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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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1. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
bromate
Equilibrium Expression
wavelength
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

2. Dirrect Method Formula
catalyst
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Beta Particles-
4.184

3. To find activation energy use the...
N=N.(0.5)^time/time half-life
isothermal
red
Arrhenius equation

4. Increase Volume
8.314 J/K mol
Molecular Orbitals (MOs)
Increase Temperature
activation energy

5. S²?
like
sulfide
s orbitals
M = square root (3RT/mm)

6. Amount of gravitational force exerted on an object
Heat
n0
Dipole Moment
Weight

7. All forms of energy except for heat
work
Electron Spin Quantum Number
strong bases
bromate

8. Liquid to gas
Law of Conservation of Energy
vaporization
Heisenberg Uncertainty Principle
salt bridge

9. R=
nu
Amino-
8.31J/Kmol
Law of Conservation of Energy

10. A monoatomic anion is named by taking...
violet
Its root and adding -ide
conjugate acid
Net Ionic Equation

11. For significant digits - trailing zeros _____ significant
Standard Temperature and Pressure
Colligative properties
group
are

12. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
are not
mol Fraction
Kinetic Molecular Theory - for ideal gases
conjugate base

13. Point where acid completely neutralizes base
actual yield/theoretical yield x 100%
equivalence point
Graham's Law
nu

14. Amount of heat needed to change a system by 1°C
lambda
q
Naming Binary Ionic Compounds
heat capacity

15. (A) - C/s
actual yield/theoretical yield x 100%
Ampere
alkyne
Molality

16. Gain of electrons - decrease in oxidation #
acid
Speed of light
cohesion
reduction

17. Heat capacity formula
C=(mass)(specific heat)
oxidizing agent
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
M1V1=M2V2

18. Forward rxn occurs when
Dipole-dipole forces
Q<K
bromate
Trigonal Planar

19. Mole Fraction
X of a = moles a/total moles
like
# protons + # neutrons
alkane

20. Positive enthalpy - heat flows into system
endless
endothermic
p orbitals
Coordination Compound

21. Theoretical yield-experimental yield/theoretical yieldx100
0
Ideal Gas Law
% error
Thermochemistry

22. Force per unit area
entropy
Bronsted-Lowry base
Pressure
1.38x10?²³J/K

23. CN¹?
fusion
cohesion
log[H+]
cyanide

24. Oxidation # of free elements
Allotrope
P of a =(X of a)(total pressure)
0
PV=nRT

25. NO2¹?
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Trigonal Planar
nitrite
Negative work value; work done by system

26. Where reduction occurs
Cathode
deposition
1 atm
E

27. Organic reaction in which two functional groups come together - resulting in the release of water
iodide
alcohol
are
condensation

28. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
dichromate
Oxidation is Loss Reduction is Gain
Lone Pair

29. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
double bond
Constant Pressure
Quantum Mechanical Model
hydrolysis

30. Ptotal=Pa+Pb+Pc....

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31. Solid to gas
perchlorate
Le Chatelier's Principle
Alpha Particles-
sublimation

32. AX5E
voltaic cells
square pyramidal
Net Ionic Equation
Molecule

33. Larger molecules which have higher mass and therefore electron density have stronger...
insoluble
Isolated System
London dispersion forces
P of a =(X of a)(total pressure)

34. Mol/L - concentration of a solution
reduction agent
Decrease Volume and Increase Temperature
are
Molarity

35. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
?Tf= kf x molality
adhesion
Bonding Pairs

36. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Scientific Method
salt bridge
Manometer
ether

37. C=2.9979*10^8 m/s
heat of fusion
Speed of light
adhesion
Root Mean Square Velocity

38. Boltzmann constant - used in calculating speed of gas per molecule
1.38x10?²³J/K
Molecular Orbitals (MOs)
octahedral
geometric isomers

39. negative ion
cohesion
Anion
Thermochemistry
Integrated Zero-Order Rate Law

40. l=0
s
Mass
Pressure of H2O must be Subtracted
deposition

41. SO3²?
adiabatic
sulfite
Atmospheric Pressure
cyanide

42. 2 or more covalently bonded atoms
Molecule
London Dispersion Forces
allotrope
Surroundings

43. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
blue-green
k=Ae^(-Ea/RT)
-(P)(Change in V)

44. Expresses how the concentrations depend on time
8.31J/Kmol
blue
Its root and adding -ide
Integrated Rate Law

45. This MUST be determined experimentally
rate law
carbohydrates
Zero-Order Rate Law
no precipitate forms

46. Only contains ions that change in reaction
actual yield/theoretical yield x 100%
Hund's Rule
p orbitals
Net Ionic Equation

47. Oxidation # of Ions
charge
standard solution
Monoprotic
?Tf= kf x molality

48. Anions or cations as needed to produce a compound with non net charge
spontaneous
first
Force = mass x acceleration
Counterions

49. AX6
octahedral
Galvanic Cell
entropy (S)
blue

50. Substances w/ critical temperatures below 25°C
Negative work value; work done by system
Heisenberg Uncertainty Principle
permanent gases
spontaneous