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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. Freezing point depression formula
Amount of atoms present
Isolated System
(moles of products that are gasses) - (moles of reactants that are gasses)
?Tf= kf x molality
2. Actual Yield/Theoretical Yield*100%
red
C=(mass)(specific heat)
Percent Yield
Aufbau Principle
3. The part of the universe one is focused upon (in thermodynamics)
system
activation energy
Speed of light
Amphoteric
4. Amine prefix
supercritical fluid
d orbitals
oxalate
Amino-
5. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
lambda
Arrhenius equation
non-
6. ... compounds are most conductive
ionic
trigonal bipyramidal
double bond
no precipitate forms
7. A molecule having a center of positive charge and a center of negative charge
Molarity
T-shape
Dipole Moment
like
8. 101 -325 Pa
1atm=?Pa
oxidizing agent
P1V1/N1T1=P2V2/N2T2
analyte
9. To find activation energy use the...
Constant Pressure
Arrhenius equation
Surroundings
high pressure - low temperature
10. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
Heisenberg Uncertainty Principle
Calorimeter
square planar
11. (# of lone pair e-)+1/2(# of shared e-)
chlorite
Entropy (S)
octahedral
Valence Electrons(assigned)
12. Significant Digits of counted things
phosphate - sulfide - carbonate - sulfate
d
endless
Molarity
13. Elements which have all electrons paired and relatively unaffected by magnetic fields
carbohydrates
diamagnetic
Ag+ - Pb2+ - Hg2+
A Roman numeral
14. 1/([A]0*k)
excess reactant
Ideal Gas Law
van't Hoff Factor
Second-Order Half Life
15. Temperature-pressure combination at which solid - liquid - and gas states appear
rate
heat of fusion
triple point
1 atm
16. 0.00°C - 1 atm
-2 - with peroxide -1
group
% error
Standard Temperature and Pressure
17. Spontaneous emission of radiation
oxide
Radioactivity
Molecular Compounds
s (fourth quantum number)
18. Occupies the space above and below a sigma bond
strong acids
d orbitals
nitrite
Pi Bond
19. H+ Acceptor
Angular Momentum Quantum Number
Bronsted-Lowry Base
Q>K
Molal FP Depression Constant
20. The chemical formed when a base accepts a proton
freezing
Hess's Law
conjugate acid
precipitate
21. BrO3¹?
Dalton's Law of Partial Pressures
bromate
Heat
alkyne
22. If anion ends in -ate - acid name ends in...
s
-ic acid
sulfate
22.4L
23. Anions or cations as needed to produce a compound with non net charge
Solute
Root Mean Square Velocity
Alkaline earth metals
Counterions
24. (organics) seven carbons
Amphoteric
Solution
hept-
22.4L
25. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
0.512°C
Molecular
Amino-
# protons (atom is defined by this)
26. Energy involved in gaining an electron to become a negative ion
d orbitals
electron affinity
pent-
6.63x10?³4Js
27. Raising heat - adding catalyst - heighten concentration - bigger surface area
allotrope
hydroxide
Cell Potential (Ecell)
methods of increasing rate
28. For significant digits - trailing zeros _____ significant
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
second
Second-Order Half Life
are
29. AX5E
Cathode
Kinetic Molecular Theory - for ideal gases
square pyramidal
bromate
30. Chemical composition of dry ice
triple point
Standard Temperature and Pressure
strong acid strong base rxn
solid CO2
31. SO4²?
Pressure of H2O must be Subtracted
Surroundings
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
sulfate
32. % yield
square planar
system
actual yield/theoretical yield x 100%
solid CO2
33. l=0
s
vaporization
experimental yield
geometric isomers
34. Anything occupying space and with mass
Scientific Method
wavelength
red
Matter
35. MnO4¹?
permanganate
v3kT/m
d orbitals
Adding
36. In ideal gas law problem - when it says "atmospheric" ...
Counterions
Pressure of H2O must be Subtracted
heat capacity
sulfate
37. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
s orbitals
Closed System
melting point
38. When gas expands ...
Cathode
catalyst
Solvent
Negative work value; work done by system
39. Ability of an atom in a molecule to attract shared electrons to itself
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
double bond
Molecule
Electronegativity
40. The driving force for a spontaneous is an increase in entropy of the universe
Kinetic Molecular Theory - for ideal gases
Net Ionic Equation
Entropy (S)
-oate
41. Osmotic pressure formula
pi=(nRT)/v
London dispersion forces
endothermic
purple --> pink
42. Substances that form H+ when dissolved in water; proton donors
Hess's Law
0.0826Latm/Kmol
Acids
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
43. Symbol for Enthalpy
1.38x10?²³J/K
Transition metals
-oic acid
H
44. Variable for spin of electron (+.5 or -.5)
# protons + # neutrons
s (fourth quantum number)
chlorate
Cathode
45. Type of system in which the energy and mass may leave or enter
Volume Metric Flask & Pipet
Hydrogen bonding
Open System
hydroxide
46. Unit of electrical potential; J/C
Molecular
Volt
hydrocarbons
Angular Momentum Quantum Number
47. neutron (symbol)
-al
Chemical Bonds
alkene
n0
48. E=mc^2
Transition metals
Specific Heat Capacity
Calorimetry
Theory of Relativity
49. Carboxylic acid ending
oxidation
-oic acid
Monoprotic
boiling point
50. Universal IMF for nonpolar molecules
London dispersion forces
Arrhenius Acid
Principal Quantum Number
Anion