Unit 1—eb-1—2011—Allison Hunt and Audrey Rabushka
Anion: has excess elctrons  negative charge
Cation: positive charge
Neutral Ionic Compounds: composed of metal cation with non-metal anion
-use simplest formula, net charge = 0
Acids: have H+ as cation, name based on anion
-ide anion, hydro__ic acid
-ate anion, __ic acid
-ite anion, __ous acid
Covalent compounds: composed of two non-metals
-farther left element written first in name except Flourine is always last and Oxygen is always last unless with
Flourine
Average Atomic Mass (from abundance):
75.78% 35Cl
24.22% 37Cl
34.969 amu
36.966 amu
M= (.7578)(34.969) + (.2422)(36.966)
M= 35.45amu
Istopic Abundance (from atomic mass): same equation, use x and 1- x as the percentages
Percent Compostion:
C6H12O6 = 180.155 amu
%C = 72.066 amu / 180.155 amu = 40.0%
%H = 12.095 amu / 180.155 amu = 6.713%
%O = 95.994 amu / 180.155 amu = 53.28%
Limiting Reactant Calculations:
Method A: use one reactant to find out how much of the other reactant is needed
Method B: use both reactants to show how much product is made
Kinetic-Molecular Theory:
-Gases consist of large numbers of molecules (or atoms) in continuous, random motion.
-These molecules have negligible volume compared to the total volume the gas occupies.
-There are negligible attractive or repulsive forces between these molecules.
-At constant temperature, the average kinetic energy of these molecules remains constant over time. (There is no net loss
of kinetic energy due to their collisions, which are perfectly elastic.)
-The molecules’ average kinetic energy is proportional to their absolute temperature. (Equipartitionof energy.)
Universal Gas Law: PV = nRT
-Pressure: 1.000 atm = 101.325 kPa = 101 325 Pa = 14.69 psi = 760.0 Torr = 760.0 mmHg
- Temperature = Kelvin = TC + 273.15
-R = 8.314 L*atm/mol*K
STP (standard temperature and pressure): 0oC and 1.00 atm, 1 mole of gas occupies 22.4 L
RMS Speed: u2= 3RT/M
-molecules’ average kinetic energy is proportional to absolute temperature
Partial Pressure: nA/ntotal = χA, if mixed in same container the toal pressure is the sum of the partial pressures
Effusion: escape into a vacuum
Diffusion: mixing into another gas
Rate A escapes / Rate B escapes = uA/uB = Square Root (MB / MA)
Real Gas Equation: (P + an2/V2) (V – bn) = nRT
-correction factor replaces pressure decrease caused by intermolecular attractions
-correction factor to remove space occupied by the gas atoms or molecules themselves