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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. Amount of product produced when limiting reactant is used up
Bronsted-Lowry base
Open System
Theoretical yield
P1V1/N1T1=P2V2/N2T2
2. AX3
4.184
trigonal planar
r1/r2
strong acids
3. Has values 1 -2 -3 -...; tells energy levels
Hess's Law
dec-
Principal Quantum Number
1 atm
4. Ecell= E°cell -RT/nF x lnQ
Entropy (S)
flouride
yellow --> green
Nernst Equation
5. Mass reactants= mass products
Law of Conservation of Mass
Hund's Rule
Antibonding Molecular Orbital
spontaneous
6. Ka=[products]^m/[reactants]^n
Pauli Exclusion 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
Acid Dissociation Constant
purple --> pink
7. AX3E2
Monoprotic
0.0821 atm L/mol K
T-shape
Force = mass x acceleration
8. Measure of the average kinetic energy of all the particles in a substance
Cg=kPg
triple point
Temperature
Solution
9. Ionizes to produce H+ ions
Monoprotic
Standard Temperature and Pressure
Arrhenius Acid
Volume Metric Flask & Pipet
10. A weak acid that changes color at or near the equivalence point
Graham's Law
square planar
Molecular Compounds
indicator
11. Oxidation # of free elements
Specific Heat Capacity
k=Ae^(-Ea/RT)
0
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
12. AX6
catalyst
square pyramidal
octahedral
equilibrium
13. Energy can't be created nor destroyed
Isotopes
hept-
Law of Conservation of Energy
square planar
14. Point at which solid?liquid occurs
melting point
freezing
-ic acid
Molarity
15. 2+ charge
trigonal planar
-ol
Kinetic Molecular Theory - for ideal gases
Alpha Particles-
16. Isotope
different # of neutrons
8.314 J/K mol
Quantum Mechanical Model
Manometer
17. Gain of electrons - decrease in oxidation #
Antibonding Molecular Orbital
Percent Yield
reduction
ether
18. (organics) five carbons
pent-
-ic acid
single bond
Matter
19. Generally insoluble anions (names)
1 atm = 760 mmHg = 101.3 kPa
phosphate - sulfide - carbonate - sulfate
96500
State Functions
20. Anions or cations as needed to produce a compound with non net charge
chromate
Counterions
London dispersion forces
a precipitate forms
21. Color of Cs (flame test)
Trigonal Planar
blue
Bronsted-Lowry Acid
viscosity
22. Color of Na (flame test)
third
yellow
Q<K
chloride
23. Expresses how the concentrations depend on time
log[H+]
Integrated Rate Law
Molar Heat Capacity
wavelength
24. Type of system in which the energy and mass may leave or enter
Barometer
Open System
Closed System
?Tb= kb x molality
25. The heat changed in a chemical reaction.
effects of IMF
group
Pressure of H2O must be Subtracted
Thermochemistry
26. AX4
tetrahedral
sublimation
8.31J/Kmol
-ous acid
27. Puts H? into solution
Bronsted-Lowry Acid
excess reactant
Arrhenius acid
London dispersion forces
28. ln[A] vs. time is a ...-order reaction
first
sulfide
Bronsted-Lowry Acid
nu
29. q cal = ?
nitrate
First-Order Rate Law
Faraday
CAT
30. Oxidation # of Polyatomic Ions
charge
but-
0
Bronsted-Lowry Acid
31. SO3²?
Standard Temperature and Pressure
heat capacity
but-
sulfite
32. The rest of the universe (in thermodynamics)
-ic acid
Work
no precipitate forms
surroundings
33. 1/[A]=kt + 1/[A]0
Integrated First-Order Rate Law
square pyramidal
linear
Integrated Second-Order Rate Law
34. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
d orbitals
deposition
LE Model
35. Energy involved in gaining an electron to become a negative ion
Arrhenius Base
permanent gases
electron affinity
Kinetic Molecular Theory - for ideal gases
36. Ionizes to produce OH- Ions
Standard Temperature and Pressure
Metalliods
Arrhenius Base
# protons + # neutrons
37. AH of formation for a substance in its stablest form (how it is found in nature)
0
Solute
Graham's Law
equivalence point
38. Forward rxn occurs when
oxidation
Q<K
strong acid strong base rxn
Isolated System
39. Group 2 metals
not spontaneous
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
red/orange
Alkaline earth metals
40. [A]=-kt + [A]0
0
Integrated Zero-Order Rate Law
s (fourth quantum number)
Isolated System
41. AX4E
see-saw
base and hydrogen gas
high pressure - low temperature
Q<K
42. 0°C and 1 atm
Cation
Law of Multiple Proportions
STP
State Functions
43. =vM2/M1
increasing
Aufbau Principle
r1/r2
f
44. Verticals on the periodic table
Zero-Order Rate Law
heat of vaporization
Counterions
group
45. ln[A]=-kt + ln[A]0
hex-
Angular Momentum Quantum Number
q
Integrated First-Order Rate Law
46. Cr2O7²?
green/yellow
dichromate
Bond enthalpy
Nernst Equation
47. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
Bond Energy
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
heat of fusion
48. The driving force for a spontaneous is an increase in entropy of the universe
moles of solute/ L of solution
Entropy (S)
-2 - with peroxide -1
indicator
49. K
1.38x10?²³J/K
acetate
perchlorate
Equilibrium constant
50. I=moles of particles/moles of solute dissolved
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