Question

Consider the electron configuration. A box holds an up and a down arrow. A box holds an up and a down arrow. A box holds an up and a down arrow.A box holds an up and a down arrow.A box holds an up and a down arrow. A box holds an up and a down arrow. A box holds an up and a down arrow.A box holds an up and a down arrow.A box holds an up arrow. 1s 2s 2p 3s 3p Which element has this electron configuration?

Answer 1

Answer:

The Argon ($Ar$) has this electron configuration.

Explanation:

The question is wrong. The correct electron configuration is :

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$

The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.

The letters s,p,d and f are called the orbitals.

The numbers 1,2,3,4,5,6 and 7 are called the levels.

The maximum numbers of electrons that the s-orbital can hold is 2 electrons.

The maximum numbers of electrons that the p-orbital can hold is 6 electrons.

The maximum numbers of electrons that the d-orbital can hold is 10 electrons.

The maximum numbers of electrons that the f-orbital can hold is 14 electrons.

The order in which the orbitals are filled is :

1s-2s-2p-3s-3p-4s-3d-4p-5s-4d-5p-6s-4f-5d-6p-7s-5f-6d-7p-6f-7d-7f

To identify the electron configuration of an element we need to count and sum the exponents of its orbitals.

The electron configuration is :

$1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$

Has the following sum of exponents : $2+2+6+2+6=18$

Therefore the total electrons of the element is 18 electrons.

The element that has 18 electrons is Argon ($Ar$)