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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. Mixing of gases
Hund's Rule
Diffusion
sulfide
salt bridge

2. AX3E
base
trigonal pyramidal
Hund's Rule
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

3. Where there are no electrons
permanganate
first
Gamma Ray-
Nodes

4. #NAME?
Strong acid weak base rxn
trigonal bipyramidal
Trigonal Bipyramidal
E

5. Electron (symbol)
e-
insoluble
Mass
hydrolysis

6. Energy involved in gaining an electron to become a negative ion
-oic acid
electron affinity
purple
heat of vaporization

7. Carbon & hydrogen compounds
Entropy (S)
Molarity
hydrocarbons
eth-

8. A homogeneous mixture with 1 phase
cohesion
s
yellow
Solution

9. Pressure Units/Conversions
1 atm = 760 mmHg = 101.3 kPa
p
geometric isomers
Diffusion

10. A monoatomic cation takes name from...
yellow
Its element
charge
Chemical Kinetics

11. NH4¹?
A Roman numeral
0 degrees C - 1 atm
ammonium
Alpha Particles-

12. ?T=k*m(solute)
bent
Molal FP Depression Constant
conjugate acid
chlorite

13. Organic reaction in which two functional groups come together - resulting in the release of water
heat capacity
First-Order Half Life
experimental yield
condensation

14. Group 1 metals
Alkali metals
Le Chatelier's Principle
equilibrium
-oic acid

15. (organics) one carbon
P1= X1P1°
Hydrogen bonding
Osmotic Pressure
meth-

16. Volume of gas @STP
22.4L
Effusion
purple --> pink
Acid Dissociation Constant

17. Two molecules with identical connectivity but different geometries
hydroxide
geometric isomers
red/orange
0.512°C

18. Higher in energy than the atomic orbitals of which it is composed
0
Antibonding Molecular Orbital
single bond
second

19. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
blue-green
hydrolysis
carbohydrates
Equivalence Point

20. Ending for alcohols
-ol
Dalton's Law
freezing
Isolated System

21. 1/([A]0*k)
Le Chatelier's Principle
third
Second-Order Half Life
chromate

22. Generally insoluble anions (names)
Limiting reactant
prop-
phosphate - sulfide - carbonate - sulfate
0

23. kb of water
1/2mv²
cohesion
0.512°C
purple --> pink

24. Ionizes to produce OH- Ions
square planar
Arrhenius Base
Equilibrium Expression
0

25. [A]0/2k
Gamma Ray-
Speed of light
dichromate
Zero-Order Half Life

26. Electron pairs found in the space between the atoms
alkene
Delta H or Enthalpy Change
Bonding Pairs
Hybridization

27. neutron (symbol)
Resonance
electrolyte
n0
Acids

28. Faraday's constant
oxidizing agent
msAT
96500
Metalliods

29. Symbol for the heat absorbed or lost molecularly (PER MOLE)
hydrocarbons
3/2RT
Cell Potential (Ecell)
AH

30. Equation to find Ea from reaction rate constants at two different temperatures
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
2nd law of thermodynamics
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
trigonal bipyramidal

31. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
Gamma Ray-
prop-
M = square root (3RT/mm)

32. (organics) ten carbons
# protons (atom is defined by this)
trigonal bipyramidal
triple bond
dec-

33. (organics) triple-bonded compound
alkyne
not spontaneous
LeChatelier's Principle
Lone Pair

34. A measure of randomness or disorder
conjugate acid
entropy
1.38x10?²³J/K
rate law

35. Phase change from gas to solid
soluble
deposition
Negative work value; work done by system
strong acids

36. Solution in flask being titrated
Theory of Relativity
analyte
Bronsted-Lowry acid
Oxidizing Agent

37. AX3E2
-(P)(Change in V)
T-shape
equivalence point
Mass

38. Speed per molecule of gas
London Dispersion Forces
q/moles
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
v3kT/m

39. 0.00°C - 1 atm
different # of neutrons
Standard Temperature and Pressure
Solubility Product (Ksp)
rate law

40. If anion ends in -ite - acid name ends in...
1atm=?mmHg/Torr
reduction agent
-ous acid
conjugate acid

41. Type of system in which the energy and mass may leave or enter
perchlorate
8.314 J/K mol
Open System
Dalton's Law of Partial Pressures

42. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
actual yield/theoretical yield x 100%
p+
Acids

43. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
red
-oate
P of a =(X of a)(total pressure)
yellow --> green

44. An equilibrium expression
octahedral
Solubility Product (Ksp)
v3RT/M(in kg)
purple --> pink

45. For colligative properties for electrolytes - the # of mols of ions/ mols of solute

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46. Color of Cs (flame test)
blue
v3RT/M(in kg)
Alkali metals
-2 - with peroxide -1

47. Ptotal=P1+P2+P3+...

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48. Unusually strong dipole forces found when H is bonded to N - O - or F
s
Octahedral
Hydrogen bonding
Q<K

49. Metal oxide + H20 ->
base
Nodes
Bond Order
sulfate

50. Driving force of the electrons
0
chloride
Oxidation is Loss Reduction is Gain
Cell Potential (Ecell)