Chemistry of the actinoids is more complex in the view of their ability to exist in different oxidation states. Further, many of the actinoid elements are radioactive which make the study of these elements rather difficult.

molecules of Glucose.

(i) The nature of the substance whether colloid or crystalloid depends upon size of the solute particles. When the size of solute particles lies between 1 to 1000 nm, it behaves as a colloid. 
(ii) The colloidal water particles of the clouds get neutralized and coagulated to bigger water drops by spraying salt.

If a is the edge length of bcc unit cell and r is the radius of atom, then
edge not covered by atom = a = 2r.
In bcc, body diagonal = \(\sqrt { 3 } a\)
\(4r=\sqrt { 3 } a\)
or    \(r=\frac { \sqrt { 3 } }{ 4 } a\)
\(\therefore \) Edge not covered by atoms = \(a-2\times \frac { \sqrt { 3 } }{ 4 } a\)
 = \(\frac { a\left( \frac { 2-\sqrt { 3 } }{ 2 } \right) }{ a } \)
= \(\frac { 2-1.732 }{ 2 } =0.134%\)%

01 M BaCI₂ solution will have higher boiling point because of large number of particles on dissociation.
\( \mathrm{NaCI} \longrightarrow \mathrm{Na}^{+}+\mathrm{CI}^{-}(2 \text { particles }) \\ \mathrm{BaCI}_2 \longrightarrow \mathrm{Ba}^{2+}+2 \mathrm{CI}^{-}(3 \text { particles }) \)

Due to low bond dissociation enthalpy, high electronegativity and large negative electron gain enthalpy halogens have a strong tendency to accept electrons and thus get reduced.
\({ X }_{ 2 }+2{ e }^{ - }\longrightarrow 2{ X }^{ - }\)
As a result, halogens act as strong oxidising agents. Their oxidising power, however, decreases from \({ F }_{ 2 }\) to \({ I }_{ 2 }\) as is evident from their electrode potentials :
\({ { E }^{ ° } }_{ { F }_{ 2 }/{ F }^{ - } }=+2.87,\ { { E }^{ ° } }_{ { Cl }_{ 2 }/{ Cl }^{ - } }=+1.36V\ ;\ { { E } }_{ { Br }_{ 2 }/{ Br }^{ - } }=+1.09V\ and\ { { E }^{ ° } }_{ { I }_{ 2 }/{ I }^{ - } }=+0.54V\)
Thus, \({ F }_{ 2 }\) is the strongest while \({ I }_{ 2 }\) is the weakest oxidising agent.

New \({ P }_{ Total }=222.2+16.6=238.8mm\) New \({ y }_{ B }=\frac { 222.2 }{ 238.8 } =0.93\)

0.423

Common salt is called de - icing agent because it lowers the freezing point of water to such an extent that it does not freeze to form ice. Hence, it is used to clear snow from roads.

Carbon atom in carbonyl compounds acquires slight positive charge and is attacked by nucleophile.
Alkenes undergo electrophilic addition whereas aldehydes and ketones undergo nucleophilic addition because in alkenes the double bond joins two carbon atoms and there is no resultant polarity.

(i) Acidic flux: SiO₂ is acidic flux.
(ii) Basic flux: CaO is basic flux.

In ccp structure, there are 8 tetrahedral voids. In dose-packed structure, there are eight spheres in the corner of the unit cell and each sphere is in contact with three others giving rise to eight tetrahedral voids.

A) S_N2 reactions involve the formation of transition state. Higher the steric hindrance, lesser the stability of transition state and lower is their reactivity towards S_N2.

b) Among the given compounds, 2-bromopentane is optically active due to presence of chiral carbon (*)

A chiral carbon have four different groups or atoms attached separately to its four valencies
c) 2-bromo-2-methylbutane is most reactive towards \(\beta \) -elimination reaction because in this case more substituted alkene is the major product.

The volume of k comes out to be nearly constant. Hence of the first order.

(i) 1 F or 96500 C  
(ii) 4.44 F or 428460 C

(i) 6-Chloro-4-ethylhexan-3-one
(ii) Pentane-2, 4-dione
(iii) 3, 3-Dimethylbutanoic acid

'A' is PCl_5. (It is a yellowish-white solid).
'B' is PCl₃ (It is a colourless oily liquid).
P₄(s) + 10Cl₂(g) \(\to\) 4PCl₅(s)
P₄(s) + 6Cl₂ (g) \(\to\) 4PCI₃(l)
PCl₅, on hydrolysis gives H₃PO₄, whereas
PCl₃, on hydrolysis gives H₃PO₃.
PCl₅ + 4H₂O \(\to\) H₃PO₄ + 5HCl
PCl₃ + 3H₂O \(\to\) H₃PO₃ + 3HCl

(i) 3Cl₂ + \(\underset {hot\ and \ conc} {6NaOH}\) \(\to\) 5NaCl + NaCIO₃ + 3H₂O
(ii) XeF₄ + 3H₂O \(\to\) XeO₃ + 6HF
(iii) SO₂ + 2NaOH \(\to\) Na₂So₃ + H₂O

If R_I is the rate of first reaction at 25°C, then as its temperature coefficient is 2, its rate at 35°C will be = 2 R₁, at 45°C = 2 x 2 R₁ = 4 R₁ and at 55°C = 2 x 4 R₁ = 8 R₁
If R₂.is the rate of the second reaction at 25°C, then as its temperature coefficient is 3, its rate at 35°C will be = 3 R₂, at 45°C = 3 x 3 R₂ = 9 R₂ and at 55°C = 3 x 9 R₂ = 27 R₂
Also, we are given R₁ = R₂, i.e., at 25°C, the rates are equal.
At 55⁰C, \({Rate\ of\ 2nd\ reaction\over Rate\ of\ 1st\ reaction}={27R_2\over 8R_1}={27\over 8}\)

(a) \((i)\ 6NaOH+3CI_{ 2 }\longrightarrow 5NaCI+NaCIO_{ 3 }+3H_{ 2 }O\)
\(\\ (ii)\ { XeF }_{ 6 }+3H_{ 2 }O\longrightarrow { XeO }_{ 3 }+6HF\) 
(b)
(i) It is due to more inter-electronic repulsion between valence electrons of oxygen atom.
(ii) \({ F }_{ 2 }\) is stronger oxidising agent and has lower bond energy than \({ CI }_{ 2 }\) therefore, \({ NF }_{ 3 }\)is a exothermic compound due to stronger N-F bond than N-CI bond i.e., energy is released in its formation whereas   \({ NCI }_{ 3 }\)is an endothermic compound i.e., energy is absorbed in its formation.
(iii) It is due to presence of two lone pairs of electrons and has \({ sp }^{ 3 }d\)hybirdisation.