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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.

1. Increase Pressure
8.31J/Kmol
Arrhenius Acid
London dispersion forces
Decrease Volume and Increase Temperature

2. ... compounds are most conductive
Weight
sulfate
Integrated First-Order Rate Law
ionic

3. Mol of solute/kg of solvent
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Law of Conservation of Mass
Hydrogen bonding
Molality

4. Driving force of the electrons
Law of Conservation of Mass
Cell Potential (Ecell)
Chemical Kinetics
Balmer Series

5. The total energy of the universe is constant - all systems tend towards minimum energy
1st law of thermodynamics
insoluble
isothermal
Le Chatelier's Principle

6. Kinetic Energy per molecule
Nernst Equation
A Roman numeral
1/2mv²
Limiting reactant

7. ?H when 1 mol of bonds is broken in the gaseous state
Bond enthalpy
Anode
+1 - except if bonded to Alkali Metal -1
carbonate

8. Variable for spin of electron (+.5 or -.5)
chlorite
s (fourth quantum number)
moles solute/kg solvent
red/orange

9. PO4³?
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Cell Potential (Ecell)
phosphate
hydrolysis

10. Group 2 metals
Alkaline earth metals
weak acid strong base rxn
Surroundings
Law of Conservation of Mass

11. Organic w/ -OH group
alcohol
Dalton's Law
Net Ionic Equation
Pauli Exclusion Principle

12. Work = ?
-(P)(Change in V)
Thermochemistry
London dispersion forces
Molar Mass of Element/ Total Molar Mass %

13. Only contains ions that change in reaction
0
Net Ionic Equation
Ampere
Law of Multiple Proportions

14. HF+ OH??H2O
weak acid strong base rxn
insoluble
P1V1/N1T1=P2V2/N2T2
Heat

15. Ptotal=P1+P2+P3+...

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16. CrO4²?
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
p
catalyst
chromate

17. Specific heat of water
4.184
endless
d
voltaic cells

18. When n=5 ->2 - color=
rate law
P1= X1P1°
spontaneous
blue-violet

19. Boltzmann constant - used in calculating speed of gas per molecule
Hund's Rule
1.38x10?²³J/K
deposition
Specific Heat (s)

20. Ketone suffix
-one
Law of Conservation of Mass
lambda
heat of vaporization

21. All cations are soluble with bromide - chloride and iodide EXCEPT
London dispersion forces
First-Order Half Life
Ag+ - Pb2+ - Hg2+
acetate

22. How to Balance a Redox Equation
adiabatic
Standard Temperature and Pressure
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
base and hydrogen gas

23. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change

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24. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Polar Covalent
-ous acid
oct-
n0

25. Group 1 and heavier Group 2 bases
Bond enthalpy
Anode
strong bases
Volume Metric Flask & Pipet

26. Ionizes to produce H+ ions
Molarity
Quantum Numbers
viscosity
Arrhenius Acid

27. Moles of solute/volume of soln(L)
Molarity
Delta H or Enthalpy Change
0 degrees C - 1 atm
8.31J/Kmol

28. Occupies the space above and below a sigma bond
Molarity
Pi Bond
M = square root (3RT/mm)
boiling point

29. The line running between the atoms
l (second quantum number)
Molality
Sigma Bond
Acid Dissociation Constant

30. The reactant in the oxidizing reaction that forces the reduction reaction to occur
rate law
Amino-
Reducing Agent
Graham's Law

31. (msubs) Can only be +1/2 or -1/2
rate law
red
Electron Spin Quantum Number
C + 273

32. SO4²?
supercritical fluid
first
Molecular Orbitals (MOs)
sulfate

33. Speed per molecule of gas
octahedral
-ic acid
-oate
v3kT/m

34. How to Find an Empirical Formula Given Grams
Specific Heat Capacity
-oic acid
Dipole-dipole forces
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

35. Has values from 0 to (n-1); tells shape of atomic orbitals
reduction agent
-2 - with peroxide -1
P1= X1P1°
Angular Momentum Quantum Number

36. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
Bond Order
Root Mean Square Velocity
v3RT/M(in kg)
complex ions

37. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
0.512°C
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Resonance

38. Absorbs/takes in heat (positive value)
square pyramidal
Multiplying
alcohol
Endothermic

39. Substances that form H+ when dissolved in water; proton donors
Increase Temperature
Acids
specific heat
Bronsted-Lowry Base

40. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Naming Binary Ionic Compounds
Calorimeter
Standard Temperature and Pressure

41. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
LE Model
Molecular
Faraday
Metalliods

42. pH=
Surroundings
log[H+]
London Dispersion Forces
double bond

43. Energy required for liquid?gas
heat of vaporization
chloride
blue
sulfate

44. r=k[A]
2nd law of thermodynamics
heat capacity
First-Order Rate Law
Nodes

45. How to Find a Weighted Average
# protons (atom is defined by this)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Second-Order Half Life
first

46. A solution that resists a change in pH - contains both a weak acid and its conjugate base
iodide
Buffer
Arrhenius Acid
indicator

47. AX6
6.63x10?³4Js
octahedral
-(q of H2O + q of cal)
q/moles

48. Non-Ideal Gas Conditions
Law of Conservation of Mass
Ionic
Equilibrium constant
high pressure - low temperature

49. ln[A] vs. time is a ...-order reaction
Nodes
force x distance = work done
first
Strong acid weak base rxn

50. AP doesn't deal with ...-order reaction - don't pick it!
third
3rd law of thermodynamics
actual yield/theoretical yield x 100%
N=N.(0.5)^time/time half-life