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Test your basic knowledge |
AP Chemistry
Start Test
Study First
Subjects
:
science
,
ap
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can
study here
.
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. Heat required to raise the system 1°C
q/moles
heat capacity
Molecule
log[H+]
2. This MUST be determined experimentally
eth-
Alkali metals
freezing
rate law
3. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
rate
Amino-
bent
triple bond
4. Molarity (M)
moles of solute/ L of solution
Molecular Compounds
Alkali metals
yellow --> green
5. 180° - sp
Molar Mass of Element/ Total Molar Mass %
Molecule
Octahedral
Linear
6. Gas to liquid
Molality
N=N.(0.5)^time/time half-life
equilibrium
condensation
7. Molecules' tendency to stick to the container
phosphate - sulfide - carbonate - sulfate
condensation
adhesion
methods of increasing rate
8. AX5E
hept-
permanent gases
flouride
square pyramidal
9. Ptotal=P1+P2+P3+...
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10. Like dissolves...
Metalliods
Law of Conservation of Mass
like
yellow --> green
11. Occupies the space above and below a sigma bond
effects of IMF
Entropy (S)
hept-
Pi Bond
12. I=moles of particles/moles of solute dissolved
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13. Energy required to break a bond
fusion
3.0x108m/s
Bond Energy
Temperature
14. Wavelength symbol
lambda
-ic acid
period
Effusion
15. What is defined by you taken from the whole universe
-(P)(Change in V)
Surroundings
System
isothermal
16. n+m (these are orders of reactants)
Calorimeter
amine
?Tf= kf x molality
Overall Reaction Order
17. Arrhenius equation
Cg=kPg
violet
voltaic cells
k=Ae^(-Ea/RT)
18. NO2¹?
Manometer
Buffered Solution
hydrolysis
nitrite
19. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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20. A measure of resistance of an object to a change in its state of motion
viscosity
Mass
system
Weight
21. Oxidation # of Hydrogen
+1 - except if bonded to Alkali Metal -1
Le Chatelier's Principle
mol Fraction
rate law
22. AX4E2
force x distance = work done
Increase Temperature
square planar
Delta H or Enthalpy Change
23. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
methoxy-
Molality
violet
24. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
seesaw
P1V1/N1T1=P2V2/N2T2
hydrolysis
a precipitate forms
25. When n=3 ->2 - color=
Law of Conservation of Mass
Entropy (S)
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
red
26. All forms of energy except for heat
work
analyte
Allotrope
single bond
27. Specific heat of water
oct-
4.184
experimental yield
pi=(nRT)/v
28. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
Hydrogen bonding
0
boiling point
29. Boiling point - melting point - viscosity - vapor pressure - surface tension
different # of neutrons
surroundings
effects of IMF
melting point
30. Change in Energy (AE) = ? (in terms of work)
sulfate
AE = q + w
Metalliods
second
31. 109.5° - sp^3
Second-Order Rate Law
Tetrahedral
adiabatic
fusion
32. Elements on staircase on periodic table
hydro-ic acid
Metalliods
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
fusion
33. (organics) seven carbons
hept-
London dispersion forces
adiabatic
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
34. Degree of disorder in a system
Manometer
lambda
entropy (S)
moles of solute/ L of solution
35. For significant digits - trailing zeros _____ significant
are
like
Antibonding Molecular Orbital
square pyramidal
36. F¹?
isothermal
titrant buret
flouride
Molality
37. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
adiabatic
Scientific Method
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
End Point
38. Driving force of the electrons
soluble
End Point
Cell Potential (Ecell)
equivalence point
39. Mol/L - concentration of a solution
heat of fusion
Arrhenius equation
3/2RT
Molarity
40. Solid to gas
3rd law of thermodynamics
sublimation
-(P)(Change in V)
heat of vaporization
41. Bomb Calorimeter
Integrated Rate Law
Constant Volume
strong acid strong base rxn
London dispersion forces
42. Hydroxides are soluble or insoluble?
complex ions
Solution
Ampere
insoluble
43. Amount of product produced when limiting reactant is used up
Trigonal Planar
anode
Theoretical yield
v3kT/m
44. H + donor
permanent gases
Bronsted-Lowry Acid
Specific Heat Capacity
activation energy
45. Group 1 metals
Boltzmann distribution
Alkali metals
double bond
surroundings
46. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
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47. Raising heat - adding catalyst - heighten concentration - bigger surface area
methods of increasing rate
-al
3rd law of thermodynamics
rate law
48. Point at which liquid?gas occurs
base and hydrogen gas
Net Ionic Equation
nu
boiling point
49. The heat changed in a chemical reaction.
Thermochemistry
non-
State Functions
hydroxide
50. Passage of gas through tiny orifice
lambda
E
yellow --> green
Effusion