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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 general formula for an amine?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
RNH2
Pour liquids using a funnel or down a glass rod
Reduction always takes place at the cathode (RED CAT) In both types of cell!

2. What measuring device would you use for very small volumes of liquids?
Big K=kf/kr
Trigonal pyramidal
Pipette (burette if need repetition)
Greenish-yellow gas

3. What is the general formula for a ketone?
RCOR
Most INsoluble except group 1 and ammonium
CnH2n
More chaotic (ex: gases made)

4. hydroxide
OH?
Clear
Cr2O7²?
Acids; HCOOCH3 is an ester

5. What are the units of the first order rate constant?
Exothermic
voltaic: - electrolytic: +
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

6. What is the test for hydrogen?
no - they're written undissociated (HAaq)
lighted splint (positive result=pop)
Cr2O7²?
MnO4?

7. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
ion pairing
Most are soluble except Ag - Pb
H+

8. Why are i factors (Van't Hoff factors) often less than ideal?
RNH2
CN?
ion pairing
How grouped results are

9. dichromate (soln + most solids)
PO4³?
ClO3?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Orange

10. thiosulfate
non-metal oxides and hydrides are covalently bonded and are acidic.
zero
S2O3²?
Salt and water

11. What is the formula for alkenes?
HClO4
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
CnH2n
A salt solution.

12. How do you clean a buret/pipette for a titration?
Kc=Kp
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Big K=kf/kr
The benzene ring (or more correctly the phenyl group - C6H5)

13. What shape is carbon dioxide?
A) any range. b) 8-10 c) 4-6
ns² electrons (first in-first out)
acids
linear

14. What are isotopes?
Identity and purity (impure compounds usually have broad & low melting points)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
are less dense than water
Iodine and CO2 (dry ice)

15. A Bronsted-Lowry base is...
Glacial acetic acid
Iodine and CO2 (dry ice)
proton acceptor.
But S° of element is not zero (except at 0K)

16. What type of polymer is nylon?
Soluble
Ksp = 4s³
Hg2²?
Synthetic condensation polymer (aka a polyamide)

17. What type of compounds are almost always colored?
it is lower and occurs over less sharp a range
Transition element compounds (except if it has a full or empty d shell)
allow for the vapor pressure of water and make sure to level levels
Ksp = 27s4

18. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
Insoluble except nitrate and acetate
voltaic: - electrolytic: +
Salt + water

19. carbonate
Ksp = 108s5
OH?
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?)
CO3²?

20. chlorine
Greenish-yellow gas
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
H+

21. Give an example of a concentrated weak acid.
Glacial acetic acid
linear
it reacts by substitution NOT addition
strong acids/bases are written as H+ or OH- ions

22. What type of metals don't react with water or acids to form H2?

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23. What is the catalyst for this reaction Ester + ?
?G=negative - E° must be positive
?G= -ve - E°= +ve
catalyst=conc H2SO4
acid + alcohol

24. If ?S is positive - are the products more or less chaotic than the reactants?
Kc=Kp
basic
Add acid to water so that the acid doesn't boil and spit
More chaotic (ex: gases made)

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

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26. If a weak acid is diluted more - what happens to its % dissociation value?
K1 x K2
Increases.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Nothing

27. What are two substances that sublime at 1 atm when heated?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Mono; di; tri; tetra; penta; hexa.
brown volatile liquid
Iodine and CO2 (dry ice)

28. What do metal oxides plus acids form?
Salt and water
H+
Salt + water
Anode

29. What things should you remember to do when collecting gas over water?
atoms
allow for the vapor pressure of water and make sure to level levels
Q=It (time in seconds)
no - they're written undissociated (HAaq)

30. Is the freezing of ice endothermic or exothermic?
ROH
Exothermic
S2O3²?
acid + alcohol

31. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Both electrons come from the same atom (just as good as a regular bond)
RNH2
Hg²?

32. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
RCOR
Ksp = 4s³
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Kc=Kp

33. How do you get Ecell for spontaneous reactions?
redox reaction
Selective absorption
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
CnH2n+2

34. What is an Alkyl group?

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35. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Kc=Kp
P2O5
Separating funnel
Heptane

36. Name some properties of Group 17
water and substances with (s) less dense than
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
C4H10
Soluble

37. What is the second law of thermodynamics?
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
Suniverse increases for spontaneous processes
Synthetic condensation polymer (aka a polyamide)
Conjugate pair (one must be a weak base or acid)

38. What process do you use to obtain the solute from a solution?
Add acid to water so that the acid doesn't boil and spit
Ksp = 108s5
Evaporation
fractional distillation

39. chromate
strong acids/bases are written as H+ or OH- ions
CrO4²?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
ClO?

40. What reacts with an acid to create hydrogen gas?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
An active metal.
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
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

41. Generally - which oxy acid is strongest?
PO4³?
The one with most oxygen atoms (highest oxidation number)
P2O5
CrO4²?

42. Name six characteristics of transition elements (or their compounds)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
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?)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
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)

43. What is the basic structure of an optical isomer?
neutralization: high K - H2O product dissociation: low K - H2O reactant
CnH2n
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
red - green - blue

44. How are metal oxides and hydrides bonded? are they acidic or basic?
They stay the same.
metal oxides and hydrides are ionically bonded and basic
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

45. What is the energy you must put into a reaction to make it start called?
non-metal oxides and hydrides are covalently bonded and are acidic.
RCHO (carbonyl at end)
Initiation energy (NOT Ea)
Increases.

46. How are more active metals reduced?
K1 x K2
water and substances with (s) less dense than
by electrolysis
no - they're written undissociated (HAaq)

47. What do nonmetal oxides plus water form?
CnH2n+2
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.
acids
?G= -ve - E°= +ve

48. What is the name of S2Cl2? (Know how to name others like this - too)
zero
Disulfur dichloride
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Insoluble (except group 1 ammonium and Ba)

49. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
#ligands=charge x2
an oxidized and reduced substance
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

50. What do group I/II metal oxides plus water form?
Products - reactants (except for BDE when it's reactants - products)
zero-th: decreases - first: constant - second: increases
bases
C2O4²?