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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. Amount of product produced when limiting reactant is used up
Bronsted-Lowry base
Open System
Theoretical yield
P1V1/N1T1=P2V2/N2T2

2. AX3
4.184
trigonal planar
r1/r2
strong acids

3. Has values 1 -2 -3 -...; tells energy levels
Hess's Law
dec-
Principal Quantum Number
1 atm

4. Ecell= E°cell -RT/nF x lnQ
Entropy (S)
flouride
yellow --> green
Nernst Equation

5. Mass reactants= mass products
Law of Conservation of Mass
Hund's Rule
Antibonding Molecular Orbital
spontaneous

6. Ka=[products]^m/[reactants]^n
Pauli Exclusion Principle
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
Acid Dissociation Constant
purple --> pink

7. AX3E2
Monoprotic
0.0821 atm L/mol K
T-shape
Force = mass x acceleration

8. Measure of the average kinetic energy of all the particles in a substance
Cg=kPg
triple point
Temperature
Solution

9. Ionizes to produce H+ ions
Monoprotic
Standard Temperature and Pressure
Arrhenius Acid
Volume Metric Flask & Pipet

10. A weak acid that changes color at or near the equivalence point
Graham's Law
square planar
Molecular Compounds
indicator

11. Oxidation # of free elements
Specific Heat Capacity
k=Ae^(-Ea/RT)
0
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

12. AX6
catalyst
square pyramidal
octahedral
equilibrium

13. Energy can't be created nor destroyed
Isotopes
hept-
Law of Conservation of Energy
square planar

14. Point at which solid?liquid occurs
melting point
freezing
-ic acid
Molarity

15. 2+ charge
trigonal planar
-ol
Kinetic Molecular Theory - for ideal gases
Alpha Particles-

16. Isotope
different # of neutrons
8.314 J/K mol
Quantum Mechanical Model
Manometer

17. Gain of electrons - decrease in oxidation #
Antibonding Molecular Orbital
Percent Yield
reduction
ether

18. (organics) five carbons
pent-
-ic acid
single bond
Matter

19. Generally insoluble anions (names)
1 atm = 760 mmHg = 101.3 kPa
phosphate - sulfide - carbonate - sulfate
96500
State Functions

20. Anions or cations as needed to produce a compound with non net charge
chromate
Counterions
London dispersion forces
a precipitate forms

21. Color of Cs (flame test)
Trigonal Planar
blue
Bronsted-Lowry Acid
viscosity

22. Color of Na (flame test)
third
yellow
Q<K
chloride

23. Expresses how the concentrations depend on time
log[H+]
Integrated Rate Law
Molar Heat Capacity
wavelength

24. Type of system in which the energy and mass may leave or enter
Barometer
Open System
Closed System
?Tb= kb x molality

25. The heat changed in a chemical reaction.
effects of IMF
group
Pressure of H2O must be Subtracted
Thermochemistry

26. AX4
tetrahedral
sublimation
8.31J/Kmol
-ous acid

27. Puts H? into solution
Bronsted-Lowry Acid
excess reactant
Arrhenius acid
London dispersion forces

28. ln[A] vs. time is a ...-order reaction
first
sulfide
Bronsted-Lowry Acid
nu

29. q cal = ?
nitrate
First-Order Rate Law
Faraday
CAT

30. Oxidation # of Polyatomic Ions
charge
but-
0
Bronsted-Lowry Acid

31. SO3²?
Standard Temperature and Pressure
heat capacity
but-
sulfite

32. The rest of the universe (in thermodynamics)
-ic acid
Work
no precipitate forms
surroundings

33. 1/[A]=kt + 1/[A]0
Integrated First-Order Rate Law
square pyramidal
linear
Integrated Second-Order Rate Law

34. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
d orbitals
deposition
LE Model

35. Energy involved in gaining an electron to become a negative ion
Arrhenius Base
permanent gases
electron affinity
Kinetic Molecular Theory - for ideal gases

36. Ionizes to produce OH- Ions
Standard Temperature and Pressure
Metalliods
Arrhenius Base
# protons + # neutrons

37. AH of formation for a substance in its stablest form (how it is found in nature)
0
Solute
Graham's Law
equivalence point

38. Forward rxn occurs when
oxidation
Q<K
strong acid strong base rxn
Isolated System

39. Group 2 metals
not spontaneous
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
red/orange
Alkaline earth metals

40. [A]=-kt + [A]0
0
Integrated Zero-Order Rate Law
s (fourth quantum number)
Isolated System

41. AX4E
see-saw
base and hydrogen gas
high pressure - low temperature
Q<K

42. 0°C and 1 atm
Cation
Law of Multiple Proportions
STP
State Functions

43. =vM2/M1
increasing
Aufbau Principle
r1/r2
f

44. Verticals on the periodic table
Zero-Order Rate Law
heat of vaporization
Counterions
group

45. ln[A]=-kt + ln[A]0
hex-
Angular Momentum Quantum Number
q
Integrated First-Order Rate Law

46. Cr2O7²?
green/yellow
dichromate
Bond enthalpy
Nernst Equation

47. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
Bond Energy
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
heat of fusion

48. The driving force for a spontaneous is an increase in entropy of the universe
moles of solute/ L of solution
Entropy (S)
-2 - with peroxide -1
indicator

49. K
1.38x10?²³J/K
acetate
perchlorate
Equilibrium constant

50. I=moles of particles/moles of solute dissolved

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