What is the relationship between the trend in ionization energy and the trend in

Question

What is the relationship between the trend in ionization energy and the trend in atomic radius? Why does this relationship exist? How does the first ionization energy of the following elements compare? Which is higher? Se and Br Cl and l Ca and As Sr and Rb Where in the periodic table are the elements with the greatest electronegativity? Where are those with the least electronegativity? How does electronegativity change from left to right across a period, or row, in the periodic table? How does electronegativity change from top to bottom down a group, family or column in the periodic table? How does the electronegativity of the following elements compare? Which is higher? Se and Br Cl and I Ca and As Sr and Rb

Explanation / Answer

1) Ionisation energy is inversely proportional to the atomic radius. Larger is the atomic radius, farther are the electrons from the nucleus and less is the attraction between nucleus and valence electrons. These electrons can be easily removed. Hence, they have low ionisation energy.

2) a. Br > Se In a period, on going from left to right, the ionisation energy increases.

b Cl > I. In a group, on moving from top to bottom, the ionisation energy decreases.

c. Ca < As

d. Sr > Rb

3) The elements with the greatest electronegativity are halogens belonging to group VII A or group 17.

The elements with least electronegativity are alkali metals belonging to group I A or 1.

4) In a period, the electronegativity increases from left to right due to increse in nuclear charge.

5) In a group, electronegativity decreases from to to bottom due to increase in atomic size.

6) a, Se < Br

b. Cl > I

c. Ca < As

d. Rb < Sr

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