Question

The atomic radius of germanium (Z = 32) is smaller than the atomic radius of potassium (Z = 19) because of:

A. a change in the n quantum number.
B. an increase in the effective nuclear charge.
C. the fact that p and d orbitals have the same orbital penetration.
D. a decrease in the effective nuclear charge.
E. germanium having 32 rather than 19 electrons.

Answer 1

The atomic radius of germanium (Z = 32) is smaller than the atomic radius of potassium (Z = 19) due to an increase in the effective nuclear charge.

Step-by-step explanation:

The atomic radius of germanium (Z = 32) is smaller than the atomic radius of potassium (Z = 19) because of B. an increase in the effective nuclear charge.

As we move across a period from left to right in the periodic table, each element generally has a smaller covalent radius than the element preceding it. This is due to the concept of effective nuclear charge, which is the pull exerted on a specific electron by the nucleus, taking into account electron-electron repulsions. For all other atoms, the inner electrons partially shield the outer electrons from the pull of the nucleus, resulting in an increase in the effective nuclear charge. As a result, the atomic radius of germanium is smaller than that of potassium.

Answer 2

The atomic radius of germanium is smaller than the atomic radius of potassium due to an increase in the effective nuclear charge.

Step-by-step explanation:

The atomic radius of germanium (Z = 32) is smaller than the atomic radius of potassium (Z = 19) because of an increase in the effective nuclear charge, option B. As we move across a period from left to right, each element has a smaller covalent radius. This can be explained by the concept of effective nuclear charge, where the inner electrons partially shield the outer electrons from the pull of the nucleus. The greater the effective nuclear charge, the more strongly the outermost electrons are attracted to the nucleus and the smaller the atomic radius.