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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 do metal oxides plus acids form?
Exothermic
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
S crystal at 0K=0
Salt + water

2. What does saturated mean? Unsaturated?
T increases exponentially the proportion of molecules with E > Ea
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
R=8.31 J/mol/K
Soluble

3. What do you use to look at burning magnesium? why?
zero
blue glass - it filters UV
They decrease (or could be the same if the solid has ONLY JUST disappeared)
S2O3²?

4. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
PO4³?
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
ROR

5. What is the general formula for an alcohol?
ROH
Synthetic condensation polymer (aka a polyamide)
Ionic compounds
Initiation energy (NOT Ea)

6. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
fruit - fish - bases
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
a-IMFs - b-molecular volume

7. Colorless doesn't mean ______
MnO4?
Silvery gray solid - brown - purple
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Clear

8. Which would cause the bulb in a conductivity apparatus to be brightest?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
0.10M HCl (more ions)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Group I metals (soft metals) are stored under oil

9. What is the second law of thermodynamics?
Sulfur
Suniverse increases for spontaneous processes
The benzene ring (or more correctly the phenyl group - C6H5)
Salt and water

10. How are metal oxides and hydrides bonded? are they acidic or basic?
Identity and purity (impure compounds usually have broad & low melting points)
metal oxides and hydrides are ionically bonded and basic
[A?]/[HA] x 100 or [BH?]/[B] x 100
Acids; HCOOCH3 is an ester

11. Does Benzene react by addition or substitution?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Greenish-yellow gas
bent
it reacts by substitution NOT addition

12. chlorite
ClO2?
Trigonal pyramidal
[A?]/[HA] x 100 or [BH?]/[B] x 100
Iodine and CO2 (dry ice)

13. A geometric (or cis-trans) isomer exists due to.....
it is lower and occurs over less sharp a range
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
ClO2?

14. Alcohols and _______ are FG isomers
ethers
Glacial acetic acid
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
?G= -ve - E°= +ve

15. If ?S is positive - are the products more or less chaotic than the reactants?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Iodine and CO2 (dry ice)
Silvery gray solid - brown - purple
More chaotic (ex: gases made)

16. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
RCHO (carbonyl at end)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
K2

17. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
yellow
Soluble
water and substances with (s) less dense than
Graduated cylinder

18. How can metals like iron and zinc be reduced?
T increases exponentially the proportion of molecules with E > Ea
chemically (ex: with carbon)
Molecules with the same molecular formulas - but different structural formulas
Ionic compounds

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

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20. hydroxide
K2
CN?
zero-th: decreases - first: constant - second: increases
OH?

21. ammonium
small size and high charge
NH4?
Mono; di; tri; tetra; penta; hexa.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

22. What do hydrocarbons form when they burn in air (oxygen)?
Saturated - Substitution (which requires more radical conditions)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
CO2 and H2O
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

23. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
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)
ROH
K2

24. Generally - which oxy acid is strongest?
CO3²?
SO4²?
CnH2n-2
The one with most oxygen atoms (highest oxidation number)

25. How does half life change for zero-th order - first order - and second order processes?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
zero-th: decreases - first: constant - second: increases
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
CO3²?

26. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
chemically (ex: with carbon)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
water and substances with (s) less dense than

27. dichromate
different forms of the same element
Cr2O7²?
Both electrons come from the same atom (just as good as a regular bond)
Saturated - Substitution (which requires more radical conditions)

28. Color (absorbance) is proportional to ________
left - ppt will form
Concentration
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)
+4-covalent - +2-ionic

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

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30. What two types of substances are present in all redox reactions?
Add acid to water so that the acid doesn't boil and spit
an oxidized and reduced substance
redox reaction
Clear

31. Does reactivity increase/decrease going down group 1 and group 17?
Trigonal pyramidal
Increases down group 1 decreases down group 17
Exothermic (?H for ANY sa/sb = -57kJ/mol)
voltaic: - electrolytic: +

32. Where are group I metals stored?
RCOR
yellow
SO4²?
Group I metals (soft metals) are stored under oil

33. What is the conjugate acid of H2PO4?
CrO4²?
Salt + water
Time?¹ - (ex. s?¹ - hr?¹ - etc)
H3PO4

34. A Bronsted-Lowry acid is...
proton donor base
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
voltaic: - electrolytic: +
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

35. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
Insoluble except nitrate and acetate
zero-th: decreases - first: constant - second: increases
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

36. If Q < Ksp a ppt ______
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Conjugate pair (one must be a weak base or acid)
Ppt will NOT form (unsaturated)
Molecules with the same molecular formulas - but different structural formulas

37. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
Glacial acetic acid
CO3²?
The one with most oxygen atoms (highest oxidation number)

38. Aromatic compounds contain what?
The benzene ring (or more correctly the phenyl group - C6H5)
Insoluble except group 1 and ammonium
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
?G= -ve - E°= +ve

39. What are the signs of ?G and E° for spontaneous reactions?
?G=negative - E° must be positive
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Combine the equations for the half reactions in the non-spontaneous direction
are less dense than water

40. What is accuracy?
OH?
hydroxides (ex: Ba(OH)2)
White precipitate
How close results are to the accepted value

41. What is the pH of 1.0M HCl? 1M NaOH?
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)
0 and 14
proton acceptor.
Acids; HCOOCH3 is an ester

42. Acid plus base make?
Evaporation
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Salt + water.
OH- and NH3

43. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
it is lower and occurs over less sharp a range
Time?¹ - (ex. s?¹ - hr?¹ - etc)
water and substances with (s) less dense than
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

44. What are two substances that sublime at 1 atm when heated?
benzene has a delocalized pi ring structure
Iodine and CO2 (dry ice)
ClO?
Ksp = s²

45. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Hg2²?
zero
allow for the vapor pressure of water and make sure to level levels
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

46. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
S crystal at 0K=0
Sulfur
ROH

47. Is the ?H formation of an element in standard state zero?
CN?
?H formation of an element in standard state=0
ROH
Most are soluble except Ag - Pb

48. What is the difference between equivalence point and end point of a titration.
Insoluble (except group 1 ammonium and Ba)
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
it reacts by substitution NOT addition
Silvery gray solid - brown - purple

49. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Silvery gray solid - brown - purple
water and substances with (s) less dense than
Decant
Graduated cylinder

50. carbonates
Insoluble except group 1 and ammonium
water and substances with (s) less dense than
No - it depends on the number of ions produced on dissolving.
by electrolysis