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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. When a cell is 'flat' What is its voltage?
The compound with the lowest Ksp value.
acids
Add acid to water so that the acid doesn't boil and spit
zero

2. What is the charge on a chlorine atom?
hydroxides (ex: Ba(OH)2)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
zero
Greenish-yellow gas

3. What is HCOOCH3?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Acids; HCOOCH3 is an ester
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
T increases exponentially the proportion of molecules with E > Ea

4. What shape is ammonia?
Trigonal pyramidal
Reduction always takes place at the cathode (RED CAT) In both types of cell!
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)
Sigma bonds are stronger than pi bonds

5. dichromate
Concentration
Cr2O7²?
metal oxides and hydrides are ionically bonded and basic
Silvery gray solid - brown - purple

6. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
benzene has a delocalized pi ring structure
Acidified
zero

7. What part of a liquid do you look at to measure its volume?
Trigonal pyramidal
Products - reactants (except for BDE when it's reactants - products)
Read the bottom of the meniscus
Decant

8. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Soluble
They decrease (or could be the same if the solid has ONLY JUST disappeared)
MnO4?
NH4?

9. What is the formula for summation?

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10. What complex ion does ammonia form with silver? copper? cadmium? zinc?
acid + alcohol
Insoluble except group 1 and ammonium
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
The benzene ring (or more correctly the phenyl group - C6H5)

11. What do group I/II metal oxides plus water form?
Transition element compounds (except if it has a full or empty d shell)
bases
A salt solution.
hydroxides (ex: Ba(OH)2)

12. Name some properties of Group 17
CH3COO?
OH?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

13. What shape is carbon dioxide?
ClO3?
linear
Evaporation
a-IMFs - b-molecular volume

14. lead iodide
RCOR
O2 needs 4F/mol H2 needs 2F/mol
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
bright yellow

15. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
zero
ionic and form hydrogen and hydroxide
Synthetic condensation polymer (aka a polyamide)

16. What type of compounds do Group 14 form?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
CO2 and H2O
+4-covalent - +2-ionic
Products - reactants (except for BDE when it's reactants - products)

17. Does Kw increase or decrease with T? Why?
benzene is less reactive than alkenes
At half equivalence - pH=pKa
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
K2

18. Color is due to ______ _______ of light.
Transition element compounds (except if it has a full or empty d shell)
Selective absorption
More chaotic (ex: gases made)
Initiation energy (NOT Ea)

19. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
|experimental - accepted|/accepted X 100
Pale purple - (orange)-yellow - red - blue - green.

20. chromate ion (soln + most solids)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
an oxidized and reduced substance
yellow
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

21. What do you need to make a polymer?
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)
ethers
?H formation of an element in standard state=0
How close results are to the accepted value

22. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
All except for lithium
Insoluble except group 1 and ammonium
Silvery gray solid - brown - purple

23. What are two allotropes of carbon?
diamond and graphite
Salt and water
Insoluble except nitrate and acetate
Glowing splint (positive result=relights)

24. What are the signs of ?G and E° for spontaneous reactions?
lighted splint (positive result=pop)
HClO4
Concentration
?G=negative - E° must be positive

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

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26. The oxidation # for acid base reactions...
Increases down group 1 decreases down group 17
Soluble
an oxidized and reduced substance
do not change

27. What do group I/II metal oxides and acids form?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
At half equivalence - pH=pKa
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Salt and water

28. How do you find the pH for a dibasic acid? (H2A)?
Perform ICE BOX calculation based on K1
NO3?
S crystal at 0K=0
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

29. bromothymol
Synthetic condensation polymer (aka a polyamide)
blue (BTB)
Mn²? - Cr³? - Cr³
CO (poisonous)

30. What is the first law of thermodynamics?
Hg²?
fruit - fish - bases
Anode - oxygen. Cathode - hydrogen
E=q + w (negative is by system - positive is on system)

31. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
allow for the vapor pressure of water and make sure to level levels
Synthetic condensation polymer (aka a polyamide)
Decant

32. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Ksp = s²
bright yellow
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

33. What does a short - sharp melting point indicate?
Mn²? - Cr³? - Cr³
The benzene ring (or more correctly the phenyl group - C6H5)
Q=It (time in seconds)
Identity and purity (impure compounds usually have broad & low melting points)

34. What are amphoteric oxides?
More chaotic (ex: gases made)
Synthesis - separation and purification of the product and its identification.
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?)
Salt + water.

35. What value of R do you use for thermo calculations? gas calculations?
NH4?
strong acids/bases are written as H+ or OH- ions
ROR
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

36. What process do you use to obtain a solvent from a solution?
No - it depends on the number of ions produced on dissolving.
Soluble
Distillation
Ions go through the salt bridge - electrons go through metal wires in the external circuit

37. perchlorate
lighted splint (positive result=pop)
ClO4?
CO3²?
Increases.

38. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Heptane

39. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Glacial acetic acid
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)
Mono; di; tri; tetra; penta; hexa.
benzene is less reactive than alkenes

40. What is H2CO3 (carbonate acid) usually written as?
Mn²? - Cr³? - Cr³
H2O + CO2 (it decomposes readily)
Orange
Ionic compounds

41. Where are group I metals stored?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Group I metals (soft metals) are stored under oil
RCHO (carbonyl at end)
Sulfur

42. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
S2O3²?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

43. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Most are soluble except Ag - Pb
benzene has a delocalized pi ring structure
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
bases

44. If a free element is involved - what type of reaction must be involved?
fractional distillation
redox reaction
brown volatile liquid
?H formation of an element in standard state=0

45. How do you get the equation for a net electrolysis reaction?
different forms of the same element
Combine the equations for the half reactions in the non-spontaneous direction
RX
Mono; di; tri; tetra; penta; hexa.

46. What process do you use to separate two liquids with different boiling points?
same KE - but PEice<PEwater
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
MnO4?
fractional distillation

47. Acids + Carbonates (bicarbonates) make?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Ksp = 108s5
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
are less dense than water

48. barium sulfate
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
Sigma bonds are stronger than pi bonds
White precipitate
Saturated - Substitution (which requires more radical conditions)

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

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50. What type of polymer is nylon?
H2O + CO2 (it decomposes readily)
zero
chemically (ex: with carbon)
Synthetic condensation polymer (aka a polyamide)