Unit 7: Chemical Reaction Types

Characteristics of Strong Electrolytes

1. Completely ionize in solution

2. high conductivity as ions act as charge carriers

Strong Electrolytes: NaCl, Na2S, MgCl2, but not MgS (low charges)

Soluble Salts

Strong Electrolytes: HCl, HBr, HI, HNO3, HClO4, HClO3, & H2SO4 and what do they do?

Strong Acids: ionize into H+ and X- in aq solution

Strong Electrolytes: NaOH, KOH, Ba(OH)2,…group ½ elements with OH- and what do they do?

Strong Bases: ionize into X+ and OH- in aq solution

Characteristics of Weak Electrolytes

1. partially ionize in solution

2. have weak conductivity due to low presence of ions

Weak Electrolytes: all acids that aren’t strong (HF,HCN,HNO2)

Weak acids

Weak Electrolytes: all bases that are not hydroxide (NH3,CN-,NO2-,F-)

Weak Bases

Characteristics of Non-electrolytes and what type are they?

1. do not ionize in solution

2. no conductivity

3. polar covalent molecules

Oxidation, electrons are…

lost

Reduction, electrons are…

gained

Rules for Oxidation Numbers: Atoms in pure elements…

are equal to zero

Rules for Oxidation Numbers: atoms in simple ions…

are equal to their ionic charge

Rules for Oxidation Numbers: polyatomic ions/binary compounds

the more electronegative atom is assigned the number based on its common valence

Rules for Oxidation Numbers: Sum of oxidation in neutral molecule

is equal to zero

Rules for Oxidation Numbers: Sum of oxidation in polyatomic ions

is equal to the charge of the ion

Rules for Oxidation Numbers: all atoms of the element in a compound or ion

have the same oxidation number

Rules for Oxidation Numbers: group ½ atoms

Group 1: +1 

Group 2: +2

What are the steps for the half-reaction method?

1. Separate redox reaction into oxidation and reduction half-reactions

2. Balance number of atoms

3. Balance charges using electrons

4. Multiply using LCM to cancel electrons

5. Recombine half-reactions & cancel electrons

6. Cancel redundancies and check for atom/charge balance

Arrhenius Acid/Base Definition

Acid: generates H+ in an aq solution

Base: generates OH- in aq solution

Bronstead-Lowry Acid/Base Definition

Acid: H+ donor

Base: H+ acceptor

Redox reactions: How do you turn an acidic balance to a basic balance?

Move the #H2O to the left side, move #H+ to the right then replace H+ with OH-