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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. Speed of Diffusion/Effusion formula
Galvanic Cell
Ionic Compounds
rate gas A/rate gas B = square root (mm A/ mm B)
Open System
2. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
Hydrogen bonding
base and hydrogen gas
spontaneous
Density
3. J/°Cmol or J/Kmol
Molar Heat Capacity
cohesion
Principal Quantum Number
96500
4. OH¹?
Q<K
hydroxide
dichromate
melting point
5. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
Ionic
London Dispersion Forces
adhesion
6. Phase change from gas to solid
precipitate
Hund's Rule
?Hvap
deposition
7. Larger molecules which have higher mass and therefore electron density have stronger...
0
London dispersion forces
Anode
1/2mv²
8. Average speed of gas
actual yield/theoretical yield x 100%
Faraday
Anode
v3RT/M(in kg)
9. Color of Ba (flame test)
but-
green/yellow
LeChatelier's Principle
van't Hoff Factor
10. (organics) four carbons
Alpha Particles-
but-
base
vaporization
11. Variable for spin of electron (+.5 or -.5)
purple
Molarity
s (fourth quantum number)
rate
12. Resistance to flow
viscosity
Closed System
Pauli Exclusion Principle
spontaneous
13. q cal = ?
Gamma Ray-
q/moles
CAT
Formal Charge
14. Mols A/ total mols - XA
mol Fraction
Pressure of H2O must be Subtracted
oxidation
2nd law of thermodynamics
15. [A]=-kt + [A]0
Pauli Exclusion Principle
Integrated Zero-Order Rate Law
Law of Conservation of Energy
work
16. (A) - C/s
k=Ae^(-Ea/RT)
Ampere
96500
Bronsted-Lowry Base
17. 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)
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Trigonal Planar
Ionic Compounds
catalyst
18. For significant digits - trailing zeros _____ significant
like
are
base
Pressure
19. r=k
Force = mass x acceleration
Zero-Order Rate Law
Calorimeter
Overall Reaction Order
20. R in instances that pertain to energy
are
Coordination Compound
8.314 J/K mol
Alpha Particles-
21. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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22. 1 sigma bond - 2 pi bonds
triple bond
Solute
Molality
Chemical Kinetics
23. 0.00°C - 1 atm
Specific Heat Capacity
Integrated First-Order Rate Law
methods of increasing rate
Standard Temperature and Pressure
24. R=
Ag+ - Pb2+ - Hg2+
Tetrahedral
conjugate base
0.0826Latm/Kmol
25. Pairs of electrons localized on an atom
precipitate
are
Zero-Order Rate Law
Lone Pair
26. AX5E
Heat
square pyramidal
E
iodide
27. For significant digits - leading zeros ____ significant
are not
Bond enthalpy
Law of Conservation of Mass
Temperature
28. Puts OH? into solution
solid CO2
Arrhenius base
oxide
London dispersion forces
29. IMF that exists in polar molecules
Dipole-dipole forces
entropy (S)
Amount of atoms present
Cathode
30. Liquid to gas
Overall Reaction Order
vaporization
Aufbau Principle
p+
31. Within a sublevel - place one e? per orbital before pairing them
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32. These orbitals are perpendicular
Pressure
indicator
p orbitals
second
33. (organics) one carbon
meth-
Magnetic Quantum Number (ml)
d orbitals
Equilibrium Expression
34. Proton donors
Bronsted-Lowry acid
AE = q + w
no precipitate forms
Hund's Rule
35. I=moles of particles/moles of solute dissolved
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36. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Positive work value; work done on system
Bond Order
Molecular
London dispersion forces
37. neutron (symbol)
activated complex (transition state)
Molality
n0
Molar Mass of Element/ Total Molar Mass %
38. Ability of an atom in a molecule to attract shared electrons to itself
Force = mass x acceleration
solid CO2
-oic acid
Electronegativity
39. High-speed electrons
critical point
Root Mean Square Velocity
Ampere
Beta Particles-
40. Measure of the average kinetic energy of all the particles in a substance
Heat Capacity (C)
vaporization
Temperature
not spontaneous
41. Heat needed to change 1 g of substance to 1°C
specific heat
Thermochemistry
prop-
Bonding Pairs
42. CrO4²?
chromate
0
Ionic Compounds
fusion
43. (organics) ten carbons
dec-
Constant Volume
Bronsted-Lowry Base
hydrolysis
44. Change in Energy (AE) = ? (in terms of work)
3/2RT
Buffered Solution
AE = q + w
-(q of H2O + q of cal)
45. Colors of Reaction when (MnO4 -) --> (Mn2+)
Ligand
hydro-ic acid
purple --> pink
Lone Pair
46. Horizontals on the periodic table
are
v3kT/m
period
Boltzmann distribution
47. PO4³?
Gamma Ray-
phosphate
Hydrogen bonding
Radioactivity
48. Solution used in titration
strong bases
titrant buret
Hund's Rule
effects of IMF
49. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Net Ionic Equation
vapor pressure
Colligative properties
s
50. r=k[A]^2
sublimation
trigonal pyramidal
Second-Order Rate Law
hex-