Chapter 6a Masses of Particles

The isotope that all isotopic masses are compared to is

• oxygen-16

• hydrogen-1

• carbon-12

• magnesium-24

The isotopic masses of these isotopes are

• H = 1

  He = 4

  Li = 7

  C = 12

• H = 1

  He = 2

  Li = 3

  C = 6

• H = 2

  He = 6

  Li = 10

  C = 18

• H = 0

  He = 2

  Li = 4

  C = 6

Relative isotopic abundance is the defined as the % of each isotope in a naturally occurring sample of an element.

• True

• False

The most common isotope of hydrogen is

• hydrogen-1

• hydrogen-2

• hydrogen-3

The most common isotope of chlorine is

• chlorine-35

• chlorine-37.

The relative atomic mass of silver is

• 106.9.

• 108.9

• 107.9

The relative atomic mass is defined as

• the mass of an atom relative to 1 kg.

• the masses of all isotopes of an element added and divided by the number of isotopes.

• the average mass of all isotopes of an element determined by their percentage abundance.

• the mass of atoms as measured by a mass spectrometer.

Using this information, the relative atomic mass of iridium, Ir, is

• 191.97

• 192.20

• 7,244.2

• 241.97

Relative molecular mass is the relative mass of molecules and relative formula mass if the relative mass of ionic compounds.

• True

• False

The relative molecular mass of CO₂ is

• 28

• 44

• 56

• 14