8.6 MidUnit Review

The sum of the atomic masses of all atoms in a substance is the ____.

• molar mass

• mole

• percent composition

• atomic number

The ___ is calculated by multiplying the number of each atom in the compound by its molar mass and adding them together.

• molar mass of a compound

• number of moles in a compound

• percent composition of elements in the compound

• atomic number of elements in the compound

What is the name for a compound that has water molecules bound to its atoms?

• polyatomic

• covalent

• hydrate

• diatomic

What quantity do you find using this equation:

(mass of element/total mass of compound) x 100%

• percent composition

• number of moles

• number of grams

• number of molecules

What is the % composition of C₁₂H₂₂O₁₁?

• C = 51%

  H = 6%

  O = 42%

• C = 42%

  H = 6%

  O = 51%

• C = 6%

  H = 42%

  O = 51%

• C = 42%

  H = 51%

  O = 6%

Which compound has a molar mass of 342 g/mole?

• C₁₂H₂₂O₁₁

• CH₂COOH

• AlPO₄

Which pairs of compounds and molar mass are matched correctly?

• NaOH = 32 g/mol

  H₂O = 16 g/mol

  O₂ = 40 g/mol

• NaOH = 40 g/mol

  H₂O = 18 g/mol

  O₂ = 16 g/mol

• NaOH = 40 g/mol

  H₂O = 32 g/mol

  O₂ = 18 g/mol

• NaOH = 40 g/mol

  H₂O = 18 g/mol

  O₂ = 32 g/mol

The mole is based on ____.

• the number of atoms in a 12 g sample of hydrogen.

• the number of atoms in a 12 g sample of carbon

• the number of molecules in a 12 g sample of water

• the number of atoms in a 12 g sample of oxygen

How many particles are in each mole of an element or compound? (Choose all that apply).

• Avogadro's number

• 6.02 x 10^21

• 6.02 x 10^22

• 6.02 x 10^25

How many moles are in 3 NaOH?

• 1

• 2

• 3

• 4