Chapter 6- Nomenclature Chapter 8:Chemical Equations Flashcards
Diatomic Molecules
Iodine Nitrogen Bromide Chloride Hydrogen Oxygen Fluoride
Ionic compounds
Metal & Non-metal
They must equal 0
Na+Cl= NaCl
Molecular Compunds
Two N.M + N.M
Cross-Over Rule
Metal first than non-metal
If the same number they will cancel out
Binary compounds contain metals
A) Metal/positive ion + Non-metal/negative ion
B) metals with more than one
Metal higher charge “ic”
Lower charge “ous”
Binary Compounds Non-metal
N2O3 –> dinitrogen trioxide
Compounds containing Polyatomic Ions
K MnO4 = KMnO4
Potassium Permagenate
Prefixs
1-mono 2-di 3-tri 4-tetra 5-penta 6-hexagon 7-hepta 8-octa 9-Nona 10-deca
Acids and Oxy-Acids
A) H + N.M
Hydro Chlor Ic
B) H + O "ate" = ic "it's" = ous H2CO3 = Carbonic Acid *hydrogen is not used*
Reactant
A chemical substance entering into a reaction
Product
A chemical substance produced from reactants by a chemical change
Heat of reaction
The quality of heat produced by chemical reactions
Activation Energy
The amount of energy needed to start a chemical reaction
Balanced Equations
# atoms in each substance # miles in each substance
Combination Reaction
A + B = AB
Metal + Oxygen = metal oxide
Metal + N.M = salt