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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. Atomic #
log[H+]
Ag+ - Pb2+ - Hg2+
# protons (atom is defined by this)
rate law
2. Like dissolves...
like
Faraday
geometric isomers
triple bond
3. If anion ends in -ite - acid name ends in...
Dipole Moment
Principal Quantum Number
-ous acid
fusion
4. Mol/L - concentration of a solution
Molarity
Arrhenius equation
Molecular Orbitals (MOs)
endless
5. Horizontals on the periodic table
Theoretical yield
period
8.314 J/K mol
actual yield/theoretical yield x 100%
6. Color of Li (flame test)
purple --> pink
T-shape
Acids
red
7. 2+ charge
Alpha Particles-
Molal BP Elevation Constant
diamagnetic
f
8. PV=nRT
Acid Dissociation Constant
Solution
Formal Charge
Ideal Gas Law
9. (organics) five carbons
Hydrogen bonding
P1V1/N1T1=P2V2/N2T2
pent-
Le Chatelier's Principle
10. Involves quantum numbers
Molecular Compounds
Quantum Mechanical Model
Bronsted-Lowry Acid
blue-green
11. All _________ compounds are electrolytes
triple bond
Ionic
Equilibrium constant
deposition
12. ClO2¹?
Surroundings
Arrhenius Base
Delta H or Enthalpy Change
chlorite
13. Atoms with the same number of protons but a different number of neutrons
PV=nRT
Isotopes
Electron Spin Quantum Number
Quantum Model
14. Substance that - when dissolved - is conductive
electrolyte
End Point
meth-
Law of Conservation of Energy
15. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Alpha Particles-
r1/r2
fusion
Molecular
16. Speed of Diffusion/Effusion formula
nitrate
rate gas A/rate gas B = square root (mm A/ mm B)
Cathode
endless
17. Rate of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Calorimeter
Isotopes
paramagnetic
18. Two molecules with identical connectivity but different geometries
Heat
allotrope
geometric isomers
0.0826Latm/Kmol
19. x can be ignored when % ionization is <5%
Magnetic Quantum Number (ml)
Law of Multiple Proportions
5% rule
Law of Multiple Proportions
20. Proton acceptors - must have an unshared pair of e?s
Bronsted-Lowry base
oct-
oxide gas and water
Molal BP Elevation Constant
21. Group 1 metals
Cathode
Its root and adding -ide
anode
Alkali metals
22. Oxidation # of Ions
hydro-ic acid
supercritical fluid
3.0x108m/s
charge
23. Non-Ideal Gas Conditions
hydro-ic acid
pent-
high pressure - low temperature
equilibrium
24. Proton (symbol)
deposition
p+
standard solution
trigonal planar
25. Oxidation # of Polyatomic Ions
Graham's Law
oxide
Arrhenius equation
charge
26. Color of Cs (flame test)
blue
Tetrahedral
Chemical Bonds
acetate
27. The driving force for a spontaneous is an increase in entropy of the universe
Trigonal Bipyramidal
non-
titrant buret
Entropy (S)
28. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
Metalliods
C=(mass)(specific heat)
nitrate
29. 1 sigma bond - 1 pi bond
s (fourth quantum number)
0
double bond
Pauli Exclusion Principle
30. A measure of resistance of an object to a change in its state of motion
Arrhenius Base
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Normality
Mass
31. Dirrect Method Formula
double bond
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
PV=nRT
32. 109.5° - sp^3
trigonal planar
Temperature
Tetrahedral
g solute/g solvent x 100
33. The mixing of native atomic orbitals to form special orbitals for bonding
Hybridization
oxidizing agent
p orbitals
STP
34. Within a sublevel - place one e? per orbital before pairing them
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35. All forms of energy except for heat
fusion
Anode
Theory of Relativity
work
36. In covalent bonds - prefixes are used to tell...
triple bond
eth-
Amount of atoms present
LE Model
37. C2H3O2¹?
Volume Metric Flask & Pipet
acetate
hept-
f
38. A solution that resists a change in its pH
Buffered Solution
square pyramidal
Arrhenius Base
Balmer Series
39. A solid or gas that can be formed when 2 or more aqueous reactants come together
Molecule
Galvanic Cell
insoluble
precipitate
40. Connects the 2 half cells in a voltaic cell
Bases
Ionic Compounds
salt bridge
standard solution
41. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
insoluble
0 degrees C - 1 atm
chlorate
Formal Charge
42. The amount of energy/heat required to raise some substance 1 degree C
London Dispersion Forces
Heat Capacity (C)
Molarity
see-saw
43. Happens at lines in phase change charts
Tetrahedral
% error
equilibrium
chromate
44. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
m (third quantum number)
Law of Multiple Proportions
?Hvap
Formal Charge
45. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Bronsted-Lowry Base
isothermal
Magnetic Quantum Number (ml)
standard solution
46. Energy required for liquid?gas
heat of vaporization
alkyne
electrolyte
STP
47. As protons are added to the nucleus - electrons are similarly added
triple bond
London dispersion forces
Boltzmann distribution
Aufbau Principle
48. (organics) single-bonded compound
Buffered Solution
red
alkane
equivalence point
49. When n=5 ->2 - color=
P1= X1P1°
square planar
Mass
blue-violet
50. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
melting point
Heisenberg Uncertainty Principle
M1V1=M2V2
hydrolysis
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