Question

Use the periodic table to write electron configurations for each of the following elements. Represent core electrons with the symbol of the previous noble gas in brackets.

a)S

Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.

B)Se

Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.

C)Sr

Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.

D) I

Express your answer in condensed form in order of increasing orbital energy as a string without blank space between orbitals. For example, [He]2s22p2 should be entered as [He]2s^22p^2.

Answer 1

(a) Atomic Number of S = 16

Closest Noble Gas to S is Ne  (Atomic number of Ne is 10)

No. electrons remaining = 16 - 10 = 6

Configuration: [Ne]3s²3p⁴.

(b) Atomic Number of Se = 34

Closest Noble Gas to Se is Ar (Atomic number of Ar is 18)

No. of electrons remaining = 34 - 18 = 16

Configuration: [Ar] 3d¹⁰4s²4p⁴  

(c) Atomic Number of Sr = 38

Closest noble gas to Sr is Kr (Atomic number of Kr is 36)

No. of electrons remaning = 38 - 36 = 2

Configuration: [Kr]5s²

(d) Atomic Number of I = 53

Closest noble gas to I is Kr (Atomic number of Kr is 36)

No. of electrons remaining = 53 - 36 = 17

Configuration: [Kr]5s²4d¹⁰5p⁵