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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. Solution used in titration
Arrhenius base
titrant buret
0
non-

2. Boiling point elevation formula
Average KE = 1/2(mass)(average speed of all particles)
triple point
First-Order Rate Law
?Tb= kb x molality

3. If anion ends in -ide - acid name ends in
hydro-ic acid
96500
Manometer
deposition

4. (organics) single-bonded compound
soluble
alkane
eth-
London dispersion forces

5. Group 1 metals
cathode
Alkali metals
Law of Conservation of Mass
?Hvap

6. # bonding e- - # antibonding e-/2
Arrhenius Base
Hybridization
Bond enthalpy
Bond Order

7. Resistance to flow
oxalate
viscosity
heat capacity
Hund's Rule

8. A solid or gas that can be formed when 2 or more aqueous reactants come together
moles of solute/ L of solution
Hydrogen bonding
precipitate
trigonal pyramidal

9. Delta H (AH) = ?
q/moles
Constant Pressure
freezing
Valence Electrons(assigned)

10. Ionizes to produce H+ ions
trigonal bipyramidal
square pyramidal
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Arrhenius Acid

11. =vM2/M1
96500
Alkaline earth metals
r1/r2
Percent Yield

12. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
4.184
trigonal pyramidal
strong acids
hydrocarbons

13. Driving force of the electrons
Second-Order Half Life
k=Ae^(-Ea/RT)
Cell Potential (Ecell)
Buffered Solution

14. J/°Cmol or J/Kmol
paramagnetic
Molar Heat Capacity
exothermic
deposition

15. (organics) one carbon
3rd law of thermodynamics
First-Order Rate Law
2nd law of thermodynamics
meth-

16. Solid to gas
sublimation
PV=nRT
% error
0

17. 1/[A] vs. time is a ...-order reaction
second
Van't Hoff factor
g solute/g solvent x 100
Solvent

18. ?Hsoln=?H1+?H2+?H3+...
Pauli Exclusion Principle
Enthalpy of Solution
1st law of thermodynamics
high pressure - low temperature

19. Measure of the change in enthalpy
chloride
Atomic Mass Unit
Delta H or Enthalpy Change
First-Order Half Life

20. Color of Li (flame test)
0
sublimation
Effusion
red

21. Happens at lines in phase change charts
equilibrium
1 atm = 760 mmHg = 101.3 kPa
strong acids
Solution

22. Elements in groups 3-12
Transition metals
different # of neutrons
ammonium
Quantum Numbers

23. Does the same as equilibrium expression - except it uses initial concentrations
q/moles
red
Reaction Quotient (Q)
System

24. l=0
Linear
s
heat capacity
Van't Hoff factor

25. Donates a single H+ Ion (... other prefixes also)
Monoprotic
London dispersion forces
0.0826Latm/Kmol
4.184

26. Occupies the space above and below a sigma bond
octahedral
0
electrolyte
Pi Bond

27. Spectrum of light when an electron drops to energy level n=2
Hund's Rule
Balmer Series
Limiting reactant
r1/r2

28. (organics) double-bonded compound
Equilibrium constant
standard solution
Ionic Compounds
alkene

29. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
P of a =(X of a)(total pressure)
insoluble
Amino-
carbonate

30. Type of system in which the energy and mass may leave or enter
Volt
sublimation
Open System
-oate

31. pH=
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
1 atm = 760 mmHg = 101.3 kPa
log[H+]
t-shape

32. CO3²?
carbonate
oxidation
Chemical Bonds
strong bases

33. Molecules' tendency to stick to the container
8.31J/Kmol
(moles of products that are gasses) - (moles of reactants that are gasses)
adhesion
Reducing Agent

34. frequency symbol
Ideal Gas Law
paramagnetic
spontaneous
nu

35. Ionizes to produce OH- Ions
Closed System
a precipitate forms
Van't Hoff factor
Arrhenius Base

36. q cal = ?
CAT
Overall Reaction Order
entropy
charge

37. Puts H? into solution
Solute
Specific Heat Capacity
Arrhenius acid
melting point

38. Proton donors
trigonal bipyramidal
Atomic Mass Unit
adhesion
Bronsted-Lowry acid

39. Boiling point - melting point - viscosity - vapor pressure - surface tension
supercritical fluid
Endothermic
effects of IMF
sulfide

40. S²?
sulfide
square planar
zero
Integrated Zero-Order Rate Law

41. (organics) ten carbons
ammonium
dec-
q
Molar Mass of Element/ Total Molar Mass %

42. x can be ignored when % ionization is <5%
Reducing Agent
5% rule
a precipitate forms
Resonance

43. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Zero-Order Rate Law
reduction agent
Quantum Model
Molality

44. Mole Fraction
X of a = moles a/total moles
London dispersion forces
# protons (atom is defined by this)
adiabatic

45. Only contains ions that change in reaction
Adding
-(q of H2O + q of cal)
Net Ionic Equation
heat capacity

46. Energy (definition)
catalyst
System
force x distance = work done
melting point

47. We cannot simultaneously determine an atom's exact path or location
Hund's Rule
heat capacity
conjugate acid
Heisenberg Uncertainty Principle

48. Ether prefix
1atm=?mmHg/Torr
Hybridization
Finding Empirical Formulas
methoxy-

49. Pressure Units/Conversions
Q>K
geometric isomers
1 atm = 760 mmHg = 101.3 kPa
Temperature

50. Point where acid completely neutralizes base
Le Chatelier's Principle
equivalence point
Bond Energy
-oic acid