Understanding Moles and Avogadro's Number

$$3.14 \times 10^{10}$$

$$6.022 \times 10^{23}$$

$$1.67 \times 10^{-24}$$

$$9.81 \times 10^{2}$$

Liter (L)

Mole (mol)

Gram (g)

Meter (m)

The number of atoms in a molecule

The molar mass = mass of one mole of a substance

The volume of a gas

The charge of an ion

The smallest particle of an element

A pure substance made of only one kind of atom

Two or more atoms chemically bonded together

A symbolic representation of a compound

$$1.00 \times 10^{3}$$

$$6.022 \times 10^{23}$$

$$1.00 \times 10^{6}$$

$$3.00 \times 10^{8}$$

$$1 \text{ mol} = 1 \text{ g}$$

$$1 \text{ mol} = 6.022 \times 10^{23} \text{ particles}$$

$$1 \text{ g} = 6.022 \times 10^{23} \text{ particles}$$

$$1 \text{ mol} = 1000 \text{ g}$$

$$0.25$$ mol

$$0.5$$ mol

$$1$$ mol

$$2$$ mol

$$29.25$$ g

$$58.5$$ g

$$117$$ g

$$120$$ g

$$2215$$ mol

$$0.146$$ mol

$$6.8$$ mol

$$18$$ mol

$$1.059\times10^{24}$$

$$6.022 \times 10^{23}$$

$$1.204 \times 10^{24}$$

$$3.011 \times 10^{23}$$