_{l}=+2, m_{s}=+\frac{1}{2}\)

17.

Which of the following is wrong statement?

(a)

The uncertainty principle is \(\Delta x . \Delta v \geq \frac{h}{4 \pi} \text { . }\)

(b)

Half filled and fully filled orbitals have greater stability due to greater exchange energy, greater symmetry and more balanced arrangement

(c)

The energy of 2s orbital is less than the energy of 2p-orbitals in case of hydrogen like atoms.

(d)

de Broglie wavelength, \(\lambda=\frac{h}{2 \pi} .\)

18.

Which of the following statements concerning the quantum numbers are correct?

(a)

Angular quantum number determines the three dimensional shape of the orbital.

(b)

The principal quantum number determines the orientation and energy of the orbital.

(c)

Magnetic quantum number determines the size of the orbital.

(d)

Spin quantum number of an electron determines the orientation of the spin of electron relative to the chosen axis

19.

Magnetic moment 2.83 BM is given by which of the following ions? [Atomic number Ti = 22, Cr = 24, Mn = 25, i = 28]

(a)

Ti³⁺

(b)

Ni²⁺

(c)

Cr²⁺

(d)

Mn²⁺

20.

The ration of de Broglie wavelengths of a deuterium atom to that of α-particles, when the velocity of the former is 5 times greater than of latter is_______.

(a)

(b)

0.2

(c)

(d)

0.4

21.

The rods of transition metals such as copper and zinc where potential difference is generated, are termed as ______.

(a)

electrodes

(b)

cathodes

(c)

anodes

(d)

None of these

22.

Water molecule is formed by the reaction,\(2 \mathrm{H}_{2}+\mathrm{O}_{2} \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}\) What does happen in this reaction?

(a)

Electrons are transferred from H to O-atom

(b)

Electrons are transferred from O to H-atom

(c)

Electrons are accepted by H from O-atom

(d)

Electrons are donated by O to H-atom

23.

Which is the best description of behaviour of bromine in the given equation?
\(\mathrm{H}_{2} \mathrm{O}+\mathrm{Br}_{2} \longrightarrow \mathrm{HBr}+\mathrm{HOBr}\)

(a)

Proton acceptor

(b)

Both oxidised and reduced

(c)

Oxidised

(d)

Reduced

24.

The algebraic sum of the oxidation number of all the atoms in a compound must be ______.

(a)

(b)

-1

(c)

zero

(d)

None of these

25.

An element if present in the free or the uncombined state, its each atom bears an oxidation number ______.

(a)

more than 1

(b)

less than 1

(c)

more than 2

(d)

zero

26.

The given reaction, CUSO₄\(+\mathrm{Zn} \longrightarrow \mathrm{Cu}+\mathrm{ZnSO}_{4}\) is an example of ______.

(a)

metal displacement reaction

(b)

non-metal displacement reaction

(c)

metal-addition reaction

(d)

non-metal addition reaction

27.

The reaction, 2H₂\(0(l) \stackrel{\Delta}{\longrightarrow} 2 \mathrm{H}_{2}(g)+0_{2}(g)\) is anexample of ______.

(a)

addition reaction

(b)

decomposition reaction

(c)

displacement reaction

(d)

None of these

28.

Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
\( E^{\ominus} \text { values: } \mathrm{Fe}^{3+} / \mathrm{Fe}^{2+}=+0.77 ; \mathrm{I}_{2} / \mathrm{I}^{-}=+0.54\)
\(\mathrm{Cu}^{2+} / \mathrm{Cu}=+0.34 ; \mathrm{Ag}^{+} / \mathrm{Ag}=+0.80 \mathrm{~V} \)

(a)

Fe³⁺ and I^-

(b)

Ag⁺ and Cu

(c)

Fe³⁺ and Cu

(d)

Ag and Fe³⁺

29.

In Daniell cell, electrons flow from ______.

(a)

cathode to anode

(b)

anode to cathode

(c)

copper to zinc

(d)

\(\mathrm{SO}_{4}^{2-} \text { to } \mathrm{Cu}^{2+}\)

30.

