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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. Moles of solute/volume of soln(L)
Balmer Series
Graham's Law
Molarity
Exothermic

2. Molarity (M)
nitrite
triple bond
Volt
moles of solute/ L of solution

3. Energy needed to vaporize a mole of a liquid
condensation
?Hvap
trigonal bipyramidal
(moles of products that are gasses) - (moles of reactants that are gasses)

4. Polyatomic Ions (bonding)
cyanide
Trigonal Planar
Covalently w/in themselves - Ionicly bonded w/ each other
activation energy

5. NH4¹?
-oate
Colligative properties
Molarity
ammonium

6. Pressure Units/Conversions
l (second quantum number)
mol
1 atm = 760 mmHg = 101.3 kPa
square pyramidal

7. IMF that occurs with FON
Hydrogen bonding
N=N.(0.5)^time/time half-life
electrolyte
charge

8. All _________ compounds are electrolytes
Molecular Compounds
Ionic
-oic acid
Adding

9. Molality =
Speed of light
purple --> pink
k=Ae^(-Ea/RT)
moles solute/kg solvent

10. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Arrhenius Base
Molecular
-one
Solvent

11. Gain of electrons - decrease in oxidation #
t-shape
Pressure of H2O must be Subtracted
octahedral
reduction

12. Lowers activation energy
soluble
Barometer
Solubility Product (Ksp)
catalyst

13. SO3²?
Electronegativity
Cg=kPg
sulfite
M = square root (3RT/mm)

14. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Manometer
activated complex (transition state)
Molarity
Pauli Exclusion Principle

15. In covalent bonds - prefixes are used to tell...
Amino-
nu
Decrease Volume and Increase Temperature
Amount of atoms present

16. How to Find an Empirical Formula Given Percentages
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
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
Joule
Kinetic Molecular Theory - for ideal gases

17. Variable for type of orbital
acetate
l (second quantum number)
Effusion
Amount of atoms present

18. Describe various properties of one orbital
viscosity
Its root and adding -ide
Quantum Numbers
Hybridization

19. Ecell= E°cell -RT/nF x lnQ
Anode
Arrhenius base
trigonal bipyramidal
Nernst Equation

20. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
m (third quantum number)
sulfite
Magnetic Quantum Number (ml)
Ideal Gas Law

21. A measure of resistance of an object to a change in its state of motion
Mass
red
Surroundings
entropy (S)

22. When n=4 ->2 - color=
cyanide
Octahedral
-ic acid
blue-green

23. Where oxidation occurs
Percent Yield
Anode
endothermic
spontaneity

24. Amount of gravitational force exerted on an object
Weight
s (fourth quantum number)
Pi Bond
heat of fusion

25. Cation first - anion second
C=(mass)(specific heat)
-2 - with peroxide -1
Naming Binary Ionic Compounds
methoxy-

26. Boltzmann constant - used in calculating speed of gas per molecule
Matter
octahedral
1.38x10?²³J/K
force x distance = work done

27. Variable for energy of e- - goes from 1 -2 -3 on up
n (first quantum number)
0
Average KE = 1/2(mass)(average speed of all particles)
0

28. A solid or gas that can be formed when 2 or more aqueous reactants come together
precipitate
(moles of products that are gasses) - (moles of reactants that are gasses)
boiling point
Zero-Order Half Life

29. ClO2¹?
chlorite
strong bases
Volt
mol Fraction

30. All cations are soluble with bromide - chloride and iodide EXCEPT
first
Ag+ - Pb2+ - Hg2+
State Functions
Allotrope

31. An equilibrium expression
adhesion
Theory of Relativity
Solubility Product (Ksp)
diamagnetic

32. Proton (symbol)
Increase Temperature
p+
Law of Conservation of Energy
permanent gases

33. CrO4²?
oxidation
Hydrogen bonding
chromate
phosphate - sulfide - carbonate - sulfate

34. A solution used in titrations whose concentration is known
heat capacity
C=(mass)(specific heat)
Linear
standard solution

35. Oxidation # of Polyatomic Ions
charge
Cathode
Acid Dissociation Constant
Manometer

36. Type of system in which the energy may escape - but the mass is conserved
permanganate
Closed System
Hydrogen bonding
adhesion

37. The reactant in the reduction reaction that forces the oxidation reaction to occur
entropy
Arrhenius Acid
Oxidizing Agent
surroundings

38. Gas to liquid
voltaic cells
Ionic
Metalliods
condensation

39. The reactant that is being oxidized - brings about reduction
Average KE = 1/2(mass)(average speed of all particles)
reduction agent
nitrite
high pressure - low temperature

40. Change that occurs at constant temperature
isothermal
period
msAT
# protons + # neutrons

41. When n=6 ->2 - color=
violet
Arrhenius Base
Exothermic
0

42. STP
0 degrees C - 1 atm
d orbitals
condensation
Thermochemistry

43. K
endless
strong acids
Trigonal Bipyramidal
Equilibrium constant

44. The rest of the universe (in thermodynamics)
Acids
Alkali metals
Temperature
surroundings

45. 1 sigma bond
isothermal
triple bond
single bond
Diffusion

46. Dirrect Method Formula
First-Order Rate Law
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
carbonate
Strong acid weak base rxn

47. Color of K (flame test)
Ionic Compounds
geometric isomers
# protons + # neutrons
purple

48. Only contains ions that change in reaction
d
boiling point
Net Ionic Equation
carbonate

49. Boiling point elevation formula
trigonal pyramidal
s orbitals
?Tb= kb x molality
Dalton's Law

50. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
LE Model
base
Delta H or Enthalpy Change
supercritical fluid