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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. Different form of same element
-ol
5% rule
allotrope
Integrated Second-Order Rate Law

2. Where there are no electrons
Law of Multiple Proportions
Nodes
Amino-
Solution

3. This MUST be determined experimentally
rate law
chlorite
Pressure of H2O must be Subtracted
blue-green

4. If Q>Ksp
nitrite
a precipitate forms
3.0x108m/s
p orbitals

5. If needed - indicate charge of metal(cation) by...
A Roman numeral
-oate
Galvanic Cell
% error

6. Oxidation # of Polyatomic Ions
Quantum Mechanical Model
Heat
hydroxide
charge

7. (# of lone pair e-)+1/2(# of shared e-)
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Valence Electrons(assigned)
strong acid strong base rxn
group

8. Atoms with the same number of protons but a different number of neutrons
AE= AH - RTAn
Isotopes
are
Colligative properties

9. Speed per molecule of gas
bond energy
v3kT/m
viscosity
single bond

10. Where oxidation occurs
Anode
strong acids
?Tb= kb x molality
Pi Bond

11. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
Isolated System
not spontaneous
blue
Dipole-dipole forces

12. O²?
oxide
charge
endless
Barometer

13. l=1
p
Reaction Quotient (Q)
strong acid strong base rxn
octahedral

14. We cannot simultaneously determine an atom's exact path or location
methoxy-
Heisenberg Uncertainty Principle
0 degrees C - 1 atm
voltaic cells

15. Theoretical yield-experimental yield/theoretical yieldx100
k=Ae^(-Ea/RT)
2nd law of thermodynamics
phosphate
% error

16. 6.022x10^23
Amount of atoms present
adiabatic
mol
Oxidizing Agent

17. Point at which solid?liquid occurs
C + 273
l (second quantum number)
melting point
red

18. IMF that occurs with FON
Hydrogen bonding
Diffusion
Alkali metals
n0

19. Calculation from K to C
Volume Metric Flask & Pipet
T-shape
entropy
C + 273

20. These orbitals are spherical
Bronsted-Lowry Base
s orbitals
London Dispersion Forces
Average KE = 1/2(mass)(average speed of all particles)

21. The likelihood that a rxn will occur "by itself"
mol Fraction
spontaneity
Kinetic Molecular Theory - for ideal gases
oxidizing agent

22. Ether prefix
Ag+ - Pb2+ - Hg2+
viscosity
acid
methoxy-

23. How to Find an Empirical Formula Given Grams
mol Fraction
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Hybridization
8.31J/Kmol

24. Substance being dissolved in a solution (lower [ ])
Solute
Cathode
Antibonding Molecular Orbital
Enthalpy of Solution

25. Solid to gas
E
actual yield/theoretical yield x 100%
sublimation
conjugate base

26. U(rms)=(3RT/M)^1/2
System
system
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Root Mean Square Velocity

27. HF+ OH??H2O
q/moles
supercritical fluid
weak acid strong base rxn
Heat Capacity (C)

28. Oxidation # of Oxygen
d
-ic acid
-2 - with peroxide -1
Volume Metric Flask & Pipet

29. 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)
Kinetic Molecular Theory - for ideal gases
Alpha Particles-
amine
Ligand

30. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
excess reactant
Ligand
Scientific Method
base

31. If anion ends in -ite - acid name ends in...
double bond
Molecular Orbitals (MOs)
solid CO2
-ous acid

32. Atomic #
nu
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
# protons (atom is defined by this)
cyanide

33. A monoatomic cation takes name from...
Alkaline earth metals
Its element
Radioactivity
Molal FP Depression Constant

34. Substances that form OH- when dissolved in water; proton acceptors
First-Order Rate Law
p+
Bases
yellow --> green

35. #NAME?
Bonding Pairs
E
Law of Conservation of Mass
Negative work value; work done by system

36. =vM2/M1
r1/r2
1 atm
T-shape
moles of solute/ L of solution

37. ClO4¹?
third
hydrolysis
3/2RT
perchlorate

38. Ideal Gas Law Formula
diamagnetic
Sigma Bond
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
PV=nRT

39. q rxn = ?
-(q of H2O + q of cal)
Mass
red
-one

40. Point at which vapor pressure=air pressure above
Quantum Model
boiling point
oxalate
Law of Multiple Proportions

41. When n=4 ->2 - color=
n0
blue-green
boiling point
heat of fusion

42. The amount of energy/heat required to raise some substance 1 degree C
amine
acid
Heat Capacity (C)
Bases

43. Temperature-pressure combination at which solid - liquid - and gas states appear
(moles of products that are gasses) - (moles of reactants that are gasses)
triple point
C + 273
Arrhenius base

44. Point where acid completely neutralizes base
equivalence point
Joule
Solubility Product (Ksp)
dichromate

45. Donates a single H+ Ion (... other prefixes also)
eth-
Pauli Exclusion Principle
Monoprotic
different # of neutrons

46. 109.5° - sp^3
Tetrahedral
purple
sulfite
Boltzmann distribution

47. When n=5 ->2 - color=
Aufbau Principle
blue-violet
diamagnetic
Colligative properties

48. Color of Li (flame test)
but-
Hybridization
red
Dalton's Law

49. Amount of product produced when limiting reactant is used up
Percent Yield
perchlorate
but-
Theoretical yield

50. Oxidation # of free elements
0
-oic acid
N=N.(0.5)^time/time half-life
Root Mean Square Velocity