Test 2 - Ch 7, 8, 9

Question 1

periodic trend - ionization energy

Answer 1

ionization energy increases up and right

(same as electronegativity and electron affinity; opposite of atomic radius)

Question 2

periodic trend - atomic radii

Answer 2

atomic radius increases bottom left (opposite of electronegativity)

Question 3

periodic trend - electron affinity

Answer 3

electron affinity increases up and right

(same as electronegativity and​ ionization energy; opposite of atomic radius)

Question 4

periodic trend - reactivity

Answer 4

reactivity increases left (towards metals!), overall

for metals, it also increases down; for non-metals, it increases up

Question 5

the higher the frequency, the ___ the wavelength

Answer 5

shorter

Question 6

the lower the frequency, the ___ the wavelength

Answer 6

longer

Question 7

the higher the frequency, the ___ the energy

Answer 7

greater

Question 8

the lower the frequency, the ___ the energy

Answer 8

lower

Question 9

formula: relationship between the speed of light, frequency, and wavelength?

Answer 9

c = ℷ x ⱱ

speed of light = wavelength x frequency

Question 10

formula: relationship between energy, wavelength, and frequency?

Answer 10

E = h x ⱱ

(where h = Planck’s constant)

energy = Planck x frequency

and ⱱ can be represented as:

c / ℷ

Question 11

what is the speed of light, c ?

Answer 11

c = 3.00 x 10^8 m/s

Question 12

what do each quantum number represent?

Answer 12

• n* = principal quantum number; the coefficient
• l* = angular momentum; 0 for s, 1 for d, 2 for p, and 3 for f
• ml* = magnetic; the constraint of options from l
  (i. e., -1, 0, 1 for l = 1; -2, -1…2 for l = 2, and so on)
• ms* = magnetic spin; either + or - 1/2; determine by orbital diagram (i.e., paramagnetic or diamagnetic?)

Question 13

add a + charge, you’ve ___ electrons; add a - charge, you’ve ___ electrons

Answer 13

positive charge = lost electrons; negative charge = gained electrons (electrons are negative!)

Question 14

polar bond means…

Answer 14

1) covalent thing only; 2) over 2.0 difference in electronegativity; 3) think of it conceptually as one end of the bond is larger - one atom is “hogging” the shared electrons

Question 15

ionic bond: what’s happening?

Answer 15

1) it’s a metal and a nonmetal, 2) two atoms, one of which is more electronegative than the other, exchange (transfer) electrons, and the charges hold the atoms together

Question 16

covalent bond: what’s happening?

Answer 16

1) metal + nonmetal, 2) atoms with high electronegativities will not lose electrons (metals and nonmetals are on opposite sides of the table!), so instead they share electrons in order to reach a stable number of valence e-

Question 17

procedure to obtain formal charge?

Answer 17

formal charge = (the atom’s total # of valence e-, from table) minus (total # of lone e- in current scenario) minus (the # of bonds that atom has in current scenario)

Question 18

periodic trend - electronegativity

Answer 18

electronegativity increases up and right

(same as electron affinity and ionization energy; opposite of atomic radius)

Question 19

quantum numbers: worked examples

Answer 19