Consider the following chemical reaction \(\mathrm{MnO}_{4}^{-}(a q)+\mathrm{I}^{-}(a q) \longrightarrow \mathrm{MnO}_{2}(s)+\mathrm{I}_{2}(s)\) Which of the following reactions is an oxidation half-reaction?

(a)

\(\mathrm{MnO}_{4}^{-}(a q) \longrightarrow \mathrm{MnO}_{2}(s)\)

(b)

\(\mathrm{I}^{-}(a q) \longrightarrow \mathrm{I}_{2}(s)\)

(c)

Both (a) and (b)

(d)

None of the above

31.

To balance the charges which of the following is added to one side of the half-reaction?

(a)

Proton

(b)

Hydrogen

(c)

Oxygen

(d)

Electrons

32.

In the reaction, \(2 \mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}+\mathrm{I}_{2} \rightarrow \mathrm{Na}_{2} \mathrm{~S}_{4} \mathrm{O}_{6}+2 \mathrm{NaI}\) I₂acts as ______.

(a)

oxidising agent

(b)

reducing agent

(c)

oxidising as well as reducing agent

(d)

None of the above

33.

In the reaction, \(2 \mathrm{KClO}_{3} \longrightarrow 2 \mathrm{KCl}+30_{2}\) the elements which have been oxidised and reduced respectively are ______.

(a)

chlorine and oxygen

(b)

oxygen and chlorine

(c)

potassium and oxygen

(d)

oxygen and potassium

34.

In the reaction, 4Na + O₂ \(\rightarrow\) 2Na₂O, sodium acts as a/an ______.

(a)

oxidising agent

(b)

reducing agent

(c)

complexing agent

(d)

None Of these

35.

In the given reaction, 2Na + S \(\rightarrow\) 7 Na2S, sulphur is ______.

(a)

oxidised

(b)

reduced

(c)

reducing agent

(d)

None of these

36.

In which of the following compounds, an element exhibits two different oxidation states?

(a)

\(\mathrm{NH}_{2} \mathrm{OH}\)

(b)

\(\mathrm{NH}_{4} \mathrm{NO}_{3}\)

(c)

\(\mathrm{N}_{2} \mathrm{H}_{4}\)

(d)

\(\mathrm{N}_{3} \mathrm{H}\)

37.

Thiosulphate reacts differently with iodine and bromine in the reactions given below
\( 2 \mathrm{~S}_{2} \mathrm{O}_{3}^{2-}+\mathrm{I}_{2} \rightarrow \mathrm{S}_{4} \mathrm{O}_{6}^{2-}+2 \mathrm{I}^{-} \)
\(\mathrm{S}_{2} \mathrm{O}_{3}^{2-}+2 \mathrm{Br}_{2}+5 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{SO}_{4}^{2-}+4 \mathrm{Br}^{-}+10 \mathrm{H}^{+} \)
Which of the following statements justifies the above dual behaviour of thiosulphate?

(a)

Bromine is a stronger oxidant than iodine

(b)

Bromine is a weaker oxidant than iodine

(c)

Thiosulphate undergoes oxidation by bromine and reduction by iodine in these reactions

(d)

Bromine undergoes oxidation and iodine undergoes reduction in these reactions

38.

Which of the following reactions represent(s) redox process?

(a)

Electrochemical process for extraction of highly reactive metals and non-metals

(b)

Manufacturing of caustic soda

(c)

Corrosion of metals

(d)

All of the above

39.

In the given reaction, \(\mathrm{CH}_{2}=\mathrm{CH}_{2}(g)+\mathrm{H}_{2}(g) \longrightarrow \mathrm{CH}_{3}-\mathrm{CH}_{3}(g)\) ethene undergoes ______.

(a)

reduction process

(b)

oxidation process

(c)

addition process

(d)

All of these

40.

Which of the following processes takes place in oxidation?

(a)

Addition of oxygen

(b)

Addition of hydrogen

(c)

Removal of oxygen

(d)

Removal of chlorine

41.

