Unit 1 review
Download
Report
Transcript Unit 1 review
Unit 1 review
By: Makoto Bowering and Nick Ennen
Charges
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 common
1+ : H, Li, Na, K, Cs, Ag
2+ : Mg, Ca, Sr, Ba, Zn, Cd
3+ : Al
Bonds
Covalent
2 non-metals
Ex:
FO
H2O
CH4
HCl
Bonds
Ionic
1 metal and 1 non-metal
EX: NaCl
NaF
MgO
Bonds
Metallic
2 Metal
EX: Diamond
Bronze
Copper
Organic compounds
1 = meth2 = eth3 = prop4 = but5+ = a normal binary scale
Alcohols have suffix ol and are and O-H bond
Percent composition
CH2O
C= 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.
Universal Gas Law
PV=NRT
P=Pressure (1.000 atm)
V=Volume (L)
N=Moles
R=constant (0.08206 L*atm/Mol*K)
T= Temperature (K = Tc + 273.15)
Standard temperature and pressure
STP273.15 k
1.00 atm
1 mole of gas
22.4 L
Real gas equation
(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
Partial Pressure
P(molecule)=(n(a)/n(total))
Root-Means-Square Speed
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)
Limiting Reagent
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.