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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. Ions are not ______.
Glowing splint (positive result=relights)
atoms
same KE - but PEice<PEwater
Soluble

2. chromate
CrO4²?
It ceases - the circuit is broken.
Insoluble
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

3. Which value of R do you use for all energy and kinetics calculations?
Ksp = 108s5
R=8.31 J/mol/K
ClO4?
NH2?

4. What is the formula for alkenes?
Greenish-yellow gas
S2O3²?
CnH2n
red - green - blue

5. Nonmetals are good _____ agents. Metals are good _______ agents.
Glacial acetic acid
P2O5
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
All except for lithium

6. silver iodide
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Pale yellow
The one with most oxygen atoms (highest oxidation number)
catalyst=conc H2SO4

7. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
same KE - but PEice<PEwater
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

8. How does the melting point of a mixture compare to the MP of a pure substance?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
CH3COO?
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.
it is lower and occurs over less sharp a range

9. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
Mono; di; tri; tetra; penta; hexa.
C2O4²?
White precipitate

10. sulfate
SO4²?
Ksp = 108s5
PO4³?
benzene has a delocalized pi ring structure

11. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Insoluble (except group 1 ammonium and Ba)
Read the bottom of the meniscus
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
proton donor base

12. What type of polymer is nylon?
ionic and form hydrogen and hydroxide
Synthetic condensation polymer (aka a polyamide)
fractional distillation
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

13. What is Big K in terms of kf and kr?
Big K=kf/kr
small size and high charge
Selective absorption
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

14. How are metal oxides and hydrides bonded? are they acidic or basic?
metal oxides and hydrides are ionically bonded and basic
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
benzene has a delocalized pi ring structure
HClO4

15. Aromatic compounds contain what?
redox reaction
The benzene ring (or more correctly the phenyl group - C6H5)
Current - time and charge on ion (moles of e used in half cell reaction)
How grouped results are

16. What is the test for hydrogen?
Acidified
are less dense than water
The benzene ring (or more correctly the phenyl group - C6H5)
lighted splint (positive result=pop)

17. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
?H-kJ - ?S-J - ?G-kJ
Ksp = 27s4
neutralization: high K - H2O product dissociation: low K - H2O reactant
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

18. cyanide
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CN?
Salt + water.

19. How do you identify which is oxidized or otherwise?
acids
ClO?
HClO4
look for changes in oxidation # - the one that goes up is oxidized and is the RA

20. Is the ?H formation of an element in standard state zero?
PO4³?
An active metal.
?H formation of an element in standard state=0
benzene is less reactive than alkenes

21. What do you use for an acid spill? base spill?
Increases down group 1 decreases down group 17
Evaporation
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Acids; HCOOCH3 is an ester

22. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
linear
ethers

23. A geometric (or cis-trans) isomer exists due to.....
RNH2
Check for air bubbles in the buret and remove the buret funnel from the buret
blue
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

24. Which of the rates changes more when temperature is increased?
K2
The benzene ring (or more correctly the phenyl group - C6H5)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

25. How can metals like iron and zinc be reduced?
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)
chemically (ex: with carbon)
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
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

26. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Big K=kf/kr
The compound with the lowest Ksp value.
Synthesis - separation and purification of the product and its identification.

27. Alcohols and _______ are FG isomers
ethers
ionic and form hydrogen and hydroxide
acids
proton acceptor.

28. mercury (II) ion
Hg²?
Increases down group 1 decreases down group 17
|experimental - accepted|/accepted X 100
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)

29. Why are noble gases stable?
ionic and form hydrogen and hydroxide
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
left - ppt will form
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

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

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31. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
S crystal at 0K=0
H2PO4?
Ksp = 4s³
CO3²?

32. dichromate
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Soluble
Cr2O7²?

33. What is the general formula for an acid?
RCOOH
catalyst=conc H2SO4
?H formation of an element in standard state=0
Pale yellow

34. What word is a clue for a redox reaction?
NO3?
brown volatile liquid
blue (BTB)
Acidified

35. What is an Alkyl group?

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36. What are isotopes?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ClO3?
Add acid to water so that the acid doesn't boil and spit

37. What type of compounds do metals/non metals form?
Ionic compounds
No - NH3 and HCl gases are extremely soluble
Graduated cylinder
Pour liquids using a funnel or down a glass rod

38. carbonate
CO3²?
An active metal.
CnH(2n+2)
Most are soluble except Ag - Pb

39. What shape is ammonia?
It ceases - the circuit is broken.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Trigonal pyramidal
Unsaturated - addition (ex: decolorize bromine solution)

40. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Kc=Kp
neutralization: high K - H2O product dissociation: low K - H2O reactant
R=8.31 J/mol/K

41. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
T increases exponentially the proportion of molecules with E > Ea
Exothermic (?H for ANY sa/sb = -57kJ/mol)
q=mc?T q=mL (or n x ?h)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

42. 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)
NH4?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
redox reaction

43. What is the general formula for an ether?
Read the bottom of the meniscus
yellow
Ksp = s²
ROR

44. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
different forms of the same element
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

45. Neutralization is an ________ reaction.
Unsaturated - addition (ex: decolorize bromine solution)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Concentration

46. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
do not change
PO4³?
Check for air bubbles in the buret and remove the buret funnel from the buret

47. What are isomers?
Group 1 hydroxides (ex: NaOH)
Initiation energy (NOT Ea)
Molecules with the same molecular formulas - but different structural formulas
Evaporation

48. What do you use to look at burning magnesium? why?
benzene has a delocalized pi ring structure
No - NH3 and HCl gases are extremely soluble
S crystal at 0K=0
blue glass - it filters UV

49. What do nonmetal oxides plus water form?
acids
water and substances with (s) less dense than
Eudiometer
Insoluble (except group 1 ammonium and Ba)

50. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
no - they're written undissociated (HAaq)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Silvery gray solid - brown - purple
CnH2n