Chemistry -- Final

Synthesis Reactions

Two compounds or elements form a compound:

A + B → AB

Decomposition Reactions

A compound decomposes into two or more elements or compounds:
AB → A + B

Decomposition of Binary Compounds

AB → A + B (Elemental products)

Decomposition of Metal Carbonates

Metal Oxide + CO2

Decomposition of Metal Hydroxides

Metal Oxide + H2O

Decomposition of Metal Chlorates

Metal Chloride + Oxygen

Decomposition of Acids

Non-metal oxide + H2O

Single Replacement

A cation in an equation replaces a cation bonded to an anion in a compound.
A + BC → B + AC

Double Replacement

The cations in each compound switch in the equation.
AB + CD → AD + CB

Combustion

A hydrocarbon burns in oxygen to produce CO2 + H2O
Ex: C8H8 + O2 → CO2 + H2O

Precipitation Reaction

In double replacement, a nonsoluble, solid product forms.

Net Ionic Equations

The removal of spectator ions from a precipitation reaction.

Redox Reactions

The transfer of electrons from chemicals

Oxidation

The loss of electrons in a redox reaction
EX: CL- → Cl

Reduction

The gain of electrons in a redox reaction
Ex: Na+ → Na

Limiting Reactant

A reactant that determines the amount of product produced.

Excess Reactant

The reactant left over after the limiting reactant has finished reacting.

Percent Yield

Actual Yield/Theoretical Yield x 100 = Percent Yield

Energy

The ability to do work or produce heat.

Potential Energy

Energy of chemical composition or position.

Kinetic Energy

Energy of Motion

Heat

Process of energy moving from cold to warm environments.

System

Area containing a thermochemistry reaction.

Surroundings

Everything other than the system.

Exothermic

Heat leaves from the system into the surroundings.

Endothermic

Heat is absorbed by the system from its surroundings.

calorie

One gram of water raised one degree celsius.

1 calorie

4.184 Joules

Joules

SI unit of heat

Specific Heat

The energy required to raise one gram of any substance 1 degree celsius.

Q

mCp Delta T

Delta T

Final temperature - initial temperature in degrees celsius.

Gas Properties

Gases take the shape and volume of their containers, have lighter and faster molecules, are easily compressed, and are less dense than solids and liquids.

Volume

Liters, mL

Pressure

Pascals, Torr, Atm, mmHg

mmHg/torr to atm

1 atm = 760 mmHg or 760 torr

Pascals to atm

1 atm = 1.01 × 10^5 Pascals or 101 KPa

Temperature

Celsius, Kelvin

Kelvin to Celsius

K = Celsius + 273

Dalton’s Law

P1 + P2 + P3 = Ptotal

Boyle’s Law

P1V1 = P2V2; Pressure is inversely related to volume.

Charles’ Law

V1T2 = V2T1; Volume is directly related to temperature.

Gay-Lussac’s Law

P1T2 = P2T1; Pressure is directly related to temperature.

Combined Gas Law

P1V1T2=P2V2T1

Ideal Gas Law

PV = nRT; Used when the number of moles is in a gas problem. Atm must be the pressure, Liters must be the volume, and T must be in Kelvin

Gas Constant R

0.0821 L atm/moles K

Graham’s Law

Rate 1/Rate 2 = SQRT(Molar mass 2/Molar mass 1);
Gases of lower molar mass diffuse and effuse faster than gases of higher molar mass.

1 mole

22.4 Liters

STP Values

T— 273 K
P— 1.0 atm

Solution

Homogeneous mixture of a solute in a solvent with tiny particles.

Colloid

Homogeneous mixture with medium-sized particles.

Suspension

Heterogeneous mixture with large particles; temporary

Electrolyte

A solution that conducts electricity.

Saturated

There is the maximum amount of solute to solvent in a solution; no more will dissolve.

Supersaturated

There is more solute than solvent; will not dissolve.

Unsaturated

There is less solute than solvent; appears dilute.

Miscible

A solution that will successfully mix

Immiscible

A solution that will not successfully mix.

Emulsion

Colloidal size droplets of one substance suspended inside another.

Emulsifying Agent

An agent that allows an emulsion to fully mix together or become miscible.

Molarity

The amount of moles of solute per Liter of solution.

Stock Solution Formula

M1V1=M2V2

Solubility

The ability of a solute to dissolve in a solvent; usually measured in grams solute per 100 grams water.

Solubility increases for solids

when temperature increases

When temperature increases in a gas

solubility decreases

Triple Point

The point at which all phases of a substance exist.

Acids Properties

• Taste sour

• Burn skin

• pH is less than 7

• Turns blue litmus paper red

• Reacts with metals

• Has more H+ than OH-

Bases Properties

• Taste bitter

• Slippery on skin

• pH is greater than 7

• Turns red litmus paper blue

• Do NOT react with metals

• Have more OH- than H+

Both Acids and Bases

• Conduct electricity

• Neutralize each other

Bronsted-Lowry Law

• Acids donate hydrogen ions

• Bases accept hydrogen ions

Conjugate acid

Substance that forms when a base receives a hydrogen ion, the reaction can be reversed by the donation of a hydrogen ion.

Conjugate base

Substance that forms when an acid donates a hydrogen ion, the reaction can be reversed by the acceptance of a hydrogen ion.

pH formula

pH = -log[H+]

pOH formula

pOH= -log[OH-]

[H+] formula

[H+] = 10^-pH

[OH-] formula

[OH-] = 10^-pOH

pH+pOH

=14.0

When does the concentration of hydrogen or hydroxide change?

When the multiplier of hydrogen or hydroxide ions is raised, the multiplier of the concentration is raised as well.