An Introduction to Chemistry Important biological elements –Carbon –Oxygen –Nitrogen –Hydrogen –Sulfur –Na –K

II.Atomic Structure A.Definition B.Analogy of structure C.Subatomic particles –1.Protons –2.Neutrons –3.Electrons

III.Electron orbitals A.Location B.Maximum number of electrons in an orbital C.Orbital filling D.Examples –1.H –2.C –3.Na –4.Si

III.Electron orbitals E.Valence electrons –1.Definition –2.Involved in chemical bond formation –3.Determines chemical properties of the atom –4.Elements with the same number of valence electrons have similar chemical properties

III.Electron orbitals E.Valence electrons –5.gaining and losing energy

IV.Periodic table

An atom with an atomic number of 13 and a mass of 22 possesses ____ electrons The answer cannot be determined

An atom with an atomic number of 13 and a mass of 22 possesses ____ valence electrons

V.Chemical Bonding A.Octet Rule –1.Definition –2.Noble Gases

V.Chemical Bonding B.Ionic Bonding –1.Example 11 Na 17 Cl

V.Chemical Bonding B.Ionic Bonding –2. Definition

Ionic bonding

What is the equation of the compound formed when 20 Ca and 17 Cl combine by ionic bonding? 1.Ca 2 Cl 2.CaCl 3.CaCl 2 4.The answer cannot be determined

V. Chemical Bonding C.Covalent bonding –1.Definition –2.Example of nonpolar covalent –3.Example of polar covalent bonding

Nonpolar Covalent

Polar Covalent Bond