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Question 1

Explain the periodic trend of I.E going across a period

Answer 1

I.E. generally ^^ going&raquo_space; a period.
- Nuclear charge also ^^. Since the valence electrons are going into the same energy level, they are shielded from the nucleus by the same number of inner electrons.
- This means that the inner electrons’ effective nuclear attraction has ^^ and it takes more energy to remove an electron

Question 2

Explain the periodic trend of I.E going down a group

Answer 2

• I.E. generally \/ going down each group.
  -Valence electrons are going into another energy further from the nucleus so even though the nuclear charge has increased, the extra shielding of the inner electrons results in a weaker attraction between the nucleus and valence electrons.
• Thus the effective nuclear attraction has \/ and it takes less energy to remove an electron.

Question 3

Explain the periodic trend of atomic radii going across a period

Answer 3

• Atoms get smaller going across each period as there is a greater nuclear charge.
• Since the electrons are going into the same energy level, valence electrons experience the same shielding effect from the inner electrons.
• So overall, there is a greater effective nuclear attraction for the outer electrons as they are pulled closer to the nucleus decreasing the size of the atoms atomic radius.

Question 4

Explain the periodic trend on atomic radii going down a group

Answer 4

• Atoms get larger going down each group as another energy level for electrons is added increasing the shielding effect on the outer electrons
• This results in a decreased electrostatic attraction between the nucleus and valence electrons.
  -This causes the distance between nucleus and valence electrons to increase making the atomic radius larger.

Question 5

Explain the periodic trend of electronegativity going across a period

Answer 5

Electronegativity increases going across a period.

-This is because nuclear charge increases, resulting in a stronger pull on the electrons towards the nucleus and a greater net electrostatic attraction.
- This decreases the atoms atomic radii and allows another atom to be closer to it. The closer the atoms are, the greater the attraction to electrons of the other atom, increasing electronegativity

Question 6

Explain the periodic trend of electronegativity going down a group

Answer 6

Electronegativity decreases going down a group.

-Both nuclear attraction and electron repulsion increase in step with an overall decrease in net electrostatic attraction.
-However, as sucessive energy levels increase atomic radii, electrostatic attraction of the nucleus together atoms decreases, so electronegativity decreases.