Chemical bonding & molecular structure practice · Mixed difficulty

The bond formed as a result of the electrostatic attraction between the positive and negative ions is termed as …

The correct order of strength of H-bond

$\mathrm{H} - \mathrm{B} - \mathrm{H}$ bond angle in $\mathrm{BH}_4^ -$ is:

In which of the following molecules/ions $\mathrm{B}{\mathrm{F}_3},\mathrm{NO}_2^ - ,\mathrm{NH}_2^ -$, and ${\mathrm{H}_2}\mathrm{O}$ the central atom is $s{p^2}$ hybridized?

In ${H_2}^ -$ ion, the bond order is

${\mathrm{H}_2}\mathrm{O}$ has a net dipole moment, while $\mathrm{Be}{\mathrm{F}_2}$ has zero dipole moment, because:

The molecule having smallest bond angle is:

Which of the following molecules has three fold axis of symmetry?

Which of the following pairs of compounds is isoelectronic and isostructural?

${NO}^{+}$has bond order

In ${\left[ {Ag{{\left( {CN} \right)}_2}} \right]^{ - 1}}$, the number of $\pi$ -bonds is

Statement-1: The ionic character exist in $H_2$ molecule but no dipole moment or bond moment exists permanently.
Statement-2: It arises so, as the two ionic forms having bond moments in opposite directions contribute equally to nullify the effect.

Which of the following statements are not correct?
A. The electron gain enthalpy of $F$ is more negative than that of $Cl.$
B. Ionization enthalpy decreases in a group of periodic table.
C. The electronegativity of an atom depends upon the atoms bonded to it.
D. $Al_2O_3$ and $NO$ are examples of amphoteric oxides.
Choose the most appropriate answer from the options given below:

The bond energies of $\mathrm{F}_2, \mathrm{Cl}_2, \mathrm{Br}_2$ and $\mathrm{I}_2$ are 155 , 244,193 and $151 \mathrm{~kJ} / \mathrm{mol}$. The weakest bond will be in

Out of the following which has highest dipole moment

Elements whose electronegativities are $1.2$ and $3.0$ form:

When an element of very low ionisation potential is allowed to react with an element of very high electron affinity, we get:

The bond angle between two hybrid orbitalsis 105°. The percentage of s-character of hybrid orbital is between

Suppose that $A$ and $B$ form the compounds $B_2 A_3$ and $B_2 A$. If 0.05 mole of $B_2 A_3$ weighs $9 g$ and 0.1 mole of $B_2 A$ weighs $10 {~g}$, the atomic weight of $A$ and $B$ respectively are

It is thought that atoms combine with each other such that the outermost orbit acquires a stable configuration of $8$ electrons. If stability were attained with $6$ electrons rather than with $8$, what would be the formula of the stable fluoride ions?

The $ICl$ molecule is:

Which of the following has highest bond angle?

Which of the following has covalent bond?

Which of the following species has only $\pi$ bonds according to MOT?

The bond order of $N_2^{+}$on the basis of molecular orbital theory is [At. number of ${N}=$ 7]

In which of the following, unpaired electrons are present? $\mathrm{K}{\mathrm{O}_2},\mathrm{AlO}_2^ - ,\mathrm{Ba}{\mathrm{O}_2},\mathrm{NO}_2^ +$

Each of the followings has non-zero dipole moment, except:

In which of the process the bond order increases and magnetic behaviour changes

${\mathrm{B}_{10}}{\mathrm{C}_2}{\mathrm{H}_{12}}$ is isoelectronic with

Statement-1: $Ag_2S$ is much less soluble in water than $Ag_2O$.

Statement-2: $S^{2-}$ is much larger than $O^{2-}$; so polarization of $S^{2-}$ is higher than $O^{2-}$.