#1 Basic Principles & HydroCarbons

Organic Compounds

• Soluble in organic solvents – CCl4

• Nonpolar

• Molecules

• Covalent bonds

• Highly flammable

• Insoluble in water (unless a polar group is present)

• Low boiling point and low melting point

• C, H, N, O, S, P, X = F, Cl, Br, I (halogens)

• X represents halogens

Inorganic compounds

• Soluble in inorganic (polar) solvents – H2O

• Polar

• Ions

• Ionic bonds, polar & nonpolar covalent bonds

• Low flammability

• soluble in water (unless a non polar group is present)

• High boiling point and high melting point

• Metals & nonmetals

Types of Ions

Cation (+)

Anion (-)

Cation

are positively charged ions, formed when an atom loses electrons

Anion

are negatively charged ions, formed when an atom gains electrons.

Types of chemical bonds

Covalent - sharing electrons

Ionic - give and take

Carbon

4 bonds

Oxygen

2 bonds

Hydrogen

1 bond

Nitrogen

3 bonds

Halogens

F, Cl, Br, I

1 bond

Valence electrons

Electrons on the outermost shell

Homologous series

Alkanes

Alkenes

Alkynes

Alkanes

General formula: C_nH_2n+2

# Bonds: single

Saturated

Ex: Methane, Ethane

Alkenes

General formula: C_nH_2n

# Bonds: double

Unsaturated

Ex: Ethene, Propene

Alkynes

General formula: C_nH_2n-2

Bonds: Triple

Unsaturated

Ex: Ethyne, Propyne

# of Cs: 1

Meth

# of Cs: 2

Eth

# of Cs: 3

Prop

# of Cs: 4

But

# of Cs: 5

Pent

# of Cs: 6

Hex

# of Cs: 7

Heat

# of Cs: 8

Oct

# of Cs: 9

Non

# of Cs: 10

Dec

Molecular Formula

• General form with total number of each atoms:

• C5H10, C4H10

Structural Formula

• Detailed form with chemical bonds between atoms

• Condensed structural

• Expanded structural

• Line angle

• Expanded

• all chemical bonds are shown

• Condensed

• H atoms attached to each C atom are grouped together

• Line angle

• C and H atoms are not written, instead represented using lines; each joint represents a carbon atom