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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 range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
Pour liquids using a funnel or down a glass rod
H+
Molecules with the same molecular formulas - but different structural formulas
A) any range. b) 8-10 c) 4-6

2. How does benzene compare in reactivity to alkenes?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
benzene is less reactive than alkenes
CH3COO?
OH- and NH3

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

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

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5. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Cu3(PO4)2
Current - time and charge on ion (moles of e used in half cell reaction)
Glacial acetic acid
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

6. What is H2CO3 (carbonate acid) usually written as?
Experimental mass/theoretical mass X 100
allow for the vapor pressure of water and make sure to level levels
H2O + CO2 (it decomposes readily)
At half equivalence - pH=pKa

7. When a cell is 'flat' What is its voltage?
zero
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
allow for the vapor pressure of water and make sure to level levels
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

8. Name C7H16
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Pale purple - (orange)-yellow - red - blue - green.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Heptane

9. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
E=q + w (negative is by system - positive is on system)
Salt + water.
Sulfur

10. Does Kw increase or decrease with T? Why?
Pale yellow
no - they're written undissociated (HAaq)
Eudiometer
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

11. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
CnH2n+2
The Faraday or Faraday's constant.
Trigonal pyramidal
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

12. What are two allotropes of carbon?
Insoluble
Group 1 hydroxides (ex: NaOH)
The benzene ring (or more correctly the phenyl group - C6H5)
diamond and graphite

13. What shape is methane?
it reacts by substitution NOT addition
Tetrahedral
H2O + CO2 (it decomposes readily)
The one with most oxygen atoms (highest oxidation number)

14. Esterification is...
acid + alcohol
fractional distillation
same KE - but PEice<PEwater
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

15. 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)
Anode - oxygen. Cathode - hydrogen
Nothing
PO4³?

16. What do you do to get rid of most of the solution from a precipitate?
Initiation energy (NOT Ea)
K2
Decant
CnH2n-2

17. What reacts with an acid to create hydrogen gas?
zero
ClO?
a-IMFs - b-molecular volume
An active metal.

18. Aromatic compounds contain what?
At half equivalence - pH=pKa
Heptane
The benzene ring (or more correctly the phenyl group - C6H5)
Pour liquids using a funnel or down a glass rod

19. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
acids
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Separating funnel

20. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
Products - reactants (except for BDE when it's reactants - products)
Cr2O7²?
HClO4

21. What is the test for hydrogen?
ClO3?
lighted splint (positive result=pop)
metal oxides and hydrides are ionically bonded and basic
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

22. What apparatus do you use to pour liquids?
Pour liquids using a funnel or down a glass rod
Ppt will NOT form (unsaturated)
basic
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

23. If Q < Ksp a ppt ______
it is lower and occurs over less sharp a range
RNH2
Group 1 hydroxides (ex: NaOH)
Ppt will NOT form (unsaturated)

24. lead compounds
NH4?
Disulfur dichloride
Insoluble except nitrate and acetate
Decant

25. sulfates
Add acid to water so that the acid doesn't boil and spit
Soluble except Ag - Pb - Ca - Sr Ba)
CO (poisonous)
Filtration

26. chromate ion (soln + most solids)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
yellow
allow for the vapor pressure of water and make sure to level levels
Synthesis - separation and purification of the product and its identification.

27. Give an example of a dilute strong acid.
zero
Ionic compounds
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)
HClO4

28. What do nonmetal oxides plus water form?
Salt + water
Pale yellow
acids
?H formation of an element in standard state=0

29. thiosulfate
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
zero-th: decreases - first: constant - second: increases
Monomer + monomer = polymer product + a simple molecule such as water or HCl
S2O3²?

30. How do you identify which is oxidized or otherwise?
proton donor base
look for changes in oxidation # - the one that goes up is oxidized and is the RA
?G=negative - E° must be positive
a-IMFs - b-molecular volume

31. What type of solutions do small - highly charged cations tend to form?
Salts (ex: CaO + SO2 ? CaSO3)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
small size and high charge
Only temperature

32. What is the general formula for a ketone?
Heat a test tube at an angle at the side of the tube (not bottom)
The one with most oxygen atoms (highest oxidation number)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
RCOR

33. What are two substances that sublime at 1 atm when heated?
They stay the same.
Iodine and CO2 (dry ice)
SO4²?
K1 x K2

34. phosphate
Salt and water
a-IMFs - b-molecular volume
PO4³?
RCHO (carbonyl at end)

35. chlorine
SO4²?
Increases.
Greenish-yellow gas
White precipitate

36. What shape is water?
T increases exponentially the proportion of molecules with E > Ea
bright yellow
bent
The dilution effect when the solutions mix. M1V1 = M2V2

37. How does the melting point of a mixture compare to the MP of a pure substance?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
blue (BTB)
it is lower and occurs over less sharp a range
PO4³?

38. What is the general formula for an acid?
RCOOH
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Cr2O7²?
Conjugate pair (one must be a weak base or acid)

39. What part of a liquid do you look at to measure its volume?
Evaporation
Read the bottom of the meniscus
HClO4
ClO3?

40. What are amphoteric oxides?
Evaporation
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
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?)
Ksp = 4s³

41. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
Evaporation
Insoluble except group 1 and ammonium
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

42. ammonium
NH4?
q=mc?T q=mL (or n x ?h)
K2
RCHO (carbonyl at end)

43. What is precision?
benzene is less reactive than alkenes
Ppt will NOT form (unsaturated)
How grouped results are
bright yellow

44. What is the general formula of an alkane?
P2O5
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
?H-kJ - ?S-J - ?G-kJ
CnH(2n+2)

45. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Anode
water and substances with (s) less dense than
Heat a test tube at an angle at the side of the tube (not bottom)

46. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
C4H10
[A?]/[HA] x 100 or [BH?]/[B] x 100
Kc=Kp

47. What are the units of the first order rate constant?
allow for the vapor pressure of water and make sure to level levels
Time?¹ - (ex. s?¹ - hr?¹ - etc)
bright yellow
ns² electrons (first in-first out)

48. What does a short - sharp melting point indicate?
do not change
RCOR
Sigma bonds are stronger than pi bonds
Identity and purity (impure compounds usually have broad & low melting points)

49. Color (absorbance) is proportional to ________
Distillation
yellow
Concentration
Reduction always takes place at the cathode (RED CAT) In both types of cell!

50. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
bent
No - it depends on the number of ions produced on dissolving.
?H formation of an element in standard state=0