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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. Puts H? into solution
nitrite
rate law
Arrhenius acid
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
2. Variable for energy of e- - goes from 1 -2 -3 on up
freezing
square pyramidal
Atomic Mass Unit
n (first quantum number)
3. Polyatomic Ions (bonding)
End Point
Resonance
Solution
Covalently w/in themselves - Ionicly bonded w/ each other
4. High-energy light
Constant Pressure
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
square pyramidal
Gamma Ray-
5. Liquid to gas
Scientific Method
vaporization
violet
P1= X1P1°
6. Ptotal=Pa+Pb+Pc....
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7. A single substance that may be an acid or a base (i.e. water)
Amphoteric
Thermochemistry
1atm=?Pa
Weight
8. Ability of an atom in a molecule to attract shared electrons to itself
non-
Electronegativity
mol
London dispersion forces
9. Aldehyde suffix
-al
base
0 degrees C - 1 atm
Polar Covalent
10. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Bases
Buffer
g solute/g solvent x 100
single bond
11. 101 -325 Pa
Angular Momentum Quantum Number
Naming Binary Ionic Compounds
1atm=?Pa
endless
12. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Tetrahedral
activation energy
ether
Boltzmann distribution
13. As protons are added to the nucleus - electrons are similarly added
Chemical Kinetics
Aufbau Principle
Exothermic
red
14. HF+ OH??H2O
weak acid strong base rxn
M1V1=M2V2
State Functions
Kinetic Molecular Theory - for ideal gases
15. AX5E
dec-
square pyramidal
Radioactivity
Integrated Zero-Order Rate Law
16. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Arrhenius Acid
Molecular
Law of Conservation of Mass
entropy
17. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
spontaneous
End Point
condensation
Counterions
18. Anions or cations as needed to produce a compound with non net charge
Counterions
chloride
Entropy (S)
vapor pressure
19. Releases/gives off heat (negative value)
Chemical Kinetics
Antibonding Molecular Orbital
Exothermic
s (fourth quantum number)
20. Proton acceptors - must have an unshared pair of e?s
Bronsted-Lowry base
End Point
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
acid
21. Peak of energy diagram
activated complex (transition state)
Amphoteric
Scientific Method
T-shape
22. (organics) six carbons
hex-
experimental yield
Arrhenius equation
Hund's Rule
23. C2H3O2¹?
cathode
acetate
Chemical Kinetics
iodide
24. I¹?
Kinetic Molecular Theory - for ideal gases
iodide
freezing
ionic
25. Thickness
viscosity
supercritical fluid
Oxidation is Loss Reduction is Gain
octahedral
26. Group 1 metals
PV=nRT
k=Ae^(-Ea/RT)
precipitate
Alkali metals
27. Work = ?
-(P)(Change in V)
q
Temperature
k=Ae^(-Ea/RT)
28. Change that occurs at constant temperature
isothermal
Effusion
Quantum Numbers
Isolated System
29. Substance being dissolved in a solution (lower [ ])
Solute
Scientific Method
1 atm = 760 mmHg = 101.3 kPa
Law of Multiple Proportions
30. 96 -485 C/mol e-
Molality
flouride
red
Faraday
31. Has values from 0 to (n-1); tells shape of atomic orbitals
LeChatelier's Principle
Angular Momentum Quantum Number
van't Hoff Factor
mol Fraction
32. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
bromate
Finding Empirical Formulas
Enthalpy of Solution
33. Carbon & hydrogen compounds
End Point
base and hydrogen gas
hydrocarbons
catalyst
34. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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35. Absorbs/takes in heat (positive value)
Endothermic
octahedral
heat capacity
Delta H or Enthalpy Change
36. Different form of same element
k=Ae^(-Ea/RT)
allotrope
m (third quantum number)
red/orange
37. (organics) ten carbons
dec-
blue-green
3rd law of thermodynamics
% error
38. =vM2/M1
r1/r2
Molal FP Depression Constant
Coordination Compound
yellow
39. AX2E - AX2E2
bent
Entropy (S)
a precipitate forms
base
40. Amount of gravitational force exerted on an object
6.63x10?³4Js
Weight
charge
Transition metals
41. Electron pairs found in the space between the atoms
nu
Bonding Pairs
Work
Formal Charge
42. CrO4²?
chromate
hydrocarbons
Alkali metals
dichromate
43. Oxidation # of Halogens
ammonium
surroundings
red
-1
44. Color of K (flame test)
t-shape
methods of increasing rate
purple
Thermochemistry
45. A solution that resists a change in its pH
Dalton's Law
Law of Conservation of Mass
Magnetic Quantum Number (ml)
Buffered Solution
46. Mol/L - concentration of a solution
P1V1/N1T1=P2V2/N2T2
mol Fraction
Solution
Molarity
47. Oxidation # of Compounds
Anode
0
Cation
square planar
48. If anion ends in -ide - acid name ends in
purple --> pink
hydro-ic acid
Its element
Heat
49. If needed - indicate charge of metal(cation) by...
end point
standard solution
period
A Roman numeral
50. 760 mmHg - 760 torr
1 atm
square pyramidal
salt bridge
P1V1/N1T1=P2V2/N2T2