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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. 96 -485 C/mol e-
Faraday
system
Molality
Oxidizing Agent
2. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
Solution
-ol
strong acids
3. Work = ?
oct-
-(P)(Change in V)
Trigonal Planar
Electron Spin Quantum Number
4. Oxidation # of free elements
chloride
Chemical Kinetics
0
Quantum Model
5. Phase change from solid to gas
sublimation
% yield
oxidizing agent
Ionic
6. Kinetic Energy per mol
but-
adhesion
phosphate - sulfide - carbonate - sulfate
3/2RT
7. Gas to solid
conjugate acid
Positive work value; work done on system
Formal Charge
deposition
8. (organics) double-bonded compound
alkene
Constant Volume
strong bases
violet
9. In covalent bonds - prefixes are used to tell...
ammonium
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Amount of atoms present
Counterions
10. Ester suffix
chloride
-oate
yellow --> green
analyte
11. The rest of the universe (in thermodynamics)
Quantum Model
Thermochemistry
surroundings
precipitate
12. Mol/L - concentration of a solution
Molarity
Hund's Rule
0.512°C
Diffusion
13. AX4
tetrahedral
paramagnetic
8.31J/Kmol
P1V1/N1T1=P2V2/N2T2
14. Gain of electrons - decrease in oxidation #
Law of Multiple Proportions
Reaction Quotient (Q)
cyanide
reduction
15. Pairs of electrons localized on an atom
Equivalence Point
Temperature
Lone Pair
l (second quantum number)
16. As protons are added to the nucleus - electrons are similarly added
Aufbau Principle
violet
s orbitals
Acid Dissociation Constant
17. # bonding e- - # antibonding e-/2
Magnetic Quantum Number (ml)
n (first quantum number)
Bond Order
Equilibrium constant
18. 0.00°C - 1 atm
fusion
Standard Temperature and Pressure
Van't Hoff factor
Le Chatelier's Principle
19. A solution that resists a change in its pH
Arrhenius Base
Integrated First-Order Rate Law
Buffered Solution
triple bond
20. OIL RIG
oxidation
Specific Heat (s)
Oxidation is Loss Reduction is Gain
Limiting reactant
21. AX2E - AX2E2
0.512°C
tetrahedral
bent
Its root and adding -ide
22. Organic w/ -OH group
Integrated First-Order Rate Law
conjugate base
alcohol
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
23. Moles of solute/volume of soln(L)
Molarity
-ous acid
iodide
bond energy
24. C2O4²?
bond energy
oxalate
third
Arrhenius acid
25. Similar to atomic orbitals - except between molecules
Coordination Compound
alkene
Molecular Orbitals (MOs)
electron affinity
26. (organics) one carbon
Oxidation is Loss Reduction is Gain
End Point
meth-
Arrhenius Base
27. Mass #
Quantum Model
insoluble
Lone Pair
# protons + # neutrons
28. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
exothermic
l (second quantum number)
Oxidation is Loss Reduction is Gain
29. When ____ significant digits - round answer to least decimal place
permanganate
hydrolysis
Adding
Hund's Rule
30. Unusually strong dipole forces found when H is bonded to N - O - or F
6.63x10?³4Js
square pyramidal
Hydrogen bonding
Molecular Orbitals (MOs)
31. IMF that occurs with FON
oxide
Equilibrium constant
Hydrogen bonding
q/moles
32. If Q>Ksp
4.184
surroundings
a precipitate forms
phosphate
33. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
End Point
PV=nRT
Balmer Series
geometric isomers
34. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
Ideal Gas Law
soluble
endless
Cathode
35. Planck's constant - used to calculate energy w/frequency
oxidizing agent
electrolyte
6.63x10?³4Js
heat of vaporization
36. The total entropy is always increasing - all systems tend towards maximum entropy
(moles of products that are gasses) - (moles of reactants that are gasses)
C + 273
2nd law of thermodynamics
Law of Multiple Proportions
37. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
yellow --> green
Bond Energy
Increase Temperature
Balmer Series
38. 1 sigma bond
single bond
1.38x10?²³J/K
Decrease Volume and Increase Temperature
zero
39. (organics) seven carbons
hept-
Transition metals
Solution
heat capacity
40. A solid or gas that can be formed when 2 or more aqueous reactants come together
precipitate
vaporization
Amount of atoms present
heat capacity
41. (organics) two carbons
dec-
eth-
melting point
CAT
42. The reactant that is being reduced - brings about oxidation
allotrope
Percent Yield
mol
oxidizing agent
43. Ending for alcohols
-ol
Percent Yield
charge
Zero-Order Half Life
44. Amount of heat needed to change a system by 1°C
-ol
heat capacity
high pressure - low temperature
allotrope
45. l=2
d
nu
T-shape
Lone Pair
46. Group 2 metals
third
Balmer Series
weak acid strong base rxn
Alkaline earth metals
47. Type of system in which the energy may escape - but the mass is conserved
Surroundings
Closed System
1.86°C
indicator
48. Oxidation # of Compounds
Law of Multiple Proportions
iodide
Kinetic Molecular Theory - for ideal gases
0
49. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Hund's Rule
Law of Conservation of Energy
n0
Resonance
50. The chemical formed when an acid donates a proton
Zero-Order Rate Law
STP
conjugate base
n0