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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 are the signs of ?G and E° for spontaneous reactions?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
?G=negative - E° must be positive
Sigma bonds are stronger than pi bonds
Molecules with the same molecular formulas - but different structural formulas

2. One mole of electrons carries 96500Coulombs - what is this quantity called?

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3. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
fruit - fish - bases
CO (poisonous)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Mono; di; tri; tetra; penta; hexa.

4. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
Both electrons come from the same atom (just as good as a regular bond)
bright yellow
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

5. What shape is carbon dioxide?
linear
Soluble except Ag - Pb - Ca - Sr Ba)
an oxidized and reduced substance
RX

6. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
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.
CnH2n
Salt and water

7. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
The benzene ring (or more correctly the phenyl group - C6H5)
voltaic: - electrolytic: +
K1 x K2
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

8. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
by electrolysis
yellow
red - green - blue

9. silver compounds
Insoluble except for nitrate and acetate
proton donor base
Iodine and CO2 (dry ice)
Group 1 hydroxides (ex: NaOH)

10. Which alkali metals float on water?
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
All except for lithium
Unsaturated - addition (ex: decolorize bromine solution)
Purple

11. hydroxide
CnH(2n+2)
OH- and NH3
SO4²?
OH?

12. What are the prefixes for the naming of binary molecular compound formulas (up to six)
ClO?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Mono; di; tri; tetra; penta; hexa.
CnH(2n+2)

13. Generally - which oxy acid is strongest?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
The one with most oxygen atoms (highest oxidation number)
More chaotic (ex: gases made)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

14. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Soluble
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Ksp = 27s4
NH4?

15. What things should you remember to do when collecting gas over water?
Filtration
CnH2n+2
Evaporation
allow for the vapor pressure of water and make sure to level levels

16. What is the general formula for an alcohol?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Sulfur
H2O + CO2 (it decomposes readily)
ROH

17. carbonate
zero-th: decreases - first: constant - second: increases
CO3²?
Increases.
Molecules with the same molecular formulas - but different structural formulas

18. What word is a clue for a redox reaction?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Acid rain - dissolves marble buildings/statues and kills trees.
Acidified
The dilution effect when the solutions mix. M1V1 = M2V2

19. What kind of bonding structure does benzene have?
Only temperature
benzene has a delocalized pi ring structure
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?

20. Esters smell like _______ and amines smell like _______ and are ______.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
RX
fruit - fish - bases
Salt + water.

21. What is precision?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
But S° of element is not zero (except at 0K)
Purple
How grouped results are

22. What apparatus do you use to separate 2 immiscible liquids?
Saturated - Substitution (which requires more radical conditions)
CnH(2n+2)
benzene is less reactive than alkenes
Separating funnel

23. Where are group I metals stored?
It ceases - the circuit is broken.
Group I metals (soft metals) are stored under oil
Purple
Ksp = 108s5

24. What is the general formula for an amine?
RNH2
Insoluble
water and substances with (s) less dense than
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

25. Acidic gases like SO2 in the atmosphere cause what environmental problems?
CN?
Synthesis - separation and purification of the product and its identification.
More chaotic (ex: gases made)
Acid rain - dissolves marble buildings/statues and kills trees.

26. 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?
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
bright yellow
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
NO3?

27. Does reactivity increase/decrease going down group 1 and group 17?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Insoluble
Increases down group 1 decreases down group 17
The Faraday or Faraday's constant.

28. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Synthetic condensation polymer (aka a polyamide)
Silvery gray solid - brown - purple
NH4?
same KE - but PEice<PEwater

29. chromate ion (soln + most solids)
Big K=kf/kr
yellow
do not change
non-metal oxides and hydrides are covalently bonded and are acidic.

30. What process do you use to obtain the solute from a solution?
neutralization: high K - H2O product dissociation: low K - H2O reactant
How close results are to the accepted value
Hg2²?
Evaporation

31. What is the sign of the anode in voltaic cells? in electrolytic cells?
blue
voltaic: - electrolytic: +
Distillation
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

32. Do anions flow to the cathode or anode?
Pale purple - (orange)-yellow - red - blue - green.
Anode
fractional distillation
Heptane

33. Both Acetic acid and ____________ are also functional isomers.
methyl formate
CrO4²?
CO2 and H2O
Combine the equations for the half reactions in the non-spontaneous direction

34. What is the first law of thermodynamics?
Tetrahedral
E=q + w (negative is by system - positive is on system)
benzene has a delocalized pi ring structure
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

35. What does a short - sharp melting point indicate?
Ksp = 27s4
Identity and purity (impure compounds usually have broad & low melting points)
red - green - blue
zero-th: decreases - first: constant - second: increases

36. During a titration what is present in the beaker at the equivalence point?
Increases down group 1 decreases down group 17
Synthesis - separation and purification of the product and its identification.
Disulfur dichloride
A salt solution.

37. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
No - NH3 and HCl gases are extremely soluble

38. phosphate
Most are soluble except Ag - Pb
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
chemically (ex: with carbon)
PO4³?

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

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40. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
0 and 14
Glacial acetic acid
P2O5

41. What do the 'a' and 'b' in Van Der Waal's equation allow for?
boiling without losing volatile solvents/reactants
q=mc?T q=mL (or n x ?h)
Soluble
a-IMFs - b-molecular volume

42. What is the general formula for an aldehyde?
More chaotic (ex: gases made)
RCOOR
Hg²?
RCHO (carbonyl at end)

43. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Soluble
acids

44. ________ are Lewis bases - because they can donate a lone pair of electrons.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Filtration
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
OH- and NH3

45. Alkanes are _________ and react by _________
They stay the same.
Saturated - Substitution (which requires more radical conditions)
No - it depends on the number of ions produced on dissolving.
it's lower and occurs over less sharp a range

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

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47. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Insoluble except for nitrate and acetate
Heptane
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

48. What are isotopes?
Soluble
ROH
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

49. perchlorate
Experimental mass/theoretical mass X 100
ionic and form hydrogen and hydroxide
ClO4?
ion pairing

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

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