Question

An element X has a total of 31 nucleons, out of which 16 are neutrons. (a) Write the electronic configuration of an atom of element X (b) Determine the group and period number of element X. (c) Give the formula of the ion formed by element X


give the answer fast please!!!​

Answer 1

Answer:

"The answer is Phosphorus (P) . We will calculate the number of protons (atomic number) of the element."

Answer 2

$\sf Answer$

Lemme tell you, first of all nucleons is the term used for total number of Protons and Neutrons collectively.

Total number of nucleons = 31

Number of Neutrons = 16.

Thus, number of protons = 15

Number of protons = Number of electrons [in case of a neutron atom]

Number of Electrons = 15

Starting with the sub parts -

a) Electronic Configuration = 2,8,5 (Bohr's structure) or 1s²2s²2p⁶3s²3p³ (Quantum model).

b) Group = No. of Valence Electron = 5 Period = No. of energy shells = 3

c) Since, it has total 5 valence electrons in its outermost shell (valence shell) in order to complete its octet it still requires 3 more electrons. Thus, X ^(-3) is the ion formed. '-ve' means it accepts electrons from a metal (donor).