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AP Chemistry 2

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. What is HCOOCH3?
Acids; HCOOCH3 is an ester
proton acceptor.
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
bases

2. How are primary alcohols turned into acids?
Soluble
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Iodine and CO2 (dry ice)

3. What is the general formula for an acid?
Separating funnel
RCOOH
no - they're written undissociated (HAaq)
MnO4?

4. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
NH4?
Ksp = s²
ion pairing

5. What process do you use to obtain the precipitate from a solution?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
|experimental - accepted|/accepted X 100
Filtration
Graduated cylinder

6. How are non-metal oxides and hydrides bonded? are they acidic or basic?
basic
Ksp = 4s³
non-metal oxides and hydrides are covalently bonded and are acidic.
Orange

7. How are more active metals reduced?
Clear
C4H10
by electrolysis
Glowing splint (positive result=relights)

8. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
water and substances with (s) less dense than
Mono; di; tri; tetra; penta; hexa.
How grouped results are

9. chlorite
Perform ICE BOX calculation based on K1
ClO2?
linear
Pour liquids using a funnel or down a glass rod

10. What do ions and electrons travel through in a voltaic/electrolytic cell?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
allow for the vapor pressure of water and make sure to level levels
Saturated - Substitution (which requires more radical conditions)
Ions go through the salt bridge - electrons go through metal wires in the external circuit

11. If a weak acid is diluted more - what happens to its % dissociation value?
Nothing
Sigma bonds are stronger than pi bonds
Increases.
look for changes in oxidation # - the one that goes up is oxidized and is the RA

12. What is the formula for percent error?
Most are soluble except Ag - Pb
|experimental - accepted|/accepted X 100
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

13. Color is due to ______ _______ of light.
RCHO (carbonyl at end)
Read the bottom of the meniscus
Selective absorption
water and substances with (s) less dense than

14. Is the standard entropy (S°) of an element zero?
Eudiometer
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
But S° of element is not zero (except at 0K)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

15. What is the formula for alkanes?
Making sigma bonds and holding lone pairs
CnH2n+2
ion pairing
CO3²?

16. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
K2
Pour liquids using a funnel or down a glass rod
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Ksp = 108s5

17. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
An active metal.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Soluble except Ag - Pb - Ca - Sr Ba)

18. The definition of acidic basic and neutral aqueous solutions is:
Conjugate pair (one must be a weak base or acid)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
It ceases - the circuit is broken.
Synthetic condensation polymer (aka a polyamide)

19. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
boiling without losing volatile solvents/reactants
CO2 and H2O

20. Do you use J or kJ for ?H - ?S - and ?G?
Read the bottom of the meniscus
a-IMFs - b-molecular volume
?H-kJ - ?S-J - ?G-kJ
an oxidized and reduced substance

21. What apparatus do you use to pour liquids?
redox reaction
Mn²? - Cr³? - Cr³
Pour liquids using a funnel or down a glass rod
Combine the equations for the half reactions in the non-spontaneous direction

22. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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23. What is reflux?
boiling without losing volatile solvents/reactants
Making sigma bonds and holding lone pairs
MnO4?
Unsaturated - addition (ex: decolorize bromine solution)

24. Acids + Carbonates (bicarbonates) make?
#ligands=charge x2
Both electrons come from the same atom (just as good as a regular bond)
Conjugate pair (one must be a weak base or acid)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

25. What is the charge on a chlorine atom?
different forms of the same element
zero
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Glacial acetic acid

26. At what point during titration do you have the perfect buffer - and what is the pH at this point?
bright yellow
How grouped results are
Add acid to water so that the acid doesn't boil and spit
At half equivalence - pH=pKa

27. hydroxides
Hg²?
Transition element compounds (except if it has a full or empty d shell)
Supercooling can occur when cooling a solvent or solution. It occurs when there's a dip and then a rise back up to the melting point on a cooling curve.
Insoluble (except group 1 ammonium and Ba)

28. chromate ion (soln + most solids)
Salt + water
ethers
O2 needs 4F/mol H2 needs 2F/mol
yellow

29. What is the formula for summation?

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30. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Soluble
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
a-IMFs - b-molecular volume

31. Acid plus base make?
Salt + water.
?H-kJ - ?S-J - ?G-kJ
Perform ICE BOX calculation based on K1
Glowing splint (positive result=relights)

32. What do you use to look at burning magnesium? why?
blue glass - it filters UV
catalyst=conc H2SO4
Decant
K1 x K2

33. What type of compounds do Group 14 form?
Anode - oxygen. Cathode - hydrogen
+4-covalent - +2-ionic
Nothing
a-IMFs - b-molecular volume

34. mercury (II) ion
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
catalyst=conc H2SO4
Glacial acetic acid
Hg²?

35. ammonium/ammonium compounds
blue (BTB)
Soluble
A salt solution.
CH3COO?

36. What steps do organic labs consist of?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Synthesis - separation and purification of the product and its identification.
linear
left - ppt will form

37. Alkenes are ________ and react by __________
bent
Unsaturated - addition (ex: decolorize bromine solution)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

38. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
OH- and NH3
At half equivalence - pH=pKa
Salt + water.
The compound with the lowest Ksp value.

39. What measuring device would you use for very small volumes of liquids?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Pipette (burette if need repetition)
Identity and purity (impure compounds usually have broad & low melting points)
Acids; HCOOCH3 is an ester

40. chlorate
proton donor base
ClO3?
zero
Mono; di; tri; tetra; penta; hexa.

41. Why are noble gases stable?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
voltaic: + electrolytic: -
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Ionic compounds

42. What are the prefixes for the naming of binary molecular compound formulas (up to six)
?G= -ve - E°= +ve
Mono; di; tri; tetra; penta; hexa.
Greenish-yellow gas
A salt solution.

43. What causes the dramatic effect of T on rate?
The Faraday or Faraday's constant.
Nothing
T increases exponentially the proportion of molecules with E > Ea
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)

44. A geometric (or cis-trans) isomer exists due to.....
Graduated cylinder
Nothing
CO (poisonous)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

45. What is the general formula for an ether?
H+
ROR
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Experimental mass/theoretical mass X 100

46. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pale purple - (orange)-yellow - red - blue - green.
methyl formate
Equivalence point is the titrant volume when the moles of acid and base are stoichiometrically equal; end point is the titrant volume when the color of the indicator permanently changes. If you choose the correct indicator - they should occur at the
Ppt will NOT form (unsaturated)

47. What are isomers?
Iodine and CO2 (dry ice)
Molecules with the same molecular formulas - but different structural formulas
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
H2PO4?

48. What is the basic structure of an optical isomer?
ROH
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Soluble
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

49. sulfate
SO4²?
E=q + w (negative is by system - positive is on system)
Ionic compounds
Identity and purity (impure compounds usually have broad & low melting points)

50. phosphate
bright yellow
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Heptane
PO4³?