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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 apparatus do you use to pour liquids?
a-IMFs - b-molecular volume
Pour liquids using a funnel or down a glass rod
lighted splint (positive result=pop)
Unsaturated - addition (ex: decolorize bromine solution)

2. What are the formulas for q?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
But S° of element is not zero (except at 0K)
CN?
q=mc?T q=mL (or n x ?h)

3. How many ligands attach to a central ion in a complex ion?
ClO2?
#ligands=charge x2
OH- and NH3
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

4. What do hydrocarbons form when they burn in air (oxygen)?
different forms of the same element
CO2 and H2O
Only temperature
red - green - blue

5. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Soluble
Glowing splint (positive result=relights)

6. What is the word equation for addition polymerisation?
acid + alcohol
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
yellow
Acid rain - dissolves marble buildings/statues and kills trees.

7. What element is used to vulcanize rubber?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Pipette (burette if need repetition)
CH3COO?
Sulfur

8. How are primary alcohols turned into acids?
a-IMFs - b-molecular volume
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
proton donor base
CO2 and H2O

9. What is a dipeptide? polypeptide? protein?
But S° of element is not zero (except at 0K)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
RX
Products - reactants (except for BDE when it's reactants - products)

10. What are isomers?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
zero
Molecules with the same molecular formulas - but different structural formulas

11. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
Perform ICE BOX calculation based on K1
proton acceptor.
strong acids/bases are written as H+ or OH- ions

12. Does reactivity increase/decrease going down group 1 and group 17?
RCOOR
ROR
Increases down group 1 decreases down group 17
Salt and water

13. What is the general formula for a ketone?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
CO (poisonous)
0.10M HCl (more ions)
RCOR

14. barium sulfate
Cr2O7²?
White precipitate
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
zero

15. Give an example of a dilute strong acid.
boiling without losing volatile solvents/reactants
HClO4
The one with most oxygen atoms (highest oxidation number)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

16. What device would you use to measure a volume of gas?
zero
Eudiometer
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
zero-th: decreases - first: constant - second: increases

17. Is the freezing of ice endothermic or exothermic?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Add acid to water so that the acid doesn't boil and spit
Saturated - Substitution (which requires more radical conditions)
Exothermic

18. What effect does increasing the size/surface area of a voltaic cell have on the cell?
MnO4?
Most are soluble except Ag - Pb
All except for lithium
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

19. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
An active metal.
RCOOR
Evaporation

20. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Acid rain - dissolves marble buildings/statues and kills trees.
NO3?
MnO4?

21. Generally - which oxy acid is strongest?
bright yellow
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
The one with most oxygen atoms (highest oxidation number)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

22. What part of a liquid do you look at to measure its volume?
Acids; HCOOCH3 is an ester
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
red - green - blue
Read the bottom of the meniscus

23. During a titration what is present in the beaker at the equivalence point?
A salt solution.
Trigonal pyramidal
bent
Increases down group 1 decreases down group 17

24. hydroxides
Pipette (burette if need repetition)
Insoluble (except group 1 ammonium and Ba)
left - ppt will form
proton donor base

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

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26. What things should you remember to do when collecting gas over water?
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)
The dilution effect when the solutions mix. M1V1 = M2V2
allow for the vapor pressure of water and make sure to level levels
0.10M HCl (more ions)

27. What is Big K in terms of kf and kr?
Big K=kf/kr
Group 1 hydroxides (ex: NaOH)
It ceases - the circuit is broken.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

28. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
CnH2n+2
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)
The dilution effect when the solutions mix. M1V1 = M2V2
Ionic compounds

29. halides
Most are soluble except Ag - Pb
H+
E=q + w (negative is by system - positive is on system)
CO3²?

30. copper sulfate
H2PO4?
blue
Soluble
voltaic: - electrolytic: +

31. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Glowing splint (positive result=relights)
Greenish-yellow gas
fruit - fish - bases
neutralization: high K - H2O product dissociation: low K - H2O reactant

32. ammonium
Insoluble
same KE - but PEice<PEwater
NH4?
10?8

33. What value of R do you use for thermo calculations? gas calculations?
Ksp = 27s4
by electrolysis
do not change
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

34. Neutralization is an ________ reaction.
diamond and graphite
Tetrahedral
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Combine the equations for the half reactions in the non-spontaneous direction

35. ________ are Lewis bases - because they can donate a lone pair of electrons.
RCOOH
zero-th: decreases - first: constant - second: increases
OH- and NH3
non-metal oxides and hydrides are covalently bonded and are acidic.

36. Name six characteristics of transition elements (or their compounds)
RNH2
0.10M HCl (more ions)
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)
Insoluble (except group 1 ammonium and Ba)

37. cyanide
CN?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
0.10M HCl (more ions)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

38. Color is due to ______ _______ of light.
Sulfur
voltaic: + electrolytic: -
R=8.31 J/mol/K
Selective absorption

39. Ca - Sr - Ba
blue glass - it filters UV
hydroxides (ex: Ba(OH)2)
All except for lithium
Anode

40. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
MnO4?
red - green - blue
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

41. carbonates
10?8
red - green - blue
Insoluble except group 1 and ammonium
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)

42. How are more active metals reduced?
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
Hg²?
How close results are to the accepted value
by electrolysis

43. How do you heat a test tube?
T increases exponentially the proportion of molecules with E > Ea
CO2 and H2O
Heat a test tube at an angle at the side of the tube (not bottom)
Soluble

44. Acid plus base make?
CnH2n+2
Salt + water.
Mn²? - Cr³? - Cr³
Heptane

45. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
0 and 14
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
redox reaction

46. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
P2O5
Trigonal pyramidal
#ligands=charge x2
Pipette (burette if need repetition)

47. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
The dilution effect when the solutions mix. M1V1 = M2V2
Ppt will NOT form (unsaturated)
Evaporation

48. What is the general formula for an acid?
RCOOH
The dilution effect when the solutions mix. M1V1 = M2V2
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Ksp = s²

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

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50. What is the formula for alkenes?
a-IMFs - b-molecular volume
CnH2n
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)
H+