Atomic Mass and Subatomic Particles

The video explains atomic mass, defined as the total number of protons and neutrons in an atom's nucleus. It uses examples of fluorine, aluminium, and chlorine to illustrate the concept. Chlorine's isotopes are introduced, showing how an element can have atoms with different atomic masses. The video sets the stage for a deeper exploration of isotopes in the next video.

What is the atomic number of an element?

• The number of neutrons in the nucleus of an atom

• The number of protons in the nucleus of an atom

• The total number of electrons in an atom

• The sum of protons and neutrons in an atom

Which subatomic particles are considered when calculating atomic mass?

• Only electrons

• Only protons

• Protons and neutrons

• Neutrons and electrons

Why are electrons not considered in the calculation of atomic mass?

• They have a significant mass

• They are located outside the nucleus

• They are negatively charged

• They have negligible mass

What is the atomic mass of fluorine?

• 19 units

• 10 units

• 18 units

• 9 units

How many neutrons are present in an aluminium atom?

• 12

• 27

• 14

• 13

What is the atomic mass of aluminium?

• 14 units

• 13 units

• 26 units

• 27 units

What is the atomic mass of chlorine with 17 protons and 18 neutrons?

• 35 units

• 36 units

• 37 units

• 34 units

What is the atomic mass of chlorine with 17 protons and 20 neutrons?

• 35 units

• 34 units

• 37 units

• 36 units

What phenomenon allows chlorine to have two different atomic masses?

• Isotopes

• Ions

• Isomers

• Allotropes

What will the next video explore?

• Atomic number

• Subatomic particles

• Isotopes

• Atomic mass