The lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group (red). in this representation, each y atom needs 1 electron(s) to complete its octet, and gains these electrons by forming 1 bond(s) with atoms of h . there are 1 unshared electron pair(s) and 1 bonding electron pair(s) in the product molecule. the bonds in the product are .

The molecule has been , where the two bonds have been formed for the sharing of 2 electrons pair between the H and Y atom.

The main group element that has the ability to form type of structure has been Group 16.

The atom required 2 electrons to complete its octet, and in order to gain two electrons, the atom form 2 bonds with the H, resulting in .

The atom forms bond with the two H atoms, thus there has been the presence of two unshared electrons pair. The bonding electrons pair are also two in the molecule.

The bond has been formed with the sharing of the electron pair. Thus it has been a covalent bond.

For more information about the bonds in the molecule, refer to the link:

link

The question is incomplete, the complete question is;

The Lewis representation above depicts a reaction between hydrogen (blue) and a main-group element from group (red).

In this representation, each Y atom needs electron(s) to complete its octet, and gains these electrons by forming bond(s) with atoms of H .

There are unshared electron pair(s) and bonding electron pair(s) in the product molecule.

The bonds in the product are (Ionic or Covalent)

1) 16

2) 2 electrons

3) 2 bonds

4) 2 unshared pairs of electrons

5) 2 bonding pairs of electrons

6) The bonds in the product are covalent

Explanation:

Group sixteen elements have six electrons on their outermost shell. These include two unshared pairs of electrons and two unpaired electrons. These two unpaired electrons can now be covalently bonded to two hydrogen atoms to give H2Y. The compound H2Y has two lone pairs and two bond pairs of electrons.

H2Y can be a general formula for all hydrides of group 16. They are all very similar in structure but gradually differ in physical and chemical properties according to the graduated variation observed down the group.

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.