Chapter 4 Flashcards
Molecule
2 or more molecules held together by covalent bond
Molecular weight
Sum of atomic weights of the atom in a molecule
Units : amu / molecule
Formula weight
Adding up atomic weights of ions
Units : amu/ molecule
Gram equivalent
Molar mass /n
Equivalent
Mass of compound (g)/ gram equivalent weight (g)
What are the units for normality
Equivalent / L
What is the formula for conversion of normality to molarity?
Molarity = normality /n
What is the formula to calculate normality ?
Molarity x n
Law of constant composition
Any pure sample of a given compound will contain the same elements in an identical mass ratio
Empirical formula
Gives the simplest whole number ratio of elements in a compound
Molecular formula
Exact number of elements in the compound
What is the formula for percent composition ?
Percent composition =
mass of element in formula / molar mass x 100
Combination reaction
Two or more reactants form one product
Decomposition reaction
Single reactant breaks down into two or more products
Combustion reaction
Hydrocarbon + oxygen –> CO2 + H2O
Single displacement reaction
When an atom or ion in a compound is replaced by another atom or ion
Double displacement reaction
Two different compounds swap places to for, two new compounds
Neutralization reaction
Double displacement reaction in which an acid reacts with a base to form a salt
Law of conservation of mass
Mass of reactants consumed equals the mass of product generated
What is the formula for percent yield?
Percent yield = actual yield/ theoretical yield x 100
When is the ending ous used ? When is the ending ic used ?
Ous - ion with lesser charge
Ic- ion with greater charge
How are the endings ite and ate used for oxyanions ?
Ite - lighter anions with less oxygen
Ate - anions with more oxygen
How are the endings hypo and per used in extended series of anions ?
Hypo - less oxygen
Per - more oxygen
