Chemistry: The Mole - Chemical Quantities

mole

Term that represents a really huge number in chemistry.

6.02 × 10²³

Avogadro’s Number

atom

Used to describe the individual particles of an element

Molecule

Used to describe the individual particles of a molecular (covalent) compound (contains nonmetals) or a diatomic element

formula unit

Used to describe the lowest ratio of the two ions in an ionic compound (cation in the front and anion in the back)

6.02 × 10²³

1 mole = how many particles

grams

1 mole = the mass of a substance in what units

22.4

1 mole = how many Liters

1

If a problem has the word “mole” in it (you are given the moles or asked to find the moles), you need __ step conversion factor to solve it.

2

If a problem does not have the word “mole” in it, you need __ step conversion factors to solve it.

1000g

1kg = how many grams

1000mg

1g = how many milligrams

1000mL

1L = how many milliliters

part/whole x100 = percent (round to the 100ths place for the percentage)

What is the formula for percent composition?

percent composition

The percent by mass of each element in a chemical formula.

molecular

The ________ formula for a compound is its true formula, as it exists in nature.

empirical

The ________ formula for a compound is a reduced version of the molecular formula. It shows the simplest whole number ration of the elements. It is also known as the “simplest formula."

sometimes

Are the empirical and molecular formulas identical?

yes

Can some compounds have different molecular formulas but the same empirical formula?