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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. Variable for type of orbital
Force = mass x acceleration
l (second quantum number)
Balmer Series
condensation
2. Change in moles (An) =?
(moles of products that are gasses) - (moles of reactants that are gasses)
bent
e-
Arrhenius Base
3. Isotope
Hydrogen bonding
Root Mean Square Velocity
System
different # of neutrons
4. Speed of light - C
3.0x108m/s
acid
Arrhenius Acid
hydrocarbons
5. 90° - d^2sp^3
Heisenberg Uncertainty Principle
Octahedral
excess reactant
bent
6. Loss of electrons - increase in oxidation #
lambda
Faraday
second
oxidation
7. Expresses how the concentrations depend on time
-ous acid
Integrated Rate Law
Q<K
trigonal bipyramidal
8. Bomb Calorimeter
Calorimetry
Constant Volume
Molality
Zero-Order Half Life
9. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Chemical Kinetics
heat capacity
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Bronsted-Lowry acid
10. AX4E
Surroundings
Law of Multiple Proportions
seesaw
heat capacity
11. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
1 atm
strong acids
chlorate
12. If anion ends in -ate - acid name ends in...
-al
-oic acid
-ic acid
Quantum Numbers
13. [A]=-kt + [A]0
Integrated Zero-Order Rate Law
Monoprotic
oxidizing agent
0
14. Change without heat transfer between the system and its surroundings
adiabatic
yellow --> green
flouride
Van't Hoff factor
15. OH¹?
# protons + # neutrons
0.0826Latm/Kmol
hydroxide
Arrhenius base
16. Average Kinetic Energy Formula
heat capacity
Oxidation is Loss Reduction is Gain
3/2RT
Average KE = 1/2(mass)(average speed of all particles)
17. CN¹?
cyanide
Ag+ - Pb2+ - Hg2+
entropy (S)
methoxy-
18. Ka=[products]^m/[reactants]^n
Acid + Base --> Salt + Water
insoluble
Acid Dissociation Constant
Amount of atoms present
19. =vM2/M1
r1/r2
trigonal bipyramidal
Heat
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
20. Kinetic Energy per mol
Electronegativity
3/2RT
Law of Conservation of Mass
Law of Conservation of Energy
21. S²?
Limiting reactant
sulfide
n (first quantum number)
% error
22. When n=6 ->2 - color=
n (first quantum number)
Acids
Equivalence Point
violet
23. Describe various properties of one orbital
Arrhenius equation
Quantum Numbers
London Dispersion Forces
endothermic
24. IMF that occurs with FON
bent
precipitate
LE Model
Hydrogen bonding
25. Energy required to break a bond
Trigonal Planar
strong acids
Molecular
Bond Energy
26. Diatomic Molecules
Work
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
First-Order Rate Law
Molality
27. Increase Volume
Acids
-oate
Increase Temperature
Arrhenius Acid
28. Color of Ca (flame test)
surroundings
cohesion
hydrocarbons
red/orange
29. 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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30. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
End Point
anode
Monoprotic
p orbitals
31. Change in Energy = ? (in terms of constant pressure; for gasses)
Metalliods
bromate
Trigonal Planar
AE= AH - RTAn
32. E=mc^2
but-
no precipitate forms
Linear
Theory of Relativity
33. The reactant in the reduction reaction that forces the oxidation reaction to occur
Q<K
Oxidizing Agent
Root Mean Square Velocity
force x distance = work done
34. Half cell in which oxidation occurs
Pauli Exclusion Principle
anode
-oic acid
ionic
35. Different form of same element
allotrope
activated complex (transition state)
hydrocarbons
red
36. Electron (symbol)
-one
1st law of thermodynamics
permanent gases
e-
37. Mass reactants= mass products
LE Model
adiabatic
bent
Law of Conservation of Mass
38. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
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39. Molecules' tendency to stick to the container
Hybridization
adhesion
alkane
square planar
40. ClO2¹?
d
system
chlorite
P of a =(X of a)(total pressure)
41. Electrons in a hydrogen atom move around the nucleus only in circular orbits
precipitate
Quantum Model
tetrahedral
C=(mass)(specific heat)
42. Point at which liquid?gas occurs
triple bond
trigonal pyramidal
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
boiling point
43. AH of formation for a substance in its stablest form (how it is found in nature)
0
acetate
Surroundings
Ionic Compounds
44. Gain of electrons - decrease in oxidation #
reduction
0
Allotrope
see-saw
45. Everything in the universe that is not defined by you as part of the system
system
Polar Covalent
trigonal bipyramidal
Surroundings
46. (msubs) Can only be +1/2 or -1/2
Electron Spin Quantum Number
Acid Dissociation Constant
1 atm = 760 mmHg = 101.3 kPa
equilibrium
47. Energy can't be created nor destroyed
?Tf= kf x molality
standard solution
phosphate
Law of Conservation of Energy
48. Oxidation # of free elements
n (first quantum number)
0
London Dispersion Forces
triple bond
49. U(rms)=(3RT/M)^1/2
Acids
Volume Metric Flask & Pipet
precipitate
Root Mean Square Velocity
50. Oxidation # of Hydrogen
ammonium
+1 - except if bonded to Alkali Metal -1
green/yellow
exothermic