The electron configuration of an element is shown below. 1s22s22p63s23p6 name the group this element belongs to in the periodic table and explain your answer. based on the electron configuration, write one chemical property of this element.

The group that this element belongs in is group 8. The element is Argon. If you add the numbers( the numbers being after the 1s, 2s, 2p, or 3p so 2,2,6,2,6) you would get 18 (sorry if that was confusing i tried to explain it as best as i could). A chemical property of Argon is that it is unreactive since it is a Noble gas.  

Name the group this element belongs to in the periodic table: Argon, whose symbol is Ar.

The Argon is a noble or inert gas.

Explanation:

There are 7 energy levels, numbered from 1 to 7, and in which electrons are distributed. Each level is divided into sub-levels. These sub-levels into which each level is divided can be up to 4 and they are called: s, p, d, f. In the sub-level s there can only be a maximum of 2 electrons, in 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 one 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.

The Electronic Configuration of the elements is the arrangement of all electrons of an element in energy levels and sub-levels (orbitals).  You know the following electron configuration:

1s²2s²2p⁶3s²3p⁶

In the periodic table the elements are arranged so that those with similar chemical properties are located close to each other.

 The column number of an element gives information about its number of valence electrons. That is, all the elements of the same group have the same number of electrons in their last layer, increases from left to right within a row and causes the chemical properties to be very similar.  For example, all the elements of group 13 contain 3 electrons in their outermost layer.

The period that an element occupies coincides with its last electronic layer. That is, an element with five electronic layers will be in the fifth period.

Looking at the previous electronic configuration, it can be seen that the last electronic layer is level 3. This indicates that the element belongs to period 3. On the other hand, it can also be seen that at that level there are 2 electrons in the sublevel and 6 electrons in the sublevel p. Adding these quantities you get that there are 8 electrons in level 3. This indicates that it belongs to group 18.

In summary, the element belongs to group 18 and period 3.  

Looking in the periodic table, you can see that the element that belongs to said group and period is the Argon, whose symbol is Ar.

The octet rule defines the property that atoms have to complete their last energy level with eight electrons to achieve stability. This is achieved by the constitution of chemical bonds.

The atoms of noble gases have completely filled valence layers, with 8 electrons in their last layer. This makes them called inert. Its inert name is due to the lack of reactivity with other elements and comply with the octet rule. This is due to its electronic configuration, because its outermost layer or valence layer is always complete, without the need to share, transfer or receive electrons forming bonds. That is, its outer layer is so stable that the element tends not to react with others except in very specific cases.

This is what happens in this case. Because this element has 8 electrons in its outermost layer, the Argon is a noble or inert gas.

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