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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. The chemical formed when a base accepts a proton
Bases
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
PV=nRT
conjugate acid
2. Amount of gravitational force exerted on an object
C + 273
M1V1=M2V2
Weight
tetrahedral
3. Where reduction occurs
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
Bronsted-Lowry base
van't Hoff Factor
Cathode
4. Change that occurs at constant temperature
1st law of thermodynamics
isothermal
perchlorate
Hund's Rule
5. AX5E
1.86°C
chloride
square pyramidal
trigonal bipyramidal
6. ClO4¹?
perchlorate
Quantum Numbers
Formal Charge
charge
7. Involves quantum numbers
Quantum Mechanical Model
AE= AH - RTAn
adhesion
Positive work value; work done on system
8. Energy needed to break a bond
bond energy
-oate
weak acid strong base rxn
Integrated Zero-Order Rate Law
9. (organics) four carbons
# protons + # neutrons
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
tetrahedral
but-
10. Dalton's Law of Partial Pressures (to find partial pressure formula)
entropy
P of a =(X of a)(total pressure)
acid
voltaic cells
11. STP
0 degrees C - 1 atm
nu
oxide gas and water
lambda
12. AP doesn't deal with ...-order reaction - don't pick it!
charge
third
moles of solute/ L of solution
Allotrope
13. In a given atom no two electrons can have the same set of four quantum numbers
C + 273
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
Pauli Exclusion Principle
anode
14. Osmotic pressure=MRT
Osmotic Pressure
System
Amount of atoms present
hex-
15. Degree of disorder in a system
Average KE = 1/2(mass)(average speed of all particles)
Ag+ - Pb2+ - Hg2+
wavelength
entropy (S)
16. Speed of light - C
Integrated Second-Order Rate Law
3.0x108m/s
l (second quantum number)
Solute
17. Gas to liquid
Amphoteric
Equilibrium constant
condensation
equilibrium
18. Organic w/ -OH group
Finding Empirical Formulas
tetrahedral
alcohol
effects of IMF
19. Carboxylic acid ending
Cathode
-oic acid
Ionic
double bond
20. Energy required for liquid?gas
carbohydrates
permanganate
Amino-
heat of vaporization
21. How to Find a Weighted Average
Alkaline earth metals
titrant buret
Solute
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
22. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Dipole Moment
effects of IMF
Manometer
Molal BP Elevation Constant
23. Type of system in which the energy may escape - but the mass is conserved
Closed System
double bond
first
oxalate
24. 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)
Molecular Compounds
zero
chloride
Molality
25. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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26. ln[A] vs. time is a ...-order reaction
first
Molar Mass of Element/ Total Molar Mass %
hydrocarbons
Law of Multiple Proportions
27. Connects the 2 half cells in a voltaic cell
salt bridge
yellow --> green
Reaction Quotient (Q)
M1V1=M2V2
28. (organics) three carbons
seesaw
AH
permanganate
prop-
29. AX5
trigonal bipyramidal
LE Model
endothermic
zero
30. l=0
oxidizing agent
Nodes
Bases
s
31. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
conjugate acid
nitrite
no precipitate forms
Finding Empirical Formulas
32. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
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33. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Equilibrium Expression
Bronsted-Lowry base
Magnetic Quantum Number (ml)
Endothermic
34. Point where acid completely neutralizes base
0.0821 atm L/mol K
Acids
Law of Conservation of Energy
equivalence point
35. Boltzmann constant - used in calculating speed of gas per molecule
Ionic Compounds
Law of Conservation of Energy
1.38x10?²³J/K
trigonal bipyramidal
36. Energy (definition)
blue-violet
force x distance = work done
Diffusion
entropy
37. A monoatomic cation takes name from...
melting point
Its element
hydrocarbons
0
38. 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)
Force = mass x acceleration
p
linear
Ionic Compounds
39. Organic reaction in which two functional groups come together - resulting in the release of water
Zero-Order Half Life
heat of fusion
condensation
f
40. Color of Cs (flame test)
conjugate acid
N=N.(0.5)^time/time half-life
prop-
blue
41. H + donor
Bronsted-Lowry Acid
cohesion
chromate
Magnetic Quantum Number (ml)
42. Moles of solute/volume of soln(L)
Molarity
3.0x108m/s
alkane
p orbitals
43. Chemical composition of dry ice
Bases
van't Hoff Factor
q
solid CO2
44. Donates a single H+ Ion (... other prefixes also)
Monoprotic
analyte
s (fourth quantum number)
Solute
45. How to Find an Empirical Formula Given Percentages
d
3rd law of thermodynamics
Arrhenius base
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
46. If Q<Ksp
q
no precipitate forms
nu
0
47. Tools NEEDED for dilution
pent-
Galvanic Cell
critical point
Volume Metric Flask & Pipet
48. Composition Formula
phosphate - sulfide - carbonate - sulfate
s
Molar Mass of Element/ Total Molar Mass %
are
49. 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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50. Variable for spin of electron (+.5 or -.5)
Alkaline earth metals
first
s (fourth quantum number)
Zero-Order Half Life