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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. The oxidation # for acid base reactions...
Group I metals (soft metals) are stored under oil
Heptane
do not change
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

2. Is the freezing of ice endothermic or exothermic?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Exothermic
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

3. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Conjugate pair (one must be a weak base or acid)
The dilution effect when the solutions mix. M1V1 = M2V2
CO (poisonous)

4. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
Hg²?
redox reaction
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

5. What is the formula for summation?

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6. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Insoluble (except group 1 ammonium and Ba)
Ksp = 108s5
Increases.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

7. What are allotropes?
HClO4
blue glass - it filters UV
different forms of the same element
Acid rain - dissolves marble buildings/statues and kills trees.

8. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Ksp = 108s5
catalyst=conc H2SO4
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

9. 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?
Salt + water.
same KE - but PEice<PEwater
Disulfur dichloride
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

10. What part of a liquid do you look at to measure its volume?
The compound with the lowest Ksp value.
Read the bottom of the meniscus
O2 needs 4F/mol H2 needs 2F/mol
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

11. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
They stay the same.
Ksp = 27s4

12. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
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
chemically (ex: with carbon)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Mn²? - Cr³? - Cr³

13. What do group I/II metal oxides plus water form?
bent
[A?]/[HA] x 100 or [BH?]/[B] x 100
Monomer + monomer = polymer product + a simple molecule such as water or HCl
bases

14. What steps do organic labs consist of?
H+
Iodine and CO2 (dry ice)
Synthesis - separation and purification of the product and its identification.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

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

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16. What are the units of the first order rate constant?
Only temperature
Initiation energy (NOT Ea)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Big K=kf/kr

17. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
ROH
do not change
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

18. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Heptane
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Acids; HCOOCH3 is an ester
Pale purple - (orange)-yellow - red - blue - green.

19. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
lighted splint (positive result=pop)
left - ppt will form
Kc=Kp
Heat a test tube at an angle at the side of the tube (not bottom)

20. What are the common strong bases?
No - it depends on the number of ions produced on dissolving.
ethers
R=8.31 J/mol/K
Group 1 hydroxides (ex: NaOH)

21. What shape is methane?
Disulfur dichloride
acid + alcohol
Tetrahedral
blue

22. chromate
E=q + w (negative is by system - positive is on system)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
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.
CrO4²?

23. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Products - reactants (except for BDE when it's reactants - products)
Add acid to water so that the acid doesn't boil and spit
They decrease (or could be the same if the solid has ONLY JUST disappeared)

24. Do you use J or kJ for ?H - ?S - and ?G?
?H-kJ - ?S-J - ?G-kJ
Acidified
Evaporation
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

25. 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
CO3²?
Silvery gray solid - brown - purple
RX

26. What is the formula for percent error?
|experimental - accepted|/accepted X 100
look for changes in oxidation # - the one that goes up is oxidized and is the RA
it reacts by substitution NOT addition
Salts (ex: CaO + SO2 ? CaSO3)

27. What does a short - sharp melting point indicate?
blue glass - it filters UV
Transition element compounds (except if it has a full or empty d shell)
Identity and purity (impure compounds usually have broad & low melting points)
Anode

28. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
Read the bottom of the meniscus
Suniverse increases for spontaneous processes
T increases exponentially the proportion of molecules with E > Ea

29. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
0.10M HCl (more ions)
bases
Decant

30. Do anions flow to the cathode or anode?
C4H10
Anode
White precipitate
Experimental mass/theoretical mass X 100

31. What is the word equation for addition polymerisation?
atoms
Tetrahedral
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
OH?

32. During a titration what is present in the beaker at the equivalence point?
proton donor base
Soluble except Ag - Pb - Ca - Sr Ba)
A salt solution.
fractional distillation

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

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34. 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?
Sulfur
It ceases - the circuit is broken.
bases
The compound with the lowest Ksp value.

35. dichromate (soln + most solids)
Orange
?H formation of an element in standard state=0
Soluble
It ceases - the circuit is broken.

36. What are amphoteric oxides?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
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?)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
C4H10

37. chromate ion (soln + most solids)
yellow
NO3?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
CH3COO?

38. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
Distillation
Initiation energy (NOT Ea)
Hg²?

39. Name C7H16
0.10M HCl (more ions)
Heptane
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
RCHO (carbonyl at end)

40. acetate
NH2?
CnH2n
CH3COO?
Silvery gray solid - brown - purple

41. oxalate
ROR
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
C2O4²?
Graduated cylinder

42. Name six characteristics of transition elements (or their compounds)
Only temperature
zero
More chaotic (ex: gases made)
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)

43. A Bronsted-Lowry base is...
proton acceptor.
proton donor base
it reacts by substitution NOT addition
q=mc?T q=mL (or n x ?h)

44. How are primary alcohols turned into acids?
C2O4²?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
ethers

45. What do you use for an acid spill? base spill?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Both electrons come from the same atom (just as good as a regular bond)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
|experimental - accepted|/accepted X 100

46. Can you collect soluble gases over water?
Perform ICE BOX calculation based on K1
Acid rain - dissolves marble buildings/statues and kills trees.
No - NH3 and HCl gases are extremely soluble
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

47. BaSO4
It ceases - the circuit is broken.
Insoluble
a-IMFs - b-molecular volume
Soluble

48. What changes Keq?
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)
Disulfur dichloride
Only temperature
Pale purple - (orange)-yellow - red - blue - green.

49. Acids + Carbonates (bicarbonates) make?
ClO3?
Current - time and charge on ion (moles of e used in half cell reaction)
Acids; HCOOCH3 is an ester
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

50. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
RCOOR
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
benzene is less reactive than alkenes
voltaic: + electrolytic: -