An element X has atomic number 13 A. Write its electronic configurationB. State the group to which X belongsC. Is X a metal or a non metalD. Write the formula of its bromide

A. The atomic number of an element tells us the number of protons in its nucleus, which is also equal to the number of electrons in a neutral atom. Element X has an atomic number of 13, so its electronic configuration can be written as:

1s² 2s² 2p⁶ 3s² 3p¹

B. Element X belongs to Group 13 (also known as Group IIIA or Group 3) of the periodic table. This group includes elements such as boron, aluminum, gallium, indium, and thallium.

C. Element X, with an atomic number of 13, is a metal. Specifically, it is a post-transition metal and is found in Group 13 of the periodic table.

D. To write the formula of its bromide, we need to determine the charge on element X when it forms an ion by losing or gaining electrons. Since it is a metal in Group 13, it typically loses three electrons to form a 3+ ion. The bromide ion (Br⁻) has a 1- charge. To balance the charges, we need one X³⁺ ion to combine with three Br⁻ ions. Therefore, the formula of its bromide is XBr₃.