Electrostatic Forces and Atomic Structure Explained

The video tutorial explains the electrostatic forces that hold atoms together, focusing on Coulomb's law. It compares the forces in hydrogen and helium atoms, introducing the concept of the shielding effect. The tutorial further explores effective nuclear charge and compares the atomic structures of lithium and beryllium, highlighting differences in shielding effects and atomic radii.

What is the primary force that holds an atom together?

• Magnetic force

• Nuclear force

• Gravitational force

• Electrostatic force

According to Coulomb's law, what does the force between two charged particles depend on?

• The product of their charges and the square of the distance between them

• The distance between them

• The sum of their charges

• The difference in their charges

In a helium atom, what effect do inner electrons have on outer electrons?

• They have no effect on outer electrons

• They repel outer electrons

• They increase the net pull on outer electrons

• They shield outer electrons from the full charge of the nucleus

What is the effective nuclear charge?

• The charge of the innermost electron

• The charge of the outermost electron

• The charge felt by an outer electron after accounting for shielding

• The total charge of the nucleus

How does the presence of inner electrons affect the force felt by outer electrons in helium?

• It increases the force

• It decreases the force

• It has no effect

• It doubles the force

What is the ratio of inner to outer electrons in lithium?

• 1 to 1

• 2 to 2

• 2 to 1

• 1 to 2

Why does beryllium have a greater effective nuclear charge than lithium?

• It has more inner electrons

• It has fewer protons

• It has a larger atomic radius

• It has an extra electron in the outer shell

What happens to the atomic radius as the effective nuclear charge increases across a period?

• It fluctuates

• It remains the same

• It decreases

• It increases

As you move from left to right across a period, what happens to the effective nuclear charge?

• It fluctuates

• It remains constant

• It increases

• It decreases

What is the main reason for the decrease in atomic radius across a period?

• Decrease in effective nuclear charge

• Increase in the number of protons

• Decrease in the number of electrons

• Increase in effective nuclear charge