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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. 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?
The compound with the lowest Ksp value.
CN?
No - NH3 and HCl gases are extremely soluble
yellow

2. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
water and substances with (s) less dense than
The Faraday or Faraday's constant.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

3. If Q > Ksp - then system shifts _______ and ppt ______
Group I metals (soft metals) are stored under oil
Soluble
left - ppt will form
water and substances with (s) less dense than

4. What do acids plus active metals form?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
P2O5
a-IMFs - b-molecular volume

5. Color (absorbance) is proportional to ________
Big K=kf/kr
are less dense than water
Concentration
no - they're written undissociated (HAaq)

6. One mole of electrons carries 96500Coulombs - what is this quantity called?

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7. Is the standard entropy (S°) of an element zero?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
But S° of element is not zero (except at 0K)
CO (poisonous)
neutralization: high K - H2O product dissociation: low K - H2O reactant

8. acetates
fractional distillation
Conjugate pair (one must be a weak base or acid)
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)
Soluble

9. When can supercooling occur? What does it look like on a cooling curve?

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10. mercury (I) ion
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Hg2²?
blue glass - it filters UV
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

11. Give an example of a dilute strong acid.
Saturated - Substitution (which requires more radical conditions)
an oxidized and reduced substance
HClO4
It ceases - the circuit is broken.

12. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
water and substances with (s) less dense than
Increases.
The dilution effect when the solutions mix. M1V1 = M2V2
H2PO4?

13. How do you compute % dissociation?
K1 x K2
[A?]/[HA] x 100 or [BH?]/[B] x 100
White precipitate
Ksp = 4s³

14. How do you get the equation for a net electrolysis reaction?
The one with most oxygen atoms (highest oxidation number)
RX
Combine the equations for the half reactions in the non-spontaneous direction
Heat a test tube at an angle at the side of the tube (not bottom)

15. What apparatus do you use to separate 2 immiscible liquids?
Salt + water
S crystal at 0K=0
ClO2?
Separating funnel

16. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
No - NH3 and HCl gases are extremely soluble
Concentration
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
do not change

17. silver compounds
10?8
proton donor base
Insoluble except for nitrate and acetate
HClO4

18. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
PO4³?
benzene has a delocalized pi ring structure
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
OH?

19. What is a dipeptide? polypeptide? protein?
Clear
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
acid + alcohol
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

20. carbonate
How grouped results are
CO (poisonous)
CO3²?
Salts (ex: CaO + SO2 ? CaSO3)

21. What process do you use to separate two liquids with different boiling points?
fractional distillation
a-IMFs - b-molecular volume
zero-th: decreases - first: constant - second: increases
No - NH3 and HCl gases are extremely soluble

22. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
A salt solution.
it reacts by substitution NOT addition
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

23. bromothymol
ethers
R=8.31 J/mol/K
CnH(2n+2)
blue (BTB)

24. What are the names and formulas of the 6 strong acids?
Transition element compounds (except if it has a full or empty d shell)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
a-IMFs - b-molecular volume
metal oxides and hydrides are ionically bonded and basic

25. Why are i factors (Van't Hoff factors) often less than ideal?
left - ppt will form
ion pairing
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
Transition element compounds (except if it has a full or empty d shell)

26. What are the signs of ?G and E° for spontaneous reactions?
?G=negative - E° must be positive
Salts (ex: CaO + SO2 ? CaSO3)
Ksp = s²
basic

27. A Bronsted-Lowry acid is...
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
CnH(2n+2)
proton donor base
T increases exponentially the proportion of molecules with E > Ea

28. What do metal oxides plus acids form?
An active metal.
Salt + water
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
bases

29. hydroxides
Iodine and CO2 (dry ice)
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
Insoluble (except group 1 ammonium and Ba)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

30. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
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)
basic
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

31. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
HClO4

32. Can you collect soluble gases over water?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Salt + water
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
No - NH3 and HCl gases are extremely soluble

33. The definition of acidic basic and neutral aqueous solutions is:
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
MnO4?
ns² electrons (first in-first out)

34. What do you need to make a polymer?
Exothermic
Ksp = 4s³
CN?
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)

35. What process do you use to obtain the solute from a solution?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Evaporation
Combine the equations for the half reactions in the non-spontaneous direction
Pale yellow

36. What do group I/II metal oxides plus water form?
Check for air bubbles in the buret and remove the buret funnel from the buret
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Nothing
bases

37. What are the prefixes for the naming of binary molecular compound formulas (up to six)
PO4³?
ethers
Mono; di; tri; tetra; penta; hexa.
ClO3?

38. A Bronsted-Lowry base is...
Orange
a-IMFs - b-molecular volume
|experimental - accepted|/accepted X 100
proton acceptor.

39. What part of a liquid do you look at to measure its volume?
C2O4²?
red - green - blue
bases
Read the bottom of the meniscus

40. barium sulfate
acids
Iodine and CO2 (dry ice)
no - they're written undissociated (HAaq)
White precipitate

41. Where are group I metals stored?
Trigonal pyramidal
Group I metals (soft metals) are stored under oil
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Combine the equations for the half reactions in the non-spontaneous direction

42. What measuring device would you use for very small volumes of liquids?
CnH2n+1 often designated 'R' ex C3H7 is propyl
Pipette (burette if need repetition)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

43. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
H3PO4
Insoluble except group 1 and ammonium
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

44. hydroxide
CnH2n-2
hydroxides (ex: Ba(OH)2)
OH?
blue

45. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
But S° of element is not zero (except at 0K)
?H-kJ - ?S-J - ?G-kJ

46. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
H2PO4?
CO (poisonous)
fractional distillation

47. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
They stay the same.
chemically (ex: with carbon)
Current - time and charge on ion (moles of e used in half cell reaction)
H2O + CO2 (it decomposes readily)

48. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
chemically (ex: with carbon)
zero-th: decreases - first: constant - second: increases
Check for air bubbles in the buret and remove the buret funnel from the buret

49. What is precision?
0.10M HCl (more ions)
Anode - oxygen. Cathode - hydrogen
The benzene ring (or more correctly the phenyl group - C6H5)
How grouped results are

50. What do ions and electrons travel through in a voltaic/electrolytic cell?
Kc=Kp
NH4?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
zero-th: decreases - first: constant - second: increases