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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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 process do you use to obtain the solute from a solution?
CnH2n
Group 1 hydroxides (ex: NaOH)
Evaporation
Silvery gray solid - brown - purple

2. How many normal boiling points and boiling points are there?

3. What do you do to get rid of most of the solution from a precipitate?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Insoluble except for nitrate and acetate
do not change
Decant

4. Is the ?H formation of an element in standard state zero?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Concentration
?H formation of an element in standard state=0
OH- and NH3

5. chromate ion (soln + most solids)
yellow
zero-th: decreases - first: constant - second: increases
ClO2?
All except for lithium

6. What type of polymer is nylon?
Iodine and CO2 (dry ice)
Synthetic condensation polymer (aka a polyamide)
diamond and graphite
#ligands=charge x2

7. What things should you remember to do when collecting gas over water?
water and substances with (s) less dense than
red - green - blue
allow for the vapor pressure of water and make sure to level levels
are less dense than water

8. hypochlorite
ns² electrons (first in-first out)
Ppt will NOT form (unsaturated)
ClO?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

9. chlorite
?H formation of an element in standard state=0
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
zero
ClO2?

10. What type of metals don't react with water or acids to form H2?

11. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
T increases exponentially the proportion of molecules with E > Ea
a-IMFs - b-molecular volume
atoms

12. Does reactivity increase/decrease going down group 1 and group 17?
RCOOH
voltaic: - electrolytic: +
Increases down group 1 decreases down group 17
Pipette (burette if need repetition)

13. If a weak acid is diluted more - what happens to its % dissociation value?
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
proton acceptor.
Increases.
allow for the vapor pressure of water and make sure to level levels

14. What is the slope of the graph of lnk vs. 1/T?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
ClO2?
Synthesis - separation and purification of the product and its identification.
-Ea/R

15. What is the word equation for addition polymerisation?
catalyst=conc H2SO4
do not change
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
it is lower and occurs over less sharp a range

16. permanganate
Ionic compounds
CH3COO?
MnO4?
ns² electrons (first in-first out)

17. Does Kw increase or decrease with T? Why?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
same KE - but PEice<PEwater
Initiation energy (NOT Ea)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

18. What are the signs of ?G and E° for spontaneous reactions?
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)
?G=negative - E° must be positive
E=q + w (negative is by system - positive is on system)
Pour liquids using a funnel or down a glass rod

19. What device would you use to measure a volume of gas?
Eudiometer
an oxidized and reduced substance
Pour liquids using a funnel or down a glass rod
Disulfur dichloride

20. Where are group I metals stored?
hydroxides (ex: Ba(OH)2)
Group I metals (soft metals) are stored under oil
zero-th: decreases - first: constant - second: increases
Mono; di; tri; tetra; penta; hexa.

21. oxalate
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
C2O4²?
Hg²?
ClO4?

22. What is the formula for alkynes?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
CnH2n-2
Q=It (time in seconds)
Soluble except Ag - Pb - Ca - Sr Ba)

23. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Most INsoluble except group 1 and ammonium
basic
Nothing
Ksp = 108s5

24. Nonmetals are good _____ agents. Metals are good _______ agents.
K2
Distillation
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

25. cyanide
an oxidized and reduced substance
CN?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Purple

26. What type of compounds do metals/non metals form?
different forms of the same element
Ionic compounds
[A?]/[HA] x 100 or [BH?]/[B] x 100
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

27. Color is due to ______ _______ of light.
No - it depends on the number of ions produced on dissolving.
Group 1 hydroxides (ex: NaOH)
Selective absorption
allow for the vapor pressure of water and make sure to level levels

28. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
RCOOH
|experimental - accepted|/accepted X 100
Exothermic

29. What do you need to make a polymer?
it's lower and occurs over less sharp a range
K2
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)
strong acids/bases are written as H+ or OH- ions

30. chlorate
NO3?
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?)
ClO3?
Anode

31. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
acids
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
RCOOH
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

32. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
The compound with the lowest Ksp value.
Ksp = 108s5
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

33. When a cell is 'flat' What is its voltage?
PO4³?
RCOOR
zero
A) any range. b) 8-10 c) 4-6

34. What is the conjugate base of NH3?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Glacial acetic acid
NH2?
Ksp = 4s³

35. How do you get the equation for a net electrolysis reaction?
Molecules with the same molecular formulas - but different structural formulas
No - it depends on the number of ions produced on dissolving.
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Combine the equations for the half reactions in the non-spontaneous direction

36. What is the general formula for a ketone?
0.10M HCl (more ions)
RCOR
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Ionic compounds

37. How are more active metals reduced?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
linear
by electrolysis
They stay the same.

38. What shape is water?
SO4²?
White precipitate
bent
0.10M HCl (more ions)

39. What is the general formula for an ether?
a-IMFs - b-molecular volume
ROR
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Acidified

40. What do the 'a' and 'b' in Van Der Waal's equation allow for?
CO2 and H2O
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
Both electrons come from the same atom (just as good as a regular bond)
a-IMFs - b-molecular volume

41. acetate
CH3COO?
Glacial acetic acid
hydroxides (ex: Ba(OH)2)
yellow

42. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
atoms
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Salt + water
Cr2O7²?

43. What is the formula of butane?
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.
C4H10
Greenish-yellow gas
Mn²? - Cr³? - Cr³

44. Esters smell like _______ and amines smell like _______ and are ______.
Most are soluble except Ag - Pb
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
linear
fruit - fish - bases

45. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
do not change
Soluble
neutralization: high K - H2O product dissociation: low K - H2O reactant
Add acid to water so that the acid doesn't boil and spit

46. If Q < Ksp a ppt ______
Salt + water
More chaotic (ex: gases made)
Ppt will NOT form (unsaturated)
voltaic: - electrolytic: +

47. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
benzene is less reactive than alkenes
H+
water and substances with (s) less dense than
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

48. What is the third law of thermodynamics?
S crystal at 0K=0
C2O4²?
Heptane
Identity and purity (impure compounds usually have broad & low melting points)

49. What are two allotropes of carbon?
They stay the same.
diamond and graphite
hydroxides (ex: Ba(OH)2)
Most are soluble except Ag - Pb

50. What steps do organic labs consist of?
OH- and NH3
CO (poisonous)
proton acceptor.
Synthesis - separation and purification of the product and its identification.