Q. No.The explanation for the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium would be :
| 1. | Pressure and volume |
| 2. | Lustre and brightness |
| 3. | Atomic size and effective nuclear charge |
| 4. | Availability in nature |
Subtopic: Ionization Energy (IE) |
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Level 1: 80%+
Hints
Given below are two statements:
| Assertion (A): | Noble gases have the highest ionization enthalpies in their respective periods. |
| Reason (R): | Noble gases have stable closed-shell electronic configurations. |
| 1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are True and (R) is not the correct explanation of (A). |
| 3. | (A) is True but (R) is False. |
| 4. | Both (A) and (R) are False. |
Subtopic: Ionization Energy (IE) |
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Level 1: 80%+
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Match List-I with List-II
Choose the correct answer from the options given below :
1. A-IV, B-I, C-III, D-II
2. A-II, B-III, C-IV, D-I
3. A-IV, B-I, C-II, D-III
4. A-III, B-IV, C-II, D-I
| List-I | List-II | ||
| (A) | Al3+ < Mg2+ < Na+ < F– | (I) | Ionisation Enthalpy |
| (B) | B < C < O < N | (II) | Metallic character |
| (C) | B < Al < Mg < K | (III) | Electronegativity |
| (D) | Si < P < S < Cl | (IV) | Ionic radii |
1. A-IV, B-I, C-III, D-II
2. A-II, B-III, C-IV, D-I
3. A-IV, B-I, C-II, D-III
4. A-III, B-IV, C-II, D-I
Subtopic: Ionization Energy (IE) | Electronegativity | Atomic Size |
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Level 1: 80%+
JEE
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First ionisation enthalpy of oxygen is less than that of nitrogen because of:
| 1. | More shielding of paired electrons in 2p orbital of oxygen. |
| 2. | Half-filled stable configuration of nitrogen. |
| 3. | More Z effective of oxygen. |
| 4. | Small atomic size of oxygen. |
Subtopic: Ionization Energy (IE) |
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Level 1: 80%+
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Which option contains an inaccurate trend regarding periodic properties?
| 1. | The Electronegativity of elements increases when moving from left to right in the periodic table. |
| 2. | Ionisation enthalpy decreases in a group from top to bottom. |
| 3. | Non-metallic character increases in moving from left to right in a period. |
| 4. | Metallic character increases in moving from left to right in a period. |
Subtopic: Ionization Energy (IE) | Electronegativity | Nature of Compound |
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Which one of the following elements, based on their electronic configurations, has the highest ionization enthalpy?
1.
2.
3.
4.
Subtopic: Ionization Energy (IE) |
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Level 1: 80%+
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Which of these sets represents the correct order of first ionisation potential?
1. K > Na > Li
2. Be > Mg > Ca
3. B > C > N
4. Ge > Si >C
1. K > Na > Li
2. Be > Mg > Ca
3. B > C > N
4. Ge > Si >C
Subtopic: Ionization Energy (IE) |
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The correct order among the following is:
| 1. | \(\mathrm{I^- > I >I^+}\) (Radii) |
| 2. | \(\mathrm{I^- > I > I^+}\) (Ionisation energy) |
| 3. | \(\mathrm{Li^+}\) (aqueous) < \(\mathrm{Na^+}\) (aqueous) < \(\mathrm{K^+}\) (aqueous) (Radii) |
| 4. | \(\mathrm{F > Cl > Br > I}\) (Electron Affinity) |
Subtopic: Ionization Energy (IE) | Electron Affinity (EA) | Atomic Size |
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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
Subtopic: Ionization Energy (IE) |
87%
Level 1: 80%+
Hints
Which of the following configurations corresponds to element of highest ionisation energy?
1. \(1s^2 2s^1\)
2. \(1s^2 2s^22p^3\)
3. \(1s^2 2s^22p^2\)
4. \(1s^2, 2s^2,2p^6,3s^1\)
1. \(1s^2 2s^1\)
2. \(1s^2 2s^22p^3\)
3. \(1s^2 2s^22p^2\)
4. \(1s^2, 2s^2,2p^6,3s^1\)
Subtopic: Ionization Energy (IE) |
87%
Level 1: 80%+
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