sp

s${\mathrm{p}}^2$

s${\mathrm{p}}^3$

ds${\mathrm{p}}^2$

Diamond

Graphite

3 Fullerenes

Coal

CO₂ can be prepared by the action of dilute hydrochloric acid on calcium carbonate. 

 CO is prepared by the dehydration of formic acid with conc. H₂SO₄. 

 CO₂ is commercially prepared by passing steam over hot coke. 

 CO is commercially prepared by passing steam over hot coke. 

 ${\mathrm{NaAlO}}_2$

 $\mathrm{Na}\left({\mathrm{Al}}_2{\mathrm{O}}_3\right)$

 ${\mathrm{NaAl}}_2\mathrm{O}$

Both (2) and (3)

 ${\mathrm{SiO}}_2 +\hspace{0.17em}4\mathrm{HF} \to {\mathrm{SiF}}_{4 }+ 2{\mathrm{H}}_2\mathrm{O}$

 $\mathrm{ZnO} + \mathrm{CO} \to \mathrm{Zn} +\hspace{0.17em}{\mathrm{CO}}_2$

 ${\mathrm{SiF}}_4 \hspace{0.17em}+ 2\mathrm{HF} \to {\mathrm{H}}_2{\mathrm{SiF}}_6$

All of the above

 Allotropy is the existence of an element in more than one form.

Allotropes have the same chemical properties but different physical properties.

Diamond and graphite are allotropes of carbon.

None of the above.

Thallium displays both +1, and +3 oxidation states.

It resembles group 1 metals in some reactions.

Thallium only shows a +1 oxidation state.

Both (1) and (2) 

Inert pair effect is because of the poor shielding of the ns² electrons by the d- and f- electrons.

 Allotropy is the existence of an element in more than one form.

Catenation is the bonding of atoms of the same element into a series, called a chain.

None of the above.

 ${\mathrm{Na}}_{}{\mathrm{BO}}_2$

 ${\mathrm{B}}_2{\mathrm{O}}_3$

 ${\mathrm{Na}}_2{\mathrm{O}}_2$

Both (1) and (2)

Diborane has two 3c-2e^- bonds.

Boric acid has a layered structure.

Four 2c-2e^- bonds are present in diborane.

All of the above

  Conc. HNO₃ can be transported in an aluminium container.

 Diamond is used as an abrasive.

 A mixture of dilute NaOH and aluminium pieces is used to declog the drain.

 Graphite can't be used as a lubricant.

 Hydrogen fluoride (HF) is a covalent compound and has very strong intermolecular hydrogen bonding.

Sodium fluoride (NaF) is an ionic compound and free F^- is available.

Both (1) and (2) 

None of the above.

 $\mathrm{Na}\left[{\mathrm{BF}}_4\right]$

 ${\mathrm{Na}}_2\left[{\mathrm{BF}}_4\right]$

 $\mathrm{Na}{\left[{\mathrm{BF}}_4\right]}_2$

None of the above 

Lead (II) reacts with Cl₂ to give PbCl₄

 Lead (IV) chloride is highly stable towards heat.

 Lead is not known to form an iodide, PbI₄

Both (1) and (3)

In diamond each carbon is sp² hybridised and in graphite, each carbon is sp³ hybridised.

1. In diamond each carbon is sp² hybridised and in graphite, each carbon is sp³ hybridised.

Graphite has a planar geometry.

Both (2) and (3)

 Tl (+1) is more stable than Tl (+3).

For group 13, the stability of the +3 oxidation state decreases down the group.

 Ge, Sn, and Pb show both the +2 and + 4 states.

None of the above.

Only a is correct

Only b is correct

Both a and b are correct

None of the above

Only iii

i, ii

ii, iii

Only ii

They have  high thermal stability, and high dielectric strength

They are used in surgical and cosmetic plant

It has  (R₂SiO) as a repeating unit

They are hydrophophilic(water loving) in nature.