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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. Elements which have all electrons paired and relatively unaffected by magnetic fields
rate
r1/r2
insoluble
diamagnetic

2. Peak of energy diagram
solid CO2
Colligative properties
activated complex (transition state)
Root Mean Square Velocity

3. AX5E
allotrope
charge
iodide
square pyramidal

4. R in ideal gas law
Specific Heat Capacity
0.0821 atm L/mol K
n0
f

5. K
freezing
Equilibrium constant
Bond Energy
t-shape

6. 2+ charge
22.4L
Second-Order Rate Law
Alpha Particles-
Specific Heat Capacity

7. ?T=k*m(solute)
First-Order Half Life
Molal BP Elevation Constant
Acid Dissociation Constant
Buffered Solution

8. Mixing of gases
Diffusion
?Tf= kf x molality
Strong acid weak base rxn
Solubility Product (Ksp)

9. # bonding e- - # antibonding e-/2
# protons + # neutrons
Thermochemistry
Bond Order
viscosity

10. OIL RIG
condensation
Exothermic
freezing
Oxidation is Loss Reduction is Gain

11. Reactant which doesn't get used up completely in a chemical reaction
oct-
excess reactant
Ideal Gas Law
(moles of products that are gasses) - (moles of reactants that are gasses)

12. l=3
seesaw
standard solution
f
P1= X1P1°

13. Force that holds atoms together
tetrahedral
Faraday
Chemical Bonds
3.0x108m/s

14. (N) number of equivalents per liter of solution
Molecular Compounds
g solute/g solvent x 100
Boltzmann distribution
Normality

15. Ether prefix
3/2RT
viscosity
methoxy-
Closed System

16. AX4E
Reducing Agent
M1V1=M2V2
Closed System
see-saw

17. Raising heat - adding catalyst - heighten concentration - bigger surface area
methods of increasing rate
AH
Open System
different # of neutrons

18. A monoatomic anion is named by taking...
mol Fraction
LE Model
Its root and adding -ide
purple --> pink

19. Kinetic Energy per molecule
AE = q + w
Joule
Endothermic
1/2mv²

20. H+ Acceptor
Bronsted-Lowry Base
end point
l (second quantum number)
Anion

21. Driving force of the electrons
rate law
Molarity
Cell Potential (Ecell)
octahedral

22. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
alcohol
Law of Conservation of Mass
Reducing Agent
Kinetic Molecular Theory - for ideal gases

23. (organics) two carbons
Open System
r1/r2
catalyst
eth-

24. Forward rxn occurs when
Q<K
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
oxidizing agent
Molar Mass of Element/ Total Molar Mass %

25. 1/[A]=kt + 1/[A]0
end point
entropy
Integrated Second-Order Rate Law
bond energy

26. The weighted average of all the isotopes that an atom can have (in g/mol)
carbohydrates
Pi Bond
linear
Atomic Mass Unit

27. The chemical formed when an acid donates a proton
adiabatic
conjugate base
rate
Hund's Rule

28. A solid or gas that can be formed when 2 or more aqueous reactants come together
C=(mass)(specific heat)
0
precipitate
London dispersion forces

29. Mol/L - concentration of a solution
Density
Molarity
Trigonal Planar
octahedral

30. (organics) ten carbons
Endothermic
dec-
amine
condensation

31. Reverse rxn occurs when
E
Principal Quantum Number
Molecular Compounds
Q>K

32. Ptotal=P1+P2+P3+...

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33. Donates a single H+ Ion (... other prefixes also)
End Point
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
Monoprotic
Amino-

34. Carboxylic acid ending
q/moles
-oic acid
Theory of Relativity
base and hydrogen gas

35. Organic w/ -O-
0.0821 atm L/mol K
Valence Electrons(assigned)
ether
Boltzmann distribution

36. Increase Pressure
geometric isomers
alkyne
catalyst
Decrease Volume and Increase Temperature

37. AP doesn't deal with ...-order reaction - don't pick it!
third
purple --> pink
Volume Metric Flask & Pipet
sulfide

38. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
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
purple --> pink
moles solute/kg solvent

39. Phase change from solid to gas
Angular Momentum Quantum Number
sublimation
Pressure of H2O must be Subtracted
# protons (atom is defined by this)

40. Energy (definition)
Trigonal Bipyramidal
Arrhenius base
force x distance = work done
melting point

41. All cations are soluble with sulfate EXCEPT
chloride
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
deposition
Monoprotic

42. Everything in the universe that is not defined by you as part of the system
deposition
Surroundings
heat of vaporization
dec-

43. (organics) six carbons
hex-
n0
Covalently w/in themselves - Ionicly bonded w/ each other
Surroundings

44. 180° - sp
strong acid strong base rxn
Calorimeter
Linear
Its element

45. Reactant that's completely used up in a chemical reaction
Limiting reactant
Law of Conservation of Mass
log[H+]
meth-

46. The actual amount of product produced in an experiment
viscosity
cohesion
Hess's Law
experimental yield

47. x can be ignored when % ionization is <5%
London dispersion forces
Law of Conservation of Mass
5% rule
Lone Pair

48. Isotope
permanent gases
different # of neutrons
heat of fusion
Net Ionic Equation

49. Combined Gas Law Formula
P1V1/N1T1=P2V2/N2T2
Electronegativity
excess reactant
Tetrahedral

50. If needed - indicate charge of metal(cation) by...
M = square root (3RT/mm)
k=Ae^(-Ea/RT)
A Roman numeral
STP

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AP Chemistry

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