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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. Arrhenius equation
chlorate
k=Ae^(-Ea/RT)
specific heat
System
2. Has values 1 -2 -3 -...; tells energy levels
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Principal Quantum Number
hydrolysis
work
3. AX4
geometric isomers
tetrahedral
spontaneity
Cell Potential (Ecell)
4. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
oxide
M = square root (3RT/mm)
diamagnetic
5. Similar to atomic orbitals - except between molecules
s (fourth quantum number)
Arrhenius acid
boiling point
Molecular Orbitals (MOs)
6. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
0.0826Latm/Kmol
hydrolysis
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
alkane
7. How to Find a Weighted Average
f
Hund's Rule
Open System
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
8. CrO4²?
Ionic Compounds
Surroundings
chromate
Root Mean Square Velocity
9. 1/([A]0*k)
system
Second-Order Half Life
-oic acid
Hydrogen bonding
10. PO4³?
permanent gases
phosphate
Anion
Equivalence Point
11. [A]=-kt + [A]0
Integrated Zero-Order Rate Law
melting
bond energy
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
12. AH of formation for a substance in its stablest form (how it is found in nature)
n0
0
Radioactivity
Magnetic Quantum Number (ml)
13. Spontaneous emission of radiation
period
Law of Conservation of Mass
Radioactivity
State Functions
14. AX4E2
square planar
heat of vaporization
Average KE = 1/2(mass)(average speed of all particles)
n0
15. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
violet
Magnetic Quantum Number (ml)
melting point
non-
16. #NAME?
trigonal planar
octahedral
E
Thermochemistry
17. When _____ significant digits - round answer to least significant digit
square pyramidal
Multiplying
4.184
Antibonding Molecular Orbital
18. Planck's constant - used to calculate energy w/frequency
Average KE = 1/2(mass)(average speed of all particles)
6.63x10?³4Js
deposition
E
19. [A]0/2k
soluble
LE Model
yellow --> green
Zero-Order Half Life
20. PV=nRT
Ideal Gas Law
Electronegativity
p orbitals
0
21. Molecules' tendency to stick to the container
Barometer
adhesion
n (first quantum number)
Bronsted-Lowry acid
22. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Diffusion
Cg=kPg
Temperature
amine
23. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals
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24. frequency symbol
Bronsted-Lowry acid
equivalence point
nu
0
25. Reactant that's completely used up in a chemical reaction
Limiting reactant
Covalently w/in themselves - Ionicly bonded w/ each other
e-
force x distance = work done
26. Positive ion
Arrhenius acid
heat capacity
Cation
-ic acid
27. Oxidation # of Hydrogen
Angular Momentum Quantum Number
AH
+1 - except if bonded to Alkali Metal -1
Standard Temperature and Pressure
28. The reactant that is being reduced - brings about oxidation
1 atm = 760 mmHg = 101.3 kPa
-oate
oxidizing agent
-ol
29. AX3
Bronsted-Lowry Base
trigonal planar
1st law of thermodynamics
Solubility Product (Ksp)
30. Cation first - anion second
Integrated Second-Order Rate Law
M = square root (3RT/mm)
Naming Binary Ionic Compounds
% error
31. Proton donors
Molality
Bronsted-Lowry acid
M = square root (3RT/mm)
Effusion
32. Bomb Calorimeter
Equilibrium constant
Constant Pressure
n (first quantum number)
Constant Volume
33. Elements on staircase on periodic table
Metalliods
Hydrogen bonding
Alkaline earth metals
Solubility Product (Ksp)
34. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
A Roman numeral
msAT
single bond
Kinetic Molecular Theory - for ideal gases
35. Substance in which something is dissolved in a solution (higher [ ])
Molar Heat Capacity
-oate
Monoprotic
Solvent
36. (# of lone pair e-)+1/2(# of shared e-)
Valence Electrons(assigned)
Ideal Gas Law
Dalton's Law
Pi Bond
37. Solution used in titration
titrant buret
Alpha Particles-
?Hvap
lambda
38. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
Density
Coordination Compound
2nd law of thermodynamics
End Point
39. Rate of Diffusion/Effusion formula
Molecular Orbitals (MOs)
Trigonal Planar
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
hydro-ic acid
40. The total entropy is always increasing - all systems tend towards maximum entropy
square pyramidal
2nd law of thermodynamics
trigonal planar
1/2mv²
41. A solid or gas that can be formed when 2 or more aqueous reactants come together
boiling point
precipitate
different # of neutrons
octahedral
42. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
Radioactivity
ether
endless
not spontaneous
43. (organics) single-bonded compound
square planar
p+
catalyst
alkane
44. Change in Energy = ? (in terms of constant pressure; for gasses)
AE= AH - RTAn
First-Order Half Life
Amino-
perchlorate
45. Lowers activation energy
Limiting reactant
critical point
catalyst
Tetrahedral
46. Faraday's constant
96500
Endothermic
H
diamagnetic
47. Change in Energy (AE) = ? (in terms of work)
conjugate acid
Solute
AE = q + w
chlorite
48. If anion ends in -ite - acid name ends in...
Hund's Rule
0
Closed System
-ous acid
49. Boltzmann constant - used in calculating speed of gas per molecule
1.38x10?²³J/K
solid CO2
adiabatic
E
50. We cannot simultaneously determine an atom's exact path or location
0.512°C
specific heat
sulfite
Heisenberg Uncertainty Principle