Question

The electronic configuration of an element x is 1s2 2s2 2p4 and y is 1s2 2s2 2p6 3s2 3p6 4s1 which element is metal?

Answer 1

Answer:

y

Explanation:

because last electron enter in s subshell means it is a member of s block element which are alkali metal

Answer 2

Answer:

The element x with the electronic configuration $1s^{2}2s^{2}2p^{4}$ is Oxygen which is a non-metal and the element y with electronic configuration $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}$ is Potassium which is a metal.

Explanation:

The distribution of electrons in an element's atomic orbitals is described by the element's electron configuration. Atomic electron configurations are represented by a common notation that includes all atomic subshells that include electrons.

The electronic configuration of element x is: $1s^{2}2s^{2}2p^{4}$  

Thus, the total number of electron present in element x = 2 + 2 + 4 = 8

The element x is Oxygen(O) as it has electron number 8.

The electronic configuration of element y is: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}$

Thus, the total number of electron present in element y = 2+2+6+2+6+1

total electron in y = 19

The element y in Potassium(K) as it has electron number 19.

Metals have 1,2 or 3 valence electron while non metals have 4,5,6 or 7 valence electron.  

In electronic configuration of potassium their is one electron in the outermost shell, so it will donate one electron to make it stable. Thus, Potassium is a metal.

Whereas, In the electronic configuration of Oxygen their are 4 electrons present in the outermost shell, so, it will take the four electron from the another element to make it stable. Thus, oxygen is a non-metal.

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