Energy of an electron in the ground state of the hydrogen atom is - 2 .18 × 10 - 18 J . Calculate the ionization enthalpy of atomic hydrogen in terms of J mol ‐ 1 .

The energy of an electron in the ground state of the hydrogen atom is - 2 .18 x 10 - 18 J . Therefore, the energy required to remove that electron from the ground state of the hydrogen atom (Ionization enthalpy) = 2 .18 × 10 - 18 J . Hence, ionization enthalpy of atomic hydrogen in terms of J mol - 1 = 2 .18 × 10 - 18 × N A J mol - 1 = 2 .18 × 10 - 18 × 6 .022 × 10 23 J mol - 1 = 1 .31 × 10 6 Jmol - 1 .

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Consider the following species :
$N^{3 -}, O^{2 -}, F^{-}, {Na}^{+}, {Mg}^{2 +} and {Al}^{3 +}$
What is common in them?

Important Questions on Classification of Elements and Periodicity in Properties

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IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 3 - Classification of Elements and Periodicity in Properties>EXERCISES>Q 3.12

Consider the following species :

N^{3 -}, O^{2 -}, F^{-}, {Na}^{+}, {Mg}^{2 +} and {Al}^{3 +}

Arrange them in the order of increasing ionic radii.

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Textbook for Class XI Chemistry Part I>Chapter 3 - Classification of Elements and Periodicity in Properties>EXERCISES>Q 3.13

Explain why cations are smaller and anions larger in radii than their parent atoms?

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Textbook for Class XI Chemistry Part I>Chapter 3 - Classification of Elements and Periodicity in Properties>EXERCISES>Q 3.14

What is the significance of the terms — ‘isolated gaseous atom’ and ‘ground state’ while defining the ionization enthalpy and electron gain enthalpy?

Hint: Requirements for comparison purposes.

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Textbook for Class XI Chemistry Part I>Chapter 3 - Classification of Elements and Periodicity in Properties>EXERCISES>Q 3.15

Energy of an electron in the ground state of the hydrogen atom is

- 2 .18 \times 10^{- 18} J .

Calculate the ionization enthalpy of atomic hydrogen in terms of

J {mol}^{‐ 1} .

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Textbook for Class XI Chemistry Part I>Chapter 3 - Classification of Elements and Periodicity in Properties>EXERCISES>Q 3.16

Among the second period elements the actual ionization enthalpies are in the order

Li < B < Be < C < O < N < F < Ne .

Explain why

Be

has higher

∆_{i} H

than

B

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11th CBSE

IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 3 - Classification of Elements and Periodicity in Properties>EXERCISES>Q 3.16

Among the second period elements the actual ionization enthalpies are in the order

Li < B < Be < C < O < N < F < Ne .

Explain why

O

has lower

∆_{i} H

than

N and F

MEDIUM

11th CBSE

IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 3 - Classification of Elements and Periodicity in Properties>EXERCISES>Q 3.17

How would you explain 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?

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11th CBSE

IMPORTANT

Textbook for Class XI Chemistry Part I>Chapter 3 - Classification of Elements and Periodicity in Properties>EXERCISES>Q 3.18

What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?

Consider the following species : N3-, O2-, F-, Na+, Mg2+ and Al3+ What is common in them?

Important Questions on Classification of Elements and Periodicity in Properties

Learn and Prepare for any exam you want !

Consider the following species :
$N^{3 -}, O^{2 -}, F^{-}, {Na}^{+}, {Mg}^{2 +} and {Al}^{3 +}$
What is common in them?