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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. An equilibrium expression
Gamma Ray-
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Solubility Product (Ksp)
heat of fusion
2. ?H when 1 mol of bonds is broken in the gaseous state
q/moles
oxidation
Bond enthalpy
conjugate acid
3. Color of Li (flame test)
strong acids
equivalence point
red
Quantum Numbers
4. AX5E
square pyramidal
Atmospheric Pressure
no precipitate forms
nitrate
5. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
voltaic cells
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
2nd law of thermodynamics
Quantum Mechanical Model
6. Resistance to flow
viscosity
-(q of H2O + q of cal)
heat capacity
Molarity
7. Ionizes to produce H+ ions
m (third quantum number)
Atmospheric Pressure
Arrhenius Acid
Covalently w/in themselves - Ionicly bonded w/ each other
8. R in ideal gas law
Force = mass x acceleration
are not
0.0821 atm L/mol K
Transition metals
9. The amount of energy/heat required to raise some substance 1 degree C
Cation
Metalliods
alkene
Heat Capacity (C)
10. Bomb Calorimeter
Constant Volume
Entropy (S)
alcohol
voltaic cells
11. q H2O = ?
msAT
hept-
Polar Covalent
Metalliods
12. Has values from 0 to (n-1); tells shape of atomic orbitals
Law of Multiple Proportions
purple --> pink
Bases
Angular Momentum Quantum Number
13. Stronger IMF= lower... weaker IMF= higher...
Cell Potential (Ecell)
M1V1=M2V2
vapor pressure
Molecule
14. AX5
% error
mol
trigonal bipyramidal
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
15. When gas expands ...
Reducing Agent
Negative work value; work done by system
specific heat
exothermic
16. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
insoluble
hydrolysis
octahedral
purple --> pink
17. (organics) four carbons
8.314 J/K mol
Calorimetry
-ol
but-
18. CN¹?
Linear
Density
cyanide
but-
19. Forward rxn occurs when
oxide
Amino-
Q<K
London Dispersion Forces
20. Increase Volume
1 atm
Principal Quantum Number
red
Increase Temperature
21. When n=4 ->2 - color=
blue-green
0
oxalate
N=N.(0.5)^time/time half-life
22. Atoms with the same number of protons but a different number of neutrons
Amino-
Isotopes
-oate
like
23. Measure of the average kinetic energy of all the particles in a substance
Temperature
Increase Temperature
bond energy
Overall Reaction Order
24. AX6
octahedral
tetrahedral
permanent gases
Gamma Ray-
25. Organic reaction in which two functional groups come together - resulting in the release of water
adiabatic
charge
?Tb= kb x molality
condensation
26. Solid to gas
sublimation
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
force x distance = work done
endless
27. Energy needed to vaporize a mole of a liquid
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
Radioactivity
?Hvap
sulfate
28. A device in which chemical energy is changed to electrical energy
Galvanic Cell
Integrated Rate Law
Law of Conservation of Energy
Pressure of H2O must be Subtracted
29. ?T=k*m(solute)
m (third quantum number)
Molal FP Depression Constant
Bronsted-Lowry Acid
-oic acid
30. Passage of gas through tiny orifice
Effusion
red
triple point
Increase Temperature
31. Absorbs/takes in heat (positive value)
bromate
Zero-Order Rate Law
Endothermic
effects of IMF
32. Non-Ideal Gas Conditions
high pressure - low temperature
entropy (S)
Solute
lambda
33. Substances that form H+ when dissolved in water; proton donors
Chemical Bonds
Acids
Arrhenius acid
Anion
34. Electron (symbol)
Anion
Adding
Aufbau Principle
e-
35. Ester suffix
hydro-ic acid
Law of Conservation of Mass
condensation
-oate
36. J/°Cmol or J/Kmol
force x distance = work done
Molar Heat Capacity
square planar
are not
37. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
-one
Polar Covalent
insoluble
State Functions
38. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals
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39. C=2.9979*10^8 m/s
melting point
Speed of light
First-Order Half Life
Theory of Relativity
40. neutron (symbol)
n0
deposition
Integrated First-Order Rate Law
First-Order Rate Law
41. AX3E
Second-Order Rate Law
Transition metals
trigonal pyramidal
phosphate - sulfide - carbonate - sulfate
42. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
oxide
Q>K
End Point
g solute/g solvent x 100
43. Horizontals on the periodic table
endless
p orbitals
period
lambda
44. Ideal Gas Law Formula
PV=nRT
Monoprotic
Isolated System
a precipitate forms
45. High-energy light
Gamma Ray-
Law of Conservation of Mass
sublimation
Net Ionic Equation
46. The rest of the universe (in thermodynamics)
surroundings
dec-
Galvanic Cell
1.38x10?²³J/K
47. Substance that - when dissolved - is conductive
octahedral
vaporization
Law of Conservation of Energy
electrolyte
48. If Q>Ksp
amine
carbohydrates
a precipitate forms
Volume Metric Flask & Pipet
49. Atomic #
Alkaline earth metals
Pressure
# protons (atom is defined by this)
sulfite
50. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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