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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. A method of investigation involving observation and theory to test scientific hypotheses
different # of neutrons
Scientific Method
Second-Order Half Life
actual yield/theoretical yield x 100%
2. Diatomic Molecules
sulfide
Bond enthalpy
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
A Roman numeral
3. 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
e-
Finding Empirical Formulas
isothermal
s
4. Ptotal=Pa+Pb+Pc....
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5. When gas compresses ...
exothermic
oxide
Manometer
Positive work value; work done on system
6. Larger molecules which have higher mass and therefore electron density have stronger...
Bronsted-Lowry base
Antibonding Molecular Orbital
London dispersion forces
Colligative properties
7. Ending for alcohols
g solute/g solvent x 100
-ol
Bond enthalpy
1 atm = 760 mmHg = 101.3 kPa
8. Phase change from gas to solid
n (first quantum number)
conjugate acid
Exothermic
deposition
9. When n=6 ->2 - color=
PV=nRT
violet
Polar Covalent
Molality
10. Temperature-pressure combination at which solid - liquid - and gas states appear
0
Anion
triple point
Arrhenius Acid
11. Faraday's constant
alkene
96500
0
Multiplying
12. r=k[A]^2
Second-Order Rate Law
not spontaneous
hex-
surroundings
13. Change that occurs at constant temperature
Calorimeter
AE= AH - RTAn
isothermal
Resonance
14. Point at which vapor pressure=air pressure above
ether
boiling point
-al
Antibonding Molecular Orbital
15. Non-Ideal Gas Conditions
0.0821 atm L/mol K
Chemical Kinetics
high pressure - low temperature
Second-Order Half Life
16. Polyatomic Ions (bonding)
Ideal Gas Law
Covalently w/in themselves - Ionicly bonded w/ each other
Formal Charge
+1 - except if bonded to Alkali Metal -1
17. The entropy of a pure perfectly formed crystal @0K is 0
weak acid strong base rxn
heat of vaporization
3rd law of thermodynamics
Speed of light
18. Point where acid completely neutralizes base
hydro-ic acid
Boltzmann distribution
equivalence point
Isolated System
19. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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20. Color of Cs (flame test)
blue
Hydrogen bonding
l (second quantum number)
Chemical Bonds
21. Symbol for the heat absorbed or lost molecularly (PER MOLE)
Force = mass x acceleration
AH
no precipitate forms
Graham's Law
22. A measure of resistance of an object to a change in its state of motion
l (second quantum number)
Mass
Heisenberg Uncertainty Principle
M = square root (3RT/mm)
23. J/°Cmol or J/Kmol
like
Molar Heat Capacity
Temperature
Amount of atoms present
24. kb of water
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
p orbitals
hydro-ic acid
0.512°C
25. For significant digits - trailing zeros _____ significant
mol Fraction
anode
like
are
26. SI unit of energy; Kg*m^2/s^2
-1
oct-
Joule
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
27. (N) number of equivalents per liter of solution
strong acids
analyte
Normality
alkyne
28. Coffee Cup Calorimeter
entropy
Coordination Compound
Constant Pressure
1 atm = 760 mmHg = 101.3 kPa
29. Electron pairs found in the space between the atoms
r1/r2
ammonium
high pressure - low temperature
Bonding Pairs
30. When n=3 ->2 - color=
red
sulfide
d
Molar Heat Capacity
31. l=3
Constant Pressure
f
entropy
spontaneity
32. Amine prefix
Hund's Rule
Heisenberg Uncertainty Principle
Amino-
22.4L
33. Heat needed to change 1 g of substance to 1°C
specific heat
Amphoteric
1.86°C
triple bond
34. Freezing point depression formula
Hess's Law
Valence Electrons(assigned)
weak acid strong base rxn
?Tf= kf x molality
35. CrO4²?
Polar Covalent
Molar Mass of Element/ Total Molar Mass %
chromate
Joule
36. Everything in the universe that is not defined by you as part of the system
Surroundings
Calorimeter
force x distance = work done
3.0x108m/s
37. # bonding e- - # antibonding e-/2
Dipole Moment
chlorite
Bond Order
Nernst Equation
38. A monoatomic anion is named by taking...
Its root and adding -ide
pi=(nRT)/v
Arrhenius Acid
Bases
39. AX3E
s
trigonal pyramidal
0 degrees C - 1 atm
-2 - with peroxide -1
40. l=1
fusion
2nd law of thermodynamics
96500
p
41. The reactant in the reduction reaction that forces the oxidation reaction to occur
Dipole-dipole forces
octahedral
Oxidizing Agent
Temperature
42. Oxidation # of Ions
charge
Arrhenius equation
Pauli Exclusion Principle
Constant Volume
43. The transfer of energy between two objects due to temperature difference
red
AE= AH - RTAn
Heat
Osmotic Pressure
44. Group 2 metals
0
6.63x10?³4Js
Beta Particles-
Alkaline earth metals
45. kf of water
t-shape
1.86°C
square pyramidal
dec-
46. Elements in groups 3-12
cathode
solid CO2
flouride
Transition metals
47. High-energy light
single bond
Force = mass x acceleration
Work
Gamma Ray-
48. Cr2O7²?
Constant Pressure
LE Model
Pi Bond
dichromate
49. K
deposition
Equilibrium constant
l (second quantum number)
moles of solute/ L of solution
50. SO3²?
sulfite
group
Sigma Bond
Heisenberg Uncertainty Principle