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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. Molecules' tendency to stick to one another
condensation
cohesion
Heat Capacity (C)
viscosity
2. Substance being dissolved in a solution (lower [ ])
Solute
-ol
chloride
3.0x108m/s
3. These orbitals are diagonal
l (second quantum number)
Bond Order
p+
d orbitals
4. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
Aufbau Principle
8.314 J/K mol
Volt
5. If anion ends in -ite - acid name ends in...
second
Exothermic
sulfate
-ous acid
6. r=k
alkene
Zero-Order Rate Law
sulfate
Overall Reaction Order
7. SO4²?
activation energy
sublimation
sulfate
increasing
8. We cannot simultaneously determine an atom's exact path or location
Heisenberg Uncertainty Principle
Counterions
Work
Its element
9. Elements which have all electrons paired and relatively unaffected by magnetic fields
Monoprotic
4.184
diamagnetic
e-
10. 1 sigma bond - 2 pi bonds
specific heat
triple bond
-al
London dispersion forces
11. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
12. Coffee Cup Calorimeter
Beta Particles-
Constant Pressure
H
isothermal
13. (organics) five carbons
pent-
tetrahedral
rate
carbohydrates
14. Solid to liquid
melting
van't Hoff Factor
red/orange
Solution
15. The heat changed in a chemical reaction.
Molar Mass of Element/ Total Molar Mass %
Thermochemistry
6.63x10?³4Js
rate gas A/rate gas B = square root (mm A/ mm B)
16. (N) number of equivalents per liter of solution
Normality
Radioactivity
Ligand
% error
17. 101 -325 Pa
octahedral
1atm=?Pa
hydro-ic acid
Linear
18. Symbol for the heat absorbed or lost molecularly (PER MOLE)
AH
PV=nRT
square pyramidal
l (second quantum number)
19. Reverse rxn occurs when
Q>K
titrant buret
single bond
Its element
20. Solution used in titration
3/2RT
voltaic cells
titrant buret
Molarity
21. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Electronegativity
Atmospheric Pressure
3rd law of thermodynamics
strong acid strong base rxn
22. Raising heat - adding catalyst - heighten concentration - bigger surface area
methods of increasing rate
blue-violet
anode
3/2RT
23. The reactant in the oxidizing reaction that forces the reduction reaction to occur
equivalence point
Reducing Agent
Strong acid weak base rxn
diamagnetic
24. Equation to find Ea from reaction rate constants at two different temperatures
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
salt bridge
red
heat of vaporization
25. Mass #
Buffered Solution
Heisenberg Uncertainty Principle
Heat
# protons + # neutrons
26. Measure of the average kinetic energy of all the particles in a substance
adiabatic
Bonding Pairs
chlorate
Temperature
27. Everything in the universe that is not defined by you as part of the system
r1/r2
sulfate
Ligand
Surroundings
28. Gain of electrons - decrease in oxidation #
Mass
AH
q
reduction
29. AX4
Bronsted-Lowry acid
trigonal bipyramidal
tetrahedral
Force = mass x acceleration
30. S²?
n (first quantum number)
3.0x108m/s
Bond Energy
sulfide
31. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
soluble
Allotrope
Buffered Solution
Cg=kPg
32. As protons are added to the nucleus - electrons are similarly added
complex ions
M1V1=M2V2
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Aufbau Principle
33. In ideal gas law problem - when it says "atmospheric" ...
blue-green
fusion
reduction agent
Pressure of H2O must be Subtracted
34. High-energy light
Manometer
Gamma Ray-
London Dispersion Forces
Transition metals
35. (organics) four carbons
electron affinity
but-
r1/r2
titrant buret
36. The reactant in the reduction reaction that forces the oxidation reaction to occur
Transition metals
permanganate
Arrhenius acid
Oxidizing Agent
37. Pure metal or metal hydride + H20 ->
Principal Quantum Number
meth-
solid CO2
base and hydrogen gas
38. Has values 1 -2 -3 -...; tells energy levels
cyanide
Principal Quantum Number
Integrated Second-Order Rate Law
Law of Definite Proportion
39. The chemical formed when an acid donates a proton
conjugate base
bent
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Exothermic
40. Speed per molecule of gas
4.184
v3kT/m
first
cohesion
41. Combined Gas Law Formula
C + 273
P1V1/N1T1=P2V2/N2T2
n0
tetrahedral
42. A monoatomic anion is named by taking...
standard solution
Speed of light
Its root and adding -ide
Work
43. Carboxylic acid ending
-oic acid
Scientific Method
tetrahedral
Molarity
44. q cal = ?
Decrease Volume and Increase Temperature
d orbitals
end point
CAT
45. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Resonance
Exothermic
Alpha Particles-
period
46. Amine prefix
Buffer
Amino-
activated complex (transition state)
Aufbau Principle
47. Cr2O7²?
Bonding Pairs
Bond Energy
dichromate
oxidation
48. Negative enthalpy - heat flows into surroundings
Lone Pair
Heat
bromate
exothermic
49. Expresses how the concentrations depend on time
conjugate acid
Ionic Compounds
Integrated Rate Law
heat of fusion
50. negative ion
Anion
rate law
sulfide
Acid Dissociation Constant