Chemistry Prep

Redox Reaction Definition

-a chemical reaction in which electrons are lost from one substance (oxidation) and added to another (reduction).
- oxidation and reduction always occur together.
- there is no net change of the number of electron

-short for Oxidation-Reduction

Nitrite (Nick the, -ite)

NO2(1-)

Carbonate (Camel had a)

CO3(2-)

Hydrogen/Bicarbonate (Camel had a, Hydrogen/Bi___ate)

HCO3(1-)

Chlorate (Clam for)

ClO3(1-)

Hydrogen Phosphate (Phoenix, Hydrogen/Bi___ate)

HPO4(2-)

Cyanide

CN(1-)

DMV Triangle (draw)

D = M/V

Gas Volume Triangle (draw)

Gas Volume (L or dm^3) = mol gas x molar volume (L/mol or 24dm^3)

Mass % Triangle (draw)

Mass % = Mass solute/Mass solution

Volume % Triangle (draw)

Volume % = Volume solute/Volume solution

Molarity Triangle (draw)

Molarity = mol solute/liters solution

Hydro- (element) -ic acid

+H, no oxygen, Binary acid

(ex. Hydrochloric Acid: HCl) (Polyatomic acids DONT INCLUDE HYDRO, ONLY BINARY ONES DO)

(element) -ic acid (acid version of -ate)

+H, normal oxygen

Base in reactions

A compound that produces OH- ions in water (Arrhenius definition);

a compound that accepts H+ ions (Brønsted-Lowry definition).

electron pair acceptor (Lewis)

these dissociate

Amount of specific substance (BU)

mole (mol)

Luminous intensity (BU)

candela (cd)

Length (BU)

meter (m)

Time (BU)

second (s)

Electric Current (BU)

ampere (A)

Mass (BU)

kilogram (kg)

SI Base Unit

the universal measurement system of basic units

Tera (T)

10^12

Giga (G)

10^9

Mega (M)

10^6

Kilo (k)

10^3

Hecto (h)

10^2

Deka (da)

10^1

Deci (d)

10^-1

Centi (c)

10^-2

Milli (m)

10^-3

Micro (u thing)

10^-6

Nano (n)

10^-9

Pico (p)

10^-12

SI Derived Units

a unit of measurement obtained by multiplication or division of different base units

NaCl or Sodium Chloride is typically a? (solute or solvent)

Solute

KI or Potassium iodide is typically a? (solute or solvent)

Solute

NaOH or Sodium Hydroxide is typically a? (solute or solvent)

Solute

NaF or Sodium Fluoride is typically a? (solute or solvent)

Solute

H20 or Water is typically a? (solute or solvent)

Solvent

CH3OH or Methanol is typically a? (solute or solvent)

Solvent

CH3CH2OH or Ethanol is typically a? (solute or solvent)

Solvent

When dealing with two compounds that are typically solvents

The larger compound becomes the solvent

Per________ate

+1 oxygen than normal

________ate

normal # of oxygens

________ite

-1 oxygen than normal

Hypo________ite

-2 oxygens than normal

Hydrogen/Bi________ate

+H, 1 charge closer to 0 than normal

Nick the Camel had Plums and Clam for Supper in Phoenix

First Consonant = Name of Ion,

The # of Consonants = # of Oxygens,

The # of Vowels = ion's negative charge

Nitrate (Nick the)

NO3(1-)

Perchlorate (Clam for, Cl is counts as one, +Per ate)

ClO4(-1)

Chlorite (Clam for, Cl is counts as one, -ite)

ClO2(1-)

Hypochlorite (Clam for, -hypo ite)

ClO(1-)

Sulfate (Supper in)

SO4(2-)

Sulfite (Supper in, -ite)

SO3(2-)

Hydrogen/Bisulfate (Supper in, Hydrogen/Bi___ate)

HSO4(-1)

Phosphate (Phoenix)

PO4(3-)

Phosphite (Phoenix, -ite)

PO3(3-)

Ammonium

NH4(1+)

Acetate

C₂H₃O₂(1-) or CH₃COO(1-)

Hydronium (strongest acid in aq. solutions)

H3O(1+)

Permaganate (Plums)

MnO4(1-)

Hydroxide

OH(1-)

Peroxide

O2(2-)

Particles Triangle (Draw)

Particles = Avogadro's # x mol

Molar Mass Triangle (draw)

Molar Mass = Mass/mol

Molar Concentration Triangle (draw)

Concentration = mol substance/ Liquid Volume (L)

Molality Triangle (draw)

Molality = mol solute / Kg solvent

Mole Fraction Triangle (draw)

MF A= mol A/total mol

Solution Chemistry Trio 1 (draw)

Solution Chemistry Trio 2 (draw)

General Mole Conversion Trio

Gas Laws Triangle (draw)

Molarity Problems: Mixture of Same Substance Solutions Concentration Equation

M1V1 + M2V2.... etc = M (V1 + V2...etc)

(ex. Two solutions of a substance are mixed in the following manner. 480ml(V1) of 1.5M first solution (M1), 520mL (V2) of 1.2M second solution (M2). What’s the final mixture (M)?

