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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.
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 do group I/II metal oxides and acids form?
Disulfur dichloride
H2O + CO2 (it decomposes readily)
Salt and water
Mono; di; tri; tetra; penta; hexa.

2. What is the formula for percent yield?
bases
water and substances with (s) less dense than
Experimental mass/theoretical mass X 100
left - ppt will form

3. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
voltaic: - electrolytic: +
Initiation energy (NOT Ea)
C4H10

4. What do metal oxides plus acids form?
Most INsoluble except group 1 and ammonium
Salt + water
Add acid to water so that the acid doesn't boil and spit
Insoluble

5. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
bright yellow
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

6. potassium permanganate
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Purple
H2O + CO2 (it decomposes readily)
acids

7. What is precision?
boiling without losing volatile solvents/reactants
How grouped results are
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
it's lower and occurs over less sharp a range

8. Name 2 ways in which you can create a buffer?
by electrolysis
acid + alcohol
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)
small size and high charge

9. What are the products of the reaction between group 1 metals and water?

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10. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
CN?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Ksp = s²
Salt + water.

11. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
ClO?
ion pairing
RCOR

12. Acids + Carbonates (bicarbonates) make?
C2O4²?
Separating funnel
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
0 and 14

13. What is HCOOCH3?
water and substances with (s) less dense than
K2
At half equivalence - pH=pKa
Acids; HCOOCH3 is an ester

14. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
same KE - but PEice<PEwater
OH- and NH3
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Read the bottom of the meniscus

15. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
RNH2
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

16. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Anode - oxygen. Cathode - hydrogen
a-IMFs - b-molecular volume
The dilution effect when the solutions mix. M1V1 = M2V2

17. Neutralization is an ________ reaction.
CrO4²?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
acid + alcohol
K2

18. lead compounds
acids
Ksp = s²
Cr2O7²?
Insoluble except nitrate and acetate

19. What process do you use to obtain the solute from a solution?
lighted splint (positive result=pop)
Soluble
Evaporation
hydroxides (ex: Ba(OH)2)

20. chlorine
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
CO2 and H2O
Iodine and CO2 (dry ice)
Greenish-yellow gas

21. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Graduated cylinder
Iodine and CO2 (dry ice)
do not change
Salts (ex: CaO + SO2 ? CaSO3)

22. What are amphoteric oxides?
Soluble
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?)
T increases exponentially the proportion of molecules with E > Ea
zero-th: decreases - first: constant - second: increases

23. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
no - they're written undissociated (HAaq)
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
CO2 and H2O

24. What device would you use to measure a volume of gas?
Both electrons come from the same atom (just as good as a regular bond)
Eudiometer
They stay the same.
More chaotic (ex: gases made)

25. Ca - Sr - Ba
basic
hydroxides (ex: Ba(OH)2)
acid + alcohol
E=q + w (negative is by system - positive is on system)

26. hydroxides
bases
PO4³?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Insoluble (except group 1 ammonium and Ba)

27. iodine - iodine solution - iodine vapor
Ppt will NOT form (unsaturated)
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
Silvery gray solid - brown - purple
allow for the vapor pressure of water and make sure to level levels

28. Where are group I metals stored?
Insoluble except group 1 and ammonium
Ionic compounds
Group I metals (soft metals) are stored under oil
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

29. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
diamond and graphite
All single: sp³ - one double: sp² - two doubles: sp - one triple: sp - two single and two lone pairs: sp³ - three single and one lone pair: sp³
zero-th: decreases - first: constant - second: increases
But S° of element is not zero (except at 0K)

30. Are weak acids (and bases) written dissociated?

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31. What is the test for oxygen?
Glowing splint (positive result=relights)
Salt + water
OH?
An active metal.

32. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
ClO2?
strong acids/bases are written as H+ or OH- ions
?G= -ve - E°= +ve

33. How do you compute % dissociation?
At half equivalence - pH=pKa
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
[A?]/[HA] x 100 or [BH?]/[B] x 100
it is lower and occurs over less sharp a range

34. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
allow for the vapor pressure of water and make sure to level levels
The one with most oxygen atoms (highest oxidation number)

35. What type of compounds do metals/non metals form?
Suniverse increases for spontaneous processes
Read the bottom of the meniscus
Salts (ex: CaO + SO2 ? CaSO3)
Ionic compounds

36. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
metal oxides and hydrides are ionically bonded and basic
RCOR
voltaic: + electrolytic: -

37. Give an example of a dilute strong acid.
HClO4
OH?
it reacts by substitution NOT addition
Add acid to water so that the acid doesn't boil and spit

38. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
water and substances with (s) less dense than
10?8
same KE - but PEice<PEwater
Identity and purity (impure compounds usually have broad & low melting points)

39. Name C7H16
Making sigma bonds and holding lone pairs
A) any range. b) 8-10 c) 4-6
Heptane
catalyst=conc H2SO4

40. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
S2O3²?
Evaporation

41. What is a dipeptide? polypeptide? protein?
Insoluble
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Anode
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

42. What type of compounds do Group 14 form?
NO3?
Anode
Time?¹ - (ex. s?¹ - hr?¹ - etc)
+4-covalent - +2-ionic

43. What is an Alkyl group?

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44. Is the freezing of ice endothermic or exothermic?
hydroxides (ex: Ba(OH)2)
The Faraday or Faraday's constant.
Soluble
Exothermic

45. How can metals like iron and zinc be reduced?
Ksp = 108s5
chemically (ex: with carbon)
?G= -ve - E°= +ve
White precipitate

46. What changes Keq?
Mono; di; tri; tetra; penta; hexa.
Big K=kf/kr
Only temperature
Soluble

47. group 1 ions/compounds
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Soluble
Most are soluble except Ag - Pb
Group 1 hydroxides (ex: NaOH)

48. Which alkali metals float on water?
All except for lithium
voltaic: + electrolytic: -
Iodine and CO2 (dry ice)
Acids; HCOOCH3 is an ester

49. Do anions flow to the cathode or anode?
left - ppt will form
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Anode
neutralization: high K - H2O product dissociation: low K - H2O reactant

50. What do you need to make a polymer?
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)
metal oxides and hydrides are ionically bonded and basic
CN?
different forms of the same element