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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. Point at which the titrated solution changes color
end point
Weight
London dispersion forces
viscosity
2. These orbitals are spherical
Pauli Exclusion Principle
experimental yield
pi=(nRT)/v
s orbitals
3. The total energy of the universe is constant - all systems tend towards minimum energy
adhesion
Its element
1st law of thermodynamics
Le Chatelier's Principle
4. R=
s
8.31J/Kmol
moles solute/kg solvent
-ol
5. 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)
Specific Heat (s)
Density
Ionic Compounds
strong acids
6. Boiling point elevation formula
Theory of Relativity
-(q of H2O + q of cal)
?Tb= kb x molality
P of a =(X of a)(total pressure)
7. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
p+
rate law
conjugate acid
rate
8. Newton's Second Law
high pressure - low temperature
Force = mass x acceleration
electron affinity
Acid Dissociation Constant
9. How to Find an Empirical Formula Given Percentages
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Net Ionic Equation
1 atm = 760 mmHg = 101.3 kPa
are
10. Increase Volume
Increase Temperature
third
Bond Order
4.184
11. Expresses how the concentrations depend on time
Integrated Rate Law
catalyst
square planar
Entropy (S)
12. Mixing of gases
Gamma Ray-
Diffusion
endothermic
Strong acid weak base rxn
13. If Q>Ksp
a precipitate forms
msAT
N=N.(0.5)^time/time half-life
Its element
14. C2H3O2¹?
Graham's Law
v3RT/M(in kg)
acetate
1.38x10?²³J/K
15. Atoms with the same number of protons but a different number of neutrons
Molecule
phosphate - sulfide - carbonate - sulfate
-(P)(Change in V)
Isotopes
16. Proton (symbol)
boiling point
r1/r2
p+
Alpha Particles-
17. The reactant in the oxidizing reaction that forces the reduction reaction to occur
E
First-Order Half Life
0.0826Latm/Kmol
Reducing Agent
18. Freezing point depression formula
?Tf= kf x molality
?Hvap
anode
Quantum Numbers
19. Ptotal=P1+P2+P3+...
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183
20. Describe various properties of one orbital
Solution
Quantum Numbers
Mass
0
21. =vM2/M1
d orbitals
Temperature
r1/r2
Balmer Series
22. In ideal gas law problem - when it says "atmospheric" ...
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Equilibrium constant
Pressure of H2O must be Subtracted
Molecular
23. Point at which solid?liquid occurs
Amount of atoms present
melting point
different # of neutrons
permanganate
24. If Q<Ksp
no precipitate forms
Chemical Bonds
Integrated Rate Law
Reducing Agent
25. (organics) two carbons
Osmotic Pressure
eth-
nitrate
violet
26. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Integrated First-Order Rate Law
Equivalence Point
lambda
Calorimeter
27. Raising heat - adding catalyst - heighten concentration - bigger surface area
Heat
exothermic
Pauli Exclusion Principle
methods of increasing rate
28. Substances w/ critical temperatures below 25°C
permanent gases
Molarity
Ligand
Arrhenius acid
29. (N) number of equivalents per liter of solution
Positive work value; work done on system
Adding
Normality
charge
30. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
third
complex ions
Second-Order Half Life
Specific Heat (s)
31. Donates a single H+ Ion (... other prefixes also)
London Dispersion Forces
heat of vaporization
Monoprotic
methoxy-
32. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Buffer
Solute
CAT
surroundings
33. Molality =
Arrhenius equation
22.4L
moles solute/kg solvent
Finding Empirical Formulas
34. Mass/volume
moles of solute/ L of solution
Density
Bronsted-Lowry base
Van't Hoff factor
35. Dalton's Law of Partial Pressures (to find partial pressure formula)
period
P of a =(X of a)(total pressure)
London dispersion forces
cohesion
36. Organic reaction in which two functional groups come together - resulting in the release of water
not spontaneous
linear
Arrhenius Acid
condensation
37. AX4E2
square planar
Calorimeter
-oate
Reaction Quotient (Q)
38. Aldehyde suffix
-al
base
Adding
Bronsted-Lowry base
39. AX5E
square pyramidal
0
allotrope
dec-
40. Oxidation # of Halogens
-1
Dalton's Law
v3RT/M(in kg)
diamagnetic
41. Mol/L - concentration of a solution
Nodes
Covalently w/in themselves - Ionicly bonded w/ each other
Adding
Molarity
42. Half-life equation
N=N.(0.5)^time/time half-life
AE= AH - RTAn
P of a =(X of a)(total pressure)
experimental yield
43. Everything in the universe that is not defined by you as part of the system
hydroxide
Surroundings
Kinetic Molecular Theory - for ideal gases
Weight
44. Molecules' tendency to stick to one another
cohesion
geometric isomers
n (first quantum number)
activation energy
45. (msubs) Can only be +1/2 or -1/2
Hydrogen bonding
Electron Spin Quantum Number
chromate
period
46. AX5
5% rule
viscosity
trigonal bipyramidal
Arrhenius base
47. A weak acid that changes color at or near the equivalence point
AE= AH - RTAn
indicator
high pressure - low temperature
eth-
48. R in ideal gas law
-1
Law of Conservation of Mass
s orbitals
0.0821 atm L/mol K
49. Coffee Cup Calorimeter
base
Constant Pressure
Law of Conservation of Energy
indicator
50. Energy required to break a bond
Bond Energy
actual yield/theoretical yield x 100%
Oxidizing Agent
s (fourth quantum number)