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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. Absorbs/takes in heat (positive value)
Ligand
spontaneity
Endothermic
Beta Particles-
2. Variable for energy of e- - goes from 1 -2 -3 on up
n (first quantum number)
triple bond
single bond
double bond
3. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Atmospheric Pressure
Resonance
T-shape
State Functions
4. OH¹?
Molar Mass of Element/ Total Molar Mass %
msAT
Root Mean Square Velocity
hydroxide
5. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
6.63x10?³4Js
End Point
Cg=kPg
Molecular Orbitals (MOs)
6. Point at which vapor pressure=air pressure above
boiling point
Ligand
red
Pressure of H2O must be Subtracted
7. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Amphoteric
anode
rate
allotrope
8. frequency symbol
Radioactivity
Chemical Bonds
electron affinity
nu
9. Bomb Calorimeter
Constant Volume
?Tf= kf x molality
Pressure
Root Mean Square Velocity
10. SO3²?
sulfite
square pyramidal
oxidation
Ionic Compounds
11. Change in Energy = ? (in terms of constant pressure; for gasses)
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
AE= AH - RTAn
Standard Temperature and Pressure
Ligand
12. The line running between the atoms
Entropy (S)
blue-green
perchlorate
Sigma Bond
13. Calculation from K to C
chlorite
C + 273
Balmer Series
Polar Covalent
14. Pairs of electrons localized on an atom
dec-
octahedral
Lone Pair
Amount of atoms present
15. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
seesaw
equivalence point
isothermal
End Point
16. Amount of gravitational force exerted on an object
different # of neutrons
Aufbau Principle
Weight
endless
17. Ptotal=Pa+Pb+Pc....
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18. The reactant that is being oxidized - brings about reduction
paramagnetic
experimental yield
reduction agent
sulfide
19. kf of water
1.86°C
Colligative properties
p orbitals
are
20. Negative enthalpy - heat flows into surroundings
chlorite
oxide gas and water
exothermic
adiabatic
21. J/°Cg or J/Kg
Oxidation is Loss Reduction is Gain
trigonal planar
Specific Heat Capacity
Molecular Orbitals (MOs)
22. Ideal Gas Law Formula
heat of fusion
anode
PV=nRT
flouride
23. When ____ significant digits - round answer to least decimal place
ionic
Adding
Ligand
single bond
24. Substances w/ critical temperatures below 25°C
Barometer
Pressure of H2O must be Subtracted
permanent gases
0
25. I¹?
iodide
Manometer
Bond Order
red
26. q H2O = ?
Dalton's Law of Partial Pressures
0
msAT
Bases
27. 1 sigma bond
oxalate
Molecular Compounds
single bond
melting point
28. When gas expands ...
Joule
Negative work value; work done by system
0
1atm=?mmHg/Torr
29. Energy required to break a bond
Bond Energy
analyte
insoluble
p orbitals
30. Energy required for melting to occur
d orbitals
heat of fusion
square pyramidal
C=(mass)(specific heat)
31. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Polar Covalent
Molecular
vaporization
mol
32. Increase Volume
6.63x10?³4Js
Increase Temperature
conjugate base
Hund's Rule
33. Temperature-pressure combination at which solid - liquid - and gas states appear
Limiting reactant
permanganate
Acids
triple point
34. Oxidation # of Hydrogen
+1 - except if bonded to Alkali Metal -1
p orbitals
Dalton's Law
1st law of thermodynamics
35. Matter can't be created nor destroyed
Dipole Moment
Law of Conservation of Mass
l (second quantum number)
0.512°C
36. J/°Cmol or J/Kmol
Molar Heat Capacity
hydro-ic acid
diamagnetic
condensation
37. H+ Acceptor
are not
Bronsted-Lowry Base
Constant Pressure
alcohol
38. The energy required to raise 1 g of substance 1 degree C
Transition metals
Specific Heat (s)
Work
Bronsted-Lowry Base
39. Cl¹?
chloride
s orbitals
phosphate - sulfide - carbonate - sulfate
not spontaneous
40. Reverse rxn occurs when
base
Q>K
vaporization
are not
41. Atomic #
# protons (atom is defined by this)
titrant buret
Graham's Law
Bronsted-Lowry base
42. Like dissolves...
Arrhenius equation
insoluble
1st law of thermodynamics
like
43. [A] vs. time is a ...-order reaction
supercritical fluid
zero
viscosity
blue
44. AX3
Law of Multiple Proportions
trigonal planar
London dispersion forces
?Tf= kf x molality
45. Ionizes to produce OH- Ions
m (third quantum number)
Quantum Mechanical Model
Law of Conservation of Mass
Arrhenius Base
46. O²?
oxide
prop-
Its root and adding -ide
Pi Bond
47. r=k[A]
condensation
vaporization
First-Order Rate Law
permanganate
48. Occupies the space above and below a sigma bond
deposition
Heat Capacity (C)
Pi Bond
Molality
49. 180° - sp
5% rule
zero
nitrite
Linear
50. We cannot simultaneously determine an atom's exact path or location
activated complex (transition state)
second
Heisenberg Uncertainty Principle
equivalence point