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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. Where reduction occurs
Covalently w/in themselves - Ionicly bonded w/ each other
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Cathode
% error
2. n+m (these are orders of reactants)
diamagnetic
AH
Overall Reaction Order
ionic
3. The weighted average of all the isotopes that an atom can have (in g/mol)
q/moles
vaporization
Atomic Mass Unit
Anode
4. Cation first - anion second
Naming Binary Ionic Compounds
oxide gas and water
Radioactivity
solid CO2
5. Carbon & hydrogen compounds
Bonding Pairs
1atm=?mmHg/Torr
P1V1/N1T1=P2V2/N2T2
hydrocarbons
6. Describe various properties of one orbital
Quantum Numbers
Scientific Method
Counterions
-one
7. frequency symbol
p+
3.0x108m/s
nu
triple bond
8. Ether prefix
freezing
1atm=?Pa
methoxy-
endothermic
9. Mol/L - concentration of a solution
Adding
triple bond
0.0821 atm L/mol K
Molarity
10. SI unit of energy; Kg*m^2/s^2
AE = q + w
Joule
s
excess reactant
11. BrO3¹?
electrolyte
Molecule
bromate
Solution
12. Elements on staircase on periodic table
Metalliods
condensation
lambda
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
13. Cr2O7²?
dichromate
cyanide
Average KE = 1/2(mass)(average speed of all particles)
Temperature
14. 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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15. The reactant that is being reduced - brings about oxidation
0
oxidizing agent
-oic acid
viscosity
16. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
Solution
3rd law of thermodynamics
increasing
17. S²?
Average KE = 1/2(mass)(average speed of all particles)
mol Fraction
Atmospheric Pressure
sulfide
18. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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19. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
s
Ligand
anode
r1/r2
20. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
v3RT/M(in kg)
Reaction Quotient (Q)
sublimation
Resonance
21. 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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22. Has values 1 -2 -3 -...; tells energy levels
Principal Quantum Number
Nodes
blue-green
Constant Volume
23. Boiling point elevation formula
Molal FP Depression Constant
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Law of Multiple Proportions
?Tb= kb x molality
24. Kinetic Energy of an individual particle formula
purple --> pink
M = square root (3RT/mm)
-ous acid
H
25. Kinetic Energy is proportional to ______
endless
Temperature
Speed of light
adiabatic
26. Expresses how the concentrations depend on time
H
Integrated Rate Law
different # of neutrons
electrolyte
27. Weakest IMFs - found in all molecules
Dalton's Law of Partial Pressures
Quantum Model
linear
London dispersion forces
28. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Formal Charge
Equilibrium Expression
Hydrogen bonding
heat capacity
29. An equilibrium expression
force x distance = work done
Solubility Product (Ksp)
Ideal Gas Law
system
30. ?Hsoln=?H1+?H2+?H3+...
square pyramidal
Enthalpy of Solution
methods of increasing rate
1 atm
31. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
octahedral
soluble
Reducing Agent
trigonal bipyramidal
32. Volume of gas @STP
dichromate
complex ions
vaporization
22.4L
33. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
PV=nRT
green/yellow
Bond Order
voltaic cells
34. Spectrum of light when an electron drops to energy level n=2
Pressure
Balmer Series
t-shape
Ag+ - Pb2+ - Hg2+
35. Solution used in titration
Hess's Law
e-
titrant buret
Its element
36. (organics) three carbons
Hydrogen bonding
prop-
octahedral
alkyne
37. Boltzmann constant - used in calculating speed of gas per molecule
Electronegativity
0
1.38x10?²³J/K
Radioactivity
38. OH¹?
methods of increasing rate
H
hydroxide
equilibrium
39. Atomic #
# protons (atom is defined by this)
Entropy (S)
Chemical Bonds
v3kT/m
40. Mol of solute/kg of solvent
n (first quantum number)
Electron Spin Quantum Number
1.86°C
Molality
41. Nonmetal oxide + H2O ->
sublimation
3rd law of thermodynamics
acid
Cation
42. Hydroxides are soluble or insoluble?
Dipole-dipole forces
hydrocarbons
insoluble
analyte
43. Isotope
phosphate - sulfide - carbonate - sulfate
0
different # of neutrons
oxidation
44. These orbitals are diagonal
Bronsted-Lowry base
oct-
d orbitals
-2 - with peroxide -1
45. Type of system in which nothing is transfered (no mass or energy); ideal
deposition
System
Root Mean Square Velocity
Isolated System
46. Type of system in which the energy and mass may leave or enter
-one
Open System
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
allotrope
47. Chemical composition of dry ice
solid CO2
Mass
Ligand
Gamma Ray-
48. Mole Fraction
X of a = moles a/total moles
but-
cohesion
conjugate acid
49. Speed of Diffusion/Effusion formula
Law of Multiple Proportions
Average KE = 1/2(mass)(average speed of all particles)
rate gas A/rate gas B = square root (mm A/ mm B)
geometric isomers
50. Color of Ca (flame test)
red/orange
Percent Yield
experimental yield
First-Order Rate Law