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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. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Glacial acetic acid
basic
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

2. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
proton donor base
All except for lithium
The compound with the lowest Ksp value.

3. What two types of substances are present in all redox reactions?
Most are soluble except Ag - Pb
A) any range. b) 8-10 c) 4-6
blue (BTB)
an oxidized and reduced substance

4. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
How close results are to the accepted value
it's lower and occurs over less sharp a range
The benzene ring (or more correctly the phenyl group - C6H5)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

5. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
Transition element compounds (except if it has a full or empty d shell)
C2O4²?
fractional distillation

6. How many faradays of electric charge do you need to produce one mole of O2? H2?
Group 1 hydroxides (ex: NaOH)
ClO?
O2 needs 4F/mol H2 needs 2F/mol
Reduction always takes place at the cathode (RED CAT) In both types of cell!

7. When is ?G zero?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
RX
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

8. How do you find the pH for a dibasic acid? (H2A)?
Products - reactants (except for BDE when it's reactants - products)
CnH2n
Perform ICE BOX calculation based on K1
0 and 14

9. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
CnH2n-2
C2O4²?
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.

10. What is the general formula for an alcohol?
ROH
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
benzene has a delocalized pi ring structure
RCOOR

11. What does the solubility of organic compounds depend on?
RCHO (carbonyl at end)
Group 1 hydroxides (ex: NaOH)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
The compound with the lowest Ksp value.

12. silver compounds
Heptane
Insoluble except for nitrate and acetate
Hg2²?
|experimental - accepted|/accepted X 100

13. A Bronsted-Lowry base is...
+4-covalent - +2-ionic
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Salt + water
proton acceptor.

14. thiosulfate
Exothermic (?H for ANY sa/sb = -57kJ/mol)
H2O + CO2 (it decomposes readily)
by electrolysis
S2O3²?

15. What are amphoteric oxides?
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?)
bright yellow
A salt solution.
Concentration

16. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Identity and purity (impure compounds usually have broad & low melting points)
Mono; di; tri; tetra; penta; hexa.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Mn²? - Cr³? - Cr³

17. Give an example of a dilute strong acid.
Anode - oxygen. Cathode - hydrogen
bright yellow
Increases.
HClO4

18. What type of solutions do small - highly charged cations tend to form?
MnO4?
brown volatile liquid
?G=negative - E° must be positive
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

19. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
Soluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Identity and purity (impure compounds usually have broad & low melting points)

20. silver iodide
Pale yellow
K1 x K2
Soluble
The compound with the lowest Ksp value.

21. Ions are not ______.
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.
do not change
atoms
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?)

22. BaSO4
More chaotic (ex: gases made)
Insoluble
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

23. permanganate
CO (poisonous)
MnO4?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

24. oxalate
'non-active' metals such as Cu - Ag - Au - Pt - etc.
C2O4²?
Ksp = 108s5
no - they're written undissociated (HAaq)

25. How does the melting point of a mixture compare to the MP of a pure substance?

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26. hydroxide
?H-kJ - ?S-J - ?G-kJ
OH?
atoms
|experimental - accepted|/accepted X 100

27. One mole of electrons carries 96500Coulombs - what is this quantity called?

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28. mercury (I) ion
Hg2²?
Big K=kf/kr
Selective absorption
Ionic compounds

29. Acidic gases like SO2 in the atmosphere cause what environmental problems?
More chaotic (ex: gases made)
Purple
Trigonal pyramidal
Acid rain - dissolves marble buildings/statues and kills trees.

30. What do group I/II metal oxides plus water form?
Most are soluble except Ag - Pb
How grouped results are
#ligands=charge x2
bases

31. What is a coordinate covalent bond?
an oxidized and reduced substance
Both electrons come from the same atom (just as good as a regular bond)
boiling without losing volatile solvents/reactants
no - they're written undissociated (HAaq)

32. What device would you use to measure a volume of gas?
Ksp = s²
An active metal.
Eudiometer
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

33. When a cell is 'flat' What is its voltage?
zero
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Glacial acetic acid
methyl formate

34. Name six characteristics of transition elements (or their compounds)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
H3PO4
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)

35. What is the general formula for an ether?
ClO3?
fractional distillation
ROR
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

36. The definition of acidic basic and neutral aqueous solutions is:
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Exothermic
basic

37. What type of compounds are almost always colored?
The benzene ring (or more correctly the phenyl group - C6H5)
Ksp = 4s³
Transition element compounds (except if it has a full or empty d shell)
Read the bottom of the meniscus

38. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Mono; di; tri; tetra; penta; hexa.
Group 1 hydroxides (ex: NaOH)
Evaporation
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

39. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
zero-th: decreases - first: constant - second: increases

40. lead iodide
Unsaturated - addition (ex: decolorize bromine solution)
bright yellow
P2O5
water and substances with (s) less dense than

41. What is the word equation for condensation polymerisation ?
The compound with the lowest Ksp value.
Insoluble (except group 1 ammonium and Ba)
CO (poisonous)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

42. Acid plus base make?
Salt + water.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
ClO?
The compound with the lowest Ksp value.

43. Is a graduated cylinder or beaker more accurate?
voltaic: - electrolytic: +
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Anode
Graduated cylinder

44. perchlorate
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Increases down group 1 decreases down group 17
fractional distillation
ClO4?

45. dichromate (soln + most solids)
Selective absorption
Orange
S crystal at 0K=0
ionic and form hydrogen and hydroxide

46. How do you identify which is oxidized or otherwise?
Salts (ex: CaO + SO2 ? CaSO3)
More chaotic (ex: gases made)
CnH2n-2
look for changes in oxidation # - the one that goes up is oxidized and is the RA

47. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Salt + water.
zero
H2O + CO2 (it decomposes readily)
same KE - but PEice<PEwater

48. Is the ?H formation of an element in standard state zero?
Making sigma bonds and holding lone pairs
O2 needs 4F/mol H2 needs 2F/mol
?H formation of an element in standard state=0
Iodine and CO2 (dry ice)

49. What type of compounds do metals/non metals form?
Synthetic condensation polymer (aka a polyamide)
Ionic compounds
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)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

50. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
0 and 14
OH?
Ksp = 108s5
brown volatile liquid

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AP Chemistry 2

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