Chapter 4: Compounds and Stoichiometry Flashcards
________ ________ is the weighted average of the masses of the naturally occurring isotopes of an element, not their weights.
Atomic weight
____________ ________ is the sum of the atomic weights of all the atoms in a molecule, and its units are atomic mass units (amu) per molecule.
molecular weight
____________ ________ of an ionic compound is found by adding up the atomic weights of the constituent ions according to its empirical formula, and its units are also amu per molecule.
formula weight
molecular weight isn’t really a thing, so we use this
A ________ is equal to the number of particles found in 12 grams of carbon-12.
mole
What are the units for molar mass?
g/mol
What are the units for molecular weight?
amu per molecule
The amount of a compound, measured in grams, that produces 1 equivalent of the particle of interest is called the ________ ________________ ____________.
gram equivalent weight
The ________________ ________ of a compound is the mass that provides 1 mole of the particle of interest.
equivalent weight
________________ is a measure of concentration, given in the units equivalents/L.
Normality
most commonly used for H+ concentration
A 1 N solution of acid contains an [H+] equal to ____ mol/L.
1
In acid-base chemistry, the gram equivalent weight represents what?
The mass of acid that yields 1 mol of H+, or the mass of base that yields 1 mol of OH-
The law of ____________ ________________ states that any pure sample of a given compound will contain the same elements in an identical mass ratio.
constant composition
The ____________ formula gives the simplest whole-number ratio of elements in a compound.
empirical
The ________________ formula gives the exact number of atoms of each element in the compound and is a multiple of the empiral formula.
molecular
Ionic compounds, such as NaCl or CaCO3, will only have ____________ formulas.
empirical
The ____________ ________________ of an element (by mass) is the % of a specific compound that is made up of a given element.
percent composition
Given the percent composition of a compound, how do you find the e.f. and m.f.?
Empirical formula:
1. Assume sample is 100 g.
2. Convert % of each element to g.
3. Divide each value by respective molar mass to find mol.
4. Divide each value by smallest mol amount.
5. Multiply by integer value to get whole number
Molecular formula:
1. Divide given molar mass by formula weight of e.f.
A ________________ reaction has 2+ reactants forming one product.
combination
A ________________ reaction is the opposite of a combination reaction: a single reactant breaks down into 2+ products.
usually heat, radiation, electrolysis
decomposition
A ____________ reaction is a special type of reaction that involves fuel, usually a hydrocarbon, and an oxidant (normally oxygen)
combustion
What are the products of a combustion reaction?
CO2 and H2O
A ________-________________ reaction occurs when an atom or ion in a compound is replaced by an atom or ion of another element.
single-displacement
In ________-________________ reactions, also known as metathesis reactions, elements from 2 different compounds swap places with each other to form 2 new compounds.
double-displacement
____________ reactions are a specific type of double-displacement reaction in which an acid reacts with a base to produce a salt and usually water.
Neutralization
