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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. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Chemical Bonds
London dispersion forces
Resonance
force x distance = work done
2. q rxn = ?
-(q of H2O + q of cal)
melting
high pressure - low temperature
1/2mv²
3. Melting
P1= X1P1°
Net Ionic Equation
perchlorate
fusion
4. (organics) six carbons
hex-
sulfate
Pi Bond
l (second quantum number)
5. Combined Gas Law Formula
P1V1/N1T1=P2V2/N2T2
non-
blue-green
Alkali metals
6. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
iodide
but-
activation energy
7. Boltzmann constant - used in calculating speed of gas per molecule
Hess's Law
1.38x10?²³J/K
third
C=(mass)(specific heat)
8. Colors of Reaction when (MnO4 -) --> (Mn2+)
Molality
purple --> pink
eth-
Bond enthalpy
9. AX5
Metalliods
d orbitals
trigonal bipyramidal
Tetrahedral
10. 96 -485 C/mol e-
AE = q + w
Quantum Model
Bronsted-Lowry base
Faraday
11. Measure of the average kinetic energy of all the particles in a substance
Law of Conservation of Energy
Arrhenius equation
Temperature
n0
12. J/°Cmol or J/Kmol
Thermochemistry
Molar Heat Capacity
Heat Capacity (C)
strong acids
13. Group 1 metals
Alkali metals
Exothermic
Electron Spin Quantum Number
0
14. Amount of heat needed to change a system by 1°C
Mass
heat capacity
blue-violet
charge
15. We cannot simultaneously determine an atom's exact path or location
Heisenberg Uncertainty Principle
not spontaneous
charge
Le Chatelier's Principle
16. Polyatomic Ions (bonding)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
violet
Covalently w/in themselves - Ionicly bonded w/ each other
Anode
17. Ionizes to produce H+ ions
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Arrhenius Acid
Integrated Rate Law
msAT
18. 6.022x10^23
Anode
Volume Metric Flask & Pipet
London dispersion forces
mol
19. Mass percent
Percent Yield
g solute/g solvent x 100
nitrate
Specific Heat (s)
20. Average speed of gas
v3RT/M(in kg)
Bronsted-Lowry acid
5% rule
Pi Bond
21. Two molecules with identical connectivity but different geometries
Ampere
geometric isomers
1.38x10?²³J/K
0.0826Latm/Kmol
22. Unit of electrical potential; J/C
blue-violet
Volt
square planar
strong acids
23. Occupies the space above and below a sigma bond
0
Average KE = 1/2(mass)(average speed of all particles)
Pi Bond
d orbitals
24. Elements on staircase on periodic table
Volt
Solution
Metalliods
m (third quantum number)
25. Mols A/ total mols - XA
mol Fraction
Hybridization
a precipitate forms
hydrocarbons
26. A measure of randomness or disorder
Closed System
entropy
different # of neutrons
Galvanic Cell
27. kb of water
0.512°C
sulfate
s
Bronsted-Lowry acid
28. Mol/L - concentration of a solution
trigonal bipyramidal
Magnetic Quantum Number (ml)
like
Molarity
29. Each orbital can hold two e?s each w/ opposite spins
a precipitate forms
Principal Quantum Number
Alpha Particles-
Pauli Exclusion Principle
30. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Osmotic Pressure
Molecular
charge
X of a = moles a/total moles
31. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
conjugate base
-(q of H2O + q of cal)
Ionic Compounds
Transition metals
32. CN¹?
State Functions
Angular Momentum Quantum Number
cyanide
green/yellow
33. AX5E
Radioactivity
square pyramidal
Van't Hoff factor
1st law of thermodynamics
34. Type of system in which the energy may escape - but the mass is conserved
Kinetic Molecular Theory - for ideal gases
Closed System
Diffusion
iodide
35. Change in Energy = ? (in terms of constant pressure; for gasses)
AE= AH - RTAn
Normality
Percent Yield
PV=nRT
36. Donates a single H+ Ion (... other prefixes also)
chlorate
Equilibrium Expression
Monoprotic
experimental yield
37. Atoms combine in fixed whole # ratios
End Point
yellow --> green
Law of Multiple Proportions
heat of fusion
38. Variable for spin of electron (+.5 or -.5)
Molar Mass of Element/ Total Molar Mass %
s (fourth quantum number)
+1 - except if bonded to Alkali Metal -1
Acid Dissociation Constant
39. Similar to atomic orbitals - except between molecules
sulfate
Molecular Orbitals (MOs)
spontaneity
Heat Capacity (C)
40. Type of system in which nothing is transfered (no mass or energy); ideal
hydrolysis
alcohol
Exothermic
Isolated System
41. Oxidation # of free elements
blue-green
trigonal planar
freezing
0
42. The measurement of heat changes
Density
Calorimetry
-(q of H2O + q of cal)
Force = mass x acceleration
43. Increase Pressure
Scientific Method
Decrease Volume and Increase Temperature
-ol
Oxidizing Agent
44. Different form of same element
effects of IMF
bromate
allotrope
strong acid strong base rxn
45. Electron (symbol)
e-
Work
Colligative properties
viscosity
46. Type of system in which the energy and mass may leave or enter
Arrhenius base
e-
sublimation
Open System
47. Gas to liquid
yellow --> green
log[H+]
endless
condensation
48. If heat capacity isn't mentioned - you can assume that q of cal is = ?
-ol
0
Ionic Compounds
Constant Pressure
49. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
-(q of H2O + q of cal)
Le Chatelier's Principle
Nernst Equation
50. Elements which have all electrons paired and relatively unaffected by magnetic fields
melting point
diamagnetic
Principal Quantum Number
Dalton's Law of Partial Pressures