Match the following : 

       Oxide         Nature 

(a) CO           (i)  Basic 

(b) BaO         (ii) Neutral 

(c) Al₂O₃          (iii) Acidic 

(d) Cl₂O₇         (iv) Amphoteric 

Which of the follwing is correct option ? 

      a       b       c         d

(1) (ii)    (i)     (iv)     (iii) 

(2) (iii)    (iv)   (i)       (ii) 

(3) (iv)    (iii)   (ii)      (i) 

(4) (i)     (ii)    (iii)     (iv) 

Identify the incorrect match.

   Name         IUPAC Official Name

a. Unnilunium    (i) Mendelevium

b. Unniltrium      (ii) Lawrecium

c. Unnilhexium   (iii) Seaborgium

d. Unununnium   (iv) Darmstadtium

1. (b), (ii)

2. (c), (iii)

3. (d), (iv)

4. (a), (i)

Match the element in column I with that in column II.
     Column-I             Column-II

(a) Copper             (i) Non-metal

(b) Fluorine           (ii) Transition metal

(c) Silicon             (iii) Lanthanoid

(d) Cerium            (iv) Metalloid

Identify the correct match :

(1) (a)-(ii),  (b)-(iv),  (c)-(i),   (d)-(iii)

(2) (a)-(ii),  (b)-(i),    (c)-(iv),  (d)-(iii)

(3) (a)-(iv), (b)-(iii),   (c)-(i),   (d)-(ii)

(4) (a)-(i),   (b)-(ii),   (c)-(iii),   (d)-(iv)

For the second period elements the correct increasing order of first ionisation enthalpy is:

1.  Li<Be<B<C<O<N<F<Ne

2.  Li<Be<B<C<N<O<F<Ne

3.  Li<B<Be<C<O<N<F<Ne

4.  Li<B<Be<C<N<O<F<Ne

In which of the following options the order of arrangement does not agree with the

variation of property indicated against it?

1. B < C < N < O (increasing first ionisation enthalpy)

2. I < Br < F < Cl (increasing electron gain enthalpy)

3. Li < Na < K < Rb (increasing metallic radius)

4. Al³⁺ < Mg²⁺ < Na⁺ <F^- (increasing ionic size)

Which one of the following orders is correct for the bond dissociation enthalpy of halogen

molecules?

1. Cl₂>Br₂>F₂>I₂               

2. Br₂>I₂>F₂>Cl₂

3. F₂>Cl₂>Br₂>I₂               

4. I₂>Br₂>Cl₂>F₂

"Metals are usually not found as nitrates in their ores'"

Out of the following two (I and II) reasons which is/are true for the above observation?

I. Metal nitrates are highly unstable.

II. Metal nitrates are highly soluble in water.

1. I and ll are true 

2. I and II are false

3. I is false but ll is true

4. l is true but ll is tase

The formation of the oxide ion O^2-(g), from oxygen atom requires first an exothermic and

then an endothermic step as shown below,

$$\begin{gathered} \mathrm{O}\left(\mathrm{g}\right) + \mathrm{e}- \stackrel{ }{\to } {\mathrm{O}}^{-}\left(\mathrm{g}\right); {∆}_{\mathrm{f}}\mathrm{H}° = -141{\mathrm{kJmol}}^{-1} \\ {\mathrm{O}}^{-}\left(\mathrm{g}\right) +\hspace{0.17em}{\mathrm{e}}^{-} \stackrel{ }{\to }{\mathrm{O}}^{2-}\left(\mathrm{g}\right); {∆}_{\mathrm{f}}\mathrm{H}° = +780 \mathrm{kJ} {\mathrm{mol}}^{-1} \end{gathered}$$

Thus, process of formation of O^2- in gas phase is unfavourable even though O^2- is

isoelectronic with neon. It is due to the fact that

1. electron repulsion outweighs the stability gained by achieving noble gas configuration

2. O^- ion has comparatively smaller size than oxygen atom

3. Oxygen is more electronegative

4. addition of electron in oxygen result in large size of the ion