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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. Atoms combine in fixed whole # ratios
Law of Conservation of Energy
Law of Multiple Proportions
Integrated Rate Law
Zero-Order Rate Law
2. Involves quantum numbers
First-Order Rate Law
boiling point
Quantum Mechanical Model
wavelength
3. Atoms with the same number of protons but a different number of neutrons
electron affinity
1.86°C
Isotopes
Transition metals
4. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
Bases
96500
Matter
5. When n=6 ->2 - color=
Constant Pressure
Multiplying
Hybridization
violet
6. The measurement of heat changes
activated complex (transition state)
Beta Particles-
Calorimetry
Bronsted-Lowry Base
7. When n=4 ->2 - color=
Dipole Moment
Standard Temperature and Pressure
Cell Potential (Ecell)
blue-green
8. Does the same as equilibrium expression - except it uses initial concentrations
Reaction Quotient (Q)
charge
Law of Conservation of Mass
Diffusion
9. Ether prefix
Delta H or Enthalpy Change
Buffer
Quantum Mechanical Model
methoxy-
10. Where reduction occurs
0
Dalton's Law
Barometer
Cathode
11. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
chlorite
yellow
spontaneous
1atm=?mmHg/Torr
12. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals
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13. For significant digits - leading zeros ____ significant
catalyst
Molecular
are not
Hydrogen bonding
14. Different form of same element
nitrite
?Hvap
allotrope
Density
15. Hydroxides are soluble or insoluble?
insoluble
Density
Alkaline earth metals
Temperature
16. To find activation energy use the...
Arrhenius equation
22.4L
effects of IMF
Quantum Numbers
17. Heat needed to change 1 g of substance to 1°C
Normality
specific heat
oxalate
Pressure
18. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
Pressure
heat of fusion
l (second quantum number)
19. 96 -485 C/mol e-
6.63x10?³4Js
Faraday
Specific Heat Capacity
A Roman numeral
20. Organic w/ -NH2
freezing
Bronsted-Lowry Base
Counterions
amine
21. Molality =
moles solute/kg solvent
blue-green
red
bond energy
22. (N) number of equivalents per liter of solution
Normality
Arrhenius Base
LE Model
Oxidizing Agent
23. Liquid to solid
blue-violet
freezing
red
Bond Energy
24. 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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25. All _________ compounds are electrolytes
moles solute/kg solvent
van't Hoff Factor
Hund's Rule
Ionic
26. NO2¹?
not spontaneous
Solubility Product (Ksp)
nitrite
Solute
27. Bomb Calorimeter
equivalence point
hydroxide
electron affinity
Constant Volume
28. Solid to liquid
melting
heat of fusion
Increase Temperature
amine
29. Idea Gas Law (actual rules)
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
Chemical Bonds
activated complex (transition state)
tetrahedral
30. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
endless
Colligative properties
Hess's Law
Radioactivity
31. Change in Energy (AE) = ? (in terms of work)
Isolated System
AE = q + w
work
vaporization
32. A solution that resists a change in pH - contains both a weak acid and its conjugate base
System
Molarity
Buffer
indicator
33. The total entropy is always increasing - all systems tend towards maximum entropy
Dalton's Law of Partial Pressures
Limiting reactant
2nd law of thermodynamics
effects of IMF
34. Gas to solid
deposition
not spontaneous
flouride
System
35. Liquid to gas
equilibrium
vaporization
p+
Faraday
36. How to Find an Empirical Formula Given Percentages
octahedral
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
London Dispersion Forces
Equilibrium Expression
37. AX4E
Hess's Law
AH
see-saw
increasing
38. n+m (these are orders of reactants)
Overall Reaction Order
first
Lone Pair
l (second quantum number)
39. Nonmetal oxide + H2O ->
rate law
acid
Electronegativity
Alpha Particles-
40. Dirrect Method Formula
no precipitate forms
phosphate
Osmotic Pressure
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
41. An element with several different forms - each with different properties (i.e. graphite & diamond)
Allotrope
electron affinity
second
van't Hoff Factor
42. Unit of electrical potential; J/C
Cg=kPg
Volt
weak acid strong base rxn
are
43. R=
8.31J/Kmol
-(q of H2O + q of cal)
Molecular Orbitals (MOs)
condensation
44. If Q>Ksp
Constant Volume
Isolated System
Alkaline earth metals
a precipitate forms
45. ?T=k*m(solute)
d orbitals
Molal BP Elevation Constant
salt bridge
Calorimetry
46. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Magnetic Quantum Number (ml)
22.4L
third
tetrahedral
47. As protons are added to the nucleus - electrons are similarly added
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Theory of Relativity
Aufbau Principle
exothermic
48. AP doesn't deal with ...-order reaction - don't pick it!
Balmer Series
Q<K
Trigonal Bipyramidal
third
49. Variable for type of orbital
l (second quantum number)
96500
Its root and adding -ide
Percent Yield
50. This MUST be determined experimentally
rate law
Positive work value; work done on system
Integrated Zero-Order Rate Law
Specific Heat (s)