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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. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
But S° of element is not zero (except at 0K)
Current - time and charge on ion (moles of e used in half cell reaction)
left - ppt will form
RCOOR

2. What electrons are lost/gained first in transition element ions?
RX
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
ns² electrons (first in-first out)
ethers

3. What do acids plus active metals form?
PO4³?
Salt + water
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Saturated - Substitution (which requires more radical conditions)

4. What type of compounds do metals/non metals form?
bases
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Ionic compounds
RCOOR

5. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Check for air bubbles in the buret and remove the buret funnel from the buret
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

6. What is Big K in terms of kf and kr?
Big K=kf/kr
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Identity and purity (impure compounds usually have broad & low melting points)
CN?

7. What is H2CO3 (carbonate acid) usually written as?
H2O + CO2 (it decomposes readily)
C4H10
R=8.31 J/mol/K
chemically (ex: with carbon)

8. What things should you remember to do when collecting gas over water?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
allow for the vapor pressure of water and make sure to level levels
same KE - but PEice<PEwater

9. Alcohols and _______ are FG isomers
ethers
bright yellow
No - it depends on the number of ions produced on dissolving.
same KE - but PEice<PEwater

10. What are two allotropes of carbon?
diamond and graphite
Initiation energy (NOT Ea)
do not change
basic

11. What is the test for hydrogen?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Initiation energy (NOT Ea)
lighted splint (positive result=pop)

12. oxalate
-Ea/R
C2O4²?
H3PO4
blue

13. How does group 1 metals' density compare to water's?
RCOOR
Synthetic condensation polymer (aka a polyamide)
Acids; HCOOCH3 is an ester
are less dense than water

14. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
S2O3²?
fruit - fish - bases
acid + alcohol

15. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
neutralization: high K - H2O product dissociation: low K - H2O reactant
voltaic: + electrolytic: -
SO4²?

16. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
?H formation of an element in standard state=0
fractional distillation
Iodine and CO2 (dry ice)

17. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
C4H10
bright yellow
Sulfur
CO (poisonous)

18. carbonate
Exothermic
Soluble except Ag - Pb - Ca - Sr Ba)
CO3²?
small size and high charge

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

20. How do you find the pH for a dibasic acid? (H2A)?
Perform ICE BOX calculation based on K1
Tetrahedral
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
redox reaction

21. barium sulfate
White precipitate
MnO4?
zero-th: decreases - first: constant - second: increases
Sulfur

22. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
?H-kJ - ?S-J - ?G-kJ
NH2?
zero
blue glass - it filters UV

23. What is the formula of copper (II) phosphate?
Disulfur dichloride
Cu3(PO4)2
Group I metals (soft metals) are stored under oil
RCHO (carbonyl at end)

24. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
CnH(2n+2)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
P2O5
lighted splint (positive result=pop)

25. chlorate
K1 x K2
#ligands=charge x2
ClO3?
SO4²?

26. What is the conjugate acid of H2PO4?
Trigonal pyramidal
proton acceptor.
left - ppt will form
H3PO4

27. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
More chaotic (ex: gases made)
RCOOH
different forms of the same element
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

28. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Ksp = s²
Anode - oxygen. Cathode - hydrogen
RCOOR
Conjugate pair (one must be a weak base or acid)

29. primary colors
The Faraday or Faraday's constant.
fractional distillation
Initiation energy (NOT Ea)
red - green - blue

30. What is reflux?
boiling without losing volatile solvents/reactants
proton acceptor.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
C2O4²?

31. Metal hydrides are _____ and form _______ and _______ when added to water
ROR
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
metal oxides and hydrides are ionically bonded and basic
ionic and form hydrogen and hydroxide

32. How do you explain trends in atomic properties using Coulomb's Law?
P2O5
Pour liquids using a funnel or down a glass rod
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

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

34. What are isotopes?
Salts (ex: CaO + SO2 ? CaSO3)
CN?
Anode - oxygen. Cathode - hydrogen
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

35. A Bronsted-Lowry base is...
zero
blue glass - it filters UV
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
proton acceptor.

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

37. What measuring device would you use for very small volumes of liquids?
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)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
ion pairing
Pipette (burette if need repetition)

38. Give an example of a concentrated weak acid.
The dilution effect when the solutions mix. M1V1 = M2V2
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
zero
Glacial acetic acid

39. Acid plus base make?
strong acids/bases are written as H+ or OH- ions
Salt + water.
Ksp = 4s³
Salt + water

40. Is the ?H formation of an element in standard state zero?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
?H formation of an element in standard state=0
Heptane
are less dense than water

41. What is the general formula for an amine?
RNH2
Ksp = 4s³
Greenish-yellow gas
#ligands=charge x2

42. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Sulfur
zero
ion pairing

43. phosphates
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Q=It (time in seconds)
CO3²?
Most INsoluble except group 1 and ammonium

44. What is the word equation for condensation polymerisation ?
C4H10
ClO4?
Increases down group 1 decreases down group 17
Monomer + monomer = polymer product + a simple molecule such as water or HCl

45. Why are i factors (Van't Hoff factors) often less than ideal?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Mono; di; tri; tetra; penta; hexa.
hydroxides (ex: Ba(OH)2)
ion pairing

46. 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?
Iodine and CO2 (dry ice)
Experimental mass/theoretical mass X 100
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
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

47. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
boiling without losing volatile solvents/reactants
Pour liquids using a funnel or down a glass rod
Decant

48. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
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)
no - they're written undissociated (HAaq)
Insoluble except for nitrate and acetate

49. chlorite
ClO2?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Synthesis - separation and purification of the product and its identification.
How grouped results are

50. What do group I/II metal oxides plus water form?
non-metal oxides and hydrides are covalently bonded and are acidic.
it's lower and occurs over less sharp a range
bases
Anode