Question

Which of the following has maximum ionization energy
(a) Ba → Ba⁺ + e⁻ (b) Be → Be⁺ + e⁻
(c) Ca → Ca²⁺ + 2e⁻ (d) Mg → Mg²⁺ + 2e⁻

Answer 1

The following has maximum ionization energy

(b) Be → Be⁺ + e⁻ i.e., Be

1. As we move down a group in the periodic table, the ionization energy decreases due to increase in size and decrease in effective nuclear charge.

2. Among the Group 2 elements there is no anomaly in the ionization energy trend.

3. Thus, Be has the highest ionization enthalpy among the group 2 elements with smallest size and highest effective nuclear charge.

Answer 2

Be → Be⁺ + e⁻ has the highest ionization energy.

Explanation:

• Ionisation enthalpy is defined as the amount of energy given to an atom to emit an electron and become a single charged cation.

• As the size of an atom increase, the electron in the outer shell of the atom is less attracted by the nucleus.

• So less energy is needed to bring an electron out of the atom.

• Thus the ionization energy decrease as we go down a group.

• Here among the options, elements of group 2 are mentioned.

• No anomaly is seen in the ionisation energy of the group 2 elements.

• Beryllium being the smallest of all of them, will have the highest ionization energy.

For more information about ionisation energy,

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Which one has more ionization energy in nitrogen and oxygen atoms​

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Define ionization energy. Name the

factors on which ionisation energy

depends? How does it vary down the

group and across a period?​