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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 is the second law of thermodynamics?
It ceases - the circuit is broken.
Suniverse increases for spontaneous processes
proton donor base
benzene is less reactive than alkenes

2. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
At half equivalence - pH=pKa
Sigma bonds are stronger than pi bonds
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Ppt will NOT form (unsaturated)

3. phosphates
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Most INsoluble except group 1 and ammonium
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)
lighted splint (positive result=pop)

4. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
#ligands=charge x2
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
[A?]/[HA] x 100 or [BH?]/[B] x 100
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

5. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Glowing splint (positive result=relights)
Add acid to water so that the acid doesn't boil and spit
Most INsoluble except group 1 and ammonium
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

6. If a weak acid is diluted more - what happens to its % dissociation value?
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)
CnH2n+1 often designated 'R' ex C3H7 is propyl
Increases.
Orange

7. What effect does increasing the size/surface area of a voltaic cell have on the cell?
CO2 and H2O
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Conjugate pair (one must be a weak base or acid)

8. How does benzene compare in reactivity to alkenes?
ROH
a-IMFs - b-molecular volume
benzene is less reactive than alkenes
Insoluble (except group 1 ammonium and Ba)

9. What causes the dramatic effect of T on rate?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Hg²?
acids
T increases exponentially the proportion of molecules with E > Ea

10. What changes Keq?
Only temperature
An active metal.
All except for lithium
Pour liquids using a funnel or down a glass rod

11. What are the common strong bases?
benzene has a delocalized pi ring structure
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Group 1 hydroxides (ex: NaOH)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

12. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
metal oxides and hydrides are ionically bonded and basic
bright yellow
CO (poisonous)
Big K=kf/kr

13. Aromatic compounds contain what?
Purple
White precipitate
The benzene ring (or more correctly the phenyl group - C6H5)
ionic and form hydrogen and hydroxide

14. What are two allotropes of carbon?
H+
diamond and graphite
proton donor base
O2 needs 4F/mol H2 needs 2F/mol

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

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16. What process do you use to separate two liquids with different boiling points?
fractional distillation
ethers
chemically (ex: with carbon)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

17. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
NH4?
an oxidized and reduced substance
linear

18. Acids + Carbonates (bicarbonates) make?
CO2 and H2O
Acid rain - dissolves marble buildings/statues and kills trees.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
ns² electrons (first in-first out)

19. What is the pH of 1.0M HCl? 1M NaOH?
R=8.31 J/mol/K
0 and 14
Synthetic condensation polymer (aka a polyamide)
Group 1 hydroxides (ex: NaOH)

20. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
CO3²?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
All except for lithium

21. What complex ion does ammonia form with silver? copper? cadmium? zinc?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
voltaic: - electrolytic: +
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Ksp = 108s5

22. What type of compounds do Group 14 form?
Ionic compounds
voltaic: + electrolytic: -
yellow
+4-covalent - +2-ionic

23. What element is used to vulcanize rubber?
Sulfur
Concentration
same KE - but PEice<PEwater
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

24. Give an example of a dilute strong acid.
lighted splint (positive result=pop)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
HClO4

25. What is accuracy?
The Faraday or Faraday's constant.
fractional distillation
How close results are to the accepted value
ns² electrons (first in-first out)

26. nitrates
Concentration
All except for lithium
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Soluble

27. oxalate
C2O4²?
left - ppt will form
boiling without losing volatile solvents/reactants
ionic and form hydrogen and hydroxide

28. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
NH4?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Pour liquids using a funnel or down a glass rod
Kc=Kp

29. What is the general formula for alkyl halides?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
RX
allow for the vapor pressure of water and make sure to level levels
They stay the same.

30. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
CH3COO?
zero
Initiation energy (NOT Ea)

31. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Saturated - Substitution (which requires more radical conditions)
Only temperature
They decrease (or could be the same if the solid has ONLY JUST disappeared)

32. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
RNH2
q=mc?T q=mL (or n x ?h)
Ksp = 108s5
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

33. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Salt + water.
basic
CnH2n+2
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

34. Alcohols and _______ are FG isomers
ethers
fruit - fish - bases
Initiation energy (NOT Ea)
voltaic: - electrolytic: +

35. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
zero
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ROH
No - it depends on the number of ions produced on dissolving.

36. What is the relationship in strength between sigma and pi bonds?
A) any range. b) 8-10 c) 4-6
Sigma bonds are stronger than pi bonds
a-IMFs - b-molecular volume
Check for air bubbles in the buret and remove the buret funnel from the buret

37. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
Insoluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
C4H10

38. What is the third law of thermodynamics?
different forms of the same element
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
S crystal at 0K=0
voltaic: + electrolytic: -

39. What shape is methane?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Most INsoluble except group 1 and ammonium
Tetrahedral
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

40. Can you collect soluble gases over water?
CnH2n
Acids; HCOOCH3 is an ester
Ions go through the salt bridge - electrons go through metal wires in the external circuit
No - NH3 and HCl gases are extremely soluble

41. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Orange
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
same KE - but PEice<PEwater
chemically (ex: with carbon)

42. Acid plus base make?
diamond and graphite
Separating funnel
Salt + water.
zero-th: decreases - first: constant - second: increases

43. group 1 ions/compounds
Soluble
RCOR
Soluble except Ag - Pb - Ca - Sr Ba)
linear

44. When a cell is 'flat' What is its voltage?
Iodine and CO2 (dry ice)
ionic and form hydrogen and hydroxide
zero
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

45. chromate ion (soln + most solids)
A salt solution.
benzene has a delocalized pi ring structure
yellow
do not change

46. What two compounds are great oxidizing agents?

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47. What do hydrocarbons form when they burn in air (oxygen)?
CO2 and H2O
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Perform ICE BOX calculation based on K1
Insoluble

48. What is HCOOCH3?
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
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Acids; HCOOCH3 is an ester
zero

49. Metal hydrides are _____ and form _______ and _______ when added to water
Big K=kf/kr
ionic and form hydrogen and hydroxide
Conjugate pair (one must be a weak base or acid)
Q=It (time in seconds)

50. What is the test for oxygen?
Synthesis - separation and purification of the product and its identification.
Glowing splint (positive result=relights)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
different forms of the same element