Indicate the number of covalent bonds that each nonmetal atom is expected to form.


a. Se is expected to form 2 covalent bonds.


b. H is expected to form 1 covalent bonds.


c. Br is expected to form 1 covalent bonds.


d. N is expected to form 3 covalent bonds.

true.

which one

a. Se is expected to form 2 covalent bonds.

b. H is expected to form 1 covalent bond.

c. Br is expected to form 1 covalent bond.

d. N is expected to form 3 covalent bonds.

To determine the number of covalent bonds that each nonmetal atom is expected to form, you need to consider the valence electrons of the atom. The valence electrons are the electrons in the outermost energy level of an atom.

a. Se (selenium) is in Group 16 of the periodic table, so it has 6 valence electrons. It needs 2 more electrons to complete its octet (8 valence electrons), so it is expected to form 2 covalent bonds.

b. H (hydrogen) is in Group 1 of the periodic table, so it has 1 valence electron. It needs 1 more electron to complete its duet (2 valence electrons), so it is expected to form 1 covalent bond.

c. Br (bromine) is in Group 17 of the periodic table, so it has 7 valence electrons. It needs 1 more electron to complete its octet (8 valence electrons), so it is expected to form 1 covalent bond.

d. N (nitrogen) is in Group 15 of the periodic table, so it has 5 valence electrons. It needs 3 more electrons to complete its octet (8 valence electrons), so it is expected to form 3 covalent bonds.