Question

The electron configuration of an element is shown below.


`1s^(2) 2s^(2) 2p^(6) 3s^(1)`

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.

Answer 1

The element belongs to Group 1 in the periodic table, also known as the Alkali Metals. One chemical property of this element is its high reactivity with water.

Step-by-step explanation:

The electron configuration of the element is
`1s^(2) 2s^(2) 2p^(6) 3s^(1)`. The element belongs to Group 1 in the periodic table, also known as the Alkali Metals. This is because it has one valence electron in its outermost energy level.

One chemical property of this element is its high reactivity with water. Due to the presence of a single valence electron, it readily loses this electron and forms a positive ion. When this element reacts with water, it produces a strong alkaline solution and releases hydrogen gas.

Answer 2

It is likely to receive one electron from another element's atom during the creation of a bond, based on the electron configuration. The arrangement of electrons in energy levels surrounding an atomic nucleus is termed electronic configuration, or electronic structure.

Fluorine's electron configuration is
`1s^22s^22p^5`

Because fluorine contains seven valence electrons, it is most likely to acquire one to create a 1-charged ion. To complete its octet, it will require one more electron. As a result, the oxidation number is 1, indicating that when fluorine interacts with another atom to form a more stable combination, it will acquire or share one electron. As a result, it is likely to acquire one electron from an atom of another element during the creation of a bond, based on the electron configuration.