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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. Idea Gas Law (actual rules)
London dispersion forces
Standard Temperature and 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
red/orange

2. Ecell= E°cell -RT/nF x lnQ
effects of IMF
Nernst Equation
Kinetic Molecular Theory - for ideal gases
msAT

3. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
Molecular Compounds
Barometer
London dispersion forces
charge

4. Oxidation # of Polyatomic Ions
Speed of light
Transition metals
prop-
charge

5. Has values from 0 to (n-1); tells shape of atomic orbitals
yellow
Resonance
Angular Momentum Quantum Number
Isolated System

6. To find activation energy use the...
Anode
rate law
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Arrhenius equation

7. Energy involved in gaining an electron to become a negative ion
1st law of thermodynamics
red
electron affinity
Cell Potential (Ecell)

8. ln[A] vs. time is a ...-order reaction
Hund's Rule
insoluble
first
adhesion

9. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
Integrated Second-Order Rate Law
Second-Order Half Life
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

10. The measurement of heat changes
Lone Pair
End Point
Calorimetry
-one

11. R in ideal gas law
reduction
q/moles
0.0821 atm L/mol K
catalyst

12. Has values 1 -2 -3 -...; tells energy levels
equivalence point
Hybridization
Enthalpy of Solution
Principal Quantum Number

13. Oxidation # of free elements
bond energy
Pauli Exclusion Principle
Monoprotic
0

14. Increase Volume
Bond Order
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
melting
Increase Temperature

15. C2O4²?
yellow
oxalate
Dipole Moment
experimental yield

16. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Enthalpy of Solution
Formal Charge
1 atm
Dipole-dipole forces

17. 180° - sp
Its element
Linear
-oate
Sigma Bond

18. Peak of energy diagram
activated complex (transition state)
Temperature
strong acid strong base rxn
iodide

19. Boltzmann constant - used in calculating speed of gas per molecule
Zero-Order Rate Law
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
1.38x10?²³J/K
m (third quantum number)

20. Describe various properties of one orbital
Quantum Numbers
bromate
Speed of light
Antibonding Molecular Orbital

21. Composition Formula
exothermic
1.86°C
Molar Mass of Element/ Total Molar Mass %
Counterions

22. Involves quantum numbers
Quantum Mechanical Model
Molecular Orbitals (MOs)
charge
perchlorate

23. A weak acid that changes color at or near the equivalence point
sublimation
Temperature
indicator
1.38x10?²³J/K

24. # bonding e- - # antibonding e-/2
lambda
Net Ionic Equation
Bond Order
oxidizing agent

25. l=1
paramagnetic
Beta Particles-
1atm=?mmHg/Torr
p

26. r=k
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Zero-Order Rate Law
conjugate base
0 degrees C - 1 atm

27. Change without heat transfer between the system and its surroundings
trigonal bipyramidal
Naming Binary Ionic Compounds
Molality
adiabatic

28. C=2.9979*10^8 m/s
ammonium
rate gas A/rate gas B = square root (mm A/ mm B)
Speed of light
triple bond

29. O²?
bond energy
oxide
Percent Yield
H

30. OH¹?
Law of Conservation of Mass
London dispersion forces
hydroxide
dec-

31. Average speed of gas
seesaw
Delta H or Enthalpy Change
v3RT/M(in kg)
rate law

32. Group 2 metals
Angular Momentum Quantum Number
Oxidizing Agent
Chemical Bonds
Alkaline earth metals

33. A device in which chemical energy is changed to electrical energy
high pressure - low temperature
s
Galvanic Cell
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

34. Like dissolves...
yellow --> green
like
condensation
Buffered Solution

35. Dirrect Method Formula
supercritical fluid
0
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
-al

36. 760mmHg/Torr
1atm=?mmHg/Torr
bond energy
Formal Charge
-al

37. Measure of the average kinetic energy of all the particles in a substance
Temperature
Allotrope
Molecular Compounds
r1/r2

38. Matter can't be created nor destroyed
Arrhenius equation
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
Law of Conservation of Mass
Covalently w/in themselves - Ionicly bonded w/ each other

39. H?+OH??H2O
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
condensation
red/orange
strong acid strong base rxn

40. 1 sigma bond
X of a = moles a/total moles
boiling point
Volume Metric Flask & Pipet
single bond

41. Point at which vapor pressure=air pressure above
Ionic Compounds
1st law of thermodynamics
0
boiling point

42. Planck's constant - used to calculate energy w/frequency
6.63x10?³4Js
Integrated Second-Order Rate Law
-ous acid
triple bond

43. CN¹?
Dipole Moment
+1 - except if bonded to Alkali Metal -1
cyanide
Antibonding Molecular Orbital

44. C2H3O2¹?
8.31J/Kmol
acetate
force x distance = work done
Ionic

45. Where oxidation occurs
Anode
Q<K
Hydrogen bonding
Exothermic

46. Energy required to break a bond
Net Ionic Equation
Bond Energy
Solute
Quantum Mechanical Model

47. Anything occupying space and with mass
methoxy-
Open System
Matter
Anode

48. Faraday's constant
experimental yield
96500
Surroundings
Molecular Orbitals (MOs)

49. Spontaneous emission of radiation
n (first quantum number)
Radioactivity
mol
Q<K

50. The line running between the atoms
Sigma Bond
Second-Order Rate Law
electron affinity
condensation