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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. Change in Energy (AE) = ? (in terms of work)
melting
are
1st law of thermodynamics
AE = q + w

2. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
high pressure - low temperature
Ionic Compounds
Net Ionic Equation
Amount of atoms present

3. (organics) five carbons
insoluble
pent-
trigonal planar
first

4. H + donor
Barometer
0.512°C
Equilibrium Expression
Bronsted-Lowry Acid

5. SO4²?
Specific Heat Capacity
-1
T-shape
sulfate

6. The actual amount of product produced in an experiment
salt bridge
strong acid strong base rxn
experimental yield
dec-

7. Force that holds atoms together
Cathode
Chemical Bonds
Faraday
Ag+ - Pb2+ - Hg2+

8. NH4¹?
activated complex (transition state)
ammonium
period
seesaw

9. For colligative properties for electrolytes - the # of mols of ions/ mols of solute

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10. kb of water
v3RT/M(in kg)
% yield
0.512°C
Equilibrium constant

11. When n=5 ->2 - color=
viscosity
blue-violet
1/2mv²
Enthalpy of Solution

12. neutron (symbol)
n0
First-Order Half Life
insoluble
anode

13. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
+1 - except if bonded to Alkali Metal -1
reduction
Ligand

14. Liquid to gas
vaporization
Integrated First-Order Rate Law
0
Work

15. Color of Ca (flame test)
Oxidation is Loss Reduction is Gain
pent-
Zero-Order Half Life
red/orange

16. Loss of electrons - increase in oxidation #
Resonance
oxidation
zero
STP

17. Change that occurs at constant temperature
no precipitate forms
isothermal
Kinetic Molecular Theory - for ideal gases
trigonal planar

18. Cl¹?
experimental yield
chloride
paramagnetic
22.4L

19. The total energy of the universe is constant - all systems tend towards minimum energy
3rd law of thermodynamics
cathode
Octahedral
1st law of thermodynamics

20. Molecules' tendency to stick to one another
g solute/g solvent x 100
oxide gas and water
phosphate
cohesion

21. In ideal gas law problem - when it says "atmospheric" ...
activated complex (transition state)
are
Pressure of H2O must be Subtracted
square pyramidal

22. MnO4¹?
?Tb= kb x molality
are not
Nodes
permanganate

23. Oxidation # of Oxygen
Second-Order Half Life
N=N.(0.5)^time/time half-life
Isolated System
-2 - with peroxide -1

24. Speed of light - C
Diffusion
3.0x108m/s
Alkaline earth metals
1st law of thermodynamics

25. ClO3²?
Acids
chlorate
prop-
Bronsted-Lowry Base

26. Mole Fraction
k=Ae^(-Ea/RT)
X of a = moles a/total moles
Quantum Mechanical Model
sulfate

27. Bomb Calorimeter
Integrated Rate Law
Hess's Law
Constant Volume
(moles of products that are gasses) - (moles of reactants that are gasses)

28. Larger molecules which have higher mass and therefore electron density have stronger...
nu
Naming Binary Ionic Compounds
London dispersion forces
Molar Mass of Element/ Total Molar Mass %

29. Generally insoluble anions (names)
oxide
Second-Order Rate Law
phosphate - sulfide - carbonate - sulfate
Decrease Volume and Increase Temperature

30. Liquid to solid
freezing
LeChatelier's Principle
r1/r2
Delta H or Enthalpy Change

31. Ether prefix
methoxy-
5% rule
nu
0

32. An equilibrium expression
Solubility Product (Ksp)
8.31J/Kmol
Molarity
Linear

33. Puts OH? into solution
Arrhenius base
supercritical fluid
Specific Heat (s)
Net Ionic Equation

34. R=
8.31J/Kmol
mol Fraction
First-Order Rate Law
titrant buret

35. Entropy in the universe is always...
experimental yield
nu
increasing
Barometer

36. Cr2O7²?
Buffer
hydrocarbons
5% rule
dichromate

37. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
no precipitate forms
Molal FP Depression Constant
Open System

38. Oxidation # of free elements
Specific Heat (s)
Molecular
0
96500

39. When n=4 ->2 - color=
v3kT/m
square pyramidal
blue-green
voltaic cells

40. Dirrect Method Formula
Electronegativity
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
single bond
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

41. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
activated complex (transition state)
Bases
-ous acid
supercritical fluid

42. AX4E
green/yellow
boiling point
Trigonal Bipyramidal
see-saw

43. IMF that exists in polar molecules
Entropy (S)
Dipole-dipole forces
Oxidizing Agent
are

44. How to Balance a Redox Equation
Reducing Agent
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
0
s orbitals

45. Driving force of the electrons
Principal Quantum Number
alkane
Cell Potential (Ecell)
nitrate

46. Solid to liquid
q
Linear
Heat
melting

47. Has values from 0 to (n-1); tells shape of atomic orbitals
Chemical Bonds
electrolyte
Specific Heat Capacity
Angular Momentum Quantum Number

48. Polyatomic Ions (bonding)
eth-
Covalently w/in themselves - Ionicly bonded w/ each other
d orbitals
actual yield/theoretical yield x 100%

49. Energy needed to vaporize a mole of a liquid
square planar
Cell Potential (Ecell)
?Hvap
Manometer

50. J/°Cg or J/Kg
Cell Potential (Ecell)
Specific Heat Capacity
endless
Net Ionic Equation

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Test your basic knowledge |

AP Chemistry

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