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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. Name 2 ways in which you can create a buffer?
strong acids/bases are written as H+ or OH- ions
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
Glacial acetic 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)

2. What things should you remember to do when collecting gas over water?
Soluble except Ag - Pb - Ca - Sr Ba)
CN?
allow for the vapor pressure of water and make sure to level levels
RX

3. Metal hydrides are _____ and form _______ and _______ when added to water
an oxidized and reduced substance
ionic and form hydrogen and hydroxide
strong acids/bases are written as H+ or OH- ions
They decrease (or could be the same if the solid has ONLY JUST disappeared)

4. What does a short - sharp melting point indicate?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Identity and purity (impure compounds usually have broad & low melting points)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Soluble except Ag - Pb - Ca - Sr Ba)

5. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
T increases exponentially the proportion of molecules with E > Ea
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
10?8
H+

6. What do you use to look at burning magnesium? why?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
The dilution effect when the solutions mix. M1V1 = M2V2
Salt and water
blue glass - it filters UV

7. Name C7H16
ClO?
Heptane
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
RCOR

8. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Pale yellow
Mono; di; tri; tetra; penta; hexa.
Increases.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

9. What changes Keq?
Only temperature
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
No - it depends on the number of ions produced on dissolving.
Soluble

10. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Pale purple - (orange)-yellow - red - blue - green.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

11. acetates
Glacial acetic acid
voltaic: + electrolytic: -
Soluble
Distillation

12. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Pale yellow
R=8.31 J/mol/K
0 and 14

13. If ?S is positive - are the products more or less chaotic than the reactants?
H3PO4
More chaotic (ex: gases made)
Increases down group 1 decreases down group 17
linear

14. When is ?G zero?
Anode - oxygen. Cathode - hydrogen
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
NH2?

15. ________ are Lewis bases - because they can donate a lone pair of electrons.
CO2 and H2O
OH- and NH3
The dilution effect when the solutions mix. M1V1 = M2V2
red - green - blue

16. How are more active metals reduced?
Sulfur
OH- and NH3
q=mc?T q=mL (or n x ?h)
by electrolysis

17. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Synthetic condensation polymer (aka a polyamide)
benzene has a delocalized pi ring structure
HClO4
H+

18. What is the sign of the anode in voltaic cells? in electrolytic cells?
voltaic: - electrolytic: +
Combine the equations for the half reactions in the non-spontaneous direction
NO3?
Acid rain - dissolves marble buildings/statues and kills trees.

19. thiosulfate
S2O3²?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
brown volatile liquid
K2

20. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
no - they're written undissociated (HAaq)
How grouped results are
NH2?

21. What is the formula for alkenes?
CH3COO?
CnH2n
Soluble
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

22. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ksp = 27s4
OH- and NH3
It ceases - the circuit is broken.

23. Esterification is...
zero
?H formation of an element in standard state=0
acid + alcohol
bases

24. What do hydrocarbons form when they burn in air (oxygen)?
diamond and graphite
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
CO2 and H2O
do not change

25. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
hydroxides (ex: Ba(OH)2)
Sigma bonds are stronger than pi bonds
Soluble

26. What process do you use to obtain a solvent from a solution?
|experimental - accepted|/accepted X 100
Distillation
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Concentration

27. 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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28. hypochlorite
NH4?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Products - reactants (except for BDE when it's reactants - products)
ClO?

29. group 1 ions/compounds
Iodine and CO2 (dry ice)
Soluble
Check for air bubbles in the buret and remove the buret funnel from the buret
C2O4²?

30. Give an example of a concentrated weak acid.
Glacial acetic acid
CN?
Identity and purity (impure compounds usually have broad & low melting points)
CO (poisonous)

31. carbonate
CO3²?
CO (poisonous)
The dilution effect when the solutions mix. M1V1 = M2V2
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

32. How does the melting point of a mixture compare to the MP of a pure substance?

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33. What does the solubility of organic compounds depend on?
Insoluble except for nitrate and acetate
Kc=Kp
redox reaction
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

34. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Unsaturated - addition (ex: decolorize bromine solution)
A) any range. b) 8-10 c) 4-6
same KE - but PEice<PEwater
RCOOR

35. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
All except for lithium
Insoluble except for nitrate and acetate
CnH(2n+2)
basic

36. Aromatic compounds contain what?
Perform ICE BOX calculation based on K1
bright yellow
The benzene ring (or more correctly the phenyl group - C6H5)
Most are soluble except Ag - Pb

37. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
The dilution effect when the solutions mix. M1V1 = M2V2
Synthesis - separation and purification of the product and its identification.
CnH2n
The compound with the lowest Ksp value.

38. hydroxides
metal oxides and hydrides are ionically bonded and basic
Exothermic (?H for ANY sa/sb = -57kJ/mol)
do not change
Insoluble (except group 1 ammonium and Ba)

39. Is the freezing of ice endothermic or exothermic?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Exothermic
Transition element compounds (except if it has a full or empty d shell)
Distillation

40. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
chemically (ex: with carbon)
[A?]/[HA] x 100 or [BH?]/[B] x 100
same KE - but PEice<PEwater

41. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
Group 1 hydroxides (ex: NaOH)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
zero-th: decreases - first: constant - second: increases

42. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
H+
CO (poisonous)
SO4²?
Ionic compounds

43. What is H2CO3 (carbonate acid) usually written as?
same KE - but PEice<PEwater
H2O + CO2 (it decomposes readily)
hydroxides (ex: Ba(OH)2)
Insoluble except for nitrate and acetate

44. What are allotropes?
How grouped results are
Soluble except Ag - Pb - Ca - Sr Ba)
different forms of the same element
Saturated - Substitution (which requires more radical conditions)

45. copper sulfate
blue
neutralization: high K - H2O product dissociation: low K - H2O reactant
Salt + water.
Cu3(PO4)2

46. cyanide
Check for air bubbles in the buret and remove the buret funnel from the buret
CN?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
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.

47. Both Acetic acid and ____________ are also functional isomers.
CO2 and H2O
CrO4²?
acids
methyl formate

48. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
More chaotic (ex: gases made)
RCOOH
The Faraday or Faraday's constant.

49. What is the test for hydrogen?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
CnH2n-2
lighted splint (positive result=pop)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

50. What is the general formula for an alcohol?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Most INsoluble except group 1 and ammonium
ROH
same KE - but PEice<PEwater