The oxide formed by the element on extreme right and in the left of periodic table are generally ______.

(a)

acidic, amphoteric respectively

(b)

acidic, basic respectively

(c)

neutral, amphoteric respectively

(d)

basic, neutral respectively

42.

Which of the following groups of elements have highly negative electron gain enthalpy?

(a)

Group-16

(b)

Group-17

(c)

Group-14

(d)

Both (a) and (b)

43.

What effect is observed, on the size of an atom when an electron is removed and in another case an electron is added to the same atom?

(a)

Size increases and decreases respectively

(b)

Size decrease and increases respectively

(c)

Size increases in both cases

(d)

Size decreases in both cases

44.

According to IUPAC,total number of groups and periods in the periodic table respectively are ______.

(a)

16, 9

(b)

18, 7

(c)

18, 9

(d)

13, 7

45.

Which of the following properties is inversely related to electronegativity?

(a)

Non-metallic properties

(b)

Metalloid properties

(c)

Ionic properties

(d)

Metallic properties

46.

Which of the following compounds is/are amphoteric in nature?

(a)

Cl₂O₇

(b)

Al₂O₃

(c)

As₂O₃

(d)

Both (b) and (c)

47.

Which of the following is/ are general characteristics of an atom with high electronegativity?

(a)

Tendency to form positive ions

(b)

Small atomic size

(c)

High ionisation potential

(d)

Both (b) and (c)

48.

Among halogens, the correct order of amount of energy released in electron gain (electron gain enthalpy) is ______.

(a)

F > Cl > Br > I

(b)

F > Cl > Br > I

(c)

F < CI > Br > I

(d)

F < Cl < Br < I

49.

In general second ionisation enthalpy of an atom will be ______.

(a)

higher than the first ionisation enthalpy

(b)

equal to the first ionisation enthalpy

(c)

higher than the third ionisation enthalpy

(d)

equal to the third ionisation enthalpy

50.

The first ionisation enthalpies of Na, Mg, AI and Si are in the order______.

(a)

Na < Mg > Al < Si

(b)

Na > Mg > Al > Si

(c)

Na < Mg < Al < Si

(d)

Na > Mg > Al < Si

51.

Consider the isoelectronic species, Na⁺.Mg²⁺, F^- and O^2-. The correct order of increasing length of their radii is ______.

(a)

\(\mathrm{F}^{-}<\mathrm{O}^{2-}<\mathrm{Mg}^{2+}<\mathrm{Na}^{+}\)

(b)

\(\mathrm{Mg}^{2+}<\mathrm{Na}^{+}<\mathrm{F}^{-}<\mathrm{O}^{2-}\)

(c)

\(\mathrm{O}^{2-}<\mathrm{F}^{-}<\mathrm{Na}^{+}<\mathrm{Mg}^{2+}\)

(d)

\(\mathrm{O}^{2-}<\mathrm{F}^{-}<\mathrm{Mg}^{2+}<\mathrm{Na}^{+}\)

52.

Which of the following radii reflect an increase in size of an atom?

(a)

van der Waals' radius

(b)

Metallic radius

(c)

Covalent (non-metallic) radius

(d)

Both (b) and (c)

53.

Out of the four blocks in which periodic table is divided, helium belongs which block?

(a)

s-block

(b)

p-block

(c)

d-block

(d)

f-block

54.

3d-transition series of elements starts with scandium which has the electronic configuration _____.

(a)

3d¹4s²

(b)

3d¹4s¹

(c)

3d² 4s²

(d)

3d³ 4s²

55.

General outer electronic configuration of d-block elements is _____.

(a)

\((n-1) d^{1-10} n s^{3}\)

(b)

\((n+1) d^{1-10} n s^{0-2}\)

(c)

\((n-1) d^{1-10} n s^{0-2}\)

(d)

\((n-1) d^{0} n s^{0-2}\)

56.

Predict the position of an element having the electronic configuration \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{1}\) _____.

(a)

Period 4, group 6

(b)

Period 6, group 4

(c)

Period 3, group 1

(d)

Period 4, group 5

57.

