redox reaction, solubility rules, ap chem

oxidation, reduction, rules, examples, solubility rules

Nitrates and acetates rules

All nitrates (NO3-) and acetates (C2H3O2-) are always soluble

Group 1 (alkali metals) elements

G1 elements, or salts, are always soluble (K+, Na+, Rb+, etc.)

Ammonium

Ammonium (NH4+) is soluble

Halides

Chloride, bromide, and iodide salts are soluble. EXCEPTIONS: Ag+, Pb+2, Hg+2

Sulfates

Most sulfate salts are soluble. EXCEPTIONS: BaSO4, PbSo4, HgSO4, CaSO4

Hydroxide

Most hydroxide salts are only slightly soluble due to partial ionization.

Strong electrolytes

KOH, NaOH

Slightly soluble

Most chromides, sulfides, carbonates, chromates, and phosphates are only slightly solubleSolutio

Solution

Homogenous mixture

Solute

Being dissolved

Solvent

Doing the dissolving

What effects dissolving?

Nature of solute and solvent

Solvent key factors

Amount determines how much is dissolved (i.e. more solvent = more dissolved)

Temperature: colder, less dissolved

Type of solvent: polar and nonpolar (water= aqueous, alcohol=tincture)

Water acts as a universal solvent (polar covalent molecule, shape)

Polar

unevenly sharing electrons in bond (if electronegativity is outside the range of 0.5 of each other).

Nonpolar

Evenly sharing electrons in bond (if electronegativity is within the range of 0.5 of each other).

Why is the unequal distribution of charge important?

Strong water= ion attraction

Where are they located in the bond?

Electronegativity can answer this.

Hydration

Attraction of ions to the uneven charges of water

What happens to ionic compounds (M and NM) regarding solubility rules?

Break into ions (some more than others), allow electric current to flow through

What happens to covalent compounds (NM and NM) regarding solubility rules?

Dissolve as molecules, stay together

What happens to nonpolar and polar ions regarding solubility rules?

They don’t dissolve

Solubility vs. Ionization

S: the amount that dissolves

I: what happens when it dissolves/ how

Redox reaction: electrons

Are being transferred from one substance to another

something HAS to gain and something HAS to lose

Oxidation rules: natural state

When atoms alone + natural state (including diatomic), they have an oxidation # of 0

Oxidation rules: monotomic

Ions will have an oxidation numver equal to their charge (i.e. O = -2)

Oxidation rules: compounds

Compounds are neutral, oxidation numbers SUMS must be 0 (H20, H=+ and x by 2 ions present, O=-2, or FeCl3, Fe=-3, Cl=+3)

Oxidation rules: polyatomic ions

Must have an oxidation number of equal to their charge (i.e. NO3-, N=+5, O=-6 because -2 × 3 ions present and need to equal -1)

Oxidation rules: oxygen

Oxygen in a compound = -2, EXCEPTION: H2O2 (peroxide) where O is -1

Oxidation rules: covalent

H=+1 ALWAYS (due to protons present)

Practice: KMnO4 (oxidation)

K = +, MnO4 = -1 where Mn = +7, O=-2 × 4 = -8

Practice: H2CO3 (oxidation)

H=+ x 2, O=-2 × 3, C=+4

Practice: NO2 (oxidation)

N=+4, O=-2 × 2

LEO GER, or OIL RIG

Lose electrons oxidations, gain electrons reduction

Oxidation is lose, reduction is gain

Practice: 2NaCl => 2Na + Cl2

(state explicitly which is oxidation and reduction)

Na= +1

Cl=+1

products: Na: +2

Cl= -2

oxidized: Na

reduced: Cl

Practice: N2 + 3H2 => 2NH3

(state explicitly which is oxidation and reduction)

Term

N= 0

H=0

products: N: -3

H= +3

oxidized: H

reduced: N