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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. (organics) eight carbons
l (second quantum number)
oct-
Reducing Agent
Exothermic

2. Color of Cs (flame test)
Bronsted-Lowry base
blue
Molar Heat Capacity
specific heat

3. r=k[A]^2
M = square root (3RT/mm)
Law of Multiple Proportions
Heat Capacity (C)
Second-Order Rate Law

4. Energy required for melting to occur
heat of fusion
allotrope
melting point
lambda

5. C2O4²?
oxalate
6.63x10?³4Js
methods of increasing rate
ionic

6. #NAME?
bromate
Angular Momentum Quantum Number
Theory of Relativity
E

7. (organics) four carbons
-al
Pi Bond
but-
0.512°C

8. Point at which the titrated solution changes color
C=(mass)(specific heat)
period
Resonance
end point

9. Polyatomic Ions (bonding)
chlorate
first
Endothermic
Covalently w/in themselves - Ionicly bonded w/ each other

10. 1/[A] vs. time is a ...-order reaction
Hess's Law
Boltzmann distribution
second
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

11. pH=
3/2RT
critical point
log[H+]
Negative work value; work done by system

12. As protons are added to the nucleus - electrons are similarly added
exothermic
Resonance
Aufbau Principle
are not

13. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
base and hydrogen gas
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
Cg=kPg

14. When gas compresses ...
diamagnetic
Oxidation is Loss Reduction is Gain
electrolyte
Positive work value; work done on system

15. If needed - indicate charge of metal(cation) by...
A Roman numeral
Quantum Numbers
chlorite
Acid Dissociation Constant

16. Releases/gives off heat (negative value)
Hess's Law
End Point
3rd law of thermodynamics
Exothermic

17. O²?
oxide
Integrated First-Order Rate Law
octahedral
charge

18. Determined by the formula h/m(in kg)v - (v=velocity)
Temperature
charge
adhesion
wavelength

19. H+ Acceptor
Bronsted-Lowry Base
effects of IMF
Amount of atoms present
solid CO2

20. Melting
Bronsted-Lowry acid
analyte
rate
fusion

21. Ptotal=P1+P2+P3+...

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22. Two molecules with identical connectivity but different geometries
AE= AH - RTAn
Nodes
entropy
geometric isomers

23. Change without heat transfer between the system and its surroundings
% yield
Heat
adiabatic
entropy (S)

24. The total energy of the universe is constant - all systems tend towards minimum energy
Endothermic
1st law of thermodynamics
green/yellow
alkane

25. The weighted average of all the isotopes that an atom can have (in g/mol)
iodide
Atomic Mass Unit
are
voltaic cells

26. Has values from 0 to (n-1); tells shape of atomic orbitals
# protons (atom is defined by this)
Positive work value; work done on system
Angular Momentum Quantum Number
Barometer

27. Similar to atomic orbitals - except between molecules
Molecular Orbitals (MOs)
yellow --> green
Integrated First-Order Rate Law
rate

28. A device used to measure Delta H
?Tf= kf x molality
conjugate base
Calorimeter
Hund's Rule

29. Isotope
?Tf= kf x molality
AH
Amount of atoms present
different # of neutrons

30. If anion ends in -ite - acid name ends in...
-ous acid
are
Speed of light
Alpha Particles-

31. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps

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32. (N) number of equivalents per liter of solution
Normality
freezing
Heat Capacity (C)
Enthalpy of Solution

33. NH4¹?
ammonium
Electronegativity
red
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

34. Heat required to raise the system 1°C
log[H+]
Molecular Compounds
Osmotic Pressure
heat capacity

35. IMF that occurs with FON
Volt
Amount of atoms present
non-
Hydrogen bonding

36. Osmotic pressure=MRT
0.512°C
Specific Heat (s)
# protons (atom is defined by this)
Osmotic Pressure

37. Average speed of gas
electron affinity
heat capacity
v3RT/M(in kg)
-oic acid

38. Nonmetal oxide + H2O ->
chlorite
-2 - with peroxide -1
permanent gases
acid

39. ?Hsoln=?H1+?H2+?H3+...
A Roman numeral
heat capacity
Enthalpy of Solution
Cg=kPg

40. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals

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41. Boiling point - melting point - viscosity - vapor pressure - surface tension
effects of IMF
Dalton's Law of Partial Pressures
Metalliods
double bond

42. Reactant which doesn't get used up completely in a chemical reaction
isothermal
AE = q + w
Molality
excess reactant

43. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
vapor pressure
analyte
Manometer

44. Mol of solute/kg of solvent
Entropy (S)
Acid Dissociation Constant
Amino-
Molality

45. Solid to liquid
q/moles
1st law of thermodynamics
adhesion
melting

46. 0.00°C - 1 atm
Standard Temperature and Pressure
0
Transition metals
freezing

47. Specific heat of water
Beta Particles-
-(P)(Change in V)
4.184
purple

48. Work = ?
Molecular Compounds
-(P)(Change in V)
base
p orbitals

49. Force that holds atoms together
Chemical Bonds
Principal Quantum Number
Linear
moles solute/kg solvent

50. Half-life equation
N=N.(0.5)^time/time half-life
m (third quantum number)
Graham's Law
-ol