Chapter 2 Periodic Table

Question 1

oxidation states

Answer 1

charges when forming bonds with other atoms

Question 2

Why are metals good conductors?

Answer 2

• valence electrons are loosely held to their atoms, free to move…. conduct heat and electricity

Question 3

why are non metals poor at donating electrons?

Answer 3

• high ionization, electron affinities, electronegativities
  0 small atomic radii and large ionic radii
• poor conductors of heat and electricity

Question 4

Effective nuclear charge (Zeff)

Answer 4

• electrostatic attraction between valence shell electrons and the nucleus
• measure of net positive charge experienced by the outermost electrons
• increases on periodic table, from left to right

Question 5

principal quantum number

Answer 5

• increases from top to bottom
• valence increased separation from the nucleus
• results in a reduction in electrostatic attraction between the valence electrons and the nucleus

Question 6

Atomic radius

Answer 6

• increases going down and decreases from left to right

Question 7

ionization energy

Answer 7

• energy required to remove an electron from gaseous species
• endothermic (required heat)
• increases from left to right and bottom to top

Question 8

first ionization energy

Answer 8

• energy necessary to remove the first electron
• Mg (g) –> Mg+ (g) + e-

Question 9

second ionization energy

Answer 9

• energy necessary to remove the second electron from the univalent cation (X+) to form the divalent cation (X2+)
• Mg+ (g) –> Mg2+ (g) + e-