Question

Along the period, which one of the following decreases:(a)Atomic radius(b) ionization energy(c)Electron affinity(d) electronegativity

Answer 1

Answer:

(a) is the correct answer

Explanation:

because effective nuclear charge increases

Answer 2

Answer:

The atomic radii decrease from left to right along a period.

Explanation:

(a) A decrease in atomic radii is observed from left to all along a period. This is often because, within a period, the electron is added to the identical valence shell. Since the effective nuclear charge increases, the outer electron is held by the nucleus more tightly, resulting in a decrease in the radii.

(b) The ionisation energy increases with an increase in atomic number across a period. This is often because the increase in the nuclear charge overweighs the shielding effect across a period.

(c) Since the dimensions decrease on moving from left to right, the added electron on the average will be closer to the nucleus. Thus,  across a period the electron affinity increases.

(d) On moving from left to right across a period, because the effective nuclear charge increases and size decreases. The electronegativity increases due to an increase in the attraction between the outer electrons and the nucleus.

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