Consider the following electronic configuration of an element (P) :

$\left[\mathrm{Xe}\right]4f^{14}5d^{1}6s^2$

Then correct statement about element 'P' is :

(1) It belongs to 6th period and the 1st group

(2) It belongs to 6th period and the 2nd group

(3) It belongs to 6th period and the 3rd group

(4) none of these 

Consider the following information about element P and Q :

                        Period number            Group number

P                               2                                 15

Q                               3                                 2

Then formula of the compound formed by P and Q element is :

(1) PQ         

(2) $P_3{Q}_2$           

(3) $P_2{Q}_3$           

(4)$P{Q}_2$

Which of the following properties of the alkaline earth metals increase from Be to Ba?

(i) Atomic radius        (ii) Ionisation energy        (iii) Nuclear charge

(1) (i) and (ii)                                 

(2) (i) and (iii)

(3) (ii) and (iii)                               

(4) (i), (ii) and (iii)

Aqueous solutions of two compounds $M_1-O-H and M_2-O-H$ are prepared in two different beakers. If, the electronegativity of $M_1=3.4 , M_2=1.2, O=3.5 and H=2.1,$ then the nature of two solutions will be respectively:

(a) acidic, basic             (b) acidic, acidic

(c) basic, acidic             (d) basic, basic

The process requiring the absorption of energy is:

1. $F\to F^{-}$

2. $H\to H^{-}$

3. $Cl\to C{l}^{-}$

4. $O\to O^{2-}$

Which of the following sequences accurately represents the correct order?

1. F>N>C>Si>Ga - non-metallic character.

2. F>O>Cl >N - oxidising property.

3. C<Si>P>N - electron affinity value.

4. All of the above.

Which of the following statements is not correct?

1.  The first ionization energy generally decreases from top to bottom within a group

2.  The atomic radius generally increases from top to bottom within a group

3.  The first ionization energy generally decreases from left to right across a period

4.  The second ionization energy of an atom is always greater than the first ionization energy

What is the general trend observed for the first ionization energies of the elements in groups 13to 17?

1.  Ionization energies tend to increase from left to right in a period and are approximately constant in a group

2.  Ionization energies tend to increase from left to right in a period and decrease from top to bottom in a group

3.  Ionization energies tend to decrease from left to right in a period and increase from top to bottom in a group

4.  Ionization energies tend to decrease from left to right a period and decrease from top to bottom in a group

Which of the following pairs of substances are allotropes?

1.  ${\mathrm{CH}}_3{\mathrm{CH}}_2\mathrm{OH} \mathrm{and} {\mathrm{CH}}_3{\mathrm{OCH}}_3$

2.  $\mathrm{Fe}{\left({\mathrm{NO}}_3\right)}_2 \mathrm{and} \mathrm{Fe}{\left({\mathrm{NO}}_3\right)}_3$

3.  NaCl and KCl

4.  ${\mathrm{O}}_2 \mathrm{and} {\mathrm{O}}_3$

 Element 114 is most likely to be a

1.  Reddish-brown volatile liquid

2.  A pale yellow-green gas

3.  A colourless crystal

4.  A grey-silvery metal