Trend in Ionisation Enthalpy
Trending Questions
Why do metals have low ionization energy?
Why is there a large increase in ionization energy of the alkali metals?
(Sc, Cr, Cu and Zn)
- Cr<Sc<Cu<Zn
- Sc<Cu<Cr<Zn
- Sc<Cr<Zn<Cu
- Sc<Cr<Cu<Zn
- C > N > O > F
- O > N > F > C
- O > F > N > C
- F > O > N > C
Amongst the elements with following electronic configurations, which one may have the highest ionisation energy? [CBSE AIPMT 2009]
[Ne]3s23p3
[Ne]3s23p2
[Ar]3d10, 4s2, 4p3
[Ne]3s23p1
An element has successive ionization enthalpy as 940, 2080, 3090, 4140, 7030, 7870, 16000 and 19, 500 KJ/mole. To which group of the periodic table does the element belong to?
14
15
16
17
Generally the ionization enthalpy in a period increases but there are some exceptions, the one which is not an exception is?
Be and B
N and O
Mg and Al
Na and Mg
I) |IP1 of ion M2+|>|EA1 of M3+|
(IP = ionization potential, and EA = electron affinity)
II) S>Se>Te>O (order of EA)
III) Li<Be<B<C (order of electronegativity)
IV) Al3+<Mg2+<Na+<F−(order of ionic size)
V) Li+>Na+<K+ (order of hydrated size)
VI) NaCl>MgCl2>AlCl3(order of lattice energy)
- (i) and (v)
- (i), (v) and (ii)
- (i), (v), and (vi)
- (i) and (iii)
Correct orders of 1st I.P. are -
(i) Li < B < Be < C
(ii) O < N < F
(iii) Be < N < Ne
(i), (ii)
(ii), (iii)
(i), (iii)
(i), (ii), (iii)
The element with the highest first ionisation potential is
Boron
Carbon
Nitrogen
Oxygen
- 1s2, 2s2, 2p6, 3s1
- 1s2, 2s2, 2p6, 3s2, 3p1
- 1s2, 2s2, 2p6, 3s2, 3p3
- 1s2, 2s2, 2p6, 3s2
Which of the following represent the correct order of increasing IE1 for Ca, Ba, S, Se and Ar?
S < Se < Ca < Ba < Ar
Ba < Ca < Se < S < Ar
Ca < Ba < S < Se < Ar
Ca < S < Ba < Se < Ar
- Na, Mg, Al, Si, P and S
- Na, Al, Mg, Si, S and P
- Mg, Na, Si, Al, P and S
- Na, Si, Mg, S, Al and P
- The hydration energy of sodium sulphate is more than its lattice energy
- The lattice energy of barium sulphate is more than is hydration energy
- The lattice energy has no role to play in solubility
- The hydration energy of sodium sulphate is less than its lattice energy
Which of the following is the only CORRECT combination?
- A-S; B-R; C-P; D-Q
- A-S; B-Q; C-Q; D-P
- A-R; B-S; C-Q; D-P
- A-P; B-Q; C-R; D-S
In halogens, with the increase of atomic number ...
Tendency to loose electrons decreases
Ionic radii decreases
Ionization potential decreases
- In MX2 (M = metal and X = halogen), covalent nature decreases.
Which of the following is the only CORRECT combination?
- A-S; B-R; C-P; D-Q
- A-S; B-Q; C-Q; D-P
- A-R; B-S; C-Q; D-P
- A-P; B-Q; C-R; D-S
Which of the following does not increase on moving down a group?
Atomic radius
Metallic character
Valence Electrons
Shells in atoms
- N>O
- Be>B
- C>B
- All of the above
Column I | Column II | ||
P | 11 | 1 | IE is maximum among the given elements |
Q | 19 | 2 | Alkali metal |
R | 37 | 3 | Largest size among the given elements |
S | 55 | 4 | Position next to Kr |
- P−1:Q−1, 2:R−1, 2:S−3, 4
- P−1, 2:Q−2, 4:R−2, 4:S−2, 3
- P−1, 2:Q−2, :R−2, 4:S−2, 3
- P−2, 3:Q−1, 2:R−2, 4:S−2, 3
- 1s1
- 1s2, 2s22p6
- 1s2, 2s22p6, 3s1
- 1s2, 2s22p2
What will be the order of Ist ionisation energy?
Li > Na > K
K > Li > Na
Na > Li > K
Li > K > Na
The factor not affecting ionisation enthalpy is?
Size of atom
Charge in the nucleus
Type of bonding in the crystal lattice
Type of electron involved
Which of the following is the only CORRECT combination?
- A-S; B-R; C-P; D-Q
- A-S; B-Q; C-Q; D-P
- A-R; B-S; C-Q; D-P
- A-P; B-Q; C-R; D-S
- 1s1
- 1s2, 2s22p6
- 1s2, 2s22p6, 3s1
- 1s2, 2s22p2
Which of the following is not the correct increasing order of ionization energy?
Cl−<Ar<K+
Au < Ag < Cu
Cs < Rb < K
K < Ca < Sc
Column I | Column II | ||
P | 11 | 1 | IE is maximum among the given elements |
Q | 19 | 2 | Alkali metal |
R | 37 | 3 | Largest size among the given elements |
S | 55 | 4 | Position next to Kr |
- P−1:Q−1, 2:R−1, 2:S−3, 4
- P−1, 2:Q−2, 4:R−2, 4:S−2, 3
- P−1, 2:Q−2, :R−2, 4:S−2, 3
- P−2, 3:Q−1, 2:R−2, 4:S−2, 3
Which of the following represent the correct order of increasing IE1 for Ca, Ba, S, Se and Ar?
S < Se < Ca < Ba < Ar
Ba < Ca < Se < S < Ar
Ca < Ba < S < Se < Ar
Ca < S < Ba < Se < Ar