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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. Mass percent
g solute/g solvent x 100
Volt
electrolyte
STP
2. Change that occurs at constant temperature
1.86°C
isothermal
wavelength
effects of IMF
3. Nonmetal oxide + H2O ->
C=(mass)(specific heat)
acid
v3kT/m
trigonal bipyramidal
4. A monoatomic cation takes name from...
carbohydrates
Its element
Law of Definite Proportion
Hydrogen bonding
5. All forms of energy except for heat
first
Manometer
carbonate
work
6. How to Find an Empirical Formula Given Grams
strong bases
red
Amphoteric
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
7. Boiling point elevation formula
?Tb= kb x molality
0
Hund's Rule
Pauli Exclusion Principle
8. Molecules' tendency to stick to the container
geometric isomers
Surroundings
Pauli Exclusion Principle
adhesion
9. Expresses how the concentrations depend on time
Integrated Rate Law
1 atm
supercritical fluid
Negative work value; work done by system
10. (organics) nine carbons
P1V1/N1T1=P2V2/N2T2
non-
yellow --> green
trigonal bipyramidal
11. When n=6 ->2 - color=
n (first quantum number)
violet
oxide gas and water
M1V1=M2V2
12. Lowers activation energy
-(q of H2O + q of cal)
Integrated Zero-Order Rate Law
Counterions
catalyst
13. J/°Cg or J/Kg
red/orange
Arrhenius acid
Specific Heat Capacity
entropy
14. Organic w/ -NH2
0
Surroundings
amine
v3kT/m
15. Color of Sr (flame test)
Scientific Method
red
Magnetic Quantum Number (ml)
carbonate
16. 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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17. F¹?
red/orange
flouride
-ol
Bond enthalpy
18. H + donor
1/2mv²
Bronsted-Lowry Acid
Arrhenius acid
period
19. Where oxidation occurs
Limiting reactant
Anode
Allotrope
0.0821 atm L/mol K
20. AX5
ether
trigonal bipyramidal
Closed System
Negative work value; work done by system
21. These orbitals are perpendicular
p orbitals
acid
1.86°C
Closed System
22. Horizontals on the periodic table
methoxy-
London dispersion forces
Valence Electrons(assigned)
period
23. R in instances that pertain to energy
Counterions
M = square root (3RT/mm)
8.314 J/K mol
Net Ionic Equation
24. AX3E2
melting
Density
T-shape
E
25. Colors of Reaction when (MnO4 -) --> (Mn2+)
Pressure
spontaneous
purple --> pink
anode
26. 2 or more covalently bonded atoms
Molecule
Cathode
mol Fraction
l (second quantum number)
27. Negative enthalpy - heat flows into surroundings
Solvent
oxidation
hydrolysis
exothermic
28. Type of system in which the energy may escape - but the mass is conserved
square planar
Solubility Product (Ksp)
1st law of thermodynamics
Closed System
29. Calculation from K to C
mol
van't Hoff Factor
red
C + 273
30. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
oxalate
Bronsted-Lowry base
Equilibrium constant
yellow --> green
31. Planck's constant - used to calculate energy w/frequency
conjugate base
6.63x10?³4Js
Metalliods
Chemical Bonds
32. Connects the 2 half cells in a voltaic cell
green/yellow
weak acid strong base rxn
Law of Multiple Proportions
salt bridge
33. Phase change from gas to solid
# protons (atom is defined by this)
square planar
deposition
Arrhenius acid
34. Organic reaction in which two functional groups come together - resulting in the release of water
condensation
Alkaline earth metals
d orbitals
Cell Potential (Ecell)
35. High-speed electrons
Beta Particles-
22.4L
Pi Bond
methods of increasing rate
36. AX2 - AX2E3
are not
linear
yellow --> green
P of a =(X of a)(total pressure)
37. If anion ends in -ite - acid name ends in...
melting
-ous acid
catalyst
methods of increasing rate
38. Ending for alcohols
Naming Binary Ionic Compounds
bent
-ol
Molecular Orbitals (MOs)
39. Symbol for the heat absorbed or lost molecularly (PER MOLE)
0
van't Hoff Factor
alkene
AH
40. CN¹?
cyanide
perchlorate
Quantum Numbers
0.0821 atm L/mol K
41. Solid to liquid
k=Ae^(-Ea/RT)
reduction agent
melting
H
42. H?+NH3?NH4
Strong acid weak base rxn
v3RT/M(in kg)
boiling point
dichromate
43. Amount of product produced when limiting reactant is used up
Theoretical yield
Mass
3rd law of thermodynamics
permanganate
44. Similar to atomic orbitals - except between molecules
third
meth-
Solubility Product (Ksp)
Molecular Orbitals (MOs)
45. Change in Energy = ? (in terms of constant pressure; for gasses)
Bond Energy
Arrhenius Base
0.512°C
AE= AH - RTAn
46. Gain of electrons - decrease in oxidation #
Molarity
Q>K
reduction
1atm=?Pa
47. U(rms)=(3RT/M)^1/2
Second-Order Rate Law
Root Mean Square Velocity
moles of solute/ L of solution
# protons (atom is defined by this)
48. Donates a single H+ Ion (... other prefixes also)
chlorite
purple
Molecular Orbitals (MOs)
Monoprotic
49. Elements which have all electrons paired and relatively unaffected by magnetic fields
diamagnetic
s
perchlorate
deposition
50. Only contains ions that change in reaction
trigonal pyramidal
Net Ionic Equation
melting
Increase Temperature