Atomic Mass: Atomic mass refers to the total mass of an atom, including the protons, neutrons, and a small contribution from electrons. It is usually expressed in atomic mass units (AMU) or grams per mole (g/mol). Atomic mass takes into account the mass of all the subatomic particles present in the atom.

Analogy: Think of a backpack that contains everything a person carries. The backpack represents the atom, and its contents—books, notebooks, snacks, and other items—represent the protons, neutrons, and electrons. The total weight of the backpack and its contents is similar to the atomic mass, which accounts for the mass of all the subatomic particles.

Relative Atomic Number: Relative atomic number is not a commonly used term in atomic structure. The atomic number itself is a unique identifier for each element and remains constant for that element. It is not typically compared or expressed in relation to anything else.

1. Atomic Mass                      12

Element Symbol                       C   

Atomic Number                      6          

2. Atomic Mass         23

Element Symbol          Na  

Atomic Number       11

3. Atomic Mass         14

Element Symbol          N

Atomic Number       7     

Relative Atomic Mass: Relative atomic mass, also known as atomic weight, is the average mass of an element’s atoms, taking into account the abundance of each naturally occurring isotope of that element. It is expressed as a weighted average. Isotopes are atoms of the same element with different numbers of neutrons.

Relative atomic mass is like calculating the average weight of a classroom of students. You would add up the individual weights of each unique student, taking into account that some weights are more common than others. The average considers both the different weights of each student (isotopes) and how many students have each weight (abundance).

Make a table to distinguish between electrons, protons and neutrons based on charge, mass, relative charge and relative mass.

Sodium (Na): Atomic number 11

• Structure: Sodium has 11 protons in its nucleus and 11 electrons orbiting around the nucleus.
• Electronic Configuration: 2, 8, 1

• Calcium (Ca): Atomic number 20

• Structure: Calcium has 20 protons in its nucleus and 20 electrons orbiting around the nucleus.
• Electronic Configuration: 2, 8, 8, 2

• Potassium (K): Atomic number 19
  • Structure: Potassium has 19 protons in its nucleus and 19 electrons orbiting around the nucleus.
  • Electronic Configuration: 2, 8, 8, 1

• Helium (He): Atomic number 2
  • Structure: Helium has 2 protons in its nucleus and 2 electrons orbiting around the nucleus.
  • Electronic Configuration: 2

• Sulphur (S): Atomic number 16
  • Structure: Sulphur has 16 protons in its nucleus and 16 electrons orbiting around the nucleus.
  • Electronic Configuration: 2, 8, 6

• Neon (Ne): Atomic number 10
  • Structure: Neon has 10 protons in its nucleus and 10 electrons orbiting around the nucleus.
  • Electronic Configuration: 2, 8

• Argon (Ar): Atomic number 18
  • Structure: Argon has 18 protons in its nucleus and 18 electrons orbiting around the nucleus.
  • Electronic Configuration: 2, 8, 8

• Chlorine (Cl): Atomic number 17
  • Structure: Chlorine has 17 protons in its nucleus and 17 electrons orbiting around the nucleus.
  • Electronic Configuration: 2, 8, 7

• Nitrogen (N): Atomic number 7
  • Structure: Nitrogen has 7 protons in its nucleus and 7 electrons orbiting around the nucleus.
  • Electronic Configuration: 2, 5

• Oxygen (O): Atomic number 8
  • Structure: Oxygen has 8 protons in its nucleus and 8 electrons orbiting around the nucleus.
  • Electronic Configuration: 2, 6

• Magnesium (Mg): Atomic number 12
  • Structure: Magnesium has 12 protons in its nucleus and 12 electrons orbiting around the nucleus.
  • Electronic Configuration: 2, 8, 2