Question

Consider elemental antimony (Sb).

(a) Based on its position in the periodic table, how many valence electrons should it have? You should not need to do any detailed calculations or write the electron configuration. Further, what block does it belong to (i.e., s, p, d, or f)?

(b) Based on its position in the periodic table, what shell (i.e., n = ?) should the valence electrons be associated with? You should not need to do any detailed calculations or write the electron configuration.

(c) Ok, ok, please write the electron configuration for antimony, both the full version and in the “Noble gas” format.

(d) Please write the orbital diagram for antimony and determine if it is paramagnetic or diamagnetic. Should a sample of pure antimony be attracted or repelled by an applied magnetic field?

(e) What would the effective nuclear charge (Zeff) be for the valence electrons in antimony? Please show your work.

(f) If possible, please answer the following. Would an atom of antimony:

(i) be larger or smaller than silicon?

(ii) be larger or smaller than germanium?

(iii) have a higher or lower first ionization energy compared to nitrogen? (iv) be more or less metallic than iodine?

Answer 1

(a) Sb (z = 51) belongs to 5th period and 15th group. It belongs to p-block and has 5 valence electron (group number - 10).

(b) Period number is the main energy level. Period is 5, hence n = 5.

(c) Electronic configuration (z = 51)

full version noble gas format:

(d) Orbital diagram valence shell is n = 5.

There are 3 unpaired electrons in 5p orbital. Hence Sb is paramagnetic and attracted by an applied magnetic field.

(e) To find the effective nuclear charge rule can be used.

- Write down the electronic configuration as follows.