Question

(03.01 MC)

The electron configuration of an element is shown below.
1s²2s²2p63s¹

Identify the group name 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 with the electron configuration 1s²2s²2p⁶3s¹ belongs to the alkali metal group (Group 1) in the periodic table and is highly reactive, especially with water and halogens.

Step-by-step explanation:

1. The electron configuration of an element is 1s²2s²2p⁶3s¹, which corresponds to the element sodium (Na).
2. This configuration indicates that sodium has one electron in its outermost 3s subshell. Therefore, it belongs to the alkali metal group (Group 1) in the periodic table. In Group 1 of the periodic table, all elements have a single valence electron, which they can easily lose to form a +1 ion, thus exhibiting similar chemical properties.
3. One distinct chemical property of an element with this electron configuration is its high reactivity, particularly with water, to form hydrogen gas and hydroxides. Alkali metals are known for their tendency to undergo exothermic reactions with water and halogens.