Question

Explain in terms of atomic structure, why cesium has a lower first ionization energy than rubidium. Determine the family/group in which each element is located

Answer 1

Explanation:

The ionization energy is the energy required to remove electrons in an atom. The valence electrons are the easiest to remove and they require little energy compared to inner electrons.

A lot of factors are responsible for the different values of ionization energy. The outermost electrons in a shell are most loosely held and they require little energy to be removed. This is the first ionization energy.

Some factors determines ionization energy:

• Nuclear charge is directly proportional to ionization energy
• Atomic radius - the larger the radius of an atom, the smaller the I.E because of the increased shielding/screening effect of inner shell electrons on the electron to be removed from the nuclear attraction.
• The more penetrating into the nucleus, a sublevel accommodating the electron is the higher the I.E.

From this, we see why Cesium has a lower first ionization energy than rubidium.

Cesium has a higher atomic radius compared to rubidium.

Both elements belong to Group I called the alkali metals.

Learn more:

Alkali metals brainly.com/question/6324347

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