Question

Write the electronic configuration of copper.(Atomic number $C_{u} =29$)

Answer 1

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Atomic Number of Copper (Cu) = 29

♣ In case of K, L, M, N shells

✍️ We know that,

K occupy 2 electrons,

L occupy 8 electrons

M occupy 18 electrons

N occupy 18 electrons

✍️ Electronic configuration :-

♦ K - 2

♦L - 8

♦M - 18

♦N - 1

Now,

♣ In case of s,p,d and f shells

✍️ Electronic Configuration :-

1${s}^{2}$ 2${s}^{2}$ 2${p}^{6}$ 3${s}^{2}$ 3${p}^{6}$ 4${s}^{1}$ 3${d}^{10}$

✍️ Now,

the question arises why it's not 4${s}^{2}$ 3${d}^{9}$

✍️It is due to full filled stability which the copper achieves when electron jump to d orbital to achieve full filled stability.

✍️Now this full filled stability is due to two reasons :-

1. Exchange energy in d orbital :-

there are 5 subshell so ten exchanges of electron is possible which imparts much stability to copper hence this process is exothermic in nature.

2. Symmetrical distribution of charge in 3d space also imparts much stability to Cu due full d orbital.

Answer 2

Atomic Number of Copper (Cu) = 29

♣ In case of K, L, M, N shells

✍️ We know that,

K occupy 2 electrons,

L occupy 8 electrons

M occupy 18 electrons

N occupy 18 electrons

✍️ Electronic configuration :-

♦ K - 2

♦L - 8

♦M - 18

♦N - 1

Now,

♣ In case of s,p,d and f shells

✍️ Electronic Configuration :-

1{s}^{2}s2 2{s}^{2}s2 2{p}^{6}p6 3{s}^{2}s2 3{p}^{6}p6 4{s}^{1}s1 3{d}^{10}d10 

✍️ Now,

the question arises why it's not 4{s}^{2}s2 3{d}^{9}d9 

✍️It is due to full filled stability which the copper achieves when electron jump to d orbital to achieve full filled stability.

✍️Now this full filled stability is due to two reasons :-

1. Exchange energy in d orbital :- 

there are 5 subshell so ten exchanges of electron is possible which imparts much stability to copper hence this process is exothermic in nature.

2. Symmetrical distribution of charge in 3d space also imparts much stability to Cu due full d orbital.