(1.5)(480) + (1.2)(520) = M (480 +520)

M= 1.344

Hypo- (element) -ous acid

+H, -2 oxygen than normal (-ic acid)

(element) -ous acid (acid version of -ite)

+H, -1 oxygen than normal (-ic acid)

Per- (element) -ic acid

+H, +1 oxygen than normal (-ic acid)

(element) -ol

-1H, +OH group (ex. Methane: CH4 -> Methanol: CH3OH)

Synthesis

A + B -> AB (elements/compounds combining to make a larger single compound)

Synthesis: To remember

1. Find oxidation #
2. If equally opposite, it yields a 1:1 ratio product; If not equal, remove current subscript then subscript swap using oxidation numbers to find product.
3. Balance

Decomposition

AB -> A + B (a compound breaking into two or more smaller substances)

Thermal Decomposition: What to look for?

Metal Carbonate Decomp.

Metal Carbonate —-heat—> Carbon Dioxide+ Metal Oxide

MgCO3 —heat—> CO2 + MgO

Metal Hydrocarbon Decomp.

Metal Hydrocarbon —-heat—> Water + Metal Oxide (ex. CaO)

(ex. Ca(OH)2) —heat—> H2O + CaO

Single Replacement

A + BC -> B + AC (elements & compounds)

(one element is substituted for another in a compound to make a new compound + a pure element)

Double Replacement

AB + CD -> AD + CB (Ionic compounds exchanging cations or anions to form new compounds)

Combustion

fuel + O2 -> H2O + CO2

(a fuel, usually a hydrocarbon reacts with oxygen gas to form carbon dioxide and water, generates heat & light in the process)

Combustion: What to look for?

Hydrocarbons (anything with C & H are often fuel sources)

And obviously O2 = other reactant

ex. C₂H₆O + 2O₂ → 3H₂O + 2CO₂

Neutralization (Type of Double Rep.)

Acid + Base -> H2O + Salt

Ionization

the process of adding or removing electrons from an atom or molecule, which gives the atom or molecule a net charge and forms an ion.

Acids do this by releasing protons H+

Arrhenius definition

Describes an acid as a compound that produces H+ or H3O+ (Hydronium) ions in water (increasing H+ concentration), and a base as a compound that produces OH- ions in water (increasing OH- concentration).

limited to only reactions that occur in water

Acid

A compound that produces H+ or H3O+ ions (cations) in water (Arrhenius definition);

a compound that donates H+ ions (Brønsted-Lowry definition).

electron pair donator (Lewis)

these ionize

lower the [H+] concentration, the weaker the acid (more basic)

In most, a hydrogen atom is bonded to a strongly electronegative element, like oxygen or one of the halogens (group/column 7).

Permanganate (Plums and)

MnO4(1-)

Synthesis/Reverse Thermal Decomposition

Metal Oxide + Carbon Dioxide → Metal Carbonate (Just reverse of Thermal Decomp.)

(ex. CaO +CO2 → CaCO3)

Molar Volume Triangle

Molar Volume = molar mass/density

Single Replacement: What to Look For Detailed:

Metal + MetalNonmetal → MetalNonmetal + Metal

(ex. Fe + CaCl2 → FeCl2 + Ca)

1. Swap

2. Subscript Swap to find first product

3. Left alone substance is the other product (balance if needed)

Nonmetal + MetalNonmetal → MetalNonmetal + Nonmetal

(Cl2 + NaBr → NaCl + Br2)

1. if there are two aqueous products swap them instead of metals

2. lone non-metal doubles

Metal + AcidNonmetal → MetalNonmetal + Hydrogen Gas (H2)

(ex. Zn + HCl → ZnCl2 + H2)

1. Same steps except, H doubles in products like the lone non-metal

Double Replacement: To Remember Detailed

Traditional (C = Cation, A = Anion)

M1NM1 + M2NM2 —>M1NM2 + M2NM1

(AgNO3 + MgCl2 → AgCl + Mg(NO3)2)

1. Metals

2. Subscript swap to find products (polyatomic ions stick together)

3. balance

Neutralization Double Rep

AcidNM1 + M2Base → M2NM1 (salt) + Water

(ex. H2SO4 + 2KOH → 2H2O + K2SO4)

1. If Hydrogen: H (Acid) is one of your metals and and hydroxide: OH (Base) is one of your non metalsthe product will yield water (H2O)

2. The other a salt from the other two reactants

Gas Evolution Double Rep

M1Carbonate(A2) + HydrogenNM2 → M1NM2 + Water + Carbon Dioxide

(ex. Na2CO3 + HCl → NaCl + H20 + CO2)

1. If Carbonate (CO3) and Hydrogen (H) are present in products they’ll form Carbonic Acid (H2CO3) which will decompose into Water (H2O) and Carbon Dioxide (CO2)

A Double Replacement Reaction that that yields a solid and an aq. from two aq. reactants is called a what?

Precipitation Reaction (Aqueous + Aqueous → Solid + Aqueous)

What does it mean if a Double Replacement reaction yields two aqueous solutions?

If a double replacement reaction doesn’t yield a precipitate (solid) there is NO REACTION

Neutralization (Type of Double Rep.): What to Look For

H (cation) + OH (anion) in products, swapping together to become H2O

(ex. H2SO4 (acid) + KOH (base) → H2O (water) + K2SO4 (salt))

Aqueous vs Liquid

Aqueous: A dissolved substance in a liquid (ex. Sodium Chloride or NaCl)

Liquid: natural fluid state of something at room temp (ex. Water or H2O)

Traditional Double Rep

Traditional

Cation1Anion1 + Cation2Anion2 —>Cation2Anion1 + Cation1Anion2

(AgNO3 + MgCl2 → AgCl + Mg(NO3)2

1. Swap Cations/Metals

2. Subscript swap to find products (polyatomic ions stick together)

3. balance