The increasing order of the strength of hydrogen bond in the following mentioned linkages
is

(i) O — H — S     (ii) O — H  — O    (iii) F – H – F   (iv) F – H – O

The boiling point of $CC{l}_4$ is higher than that of $CHC{l}_3$ because :

Assertion : Compounds of ${\mathrm{Hg}}^{2+}$ ions having an ionic radius of 116 pm are move covalent in character

Reason : For two ions of the same size and charge, one with an (n-1)${\mathrm{d}}^{10}{\mathrm{ns}}^0.$ electronic configuration

                 will be more polarizing than a cation with an (n-1)${\mathrm{s}}^2$ (n-1)${\mathrm{p}}^6{\mathrm{ns}}^0,$ electronic configuration.

Assertion : In tetrahedral hybridisation i.e., in ${\mathrm{sp}}^3$ hybridisation all p-orbitals are involved and no

                   p-orbital is left for coming with $\mathrm{\pi }$-bonds.

Reason : Central atom can not form double bonds in the molecules or species having ${\mathrm{sp}}^3$hybridisation.

The enolic form of acetone contains how many $\sigma$ bonds (a), $\mathrm{\pi }$ bonds (b) and lone pairs (c)-

The number of sigma ($\mathrm{\sigma }$) and pi ($\mathrm{\pi }$) bonds in pent-2-en-4-yne is:

Assertion : $\mathrm{C}\mathcal{l}$ F bond angle P = bond angle Q but not precisely $90°.$

Reason : The molecule is slight bent T-shaped and there is repulsion between lone pairs of electrons.

Assertion : ${\mathrm{N}}_2{{\mathrm{F}}_3}^{+}$ is planar at each nitrogen atom.

Reason : ${\mathrm{N}}_3\mathrm{H},$ the bond angle $\mathrm{H}‐\mathrm{N}‐\mathrm{N}$ is $120°$ and both the $\mathrm{N}‐\mathrm{H}$ bond lengths are not equal.

Assertion : Carbon has unique ability to form $\mathrm{p\pi }-\mathrm{p\pi }$ multiple bonds with itself and with other

                  atoms of small size and high electronegativity.

Reason : Heavier elements of group ${14}^{\mathrm{th}}$ do not form $\mathrm{p\pi }-\mathrm{p\pi }$ multiple bonds with itself because

               their atomic orbitals are too large and diffuse to have effective overlapping.

Assertion : ${\mathrm{NO}}^{+}$ and ${\mathrm{CN}}^{-}$ both have same bond order and magnetism

Reason : ${\mathrm{NO}}^{+}$ and ${\mathrm{CN}}^{-}$ are isoelectornic species.

Assertion : Crystals of hydrated calcium sulphate $\left(\mathrm{gypsum} : {\mathrm{CaSO}}_4, 2{\mathrm{H}}_2\mathrm{O}\right)$ are soft and easily cleaved.

Reason : Crystals of anhydrous calcium sulphate $\left(\mathrm{anhydrite} : {\mathrm{CaSO}}_4\right)$ are very hard and very difficult

               to cleave.

 When two atoms combine to form a molecule, energy is:

A compound having the Highest Melting Point :

The diamagnetic species among the following is-

Which of the statements are not true for AlCl₃-

Valency expresses-

Which among the following compounds has a maximum value of lattice energy?

A Compound with maximum ionic character is formed from-

The crystal lattice of electrovalent compound is composed of :

Ions are formed from neutral atoms by-

Most covalent compound among the following is :

The correct order of covalent bond character among LiCl, BeCl₂, BCl₃ and CCl₄, is -

Which follows octet rule-

The type of bonds present in N₂O₅ are-

Which is not true according to VBT-

Which of the following species has a bond angle of 120 °?

$$\begin{gathered} 1. S{F}_6 \\ 2. NC{l}_3 \\ 3. BC{l}_3 \\ 4. P{H}_3 \end{gathered}$$

The hybridisations of atomic orbitals of nitrogen in NO⁺, NO^-₃ and NH₃ respectively are

Which of the following pairs of species have the same bond order?

In which of the following molecules, all atoms are coplanar?

1.  

2.  

3.  

4.  

Among $Ca{H}_2, Be{H}_2, Ba{H}_2$ the order of ionic character is