1. Covalent and Ionic Bonding
Mrs. Butsch 8th Grade Science

2. Compounds
Compound: Atoms of more than one type of element that are chemically bonded together.
One Oxygen atom
2 Hydrogen atoms

3. Examples of Compounds:
Alcohol  C2H5OH
Salt  NaCl
Water  H2O
Sugar  C12H22O11
Methane  CH4
Carbon Dioxide  CO2

4. Bohr Model of an Atom

5. Sodium (Na) Atom
Sodium (Na)
11 Protons
12 Neutrons
11 Electrons

6. Neon (Ne) Atom
Neon (Ne)
10 Protons
10 Neutrons
10 Electrons

7. Chlorine (Cl) Atom
Chlorine (Cl)
17 Protons
18 Neutrons
17 Electrons

8. Bonding
Bonding- The forces that hold the atoms together in compounds are called chemical bonds.

9. Covalent Bonds
Covalent Bonds- The type of bond that forms by sharing outer electrons.
A group of atoms connected by covalent bonds are called molecules.

10. Covalent Bonds Water Molecule
Two atoms of hydrogen can share electrons with one atom of oxygen to form one water molecule.

11. Covalent Bonds- Non-metals
Each of the hydrogen atoms has one electron in tits outermost level and the oxygen has six electrons in its outermost level. This causes them to bond together.
Both hydrogen and oxygen atoms become stable.

12. Ionic Bonds– Metal and Non-metals
Ionic Bonds combine atoms when they are positively and negatively charged.
Ions: electrically charged atom whose charge results from an atom losing or gaining electrons.
Ions are attracted to each other when they have positive and negative charges

13. Valence Electrons
Electrons in the outer most shell of an atom that can participate in forming chemical bonds with other atoms

14. Octet Rule
This rule states that, except for Hydrogen, an atom combines with other atoms to form bonds in order to have 8 electrons in its valence shell.

15. Lewis Dot Symbols
Representations of the elements which give a dot (.) for each valence electron on the atom.