Covalent Bonding

Explain why non-metals form covalent bonds instead of ionic bonds.

Covalent bonding is when two non-metal atoms share valence electrons to get an outer electron shell, this is different because both atoms need to obtain a full outer shell

directional → form along a specific axis between atoms
e.g Water H2O, Oxygen O2, Methane CH4

Identify and describe single, double, and triple covalent bonds.

Single bond	two atoms share 1 pair of electron	H2, Cl
Double bond	Two atoms share 2 pairs of electrons	O2, CO2 , H20
Triple Bond	Two atoms share 3 pairs of electron	N2

Compare the properties of covalent and ionic compounds. ← no direct question but needed

Property	Covalent	Ionic

Low melting and boling point	Weak intermolecular forces require little energy to break
non conductors of electricity	No free moving charged particles to carry an electric current in solid, liquid, gaseous states
solubility varies	polar covalents molecules dissolve Non polar molecules do not
Soft/gas at room temp	covalent molecule substances are often gasses/soft solids

Give examples of covalent compounds and their uses.

polar = dissoves

non polar = doesn’t dissolve

Types of substances

Covalent molecular substances: small groups of atoms held together by strong covalent bonds but with weak intermolecular forces( other molecules) e.g water , carbon dioxide, Ammmonia (NH3)

Forces holding molecules together (intramoecular force) are strong

but forces between molecules (intermolecular forces are weak)

Covalent network substances: Large continuous networks of atoms covalnetly bonded, forming very strong structures e.g diamond c, silicon dioxide (SiO2)

Application

medicine fuels and food chemistry

Carbon based molecules form basis of life (DNA, proteins, carbohydrates)

Pharmaceuticals rely on covalent compounds for drug design

Plastics and synthetic materials are made from long chains of covalnet bonds