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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. The chemical formed when a base accepts a proton
Trigonal Bipyramidal
Electronegativity
conjugate acid
Second-Order Half Life

2. Colors of Reaction when (MnO4 -) --> (Mn2+)
purple --> pink
Speed of light
l (second quantum number)
triple point

3. Chemical composition of dry ice
Ligand
solid CO2
?Tb= kb x molality
endless

4. When ____ significant digits - round answer to least decimal place
Solute
1 atm
Adding
sublimation

5. Group 1 metals
Alkali metals
Sigma Bond
log[H+]
Hydrogen bonding

6. Increase Pressure
Decrease Volume and Increase Temperature
viscosity
heat capacity
see-saw

7. Symbol for the heat absorbed or lost molecularly (PER MOLE)
AH
r1/r2
0.0821 atm L/mol K
Theory of Relativity

8. Peak of energy diagram
Reducing Agent
activated complex (transition state)
allotrope
Density

9. 1 sigma bond - 2 pi bonds
-(q of H2O + q of cal)
vapor pressure
triple bond
red

10. Nonmetal oxide + H2O ->
acid
force x distance = work done
q/moles
Volume Metric Flask & Pipet

11. A solution that resists a change in its pH
salt bridge
Buffered Solution
system
purple

12. The likelihood that a rxn will occur "by itself"
1/2mv²
spontaneity
1atm=?mmHg/Torr
London dispersion forces

13. Experimental yield/theoretical yieldx100
Law of Conservation of Mass
% yield
Constant Pressure
Law of Definite Proportion

14. 6.022x10^23
Molecular
-al
mol
s (fourth quantum number)

15. Osmotic pressure=MRT
n (first quantum number)
Osmotic Pressure
v3RT/M(in kg)
log[H+]

16. Phase change from solid to gas
sulfide
Bronsted-Lowry acid
sublimation
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

17. Force that holds atoms together
nu
Positive work value; work done on system
Chemical Bonds
blue-violet

18. Different form of same element
period
allotrope
-(P)(Change in V)
Its element

19. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
green/yellow
end point
Density

20. Carbon & hydrogen compounds
Law of Definite Proportion
Bases
hydrocarbons
octahedral

21. These orbitals are diagonal
p+
d orbitals
Speed of light
entropy (S)

22. Ending for alcohols
# protons + # neutrons
-(q of H2O + q of cal)
Temperature
-ol

23. Equation to find Ea from reaction rate constants at two different temperatures
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
0.0821 atm L/mol K
permanganate
end point

24. The part of the universe one is focused upon (in thermodynamics)
system
endless
single bond
standard solution

25. Ether prefix
Solvent
methoxy-
Amphoteric
(moles of products that are gasses) - (moles of reactants that are gasses)

26. Ester suffix
supercritical fluid
-oate
Ideal Gas Law
Boltzmann distribution

27. Energy required for liquid?gas
q/moles
moles solute/kg solvent
-ous acid
heat of vaporization

28. Arrhenius equation
Root Mean Square Velocity
spontaneity
Molality
k=Ae^(-Ea/RT)

29. Reverse rxn occurs when
Temperature
insoluble
surroundings
Q>K

30. % yield
red/orange
group
First-Order Rate Law
actual yield/theoretical yield x 100%

31. Freezing point depression formula
?Tf= kf x molality
Law of Definite Proportion
base and hydrogen gas
Molecule

32. Ideal Gas Law Formula
PV=nRT
Effusion
effects of IMF
d

33. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
effects of IMF
strong acid strong base rxn
Resonance
0.512°C

34. The reactant that is being reduced - brings about oxidation
base and hydrogen gas
phosphate - sulfide - carbonate - sulfate
oxidizing agent
oct-

35. Oxidation # of Hydrogen
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
isothermal
+1 - except if bonded to Alkali Metal -1
period

36. Carbon - hydrogen - oxygen compounds
# protons (atom is defined by this)
carbohydrates
permanganate
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

37. Oxidation # of Polyatomic Ions
hydrocarbons
charge
Heat Capacity (C)
C=(mass)(specific heat)

38. Energy needed to break a bond
Hess's Law
bond energy
phosphate - sulfide - carbonate - sulfate
1atm=?Pa

39. ?T=k*m(solute)
oxidizing agent
CAT
System
Molal FP Depression Constant

40. ... compounds are most conductive
first
pi=(nRT)/v
% error
ionic

41. How to Find a Weighted Average
blue
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
M = square root (3RT/mm)
Oxidation is Loss Reduction is Gain

42. The chemical formed when an acid donates a proton
Buffer
vaporization
0
conjugate base

43. 180° - sp
Linear
bromate
salt bridge
alkane

44. ln[A] vs. time is a ...-order reaction
square planar
first
octahedral
Osmotic Pressure

45. The energy required to raise 1 g of substance 1 degree C
fusion
Heat
Specific Heat (s)
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

46. Formula used when diluting stock solution (to find amount of water or stock needed)
condensation
solid CO2
Radioactivity
M1V1=M2V2

47. IMF that exists in polar molecules
Nodes
Dipole-dipole forces
violet
Octahedral

48. Energy required for melting to occur
Integrated Second-Order Rate Law
system
heat of fusion
Polar Covalent

49. Type of system in which the energy and mass may leave or enter
prop-
Open System
trigonal planar
high pressure - low temperature

50. Proton (symbol)
q/moles
carbonate
p+
M1V1=M2V2