For each of the following compounds, identify what type of bonding holds them together. Column A
1.
NaCl:
NaCl
2.
Hg:
Hg
3.
CO2:
CO2
4.
CH4:
CH4
5.
Li2O:
Li2O
6.
Ag:
Ag

Column B
a.
ionic
b.
metallic
c.
covalent

Explanation

NaCl:  Ionic crystal lattice forces

Hg:   Metallic bonding

CO₂:  London dispersion forces

CH₄:  London dispersion forces

Li₂O:  Ionic crystal lattice forces

Ag:  Metallic bonds

Ionic crystal lattice forces are strong electrostatic force of attraction between oppositely charged ions arranged into a crystal lattice of ionic compound. NaCl and Li₂O are ionic compounds

London dispersion forces holds the molecules of carbon dioxide and methane. They are weak attractions found between non-polar (and polar) molecules.

Metallic bonds exists between Mercury and Gold atoms. This is due to sea of electrons present.

2b2t

explanation:

2b2t

since electrons are negative the answer is neagtaive