Chapter 7 - Quantifying Atoms & Compounds

Question 1

Avogrado’s Constant

Answer 1

The number of particles in one mole, equal to 6.02 x 10^23.

Question 2

Carbon-12

Answer 2

The standard reference for relative mass, with carbon 12 being equal to 12 units exactly.

Question 3

Empirical Formula

Answer 3

The simplest whole number ratio of the elements in a compound.

Question 4

Mass Spectrometer

Answer 4

A device used to measure the relative isotopic masses of an element, as well as their abundances.

Question 5

Mass Spectrum

Answer 5

A graph that represents the abundance of different isotopes.

Question 6

Molar Mass

Answer 6

The mass of one mol, measured in grams per mole. Note: molar mass is equivalent to relative atomic mass.

Question 7

Mole (Mol)

Answer 7

A unit of measurement, equal to 6.02 x 10^23 particles.

Question 8

Molecular Formula

Answer 8

The actual number of atoms of each type in a molecule.

Question 9

Percentage Composition

Answer 9

The percentage by mass of an element in a compound. For example, 57.5% of sodium hydroxide’s mass is sodium.

Question 10

Relative Atomic Mass

Answer 10

The weighted mean of all the isotopic masses of an element, relative to carbon 12.

Question 11

Isotopic Abundance

Answer 11

The percentage of a particular isotope found naturally. For example: 75% of chlorine atoms are chlorine 35.

Question 12

Relative Isotopic Mass

Answer 12

The mass of an isotope relative to carbon 12.

Question 13

Relative Mass

Answer 13

The mass of an element or compound measured in relation to carbon 12 being taken as 12 units exactly.