Covalent Bonds

Chapter 5 Section 3

Covalent Bonds

Remember…covalent bonds form between two nonmetals

The bonds form when electrons are shared between atoms, not transferred

This happens because neither atom will take the electrons from the other, they attract them at the same time.

Single Bonds

Ionic compounds only form single bonds when there are a pair of electrons between atoms

This molecule has 5 single bonds

Single and Double/Triple Bonds

Covalent (molecular) compounds can form single, double, and triple bonds

Each bond has a pair of electrons between atoms

Single and Double/Triple Bonds

Covalent Bonds

The electrons are sometimes shared equally when the same element bonds with itself (BrINClHOF). This is called a nonpolar bond.

Sometimes they are shared unequally when one atom is slightly stronger than the other. This is called a polar bond.

Covalent Bonds

Properties of Molecular Compounds

Some form crystal shapes, most do notLow melting points compared to ionic

compoundsDo not conduct electricity in solution

(dissolved in water)

Writing Covalent Formulas

Use the same procedure as for ionic formulas

Example: C Br C4+ Br1-

CBr4

Example: N S N5+ S2-

N2S5

Naming Covalent Formulas

Use the same procedure as for ionic formulas

Add Latin prefix that matches the subscript for the element to each part of formula name1= mono 6= hexa

2= di 7= hepta

3= tri 8= octa

4= tetra 9= nona

5= penta 10= deca

Naming Covalent Formulas

Example: CBr4

Carbon tetrabromideN2S5

Dinitrogen pentasulfideH2O

Dihydrogen monoxideCO2

Carbon dioxide