Relative Atomic Mass and Relative Molecular Mass
Chemistry ⇒ Atomic Structure and the Periodic Table
Relative Atomic Mass and Relative Molecular Mass starts at 9 and continues till grade 12.
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Describe how the relative atomic mass of an element is determined experimentally.
Explain the difference between relative atomic mass and mass number.
Explain why the relative atomic mass of most elements is not a whole number.
Explain why the relative molecular mass of a compound is important in chemical calculations.
Which of the following best describes the term 'relative formula mass'?
(1) The mass of one molecule in grams
(2) The sum of the relative atomic masses of the atoms in a formula unit
(3) The mass of one mole of a substance
(4) The mass of a single atom
Which of the following best explains why the relative atomic mass of chlorine is 35.5?
(1) Chlorine has only one isotope
(2) Chlorine is a mixture of two isotopes with different abundances
(3) Chlorine atoms lose electrons
(4) Chlorine reacts with hydrogen
Which of the following compounds has the highest relative molecular mass?
(1) H2O
(2) CO2
(3) NH3
(4) CH4
Which of the following is NOT a reason why isotopic abundances affect the relative atomic mass of an element?
(1) Different isotopes have different masses
(2) Isotopes have different chemical properties
(3) The percentage of each isotope varies
(4) The average is calculated based on abundance
Fill in the blank: The relative atomic mass of hydrogen is approximately ______.
Fill in the blank: The relative atomic mass of oxygen is approximately ______.
Fill in the blank: The relative atomic mass of sodium is approximately ______.
Fill in the blank: The relative molecular mass of carbon dioxide (CO2) is ______. (C = 12.0, O = 16.0)
True or False: The relative atomic mass of an element can be determined using mass spectrometry.
True or False: The relative atomic mass of an element is always less than its mass number.
True or False: The relative atomic mass of chlorine is not a whole number because chlorine exists as a mixture of isotopes.
True or False: The relative molecular mass of a compound is the sum of the relative atomic masses of all the atoms in its formula.
