C2.5 - Explaining Trends (Finished)

Question 1

What are the three factors that affect the electrostatic attraction of an atom?

Answer 1

• Size of positive charge
• Shielding effect of electrons
• Distance between nucleus and outer shell

Question 2

Why do non-metals get less reactive going down the group?

Answer 2

They want to gain electrons, and because of less electrostatic attraction going down the group, gaining electrons gets harder so therefore reactivity decreases.

Question 3

How does a larger positive charge size in the nucleus affect electrons?

Answer 3

It creates a greater electrostatic attraction making the atom hold onto electrons “stwonger”

Question 4

What do the electrons in the shells in atoms do to affect the electrostatic attraction felt by the electrons in the next shell?

Answer 4

They provide a shielding effect to ‘shield’ the outer electrons from the positive charge, decreasing the electrostatic attraction felt by the next electron(s)

Question 5

Does distance between the outermost electrons and nucleus of an atom affect how much attraction is felt by the outer electrons?

Answer 5

Yes

Question 6

Why does Lithium with a smaller nuclear charge of 3 still has a stronger attraction than sodium with a charge of 11?

Answer 6

The other two factors of distance and shielding effect outweigh nuclear charge

Question 7

Will an incoming electron experience more attraction going into th écouter shell of fluorine (F) or chlorine (Cl)?

Answer 7

Florine, the chlorine atom has more electrons to shield the effects of the charge and is the largest.

Question 8

Which of these atoms will have electrons in its outermost shell experiencing the most attraction?
Helium, fluorine, potassium or lithium?

Answer 8

Fluorine …. right?

Question 9

Why do group 1-3 elements increase in reactivity going down the groups?

Answer 9

As they want to loose electrons and due to less electrostatic attraction going down, that gets easier.