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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. Freezing point depression formula
indicator
?Tf= kf x molality
force x distance = work done
van't Hoff Factor
2. Driving force of the electrons
Cell Potential (Ecell)
0
Molecular Orbitals (MOs)
Molality
3. AX4E2
System
square planar
chlorite
Decrease Volume and Increase Temperature
4. Reactant that's completely used up in a chemical reaction
Limiting reactant
Molecular
Molality
Decrease Volume and Increase Temperature
5. Amount of product produced when limiting reactant is used up
activation energy
AE= AH - RTAn
Theoretical yield
0
6. U(rms)=(3RT/M)^1/2
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Root Mean Square Velocity
Cell Potential (Ecell)
Its element
7. Amine prefix
bromate
Anion
Integrated Zero-Order Rate Law
Amino-
8. Point at which liquid?gas occurs
different # of neutrons
boiling point
green/yellow
Dalton's Law of Partial Pressures
9. The reactant in the reduction reaction that forces the oxidation reaction to occur
LE Model
purple
AE= AH - RTAn
Oxidizing Agent
10. 1 sigma bond - 1 pi bond
pent-
double bond
Manometer
+1 - except if bonded to Alkali Metal -1
11. Electron pairs found in the space between the atoms
period
Bonding Pairs
Angular Momentum Quantum Number
violet
12. (organics) one carbon
Molecule
but-
Adding
meth-
13. AX4E
Bond Order
vaporization
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
seesaw
14. Oxidation # of Halogens
phosphate - sulfide - carbonate - sulfate
oxalate
pi=(nRT)/v
-1
15. Point at which the titrated solution changes color
+1 - except if bonded to Alkali Metal -1
end point
Reducing Agent
flouride
16. MnO4¹?
Percent Yield
sulfate
permanganate
Law of Multiple Proportions
17. Variable for type of orbital
l (second quantum number)
Thermochemistry
log[H+]
different # of neutrons
18. Positive enthalpy - heat flows into system
endothermic
CAT
Hess's Law
endless
19. AX4E2
square planar
Bond Order
oxidation
AH
20. A given compound always has exactly the same proportion of elements by mass
oxide
ionic
activation energy
Law of Definite Proportion
21. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
solid CO2
Pi Bond
actual yield/theoretical yield x 100%
Ligand
22. Has values from 0 to (n-1); tells shape of atomic orbitals
Atmospheric Pressure
+1 - except if bonded to Alkali Metal -1
Angular Momentum Quantum Number
entropy
23. negative ion
moles of solute/ L of solution
Bronsted-Lowry acid
Hybridization
Anion
24. Molecules' tendency to stick to one another
strong acid strong base rxn
precipitate
cohesion
red
25. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
yellow --> green
Diffusion
base and hydrogen gas
Sigma Bond
26. (organics) single-bonded compound
Specific Heat Capacity
carbonate
Root Mean Square Velocity
alkane
27. Idea Gas Law (actual rules)
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
Lone Pair
msAT
Ampere
28. Ptotal=P1+P2+P3+...
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29. Metal oxide + H20 ->
increasing
double bond
base
Law of Multiple Proportions
30. Change in Energy = ? (in terms of constant pressure; for gasses)
p+
AE= AH - RTAn
n (first quantum number)
yellow
31. IMF that occurs with FON
Hydrogen bonding
Arrhenius base
but-
Decrease Volume and Increase Temperature
32. ln[A] vs. time is a ...-order reaction
allotrope
chromate
% error
first
33. Specific heat of water
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
First-Order Rate Law
4.184
octahedral
34. =vM2/M1
0
green/yellow
r1/r2
T-shape
35. A molecule having a center of positive charge and a center of negative charge
?Hvap
Dipole Moment
trigonal planar
surroundings
36. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
N=N.(0.5)^time/time half-life
blue-green
Cg=kPg
boiling point
37. Mol/kg of solvent - used in calculating colligative properties
insoluble
Molality
v3kT/m
Integrated Rate Law
38. The chemical formed when a base accepts a proton
Standard Temperature and Pressure
conjugate acid
s (fourth quantum number)
electrolyte
39. As protons are added to the nucleus - electrons are similarly added
Limiting reactant
Aufbau Principle
Overall Reaction Order
Increase Temperature
40. E=mc^2
Theory of Relativity
AE= AH - RTAn
m (third quantum number)
allotrope
41. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
Bond Energy
Finding Empirical Formulas
seesaw
fusion
42. The amount of energy/heat required to raise some substance 1 degree C
Anion
effects of IMF
hept-
Heat Capacity (C)
43. Boltzmann constant - used in calculating speed of gas per molecule
Heisenberg Uncertainty Principle
Dalton's Law
condensation
1.38x10?²³J/K
44. Elements which have unpaired electrons and highly affected by magnetic fields
Force = mass x acceleration
paramagnetic
octahedral
meth-
45. Delta H (AH) = ?
q/moles
?Hvap
octahedral
Oxidizing Agent
46. Pairs of electrons localized on an atom
blue-violet
Lone Pair
hept-
chlorate
47. Measure of the average kinetic energy of all the particles in a substance
Heat
-ic acid
Temperature
Solute
48. A measure of resistance of an object to a change in its state of motion
Second-Order Rate Law
Mass
boiling point
Oxidation is Loss Reduction is Gain
49. Molecules' tendency to stick to the container
sublimation
double bond
adhesion
Integrated First-Order Rate Law
50. Point at which vapor pressure=air pressure above
allotrope
-one
Ampere
boiling point