U4 AP Chem

Chemicals Reactions

Oxidation

The substance becomes more positive, Loss of Electrons, reducing agent

Reduction

The substance becomes more negative, Gain of Electrons, oxidizing agent

Physical Change

Overcoming IMFS (Phase Change L

Chemical Change

bonds are broken and new bonds form, color change, formation of precipitate/gas, temperature change, Combustion, Rusting

Synthesis

A+B = AB

Decomposition

AB = A + B

Single Replacement

A + BC = B + AC

Double replacement

AB + CD = AD + CB

Combustion

fuel + O2 = CO2 + H2O + Energy

Precipitation

Double Replacement with Precipitate

Acid-Base

Double Replacement with H+ Transfer

Redox

electron transfer

Solubility Rules

All group 1 alkali metal ions, ammonium ion (NH4+), Nitrate ion (NO3

Acid

any substance capable of donating a proton (H+)

Base

any substance capable of accepting a proton (H+)

Generic Acid Equation

HA + H2O (l) = H3O + A

Strong Acid+base Equation

HCI => H+ + Cl

Strong Acids

HCl HBr HI HClO4 H2SO4 HNO3

Strong Bases

All group 1 + OH, All group 2 + OH

Weak Acid+base equation

HF + H2O = H3O+ + F

pH Levels

acid

Titrant

known concentration in buret

Analyte

unknown concentration in flask

Equivalence Point

When all the analyte has reacted, changes color

Oxidation Numbers

elemental form = 0, monatomic ion = charge on ion (Na+ = 1), group 1 metals in compounds = 1, group 2 metals in compounds = +2, F =