Chem 101 - unit 2 naming & electronegativity

CO₃ ^2-

carbonate

HCO₃ ^-

Hydrogen carbonate or bicarbonate

CH₃COO^-

acetate

CN^-

cyanide

SCN^-

Thiocyanate

CIO^-

hypochlorite

CIO₂^-

chlorite

CIO₃^-

chlorate

CIO₄^-

perchlorate

CrO₄^2-

chromate

Cr₂O₇^2-

dichromate

MnO₄^-

Permanganate

N₃^-

azide

NH₄⁺

ammonium

NO₂^-

nitrite

NO₃^-

nitrate

OH^-

hydroxide

O₂^2-

peroxide

PO₄^3-

phosphate

HPO₃^2-

hydrogen phosphate

H₂PO₄^-

hydrogren phosphate

S₂^2-

disulfide

SO₃^2-

sulfite

SO₄^2-

sulfate

HSO₃^-

hydrogen sulfite or bisulfite

HSO₄^-

hydrogen sulfate or bisulfate

CIO^-

hypochlorite

CIO₂^-

chlorite

CIO₃^-

chlorate

CIO₄^-

perchlorate

BrO

hyperbromite

BrO₂^-

bromite

BrO₃^-

bromate

BrO₄^-

perbromate

IO-

hyperiodite

IO₂^-

iodite

IO₃^-

iodate

IO₄^-

periodate

H and P ; EN value

2.1

C and S and I ; EN value

2.5

N and CI ; EN value

3.0

O ; EN value

3.5

F ; EN value

4.0

Se ; EN value

2.4

Br ; EN value

2.8

polarizable

ability for atom to create a temporary dipole

Zeff

magnitude of nuclear charge actually felt by electrons after shielding

As atom size decreases Zeff…

increase — shorter distance stronger pull from nucleus

As atomic size decreases atomic radius…

decreases

as atom size decreases polarizability…

decreases — atoms held more tight harder to move around/take away

as atomic size decreases lattice energy…

increases — held more tightly, creates a stronger attraction, with more negative Eel making greater lattice magnitude

lattice energy (LE)

energy released when oppositely charged gaseous ions come together to form an ionic solid

Electrostatic Potential Energy (Eel)

potential energy associated with attraction or repulsion between ions -- more negative means stronger attraction, more stable & less negative means weaker attraction, less stable — this is Q+ and Q-

Ranking lattice energies (LE)

1. look at charge and largest charge is most negative energy - smallest size, stronger attraction, more negative energy, more stable, more energy needed to separate ions

2. if same charge/electron number look who has the most protons -- most stable, smallest size

Ionization (IE)

amount of energy required to remove an electron from ground state in a gaseous state atom/ion —- equation is Mg(g) → Mg⁺ (g) + e- if second ionization Mg⁺ (g) → Mg²⁺ (g) + e-

as atomic size increases, Zeff decreases, IE …

increases — electrons closer to nucleus, attraction tighter together, more energy required to remove an electron

IE exceptions group 2 higher than group 13

electron in group 2 removed from s orbital and group 13 from p orbital which is easier to remove making group 2 have more energy

IE exception group 15 higher energy than group 16

group 15 has a 2p3 orbital which is harder to remove an electron from than group 16 2p4 orbital because they repel each other

electron affinity

energy required to add an electron from a ground state gaseous state atom/ion, no periodic table predictions— equation is Mg (g) + e- → Mg -

4 prefix

tetra

5 prefix

penta

6 prefix

hexa

7 prefix

hepta

8 prefix

octa

9 prefix

nona

10 prefix

deca

Assymetric stretch

IR active (greenhouse gas) — bc vibration with uneven stretch changes diapole

Symmetric Stretch

IR inactive — diapole doesnt change