chem 101 test 3

Naming ionic compounds

cations are listed first, followed by anions in their ionic form, ending in "ide". Use proper suffix if applicable.

roman numeral after transition metal

denotes the positive ion charge

ammonium

NH4+

hydronium

H3O+

peroxide

O2 2-

hydroxide

OH-

acetate

CH3COO-

cyanide

CN-

azide

N3-

carbonate

CO3 2-

bicarbonate

HCO3-

nitrate

NO3-

nitrite

NO2-

sulfate

SO4 2-

hydrogen sulfate

HSO4-

sulfite

SO3 2-

hydrogen sulfite

HSO3 -1

phosphate

PO4 3-

hydrogen phosphate

HPO4 2-

Dihydrogen Phosphate

H2PO4 -1

perchlorate

ClO4 -1

chlorate

ClO3 -1

chlorite

ClO2 -1

hypochlorite

ClO-

chromate

CrO4 2-

dichromate

Cr2O7 2-

permanganate

MnO4 -1

polyatomic ion

Polyatomic ions are groups of covalently bonded atoms that carry a net electrical charge. When polyatomic ions bond with other ions, they form ionic compounds

'ate' vs. 'ite'

-ate has one more oxygen atom than -ite

'per' vs. 'ate' vs. 'hypo'

"per" means even more O than "ate"; and "hypo" means even fewer O than "ite"

Bonding within polyatomic ions

Within a polyatomic ion, there is covalent bonding. The Ionic bonds occur between the entire polyatomic ion and another ion

Mono

1

di

2

tri

3

tetra

4

penta

5

hexa

6

HEPTA

7

DECA

10

acid definition

an acid is a compound that will dissolve in water to form H+ ions and some anion. These H+ then form H3O+ with water. The H3O+ then are what determines the pH of any acid.

Strong acid versus weak acid

strong acids completely dissociate in water while weak acids only partially dissolve (some of the intact acid still remains)

HF

hydrofluoric acid

HCl

hydrochloric acid

HBr

hydrobromic acid

HI

hydroiodic acid

H2S

hydrosulfuric acid

Acetic Acid

HC2H3O2

nitric acid

HNO3

Nitrous acid

HNO2

Perchloric acid

HClO4

Carbonic Acid

H2CO3

Sulfuric acid

H2SO4

Sulfurous acid

H2SO3

Phosphoric Acid

H3PO4

Name/write all the strong acids and what being a strong acid means

HBr hydrobromic acid

HCl hydrochloric acid

HI hydroiodic acid

HNO3 nitric acid

HClO4 perchloric acid

H2SO4 sulfuric acid

All other acids in this class will be weak acids (they will only partially dissociate). These strong acids will entirely break down.

Bronsted definition of acids and bases - overview

acids are proton donors and bases are proton acceptors

Bronsted definition of acids

Acid: Proton donor B

• Will have an H somewhere in

the chemical formula that can

dissociate to form H+

• Not all things with H are

acids!!

• Usually, if the H is bound

to carbon, it is not an acidic H

• C2H4 is not an acid

• Some acids (H2SO4) can give

off more than one H. (only the

first one is strong, though!)

Neutralization Reaction

a reaction in which an acid and a base react in an aqueous solution to produce a salt and water

Strong Bases

a base that completely dissociates in a solution - figure out if u need to know these?

Precipitation reactions

dissolved substances (aq) react to form a solid. A precipitate will form when a substance's concentration exceeds its solubility

solubility

the extent to which a substance will dissolve in a solvent (often water)

double replacement reaction

two species (often salts) react to swap cations and anions

• acid/base reactions can also be double replacement

How do we know if a salt will be soluble or insoluble (i.e. form a precipitate)

use solubility rules (don't need to memorize)

spectator ions

any ions that are both aqueous before and after the reaction. They are not participating in the precipitation reaction, so can be eliminated to form the net ionic equation

Net ionic equation

the chemical equation with only the ions that are participating in the precipitation. The spectator ions are left out

chemical reaction

the process by which one or more substances change to produce one or more different substances. If two aqueous reactants form a solid, liquid, gas, as a product that needs to be included in the net ionic equation because that is a change into a different substance. Weak acids and bases need to be included in the net ionic equation bc they do not fully dissociate

Redox reaction

A chemical reaction involving the transfer of one or more electrons from one reactant to another

Oxidizing and reducing agents

opposite of what is oxidized/reduced. So if something is oxidized, it is the reducing agent because it is what enables the reduction.

write/review the rules for assigning oxidation states

do it

write/review the steps for balancing half reactions

do it

Bronsted definition of bases

Base: Proton acceptor

• Will often (but not always)

have OH somewhere in the chemical formula that can dissociate to form OH-

• Often alkali or alkaline earth metals with OH or (OH)2 - These are strong bases!

• NH3 is a common base that

does not contain OH-. Instead,

it performs the following

reaction in water:

NH3 (aq) + H2O(l) ’ NH4

• (aq

Difference between inter and intra molecular forces

inter is forces between molecules while intra is what holds molecules together

Intermolecular Forces (IMFs)

forces of attraction or repulsion between molecules

• This is what keeps solid and liquid gas molecules held togethe