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What is the shape of the $C l F_{3}$ molecule?

Trigonal planar

Trigonal pyramid

T-shaped

Tetrahedral

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Which of the following species/molecules does not have same number of bond pairs and lone pairs?

$O C N^{-}$

$H_{2} O$

$C_{2} H_{2} C l_{2}$

$O_{3}$

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$O_{2} F_{2}$ is an unstable yellow orange solid and $H_{2} O_{2}$ is a colourless liquid both have O $—$ O bond and

O $—$ O bond length in $H_{2} O_{2}$ and $O_{2} F_{2}$ respectively is:

1.22 A, 1.48

1.48 A, 1.22A

1.22 A, 1.22A

1.48 A, 1.48A

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The bond length of the S $—$ O bond in maximum in which of the following compounds?

$S O C I_{2}$

$S O B r_{2}$

$S O F_{2}$

All have the same length

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solubillity of alkali metal fluorides increases down the group select correct explanation for given statement :

Hydration energy increase and lattice energy decrease down the group

both energy decrease down the group but decrease in hyderation energy is rapid

both energy decrease down the group but decrease in lattice energy is rapid

both energy decrease down the group but increase in hyderation energy is rapid

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Explanation

(c) Althogh both hyderation and lattice energies of alkali metal flourides decrease down the group and hyderation energy dominate ove lattice energy, therefore, solubility increase down the group.

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In which of the following compounds B $—$ F bond length is shortest ?

$B {F_{4}}^{-}$

$B F_{3} \leftarrow N H_{3}$

$B F_{3}$

$B F_{3} \leftarrow N {(C H_{3})}_{3}$

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Explanation

(c) Only in $B F_{3}$ p $π$ -p $π$ back bonding is possible due to which B $—$ F bond length is shortest. In order compounds, p-orbital at boron is not possible.

Water molecules are hexagonally closed packed in ice with the help of H-bonds, hence due to existance of voids/interstitial spaces it has cage like structure with less density than water.

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In terms of polar character which of the following order is correct ?

$N H_{3} < H_{2} O < H F < H_{2} S$

$H_{2} S < N H_{3} < H_{2} O < H F$

$H_{2} O < N H_{3} < H_{2} S < H F$

$H F < H_{2} O < N H_{3} < H_{2} S$

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Explanation

(b) As electronegativity difference of bond increase, polar character also increase.

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The correct order or boiling point is:

$T_{2} < D_{2} < H_{2}$

n-pentane<neo pentane

Xe<Ar<He

m-nitrophenol>o-nitrophenol

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The linear structure is possessed by :

$S n C l_{2}$

$N C O^{-}$

$N {O_{2}}^{+}$

$C S_{^{2}}$

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Explanation

(d ) $S = C = S$

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Cis-butene dioic acid $\overset{K_{a_{1}} {- H^{+}}}{⇌} {X^{-}}_{1} \overset{K_{a_{2}} {- H^{+}}}{⇌} X_{2}^{2 -}$

Trans-butene dioic acid $\overset{K_{a_{1}}' {- H^{+}}}{⇌} {Y^{-}}_{1} \overset{K_{a_{2}} \cdot {- H^{+}}}{⇌} Y_{2}^{2 -}$

The incorrect statement regarding above the information is:

$X_{2}^{2 -}$ species is more basic than $Y_{2}^{2 -}$ species

$X_{1}^{-}$ species is more basic than $Y_{1}^{-}$ species

$K_{a 1}$ is greater than $K'_{a 2}$

$K'_{a 2}$ is greater than $K'_{a 2}$

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Explanation

In the cis isomer, both carboxyl groups are on the same side of the carbon chain, making the negative charges closer. This increases the electrostatic repulsion between the carboxylate anions, making the cis isomer less stable and more acidic than the trans isomer.

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