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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. Unusually strong dipole forces found when H is bonded to N - O - or F
hept-
Mass
Hydrogen bonding
soluble
2. NO3¹?
Equivalence Point
nitrate
anode
Arrhenius Acid
3. (organics) double-bonded compound
alkene
Quantum Mechanical Model
alkane
strong acids
4. Increase Volume
Increase Temperature
red
sublimation
endothermic
5. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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6. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Percent Yield
rate
alkene
Isotopes
7. When n=6 ->2 - color=
g solute/g solvent x 100
oxidizing agent
r1/r2
violet
8. AH of formation for a substance in its stablest form (how it is found in nature)
T-shape
Magnetic Quantum Number (ml)
0
Coordination Compound
9. HF+ OH??H2O
Alpha Particles-
weak acid strong base rxn
seesaw
purple
10. Cr2O7²?
chlorate
1.86°C
critical point
dichromate
11. Entropy in the universe is always...
LE Model
see-saw
-ic acid
increasing
12. Expresses how the concentrations depend on time
Integrated Rate Law
2nd law of thermodynamics
eth-
bent
13. Oxidation # of Compounds
H
Radioactivity
indicator
0
14. 90° - d^2sp^3
viscosity
Surroundings
Octahedral
1/2mv²
15. Diatomic Molecules
entropy (S)
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
-1
bromate
16. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
Its root and adding -ide
+1 - except if bonded to Alkali Metal -1
flouride
17. Kinetic Energy is proportional to ______
Temperature
System
Coordination Compound
Quantum Model
18. Pairs of electrons localized on an atom
Lone Pair
electrolyte
dec-
Work
19. Energy involved in gaining an electron to become a negative ion
(moles of products that are gasses) - (moles of reactants that are gasses)
Law of Conservation of Mass
hex-
electron affinity
20. Oxidation # of Oxygen
titrant buret
0
-2 - with peroxide -1
yellow --> green
21. Change that occurs at constant temperature
isothermal
eth-
s
Volume Metric Flask & Pipet
22. Oxidation # of Hydrogen
rate law
+1 - except if bonded to Alkali Metal -1
yellow
adhesion
23. Phase change from gas to solid
v3RT/M(in kg)
Counterions
deposition
melting point
24. The rest of the universe (in thermodynamics)
3rd law of thermodynamics
Dipole Moment
surroundings
standard solution
25. A measure of randomness or disorder
entropy
1 atm
Amount of atoms present
Buffered Solution
26. Specific heat of water
Linear
hex-
4.184
Lone Pair
27. CrO4²?
cathode
Aufbau Principle
3/2RT
chromate
28. Heat capacity formula
Diffusion
eth-
Anion
C=(mass)(specific heat)
29. 1/[A] vs. time is a ...-order reaction
second
Law of Conservation of Mass
Average KE = 1/2(mass)(average speed of all particles)
Reaction Quotient (Q)
30. [A]=-kt + [A]0
trigonal pyramidal
Integrated Zero-Order Rate Law
-(q of H2O + q of cal)
-ol
31. 120° - sp^2
Trigonal Planar
strong acids
linear
Reducing Agent
32. Ability of an atom in a molecule to attract shared electrons to itself
red/orange
Electronegativity
T-shape
1 atm = 760 mmHg = 101.3 kPa
33. J/°Cmol or J/Kmol
Molar Heat Capacity
Lone Pair
Endothermic
Arrhenius acid
34. neutron (symbol)
dec-
n0
conjugate base
acetate
35. SI unit of energy; Kg*m^2/s^2
Ag+ - Pb2+ - Hg2+
Joule
Bronsted-Lowry base
alcohol
36. Boiling point - melting point - viscosity - vapor pressure - surface tension
effects of IMF
solid CO2
Bronsted-Lowry base
sulfite
37. An element with several different forms - each with different properties (i.e. graphite & diamond)
1/2mv²
trigonal planar
Le Chatelier's Principle
Allotrope
38. Dirrect Method Formula
k=Ae^(-Ea/RT)
1/2mv²
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Arrhenius equation
39. Matter can't be created nor destroyed
triple bond
(moles of products that are gasses) - (moles of reactants that are gasses)
alkane
Law of Conservation of Mass
40. Amount of heat needed to change a system by 1°C
?Tb= kb x molality
Its element
8.31J/Kmol
heat capacity
41. 90°&120° - dsp^3
not spontaneous
Trigonal Bipyramidal
Valence Electrons(assigned)
Osmotic Pressure
42. Ending for alcohols
trigonal bipyramidal
-ic acid
-ol
Molecular
43. All forms of energy except for heat
Q>K
Linear
work
adiabatic
44. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
red/orange
Volt
insoluble
moles of solute/ L of solution
45. AX4E2
System
square planar
Increase Temperature
1st law of thermodynamics
46. % yield
green/yellow
actual yield/theoretical yield x 100%
Cathode
Equilibrium constant
47. Occupies the space above and below a sigma bond
anode
diamagnetic
Bonding Pairs
Pi Bond
48. A molecule having a center of positive charge and a center of negative charge
mol Fraction
phosphate
Volume Metric Flask & Pipet
Dipole Moment
49. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
1atm=?mmHg/Torr
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Law of Multiple Proportions
Dalton's Law
50. Ketone suffix
Quantum Mechanical Model
-one
sulfate
mol