Final Test!

NH₄⁺

ammonium

CO₃²⁻

carbonate

ClO₃⁻

chlorate

ClO₂⁻

chlorite

ClO₄⁻

perchlorate

ClO⁻

hypochlorite

OH⁻

hydroxide

NO₃⁻

nitrate

NO₂⁻

nitrite

PO₄³⁻

phosphate

PO₃³⁻

phosphite

H₂PO₄⁻

dihydrogen phosphate

HPO₄²⁻

hydrogen phosphate

SO₄²⁻

sulfate

SO₃²⁻

sulfite

HSO₄⁻

hydrogen sulfate (or bisulfate)

HCO₃⁻

hydrogen carbonate (or bicarbonate)

CN⁻

cyanide

BrO₄⁻

perbromate

BrO₃⁻

bromate

BrO₂⁻

bromite

BrO⁻

hypobromite

IO₄⁻

periodate

IO₃⁻

iodate

IO₂⁻

iodite

IO⁻

hypoiodite

CH₃COO⁻ (or C₂H₃O₂⁻)

acetate

1

Mono

2

Di

3

Tri

4

Tetra

6

Hexa

7

Hepta

8

Octa

9

Nona

10

Deca

5

Penta

Bond Order

Number of bonds between 2 atoms

increases, decreases

As the bond order ____ the bond length _____

increases, increases

As the bond order ____ the bond energy _____

Formal Charge

(# of valence)-(#of bonds)-(# of lone electrons)=

Linear, 180

2 ED, 0 Non-bonding pairs

Trigonal Planar, 120

3 ED, 0 Non-bonding pairs

Bent,

3 Ed, 1 Non-bonding pair

Tetrahedra,l 109.5

4 ED, 0 Non-bonding pairs

Trigonal Pyramidal,

4 ED, 1 Non-bonding pairs

Bent, << 109.5

4 ED, 2 Non-bonding pairs

Trigonal Bipyramidal, 120, 90

5 ED, 0 Non-bonding pairs

SeeSaw

5 ED, 1 nonbonding pair

T-shape

5 ED, 2 nonbonding pairs

Linear

5ED, 3 nonbonding pairs

Octahedral 90

6ED, 0 non-bonding pairs

Square Pyramidal

6ED, 1 non-bonding pair

Square Planar

6ED, 2 non-bonding pairs

Central Atom

(A)BU

# of bonding ED

A(B)U

# of nonbonding/unbonding Eds

AB(U)

London Dispersion Forces

In “Induced dipole”, two particles will be attracted to each other weakly briefly. All molecules have this. Weakest IMF

Dipole-Dipole

Happens in polar molecules. Stronger than London, weaker than hydrogen

Hydrogen Bonding

Occurs when hydrogen is bonded to Nitrogen, Oxygen, or Fluorine. Strongest IMF within bonding of two nonmetals.

The higher the melting point

The stronger the IMF...

Ion-Dipole

Strongest IMF, occurs when a metal is bonded with a nonmetal.

sp

Linear Hybridization

sp^2

Trigonal Planar Hybridization

sp^3

Tetrahedral Hybridization

sp^3d

Trigonal Bipyramidal Hybridization

sp^3d^2

Octahedral Hybridization

1 sigma

Single Bond

1 sigma 1 pi

Double Bond

10^12

tera (T)

10^9

Giga (G)

10^6

Mega (M)

10^3

Kilo (k)

10^-1

deci (d)

10^-2

cent (c)

10^-3

milli (m)

10^-6

micro (u)

10^-9

nano (n)

10^-12

pico (p)

Intensive

Boiling Point, color, temperature, luster, hardness

Extensive

volume, mass, size, weight, length

isotopes

nuclides with the same atomic number but different mass number

unstable

All nuclei z> or equal to 83 will be ____, as well as Te (43)and Pm (61)

stable

Nuclides are most likely to be ____ if the isotope and atomic mass are close.

stable.

Nuclei with even numbers of protons and/or neutrons are more _____

c=speed of light=wavelengthxfrequency

Energy Equation

Cr [Ar] 4s^1 3d^5, Cu [Ar] 4s^1 3d^10

orbital anomalies

has all electrons paired

diamagnetic

has unpaired electrons

paramagnetic

Trends

Ionization Energy Exceptions

3A and 6A elements have lower IE than the 2A and 5A elements respectively

Group 1 Elements (Li, Na, K, Rb, Cs) and NH4, NO3, C2H3O2, ClO3

Always soluble

Most Group 17 anions (Cl, Br, I, F): Except with Ag, Hg2+, Pb2+, SO42-: Except with Ag, Hg2+, Pb2+, Ca2+, Sr2+, Ba2+

Usually soluble

CO32-, PO43-, CrO42-, S2-, (M(OH): Expect with Ba(OH)2, Sr(OH)2, Ca(OH)2

Usually insoluble

HCl, HBr, HI, HNO3, HClO4, HClO3, H2SO4

Strong Acids

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

Strong Bases

Oxidation

Loss of electrons by a substance

Reduction

Gain of electrons by a substance

+1,-1

Hydrogen is __ when paired with a nonmetal, and __ when paired with a metal