Question

Identify the atom represented by this electron configuration and elaborate on its bonding properties.

1s22s22p63s23p64s23d5

A) .Chromium is a transition with a half full-valence orbital and can form up to six bonds. B) Antimony is a metalloid that can form five covalent bonds or three metallic bonds. C) Manganese is a transition metal that can form up to five stable ionic bonds D) Bromine is a non-metal that forms one ionic bond or a variable number of covalent bonds.

Answer 1

Answer:
The given electronic configuration represents Manganese.

Step-by-step explanation:
The given electronic configuration is....

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d⁵

As the valence shell is 4 in electronic configuration so it is present in 4rth period in periodic table. And according to definition of transition elements, transition elements has partially filled d-orbital. i.e.

(n - 1)d
As, n = 4
So,
(4 - 1)d

3d

So tracking 4rth period, we found Mn with given electronic configuration.
Also,
"Manganese is a transition metal that can form up to five stable ionic bonds". It means that the five electrons present in d-orbital are transferred and Mn converts into Mn⁺⁵.