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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. In ideal gas law problem - when it says "atmospheric" ...
0
work
Pressure of H2O must be Subtracted
H

2. Hydroxides are soluble or insoluble?
insoluble
cyanide
Tetrahedral
Theory of Relativity

3. Puts OH? into solution
Nernst Equation
oxide gas and water
effects of IMF
Arrhenius base

4. Electron pairs found in the space between the atoms
Bonding Pairs
Quantum Numbers
Negative work value; work done by system
permanganate

5. # bonding e- - # antibonding e-/2
Bond Order
purple --> pink
8.31J/Kmol
Bronsted-Lowry Base

6. Stronger IMF= lower... weaker IMF= higher...
msAT
square pyramidal
methods of increasing rate
vapor pressure

7. #NAME?
critical point
hex-
experimental yield
E

8. Organic w/ -O-
Graham's Law
Theory of Relativity
ether
Alkali metals

9. Different form of same element
moles of solute/ L of solution
rate gas A/rate gas B = square root (mm A/ mm B)
allotrope
Anode

10. Measure of the change in enthalpy
charge
viscosity
Delta H or Enthalpy Change
Law of Multiple Proportions

11. R=
v3kT/m
anode
-al
0.0826Latm/Kmol

12. kf of water
Dipole Moment
octahedral
square pyramidal
1.86°C

13. Mass/volume
period
surroundings
Diffusion
Density

14. Change in moles (An) =?
Endothermic
First-Order Half Life
(moles of products that are gasses) - (moles of reactants that are gasses)
diamagnetic

15. CO3²?
Boltzmann distribution
like
carbonate
3rd law of thermodynamics

16. Force per unit area
Electron Spin Quantum Number
Pressure
1.86°C
Density

17. When n=6 ->2 - color=
-one
violet
Metalliods
are not

18. The chemical formed when an acid donates a proton
heat capacity
base
conjugate base
sulfate

19. Atoms with the same number of protons but a different number of neutrons
Isotopes
first
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
8.31J/Kmol

20. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
Antibonding Molecular Orbital
LE Model
triple point
s (fourth quantum number)

21. Group 2 metals
nitrate
Faraday
Alkaline earth metals
endothermic

22. Change that occurs at constant temperature
T-shape
mol Fraction
Equilibrium Expression
isothermal

23. Matter can't be created nor destroyed
Naming Binary Ionic Compounds
Speed of light
Law of Conservation of Mass
Constant Volume

24. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
-(P)(Change in V)
indicator
Atmospheric Pressure
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

25. To find activation energy use the...
Arrhenius equation
boiling point
?Tf= kf x molality
critical point

26. Measure of the average kinetic energy of all the particles in a substance
Temperature
permanent gases
Ligand
X of a = moles a/total moles

27. A given compound always has exactly the same proportion of elements by mass
viscosity
Alkaline earth metals
Integrated Rate Law
Law of Definite Proportion

28. Similar to atomic orbitals - except between molecules
Molarity
entropy
Bronsted-Lowry Acid
Molecular Orbitals (MOs)

29. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Law of Multiple Proportions
8.31J/Kmol
Speed of light
Arrhenius acid

30. [A] vs. time is a ...-order reaction
zero
Theoretical yield
-oate
Alpha Particles-

31. (N) number of equivalents per liter of solution
Heat
Normality
Bond enthalpy
Ionic

32. Half cell in which oxidation occurs
anode
viscosity
not spontaneous
blue-green

33. Ecell= E°cell -RT/nF x lnQ
indicator
Formal Charge
Nernst Equation
Diffusion

34. Group 1 metals
actual yield/theoretical yield x 100%
-2 - with peroxide -1
Alkali metals
London dispersion forces

35. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
third
Cg=kPg
2nd law of thermodynamics
Enthalpy of Solution

36. Positive ion
Equilibrium constant
Calorimetry
Cation
Pi Bond

37. For significant digits - trailing zeros _____ significant
are
Antibonding Molecular Orbital
8.314 J/K mol
Bronsted-Lowry base

38. Oxidation # of Ions
octahedral
allotrope
charge
Integrated First-Order Rate Law

39. Anything occupying space and with mass
sulfite
charge
zero
Matter

40. Molecules' tendency to stick to the container
adhesion
trigonal bipyramidal
-(P)(Change in V)
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

41. Positive enthalpy - heat flows into system
Temperature
Hund's Rule
endothermic
Pressure

42. H?+NH3?NH4
Strong acid weak base rxn
geometric isomers
permanganate
Exothermic

43. All cations are soluble with sulfate EXCEPT
Valence Electrons(assigned)
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
blue
melting

44. U(rms)=(3RT/M)^1/2
Root Mean Square Velocity
Hydrogen bonding
Ionic
trigonal planar

45. Mols A/ total mols - XA
mol Fraction
Gamma Ray-
purple
1 atm

46. pH=
Arrhenius acid
Calorimetry
Alpha Particles-
log[H+]

47. Liquid to gas
?Tf= kf x molality
Ideal Gas Law
vaporization
-oate

48. What is defined by you taken from the whole universe
First-Order Rate Law
X of a = moles a/total moles
Average KE = 1/2(mass)(average speed of all particles)
System

49. Temperature-pressure point after which gas can no longer form liquid
critical point
period
actual yield/theoretical yield x 100%
acetate

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

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