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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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1. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Heat Capacity (C)
Hydrogen bonding
hydrocarbons
Boltzmann distribution

2. If anion ends in -ate - acid name ends in...
actual yield/theoretical yield x 100%
-ic acid
+1 - except if bonded to Alkali Metal -1
electrolyte

3. Negative enthalpy - heat flows into surroundings
Anode
Isolated System
entropy
exothermic

4. Mixing of gases
Ampere
-one
e-
Diffusion

5. [A]=-kt + [A]0
freezing
# protons (atom is defined by this)
Integrated Zero-Order Rate Law
0 degrees C - 1 atm

6. NO3¹?
Molal BP Elevation Constant
nitrate
First-Order Half Life
cathode

7. Ester suffix
ammonium
8.31J/Kmol
lambda
-oate

8. Ionizes to produce OH- Ions
Arrhenius Base
Solubility Product (Ksp)
l (second quantum number)
96500

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

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10. Solution used in titration
non-
Chemical Kinetics
titrant buret
Delta H or Enthalpy Change

11. Aldehyde suffix
Positive work value; work done on system
Constant Volume
-al
Reaction Quotient (Q)

12. Passage of gas through tiny orifice
Effusion
Bond enthalpy
zero
Gamma Ray-

13. NH4¹?
Molecular
Aufbau Principle
cathode
ammonium

14. (A) - C/s
PV=nRT
fusion
% error
Ampere

15. Cation first - anion second
alkyne
Naming Binary Ionic Compounds
strong acid strong base rxn
0.0826Latm/Kmol

16. l=3
analyte
f
endless
First-Order Half Life

17. Molarity (M)
moles of solute/ L of solution
precipitate
Oxidation is Loss Reduction is Gain
AH

18. To find activation energy use the...
Arrhenius equation
permanent gases
v3kT/m
viscosity

19. Happens at lines in phase change charts
strong acids
0.0821 atm L/mol K
First-Order Rate Law
equilibrium

20. Larger molecules which have higher mass and therefore electron density have stronger...
Temperature
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
London dispersion forces
-(q of H2O + q of cal)

21. Chemical composition of dry ice
solid CO2
M1V1=M2V2
meth-
Hess's Law

22. 1 sigma bond
Bond Energy
heat of vaporization
single bond
m (third quantum number)

23. Variable for type of orbital
log[H+]
carbohydrates
l (second quantum number)
meth-

24. Group 1 metals
Alkali metals
Ideal Gas Law
M1V1=M2V2
Anode

25. In a given atom no two electrons can have the same set of four quantum numbers
X of a = moles a/total moles
hydroxide
geometric isomers
Pauli Exclusion Principle

26. The weighted average of all the isotopes that an atom can have (in g/mol)
chloride
-oate
Bronsted-Lowry acid
Atomic Mass Unit

27. Molecules' tendency to stick to one another
cohesion
conjugate acid
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

28. Phase change from gas to solid
AH
deposition
see-saw
Hess's Law

29. AX5
endless
Manometer
trigonal bipyramidal
period

30. Molality =
Law of Conservation of Mass
Multiplying
-oic acid
moles solute/kg solvent

31. Specific heat of water
k=Ae^(-Ea/RT)
supercritical fluid
4.184
Constant Volume

32. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Acid + Base --> Salt + Water
endless
catalyst
-one

33. AX4E
k=Ae^(-Ea/RT)
Electronegativity
seesaw
Molecular Compounds

34. Point at which liquid?gas occurs
boiling point
force x distance = work done
heat capacity
Bronsted-Lowry Base

35. Universal IMF for nonpolar molecules
Pressure
London dispersion forces
permanganate
melting

36. E?s fill the lowest energy orbital first - then work their way up
Law of Multiple Proportions
spontaneous
precipitate
Aufbau Principle

37. Delta H (AH) = ?
State Functions
q/moles
Zero-Order Half Life
mol Fraction

38. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Transition metals
Formal Charge
hydrolysis
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

39. Anything occupying space and with mass
Matter
deposition
entropy
voltaic cells

40. (organics) five carbons
complex ions
Endothermic
pent-
heat capacity

41. When n=5 ->2 - color=
Kinetic Molecular Theory - for ideal gases
Its element
blue-violet
hydroxide

42. R in ideal gas law
0.0821 atm L/mol K
viscosity
Barometer
P1= X1P1°

43. ?T=k*m(solute)
Dalton's Law
charge
Molal FP Depression Constant
-(P)(Change in V)

44. How to Balance a Redox Equation
PV=nRT
Balmer Series
Adding
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

45. Color of Ba (flame test)
trigonal bipyramidal
4.184
Negative work value; work done by system
green/yellow

46. If Q<Ksp
square planar
eth-
no precipitate forms
vapor pressure

47. 101 -325 Pa
Adding
1atm=?Pa
Integrated Zero-Order Rate Law
0

48. r=k
sulfate
Colligative properties
Zero-Order Rate Law
Octahedral

49. .69/k
Radioactivity
First-Order Half Life
dec-
alkene

50. Ketone suffix
octahedral
perchlorate
-one
eth-

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AP Chemistry

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