Chapter 4-chemical compounds Flashcards
Molecule
Combination of two or more atoms held together by covalent bonds
Formula unit
Used for ionic compounds as an ions and cat ions do not have a covalent bond
Equivalent weight
Amount of a compound that produces one equivalent of a particle in question.
Graham equivalent weight
Mass of a compound needed to produce one equivalent of a particle.
Normality (N)
Equivalents/volume in L
Molarity= N/n
Law of constant composition
A pure sample of a compound will contain the same elements in an identical mass ratio as the reactants are used to form it
Empirical formula
The simplest whole number ratio of element in a compound
Molecular formula
Actual number of atoms of each element in a compound
Percent composition
Mass of element, times number of moles of that element/ molar mass
Combination reactions
Use two or more reactants to form one product
Decomposition reaction
A single reactant breaks down into multiple products
Combustion reaction
Uses a fuel, typically a hydrocarbon, + O2 = resulting in its breakdown and formation of carbon dioxide and water
Single displacement reaction
Typically with metals, an atom or ion replaces it’s counterpart in a compound
Double displacement reaction
Elements from two compounds trade places
Neutralization reaction
And acid reacts with a base to produce a salt
Theoretical yield
Maximum amount of a product that can be generated from a predicted balanced equation
Actual yield
The actual amount of product actually obtained during a reaction
Percent yield
Actual/theoretical yield
Cat ions
Positively charged Atoms, typically metals
Cations
Net charged atoms typically non-metals.
Ionic bond
Attraction between the positive charge of a cat ion and the negative charge of an anion
Electrolytes
A solution that enables ionic compounds to freely move allowing for the conductivity of electricity
