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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.
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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 can form during the combustion of hydrocarbons in a limited supply of oxygen?
CO (poisonous)
Most INsoluble except group 1 and ammonium
atoms
0 and 14

2. What is the third law of thermodynamics?
S crystal at 0K=0
+4-covalent - +2-ionic
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
water and substances with (s) less dense than

3. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
[A?]/[HA] x 100 or [BH?]/[B] x 100
ClO3?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

4. Acids + Carbonates (bicarbonates) make?
Group I metals (soft metals) are stored under oil
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Sigma bonds are stronger than pi bonds
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

5. What equipment do you need for a titration?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Q=It (time in seconds)
?G= -ve - E°= +ve
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

6. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
0 and 14
Insoluble except for nitrate and acetate
Insoluble

7. For a dibasic acid (H2A) - [A²?]= ____ ?
The Faraday or Faraday's constant.
K2
The benzene ring (or more correctly the phenyl group - C6H5)
Unsaturated - addition (ex: decolorize bromine solution)

8. 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?
Soluble
Nothing
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
It ceases - the circuit is broken.

9. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
A) any range. b) 8-10 c) 4-6
ClO2?
Initiation energy (NOT Ea)

10. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Insoluble except nitrate and acetate
Reduction always takes place at the cathode (RED CAT) In both types of cell!
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

11. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Ppt will NOT form (unsaturated)
linear
water and substances with (s) less dense than
no - they're written undissociated (HAaq)

12. What do nonmetal oxides plus water form?
Purple
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
acids
H2O + CO2 (it decomposes readily)

13. Give an example of a concentrated weak acid.
Glacial acetic acid
C4H10
Mn²? - Cr³? - Cr³
K2

14. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Insoluble (except group 1 ammonium and Ba)
atoms
Anode - oxygen. Cathode - hydrogen
Heptane

15. What steps do organic labs consist of?
by electrolysis
Pour liquids using a funnel or down a glass rod
Synthesis - separation and purification of the product and its identification.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

16. Colorless doesn't mean ______
Greenish-yellow gas
SO4²?
Clear
Evaporation

17. What is the sign of the anode in voltaic cells? in electrolytic cells?
They stay the same.
zero
voltaic: - electrolytic: +
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

18. 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?
CnH(2n+2)
a-IMFs - b-molecular volume
An active metal.

19. What are the names and formulas of the 6 strong acids?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Exothermic
0 and 14

20. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
A) any range. b) 8-10 c) 4-6
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
water and substances with (s) less dense than
acid + alcohol

21. What is the conjugate base of NH3?
The dilution effect when the solutions mix. M1V1 = M2V2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
blue glass - it filters UV
NH2?

22. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
Glacial acetic acid
Only temperature
Big K=kf/kr

23. What process do you use to obtain a solvent from a solution?
blue (BTB)
Distillation
Salts (ex: CaO + SO2 ? CaSO3)
CO3²?

24. What is the general formula for an acid?
water and substances with (s) less dense than
CnH2n+1 often designated 'R' ex C3H7 is propyl
RCOOH
It ceases - the circuit is broken.

25. What shape is water?
Pale purple - (orange)-yellow - red - blue - green.
bent
How grouped results are
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

26. What is the formula for percent yield?
K1 x K2
Experimental mass/theoretical mass X 100
Identity and purity (impure compounds usually have broad & low melting points)
ns² electrons (first in-first out)

27. Which of the rates changes more when temperature is increased?
Hg²?
Insoluble (except group 1 ammonium and Ba)
Both electrons come from the same atom (just as good as a regular bond)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

28. What things should you remember to do when collecting gas over water?
PO4³?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
allow for the vapor pressure of water and make sure to level levels
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

29. mercury (II) ion
Tetrahedral
H2PO4?
Hg²?
Soluble except Ag - Pb - Ca - Sr Ba)

30. What do hydrocarbons form when they burn in air (oxygen)?
Check for air bubbles in the buret and remove the buret funnel from the buret
CO2 and H2O
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
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.

31. How are more active metals reduced?
chemically (ex: with carbon)
by electrolysis
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Combine the equations for the half reactions in the non-spontaneous direction

32. hypochlorite
Distillation
ClO?
C4H10
P2O5

33. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Suniverse increases for spontaneous processes
no - they're written undissociated (HAaq)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

34. What is HCOOCH3?
q=mc?T q=mL (or n x ?h)
Acids; HCOOCH3 is an ester
Insoluble except for nitrate and acetate
blue (BTB)

35. oxalate
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
C2O4²?
H3PO4
Saturated - Substitution (which requires more radical conditions)

36. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Cr2O7²?
same KE - but PEice<PEwater
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?)
A salt solution.

37. hydroxide
OH?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
NH2?
water and substances with (s) less dense than

38. acetate
CH3COO?
linear
non-metal oxides and hydrides are covalently bonded and are acidic.
Mono; di; tri; tetra; penta; hexa.

39. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
are less dense than water
Ksp = 27s4
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)
O2 needs 4F/mol H2 needs 2F/mol

40. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Pour liquids using a funnel or down a glass rod
Read the bottom of the meniscus
S crystal at 0K=0
non-metal oxides and hydrides are covalently bonded and are acidic.

41. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Ksp = 27s4
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Pour liquids using a funnel or down a glass rod

42. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
The Faraday or Faraday's constant.
CnH2n-2
same KE - but PEice<PEwater

43. Ca - Sr - Ba
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
An active metal.
hydroxides (ex: Ba(OH)2)
10?8

44. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
OH- and NH3
The benzene ring (or more correctly the phenyl group - C6H5)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
?H-kJ - ?S-J - ?G-kJ

45. dichromate
The benzene ring (or more correctly the phenyl group - C6H5)
They stay the same.
RCOR
Cr2O7²?

46. Color is due to ______ _______ of light.
Most are soluble except Ag - Pb
Selective absorption
Greenish-yellow gas
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)

47. Do you use J or kJ for ?H - ?S - and ?G?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
#ligands=charge x2
The compound with the lowest Ksp value.
?H-kJ - ?S-J - ?G-kJ

48. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
At half equivalence - pH=pKa

49. nitrates
CO3²?
ClO4?
red - green - blue
Soluble

50. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
CO3²?
Ksp = s²
CO (poisonous)
Reduction always takes place at the cathode (RED CAT) In both types of cell!