Unit 1 reviewBy: Makoto Bowering and Nick Ennen

Anions (has excess electron)–Has a negative charge

Most common-1 charge : H-, F-, Cl-, Br-, I-, OH--2 charge : O, O2, S-3 charge : N

Charges

Cations (has a less electrons)Has a positive charge

Most common1+ : H, Li, Na, K, Cs, Ag2+ : Mg, Ca, Sr, Ba, Zn, Cd3+ : Al

Charges

Covalent 2 non-metals

Ex: FOH2OCH4HCl

Bonds

Ionic1 metal and 1 non-metal

EX: NaClNaFMgO

Bonds

Metallic2 Metal

EX: DiamondBronzeCopper

Bonds

1 = meth- 2 = eth- 3 = prop- 4 = but- 5+ = a normal binary scale

Alcohols have suffix ol and are and O-H bond

Organic compounds

CH2OC= 40%H= 6.72%O= 53.28%Assume that the percent can be changed into grams and perform stoichiometry to get it to Moles. Once in moles divide by the lowest value to get the empirical forulma.

Percent composition

PV=NRT

P=Pressure (1.000 atm)V=Volume (L)N=MolesR=constant (0.08206 L*atm/Mol*K)T= Temperature (K = Tc + 273.15)

Universal Gas Law

STP-273.15 k1.00 atm1 mole of gas22.4 L

Standard temperature and pressure

(P+a(n/V)’2)(V-bn)= nRT

First part = The factor that the regular PV=nRT value is off because of the fact that IMFA was not included Second part =The factor that the regular PV=nRT value is off because it now does not include the molecules themselves

Real gas equation

P(molecule)=(n(a)/n(total))

Partial Pressure

This is the speed at which a molecule is moving.

Urms= 3RT/M (all under a square root sign)

M=Molar mass (Kg/mol)R= constant (8.314 J/Mol*K)T= Temperature (K)

Root-Means-Square Speed

The limiting reagent limits the reaction from producing the greatest it can. The limiting reagent runs out before the excess reagent does.

To find the value of the limiting reagent and excess reagent, all that is needed is stochiometery

Limiting Reagent

EX: A 2.00g sample of ammonia is mixed with 4.00g of oxygen. Which is the limiting reactant and how much excess reactant remains after the reaction has stopped?

Limiting Reagent

Step 1: write a balanced reaction

4NH3 + 5O2 4NO + 6H2O

Limiting Reagent

Step 2: finding which is limiting Use stoichiometry to calculate how much product is produced by each reactant. You can start with either reactant, and you can calculate for either product, but the product must be the same for both in order for the amounts to be compared.

Limiting Reagent

Step 3: finding the excess

To find the amount of excess reactant, we must calculate how much of the non-limiting reactant actually did react with the limiting reactant.

Limiting Reagent