Match the following

	Column I (molecules)		Column II ( number of lone pair on central atom)
A	NH3	1	Three
B	H2O	2	Two
C	XeF2	3	Zero
D	CH4	4	Four
		5	One

• A B C D

  5 1 3 2

• A B C D

  3 1 2 5

• A B C D

  5 1 2 3

• A B C D

  1 5 3 4

Identify the order in which the spin only magnetic moment (in BM) increases for the following four ions

(I) Fe²⁺

(II) Ti²⁺

(III) Cu²⁺

(IV) V²⁺

• I, II, IV, III

• IV, I, II, III

• III, IV, I, II

• III, II, IV, I

The formal charges of N₍₁₎, N₍₂₎ and O atoms in the following figure are respectively

• +1, -1, 0

• -1, +1, 0

• +1, +1, 0

• -1, -1, 0

In which of the following pairs, the central atoms have the same number of lone pairs of electrons?

• PCl₅, BrF₅

• XeF₂, ICl

• XeF₄, ClO${}_4^{-}$

• SCl₄, CH₄

Identify the correct set.

• Molecule	Hybridisation of central atom	Shape
  PCl5	dsp3	square pyramidal

• [Ni(CN)4]2-

  sp3

  tetrahedral

• SF6

  sp3d2

  octahedral

• IF3

  dsp3

  pyramidal

Which one of the following statements is correct?

• Hybrid orbitals do not form σ bonds.

• Lateral overlap of p-orbitals or p- and d-orbitals produces $\mathrm{\pi }$-bonds.

• The strength of bonds follows the order-

  σ_p-p < σ_s-s < $\mathrm{\pi }$_p-p

• s-orbitals do not form σ bonds.

The formal charges of C and O atoms in CO₂ ( :Ö= C=:Ö) are respectively

• 1, -1

• -1,1

• 2,-2

• 0,0

According to molecular orbital theory, the total number of bonding electron pairs in O₂ is

• 2

• 3

• 5

• 4

469.

Which of the following does not have triple bond between the atoms?

• N₂

• CO

• NO

• C${}_2^{2-}$

In which one of the following pairs the two species have identical shape, but differ in hybridisation?

• I${}_3^{-}$, BeCl₂

• NH₃, BF₃

• XeF₂, I${}_3^{-}$

• NH${}_4^{+}$, SF₄