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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. Heat capacity formula
acetate
C=(mass)(specific heat)
1/2mv²
Metalliods
2. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
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3. Kinetic Energy per molecule
Cation
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
Equilibrium constant
1/2mv²
4. Electron pairs found in the space between the atoms
Solvent
Polar Covalent
t-shape
Bonding Pairs
5. SO4²?
Buffered Solution
Naming Binary Ionic Compounds
surroundings
sulfate
6. Pure metal or metal hydride + H20 ->
equivalence point
base and hydrogen gas
cyanide
blue
7. 96 -485 C/mol e-
% error
Bond Energy
Faraday
Q>K
8. Organic w/ -OH group
force x distance = work done
alcohol
prop-
P1= X1P1°
9. Raoult's Law - relations between vapor pressure and concentrations
?Tb= kb x molality
P1= X1P1°
Aufbau Principle
Bronsted-Lowry acid
10. Pressure Units/Conversions
yellow --> green
1 atm = 760 mmHg = 101.3 kPa
Molecular
equilibrium
11. kb of water
Force = mass x acceleration
s
0.512°C
diamagnetic
12. Spontaneous emission of radiation
insoluble
Radioactivity
8.31J/Kmol
-1
13. Speed of light - C
Bases
3.0x108m/s
weak acid strong base rxn
oxide gas and water
14. An equilibrium expression
Solubility Product (Ksp)
Bronsted-Lowry Base
Counterions
Equilibrium constant
15. 90°&120° - dsp^3
vapor pressure
Naming Binary Ionic Compounds
Trigonal Bipyramidal
Finding Empirical Formulas
16. Color of Ba (flame test)
reduction agent
Temperature
red
green/yellow
17. The line running between the atoms
Molal BP Elevation Constant
Sigma Bond
oxide
endothermic
18. The transfer of energy between two objects due to temperature difference
Heat
0.0826Latm/Kmol
H
spontaneous
19. Half-life equation
N=N.(0.5)^time/time half-life
State Functions
Trigonal Planar
cohesion
20. Occupies the space above and below a sigma bond
Pi Bond
are
Dalton's Law
dichromate
21. Two molecules with identical connectivity but different geometries
Bases
r1/r2
geometric isomers
Atmospheric Pressure
22. AX6
Density
octahedral
Arrhenius equation
Anode
23. 1 sigma bond
Scientific Method
standard solution
Cg=kPg
single bond
24. Substances that form OH- when dissolved in water; proton acceptors
Bases
v3kT/m
q/moles
log[H+]
25. Has values from 0 to (n-1); tells shape of atomic orbitals
0
Valence Electrons(assigned)
Angular Momentum Quantum Number
Arrhenius base
26. Mass/volume
red
Increase Temperature
Chemical Bonds
Density
27. IMF that exists in polar molecules
blue-green
Speed of light
Dipole-dipole forces
First-Order Rate Law
28. Variable for spin of electron (+.5 or -.5)
s (fourth quantum number)
Thermochemistry
Bond enthalpy
red
29. Stronger IMF= lower... weaker IMF= higher...
vapor pressure
Amphoteric
r1/r2
Law of Multiple Proportions
30. Planck's constant - used to calculate energy w/frequency
boiling point
6.63x10?³4Js
State Functions
are
31. (organics) ten carbons
dec-
alkene
heat of fusion
Alkali metals
32. ClO3²?
chlorate
Arrhenius acid
specific heat
ionic
33. PV=nRT
ionic
entropy (S)
Ideal Gas Law
ammonium
34. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Law of Multiple Proportions
Pressure
Polar Covalent
Dipole-dipole forces
35. A monoatomic cation takes name from...
Its element
first
nitrate
melting point
36. The chemical formed when a base accepts a proton
charge
Metalliods
conjugate acid
oxalate
37. When gas compresses ...
charge
Positive work value; work done on system
a precipitate forms
electron affinity
38. The measurement of heat changes
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Calorimetry
permanganate
electron affinity
39. Significant Digits of counted things
endless
Adding
Molarity
Integrated Second-Order Rate Law
40. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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41. Change in moles (An) =?
Manometer
Cg=kPg
(moles of products that are gasses) - (moles of reactants that are gasses)
increasing
42. Osmotic pressure=MRT
Osmotic Pressure
Density
Dalton's Law
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
43. Force per unit area
trigonal bipyramidal
Pressure
system
Buffered Solution
44. Formula used when diluting stock solution (to find amount of water or stock needed)
square pyramidal
base and hydrogen gas
M1V1=M2V2
1atm=?Pa
45. CN¹?
bond energy
voltaic cells
cyanide
surroundings
46. Thickness
viscosity
Buffer
Quantum Model
ionic
47. Aldehyde suffix
Specific Heat (s)
Aufbau Principle
oxalate
-al
48. Proton acceptors - must have an unshared pair of e?s
Hydrogen bonding
Endothermic
Bronsted-Lowry base
Chemical Bonds
49. Energy required to break a bond
1 atm
perchlorate
pi=(nRT)/v
Bond Energy
50. Carboxylic acid ending
-oic acid
oxide gas and water
permanent gases
Acid + Base --> Salt + Water
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