Periodic Table Trends

Question 1

Atomic radius

Answer 1

Half the distance between the nuclei in a molecule consisting of two identical atoms

Question 2

Trends for atomic radii

Answer 2

Decreases going from left to right

Increases going down a group

Question 3

Ionization energy

Answer 3

Energy required to remove an electron from an atom in its gaseous states

Question 4

Why does the ionization energy increase as you keep on removing

Answer 4

The nucleus draws the electrons closer which makes the forces string which take more energy to remove

Question 5

What happens when all valence electrons are removed

Answer 5

You have to remove a core electron and the ionization energy increases tremendously

Question 6

Trends in ionization energy

Answer 6

Decreases as you go down a group: size of the orbital increase electrons move farther apart causes weaker attractions
Increases going left to right more strongly bound to nucleus as moving to the right

Question 7

Exceptions from ionization trends

Answer 7

Decreases going from Be to B because electrons in the final 2s orbital provide some shielding for electrons in 2p orbital
Decrease in ionization going from nitrogen to oxygen: extra electron repulsion from doubly occupied p orbital

Question 8

Electron affinity

Answer 8

Energy change associated with the addition of an electron to its gaseous state

Question 9

Trends for electron affinity

Answer 9

Becomes more negative going from left to right across a period

Question 10

Oxygen and electron affinity

Answer 10

The increase in oxygens nuclear number is sufficient to overcome the repulsion’s associated with putting a 2nd electrons into an already occupied 2p orbital