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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. Change that occurs at constant temperature
5% rule
isothermal
Molar Heat Capacity
bond energy
2. Ester suffix
phosphate
geometric isomers
diamagnetic
-oate
3. ... compounds are most conductive
ionic
trigonal pyramidal
Boltzmann distribution
yellow --> green
4. Oxoacid solution (such as HSO4-) forms...
prop-
oxide gas and water
eth-
weak acid strong base rxn
5. How to Balance a Redox Equation
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
acid
Oxidation is Loss Reduction is Gain
C + 273
6. S²?
sulfide
mol Fraction
first
Covalently w/in themselves - Ionicly bonded w/ each other
7. kf of water
1.86°C
Standard Temperature and Pressure
fusion
-(q of H2O + q of cal)
8. These orbitals are spherical
sulfite
s orbitals
Amount of atoms present
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
9. Type of system in which the energy may escape - but the mass is conserved
Weight
3.0x108m/s
Barometer
Closed System
10. Increase Volume
equivalence point
Increase Temperature
0
phosphate - sulfide - carbonate - sulfate
11. l=0
bent
Its element
s
dichromate
12. Significant Digits of counted things
1 atm
e-
endless
Quantum Model
13. (organics) single-bonded compound
Q<K
Linear
alkane
System
14. Temperature-pressure point after which gas can no longer form liquid
Arrhenius acid
critical point
Oxidation is Loss Reduction is Gain
meth-
15. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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16. Variable for spin of electron (+.5 or -.5)
Ideal Gas Law
Delta H or Enthalpy Change
Scientific Method
s (fourth quantum number)
17. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
v3kT/m
hydro-ic acid
Atmospheric Pressure
strong acids
18. Carboxylic acid ending
paramagnetic
Solute
Root Mean Square Velocity
-oic acid
19. All forms of energy except for heat
yellow --> green
purple
work
n0
20. I=moles of particles/moles of solute dissolved
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21. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
1.38x10?²³J/K
Antibonding Molecular Orbital
Atmospheric Pressure
heat capacity
22. AX3E2
t-shape
Hydrogen bonding
Decrease Volume and Increase Temperature
hydrolysis
23. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Thermochemistry
alkane
?Hvap
Polar Covalent
24. Negative enthalpy - heat flows into surroundings
exothermic
Open System
endothermic
precipitate
25. Energy required for melting to occur
Limiting reactant
London Dispersion Forces
0
heat of fusion
26. The likelihood that a rxn will occur "by itself"
electron affinity
square pyramidal
spontaneity
E
27. AX4E
Root Mean Square Velocity
Metalliods
see-saw
Scientific Method
28. Like dissolves...
like
Arrhenius Acid
Bronsted-Lowry acid
actual yield/theoretical yield x 100%
29. Absorbs/takes in heat (positive value)
Law of Multiple Proportions
Arrhenius base
square pyramidal
Endothermic
30. Organic w/ -O-
boiling point
paramagnetic
ether
Reducing Agent
31. Group 1 metals
Alkali metals
X of a = moles a/total moles
Normality
AE= AH - RTAn
32. (organics) triple-bonded compound
Hund's Rule
6.63x10?³4Js
alkyne
Electron Spin Quantum Number
33. Reverse rxn occurs when
Equivalence Point
Metalliods
Q>K
LeChatelier's Principle
34. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
vapor pressure
Molecular
blue-violet
Ampere
35. Verticals on the periodic table
group
Molality
3.0x108m/s
system
36. Heat capacity formula
Arrhenius base
salt bridge
trigonal bipyramidal
C=(mass)(specific heat)
37. Amount of gravitational force exerted on an object
Weight
standard solution
2nd law of thermodynamics
-(q of H2O + q of cal)
38. Ptotal=Pa+Pb+Pc....
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39. Half cell in which oxidation occurs
Delta H or Enthalpy Change
anode
(moles of products that are gasses) - (moles of reactants that are gasses)
strong bases
40. Electron (symbol)
?Tb= kb x molality
Endothermic
conjugate base
e-
41. Measure of the average kinetic energy of all the particles in a substance
endless
strong acids
titrant buret
Temperature
42. In covalent bonds - prefixes are used to tell...
Amount of atoms present
Faraday
A Roman numeral
Trigonal Planar
43. Universal IMF for nonpolar molecules
Matter
?Hvap
Arrhenius Base
London dispersion forces
44. q H2O = ?
effects of IMF
Tetrahedral
Quantum Mechanical Model
msAT
45. Electron pairs found in the space between the atoms
surroundings
% error
deposition
Bonding Pairs
46. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
vapor pressure
Polar Covalent
Heat
47. Cl¹?
Monoprotic
Equilibrium constant
Balmer Series
chloride
48. STP
Ag+ - Pb2+ - Hg2+
0 degrees C - 1 atm
AH
analyte
49. (msubs) Can only be +1/2 or -1/2
spontaneous
Electron Spin Quantum Number
Formal Charge
perchlorate
50. Mass #
1.86°C
square planar
# protons + # neutrons
Integrated Zero-Order Rate Law