Quiz 1

Question 1

List the principal quantum numbers

Answer 1

n, l, ml, ms

Question 2

n

Answer 2

1, 2, 3, 4...
Energy level (the 2 in 2s)

Question 3

l

Answer 3

determines the shape of the orbital
0 = s
1 = p
2 = d
3 = f

Question 4

ml

Answer 4

the range of integers between positive and negative orbital shape.
+l … 0 … -l

Question 5

ms

Answer 5

spin: either +.5 or -.5

Question 6

Molecular Shapes

Answer 6

Linear
Trigonal Planar
Tetrahedral 
Trigonal Bi-pyramidal 
Octahedral

Question 7

Atomic Radii trend

Answer 7

Bottom left is best

opposite of ionization energy

Question 8

Ionization Energy

Answer 8

Top right is best, which means bottom left are more reactive elements.
IE is the amount of energy needed to pull off electrons. First group just gives em up.

Question 9

Electron Affinity

Answer 9

Amount of energy released when an electron is added to a neutral atom. More negative (energy released) as you move right across table.

Question 10

Electronegativity

Answer 10

Highest in top right corner of table (ignoring noble gasses)
Measure of the tendency of an atom or molecule to attract electrons.
If EN is similar, a bond is more likely

Question 11

Gerade

Answer 11

Sigma bonding

Pi anti-bonding

Question 12

Ungerade

Answer 12

Sigma anti-bonding

Pi bonding

Question 13

Node types

Answer 13

Angular node:
S has none
P has 1
D has 2

Radial node:
4D has 1

Question 14

Polarizeability

Answer 14

Large and charged are highly polarizeable

No noble gas configuration helps

Question 15

Bonding MO vs Non-bonding MO

Answer 15

bonding is lower in energy

Question 16

Bond Order

Answer 16

used to determine number of bonds in product
(Bonding - AB) / 2

A higher bond order means more bond energy and shorter bond length