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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. Organic w/ -O-
ether
green/yellow
# protons (atom is defined by this)
oxidation
2. Average speed of gas
Matter
v3RT/M(in kg)
red
single bond
3. The total energy of the universe is constant - all systems tend towards minimum energy
Law of Multiple Proportions
soluble
nu
1st law of thermodynamics
4. AX4
Molar Heat Capacity
tetrahedral
triple bond
Coordination Compound
5. neutron (symbol)
Ampere
n0
insoluble
cathode
6. 1 sigma bond - 2 pi bonds
triple bond
Law of Multiple Proportions
Formal Charge
Balmer Series
7. Driving force of the electrons
oxalate
Cell Potential (Ecell)
Lone Pair
blue-violet
8. The rest of the universe (in thermodynamics)
alcohol
N=N.(0.5)^time/time half-life
surroundings
Oxidation is Loss Reduction is Gain
9. Moles of solute/volume of soln(L)
AH
Percent Yield
P of a =(X of a)(total pressure)
Molarity
10. Boltzmann constant - used in calculating speed of gas per molecule
Cell Potential (Ecell)
1.38x10?²³J/K
moles solute/kg solvent
lambda
11. If needed - indicate charge of metal(cation) by...
A Roman numeral
0 degrees C - 1 atm
heat capacity
AH
12. OH¹?
hydroxide
Cell Potential (Ecell)
T-shape
Cathode
13. Heat needed to change 1 g of substance to 1°C
Integrated Rate Law
specific heat
Bronsted-Lowry Acid
Diffusion
14. 1 sigma bond
prop-
-oate
single bond
work
15. Hydroxides are soluble or insoluble?
Integrated Zero-Order Rate Law
insoluble
bent
Bronsted-Lowry base
16. Work = ?
-(P)(Change in V)
Solvent
1.38x10?²³J/K
3/2RT
17. All _________ compounds are electrolytes
Ionic
analyte
octahedral
anode
18. The measurement of heat changes
Pressure of H2O must be Subtracted
?Tb= kb x molality
trigonal pyramidal
Calorimetry
19. Involves quantum numbers
Quantum Mechanical Model
octahedral
permanent gases
Specific Heat (s)
20. For significant digits - leading zeros ____ significant
surroundings
are not
viscosity
Dipole-dipole forces
21. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
Law of Definite Proportion
Closed System
End Point
Pressure
22. Oxidation # of Hydrogen
1 atm = 760 mmHg = 101.3 kPa
electrolyte
effects of IMF
+1 - except if bonded to Alkali Metal -1
23. Universal IMF for nonpolar molecules
nitrite
London dispersion forces
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
6.63x10?³4Js
24. AX6
bond energy
First-Order Half Life
octahedral
Sigma Bond
25. Reactant which doesn't get used up completely in a chemical reaction
blue
Integrated Rate Law
excess reactant
-(P)(Change in V)
26. Increase Volume
Ionic Compounds
precipitate
Law of Multiple Proportions
Increase Temperature
27. Happens at lines in phase change charts
Beta Particles-
Pressure
equilibrium
cathode
28. H?+NH3?NH4
London Dispersion Forces
Calorimeter
Strong acid weak base rxn
% yield
29. SO3²?
8.314 J/K mol
sulfite
third
Quantum Numbers
30. Cr2O7²?
bond energy
-oate
dichromate
Arrhenius Base
31. AH of formation for a substance in its stablest form (how it is found in nature)
0
State Functions
Nernst Equation
activation energy
32. Symbol for Enthalpy
methods of increasing rate
flouride
Beta Particles-
H
33. These orbitals are diagonal
Q<K
d orbitals
Counterions
Van't Hoff factor
34. CO3²?
sulfide
carbonate
Graham's Law
n (first quantum number)
35. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
Diffusion
Monoprotic
hydrolysis
p orbitals
36. The chemical formed when an acid donates a proton
nu
Monoprotic
conjugate base
Integrated Second-Order Rate Law
37. Positive ion
-2 - with peroxide -1
Cation
Alkali metals
third
38. 2+ charge
Alpha Particles-
s (fourth quantum number)
first
1 atm
39. The amount of energy/heat required to raise some substance 1 degree C
blue-green
AE= AH - RTAn
purple --> pink
Heat Capacity (C)
40. What is defined by you taken from the whole universe
v3RT/M(in kg)
System
allotrope
alkyne
41. Anything occupying space and with mass
Oxidation is Loss Reduction is Gain
Bond Order
d orbitals
Matter
42. Horizontals on the periodic table
period
experimental yield
insoluble
State Functions
43. Where reduction occurs
phosphate
Principal Quantum Number
Cathode
van't Hoff Factor
44. Ka=[products]^m/[reactants]^n
Overall Reaction Order
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Bonding Pairs
Acid Dissociation Constant
45. J/°Cmol or J/Kmol
London dispersion forces
bromate
Molar Heat Capacity
acid
46. Effusion of a gas is inversely proportional to the square root of the molar mass
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47. Does the same as equilibrium expression - except it uses initial concentrations
Second-Order Half Life
Work
charge
Reaction Quotient (Q)
48. H + donor
chromate
analyte
Bronsted-Lowry Acid
red/orange
49. Stronger IMF= lower... weaker IMF= higher...
Overall Reaction Order
vapor pressure
Balmer Series
voltaic cells
50. The minimum energy that molecules must possess for collisions to be effective - Ea
Dalton's Law of Partial Pressures
activation energy
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
electrolyte