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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. r=k[A]^2
0.0826Latm/Kmol
Second-Order Rate Law
Kinetic Molecular Theory - for ideal gases
alcohol
2. r=k
q
Negative work value; work done by system
Zero-Order Rate Law
activated complex (transition state)
3. If Q>Ksp
purple
Bronsted-Lowry Base
a precipitate forms
yellow
4. Variable for orientation of orbital (-1 through +1)
Exothermic
Cell Potential (Ecell)
m (third quantum number)
Octahedral
5. 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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183
6. 760mmHg/Torr
1atm=?mmHg/Torr
oxide gas and water
blue
% error
7. (msubs) Can only be +1/2 or -1/2
Equilibrium constant
d
Electron Spin Quantum Number
0.512°C
8. Unit of electrical potential; J/C
different # of neutrons
8.314 J/K mol
Volt
standard solution
9. Energy required for melting to occur
2nd law of thermodynamics
sulfide
heat of fusion
trigonal bipyramidal
10. Change in Energy (AE) = ? (in terms of work)
Bond enthalpy
Ag+ - Pb2+ - Hg2+
AE = q + w
heat capacity
11. Mass percent
endothermic
reduction agent
Zero-Order Half Life
g solute/g solvent x 100
12. Symbol for the heat absorbed or lost molecularly (PER MOLE)
AH
Galvanic Cell
are not
soluble
13. Where oxidation occurs
single bond
Acid Dissociation Constant
Anode
5% rule
14. Ketone suffix
-one
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
salt bridge
T-shape
15. Faraday's constant
Atomic Mass Unit
96500
red
1 atm = 760 mmHg = 101.3 kPa
16. .69/k
First-Order Half Life
end point
Limiting reactant
yellow --> green
17. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
charge
mol Fraction
Molecular Compounds
LeChatelier's Principle
18. Nonmetal oxide + H2O ->
condensation
acid
entropy
-ic acid
19. Involves quantum numbers
-(q of H2O + q of cal)
triple point
sulfite
Quantum Mechanical Model
20. Energy involved in gaining an electron to become a negative ion
London dispersion forces
high pressure - low temperature
AE = q + w
electron affinity
21. (organics) five carbons
Acids
Metalliods
Dipole Moment
pent-
22. As protons are added to the nucleus - electrons are similarly added
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Effusion
Aufbau Principle
oxalate
23. When n=3 ->2 - color=
charge
Law of Conservation of Mass
r1/r2
red
24. Dirrect Method Formula
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
log[H+]
Cell Potential (Ecell)
?Tb= kb x molality
25. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Ionic
Acid + Base --> Salt + Water
Molar Heat Capacity
1st law of thermodynamics
26. ln[A] vs. time is a ...-order reaction
1 atm
Colligative properties
lambda
first
27. Cation first - anion second
Naming Binary Ionic Compounds
oxide gas and water
Sigma Bond
Integrated First-Order Rate Law
28. Puts H? into solution
boiling point
Arrhenius acid
M = square root (3RT/mm)
Ideal Gas Law
29. Color of Li (flame test)
A Roman numeral
Molecule
red
Law of Conservation of Mass
30. For significant digits - trailing zeros _____ significant
Molecular
period
entropy (S)
are
31. Equation to find Ea from reaction rate constants at two different temperatures
E
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
C + 273
carbonate
32. Different form of same element
allotrope
entropy (S)
Cg=kPg
Pressure of H2O must be Subtracted
33. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
red/orange
Entropy (S)
conjugate base
34. kb of water
Bond Energy
Exothermic
Metalliods
0.512°C
35. Oxidation # of Ions
increasing
chromate
Law of Conservation of Energy
charge
36. Mass #
# protons + # neutrons
like
Aufbau Principle
v3kT/m
37. Mol/L - concentration of a solution
Molecular Orbitals (MOs)
carbohydrates
Molarity
nu
38. These orbitals are perpendicular
single bond
Alkali metals
p orbitals
Multiplying
39. Mass/volume
Volt
PV=nRT
Density
base
40. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
Ligand
vapor pressure
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
purple --> pink
41. 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)
oxide gas and water
Ionic Compounds
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
endless
42. Generally insoluble anions (names)
Positive work value; work done on system
Atomic Mass Unit
Electron Spin Quantum Number
phosphate - sulfide - carbonate - sulfate
43. Energy required to break a bond
hydrocarbons
v3RT/M(in kg)
d orbitals
Bond Energy
44. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
f
Le Chatelier's Principle
P1V1/N1T1=P2V2/N2T2
45. Atoms combine in fixed whole # ratios
chlorite
3/2RT
Law of Multiple Proportions
6.63x10?³4Js
46. AX4
Anion
Constant Volume
tetrahedral
Linear
47. When n=4 ->2 - color=
Resonance
Ideal Gas Law
eth-
blue-green
48. Proton donors
Molarity
Gamma Ray-
Q>K
Bronsted-Lowry acid
49. AX6
pent-
octahedral
p+
Arrhenius acid
50. Group 2 metals
Alkaline earth metals
% yield
hydrolysis
Second-Order Rate Law