For the tribes of alkene or alkyne isomers which already has given the name by the way:

a. Alkene or alkyne name in front of numbers written that states the location of double bonds. Number of double bonds was made in every detail.

b. For tribes that have branches, named as the branched alkanes.

WITH CHAIN ​​branched alkanes

- Name of alkanes based on the longest chain C

- In front of the name is written alkananya number and name of the branch (alkyl)

- If there are several branches of the same then the branch name is mentioned once but equipped with a prefix that states the amount of the entire branch. The atomic number of the branch C is bound to be written as an existing branch (number of numbers in write = the prefix is used)

- For the different branches are sorted in alphabetical order.

Straight-chain alkanes

- The series of homologous or homologous series is a series of compounds having similar chemical properties and each tribe  at odds successive CH2 

- Alkyl groups is occurring when an H atom from alkanes removed

- Notation alkyl is R. Alkyl same name with alkenes origin, with the suffix replaced by ana-il.

hydrocarbon compounds

Hydrocarbon compounds are compounds of carbon that consists of only C and H atoms only. Based on the existing bonds in the chain C, hydrocarbon compounds distinguished by:

- Compounds saturated hydrocarbons (alkanes)

Saturated hydrocarbons called alkanes or paraffins, the formula CnH2n +2. Saturated hydrocarbons (alkanes) is divided into straight chain alkanes and branched chains.

- Compounds are unsaturated hydrocarbons (alkenes and alkynes)

BONDING CARBON COMPOUNDS

Based on the chains used to form covalent bonds between atoms in a compound of carbon, the carbon compounds distinguished by:

1. saturated bond

Unsaturated bond in question is a single bond in which the constituent atoms (C atoms mainly) covalently bonded to the chain.

2. Unsaturated bond

The definition of an unsaturated bond is a double bond or triple bond. The constituent atoms are bonded with 2 or 3 chains covalently at once. Based on the number of other C atoms are bonded to one carbon atom in the chain C, then C atoms can be divided into:

a. Primary C atoms, ie C atoms are bonded to one other C atom

b. Secondary C atoms, ie C atom attached to two other C atoms

c. Tertiary C atoms, ie C atom attached to three other C atoms

d. Kwarterner C atoms, ie C atoms are bonded to four other C atoms.

FORMS OF mOLECULES

One method to predict the molecular shape is the electrolyte pair repulsion theory or the valence shell electron sheell Valance Pair Repulsion (VSEPR). The basis of this theory is the valence electron pairs around the central atom will try as far as possible from each other to minimize repulsion. Valence electron pairs are bonding pairs and lone pairs. Molecules or ions that do not have a lone pair of electrons around atoms freely around the center has 4 basic geometry which depends on the number of bonds on the central atom is linear, flat triangle (trigonal planar), bipiramida triangle (trigonal bipiramid), and octahedral.

Molecular shape is determined by the number of hybrid orbitals.

For example:

- Molecular orbital s then form spherical (ball)

- P orbitals of the molecule forms a ball twist.

TYPES OF CHEMICAL BONDING

A. Ionic bond

Ionic bonding can occur because of the handover of electrons between atoms. This bond is formed between:

- The positive ions with negative ions (by electrostatic force)

- Atom-atom ionization potential of small-energy with the atoms of large electron affinity

- Atom-atom element IA, IIA with atoms large electronegativity

- Small electronegativity atoms with atoms of the large electronegativity.

The properties of ionic compounds:

- If liquid can conduct electricity

- If the solid can be shaped crystals

- Boiling point and high melting

- Soluble in polar solvents

- Hard but brittle

B. Covalent bonds

Covalent bonding occurs by the use of shared electron pairs. This bonding occurs among the nonmetallic elements of low electronegativity difference. According to the octet rule, in the bonded atoms will try to get the electronic configuration of noble gases are stable, which has totaled eight valence electrons. However, there are some covalent molecules have structures that do not meet the Lewis octet rule.

The division of a covalent bond

a. Nonpolar covalent bond: if the pair of electrons shared equally strong interest to all atoms.

Characteristics:

- The dipole moment = 0

- Contains the same type of atom

- Forms a symmetrical molecule

b. Polar covalent bonds: if the pair shared electrons more strongly attracted to one atom.

Characteristics:

- The dipole moment> 0

- The difference between the electronegativity of bonded atoms

- The shape is not symmetrical molecule

c. Semi-polar bond (coordinate covalent) bond occurs when electrons pair together only come from one atom.

Covalent properties:

- Polar covalent compounds can conduct electricity

- Nonpolar covalent compounds can conduct electricity

- Boiling point and melting was relatively lower than ionic compounds

- Soluble in nonpolar solvents

- Easy to evaporate

Ionic bonding and covalent bonding is an intramolecular bonds that bind atoms in molecules. While the bond that unites responsible molecules are called intermolecular. Intramolecular bonds cause the molecules attract each other with neighboring molecules. Intramolecular and intermolecular bonds referred to collectively as the chemical bonds.

C. Other chemical bonds

a. Hydrogen bonds: H atoms bond with other atoms a large electronegativity (other atoms are from different molecules)

b. Metallic bond: Occurs due to dense arrangement of metal atoms, so that the electrons in their outermost shells to move freely

c. Bond Van Der Walls: Occurs because of the forces of attraction between molecules is very weak.

role of electrons in chemical bonds

Atoms are said to be stable if the same electron configuration noble gas configuration (structure duplet or octet).

- Structure duplet

has two electrons in the outer shell (similar to the configuration of Helium)

- Structure of octets

have 8 electrons in the outer shell (with Ne, Ar, Kr, Xe, Rn).

the number of unpaired electron orbital

For the transition elements. Practical formula:

1. Atomic Number VIIA + (1-7)

Electrons = Number of atoms - (atomic number VIIIA + 2)

2. Atomic Number VIIIA + (8-12)

Electrons = (1 / 2 VIIIA + 6) - Orbital full.