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Final Exam
Manchester Community College
92
Chemistry
Undergraduate 1
05/06/2011

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Cards

Term
2 Types of Matter
Definition
Pure & Mixtures
Term
2 Types of Pure Substances
Definition
Elements & Compounds
Term
2 Types of Mixtures
Definition
Homogenous & Heterogenous
Term
Physical Properties
Definition
Anything observed without changing the substance or forming new substance
Term
Chemical Properties
Definition
Observed through forming new substances
Term
A glass of milk souring is a _____ change?
Definition
Chemical change
Term
A ice cube melting is a _____ change?
Definition
physical
Term
Kilo-
Definition
10^3
Term
Centi-
Definition
10^-2
Term
Nano-
Definition
10^-9
Term
Deci-
Definition
10^-1
Term
Milli-
Definition
10^-3
Term
Founder of Modern Atomic Theory. formed the atomic theory, which states that all matter is composed of tiny, indestructible particles called atoms that are all alike and have the same atomic weight.
Definition
John Dalton
Term
JJ Thompson
Definition
discovered the electron and developed the plum-pudding model of the atom.
Term
used the results of his gold-foil experiment to state that all the mass of an atom were in a small positively-charged ball at the center of the atom.
Definition
Ernest Rutherford
Term
Father of modern chemistry. Law of Conservation of matter.
Definition
Antoine Levoisier
Term
Aristotle's Atomic Theory
Definition
Everything made of 4 elements: fire, water, earth and air
Term
Bond Involving electron sharing
Definition
Covalent
Term
Bond involving electron transfer
Definition
Ionic Bond
Term
Molar Mass
Definition
Add g/mol
Term
Atomic weight
Definition
amu
Term
% Composition
Definition
Part/Whole * 100= ___%
Term
Empirical formula
Definition
Simplest whole # ratio
Term
Steps of Stoichiometry
Definition
1. Bal Eqn
2. Convert moles (divide g by mm)
3. Compare moles given to moles unknown( unknown/given)
4. Convert to whatever
Term
(g)->moles
Definition
Divide by mm
Term
moles->particles
Definition
Multiply by Avogadro's #
Term
Precipitate Reaction
Definition
Often involve Ionic Compounds
X (aq)+ y(aq) -> Z(s)+A(aq)

