1. Types of Bonds 2
Section 19.2 part 2

2. Covalent bonding Group 4A- have 4 valence electrons
Too much energy is required to lose or gain 4 electrons, so these atoms share electrons
Covalent Bonding- attraction that occurs between atoms when they share electrons
Made up of 2 nonmetals
Molecule- neutral particle formed when elements covalently bond
Ionic bonds result in formula units instead of molecules

3. Covalent Bonding
Single Covalent Bond- made up of 2 shared electrons, usually one from one atom and the 2nd from the other atom
Double Covalent bond- 4 electrons shared
Triple Covalent bond- 6 electrons shared

4. Covalent Bonding
Electrons are not always shared equally in covalent bonds-
Strength of attraction for electrons varies due to: size of atom, charge of nucleus, and total number of electrons
Less attraction for electrons far from the nucleus
Greater + charge in nucleus = greater attraction for electrons

5. Covalent Bonding
Unequal sharing of electrons- each atom attracts the shared electrons, but one atom has a greater attraction than the other
Polar molecule- one end slightly + and one end slightly negative due to unequal electron sharing
Nonpolar molecule- electrons are shared equally by the atoms in the molecule
Made up of 2 atoms of the same element- diatomic molecules- usually

6. Diatomic Molecules
Hydrogen, nitrogen, chlorine, fluorine, bromine, iodine, oxygen
There are 7 and they form a 7 on the periodic table (except for H)