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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. The driving force for a spontaneous is an increase in entropy of the universe
Entropy (S)
end point
Density
Dalton's Law of Partial Pressures
2. Raising heat - adding catalyst - heighten concentration - bigger surface area
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
e-
Reducing Agent
methods of increasing rate
3. C2H3O2¹?
-1
Decrease Volume and Increase Temperature
not spontaneous
acetate
4. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
heat of vaporization
hydrolysis
Ionic
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
5. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
Root Mean Square Velocity
State Functions
insoluble
Bronsted-Lowry Acid
6. Involves quantum numbers
different # of neutrons
End Point
Hund's Rule
Quantum Mechanical Model
7. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Speed of light
Polar Covalent
Integrated Second-Order Rate Law
Molal FP Depression Constant
8. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
Sigma Bond
supercritical fluid
Calorimeter
endothermic
9. Universal IMF for nonpolar molecules
P1V1/N1T1=P2V2/N2T2
Positive work value; work done on system
London dispersion forces
not spontaneous
10. Ester suffix
Calorimeter
-oate
Open System
Finding Empirical Formulas
11. (organics) eight carbons
Acid Dissociation Constant
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
oct-
-one
12. ClO4¹?
bent
vapor pressure
perchlorate
# protons + # neutrons
13. Forward rxn occurs when
3/2RT
Hydrogen bonding
Q<K
heat capacity
14. The line running between the atoms
allotrope
Transition metals
blue
Sigma Bond
15. Symbol for Total Heat absorbed or released
permanganate
Molar Mass of Element/ Total Molar Mass %
Specific Heat (s)
q
16. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
0
0.0821 atm L/mol K
3rd law of thermodynamics
17. CO3²?
second
carbonate
-(q of H2O + q of cal)
Molecule
18. Group 2 metals
Diffusion
Alkaline earth metals
electron affinity
Osmotic Pressure
19. AX6
trigonal planar
Monoprotic
octahedral
Cg=kPg
20. Cr2O7²?
double bond
yellow
phosphate
dichromate
21. Increase Volume
Increase Temperature
trigonal bipyramidal
octahedral
Osmotic Pressure
22. Formula used when diluting stock solution (to find amount of water or stock needed)
Molal FP Depression Constant
analyte
M1V1=M2V2
effects of IMF
23. Ending for alcohols
deposition
Delta H or Enthalpy Change
-ol
acid
24. Osmotic pressure formula
iodide
pi=(nRT)/v
Law of Multiple Proportions
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
25. x can be ignored when % ionization is <5%
Solubility Product (Ksp)
Solvent
Open System
5% rule
26. A measure of resistance of an object to a change in its state of motion
Mass
Pressure
Molecular Compounds
flouride
27. F¹?
oct-
flouride
conjugate acid
chloride
28. If Q>Ksp
-(q of H2O + q of cal)
methoxy-
a precipitate forms
dec-
29. (A) - C/s
T-shape
d
Ampere
P of a =(X of a)(total pressure)
30. Oxidation # of Ions
charge
Theory of Relativity
STP
boiling point
31. When n=5 ->2 - color=
endless
Kinetic Molecular Theory - for ideal gases
blue-violet
Diffusion
32. Where oxidation occurs
system
tetrahedral
Anode
work
33. When gas compresses ...
rate law
sublimation
Positive work value; work done on system
M = square root (3RT/mm)
34. Half-life equation
0.512°C
Ionic
N=N.(0.5)^time/time half-life
solid CO2
35. Verticals on the periodic table
3.0x108m/s
Entropy (S)
group
e-
36. 0.00°C - 1 atm
d orbitals
Dipole Moment
Integrated First-Order Rate Law
Standard Temperature and Pressure
37. AX4E2
square planar
Nodes
rate
Aufbau Principle
38. Substances that form H+ when dissolved in water; proton donors
Acids
Positive work value; work done on system
perchlorate
voltaic cells
39. Specific heat of water
4.184
catalyst
Density
N=N.(0.5)^time/time half-life
40. ClO3²?
Hybridization
Trigonal Planar
chlorate
Zero-Order Rate Law
41. ?T=k*m(solute)
reduction
-ous acid
heat capacity
Molal BP Elevation Constant
42. Occupies the space above and below a sigma bond
Polar Covalent
Boltzmann distribution
Pi Bond
Its element
43. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
iodide
Diffusion
Graham's Law
Chemical Kinetics
44. (organics) nine carbons
nitrate
3.0x108m/s
non-
freezing
45. [A] vs. time is a ...-order reaction
Reducing Agent
Q>K
zero
flouride
46. Proton donors
pi=(nRT)/v
Bronsted-Lowry acid
Balmer Series
exothermic
47. Pressure Units/Conversions
-(P)(Change in V)
1 atm = 760 mmHg = 101.3 kPa
Constant Volume
alkyne
48. Spontaneous emission of radiation
flouride
adhesion
d
Radioactivity
49. Oxidation # of Halogens
d orbitals
-1
triple bond
Polar Covalent
50. Hydroxides are soluble or insoluble?
solid CO2
1 atm
insoluble
Quantum Model
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