Unit 4 Ap chem notes study guide

metals have low or high ionization energy?

low ionization energy

non metals

Electronegative: Form anions by gaining electrons

non metals have low or high ionization energy?

high ionization energy

chemical properties of non metals

react with metal → anions ( gains electrons)

metallic character decreases ( right or left?)

right

metallic character increases ( up or down ?)

down

if IE goes down, what happens to the electrons?

more likely to lose electrons

what is the most metallic element on the PT?

Fr (francium)

non metallic character increases ( right or left?)

right

non metallic character decreases ( up or down?)

down

if IE increases, and EA is more negative (increases) going right, what is going to happen to the electrons?

Most likely to gain electrons

most non metallic element?

F ( Fluorine)

EA increases ( right or left?)

EA right

EA decreases ( up or down?)

down

energy change when an atom gains an electron to form a ( positive or negatively??) charged ion

negatively

is it endothermic or exothermic If it gains energy?

endothermic

is it endothermic or exothermic If it loses energy?

exothermic

metals have high or low EA??

low EA ( loses electrons)

non metals have a high or low EA

high EA ( gains electrons)

If it gains protons, then the nuclear charge (increases or decreases??)

increases, easier to accept an electron

Zeff increases moving ( left or right) because there is a (weaker or stronger) attraction between the valence electrons and the nucleus as the atomic radius decreases

right; stronger

zeff fourmula

Zeff=Z-S

z= actual nuclear charge

s= charge screened by other electrons

Electron-nucleus attraction effects:

small atom, high IE, large electron affinity

Electron-electron repulsion effect

large atom, small IE, small or 0 electron affinity

atomic radii increases ( upwards or downwards?)

downwards

atomic radii decreases ( going left or right??)

going right

most electronegative element?

F; draw electrons towards itself when bonded

least electromagnetic

Cs; give away electrons when bonded

IE decreases what else increases…

number of shells and and AR increases, requires less energy to remove an electron

If IE increases what happens?

nuclear charge increases and more energy required to remove electrons ( charge increases so more ionization energy in periods left right)

IE increases form left to right ( true or false)

true

IE decreases from top to bottom ( true or false)

true

if a core electron is removed, what happens to the IE?

it is high/ increases

Large jump in the energy given = move to a

different shell ( moved to core electrons)

cations: (subtract or add electrons in reverse filling order)

subtract

Anions : (subtract or add in reverse filling order)

add

Transition metal cations: (subtract or add) from highest n-value orbitals

subtract ( in the beginning)

cations have a (larger or smaller atomic radius?

smaller atomic radius

anions have a smaller or larger atomic radius

larger atomic radius

Pauli’s Exclusion Principle:

each electron within any orbital has its own magnetic spin of either N or S

Aufbau Principle

electrons in ground state of the atom will occupy the lowest energy orbitals first, and only fill the higher energy orbitals when no lower energy orbitals are left

Hund’s Rule

electrons fill into empty orbitals within the same sublevel before they double up

Electrons remain as far as possible from each other by occupying different orbitals