Subatomic Particles and Atomic Structure

The video tutorial introduces the concept of subatomic particles, focusing on protons, neutrons, and electrons. It explains their properties, locations within an atom, and how to count them using the periodic table. The tutorial also covers how to calculate the number of neutrons and understand ions and their charges. A humorous analogy is used to illustrate the concept of gaining and losing electrons.

What is the main reason a regular microscope cannot be used to view subatomic particles?

• They are too large to be seen.

• They are too dark to be seen.

• They are too small to be seen.

• They are too bright to be seen.

Which subatomic particle is positively charged?

• Photon

• Electron

• Neutron

• Proton

What is the charge of a neutron?

• Neutral

• Negative

• Variable

• Positive

How many protons does Boron have if its atomic number is 5?

• 10

• 5

• 3

• 7

If an element has an atomic number of 79, how many electrons does it have?

• 99

• 79

• 59

• 39

How do you calculate the number of neutrons in an atom?

• Divide the atomic number by the mass number.

• Subtract the atomic number from the mass number.

• Multiply the atomic number by the mass number.

• Add the atomic number to the mass number.

Iron has an atomic number of 26 and a mass number of 56. How many neutrons does it have?

• 82

• 56

• 30

• 26

What happens to an atom when it gains an electron?

• It becomes positively charged.

• It becomes negatively charged.

• It becomes unstable.

• It remains neutral.

Chlorine has 17 protons and a negative charge. How many electrons does it have?

• 16

• 17

• 18

• 19

If calcium has a positive charge of 2, how many electrons does it have compared to its protons?

• It has 4 more electrons than protons.

• It has the same number of electrons as protons.

• It has 2 fewer electrons than protons.

• It has 2 more electrons than protons.