Test: Chemical Bonding & Molecular Structure - 1 - NEET MCQ

Only in CH₃CH₂OH, carbon has sp³ hybridisation. In other molecules, the carbon atom has multiple bonds.

The bond order of given molecules are:
NO = 2.5, NO⁺ = 3, O₂ = 2, NO^– = 2
Larger the bond order, the smaller the bond length.
NO⁺ has the largest bond order 3.
Therefore, it will have the smallest bond length.
Hence option A is the answer.

The correct option is D.

• The proportion of covalent character in ionic bond is decided by polarisability of the metal cation as well as the electronegativity of both the elements involved in bonding.
• Polarisability is also decided by the density of +ve charge on the metal cation. 
• AlCl3 shows maximum covalent character. This is because Al cation has 3 unit +ve charge and shows strong tendency to distort the electron cloud

• In NO₃, the central N atom has 3 bonding domains and zero lone pairs of electrons.
• In NO₂, the central N atom has 2 bonding domains and zero lone pairs of electrons.
• In NH₄, the central N atom has 4 bonding domains and zero lone pairs of electrons.
• The Hybridization of N atom in NO₃^–, NO₂⁺, NH₄⁺ are sp², sp, sp³ respectively.

Hence option A is the answer.

 In NaCl the ions are not free in solid state but they are strongly bonded through electrostatic forces, hence is not a good conductor of electricity in solid state
A canonicalstructure is also known as a resonance structure, i.e. one of possibly more than one contributing structures that combine to produce the true, resonance hybrid structure. The arrangement of atoms remains the same.
Correct option is A and C.

Electron gain enthalpy is the energy released when an electron is gained by an isolated gaseous atom to form an isolated gaseous anion.

In H₂SO₄, S has more than 8 electrons in the valence shell.

CaC₂ can be divided into two ions: Ca²⁺, C₂^2-

• There is a triple bond, between two carbon.
• Among three bonds one is sigma, bond and the remaining two are pi bond.

• The most electronegative element is F. Its atomic number is 9.
• So, the electronic configuration is 2s²2p⁵.

The stability of an ionic bond is directly proportional to lattice energy.

Arrows represent the direction of the dipole moment.

The Lewis structure of NO molecule can be represented as:

• It is observed that the total no. of unbonded electrons is odd.
• Therefore, there must be an incompletely filled subshell.

Thus, NO is paramagnetic in nature.

Bond length is inversely proportional to bond order.

O²⁺₂ has bond highest bond order as electrons are removed from antibonding MO.

Bond order is directly proportional to bond strength. The higher the bond order, the stronger the pull between the two atoms and the shorter the bond length.

Correct order is: C≡O > C=O > C-O

Single bond has higher bond length than multiple bond.

In the BF₃ molecule, the dipole moment is zero because the B-F bonds are oriented at an angle of 120⁰ to one another resulting, all dipoles cancel out each other.

C₂ has 1 double bond, so it is sp² hybridized while C₃ has 2 double bonds so it is sp hybridized.

• The species which have the same number of total electrons will have the same bond order.
• CN⁻ and NO⁺ each have 14 electrons and they will have the same bond order.

Quartz/silica have extended covalent bond network.

Due to the presence of two lone pairs on O in H₂O bond angle reduce to 104º from 109º.
 

The order of Repulsion: lone pair-lone pair > lone pair-bond pair > bond pair-bond pair

Due to the extra lone pair electron, the shape becomes bent.

It will lead to an octahedral structure assuming that there are no unpaired electrons in the central atom. In case there are any , you have to consider the shape that bonding pairs of electrons are in.

so sp³d² hybridization will lead to octahedral geometry.

CO , N₂ and NO⁺ have same number of electrons = 14.

O is more electronegative than N which is more electronegative than C.