AP Chem Unit 3 Review

Solution

Homogenous mixtures of 2 or more substances

What is the solvents abundance as compared to the solute in a solution?

The solvent always have the highest abundance

What

Solvents

Dissociation

When an ionic substance dissolves in water, the solvent pulls the individual ion from the crystal and solvates them

Electrolyte

Substances that dissociate into ions when dissolved in water

Solubility of non electrolytes

A non electrolyte may dissolve in water but it does not dissociate into ions when doing so

Solubility of strong electrolyte

Dissociates completely when dissolved in water

Strong electrolytes

Strong acids, bases, and ionic coumpounds

Strong Acids

HBr, HI, HNO3, HCLO4, HCLO3, HCL, H2SO4

Strong Bases

BaOH, CaOH, SrOH, and group 1 with OH

Weak Electrolyte solubility, what are weak electrolytes

Only dissociates partially when dissolved in water, weak electrolytes are weak acids and bases

What do soluble ionic compounds tend to be? are there exceptions?

Electrolytes

What do molecular compounds tend to be? Exceptions?

Non electrolytes, exceptions are acids and bases

What makes a substance more likely to be soluble in another substance

If the substances have more similar intermolecular forces(primarily London dispersion forces, dipole–dipole interactions, and hydrogen bonding), one substance is more likely soluble in another

What creates a polar bond?

Unequal electro negatives(atoms ability to attract shared electrons)

Are all molecules containing polar bonds polar? why

No because even if bonds are polar, the molecule can be nonpolar when the dipole vectors cancel each other due to symmetry.

How can you determine if there exists 2 types of dipoles on the exterior of molecule=polarity

Looking at the dipoles and molecule shape

The strength of what type of forces make it possible for ionic substances to dissolve in polar solvents?

Ion-Dipole interactions

What are ion-dipole interactions

electrostatic attractions between a fully charged ion and the oppositely charged end of a polar molecule, crucial for dissolving ionic compounds in polar solvents.

What are Dipole-Dipole interactions

Molecules that have permanent dipoles are attracted to each other

What is attraction like in a dipole-dipole interaction

The positive end of one is attracted to the negative end of another, and vise versa

when is dipole-dipole important

Only when the molecules are close to each other

What does higher polarity chemically change

It makes a higher boiling point

Dipole-dipole interactions experiences when H+ is bonded to N.O, or F are unsually strong

Hydrogen bonding

Metathesis(exchange) reactions

Double Replacement

What does a metathesis reaction produce

Precipitates

When are precipitates formed in metathesis

When one mixes, ions form compounds that are insoluble(precipitates)

Redox Reactions

Single displacement, combustion, synthesis, decomposition

What are redox reactions

Reactions that involve substances that are oxidized and reduced

When does oxidation reaction occur

When an atom or ion loses electrons

When does a reduction reaction occur

When an ion/atom gains electrons

For a substance that gains an electron and one that loses an electron, one cannot occur without the the other is true only for what type of reaction?

Oxidation-Reduction Reactions

What type of metathesis does not give the product expected

Gas forming reactions, expected product decomposes to give a gaseous product

What must all double replacement reactions have?

A driving force/reason why the reaction will go into completion

What is the driving force?

The removal of at least one pair of ions from a solution

What are the 3 driving forces?

Gas formation, precipitation, and electrolytes

What are the common gas forming reactions?

H2S: Any sulfide(salt of S²-), and any acid form H2S(g) and a salt.

CO2:Any carbonate(salt of Co3²-) and any acid forms CO2(g), water and a salt

SO2: Any sulfite(salt of SO3²-) and any acid forms So2(g), water and a salt

NH3: Any ammonium salt and any soluble strong OH- reacts upon heating to form NH3(g), water and a salt

Main things about Acids

Release H+

Both Arrhenius & Bronstead-Lowry

Strong acids completely dissociate

Weak acids only partially dissociate

Main things about Bases

Substances that increse the concentration of OH- when dissolved in water; Arrhenius

Proton-acceptors(Bronstead-Lowry)

Strong bases completely dissocate

Weak bases partially dissociate

What do acids and bases release in acid-base reactions?

Acids release H+ and bases release OH-

What do other ions in acid base reactions produce?

ionic salts

What is an acid base reaction called

A neutralization reaction

What should you do with strong acids/bases and weak acids/bases in reactions

Completely dissociate strong acids/bases, but don’t separate weak acids/bases

What happens in Bronstead-Lowry reactions?

Acids release H+ ions, bases accept H+ ions, but bases must have a place to put an H+, like a non-bonded pair of electrons.

What is a product of an acid, what about a base?

Conjugate base, bases produce a conjugate acid

When does an acid classify as an electrolyte

If it is strong

When does a base qualify as an electrolyte

If it is strong and soluble.

Properties of Acids

They are sour, and turn litmus paper red

Properties of bases

They are bitter and slippery, and make litmus paper blue.

Arrhenius acid

Substance that when dissolved in water, increases the concentration of H+ ions(hydronium, H3O+)

Arrhenius base

Substance that when dissolved in water, increases the concentration of OH-

Bronstead-Lowry acid

proton donor; it must have a removable H+

Bronstead-Lowry base

Proton acceptor; must have a pair of nonbonding electrons to accept an H+

What type of substance can both accept and donate protons(act as an acid and base)

An amphiprotic substance

What is titration

A volumetric analysis to determine concentration

Stoic point

The point of equivalence

what is the difference in moles of acid compared to base in an acid-base reaction

They are equal

Oxidizing agent

The reactant reduced

Reducing agent

Reactant oxidized

Oxidation rules

Elements=0(Fe, H2)

Hydrogen +1; except in metal hydrides(NaH), then it is -1

Oxygen=-2; except in peroxides(H2O2, O=-1)

Group 1=+1, Group 2=+2

In a compound, oxidation numbers must balance out to a net charge of 0.