JEE Questions for Chemistry Chemical Bonding And Molecular Structure Quiz 13 - MCQExams.com

In (c), each C and O atom has octet of electrons.

C₂H₂ has linear structure.

Electronic configuration of Cu²⁺ is

The overlap between s – and p –orbitals occurs along internuclear axis and hence the angle is 180º.

Metallic bonds have electrostatic attraction on all sides and hence do not have directional characteristics.

BeF₂ is linear and hence has zero dipole moment while H₂O, being a bent molecule, has a finite or non-zero dipole moment.

PCl₃ has 3 bond pairs and one lone pair, therefore, in accordance with VSEPR theory , it has pyramidal shape .

Only O₂ ^-(2 × 8 + 1 = 7 ) has old number of electrons and hence is paramagnetic . All the remaining molecules/ ions, i.e, CN^- (6 + 7 + 1 = 4),CO(6 + 8 = 14) and NO⁺ (7 +8 - 1 = 14)have even number of electrons which are paired and hence are diamagnetic.

BF₃ is triangular planar and hence has zero dipole moment.

According to VSEPR theory, a molecule with six bond pairs must be octahedral.

A σ - bond is stronger than a π-bond hence option (a) is not correct.

H₂O shows maximum hydrogen bonding because each H₂O molecule is linked to four H₂O molecules through hydrogen bond.

All bond angles in CCl4 are of 109º 28’.

CO₂ has sp-hybridization and is linear. SO₂ and CO₃²⁻are planar (sp²) while SO₄^2- is tetrahedral (sp³).

For compounds containing ions of same charge, lattice energy increases as the size the ions decrease. Thus, NaF has highest lattice energy.

Electronegativity difference (EN) is highest in RbCl (3 – 0.8 = 2.2) and least in BeCl₂ (3 - 1.5 =1.5) and hence option (b) is correct.

NH₃ has much higher b.p than PH₃ due to H-bonding .

Element (X) of group VA (or 15) has a normal valency of three while element (Y) of group VIA (or 16) has a normal valency of 2. Therefore, the formula of the compound is X₂Y₃.

Electrostatic forces of attraction are reduced to 1/80^th in water

BH₃ has sp² - hybridization and hence does not have tetrahedral structure while all others have tetrahedral structures.

H- bond is the weakest.

The stability of the ionic bond depends upon the lattice energy which is expected to be more between Mg and F due to +2 charge on MG atom.

Chemical bonds.

The C-C bond distance decreases as the multiplicity of the bond increases. Thus, bond distance decreases in the order :butane (1.54Å) > benzene (1.39 Å) > ethene ( 1.34 Å) >ethyne ( 1.20 Å).