Chemistry (Exam 4)

ionization energy trend

increases across a period and decreases down a group

ionization energy exceptions

groups 2 & 13 switch and groups 15 & 16 switch

What does l represent?

the shape of the orbit

What does n represent?

energy level

What does ml represent?

the orientation of the orbit

What does ms represent?

spin number

s sub-shell

l=0

p sub-shell

l=1

d sub-shell

l=2

f sub-shell

l=3

possible n values

any positive integer greater than 0

possible l values

0 to (n-1)

possible ml values

-l to l

possible ms values

1/2 or -1/2

What type of an orbital experiences penetration?

s orbitals, because they have no nodes at the nucleus

Aufbau Principle

electrons fill in lower energy levels first

Hund's Rule

electrons fill orbitals singly with parallel orbitals before pairing

electron configuration exceptions

chromium, copper, molybdenum, silver, gold

Zeff Trend

increases across a period, and decreases down a group due to shielding

electron affinity trend

increases across a period and decreases down a group

electron affinity trend exceptions

1 & 2 switch, 14 & 15 switch

atomic radius trend

decreases across a group and increases down a group

polarizability

decreases across a group and increases down a group

electronegativity trend

increases across a period, decreases down a group

lattice energy

increases with increasing ionic charge and decreasing ionic size

octet rule exceptions

boron (sometimes aluminum and beryllium), expanded valence shells, free radicals

expanded valence shells

atoms in or above row 3 can expand their valence shell to have more than 8 electrons

free radical

highly reactive species with one unpaired electron

wavelength and frequency are __________ proportional

inversely

electromagnetic spectrum in order of increasing wavelength

gamma rays, x rays, ultraviolet, visible light, infrared radiation, microwaves, radio waves

electromagnetic spectrum in order of increasing frequency

radio waves, microwaves, infrared radiation, visible light, ultraviolet, x rays, gamma rays

real gases behave most like ideal gases at

low pressure and high temperature

In the van der Waals equation, a

corrects for intermolecular interactions

In the van der Waals equation, b

corrects volume to account for non-negligible molecules

light's particle properties

quantized into photons

light's wave properties

diffraction, refraction

Bohr Postulates

1) Atoms revolve around the nucleus on fixed circular orbitals
2) Electrons can jump from one orbital to another, and emit or absorb energy when they do

Pauli's Exclusion Principle

no two electrons can have identical values for all four quantum numbers

paramagnetic

has unpaired electrons

diamagnetic

has no unpaired electrons

energy is emitted when

an electron moves from a higher energy level to a lower energy level

energy is absorbed when

an electron moves from a lower energy level to a higher energy level

electron affinity

the amount of energy released when an electron is added

ionization energy

the energy required to remove an electron