SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. (organics) eight carbons
sulfide
oct-
Percent Yield
yellow --> green
2. A measure of resistance of an object to a change in its state of motion
Mass
condensation
Bases
non-
3. Has values 1 -2 -3 -...; tells energy levels
Principal Quantum Number
red
permanganate
not spontaneous
4. Point at which vapor pressure=air pressure above
boiling point
Open System
0
Bronsted-Lowry base
5. A solid or gas that can be formed when 2 or more aqueous reactants come together
precipitate
specific heat
Molar Heat Capacity
voltaic cells
6. The likelihood that a rxn will occur "by itself"
Effusion
spontaneity
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
H
7. AP doesn't deal with ...-order reaction - don't pick it!
third
oxidation
chromate
standard solution
8. 1/([A]0*k)
n0
E
p
Second-Order Half Life
9. Proton acceptors - must have an unshared pair of e?s
Faraday
k=Ae^(-Ea/RT)
yellow
Bronsted-Lowry base
10. When _____ significant digits - round answer to least significant digit
Multiplying
t-shape
N=N.(0.5)^time/time half-life
(moles of products that are gasses) - (moles of reactants that are gasses)
11. BrO3¹?
Van't Hoff factor
3/2RT
Ideal Gas Law
bromate
12. Substances that form OH- when dissolved in water; proton acceptors
Bases
Ligand
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Normality
13. Variable for orientation of orbital (-1 through +1)
Principal Quantum Number
Barometer
Pauli Exclusion Principle
m (third quantum number)
14. Carbon & hydrogen compounds
hydroxide
purple
Molarity
hydrocarbons
15. 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
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
16. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
Amino-
activation energy
hydrolysis
Arrhenius equation
17. Amount of gravitational force exerted on an object
Reducing Agent
Weight
melting point
hydrocarbons
18. Half cell in which oxidation occurs
single bond
anode
viscosity
LeChatelier's Principle
19. MnO4¹?
permanganate
mol Fraction
entropy (S)
linear
20. 96 -485 C/mol e-
# protons (atom is defined by this)
Integrated First-Order Rate Law
Molality
Faraday
21. Increase Volume
trigonal bipyramidal
Increase Temperature
analyte
Arrhenius Base
22. Negative enthalpy - heat flows into surroundings
Ag+ - Pb2+ - Hg2+
Molality
exothermic
alcohol
23. Group 1 metals
STP
square planar
Alkali metals
strong bases
24. Planck's constant - used to calculate energy w/frequency
nitrite
prop-
6.63x10?³4Js
green/yellow
25. The weighted average of all the isotopes that an atom can have (in g/mol)
Bronsted-Lowry Acid
amine
moles solute/kg solvent
Atomic Mass Unit
26. ?T=k*m(solute)
Standard Temperature and Pressure
freezing
Hess's Law
Molal FP Depression Constant
27. Amount of product produced when limiting reactant is used up
Theoretical yield
4.184
Work
condensation
28. Thickness
End Point
r1/r2
AE = q + w
viscosity
29. =vM2/M1
Electronegativity
Ligand
r1/r2
allotrope
30. Idea Gas Law (actual rules)
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
Radioactivity
viscosity
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
31. SO3²?
k=Ae^(-Ea/RT)
Amount of atoms present
meth-
sulfite
32. (# of lone pair e-)+1/2(# of shared e-)
salt bridge
0.512°C
Buffer
Valence Electrons(assigned)
33. Everything in the universe that is not defined by you as part of the system
Multiplying
Surroundings
blue-green
condensation
34. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
electron affinity
Chemical Kinetics
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Strong acid weak base rxn
35. 1 sigma bond - 1 pi bond
-al
double bond
-oate
Average KE = 1/2(mass)(average speed of all particles)
36. Electron (symbol)
chlorite
nitrite
London dispersion forces
e-
37. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
0
London dispersion forces
Delta H or Enthalpy Change
38. The total energy of the universe is constant - all systems tend towards minimum energy
+1 - except if bonded to Alkali Metal -1
ammonium
1st law of thermodynamics
Work
39. A solution that resists a change in its pH
Buffered Solution
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Acid + Base --> Salt + Water
Exothermic
40. Substance that - when dissolved - is conductive
% error
melting
rate gas A/rate gas B = square root (mm A/ mm B)
electrolyte
41. Type of system in which the energy may escape - but the mass is conserved
-ol
base and hydrogen gas
Closed System
no precipitate forms
42. These orbitals are diagonal
Force = mass x acceleration
Magnetic Quantum Number (ml)
0
d orbitals
43. 1 sigma bond - 2 pi bonds
triple bond
1atm=?Pa
Coordination Compound
deposition
44. 2 or more covalently bonded atoms
paramagnetic
Molecule
phosphate
indicator
45. Kinetic Energy per mol
?Tb= kb x molality
3/2RT
3rd law of thermodynamics
permanent gases
46. AX2E - AX2E2
n (first quantum number)
bent
Delta H or Enthalpy Change
Theory of Relativity
47. Unit of electrical potential; J/C
-(q of H2O + q of cal)
Volt
Hund's Rule
carbohydrates
48. Bomb Calorimeter
Trigonal Planar
Zero-Order Half Life
Constant Volume
Bronsted-Lowry Acid
49. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
strong acids
sulfate
8.31J/Kmol
triple point
50. Absorbs/takes in heat (positive value)
0 degrees C - 1 atm
Endothermic
Temperature
Molar Mass of Element/ Total Molar Mass %