Lecture 4

Question 1

transition metals

Answer 1

elements with d orbitals in their valence (outer/bonding) orbitals

Question 2

atom bonding determination

Answer 2

outer nodes, lobes, and phases determine how atoms bond by overlapping their valence orbitals

Question 3

electron bonding determination

Answer 3

shape and orientation of outer orbitals determine electron bonding

Question 4

energy of s orbitals

Answer 4

• the highest electron density is away from the nucleus, w/ inner lobes and nodes depending on the principal quantum number
• E3s > E2s > E1s

Question 5

s, p, d orbitals in a H atom

Answer 5

• # of inner nodes is s > p > d
• s orbital extends further than p, which extends further than d
• # of inner lobes of electron density is opposite, countering the effects of differences in outer edge distance of the orbital
• Es = Ep = Ed

Question 6

s orbital

Answer 6

• no outer nodes

- surface of the sphere are all of the same phase

Question 7

p orbitals

Answer 7

• one planar node on nucleus, perpendicular to the orbital
• phases are opposite on opposite sides of the node
• along x, y, z axes

Question 8

d orbitals

Answer 8

• two planar nodes between lobes of electron density

- opposite lobes have the same phases

Question 9

Aufbau (building-up) Principle

Answer 9

add electrons to orbitals in order to lowest to highest orbital energy

Question 10

Pauli exclusion Principle

Answer 10

two electrons in the same orbital must have opposite spins

Question 11

Hund’s Rule

Answer 11

electrons don’t pair until all orbitals are occupied

Question 12

shape of atomic orbitals (AO)

Answer 12

orbitals of poly electron atoms have the same shape as H atom orbitals