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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. Expresses how the concentrations depend on time
Integrated Rate Law
(moles of products that are gasses) - (moles of reactants that are gasses)
Graham's Law
trigonal pyramidal

2. Where there are no electrons
Effusion
-ic acid
-ol
Nodes

3. An equilibrium expression
Solubility Product (Ksp)
oxalate
Nodes
-one

4. Amount of heat needed to change a system by 1°C
no precipitate forms
heat capacity
Hund's Rule
mol Fraction

5. Boiling point elevation formula
Heat
3rd law of thermodynamics
?Tb= kb x molality
Formal Charge

6. The line running between the atoms
van't Hoff Factor
square planar
Magnetic Quantum Number (ml)
Sigma Bond

7. If heat capacity isn't mentioned - you can assume that q of cal is = ?
Aufbau Principle
Molality
phosphate
0

8. (organics) double-bonded compound
sublimation
hydrocarbons
alkene
red

9. Heat capacity formula
C=(mass)(specific heat)
triple bond
Monoprotic
T-shape

10. AX5
trigonal bipyramidal
hept-
hydrocarbons
perchlorate

11. A measure of randomness or disorder
entropy
Integrated Second-Order Rate Law
phosphate
n0

12. (organics) single-bonded compound
Bases
alkane
sulfate
Amphoteric

13. We cannot simultaneously determine an atom's exact path or location
Heisenberg Uncertainty Principle
zero
LE Model
Molecular

14. Significant Digits of Conversion Factors
l (second quantum number)
allotrope
single bond
endless

15. (organics) triple-bonded compound
Q<K
alkyne
trigonal planar
ammonium

16. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
Atmospheric Pressure
deposition
trigonal bipyramidal

17. 90°&120° - dsp^3
Molarity
n (first quantum number)
Trigonal Bipyramidal
LeChatelier's Principle

18. Point at which solid?liquid occurs
melting point
paramagnetic
Its element
Ionic

19. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
second
supercritical fluid
anode
Arrhenius Base

20. Actual Yield/Theoretical Yield*100%
different # of neutrons
Percent Yield
0
0

21. Color of Sr (flame test)
viscosity
red
0.0826Latm/Kmol
Mass

22. Elements in groups 3-12
nitrite
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
Transition metals
C + 273

23. If Q>Ksp
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
96500
system
a precipitate forms

24. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Pressure
Colligative properties
effects of IMF
Tetrahedral

25. Equation to find Ea from reaction rate constants at two different temperatures
Kinetic Molecular Theory - for ideal gases
alcohol
Root Mean Square Velocity
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

26. negative ion
Heat Capacity (C)
First-Order Half Life
alkyne
Anion

27. Matter can't be created nor destroyed
96500
2nd law of thermodynamics
Law of Conservation of Mass
Resonance

28. Driving force of the electrons
vaporization
precipitate
Dalton's Law
Cell Potential (Ecell)

29. When n=5 ->2 - color=
nu
Multiplying
0 degrees C - 1 atm
blue-violet

30. 760mmHg/Torr
r1/r2
s orbitals
1atm=?mmHg/Torr
Molarity

31. R=
0.0826Latm/Kmol
Thermochemistry
Molar Mass of Element/ Total Molar Mass %
Dalton's Law of Partial Pressures

32. [A]=-kt + [A]0
dichromate
f
Integrated Zero-Order Rate Law
Equilibrium Expression

33. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
Cation
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
voltaic cells
van't Hoff Factor

34. Atoms with the same number of protons but a different number of neutrons
Isotopes
Q<K
Zero-Order Half Life
22.4L

35. Molecules' tendency to stick to one another
State Functions
critical point
cohesion
square planar

36. Pressure Units/Conversions
1 atm = 760 mmHg = 101.3 kPa
Polar Covalent
Volt
deposition

37. Aldehyde suffix
hydrolysis
-al
Joule
T-shape

38. H+ Acceptor
Bronsted-Lowry Base
hydrocarbons
q/moles
heat capacity

39. Measure of the change in enthalpy
Delta H or Enthalpy Change
-ous acid
phosphate - sulfide - carbonate - sulfate
eth-

40. The heat changed in a chemical reaction.
Molecular Orbitals (MOs)
Thermochemistry
Second-Order Rate Law
Ag+ - Pb2+ - Hg2+

41. 1/[A] vs. time is a ...-order reaction
oxide gas and water
second
M = square root (3RT/mm)
Root Mean Square Velocity

42. Resistance to flow
single bond
Boltzmann distribution
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
viscosity

43. Measure of the average kinetic energy of all the particles in a substance
Temperature
8.314 J/K mol
fusion
msAT

44. Raoult's Law - relations between vapor pressure and concentrations
2nd law of thermodynamics
LE Model
P1= X1P1°
red

45. (organics) eight carbons
precipitate
Hybridization
oct-
Acids

46. Average speed of gas
paramagnetic
Chemical Kinetics
v3RT/M(in kg)
Net Ionic Equation

47. Larger molecules which have higher mass and therefore electron density have stronger...
blue-green
condensation
London dispersion forces
q/moles

48. Temperature-pressure combination at which solid - liquid - and gas states appear
charge
solid CO2
triple point
Oxidizing Agent

49. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
Aufbau Principle
Constant Volume
strong acids
End Point

50. Energy required for liquid?gas
melting point
Aufbau Principle
heat of vaporization
lambda