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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. How can metals like iron and zinc be reduced?
Heptane
chemically (ex: with carbon)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
-Ea/R

2. Acid plus base make?
Evaporation
|experimental - accepted|/accepted X 100
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Salt + water.

3. What process do you use to obtain the precipitate from a solution?
H2O + CO2 (it decomposes readily)
Greenish-yellow gas
Filtration
+4-covalent - +2-ionic

4. What two types of substances are present in all redox reactions?
voltaic: - electrolytic: +
an oxidized and reduced substance
Orange
red - green - blue

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

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6. What is Big K in terms of kf and kr?
Soluble except Ag - Pb - Ca - Sr Ba)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Big K=kf/kr
Group 1 hydroxides (ex: NaOH)

7. When combining half equations - what do you do to E° values when multiplying coefficients?
CO2 and H2O
bright yellow
benzene has a delocalized pi ring structure
Nothing

8. Acidic gases like SO2 in the atmosphere cause what environmental problems?
metal oxides and hydrides are ionically bonded and basic
Ksp = 108s5
Acid rain - dissolves marble buildings/statues and kills trees.
Synthetic condensation polymer (aka a polyamide)

9. What is the general formula for an aldehyde?
RCHO (carbonyl at end)
H3PO4
Ksp = s²
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

10. chlorine
Greenish-yellow gas
RCOR
ClO2?
CnH2n

11. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
O2 needs 4F/mol H2 needs 2F/mol
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Clear

12. Name six characteristics of transition elements (or their compounds)
Good catalysts - form multiple oxidation states - often paramagnetic - good structural metals - form a host of alloys (similar sized atoms) - have similar I energies (inner filling)
proton acceptor.
Distillation
do not change

13. Where are group I metals stored?
No - NH3 and HCl gases are extremely soluble
Insoluble (except group 1 ammonium and Ba)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Group I metals (soft metals) are stored under oil

14. hypochlorite
ClO?
0 and 14
Cu3(PO4)2
NH2?

15. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ClO3?
same KE - but PEice<PEwater
fractional distillation

16. Aromatic compounds contain what?
Identity and purity (impure compounds usually have broad & low melting points)
The benzene ring (or more correctly the phenyl group - C6H5)
C4H10
R=8.31 J/mol/K

17. What is the second law of thermodynamics?
zero
left - ppt will form
Check for air bubbles in the buret and remove the buret funnel from the buret
Suniverse increases for spontaneous processes

18. How many faradays of electric charge do you need to produce one mole of O2? H2?
Conjugate pair (one must be a weak base or acid)
O2 needs 4F/mol H2 needs 2F/mol
An active metal.
do not change

19. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Current - time and charge on ion (moles of e used in half cell reaction)
White precipitate
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Ksp = 4s³

20. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
CnH2n+2

21. What is the general formula for alkyl halides?
ROH
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
RX

22. bromothymol
Acid rain - dissolves marble buildings/statues and kills trees.
blue (BTB)
At half equivalence - pH=pKa
Acidified

23. What is the general formula for an ester?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Perform ICE BOX calculation based on K1
RCOOR
Synthesis - separation and purification of the product and its identification.

24. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
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
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)
voltaic: + electrolytic: -

25. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
Big K=kf/kr
R=8.31 J/mol/K
Increases.

26. How does group 1 metals' density compare to water's?
Pale purple - (orange)-yellow - red - blue - green.
RCHO (carbonyl at end)
are less dense than water
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

27. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
?G=negative - E° must be positive
Pale yellow
do not change

28. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
blue (BTB)
acids
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

29. How do you compute % dissociation?
CnH2n-2
Initiation energy (NOT Ea)
[A?]/[HA] x 100 or [BH?]/[B] x 100
water and substances with (s) less dense than

30. What is a dipeptide? polypeptide? protein?
proton donor base
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
S crystal at 0K=0
do not change

31. What is HCOOCH3?
NH4?
Insoluble
Acids; HCOOCH3 is an ester
Experimental mass/theoretical mass X 100

32. Does Kw increase or decrease with T? Why?
hydroxides (ex: Ba(OH)2)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
H2O + CO2 (it decomposes readily)

33. What are isomers?
Identity and purity (impure compounds usually have broad & low melting points)
ClO3?
it reacts by substitution NOT addition
Molecules with the same molecular formulas - but different structural formulas

34. What apparatus do you use to separate 2 immiscible liquids?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Only temperature
Separating funnel
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

35. Does Benzene react by addition or substitution?
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.
diamond and graphite
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)
it reacts by substitution NOT addition

36. How are strong ones written?
bent
it is lower and occurs over less sharp a range
strong acids/bases are written as H+ or OH- ions
Greenish-yellow gas

37. nitrates
NH2?
C2O4²?
T increases exponentially the proportion of molecules with E > Ea
Soluble

38. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
CnH2n-2
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Kc=Kp
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

39. mercury (II) ion
Hg²?
No - NH3 and HCl gases are extremely soluble
0 and 14
redox reaction

40. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
acids
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
?H formation of an element in standard state=0

41. perchlorate
C4H10
ClO4?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

42. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Anode
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Kc=Kp
NO3?

43. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Insoluble except group 1 and ammonium

44. The definition of acidic basic and neutral aqueous solutions is:
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.
neutralization: high K - H2O product dissociation: low K - H2O reactant
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?]

45. primary colors
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Sulfur
red - green - blue

46. ammonium
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?)
NH4?
0 and 14
Iodine and CO2 (dry ice)

47. Both Acetic acid and ____________ are also functional isomers.
blue (BTB)
Iodine and CO2 (dry ice)
methyl formate
catalyst=conc H2SO4

48. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
Synthetic condensation polymer (aka a polyamide)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Salts (ex: CaO + SO2 ? CaSO3)

49. What are the common strong bases?
Kc=Kp
bright yellow
Group 1 hydroxides (ex: NaOH)
H+

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

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