Chapter 4-chemical compounds Flashcards
(22 cards)
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