The symbol and name according to the IUPAC system for the element with atomic number = 120,respectively are _____.

(a)

Ubn and unbinilium

(b)

Ubn and unbiunium

(c)

Ubn and unnilbium

(d)

Ubn and unnilium

58.

Who developed the long form of the periodic table?

(a)

Niels Bohr

(b)

Moseley

(c)

Mendeleef

(d)

Lothar Meyer

59.

Elements having similar outer shell electronic configuration in their atoms are arranged in _____.

(a)

groups

(b)

vertical columns

(c)

families

(d)

All of these

60.

Which of the following statements is incorrect?

(a)

Mendeleev's arranged elements in horizontal rows and vertical columns

(b)

Mendeleev's arranged elements in order of their increasing atomic number

(c)

Mendeleev's system of classifying elements was more elaborate than that of Lother Meyer

(d)

None of the above

61.

The atomic numbers of elements X, Y, and Z are 19,21and 25 respectively. The number of electrons present in the M-shell of these elements follow the order _______.

(a)

Z > X > Y

(b)

X > Y > Z

(c)

Z > Y > X

(d)

Y > Z > X

62.

The only series of lines appear in the visible region of the electromagnetic spectrum of hydrogen is _______.

(a)

Lyman series

(b)

Balmer series

(c)

Paschep series

(d)

Pfund series

63.

Major development(s) responsible for the formulation of Bohr's model of atom were _______.

(a)

dual character of the electromagnetic radiation

(b)

experimental results regarding atomic spectra which can be explained only by assuming quantised electronic energy levels in atoms

(c)

Both (a) and (b)

(d)

None of the above

64.

Which of the following statements is/are correct regarding Rutherford scattering experiment?

(a)

Most of the α-particles passed through the gold foil remain undeflected

(b)

A small fraction of the α-particles was deflected by small angles

(c)

A very few a-particles (1 in 20000) bounced back, i.e. were deflected by nearly 180^o

(d)

All of the above

65.

Number of angular nodes for 4 d orbital is ______

(a)

(b)

(c)

(d)

66.

Orbital angular momentum depends on _________

(a)

(b)

n and l

(c)

n and m

(d)

m and s

67.

The probability density plots of Is and 2s orbitals are given in figure.

The density of dots in a region represents the probability density of finding electrons in the region.
On the basis of above diagram which of the following statements is incorrect?

(a)

1s and 2s orbitals are spherical in shape

(b)

The probability of finding the electron is maximum near the nucleus

(c)

The probability of finding the electron at a given distance is equal in all directions

(d)

The probability density of electrons for 2s orbital decreases uniformly as distance from the nucleus increases

68.

The plot of orbital wave function \(\psi\),(r) as a function of distance r of the electron from the nucleus for 2s orbital is _______.

(a)

(b)

(c)

(d)

69.

The correct set of four quantum numbers for the valence electrons of rubidium atom (Z = 37) is _______.

(a)

\(5,0,0,+\frac{1}{2}\)

(b)

\(5,1,0,+\frac{1}{2}\)

(c)

\(5,1,1,+\frac{1}{2}\)

(d)

\(5,0,1,+\frac{1}{2}\)

70.

Probability of finding an electron at a point with in an atom is_______.

(a)

equal to the \(|\psi|^{2}\) 12at that point

(b)

proportional to the \(|\psi|^{2}\) 12at that point

(c)

inversely proportional to the \(|\psi|^{2}\) at the point

(d)

None of the above

71.

In atom, an electron is moving with a speed of 600 m/ s with an accuracy of 0.005%. Certainty with which the position of the electron can be located is_______. (h = 6.6 x 10-34 kg m² s^-1, mass of electron, e_m = 6.6 x 10^-31 kg)

(a)

1.52 x 10^-4 m

(b)

5.10 x 10^-3 m

(c)

1.92 x 10^-3 m

(d)

3.84 x 10^-3 m

72.

Which of the following statement is not correct regarding Bohr's model of hydrogen atom?

