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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 are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Products - reactants (except for BDE when it's reactants - products)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Pale yellow
ethers

2. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Hg²?
Ksp = 27s4
Soluble
CrO4²?

3. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
chemically (ex: with carbon)
Salt and water
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

4. Is the freezing of ice endothermic or exothermic?
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 -
Iodine and CO2 (dry ice)
basic

5. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
acids
zero
Products - reactants (except for BDE when it's reactants - products)

6. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
C2O4²?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

7. What is a dipeptide? polypeptide? protein?
proton acceptor.
linear
it is lower and occurs over less sharp a range
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

8. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
#ligands=charge x2
Trigonal pyramidal
bases
same KE - but PEice<PEwater

9. What reacts with an acid to create hydrogen gas?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
An active metal.
Kc=Kp
The dilution effect when the solutions mix. M1V1 = M2V2

10. hydroxides
Graduated cylinder
Insoluble (except group 1 ammonium and Ba)
it's lower and occurs over less sharp a range
Conjugate pair (one must be a weak base or acid)

11. chlorate
A salt solution.
ClO3?
different forms of the same element
They decrease (or could be the same if the solid has ONLY JUST disappeared)

12. What are hybrid orbitals used for?
zero
Making sigma bonds and holding lone pairs
?H-kJ - ?S-J - ?G-kJ
Ksp = 108s5

13. What is HCOOCH3?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
0 and 14
The compound with the lowest Ksp value.
Acids; HCOOCH3 is an ester

14. BaSO4
They decrease (or could be the same if the solid has ONLY JUST disappeared)
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.
Iodine and CO2 (dry ice)
Insoluble

15. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
Cr2O7²?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
H+

16. What is an Alkyl group?

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17. nitrates
Ionic compounds
Soluble
OH?
blue

18. cyanide
Glowing splint (positive result=relights)
CN?
Anode - oxygen. Cathode - hydrogen
Most are soluble except Ag - Pb

19. What are the signs for ?G and E° for spontaneous reactions?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
?G= -ve - E°= +ve
Disulfur dichloride

20. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pale purple - (orange)-yellow - red - blue - green.
A) any range. b) 8-10 c) 4-6
OH?
PO4³?

21. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Cr2O7²?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
A) any range. b) 8-10 c) 4-6

22. What do you need to make a polymer?
benzene is less reactive than alkenes
White precipitate
It ceases - the circuit is broken.
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)

23. phosphates
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
Check for air bubbles in the buret and remove the buret funnel from the buret
Most INsoluble except group 1 and ammonium
RCHO (carbonyl at end)

24. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Selective absorption
The dilution effect when the solutions mix. M1V1 = M2V2
benzene has a delocalized pi ring structure

25. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
non-metal oxides and hydrides are covalently bonded and are acidic.
it is lower and occurs over less sharp a range
K1 x K2
voltaic: - electrolytic: +

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

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27. What is a coordinate covalent bond?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
No - it depends on the number of ions produced on dissolving.
CH3COO?
Both electrons come from the same atom (just as good as a regular bond)

28. Give an example of a concentrated weak acid.
zero
Disulfur dichloride
Glacial acetic acid
a-IMFs - b-molecular volume

29. What word is a clue for a redox reaction?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Big K=kf/kr
0.10M HCl (more ions)
Acidified

30. What changes Keq?
Only temperature
Soluble
Exothermic
Anode

31. The definition of acidic basic and neutral aqueous solutions is:
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
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.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

32. What kind of bonding structure does benzene have?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Anode
benzene has a delocalized pi ring structure
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

33. Does Kw increase or decrease with T? Why?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Disulfur dichloride
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

34. What are two allotropes of carbon?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
bases
diamond and graphite
zero

35. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
?G=negative - E° must be positive
Unsaturated - addition (ex: decolorize bromine solution)

36. What process do you use to obtain the precipitate from a solution?
water and substances with (s) less dense than
CO (poisonous)
Identity and purity (impure compounds usually have broad & low melting points)
Filtration

37. What do the 'a' and 'b' in Van Der Waal's equation allow for?
0 and 14
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
CO (poisonous)
a-IMFs - b-molecular volume

38. Which would cause the bulb in a conductivity apparatus to be brightest?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
it reacts by substitution NOT addition
0.10M HCl (more ions)

39. What is the formula for alkynes?
CnH2n-2
chemically (ex: with carbon)
a-IMFs - b-molecular volume
Filtration

40. Which alkali metals float on water?
All except for lithium
CnH2n
Trigonal pyramidal
Ksp = 108s5

41. How do you clean a buret/pipette for a titration?
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
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Insoluble except for nitrate and acetate
Salt and water

42. bromine
Suniverse increases for spontaneous processes
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
brown volatile liquid
Distillation

43. How do you get Ecell for spontaneous reactions?
Check for air bubbles in the buret and remove the buret funnel from the buret
Mono; di; tri; tetra; penta; hexa.
Clear
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

44. What is the conjugate acid of H2PO4?
fractional distillation
it's lower and occurs over less sharp a range
H3PO4
ROH

45. What is the third law of thermodynamics?
strong acids/bases are written as H+ or OH- ions
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
S crystal at 0K=0

46. dihydrogen phosphate
-Ea/R
bases
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
H2PO4?

47. What type of compounds do metals/non metals form?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Ionic compounds
At half equivalence - pH=pKa
The benzene ring (or more correctly the phenyl group - C6H5)

48. Alcohols and _______ are FG isomers
Combine the equations for the half reactions in the non-spontaneous direction
All except for lithium
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
ethers

49. Can you collect soluble gases over water?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
H3PO4
No - NH3 and HCl gases are extremely soluble
|experimental - accepted|/accepted X 100

50. What is the relationship in strength between sigma and pi bonds?
CO2 and H2O
Sigma bonds are stronger than pi bonds
[A?]/[HA] x 100 or [BH?]/[B] x 100
At half equivalence - pH=pKa