AIIMS Chemistry Chemical Bonding And Molecular Structure Class 11 Questions

Which of the following number of lone pair at central atom zero XeO₃, XeO₂F₂, XeO₄, XeO₃F₂, Ba₂XeF₄

The structures of BO₃³⁻ and SO₃²⁻ is shown below.

The formula is A₀.₈O. This means 80 Å atoms are related to 100 Ω atoms. Let’s assume that 'x' atoms of A are available as A²⁺ ion and (80 − x) are available as A³⁺ ion. The value of x can be calculated as: x ײ⁺ (80 − x) − 3 = 100 × 2 2x + 240 − 3x = 200 x = 40 Therefore, the fraction of A atoms can be calculated as:

The F–C bond has σ and π characteristics because of some back-bonding between d-orbital of metal and p-orbital of carbon.

Assertion: For liquid dishwashing non-ionic type of detergent are used: Reason: Remove grease and oil by micelle formation.

NF₃ = 3bp + 1 lp = 4 e⁻ pair And H₂O = 2bp + 2 lp = 4 e⁻ pair. Thus, both NF₃ and H₂O are sp³ hybridized.

According to L.P−L.P > L.P−B.P > B.P−B.P repulsion, the correct order of S−S bond length will be: I > II > III

The dimer is shown below.

Which has least covalent radius.

Which of the following reacts most slowly with nitric acid?

Which of the following is incorrect about cyanogen gas?

Assertion: $\text{I}_2\text{O}_5$ is used to detect $\text{CO}$ Reason: In $\text{I}_2\text{O}_5$, the oxidation number of I is 5.

PCl₅, BrF₅, IF₇

The ion that has sp³d² hybridization for the central atom is:

An equimolar mixture of CO and H₂ is obtained when steam is passed over red hot coke. It is also named as syn gas. The reaction is, H₂O(g) + C → CO + H₂

The electronic configuration of O₂ is, σ1s² σ*1s² σ2s² σ*2s² σ2p² π2p² = π2p² π*2pₓ = π*2pₓ π*2pᵧ. When electron is added in O₂ to form O₂⁻, the added electron goes to π*2pₓ or π*2pᵧ.

Due to similar molecular bonding, the S₂ molecule is paramagnetic like O₂. It has two unpaired electrons in the anti-bonding t₂g orbitals.

Assertion: H₂⁺ and ions have the same bond order. Reason: H₂⁺ is less stable than H₂⁻.

Ionic compounds have high melting and boiling points due to stronger electrostatic force of attraction between oppositely charged ions. Lattice enthalpy is directly proportional to the electrostatic forces among the ions.

Assertion: $\text{SF}_4$ molecule has see-saw geometry. Reason: In $\text{SF}_4$ molecule sulphur has four bond pair and one lone pair.

The shapes of SF₄ and XeF₂ respectively are

The oxygen molecule contain at least one electron in bonding molecular orbital (σ2p). The energy level diagram of O₂ is shown below:

Among the following, the true statements are: I. $\text{PH}_5$ and $\text{BiCl}_5$ do not exist II. $p\pi - d\pi$ is present in $\text{SO}_2$. III. electrons travel with speed of light. IV. $\text{SF}_4$ and $\text{CH}_4$ has same shape. V. $\text{I}_3^+$ has bent shape.

In the following questions a statement of Assertion (A) followed by a statement of Reason (R) is given. Choose the correct answer out of the following choice. Assertion (A) Superoxides of alkali metals are paramagnetic in nature. Reason (R) Superoxide contain the ion which has one unpaired electron.

The shapes of SF₄ and XeF₂ respectively are

Consider the statement I. Bond length in N₂⁺ is 0.02Å greater than in N₂. II. Bond length of NO⁺ is 0.09 Å less than in NO. III. O₂²⁻ has shorter bond length than O₂. Which of the following statements are true?

Total number of antibonding electrons present in O₂ will be

In BF₃, the B – F bond length is 1.30 Å, when BF₃ is allowed to be treated with Me₃N, it forms an adduct, Me₃N→BF₃, the bond length of B – F in the adduct is

Which of the following statement is not true for hydrolysis of XeF₆?

Bleaching powder does not contain

Which of the following ion does not exist?

The dipole moment is minimum in

N⁻N bond length is minimum in

Assertion : ClF₃ has T⁻shape structure. Reason : It has two lone pairs arranged at 180° angle.

Assertion : O₂ is paramagnetic. Reason : It has one unpaired electron.

Assertion: $\text{HC}\equiv\text{C}^-$ is more stable than $\text{H}_2\text{C}=\text{CH}^-$. Reason: $\text{HC}\equiv\text{C}^-$ has more s-character than $\text{H}_2\text{C}=\text{CH}^-$.

In solid ice, oxygen atom is surrounded

Decreasing order of bond angle is

The number of σ- and π-bonds present in pent-4-ene-1-yne is

Assertion : R₃P=O exists but R₃N=O does not exist. Reason : P is more electronegative than N.

The phosphate of a metal has the formula MHPO₄. The formula of its chloride would be

The shape and hybridisation of some xenon oxyfluorides are given. Choose the wrong set.

Assertion: PCl₅ is covalent in gaseous and liquid states but ionic in solid state. Reason: PCl₅ in solid state consists of tetrahedral PCl₄⁺ cation and octahedral PCl₆⁻ anion.

Assertion: Bond energy and bond dissociation energy have identical value for diatomic molecules. Reason: Greater the bond dissociation energy, less reactive is the bond.

KF combines with HF to form KHF₂. This compound contains the species

The molecules having the same hybridization, shape and number of lone pairs of electrons are

Which of the following fluorides has the lowest melting point?

Assertion: Cu(OH)₂ is soluble in NH₄OH but not in NaOH. Reason: Cu(OH)₂ forms a soluble complex with NH₃.

Bond length order is

Which of the following does not contain any coordinate bond?