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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. Connects the 2 half cells in a voltaic cell
third
salt bridge
Entropy (S)
0.0826Latm/Kmol
2. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Law of Multiple Proportions
t-shape
Cathode
E
3. Change in Energy = ? (in terms of constant pressure; for gasses)
second
lambda
0.0821 atm L/mol K
AE= AH - RTAn
4. Faraday's constant
STP
96500
First-Order Half Life
equivalence point
5. 760mmHg/Torr
endless
1atm=?mmHg/Torr
mol
Cg=kPg
6. Ka=[products]^m/[reactants]^n
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
cyanide
Acid Dissociation Constant
Increase Temperature
7. Amount of product produced when limiting reactant is used up
Integrated Rate Law
Ligand
Alkali metals
Theoretical yield
8. Occupies the space above and below a sigma bond
Pi Bond
voltaic cells
Pauli Exclusion Principle
1atm=?Pa
9. C=2.9979*10^8 m/s
standard solution
Theoretical yield
Anion
Speed of light
10. Rate of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Formal Charge
voltaic cells
amine
11. (organics) one carbon
high pressure - low temperature
meth-
Gamma Ray-
oxidation
12. Ecell= E°cell -RT/nF x lnQ
Aufbau Principle
supercritical fluid
Nernst Equation
experimental yield
13. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Anode
Zero-Order Half Life
Endothermic
14. When n=4 ->2 - color=
Arrhenius Base
X of a = moles a/total moles
blue-green
critical point
15. Symbol for Enthalpy
Pressure of H2O must be Subtracted
Q<K
H
reduction agent
16. ?T=k*m(solute)
Linear
PV=nRT
Equilibrium Expression
Molal BP Elevation Constant
17. Substance being dissolved in a solution (lower [ ])
Heisenberg Uncertainty Principle
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
Solute
methoxy-
18. Proton donors
Bronsted-Lowry acid
AH
Buffered Solution
Gamma Ray-
19. ln[A]=-kt + ln[A]0
STP
1/2mv²
Pi Bond
Integrated First-Order Rate Law
20. 0°C and 1 atm
STP
triple bond
k=Ae^(-Ea/RT)
l (second quantum number)
21. Mass/volume
Density
Theory of Relativity
e-
Q>K
22. AX3E2
paramagnetic
melting
t-shape
van't Hoff Factor
23. The rest of the universe (in thermodynamics)
single bond
Temperature
surroundings
Q>K
24. ?H when 1 mol of bonds is broken in the gaseous state
Bond enthalpy
Van't Hoff factor
London dispersion forces
Ionic Compounds
25. OIL RIG
critical point
viscosity
Oxidation is Loss Reduction is Gain
Specific Heat Capacity
26. Change that occurs at constant temperature
Matter
isothermal
Manometer
End Point
27. Anions or cations as needed to produce a compound with non net charge
Counterions
1.38x10?²³J/K
dichromate
Joule
28. A measure of randomness or disorder
1/2mv²
indicator
entropy
endothermic
29. Half-life equation
N=N.(0.5)^time/time half-life
Formal Charge
Anion
?Tb= kb x molality
30. If anion ends in -ite - acid name ends in...
-ous acid
heat of fusion
Balmer Series
Bonding Pairs
31. A method of investigation involving observation and theory to test scientific hypotheses
-1
green/yellow
heat capacity
Scientific Method
32. What is defined by you taken from the whole universe
Osmotic Pressure
Normality
Molal BP Elevation Constant
System
33. We cannot simultaneously determine an atom's exact path or location
-oate
1 atm = 760 mmHg = 101.3 kPa
activation energy
Heisenberg Uncertainty Principle
34. All forms of energy except for heat
rate
work
Pressure
Reaction Quotient (Q)
35. 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
36. Energy needed to vaporize a mole of a liquid
a precipitate forms
% error
?Hvap
-oate
37. AX4E2
Heat Capacity (C)
l (second quantum number)
square planar
22.4L
38. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
Pi Bond
Kinetic Molecular Theory - for ideal gases
mol
P1V1/N1T1=P2V2/N2T2
39. # bonding e- - # antibonding e-/2
Cation
Metalliods
mol Fraction
Bond Order
40. Electron pairs found in the space between the atoms
acetate
Kinetic Molecular Theory - for ideal gases
Bonding Pairs
Resonance
41. Ability of an atom in a molecule to attract shared electrons to itself
supercritical fluid
Electronegativity
specific heat
Exothermic
42. F¹?
flouride
Solute
Bonding Pairs
critical point
43. Energy can't be created nor destroyed
Law of Conservation of Energy
exothermic
Oxidation is Loss Reduction is Gain
Gamma Ray-
44. Raoult's Law - relations between vapor pressure and concentrations
P1= X1P1°
strong bases
trigonal planar
precipitate
45. Moles of solute/volume of soln(L)
meth-
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
red
Molarity
46. A solution used in titrations whose concentration is known
Acid Dissociation Constant
3/2RT
standard solution
Graham's Law
47. Symbol for Total Heat absorbed or released
anode
3/2RT
q
endothermic
48. AX6
Negative work value; work done by system
STP
octahedral
Transition metals
49. HF+ OH??H2O
weak acid strong base rxn
Its element
octahedral
e-
50. [A]=-kt + [A]0
activation energy
Transition metals
Volt
Integrated Zero-Order Rate Law