Ionization Enthalpy

Q. Fill in the blanks from the choices given in brackets:
(i) The energy required to remove an electron from a neutral isolated gaseous atom and convert it into a positively charged gaseous ion is called _______________. (electron affinity, ionisation potential, electronegativity)
(ii) The compound that does not have a lone pair of electrons is _______________. (water, ammonia, carbon tetra chloride)
(iii) When a metallic oxide is dissolved in water, the solution formed has a high concentration of _______________ ions. ($H^{+}.H_3{O}^{+},O{H}^{-}$)
(iv) Potassium sulphite on reacting with hydrochloric acid releases ______________ gas. ($C{l}_2,S{O}_2,H_{2}S$)
(v) The compound formed when ethene reacts with Hydrogen is _______________. ($C{H}_4,C_2{H}_6,C_3{H}_8$)

Q.

Which of the following statement is not correct about the periodic classification of elements?

1. The properties of elements are the periodic functions of their atomic numbers

2. Non-metallic elements are lesser in number than metallic elements

3. The first ionization energies along a period do not vary in a regular manner with increase in atomic number

4. For transition elements, the sub-shells are filled with electrons monotonically with increase in atomic number

Q.

The factor not affecting ionisation enthalpy is?

1. Size of atom

2. Charge in the nucleus

3. Type of electron involved

4. Type of bonding in the crystal lattice

Q.

Generally the ionization enthalpy in a period increases but there are some exceptions, the one which is not an exception is?

1. Be and B

2. N and O

3. Na and Mg

4. Mg and Al

Q. Choose the correct order of second ionization enthalpy:

1. O > F > N > C
2. F > O > N > C
3. C > N > O > F
4. O > N > F C

Q. Choose correct order of increasing ionization enthalpy.

1. P < S < As
2. As < S < P
3. As < P < S
4. S < P < As

Q.

Which of the following configurations represent atoms of the elements having the highest second ionization energy?

1. 

2. 

3. 

4. 

Q.

The second ionization potential of an element M is the energy required to

1. Remove one mole of electron from one mole of gaseous anion

2. Remove 2 moles of electrons from one mole of gaseous atoms

3. Remove one mole of electron from one mole of gaseous cation of the element

4. Remove one mole of electron from one mole of monovalent gaseous cation of the element

Q.

On moving across a period, the atomic size decreases and nuclear charge increases and therefore the force of attraction exerted by the nucleus on the electron in the outermost shell increases.
Potassium forms $K^{+}$ ion but it does not form $K^{2+}$ because of;

1. Low value of $(I.E.{)}_1$ and high value of $(I.E.{)}_2$

2. Very low value of $(I.E.{)}_{1}and(I.E.{)}_2$

3. Very high value of $(I.E.{)}_{1}and(I.E.{)}_2$

4. Low value of $(I.E.{)}_1$ and low value of $(I.E.{)}_2$

Q. An element has successive ionization enthalpies as $1^{st}$ (940), 2080, 3090, 4140, 7030, 7870, 16000 and 19500 kJ $mo{l}^{-1}$^. To which group of the periodic table does this element belong?

1. 14
2. 15
3. 16
4. 17