(a)

Energy of the electrons in the orbit is quantized

(b)

The electron in the orbit nearest to the nucleus has the lowest energy

(c)

Electrons revolve in different orbits around the nucleus

(d)

The position and velocity of the electrons in the orbit cannot be determined simultaneously

73.

An electron is moving in Bohr's fourth orbit. Its de-Broglie wavelength is λ Calculate the circumference of the fourth orbit.

(a)

2 λ

(b)

4 λ

(c)

4/λ

(d)

2/λ

74.

Calculate the wavelength (in nanometer) associated with a proton moving at 1.0 x 10³ms' _______.(Mass of proton = 1.67 x 10^-27 kg and h = 6.63 x 10^-34Js)

(a)

0.032 nm

(b)

0.40 nm

(c)

2.5 nm

(d)

14.0 nm

75.

Which of tM following is the energy of a possible excited state of hydrogen?

(a)

+13.6eV

(b)

-6.8 eV

(c)

-3.4eV

(d)

+6.8eV

76.

The first line in the Balmer series in the H atom will have the frequency _______.

(a)

3.29 x 10¹⁵ S^-1

(b)

4.57 x 10¹⁴ S^-1

(c)

8.22 x 10¹⁵ S^-1

(d)

8.02 x 10¹⁴ S^-1

77.

The ionisation enthalpy of hydrogen atom is 1.312 x 10⁶J mol^-1. The energy required to excite the electron in the atoms from n₁ = 1 to n2 = 2 is_______.

(a)

6.56 x 10⁵ J mol^-1

(b)

9.84 x 10⁵ J mol^-1

(c)

7.56 x 10⁵J mol^-1

(d)

8.51 x 10⁵ J mol^-1

78.

The electronic transition from n = 2 to n = 1will produce the shortest wavelength in (where, n = principal quantum number) _______.

(a)

He⁺

(b)

(c)

H⁺

(d)

Li²⁺

79.

Which of the following conclusions could not be derived from Rutherford's a-particle scattering experiment?

(a)

Most of the space in the atom is empty

(b)

The radius of the atom is about 10^-10 m while that of nucleus is 10^-15 m

(c)

Electrons move in a circular path of fixed energy called orbits

(d)

Electrons and the nucleus are held together by electrostatic forces of attraction

80.

The orbital with n = 3 and 1 = 2 is _______.

(a)

(b)

(c)

(d)

81.

The idea of stationary orbits was first given by _______.

(a)

Rutherford

(b)

J.J. Thomson

(c)

Niels Bohr

(d)

Max Planck

82.

The Balmer series in the spectrum of hydrogen atom falls in _______.

(a)

ultraviolet region

(b)

visible region

(c)

infrared region

(d)

none of these

83.

In a sodium atom (atomic number = 11 and mass number = 23) and the number of neutrons is _______.

(a)

equal to the number of protons

(b)

less than the number of protons

(c)

greater than the number of protons

(d)

none of these

84.

Cathode rays are deflected by _______.

(a)

electric field only

(b)

electric and magnetic field

(c)

magnetic field only

(d)

none of these

85.

The oxidation number of carbon 'is zero in ______.

(a)

HCHO

(b)

CH₂Cl₂

(c)

C₁₂H₂₂O₁₁

(d)

All the above

86.

Among the following molecules, in which does bromine show the maximum oxidation number?

(a)

Hg₂ (Br0₃)₂

(b)

Br - Cl

(c)

KBrO₄

(d)

Br₂

87.

Which of the following species are not known?

(a)

AgOH

(b)

PbI₄

(c)

PI₅

(d)

SH₆

88.

In halogens, which of the following, increases from iodine to fluorine?

(a)

Bond length

(b)

Electronegativity

(c)

The ionization energy of the element

(d)

Oxidizing power

89.

Which of the following oxides is neutral?

(a)

Sn0₂

(b)

(c)

Al₂O₃

(d)

Na₂O

90.

The highest ionization energy is exhibited by _____.

