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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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 name of S2Cl2? (Know how to name others like this - too)
Synthesis - separation and purification of the product and its identification.
Disulfur dichloride
[A?]/[HA] x 100 or [BH?]/[B] x 100
ClO?

2. Which alkali metals float on water?
All except for lithium
Sigma bonds are stronger than pi bonds
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
NH4?

3. What shape is methane?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Tetrahedral
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

4. Colorless doesn't mean ______
No - NH3 and HCl gases are extremely soluble
Clear
Soluble
ion pairing

5. What two types of substances are present in all redox reactions?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Salt and water
?H-kJ - ?S-J - ?G-kJ
an oxidized and reduced substance

6. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
0 and 14
They decrease (or could be the same if the solid has ONLY JUST disappeared)

7. How do you compute % dissociation?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
benzene has a delocalized pi ring structure
[A?]/[HA] x 100 or [BH?]/[B] x 100
Making sigma bonds and holding lone pairs

8. What do you use for an acid spill? base spill?
Nothing
boiling without losing volatile solvents/reactants
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

9. mercury (I) ion
acids
Hg2²?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
benzene has a delocalized pi ring structure

10. How many normal boiling points and boiling points are there?

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11. BaSO4
Insoluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
blue glass - it filters UV
Greenish-yellow gas

12. What measuring device would you use for very small volumes of liquids?
Products - reactants (except for BDE when it's reactants - products)
fractional distillation
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Pipette (burette if need repetition)

13. What part of a liquid do you look at to measure its volume?
bent
CnH2n-2
Current - time and charge on ion (moles of e used in half cell reaction)
Read the bottom of the meniscus

14. What do group I/II metal oxides plus water form?
+4-covalent - +2-ionic
Big K=kf/kr
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
bases

15. Why are i factors (Van't Hoff factors) often less than ideal?
Check for air bubbles in the buret and remove the buret funnel from the buret
ion pairing
voltaic: + electrolytic: -
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

16. Name six characteristics of transition elements (or their compounds)
CH3COO?
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)
Soluble except Ag - Pb - Ca - Sr Ba)
Soluble

17. lead compounds
Making sigma bonds and holding lone pairs
Insoluble except nitrate and acetate
The Faraday or Faraday's constant.
diamond and graphite

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

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19. hydroxides
zero-th: decreases - first: constant - second: increases
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Pale yellow
Insoluble (except group 1 ammonium and Ba)

20. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
S crystal at 0K=0
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
More chaotic (ex: gases made)

21. What should you check for before you begin titrating?
Transition element compounds (except if it has a full or empty d shell)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
an oxidized and reduced substance
Check for air bubbles in the buret and remove the buret funnel from the buret

22. What is the test for hydrogen?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
lighted splint (positive result=pop)
Experimental mass/theoretical mass X 100
same KE - but PEice<PEwater

23. Is a graduated cylinder or beaker more accurate?
are less dense than water
Graduated cylinder
ionic and form hydrogen and hydroxide
Time?¹ - (ex. s?¹ - hr?¹ - etc)

24. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
The dilution effect when the solutions mix. M1V1 = M2V2
At half equivalence - pH=pKa
it reacts by substitution NOT addition
Reduction always takes place at the cathode (RED CAT) In both types of cell!

25. When a cell is 'flat' What is its voltage?
Hg²?
Filtration
zero
CnH2n+2

26. During a titration what is present in the beaker at the equivalence point?
Soluble
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
A salt solution.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

27. Acids + Carbonates (bicarbonates) make?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Big K=kf/kr
acids

28. 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)
Pale yellow
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Ksp = 27s4

29. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Monomer + monomer = polymer product + a simple molecule such as water or HCl
H+
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

30. cyanide
Salt + water.
CN?
The dilution effect when the solutions mix. M1V1 = M2V2
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

31. What is the general formula for an amine?
methyl formate
lighted splint (positive result=pop)
metal oxides and hydrides are ionically bonded and basic
RNH2

32. What is the general formula of an alkane?
Salt + water.
CnH(2n+2)
H+
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

33. What do group I/II metal oxides and acids form?
NH4?
Decant
Cr2O7²?
Salt and water

34. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
do not change
H2O + CO2 (it decomposes readily)
Ksp = 27s4
Exothermic

35. What are the formulas for q?
Equivalence point is the titrant volume when the moles of acid and base are stoichiometrically equal; end point is the titrant volume when the color of the indicator permanently changes. If you choose the correct indicator - they should occur at the
Molecules with the same molecular formulas - but different structural formulas
q=mc?T q=mL (or n x ?h)
Most are soluble except Ag - Pb

36. What is the test for oxygen?
Insoluble except nitrate and acetate
Insoluble
Glowing splint (positive result=relights)
The compound with the lowest Ksp value.

37. bromine
boiling without losing volatile solvents/reactants
RX
different forms of the same element
brown volatile liquid

38. What are two allotropes of carbon?
S crystal at 0K=0
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
diamond and graphite
H+

39. ammonium
How grouped results are
Insoluble (except group 1 ammonium and Ba)
NH4?
same KE - but PEice<PEwater

40. What is the formula of butane?
Concentration
+4-covalent - +2-ionic
C4H10
Salts (ex: CaO + SO2 ? CaSO3)

41. What value of R do you use for thermo calculations? gas calculations?
brown volatile liquid
ClO?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

42. What do hydrocarbons form when they burn in air (oxygen)?
proton acceptor.
CO2 and H2O
CH3COO?
Ksp = 108s5

43. primary colors
brown volatile liquid
O2 needs 4F/mol H2 needs 2F/mol
Time?¹ - (ex. s?¹ - hr?¹ - etc)
red - green - blue

44. How do you heat a test tube?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Check for air bubbles in the buret and remove the buret funnel from the buret
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Heat a test tube at an angle at the side of the tube (not bottom)

45. What process do you use to obtain the precipitate from a solution?
Read the bottom of the meniscus
Filtration
[A?]/[HA] x 100 or [BH?]/[B] x 100
Clear

46. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
basic
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
voltaic: + electrolytic: -

47. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
ROR
an oxidized and reduced substance
Cu3(PO4)2

48. What device would you use to measure a volume of gas?
Eudiometer
Add acid to water so that the acid doesn't boil and spit
?G=negative - E° must be positive
ion pairing

49. What is the general formula for an ether?
ROR
Soluble
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Experimental mass/theoretical mass X 100

50. What causes the dramatic effect of T on rate?
ROH
Read the bottom of the meniscus
Exothermic
T increases exponentially the proportion of molecules with E > Ea