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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. Theoretical yield-experimental yield/theoretical yieldx100
Atmospheric Pressure
% error
Heat Capacity (C)
sulfide
2. 90° - d^2sp^3
charge
-al
Molality
Octahedral
3. 109.5° - sp^3
triple bond
Tetrahedral
0
seesaw
4. (organics) ten carbons
dec-
Hydrogen bonding
1.38x10?²³J/K
Volume Metric Flask & Pipet
5. Absorbs/takes in heat (positive value)
Ionic Compounds
Isotopes
trigonal pyramidal
Endothermic
6. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
P of a =(X of a)(total pressure)
Finding Empirical Formulas
Kinetic Molecular Theory - for ideal gases
Increase Temperature
7. The line running between the atoms
Sigma Bond
Balmer Series
permanganate
dichromate
8. To find activation energy use the...
eth-
Arrhenius equation
condensation
group
9. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Magnetic Quantum Number (ml)
Bronsted-Lowry Acid
chloride
purple --> pink
10. What is defined by you taken from the whole universe
permanganate
System
p
endothermic
11. Substance being dissolved in a solution (lower [ ])
Positive work value; work done on system
Solute
Ionic
solid CO2
12. Half-life equation
N=N.(0.5)^time/time half-life
sublimation
Antibonding Molecular Orbital
+1 - except if bonded to Alkali Metal -1
13. The chemical formed when an acid donates a proton
a precipitate forms
conjugate base
red
blue-violet
14. For significant digits - trailing zeros _____ significant
t-shape
are
0
alkane
15. AX2 - AX2E3
Nernst Equation
blue-violet
viscosity
linear
16. Gain of electrons - decrease in oxidation #
Metalliods
Volume Metric Flask & Pipet
reduction
high pressure - low temperature
17. When n=5 ->2 - color=
Arrhenius equation
Monoprotic
blue-violet
third
18. Peak of energy diagram
First-Order Half Life
activated complex (transition state)
Percent Yield
Effusion
19. ClO2¹?
E
Kinetic Molecular Theory - for ideal gases
Anode
chlorite
20. The minimum energy that molecules must possess for collisions to be effective - Ea
T-shape
Galvanic Cell
% error
activation energy
21. I=moles of particles/moles of solute dissolved
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22. Substances that form OH- when dissolved in water; proton acceptors
Bases
Reaction Quotient (Q)
nu
-oic acid
23. Speed per molecule of gas
insoluble
Normality
v3kT/m
conjugate base
24. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
high pressure - low temperature
acid
single bond
25. Average speed of gas
v3RT/M(in kg)
Barometer
trigonal pyramidal
Bonding Pairs
26. Mass/volume
0.512°C
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Volume Metric Flask & Pipet
Density
27. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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28. H+ Acceptor
dec-
Bronsted-Lowry Base
-ic acid
Law of Multiple Proportions
29. When n=6 ->2 - color=
boiling point
violet
nitrite
Counterions
30. AX4
Root Mean Square Velocity
Integrated Second-Order Rate Law
tetrahedral
v3RT/M(in kg)
31. Polyatomic Ions (bonding)
-ic acid
Molal BP Elevation Constant
period
Covalently w/in themselves - Ionicly bonded w/ each other
32. AP doesn't deal with ...-order reaction - don't pick it!
Calorimeter
experimental yield
Amphoteric
third
33. Color of Cs (flame test)
phosphate
s
deposition
blue
34. For significant digits - leading zeros ____ significant
0
are not
Second-Order Rate Law
Bases
35. Bomb Calorimeter
Pauli Exclusion Principle
bent
Constant Volume
acetate
36. Work = ?
Magnetic Quantum Number (ml)
insoluble
-1
-(P)(Change in V)
37. Only contains ions that change in reaction
Net Ionic Equation
0.0826Latm/Kmol
rate
non-
38. r=k[A]^2
Coordination Compound
Second-Order Rate Law
Trigonal Bipyramidal
heat capacity
39. Color of Li (flame test)
Zero-Order Half Life
Amount of atoms present
Solvent
red
40. Weakest IMFs - found in all molecules
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
London dispersion forces
Overall Reaction Order
-one
41. [A]0/2k
Quantum Mechanical Model
Zero-Order Half Life
nu
single bond
42. AX6
1atm=?Pa
Dipole-dipole forces
octahedral
endless
43. Like dissolves...
like
Molar Heat Capacity
alkyne
high pressure - low temperature
44. Ka=[products]^m/[reactants]^n
Law of Multiple Proportions
Integrated Rate Law
Naming Binary Ionic Compounds
Acid Dissociation Constant
45. Liquid to gas
Multiplying
Ampere
3/2RT
vaporization
46. [A]=-kt + [A]0
Arrhenius acid
Osmotic Pressure
Weight
Integrated Zero-Order Rate Law
47. Heat capacity formula
endless
s orbitals
Constant Volume
C=(mass)(specific heat)
48. Oxidation # of free elements
alkyne
chlorite
0
Arrhenius Acid
49. Carboxylic acid ending
moles of solute/ L of solution
square planar
wavelength
-oic acid
50. Ideal Gas Law Formula
PV=nRT
Temperature
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
red
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