Studied by 2 peopleVSEPR
the repulsion of electron pairs which may cause different shapes.
Valance shell electron pair reduction, the repulsion of electon pairs surrounding an atom causes the pairs to be oriented as far apart as possible.
AXe Notation
A= element, X= # of atoms bonded to central atom, E= pair of unshared electrons.
Metallic bonds are
bonds between two metal atoms.
Ionic bonds are
attractions between oppositely charged ions (metal and nonmetal)
covalant bond
a chemical bond that involves the sharing of electron pairs between atoms. Two nonmetals.
Hydrogen bonds are
weaker molecule bonding. Involves Nitrogen, ,oxygen, and flourine. hydrogen bonding is weaker than an ionic or covalent bond
Group
A column on the periodic table (vertical, up & down) determines number of valance electrons
Period
A horizontal row of elements in the periodic table. Shows energy level.
octet rule
States that atoms lose, gain or share electrons in order to acquire a full set of eight valence electrons
duet rule
Hydrogen and Helium only want two electrons
Enthalpy
Measure of heat that is produced or absorbed in a chemicle reaction
Polar dissolves
polar
nonpolar dissolves
nonpolar
Bond strenght least to greatest
Hydrogen, Nonpolar covalant, polar covalant, ionic
Hydrogen bonds and Ice
The hydrogen bonds to the oxygen atoms. causing ice to form. allows ice to be less dense than liquid water.
1 calorie = ____ joules
4.184
1000 calories = ___ kcal
1 kcal
1000 Joules is _______________ KJ
1 kJ
1000 calories = __ Calories
1 Calorie
STP (standard temperature and pressure)
temp: 0 celcius = 273 kalvin. \n PRessure: 22.4 l \n 22.4 l =
Pressure, temperature, and volume relationships
When pressure goes up, volume goes down: \n volume goes up, temp goes up.
Daltons law of partial pressure
the total pressure exerted by a mixture of gasses is the same as the particle pressures of all the gasses present. pTotal = P1 + P2.
homogeneous solution
mixture (all parts look the same)
heterogeneous solution
A mixture in which different parts can be easily distinguished
aqueous solution
a solution in which water is the solvent
Solvent
Substance present in the largest amount
solute
other substances in the solution.
Titrations
method of finding normalty of adding another substance with a known molarity. NaVa = NbVb. If finding molarty, convert N to M before doing caluclation so the units are the same
Oxidization
Lose electrons (+)
Reduction
Gains electrons (-)
Arrenenius acid and base
Produces (H+) and (OH-)
Brownsted acid and base
Donates Protron(acid) and accepts protron(base)
what kind of compound is a salt
ionic compound
electronegativity trends on the perioic table are the same as
ionization energy
0-0.4
nonpolar covalent
0.5-1.7
polar covalent
1.8+
ionic
nonpolar covalent
electrons shared between nonmetals, often the same element (02), electronegativity differnece 0-0.4
polar covalent
unequal sharing of electrons between nonmentals, electronegativity difference 0.5-1.7
valance electrons
electrons in the outermost energy level, can be found based on group number on the periodic table
pauli exculusion principle
each orbital can have a maximum of 2 electrons and they must have opposite spins
hunds rule
if a sublevel has more than 1 orbital, then the electrons will not “pair up” until all the orbitals have one electron.
Atomic size increases
as you move left and down
ionization energy increases
as you move up and right
chemical activity in metals increases
as you move left and down
chemical activity in nonmentals increases
as you move up and right
electronegativity increases
as you move up and right
delta H
change in enthelapy
to calculate delta H
T Chart:
-take grams of element/compound in the problem
-take the molar mass of that compound
-Put one mole above the molar mass
-put the number of moles in the problem below and across the 1
-Put the delta H or KJ of heat above the number of moles in the problem
-multiply the numbers on top and divide each number in the bottom
specific heat capacity
Q (energy in J) = s (specific heat capacity) x m (mass in g) x (Tfinal-Tinital) (temperature in degrees c)
bond strength
amount of energy needed to break a chemical bond,
triple double single (greatest to weakest)
Hydrogen, Nonpolar covalant, polar covalant, ionic (weakest to greates)
Boyle’s Law
P1V1 = P2V2
inversley related, one goes up other goes down
temperature constant
Charels’s Law
V1/T1 = V2/T2
Directly related, one goes up other goes up
pressure constant
combined gas law
(P1V1)/T1 = (P2V2)/T2
ideal gas law
pv=nrt
r=0.08206, universal gas constant
Dalton’s Law Calculation
-Find number of moles of each substance using molar mass and t charts
-Find partial pressures of each using P = nrt/v
-Add the partial pressures together to find the total pressure
to find kelvin
add 273 to c
to find celcius
subtract 273 from k
concentrated
lots of solute in it
dilute
little solute in it
Molarity =
moles of soulute/liters of soultion
finding mass of the solution using molarity
times the volume by molairty
finding volume of the solution using molairty
divide the mass by the molarity
solubility
how much solute can complelty dissolve in a solvent
saturated
solution that has dissolved all the solute it can at a specific temperature
unsaturated
solution that has NOT dissolved all the solute it can at a specfic temperature
supersaturated
a solution that has more solute dissolved in it than normally possible at a given temperature
solubility usually increases as
the temperature of the solution increases
how to speed up the process of dissolving
-stir
-raise the temperature
-increase the surface area
Absolute zero
0 Kelvin
-273 Celcius
Acids
-H+
-taste sour
-Ph 0-6
-Proton Donor
Bases
-OH-
-taste bitter
-Ph 8-14
-Proton Acceptor
-Soapy/Slippery
the subscript of H or OH tells
if the acid or base is mono, di, or triprotic.
The larger the subscript, the more acdic or basic the substance will be.
Normality
moles of H or OH/liters of solution
if you already have the molarity
multiply by the mono, di, or tri for the normality (if given normality, divide by these to find molarity)
when doing oxidation and reduction problems
single elements = 0
compounds = charges on pink sheet
Balancing half reactions
2 products = oxidation (smaller to bigger)
1 product= reduction (bigger to smaller)
reactions occur when activation energy is
supplied by collisions
catalysts work by
lowering activation energy
be able to know and label this
exothermic energy diagram
be able to know and label this
endothermic energy diagram
exothermic energy
-detla H, heat is released
endothermic energy
+delta H, heat is absorbed
homogeneous equllibrilluim
substances that are present in the same physical state
heterogeneous equllibrilluim
involves substances in more than 1 physical state
noble gases are
not reactive
pressure
the constant bombardment of the walls of a container by the moving molecules of a gas
factors that affect the speed of a reaction
-nature of reactants
-temperature of reactants
-presence of a catalyst
Nuteralized subatances (H20 and salt)
have a ph of 7
Note 
Flashcard (29)