1. (02.04 MC) An atom's electron configuration ends with 3p². If another atom has elght more electrons, what would be the continuation of the electron configuration? (5 points)

Considering the electronic configuration, the electronic configuration of the element with 8 more electrons is:  3p⁶ 4s² 3d²

The Electronic Configuration of the elements is the arrangement of all electrons of an element in energy levels and sub-levels (orbitals).  

There are 7 energy levels, in which electrons are distributed, logically in order according to their energy level.

Each level is divided into sub-levels. These sub-levels into which each level is divided can be up to 4. These 4 sub-levels are called: s, p, d, f.

In the sub-level s there can only be a maximum of 2 electrons, in sub-level p there can be a maximum of 6 electrons, in the sub-level d 10 electrons and finally in the sub-level f there can be a maximum of 14 electrons.

In level 1 there is only 1 sub-level, which will be the s. In level 2 there are 2 sub-levels, the s and the p. At level 3 there are 3 sub-levels: s, p and d. And at level 4 there are 4 sub-levels, the s, the p, the d and the f.

Aufbau's principle is a principle of atomic physics, which explains how electrons are accommodated in their orbits around the nucleus of the atom. This principle states that the filling of these orbitals occurs in increasing order of energy, that is, from the orbitals of lower energy to those of higher energy.

In this case, the electronic configuration of the element ends with 3p².  Another element having 8 more electrons.

In first place, you need to complete the 3p orbital by adding 4 electrons:

3p² + 4 electrons = 3p⁶

Then, you need to fill the 4s orbital with 2 electrons. This is so because 4s has a lower energy level compared to 3d.

4s²

Finally, you fill the 3d orbital with the remaining 2 electrons.

3d²

In summary , the electronic configuration of the element with 8 more electrons is:  3p⁶ 4s² 3d²

Learn more about electronic configuration:

3p⁶ 4s² 3d²

Explanation:

From the question given above,

The electronic configuration of the element ends with 3p².

Another element having 8 more electrons will have the following electronic configuration as illustrated below:

Step 1:

Complete the 3p orbital by adding 4 electrons:

3p² + 4 electrons = 3p⁶

Step 2:

Fill the 4s orbital. This is so because 4s has a lower energy level compared to 3d.

4s²

Step 3:

Fill the 3d orbital with the remaining electrons i.e 2

3d²

Summary:

The continuation of the electronic configuration of the element with 8 more electrons is:

3p⁶ 4s² 3d²

8 carbon atoms forming single bonds with 18 hydrogen atoms; a triple bond exists between the third and fourth carbon atom from the right

explanation:

first one is the correct answer