(a)

halogens

(b)

alkaline earth metals

(c)

transition metals

(d)

noble gases

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Multiple Choice Question

90 x 1 = 90

(a)
\(\mathrm{Al} / \mathrm{Al}^{3+} \ \ \mathrm{E}^{\ominus}=-1.66 \)

(d)
\(\mathrm{Ag}^{+} \)

(d)
\(\mathrm{MnCl}_{3} \longrightarrow \mathrm{MnCl}_{2}+\frac{1}{2} \mathrm{Cl}_{2} \)

(a)
\(\mathbf{C u}+\mathbf{M g}^{2+} \longrightarrow \)

(a)
Y > Z > X

(b)
\(\mathbf{M n} \mathbf{O}_{4}^{-} \text {in basic medium }\)

10.

11.

(a)
Helium has the highest first ionisation enthalpy in the periodic table.

12.

(a)
Si < P < C < N

13.

(a)
Sr

14.

(a)
CI^-, S^2-, P^3-

15.

(b)
n = 2
l = 1
m_l= +1

16.

(a)
\((i) n=3, l=2, m_{l}=-2, m_{s}=-\frac{1}{2} \)
\((ii) n=3, l=2, m_{l}=-1, m_{s}=-\frac{1}{2}\)

17.

18.

(a)
Angular quantum number determines the three dimensional shape of the orbital.

19.

(b)
Ni²⁺

20.

(d)
0.4

21.

(a)
electrodes

22.

(a)
Electrons are transferred from H to O-atom

23.

(b)
Both oxidised and reduced

24.

25.

(d)
zero

26.

(a)
metal displacement reaction

27.

(b)
decomposition reaction

28.

(d)
Ag and Fe³⁺

29.

(b)
anode to cathode

30.

(b)
\(\mathrm{I}^{-}(a q) \longrightarrow \mathrm{I}_{2}(s)\)

31.

(d)
Electrons

32.

(a)
oxidising agent

33.

(b)
oxygen and chlorine

34.

(b)
reducing agent

35.

(b)
reduced

36.

(a)
\(\mathrm{NH}_{2} \mathrm{OH}\)

37.

(a)
Bromine is a stronger oxidant than iodine

38.

(d)
All of the above

39.

(a)
reduction process

40.

(a)
Addition of oxygen

41.

(b)
acidic, basic respectively

42.

(d)
Both (a) and (b)

43.

(b)
Size decrease and increases respectively

44.

(b)
18, 7

45.

(d)
Metallic properties

46.

(d)
Both (b) and (c)

47.

(d)
Both (b) and (c)

48.

49.

(a)
higher than the first ionisation enthalpy

50.

(a)
Na < Mg > Al < Si

51.

(d)
\(\mathrm{O}^{2-}<\mathrm{F}^{-}<\mathrm{Mg}^{2+}<\mathrm{Na}^{+}\)

52.

(a)
van der Waals' radius

53.

(b)
p-block

54.

(a)
3d¹4s²

55.

56.

(a)
Period 4, group 6

57.

(a)
Ubn and unbinilium

58.

(a)
Niels Bohr

59.

(d)
All of these

60.

(b)
Mendeleev's arranged elements in order of their increasing atomic number

61.

62.

(b)
Balmer series

63.

64.

(d)
All of the above

65.

66.

(a)
l

67.

(d)
The probability density of electrons for 2s orbital decreases uniformly as distance from the nucleus increases

68.

69.

(a)
\(5,0,0,+\frac{1}{2}\)

70.

(b)
proportional to the \(|\psi|^{2}\) 12at that point

71.

72.

(d)
The position and velocity of the electrons in the orbit cannot be determined simultaneously

73.

(b)
4 λ

74.

(b)
0.40 nm

75.

76.

(b)
4.57 x 10¹⁴ S^-1

77.

(b)
9.84 x 10⁵ J mol^-1

78.

(d)
Li²⁺

79.

80.

81.

82.

(b)
visible region

83.

84.

(b)
electric and magnetic field

85.

(d)
All the above

86.

87.

88.

89.

(b)
CO

90.

(b)
alkaline earth metals

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