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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. Elements which have unpaired electrons and highly affected by magnetic fields
log[H+]
sublimation
paramagnetic
viscosity
2. The driving force for a spontaneous is an increase in entropy of the universe
C=(mass)(specific heat)
Entropy (S)
Ligand
group
3. Ability of an atom in a molecule to attract shared electrons to itself
(moles of products that are gasses) - (moles of reactants that are gasses)
CAT
Electronegativity
Bronsted-Lowry Acid
4. Mol/kg of solvent - used in calculating colligative properties
oxalate
square planar
Molality
Arrhenius Acid
5. (N) number of equivalents per liter of solution
Normality
2nd law of thermodynamics
condensation
rate law
6. Pure metal or metal hydride + H20 ->
base and hydrogen gas
Ampere
cyanide
Atmospheric Pressure
7. Nonmetal oxide + H2O ->
acid
tetrahedral
amine
Buffer
8. Substance in which something is dissolved in a solution (higher [ ])
alcohol
-(P)(Change in V)
Solvent
trigonal bipyramidal
9. Ether prefix
Acid + Base --> Salt + Water
PV=nRT
methoxy-
Allotrope
10. The weighted average of all the isotopes that an atom can have (in g/mol)
Atomic Mass Unit
melting
hept-
like
11. The reactant in the reduction reaction that forces the oxidation reaction to occur
Oxidizing Agent
acid
rate
Theory of Relativity
12. AX4E2
1st law of thermodynamics
square planar
STP
supercritical fluid
13. Molarity (M)
moles of solute/ L of solution
Overall Reaction Order
lambda
log[H+]
14. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
P1V1/N1T1=P2V2/N2T2
Gamma Ray-
Magnetic Quantum Number (ml)
diamagnetic
15. Variable for type of orbital
AH
Tetrahedral
s (fourth quantum number)
l (second quantum number)
16. R in instances that pertain to energy
M = square root (3RT/mm)
yellow
alkane
8.314 J/K mol
17. # bonding e- - # antibonding e-/2
adhesion
Bond Order
Monoprotic
Bonding Pairs
18. Polyatomic Ions (bonding)
yellow --> green
oxide gas and water
Covalently w/in themselves - Ionicly bonded w/ each other
geometric isomers
19. Average Kinetic Energy Formula
22.4L
t-shape
see-saw
Average KE = 1/2(mass)(average speed of all particles)
20. Point at which solid?liquid occurs
conjugate acid
Acid + Base --> Salt + Water
melting point
-al
21. q rxn = ?
Atmospheric Pressure
Pressure of H2O must be Subtracted
melting point
-(q of H2O + q of cal)
22. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Formal Charge
-al
Arrhenius acid
electrolyte
23. (organics) one carbon
q/moles
meth-
complex ions
Isolated System
24. Point at which the titrated solution changes color
Hydrogen bonding
critical point
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
end point
25. Energy needed to vaporize a mole of a liquid
?Hvap
endothermic
precipitate
second
26. Connects the 2 half cells in a voltaic cell
Aufbau Principle
salt bridge
a precipitate forms
3.0x108m/s
27. 109.5° - sp^3
0
Tetrahedral
Ionic
H
28. Substance being dissolved in a solution (lower [ ])
square planar
carbonate
Solute
?Hvap
29. Symbol for the heat absorbed or lost molecularly (PER MOLE)
analyte
Tetrahedral
spontaneous
AH
30. CN¹?
work
2nd law of thermodynamics
cyanide
v3RT/M(in kg)
31. l=2
Radioactivity
d
3/2RT
Temperature
32. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
2nd law of thermodynamics
deposition
Delta H or Enthalpy Change
not spontaneous
33. (organics) two carbons
experimental yield
Open System
eth-
Molarity
34. Energy needed to break a bond
bond energy
rate law
dichromate
H
35. Osmotic pressure formula
pi=(nRT)/v
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Solubility Product (Ksp)
v3kT/m
36. (organics) five carbons
freezing
permanganate
pent-
Matter
37. Puts OH? into solution
Arrhenius base
Molar Mass of Element/ Total Molar Mass %
critical point
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
38. kf of water
1.86°C
Volt
% yield
Law of Conservation of Energy
39. Mass reactants= mass products
n (first quantum number)
anode
AH
Law of Conservation of Mass
40. The reactant that is being oxidized - brings about reduction
Heat Capacity (C)
reduction agent
State Functions
Counterions
41. Molecules' tendency to stick to one another
s
cohesion
AE = q + w
Dalton's Law
42. Type of system in which nothing is transfered (no mass or energy); ideal
red
Isolated System
Integrated Zero-Order Rate Law
Colligative properties
43. Universal IMF for nonpolar molecules
Molar Heat Capacity
Electron Spin Quantum Number
Heisenberg Uncertainty Principle
London dispersion forces
44. When _____ significant digits - round answer to least significant digit
Barometer
Multiplying
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Hess's Law
45. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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46. IMF that exists in polar molecules
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Scientific Method
Cation
Dipole-dipole forces
47. Amount of gravitational force exerted on an object
solid CO2
Weight
Bond Order
alkyne
48. 101 -325 Pa
Sigma Bond
1atm=?Pa
Tetrahedral
boiling point
49. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
non-
cohesion
Allotrope
50. kb of water
methods of increasing rate
Quantum Numbers
sulfite
0.512°C