Lesson Plan: C1.1.08

Hamble Lesson Observation Plan
Learning About
What is relative atomic mass?
Keywords:
  • Relative atomic mass: the average mass of an atom when taking into consideration the proportions of the different isotopes of an element. (1)
  • Mass number: the total number of protons and neutrons within an atom of an element. (1)
  • Atomic number: the number of protons found in the nucleus of an atom of an element. (1)
  • Isotope: an atom of the same element with the same number of protons but a different number of neutrons. (1)
Memory Anchor:
Method Precise Learning Objective Linked Question / Activity
(Designed for maximum working out)		 Stepping Stones Pitstop Check
(Thinking Map)
Atoms of the same element can have different numbers of neutrons; these atoms are called isotopes of that element. What is an isotope?

Determine the element using RAM periodic table. link to measurement errors.
Atoms can be represented as shown in this example: (periodic table tile for sodium with mass and atomic number) What do the individual tiles of the periodic table tell us?
Students should be able to calculate the numbers of protons, neutrons and electrons in an atom or ion, given its atomic number and mass number. Calculate the number of protons, neutrons and electrons in an atom of Cobalt. Mass number = 59 and Atomic number = 27
Students should be able to relate size and scale of atoms to objects in the physical world. How large are atoms? a) 1 × 10-6 m b) 1 × 10-8 m c) 1 × 10-10 m
The relative atomic mass of an element is an average value that takes account of the abundance of the isotopes of the element. Why does chlorine have a mass number of 35.5?
Students should be able to calculate the relative atomic mass of an element given the percentage abundance of its isotopes. What is the relative atomic mass of bromine where there are two isotopes of Bromine, 50% Br-79 and 50% Br-81?
Links To the Big Ideas
ForcesParticlesEnergyCells