Chemical Bonding and Molecular Structure · Chemistry · COMEDK

Identify the pair of molecules in which one of them is a molecule with an odd electron and the other has an expanded octet.

Which of the following two molecular species are Diamagnetic in nature?

$$[\mathrm{A}]=\mathrm{O}_2^{-} \quad[\mathrm{B}] .=\mathrm{N}_2^{+} \quad[\mathrm{C}]=\mathrm{C}_2 \quad[\mathrm{D}]=\mathrm{O}_2{ }^{2-}$$

Choose the incorrect statement from the following:

A. Isoelectronic molecules/ions have the same bond order.

B. Dipole moment of $$\mathrm{NH}_3$$ is greater than that of $$\mathrm{NF}_3$$.

C. The Carbon in Methyl Carbocation is $$\mathrm{sp}^3$$ hybridised.

D. The stability of an ionic compound is measured in terms of its lattice enthalpy and not simply based on attaining Octet configuration.

$$ \text { From the following pair of compounds, identify the incorrect pair in terms of the covalent character. } $$

The bond dissociation enthalpy of the species in their correct order is:

In the following question a statement of Assertion (A) followed by a statement of Reason (R) is given. Choose the correct option out of the choices given below.

Assertion (A): A molecule of $$\mathrm{SF}_4$$ is see-saw shaped, while that of $$\mathrm{CIF}_3$$ is T-shaped.

Reason(R): SF$$_4$$ has two lone pair of electrons. But CIF$$_3$$ has one pair of electrons.

On the basis of VSEPR theory, match the molecules listed in Column I with their shapes given in Column II.

Identify the pair of molecules, both of which have positive values of Dipole moment.

Given below are 4 molecular species/ions. Identify the species/ion which exhibits diamagnetic nature.

$$[\mathrm{A}]=\mathrm{N}_2^{+} \quad[\mathrm{B}]=\mathrm{O}_2^{-} \quad[\mathrm{C}]=\mathrm{B}_2 \quad[\mathrm{D}]=\mathrm{C}_2$$

Which of these represents the correct order of decreasing bond order?

Pick up the correct statement.

Total number of $$\sigma$$ and $$\pi$$ bonds in ethene molecule is

Which of these molecules have non-bonding electron pairs on the cental atom?

$$\mathrm{I}: \mathrm{SF}_4 : \mathrm{II}: \mathrm{ICl}_3 : \mathrm{III}: \mathrm{SO}_2$$

Identify the correct statement describing the characteristics of $$\mathrm{C}_2$$ molecule.

In the following question, Assertion (A) is given followed by a statement of Reason (R). Choose the correct answer.

Assertion (A): $$\pi\left(2 p_x\right), \pi\left(2 p_y\right), \pi^*\left(2 p_x\right), \pi^*\left(2 p_y\right)$$ molecular orbitals have one nodal plane each.

Reason $$(\mathrm{R})$$ : All the molecular orbitals formed by the sideways overlapping have one nodal plane.

Arrange the following in the decreasing order of their Dipole moments.

a. Chlorobenzene

b. 1,2-Dichlorobenzene

c. 1,3-Dichlorobenzene

d. 1,4-Dichlorobenzene.

Which of the following molecules does not exhibit dipole moment?

(i) CCl$$_4$$ (ii) CO$$_2$$ (iii) NH$$_3$$ (iv) CHCl$$_3$$ (v) H$$_2$$O (vi) CH$$_3$$$$-$$O$$-$$CH$$_3$$

Increasing order of bond order of oxygen and its ions is

The P-O bond order in PO$$_4^{3-}$$ is

Which of the following compound does not exists?

Find the correct order of C$$-$$O bond length among CO, CO$$_3^{2-}$$, CO$$_2$$.

Which of the following pairs of ions in iso-electronic and iso-structural?

Find the compound which have both polar and non-polar covalent bonds.

In acetylene molecule, between the carbon atoms there are

During the formation of a chemical bond

For a stable molecule the value of bond order must be

The number of antibonding electron pairs in O$$_2^{2-}$$ molecular ion on the basis of molecular orbital theory is

[Atomic number of O is 18]