Intramolecular Bonds Ionic Bonds – metal (gives e-, cation) with non-metal (takes e-, anion) - GLUE: electrostatic attraction Covalent Bonds – non-metal atoms (polarity of bond depends on electronegativity difference of atoms) - GLUE: share e- Metallic Bonds –metal atoms - GLUE: sea of electrons e-

Names/Formulas of Compounds Ionic Compounds : (Note: 1st atom is metal OR ammonium) Atom + Atom-ide If 1st atom is a metal you don’t know the charge of…use Roman Numerals If you cross charges, SIMPLIFY If you cross a 2 charge or higher next to a polyatomic ion…use parentheses! Know Polyatomic Ions: Ammonium – NH4+ Carbonate – CO32- Hydroxide – OH- Chromate – CrO42- Cyanide – CN- Dichromate – Cr2O72- Nitrite – NO2 - Sulfite – SO32- Nitrate – NO3 - Sulfate – SO4 2- Bicarbonate - HCO3- Phosphate – PO43- Acetate – C2H3O2- Permanganate – MnO4- Write the formula: Magnesium chloride  d. Aluminum hydroxide  Iron (III) phosphide  e. Calcium bicarbonate  Lead (IV) sulfate  f. Gold nitrite  Write the name: Cu2O  c. Zn3(PO4)2  KCl  d. Ag2Cr2O7 

Names/Formulas of Compounds Covalent Compounds : (Note: 1st atom is non-metal, prefixes are present) Prefix-Atom + Prefix-Atom-ide Never use mono- on 1st atom NEVER SIMPLIFY Don’t think!!!... Just do what it says!!! Know Prefixes: 1 – mono 6 – hexa 2 – di 7 – hepta 3 – tri 8 – octa 4 – tetra 9 – nona 5 – penta 10 – deca Write the formula: tetraphosphorus octaoxide c. Disulfur monophosphide Carbon trioxide d. Hexafluorine decabromide Write the name: SO4  c. N5H9  CO3  d. P7Cl10 

Dot Diagrams Rules: Draw the dot diagrams: F2 b. O2 c. N2 d. HF Put the atom by itself in the middle. Surround it by the other atoms. Hydrogen goes on the outside ALWAYS! Atoms want to maximize electron repulsion and get as far away from each other as possible. Draw the dot diagrams: F2 b. O2 c. N2 d. HF H2O f. CO2 g. SiS2 h. BCl3 i. CBr4 j. C2H6 k. C2H4 l. C2H2

VSEPR Practice Compound Dot Diagram Shape Name Bond Angle(s) Polarity Hybridization H2 HCl SiO2 CF4 H2S PH3 Si2H4