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AP Chemistry

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Organic w/ -OH group
LE Model
nu
3.0x108m/s
alcohol

2. Organic w/ -O-
Pauli Exclusion Principle
Amphoteric
Cell Potential (Ecell)
ether

3. When n=4 ->2 - color=
Acid + Base --> Salt + Water
Molarity
blue-green
Density

4. Equation to find Ea from reaction rate constants at two different temperatures
First-Order Rate Law
Temperature
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
critical point

5. Color of Cs (flame test)
Buffered Solution
Arrhenius Base
bromate
blue

6. Organic w/ -NH2
strong bases
square planar
Reaction Quotient (Q)
amine

7. H + donor
Naming Binary Ionic Compounds
PV=nRT
Bronsted-Lowry Acid
s (fourth quantum number)

8. Does the same as equilibrium expression - except it uses initial concentrations
Arrhenius Base
Reaction Quotient (Q)
work
yellow

9. 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
Cathode
Linear
0

10. Composition Formula
Molar Mass of Element/ Total Molar Mass %
Transition metals
0
Octahedral

11. Thickness
Scientific Method
viscosity
Principal Quantum Number
Limiting reactant

12. High-energy light
Heat Capacity (C)
Gamma Ray-
cohesion
charge

13. How to Balance a Redox Equation
t-shape
moles solute/kg solvent
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
Hess's Law

14. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
-(P)(Change in V)
activated complex (transition state)
Open System
Equivalence Point

15. R=
LeChatelier's Principle
0.0826Latm/Kmol
activated complex (transition state)
ionic

16. (organics) single-bonded compound
3.0x108m/s
s (fourth quantum number)
alkane
pent-

17. Speed per molecule of gas
v3kT/m
AE = q + w
Octahedral
London Dispersion Forces

18. Loss of electrons - increase in oxidation #
violet
bromate
Calorimeter
oxidation

19. Amount of gravitational force exerted on an object
Temperature
M1V1=M2V2
oxide
Weight

20. Spectrum of light when an electron drops to energy level n=2
Balmer Series
q
+1 - except if bonded to Alkali Metal -1
Q>K

21. Kinetic Energy of an individual particle formula
Arrhenius Base
Its element
T-shape
M = square root (3RT/mm)

22. 760mmHg/Torr
0
1atm=?mmHg/Torr
Exothermic
solid CO2

23. ?H when 1 mol of bonds is broken in the gaseous state
fusion
Balmer Series
Metalliods
Bond enthalpy

24. n+m (these are orders of reactants)
Coordination Compound
T-shape
Overall Reaction Order
M = square root (3RT/mm)

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

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26. Ptotal=P1+P2+P3+...

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27. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
soluble
hydrolysis
vapor pressure
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

28. Change in Energy (AE) = ? (in terms of work)
Arrhenius base
heat capacity
AE = q + w
hex-

29. Ending for alcohols
Entropy (S)
Cathode
s (fourth quantum number)
-ol

30. x can be ignored when % ionization is <5%
Magnetic Quantum Number (ml)
5% rule
Arrhenius Base
6.63x10?³4Js

31. Arrhenius equation
Molarity
Polar Covalent
Van't Hoff factor
k=Ae^(-Ea/RT)

32. CO3²?
sulfite
boiling point
Hund's Rule
carbonate

33. Temperature-pressure combination at which solid - liquid - and gas states appear
M1V1=M2V2
are
End Point
triple point

34. Ester suffix
octahedral
oct-
-oate
A Roman numeral

35. Ecell= E°cell -RT/nF x lnQ
anode
Nernst Equation
supercritical fluid
Electronegativity

36. Specific heat of water
Bronsted-Lowry Acid
4.184
electrolyte
Ionic

37. ?T=k*m(solute)
heat capacity
Molal FP Depression Constant
mol Fraction
Naming Binary Ionic Compounds

38. Aldehyde suffix
s (fourth quantum number)
-al
AH
1/2mv²

39. The weighted average of all the isotopes that an atom can have (in g/mol)
Atomic Mass Unit
heat capacity
Ligand
alkyne

40. Change that occurs at constant temperature
Graham's Law
isothermal
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Ionic Compounds

41. The total energy of the universe is constant - all systems tend towards minimum energy
Integrated Rate Law
1st law of thermodynamics
acetate
alkane

42. Where reduction occurs
0
group
Cathode
nitrite

43. AX3E2
oxidation
T-shape
hydrolysis
purple

44. A solution that resists a change in pH - contains both a weak acid and its conjugate base
paramagnetic
Octahedral
hydroxide
Buffer

45. A measure of resistance of an object to a change in its state of motion
Quantum Numbers
rate
pent-
Mass

46. A method of investigation involving observation and theory to test scientific hypotheses
-ous acid
Scientific Method
soluble
Hund's Rule

47. Within a sublevel - place one e? per orbital before pairing them

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48. Degree of disorder in a system
analyte
entropy (S)
deposition
Allotrope

49. AX5
trigonal bipyramidal
3/2RT
perchlorate
t-shape

50. Carbon - hydrogen - oxygen compounds
Pressure of H2O must be Subtracted
Multiplying
blue
carbohydrates

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AP Chemistry

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