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AP Chemistry

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Increase Pressure
p
ammonium
Decrease Volume and Increase Temperature
Balmer Series

2. STP
t-shape
first
0 degrees C - 1 atm
?Hvap

3. Ecell= E°cell -RT/nF x lnQ
% yield
Calorimetry
violet
Nernst Equation

4. Mixing of gases
mol Fraction
Open System
Diffusion
3rd law of thermodynamics

5. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Pauli Exclusion Principle
complex ions
Chemical Bonds
Polar Covalent

6. Change in moles (An) =?
Van't Hoff factor
phosphate
(moles of products that are gasses) - (moles of reactants that are gasses)
oxide gas and water

7. Elements on staircase on periodic table
sulfite
Linear
Metalliods
Theory of Relativity

8. The total energy of the universe is constant - all systems tend towards minimum energy
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
adiabatic
1st law of thermodynamics
zero

9. Moles of solute/volume of soln(L)
Molarity
-ol
Specific Heat Capacity
Bronsted-Lowry base

10. Reverse rxn occurs when
Q>K
pent-
CAT
Polar Covalent

11. Happens at lines in phase change charts
reduction
Second-Order Rate Law
Molality
equilibrium

12. How to Find an Empirical Formula Given Percentages
period
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
X of a = moles a/total moles
oxide gas and water

13. AX2E - AX2E2
3rd law of thermodynamics
?Tb= kb x molality
bent
exothermic

14. Formula used when diluting stock solution (to find amount of water or stock needed)
-(P)(Change in V)
M1V1=M2V2
Ampere
increasing

15. How to Find a Weighted Average
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Osmotic Pressure
Lone Pair
Heat Capacity (C)

16. (organics) seven carbons
Integrated Zero-Order Rate Law
hept-
vapor pressure
conjugate acid

17. Volume of gas @STP
22.4L
vapor pressure
activation energy
boiling point

18. Kinetic Energy per mol
3/2RT
Manometer
Faraday
Closed System

19. Substance being dissolved in a solution (lower [ ])
Heat Capacity (C)
Graham's Law
p
Solute

20. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Chemical Kinetics
Counterions
Galvanic Cell
Net Ionic Equation

21. [A] vs. time is a ...-order reaction
Electronegativity
Hund's Rule
deposition
zero

22. 0°C and 1 atm
C + 273
Lone Pair
STP
permanganate

23. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
Finding Empirical Formulas
AH
n (first quantum number)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

24. Effusion of a gas is inversely proportional to the square root of the molar mass

25. ln[A] vs. time is a ...-order reaction
first
Hybridization
Ionic Compounds
Positive work value; work done on system

26. Phase change from solid to gas
Bonding Pairs
CAT
sublimation
First-Order Half Life

27. Atoms combine in fixed whole # ratios
Law of Definite Proportion
Molar Mass of Element/ Total Molar Mass %
3/2RT
Law of Multiple Proportions

28. Boiling point - melting point - viscosity - vapor pressure - surface tension
Calorimeter
critical point
charge
effects of IMF

29. Energy needed to vaporize a mole of a liquid
?Hvap
ammonium
Dalton's Law
Antibonding Molecular Orbital

30. ... compounds are most conductive
exothermic
equivalence point
ionic
3.0x108m/s

31. IMF that occurs with FON
Volt
phosphate
Hydrogen bonding
6.63x10?³4Js

32. When n=6 ->2 - color=
-2 - with peroxide -1
4.184
Strong acid weak base rxn
violet

33. ClO3²?
green/yellow
chlorate
E
bent

34. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
Molecular Compounds
Angular Momentum Quantum Number
excess reactant
Temperature

35. Gain of electrons - decrease in oxidation #
rate
reduction
Temperature
sublimation

36. Oxidation # of Oxygen
fusion
ether
-2 - with peroxide -1
are not

37. kb of water
m (third quantum number)
0.512°C
entropy
-al

38. Mass #
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
Constant Volume
# protons + # neutrons
trigonal bipyramidal

39. Oxidation # of Polyatomic Ions
charge
Reducing Agent
like
Solution

40. H?+NH3?NH4
alcohol
Strong acid weak base rxn
Chemical Kinetics
weak acid strong base rxn

41. (organics) one carbon
meth-
Faraday
critical point
% yield

42. Consists of a complex ion - a transition metal with attached ligands - and counterions
oxide
Temperature
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Coordination Compound

43. Oxidation # of Ions
1st law of thermodynamics
Bronsted-Lowry acid
charge
Principal Quantum Number

44. Unit of electrical potential; J/C
0
Volt
Counterions
Alkali metals

45. Amount of gravitational force exerted on an object
Density
1 atm
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Weight

46. (organics) six carbons
boiling point
insoluble
hex-
Calorimeter

47. Ionizes to produce OH- Ions
chlorite
p+
Kinetic Molecular Theory - for ideal gases
Arrhenius Base

48. Oxidation # of Halogens
-1
g solute/g solvent x 100
equivalence point
Molar Mass of Element/ Total Molar Mass %

49. The reactant that is being reduced - brings about oxidation
cyanide
Reaction Quotient (Q)
oxidizing agent
Trigonal Bipyramidal

50. Thickness
-(q of H2O + q of cal)
d
k=Ae^(-Ea/RT)
viscosity