Z is precipitate
Anions Pair with Cations
Unsoluble is precipitate (see rules)
Term
Acid Base Rxn
Definition
Forms salt and water
Term
LEO THE LION SAYS GER
Definition
Loss electrons oxidation
Gain electrons reduced
Term
Redox Rxns
Definition
Electron transfer...follow oxidation rules given (not in a compound # is 0)
Term
Pressure
Definition
=F/A
Term
Boyles Law
Definition
As P increases V decreases (INVERSE)
Term
Charles Law
Definition
as temp increases V increases
Term
Gay-Lusaac's Law
Definition
As Temp increases P increases
Term
Ideal Gas Law
Definition
PV=nRT
P= Pressure, V=volume, T=Temp (Kelvins only), n=moles, R=0.0821 liter·atm/mol·K
Term
1st Law of Thermodynamics
Definition
ΔE=work+heat loss
Term
Enthalpy
Definition
Heat(Q) at constant P
Term
Calorimetry
Definition
q=m.sΔT
q=heat, m=mass, s=specefic heat, ΔT
Term
Wavelength Eqn
Definition
c = λ × f
c=speed of light,λ=wavelength, f=frequency
Term
Max Plank
Definition
Said energy is Quantized
Term
Einstein
Definition
e=mc^2 and photoelectric effect
Term
Neils Bohr
Definition
Electrons orbit the nucleus
Term
Molarity
Definition
moles of solute/L of solution
or m=n/V (in L)
Term
Dilution
Definition
Decreases concentration not moles
Term
Acid
Definition
Proton Donator
Term
Base
Definition
Proton Acceptor
Term
Salts
Definition
Ionic compound of cation (NOT H) and anion (NOT OH- or O2-)
Term
Net Ionic Equation
Definition
Then, you break apart the soluble molecules into the two ions that are formed (one positive and one negative). You will have to use the solubility rules to do this, they can be found online. If something is insoluble, it should not be broken apart. Write the reaction out with all of the separated ions. This is called the Total Ionic Equation. Then, you simplify by canceling things out if they appear on both sides of the reaction, resulting in the Net Ionic Equation.
Term
Ionic Compounds do/do not exist as gases
Definition
Do not
Term
Normal Atmospheric Conditions
Definition
25 degrees C & 1 atm pressure
Term
Force
Definition
Mass x Acceleration
Term
Pressure
Definition
Force/ Area
Term
Manometer
Definition
Used to measure pressure of gases other than atmospheres
Term
Plasma V Gas
Definition
Charged / Not charged
vol is not def / vol not definate
compress / compress
Move in straight lines like pong
Term
Molar Mass
Definition
mass/mole M=m/n or rewritten as n=m/M
Term
PV=mRT/M
Definition
Term
Density=
Definition
M/V
Term
m/v=PM/RT
Definition
Term
D=PM/RT
Definition
Term
1 Mol of Gas at Rm Temp
Definition
22.4L
Term
Ideal Gas V Real
Definition
M but not v / m & v
dont attract or repulse / at high temps do not exhibit ideal behavior
same as above/hi Pressure real gases attract
Term
Heat
Definition
transfer of energy btw bodies
Term
Temperature
Definition
Measure of av KE
Term
1st law
Definition
change in E equals work plus heat loss
Term
DeBroglie
Definition
Waves can act like particles and particles like waves (Wave particle duality)
Term
Heisenberg
Definition
Uncertainty of the position of a particle in time-photon can bump into it
Term
Schrodinger
Definition
showed how particles transition from different waves, assigned quantum #s
Term
Quantum #s
Definition
1st tells main level, 2nd sub, 3rd Orbital, 4th Spin
Term
Mendelev
Definition
varied rows with similar prop. in different lengths, leaving blanks for undiscovered elements.
Term
Newlands
Definition
Created a 7x7 periodic table based on atomic mass not atomic #
Term
Alkaline elements
Definition
1st column except H
Term
Alkaline Earth
Definition
Second column
Term
Halogens
Definition
Second to last column 7a
Term
Noble Gas
Definition
Last column
Term
Atomic #
Definition
increases L to Right top to bottom
Term
Atomic radius
Definition
Increases right to left top to bottom
Term
Ionization energy
Definition
increases bottom to top and left to right
Term
Electronegativity
Definition
Increases bottom to top and left to right
Term
Lattice energy
Definition
Increases with charge (small distance is akin to higher lattive energy also)
Term
Single Covalent Bond
Definition
Longest weakest
Term
Triple covalent bond
Definition
shortest and strongest
Term
ABE
Definition
A: Central B: Bond E: Lone pair
Term
Exceptions to the Octet Rule
Definition
Having too few valence electrons to ever obtain an octet.

Hydrogen, Beryllium and Boron have two few valence electrons to ever obtain a full octet. See this.
Hydrogen can have at most 2 valence electrons after it shares its electron with another atom.
Beryllium will have 4 valence electrons after it has finished bonding.
Boron will have 6 valence electrons after it shares its valence electrons with other atoms.

2. Expanding the octet to have 10, 12 or 14 valence electrons instead of 8.

elements in periods 3, 4, 5, 6 and 7 can expand their octet to have 10, 12, or 14 valence electrons.
Term
Nuclear Reactors
Definition
Fission
Term
Hydrocarbons
Definition
Hydrogen and carbon (exceptions: CO2, CO, CN-1, Carbonates, Bicarbonates, CO3-2, HCO3-)
Term
Alliphatic Hydrocarbons
Definition
Alkanes, alkynes, cycloalkanes, alkenes
Term
Aromatic Hydrocarbons
Definition
Moth balls (napthalene). Atleast 1 benzene ring C6H6
Term
Alkanes
Definition
single bond between C. CnH2n+2
Term
Alkynes
Definition
1 triple bond btw carbon atoms. CnH2n-2
Term
Cycloalkanes
Definition
single bond between C atoms. CnH2n. ex butane in a ring is cyclobutane.
Term
Alkenes
Definition
at least one dbl bond btw c. CnH2n
Term
Naming Alkanes
Definition
Location-#of C+yl-Parent Name
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