Which element has this electron configuration [he] 2s22p2

Element: Carbon

Explanation:

Electronic configuration:

The electronic configuration is the arrangement of electrons in orbitals (s, p, d, f, g, h so on) according to quantum number and Aufbau rule.

An atom of element have orbitals, and electrons are revolving in it.

There are quantum numbers that describe the number of electron in specific shell.

According to Aufbau electron occupied in the lowest energy level before occupying the highest energy level.

According to this the electronic configuration is

1s², 2s², 2p⁶ and so on

So,

"s" orbital accommodate maximum of 2 electrons

"p" orbital accommodate maximum of 6 electrons

The 1st orbital is 1s and it only can occupy 2 electrons the next coming electron goes into 2s that also can occupy 2 electrons and the further electrons will go to 2p orbital.

Given electron configuration:

[He], 2s², 2p²

Helium in bracket [He] represent existence of 2 electrons in 1s²

So,

Along counting with 2 electrons as represented by  [He] this show 6 electrons are there in electronic configuration of an element.

As it have its 2 outer most electrons are in the "p" orbital so it belog to P block element.

This configuration also can be written as

1s², 2s², 2p²

In the periodic table as, carbon have atomic number 6 and this element have 6 electrons and have the same electronic configuration.

So, this electronic configuration is for Carbon element.

< > according to newton's third law of motion, forces always act in equal but opposite pairs. another way of saying this is for every action, there is an equal but opposite reaction.< >

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.