The electron configuration of an element is shown below. 1s22s22p5

Name the group this element belongs to in the periodic table and explain your answer.

Based on the electron configuration, explain how many electrons it is likely to receive from the atom of another element during the formation of a bond. (10 points)

1. Halogen group.

2. The element will receive 1 electron.

Explanation:

1. The configuration:

1s²

2s² 2p⁵

We have that the last orbital is "p", with 5 electrons, so the element belongs to the block "p" of the periodic table, and since it is p⁵ the group is the halogens. Every block in the periodic table is given by the electron filling in the last orbital:      

Block "s": group of Alkali metals (s¹), Alkaline earth metals (s²).    

Block "p": Triels (p¹), Tetrels (p²), Pnicto­gens (p³), Chal­co­gens (p⁴), Halogens (p⁵) and Noble gases (p⁶).                            

Block "d": Transition metals        

Block "f": Lanthanides and Actinides.

2. During the formation of a bond, the element will receive 1 electron in order to get full valence shell (2s² 2p⁶) and so gain stability for having eight electrons in their outermost shell (octet rule).  

I hope it helps you!

your answer is a. the enthalpy of formation for a pure element in its standard state is always positive.

catya your not at all which answer i've seen you do this on another question!