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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. Color of Cs (flame test)
blue
Beta Particles-
condensation
Quantum Mechanical Model
2. Symbol for Enthalpy
sulfate
hept-
H
m (third quantum number)
3. Proton donors
Amount of atoms present
nitrate
excess reactant
Bronsted-Lowry acid
4. Elements on staircase on periodic table
Percent Yield
Metalliods
+1 - except if bonded to Alkali Metal -1
rate gas A/rate gas B = square root (mm A/ mm B)
5. Occupies the space above and below a sigma bond
Pi Bond
AH
Equivalence Point
Dalton's Law
6. Puts H? into solution
r1/r2
Arrhenius acid
acetate
solid CO2
7. Half cell in which oxidation occurs
anode
nitrate
Hund's Rule
Quantum Model
8. (msubs) Can only be +1/2 or -1/2
reduction
M = square root (3RT/mm)
boiling point
Electron Spin Quantum Number
9. The reactant that is being reduced - brings about oxidation
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
oxidizing agent
Volume Metric Flask & Pipet
see-saw
10. Energy required for melting to occur
Osmotic Pressure
heat of fusion
n0
chromate
11. AX5E
Work
see-saw
square pyramidal
Molality
12. E=mc^2
Theory of Relativity
activation energy
Bond Order
Naming Binary Ionic Compounds
13. This MUST be determined experimentally
complex ions
force x distance = work done
Alpha Particles-
rate law
14. Pairs of electrons localized on an atom
blue-green
pent-
Polar Covalent
Lone Pair
15. Measure of the average kinetic energy of all the particles in a substance
Q<K
Temperature
but-
Amphoteric
16. 6.022x10^23
freezing
mol
geometric isomers
Heisenberg Uncertainty Principle
17. Point at which vapor pressure=air pressure above
-ous acid
end point
boiling point
permanganate
18. (organics) two carbons
eth-
0.512°C
sulfide
0
19. These orbitals are diagonal
Molar Mass of Element/ Total Molar Mass %
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
d orbitals
entropy (S)
20. Half cell in which reduction occurs
square pyramidal
Bond Energy
cathode
cohesion
21. Pure metal or metal hydride + H20 ->
base and hydrogen gas
phosphate
group
second
22. Anions or cations as needed to produce a compound with non net charge
Amphoteric
complex ions
Heat
Counterions
23. These orbitals are spherical
Isotopes
insoluble
boiling point
s orbitals
24. ?T=k*m(solute)
Counterions
methods of increasing rate
acetate
Molal BP Elevation Constant
25. Oxidation # of Compounds
0
-ol
Speed of light
Chemical Bonds
26. ?T=k*m(solute)
trigonal bipyramidal
Molal FP Depression Constant
Law of Multiple Proportions
Reaction Quotient (Q)
27. BrO3¹?
T-shape
methoxy-
bromate
charge
28. When ____ significant digits - round answer to least decimal place
Adding
trigonal bipyramidal
Molecule
Gamma Ray-
29. Change in moles (An) =?
(moles of products that are gasses) - (moles of reactants that are gasses)
see-saw
permanent gases
bond energy
30. A homogeneous mixture with 1 phase
Solution
Equivalence Point
Hydrogen bonding
Isotopes
31. AH of formation for a substance in its stablest form (how it is found in nature)
diamagnetic
0
-ous acid
experimental yield
32. I¹?
M1V1=M2V2
Closed System
diamagnetic
iodide
33. The heat changed in a chemical reaction.
Dalton's Law
nitrate
Thermochemistry
London dispersion forces
34. Type of system in which the energy and mass may leave or enter
Joule
Open System
End Point
electron affinity
35. Similar to atomic orbitals - except between molecules
Molecular Orbitals (MOs)
melting
London Dispersion Forces
Quantum Mechanical Model
36. Metal oxide + H20 ->
p+
Reaction Quotient (Q)
base
ammonium
37. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
Finding Empirical Formulas
deposition
van't Hoff Factor
analyte
38. 180° - sp
0.512°C
Linear
purple --> pink
Its element
39. ... compounds are most conductive
ionic
hydroxide
Naming Binary Ionic Compounds
hydrocarbons
40. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
Molecular Compounds
Its element
voltaic cells
Aufbau Principle
41. AX3E2
Electron Spin Quantum Number
H
chlorate
t-shape
42. Composition Formula
Reaction Quotient (Q)
phosphate - sulfide - carbonate - sulfate
Molar Mass of Element/ Total Molar Mass %
deposition
43. Solution used in titration
hydrocarbons
titrant buret
E
Standard Temperature and Pressure
44. Force that holds atoms together
Chemical Bonds
Volt
methoxy-
AE= AH - RTAn
45. How to Find an Empirical Formula Given Percentages
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
force x distance = work done
# protons (atom is defined by this)
Polar Covalent
46. The mixing of native atomic orbitals to form special orbitals for bonding
Bases
N=N.(0.5)^time/time half-life
Octahedral
Hybridization
47. Planck's constant - used to calculate energy w/frequency
Integrated Second-Order Rate Law
red/orange
6.63x10?³4Js
Cg=kPg
48. Speed per molecule of gas
pent-
seesaw
0
v3kT/m
49. Change that occurs at constant temperature
condensation
triple bond
isothermal
amine
50. 1/[A]=kt + 1/[A]0
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
permanent gases
Integrated Second-Order Rate Law
k=Ae^(-Ea/RT)
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