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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. Average Kinetic Energy Formula
Isotopes
Hess's Law
square pyramidal
Average KE = 1/2(mass)(average speed of all particles)
2. Gas to solid
adiabatic
deposition
Arrhenius Base
Osmotic Pressure
3. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Bond Order
Theory of Relativity
system
Ionic Compounds
4. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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5. kf of water
1.86°C
methoxy-
Magnetic Quantum Number (ml)
Theoretical yield
6. Only contains ions that change in reaction
Net Ionic Equation
amine
3/2RT
Molarity
7. Energy required to break a bond
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Reaction Quotient (Q)
Bond Energy
oxalate
8. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
anode
phosphate
Cg=kPg
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
9. AX3E
8.314 J/K mol
1.38x10?²³J/K
trigonal pyramidal
Alkali metals
10. SI unit of energy; Kg*m^2/s^2
k=Ae^(-Ea/RT)
Joule
(moles of products that are gasses) - (moles of reactants that are gasses)
Coordination Compound
11. Point at which liquid?gas occurs
hydrolysis
boiling point
Reducing Agent
Covalently w/in themselves - Ionicly bonded w/ each other
12. The line running between the atoms
Bronsted-Lowry Acid
blue-green
4.184
Sigma Bond
13. C2H3O2¹?
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
a precipitate forms
Cation
acetate
14. PV=nRT
green/yellow
reduction agent
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Ideal Gas Law
15. Does the same as equilibrium expression - except it uses initial concentrations
yellow
Reaction Quotient (Q)
alkane
London dispersion forces
16. Atoms with the same number of protons but a different number of neutrons
single bond
Dipole-dipole forces
Isotopes
Bronsted-Lowry Acid
17. AX4E
Integrated Rate Law
seesaw
hydroxide
moles solute/kg solvent
18. The chemical formed when an acid donates a proton
Net Ionic Equation
conjugate base
v3kT/m
Radioactivity
19. Ptotal=P1+P2+P3+...
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20. Half cell in which oxidation occurs
single bond
octahedral
anode
?Tb= kb x molality
21. (organics) nine carbons
Temperature
3.0x108m/s
non-
purple
22. Change that occurs at constant temperature
Pi Bond
Joule
seesaw
isothermal
23. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Octahedral
rate
0
m (third quantum number)
24. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Hund's Rule
System
Buffer
Root Mean Square Velocity
25. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
Dipole-dipole forces
?Tf= kf x molality
complex ions
Principal Quantum Number
26. The actual amount of product produced in an experiment
experimental yield
sulfate
like
eth-
27. These orbitals are diagonal
Alpha Particles-
Volt
d orbitals
Tetrahedral
28. Tools NEEDED for dilution
Volume Metric Flask & Pipet
Anode
Linear
reduction agent
29. Freezing point depression formula
AE= AH - RTAn
insoluble
green/yellow
?Tf= kf x molality
30. Symbol for Enthalpy
Ionic
system
H
cathode
31. Reactant which doesn't get used up completely in a chemical reaction
carbohydrates
Cg=kPg
oxidation
excess reactant
32. [A] vs. time is a ...-order reaction
zero
Bronsted-Lowry Acid
Force = mass x acceleration
Counterions
33. 2+ charge
equilibrium
Reaction Quotient (Q)
Alpha Particles-
Solution
34. These orbitals are perpendicular
p orbitals
rate
Anion
Ligand
35. 90°&120° - dsp^3
soluble
Trigonal Bipyramidal
freezing
Thermochemistry
36. Energy involved in gaining an electron to become a negative ion
Metalliods
electron affinity
Electron Spin Quantum Number
Graham's Law
37. Spectrum of light when an electron drops to energy level n=2
Polar Covalent
Balmer Series
different # of neutrons
t-shape
38. Speed of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm A/ mm B)
Law of Conservation of Mass
amine
Constant Pressure
39. Symbol for Total Heat absorbed or released
log[H+]
insoluble
q
bromate
40. Solution used in titration
titrant buret
LeChatelier's Principle
vaporization
square pyramidal
41. If needed - indicate charge of metal(cation) by...
London dispersion forces
weak acid strong base rxn
6.63x10?³4Js
A Roman numeral
42. A homogeneous mixture with 1 phase
0.512°C
rate law
Solution
Oxidizing Agent
43. Atoms combine in fixed whole # ratios
-ous acid
Law of Multiple Proportions
Integrated Second-Order Rate Law
Oxidizing Agent
44. Unit of electrical potential; J/C
deposition
amine
Volt
conjugate acid
45. ClO3²?
Hybridization
Magnetic Quantum Number (ml)
bromate
chlorate
46. (N) number of equivalents per liter of solution
acid
Normality
hydro-ic acid
high pressure - low temperature
47. What is defined by you taken from the whole universe
wavelength
viscosity
System
3rd law of thermodynamics
48. Electron (symbol)
e-
alcohol
Standard Temperature and Pressure
-al
49. C2O4²?
Anode
oxalate
voltaic cells
Balmer Series
50. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
CAT
Specific Heat Capacity
Finding Empirical Formulas
different # of neutrons