Chem 1127 final review

Pure Substance

Consists of only one element or compound

Mixture

Consists of two or more different substances not chemically joined

Law of Definite Proportion

Given compound always contains exactly the same proportion of elements by mass

Law of Multiple Proportions

When two elements form a series of compounds, the ratios of the masses of the second element that combine with one gram of the first element can always be reduced to small whole numbers

Group 1 Ionic Charges

\+1

Group 2 Ionic Charges

\+2

Group 3 Ionic Charges

\+3

Group 4 Ionic Charges

\+4

Group 5 Ionic Charges

\-3

Group 6 Ionic Charges

\-2

Group 7 Ionic Charges

\-1

Group 8 Ionic Charges

0

Naming Compounds

1\. Ionic or molecular?

2\. Add -ide to end of second compound

3\. Roman Numerals (Ionic)

Insert roman numerals after transition metal to balance nonmetal charge

4\. Prefixes (Molecular)

No mono- for first element

Ionic

has a metal (everything left of staircase, not H, including Al)

Molecular

Two nonmetals (right of staircase and H)

Metalloids

On staircase, not Al

NH4+

Ammonium

SO4 2-

Sulfate

HSO4-

Hydrogen Sulfate

SO3 2-

Sulfite

NO3-

Nitrate

NO2-

Nitrite

PO4 3-

Phosphate

HPO4 2-

Hydrogen phosphate

H2PO4 2-

Dihydrogen phosphate

PO3-

Phosphite

CN-

Cyanide

SCN-

Thiocyanate

HCO3-

Hydrogen Carbonate

S2O3 2-

Thiosulfate

H3O+

Hydronium

OH-

HYdroxide

O2 2-

Peroxide

C2H3O2-

Acetate

ClO4-

Perchlorate

ClO3-

Chlorate

ClO2-

Chlorite

ClO-

Hypochlorite

CrO4 2-

Chromate

Cr2O7 2-

Dichromate

MnO4 2-

Permanganate

CNO-

Cyanate

CO3 2-

Carbonate

C2O4 2-

Oxalate

Hg 2+

Mercury (I)

NH3

Ammonia

H2SO4

Sulfuric Acid

HC2H3O2

Acetic Acid

HClO3

Chloric Acid

HNO3

Nitric Acid

HBrO3

Bromic Acid

H3PO4

Phosphoric Acid

HCl

Hydrochloric Acid

HClO2

Chlorous acid

HBr

Hydrobromic Acid

Percent Composition Approach

Grams of each element

Grams --> moles of each element

Ratio of moles (multiply to whole numbers)

= Empirical mass

Divide into given mass for Molecular mass

Precipitate

Insoluble ionic solid products of reaction

Double Replacement Reaction Form

AB + CD --> AD + CB

Precipitation Reaction

Double replacement reaction that occurs in aqueous solution and one of the products is insoluble

Solubility Rules

1\. Salts formed with group 1 cations and NH4+ cations are soluble. Exceptions for some Li+ salts.

2\. Acetates, nitrates, and perchlorates are soluble,

3\. Bromides, chlorides, and iodides are soluble.

4\. Sulfates are soluble except with Ca2+, Sr2+, and Ba2+

5\. Salts containing Ag, Pb, and Hg(I) are insoluble.

6\. Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble. Sulfides formed with group 2 cations and hydroxides formed with Ca, Ba, Sr, are exceptions.

Group 1 Name

Hydrogen and Alkali Metals

Group 2 Name

Alkaline Earth Metals

Group 17 Name

Halogens

Group 18 Name

Noble Gases

Groups 3-12

Transition Metals

Cation

Has lost electrons, positive charge

Anion

Has gained electrons, negative charge

Balanced Net Ionic Equation

1\. Write out reaction (use solubility rules, etc.) and balance.

2\. Split up (aq) compounds into ions.

\n 3. Cancel ions on both sides.

\n

Oxidation-Reduction Reaction

Chemical reaction that involves the transfer of electrons between two species. Any reaction where oxidation number of molecule, atom, ion, changes by gaining or losing an electron.

Rules for Oxidation States

1\. Oxidation number for atom is 0.

2\. Total oxidation states of all atoms in neutral species is 0..

For ion, is equal to ion charge.

3\. Group 1: +1; Group 2: +2

4\. Oxidation of fluorine in compounds is -1.

5\. Hydrogen is +1.

6\. Oxygen is -2.

7\. In binary metal compounds, group 17 elements have -1, group 16: -2, group 15: -3.

OIL RIG

Oxidation is loss (of electrons)

Reduction is gain (of electrons)

Oxidizing Agent

Ion or molecule that accepts electrons (is reduced)

Reducing Agent

Ion or molecule that donates electrons (is oxidized)

MaVa = MbVb

Acid solution required volume of base solution for neutralization.

Gay-Lussac's Law

P1/T1=P2/T2

Charles Law

V1/T1=V2/T2

Boyles Law

P1V1=P2V2

Avogadros Law

V1/n1=V2/n2

Combined Gas Law

P1V1/T1=P2V2/T2

K to Cº

K - 273.15 = C

Cº to K

C + 273.15 = K

Partial Pressures Total

Ptotal = P1 + P2 + ... Pn

Mole Fraction

Xa = moles of A / total moles in solution

Xa = Pa / Ptotal

Coffee cup calorimeter problems

∆Hrxn = Qrxn = Qcalorimeter = -mc∆T

Solve for Qcalorimeter and/or Qsubstance

∆Hº

Reaction of standard enthalpy change, preset pressure/temperature

∆Hrxn

Change of enthalpy of reaction

∆Hºrxn

Occurs at 25º C and 1 atm

∆H formula

∆H = ∆Hproducts - ∆Hreactants

∆Hf for Species in Natural State (i.e. N2)

0

Energy for Electron Transitions

E = -2.18 x 10E18 • (nf^-2 - ni^-2)

ml Definition

Orientation in Space

n Definition

Size of orbital

ms Definition

Magnetic Moment

l Definition

shape of orbital

n Possible Values

1, 2, 3, 4...

l Possible Values

0, 1, 2, 3...

ml Possible Values

\-l, ... -1, 0, 1, ... l

ms Possible Values

\+1/2, -1/2

Ionization Energy Trend

up and right

Atomic Radius Trend

down and left