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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. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
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
prop-
Nodes
Resonance
2. Color of Li (flame test)
Law of Conservation of Mass
-1
Molecule
red
3. Forward rxn occurs when
Q<K
Principal Quantum Number
Scientific Method
complex ions
4. Variable for energy of e- - goes from 1 -2 -3 on up
Barometer
q/moles
Magnetic Quantum Number (ml)
n (first quantum number)
5. The chemical formed when a base accepts a proton
Joule
complex ions
conjugate acid
First-Order Rate Law
6. l=2
geometric isomers
acetate
d
work
7. We cannot simultaneously determine an atom's exact path or location
surroundings
titrant buret
Heisenberg Uncertainty Principle
Integrated Rate Law
8. Wavelength symbol
lambda
Osmotic Pressure
mol Fraction
Scientific Method
9. Ideal Gas Law Formula
spontaneity
blue-violet
PV=nRT
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
10. 760mmHg/Torr
violet
endless
End Point
1atm=?mmHg/Torr
11. NO2¹?
acetate
Quantum Numbers
Volt
nitrite
12. Oxidation # of free elements
0
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Molecule
mol
13. As protons are added to the nucleus - electrons are similarly added
Bond Energy
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
Bonding Pairs
Aufbau Principle
14. CN¹?
Zero-Order Half Life
Dipole Moment
oxidation
cyanide
15. (organics) one carbon
0
Pauli Exclusion Principle
meth-
Hund's Rule
16. Faraday's constant
Entropy (S)
Theoretical yield
96500
group
17. If Q>Ksp
Molecular Compounds
-al
a precipitate forms
3.0x108m/s
18. 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)
Galvanic Cell
Molecular Compounds
allotrope
Ionic Compounds
19. Ketone suffix
3rd law of thermodynamics
lambda
-one
strong acid strong base rxn
20. E=mc^2
condensation
Gamma Ray-
Theory of Relativity
Cathode
21. Composition Formula
22.4L
Octahedral
Molar Mass of Element/ Total Molar Mass %
rate gas A/rate gas B = square root (mm A/ mm B)
22. Point where acid completely neutralizes base
charge
equivalence point
no precipitate forms
blue-violet
23. Gain of electrons - decrease in oxidation #
standard solution
endless
Diffusion
reduction
24. C2O4²?
Atmospheric Pressure
oxalate
Hydrogen bonding
strong acids
25. ?H when 1 mol of bonds is broken in the gaseous state
System
Cation
Bond enthalpy
second
26. PO4³?
Second-Order Rate Law
Manometer
base
phosphate
27. 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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28. Spontaneous emission of radiation
f
Second-Order Half Life
Radioactivity
Percent Yield
29. Pressure Units/Conversions
Graham's Law
M1V1=M2V2
1 atm = 760 mmHg = 101.3 kPa
Molecular
30. A measure of resistance of an object to a change in its state of motion
Mass
Molarity
Acid + Base --> Salt + Water
0
31. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
phosphate
Volume Metric Flask & Pipet
Trigonal Bipyramidal
32. Absorbs/takes in heat (positive value)
Quantum Numbers
q
melting point
Endothermic
33. Gas to solid
deposition
Alkaline earth metals
Cathode
-(q of H2O + q of cal)
34. SI unit of energy; Kg*m^2/s^2
purple
Cation
Joule
a precipitate forms
35. U(rms)=(3RT/M)^1/2
Root Mean Square Velocity
Anode
Atmospheric Pressure
Joule
36. Ability of an atom in a molecule to attract shared electrons to itself
Electronegativity
Isolated System
vaporization
Equilibrium Expression
37. For significant digits - trailing zeros _____ significant
g solute/g solvent x 100
are
weak acid strong base rxn
Pauli Exclusion Principle
38. Ester suffix
-oate
Heat
Temperature
Adding
39. OH¹?
Surroundings
Pi Bond
hydroxide
Magnetic Quantum Number (ml)
40. Organic reaction in which two functional groups come together - resulting in the release of water
Integrated Zero-Order Rate Law
Calorimeter
condensation
STP
41. Color of Cs (flame test)
Boltzmann distribution
blue
Transition metals
ammonium
42. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Faraday
Colligative properties
moles solute/kg solvent
Galvanic Cell
43. Average Kinetic Energy Formula
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
0
Average KE = 1/2(mass)(average speed of all particles)
chromate
44. S²?
Solvent
Balmer Series
sulfide
adhesion
45. Ptotal=Pa+Pb+Pc....
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46. AX4E2
Solvent
square planar
M1V1=M2V2
complex ions
47. Work = ?
strong bases
-(P)(Change in V)
PV=nRT
reduction
48. AX5
Solubility Product (Ksp)
trigonal bipyramidal
Hydrogen bonding
Normality
49. The part of the universe one is focused upon (in thermodynamics)
system
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
equilibrium
Equilibrium Expression
50. Mass/volume
bromate
0.0821 atm L/mol K
flouride
Density