CHEM 101 Exam 2 Study CHUNK 2: Periodic trends

How many quantum numbers are there

4 quantum numbers

what are the names of the quantum numbers

principal quantum number, angular momentum quantum number,Magnetic quantum number, spin quantum number

principal quantum number

Indicates energy level

angular momentum quantum number

indicates sub level shape

Magnetic Quantum Number (ml)

indicates orbital orientation

spin quantum number

indicates electron spin

number of orbital / maximum electrons

s=1 p=3 d=5 f=7 / s=2 p=6 d=10 f=14

periods(rows)

indicates number of electron shells

groups(columns)

elements have similar properties

elements have same number of valence electrons

numbered 1-18

Blocks

group 1-2 = s orbitals

group 13-18 = p orbital

transition metals = d orbitals

lanthanides and actinides = f orbitals

group 1

alkali metals

alkali metals

most reactive

silver metals

reactivity increases down the group

Group 2

Alkaline Earth Metals

Alkaline Earth Metals

less reactive than alkali metals

reactivity increases down the group

group 3-12

transition metals

group 13

Boron Group

group 14

carbon group

group 15

nitrogen

group 16

oxygen

group 17

halogen group

Group 18: Noble Gases

noble gasses

noble gases

unreactive

Halogens

most reactive nonmetal

Trends for atmoic radius

across= decrease - nuclear charge increases added to same shell stronger pull on electrons

down = increases - more distance from nuclear so weaker pull

Ionic radius

cations

anions

cations = ionic radius

smaller than parents

lost elecronts

np+ < na

anions = ionic radius

larger than parent atmos

gained electrons

cl->cl

what element does not form ions

noble gases

ionization energy

across= increases - hold tight

down = decreases - dont hold tight

metals have low

non metals have high

noble gases have highest

Electronegativity

across= increases

down = decreases

most is F

least is group 1

noble = none

Metals reactivity

increases down a group

decreases across a period

Nonmetals

decreases down a group

increases across a group

nuclear charge

number of protons in nucleus

increasing across and down

stronger pull

shielding electrons

inner blocks outer

increases down a group

stays constant

distance from nucleus

increases down

decreases across

atomic radius

across - decreases

down - increases

ionic radius

across - varies

down - increases

ionization Radius:

across - increases

down - decreases

Electronegativity

across - increases

down - decreases

Metal Reactivity

across - decreases

down - increases

nonmetal reactivity

across - increases

down - decreases