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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. I¹?
STP
Nodes
Boltzmann distribution
iodide

2. l=3
base
vaporization
force x distance = work done
f

3. The measurement of heat changes
N=N.(0.5)^time/time half-life
Covalently w/in themselves - Ionicly bonded w/ each other
Ag+ - Pb2+ - Hg2+
Calorimetry

4. Universal IMF for nonpolar molecules
Heat Capacity (C)
London dispersion forces
hydrocarbons
square planar

5. How to Balance a Redox Equation
-one
3/2RT
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
increasing

6. Tools NEEDED for dilution
Volume Metric Flask & Pipet
Dipole Moment
condensation
third

7. When n=3 ->2 - color=
2nd law of thermodynamics
red
Kinetic Molecular Theory - for ideal gases
Overall Reaction Order

8. Does the same as equilibrium expression - except it uses initial concentrations
-oate
chlorate
excess reactant
Reaction Quotient (Q)

9. Absorbs/takes in heat (positive value)
1atm=?mmHg/Torr
Endothermic
meth-
solid CO2

10. Resistance to flow
oxide gas and water
P1V1/N1T1=P2V2/N2T2
viscosity
Thermochemistry

11. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Colligative properties
not spontaneous
Limiting reactant
paramagnetic

12. The rest of the universe (in thermodynamics)
Average KE = 1/2(mass)(average speed of all particles)
spontaneous
surroundings
eth-

13. 1 sigma bond - 1 pi bond
Second-Order Half Life
blue-violet
carbohydrates
double bond

14. Point where acid completely neutralizes base
equivalence point
triple bond
Law of Multiple Proportions
Thermochemistry

15. Higher in energy than the atomic orbitals of which it is composed
single bond
v3RT/M(in kg)
Antibonding Molecular Orbital
excess reactant

16. O²?
Calorimeter
hydro-ic acid
Magnetic Quantum Number (ml)
oxide

17. Work = ?
third
Colligative properties
-(P)(Change in V)
1st law of thermodynamics

18. Color of Sr (flame test)
reduction agent
red
freezing
Molecular Compounds

19. (organics) nine carbons
activation energy
AE= AH - RTAn
Arrhenius base
non-

20. Substances w/ critical temperatures below 25°C
-ol
permanent gases
Calorimeter
Amphoteric

21. A solution that resists a change in its pH
paramagnetic
Its root and adding -ide
Isolated System
Buffered Solution

22. Solid to liquid
Strong acid weak base rxn
melting
alkene
meth-

23. Raoult's Law - relations between vapor pressure and concentrations
P1= X1P1°
rate law
alkene
Endothermic

24. Has values from 0 to (n-1); tells shape of atomic orbitals
3rd law of thermodynamics
mol Fraction
Angular Momentum Quantum Number
Root Mean Square Velocity

25. Where reduction occurs
Cathode
Closed System
-(q of H2O + q of cal)
heat of vaporization

26. A homogeneous mixture with 1 phase
s
Open System
Solution
Volt

27. 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
Cation
Temperature
LE Model
Finding Empirical Formulas

28. Energy can't be created nor destroyed
% error
Law of Conservation of Energy
heat capacity
Force = mass x acceleration

29. A device in which chemical energy is changed to electrical energy
Linear
second
Galvanic Cell
Atmospheric Pressure

30. Substances that form OH- when dissolved in water; proton acceptors
X of a = moles a/total moles
first
Average KE = 1/2(mass)(average speed of all particles)
Bases

31. Spectrum of light when an electron drops to energy level n=2
hydroxide
London dispersion forces
Alkali metals
Balmer Series

32. Amount of product produced when limiting reactant is used up
Theoretical yield
Tetrahedral
Dalton's Law
1st law of thermodynamics

33. Involves quantum numbers
k=Ae^(-Ea/RT)
Quantum Mechanical Model
deposition
titrant buret

34. Metal oxide + H20 ->
mol Fraction
base
double bond
Calorimetry

35. Faraday's constant
+1 - except if bonded to Alkali Metal -1
96500
reduction agent
0

36. Coffee Cup Calorimeter
Constant Pressure
Decrease Volume and Increase Temperature
Faraday
Amphoteric

37. Heat needed to change 1 g of substance to 1°C
see-saw
specific heat
Specific Heat Capacity
Graham's Law

38. Matter can't be created nor destroyed
green/yellow
Law of Conservation of Mass
Matter
heat of vaporization

39. Elements in groups 3-12
Mass
trigonal planar
square planar
Transition metals

40. Variable for spin of electron (+.5 or -.5)
Ag+ - Pb2+ - Hg2+
s (fourth quantum number)
Gamma Ray-
E

41. When gas compresses ...
Positive work value; work done on system
trigonal bipyramidal
specific heat
Integrated Rate Law

42. Point at which solid?liquid occurs
oxalate
melting point
Balmer Series
t-shape

43. Ester suffix
Ampere
Reducing Agent
-oate
Trigonal Planar

44. Theoretical yield-experimental yield/theoretical yieldx100
hydroxide
% error
Manometer
Resonance

45. Type of system in which nothing is transfered (no mass or energy); ideal
Pauli Exclusion Principle
Magnetic Quantum Number (ml)
Isolated System
Force = mass x acceleration

46. ?H when 1 mol of bonds is broken in the gaseous state
p orbitals
?Tf= kf x molality
Bond enthalpy
alkyne

47. Horizontals on the periodic table
period
Increase Temperature
Theoretical yield
electrolyte

48. R=
Calorimetry
Integrated First-Order Rate Law
8.31J/Kmol
London dispersion forces

49. Increase Volume
reduction
Its element
Increase Temperature
LE Model

50. Hydroxides are soluble or insoluble?
insoluble
like
5% rule
London dispersion forces