U1 - Trends of the Periodic Table

Question 1

•Atomic Radius

Answer 1

•Distance between the nucleus and valence e-

Question 2

•Effective Nuclear Charge (Zeff)

Answer 2

•Describes strength of attraction between nucleus and valence e-

Question 3

•Law of Electrostatics

Answer 3

• Unlike charges attract

* Like charges repel

Question 3

•Effective Nuclear Charge and Radius Size

Answer 3

• On the same period:
• More protons means greater Zeff
• Smaller radius
• More protons = Greater Zeff

Question 4

•Shielding Effect

Answer 4

• To decrease Zeff

* Number of filled orbitals between the nucleus and the valence e-

Question 5

•Shielding Effect, Effective Nuclear Charge, and Radius Size

Answer 5

• The greater the shielding effect, the weaker the Zeff, the larger the radius
• The weaker the shielding effect, the stronger the Zeff, the smaller the radius
• The shielding effect does not matter and more protons, stronger Zeff, smaller radius
• The shielding effect does not matter and less protons, weaker Zeff, bigger radius

Question 6

•Ionization Energy

Answer 6

•The amount of energy needed to remove a valence e-

Question 7

•Ionization Energy General Formula

Answer 7

• A = any element

* A + energy –> A (+) + e-

Question 8

•Ionization Energy, Zeff, Radius Size

Answer 8

• Larger radius = Less ionization energy
• Less Zeff = Less ionization energy
• Smaller radius = More ionization energy
• More Zeff = More ionization energy

Question 9

• 1st Ionization
• 2nd Ionization
• General Equation

Answer 9

•A = any element

• Amount of energy required to remove the 1st e-
• A + energy –> A (+) + e-
• Amount of energy required to remove the 2nd e-
• A (+) + ENERGY –> A (2+) + e-

•After loss of first e-, there will be less e- for the remaking e-, so increase in Zeff and increase in ionization energy

Question 10

•Ionization Energy Trends in the Periodic Table

Answer 10

• Left to right in a period = Increase in ionization energy

* Up to down in a group = Decrease in ionization energy

Question 12

•Electron Affinity

Answer 12

•The energy absorbed or released when an electron is added to a neutral atom

Question 13

•Electron Affinity Trends in the Periodic Table

Answer 13

• Left to right in a period = Increase in electron affinity
• Up to down in a group = Decrease in electron affinity
• Reversed for noble gases

Question 14

•Electronegativity

Answer 14

• The relative ability of an atom to attract shared electrons
• Value is found on the periodic table

Question 15

•Electronegativity Trends in the Periodic Table

Answer 15

• Left to right in a period = Increase in electronegativity

* Up to down in a group = Decrease in electronegativity

Question 16

•Electron Affinity General Formula

Answer 16

• A = any element

* A + e- –> A (-) + energy

Question 17

•Ionic Radius

Answer 17

•Comparing the radius of ions