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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. r=k[A]^2
Chemical Bonds
Second-Order Rate Law
wavelength
nitrite
2. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
C=(mass)(specific heat)
paramagnetic
-ol
3. q cal = ?
Octahedral
Transition metals
CAT
Molecular
4. PO4³?
Integrated Rate Law
log[H+]
Joule
phosphate
5. C=2.9979*10^8 m/s
Osmotic Pressure
M = square root (3RT/mm)
Lone Pair
Speed of light
6. Average speed of gas
Linear
sulfate
Integrated First-Order Rate Law
v3RT/M(in kg)
7. Describe various properties of one orbital
X of a = moles a/total moles
Quantum Numbers
Alkaline earth metals
prop-
8. Anions or cations as needed to produce a compound with non net charge
Counterions
triple bond
Principal Quantum Number
Bases
9. The reactant that is being reduced - brings about oxidation
Law of Multiple Proportions
Integrated Second-Order Rate Law
Acid + Base --> Salt + Water
oxidizing agent
10. Spectrum of light when an electron drops to energy level n=2
Molality
Molecule
supercritical fluid
Balmer Series
11. q H2O = ?
iodide
Enthalpy of Solution
octahedral
msAT
12. J/°Cg or J/Kg
First-Order Half Life
standard solution
Volume Metric Flask & Pipet
Specific Heat Capacity
13. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
freezing
Linear
% error
Equilibrium Expression
14. Oxidation # of Ions
Cell Potential (Ecell)
22.4L
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
charge
15. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
soluble
oxidizing agent
Beta Particles-
electrolyte
16. Lowers activation energy
msAT
Balmer Series
catalyst
Anode
17. Newton's Second Law
Delta H or Enthalpy Change
Acids
Force = mass x acceleration
1 atm = 760 mmHg = 101.3 kPa
18. Elements which have all electrons paired and relatively unaffected by magnetic fields
LeChatelier's Principle
diamagnetic
3/2RT
Molal BP Elevation Constant
19. [A]0/2k
oxide
Zero-Order Half Life
violet
London Dispersion Forces
20. Substances w/ critical temperatures below 25°C
permanent gases
Ag+ - Pb2+ - Hg2+
adiabatic
sublimation
21. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Atmospheric Pressure
Radioactivity
chlorate
Solution
22. Group 1 and heavier Group 2 bases
-oate
strong acids
Surroundings
strong bases
23. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
allotrope
Ionic
alkene
24. Heat capacity formula
C=(mass)(specific heat)
Normality
viscosity
Specific Heat Capacity
25. Molality =
actual yield/theoretical yield x 100%
are
P1V1/N1T1=P2V2/N2T2
moles solute/kg solvent
26. Carbon - hydrogen - oxygen compounds
square pyramidal
Bronsted-Lowry Acid
carbohydrates
hydrolysis
27. frequency symbol
M = square root (3RT/mm)
nu
1atm=?Pa
1 atm = 760 mmHg = 101.3 kPa
28. Type of system in which the energy may escape - but the mass is conserved
Theoretical yield
Closed System
-oate
LeChatelier's Principle
29. Specific heat of water
4.184
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Integrated Zero-Order Rate Law
oxide
30. Energy required for liquid?gas
non-
Standard Temperature and Pressure
heat of vaporization
Hess's Law
31. AX5E
oxidation
cyanide
Normality
square pyramidal
32. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Oxidation is Loss Reduction is Gain
Cg=kPg
p
sulfite
33. Phase change from solid to gas
double bond
third
red
sublimation
34. Matter can't be created nor destroyed
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Pi Bond
Monoprotic
Law of Conservation of Mass
35. K
Cg=kPg
Equilibrium constant
chromate
conjugate acid
36. Change without heat transfer between the system and its surroundings
Arrhenius Base
Electron Spin Quantum Number
Acid Dissociation Constant
adiabatic
37. In a given atom no two electrons can have the same set of four quantum numbers
Specific Heat (s)
analyte
Pauli Exclusion Principle
Buffered Solution
38. SO3²?
Hess's Law
Arrhenius Base
sulfite
1/2mv²
39. We cannot simultaneously determine an atom's exact path or location
Surroundings
Molar Mass of Element/ Total Molar Mass %
Dipole Moment
Heisenberg Uncertainty Principle
40. I=moles of particles/moles of solute dissolved
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41. ln[A] vs. time is a ...-order reaction
Pi Bond
first
complex ions
Dipole-dipole forces
42. Where there are no electrons
Q>K
Nodes
phosphate - sulfide - carbonate - sulfate
AE = q + w
43. Larger molecules which have higher mass and therefore electron density have stronger...
London dispersion forces
Quantum Numbers
?Hvap
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
44. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
square pyramidal
strong acids
Temperature
chromate
45. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Ionic
Calorimeter
Molecular
-ol
46. When gas compresses ...
red
Molal FP Depression Constant
isothermal
Positive work value; work done on system
47. Puts OH? into solution
Hydrogen bonding
Arrhenius base
blue-green
meth-
48. 2 or more covalently bonded atoms
allotrope
Molecule
Bonding Pairs
yellow
49. ClO4¹?
Its root and adding -ide
perchlorate
phosphate
Molecule
50. AX3E2
First-Order Rate Law
cohesion
T-shape
Radioactivity