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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. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Insoluble (except group 1 ammonium and Ba)
Selective absorption
water and substances with (s) less dense than
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

2. What should you check for before you begin titrating?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Ksp = 108s5
Check for air bubbles in the buret and remove the buret funnel from the buret
Decant

3. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
bent
Anode - oxygen. Cathode - hydrogen
How grouped results are
CnH2n+2

4. What shape is carbon dioxide?
It ceases - the circuit is broken.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Greenish-yellow gas
linear

5. What is the conjugate base of NH3?
proton acceptor.
An active metal.
zero-th: decreases - first: constant - second: increases
NH2?

6. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Perform ICE BOX calculation based on K1
a-IMFs - b-molecular volume
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Group I metals (soft metals) are stored under oil

7. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
do not change
How close results are to the accepted value
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
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)

8. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Ksp = s²
ROR
Heat a test tube at an angle at the side of the tube (not bottom)

9. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
-Ea/R
Pour liquids using a funnel or down a glass rod

10. If Q < Ksp a ppt ______
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)
Silvery gray solid - brown - purple
CH3COO?
Ppt will NOT form (unsaturated)

11. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
ClO?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
K1 x K2
The benzene ring (or more correctly the phenyl group - C6H5)

12. Neutralization is an ________ reaction.
The benzene ring (or more correctly the phenyl group - C6H5)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
PO4³?
different forms of the same element

13. dichromate
Cr2O7²?
no - they're written undissociated (HAaq)
bent
it is lower and occurs over less sharp a range

14. A Bronsted-Lowry acid is...
ClO4?
Sigma bonds are stronger than pi bonds
Molecules with the same molecular formulas - but different structural formulas
proton donor base

15. What is the test for oxygen?
S crystal at 0K=0
Increases.
Glowing splint (positive result=relights)
?H formation of an element in standard state=0

16. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
Trigonal pyramidal
Acidified
voltaic: - electrolytic: +

17. What reacts with an acid to create hydrogen gas?
An active metal.
yellow
Ksp = 4s³
+4-covalent - +2-ionic

18. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
A) any range. b) 8-10 c) 4-6
Acid rain - dissolves marble buildings/statues and kills trees.
same KE - but PEice<PEwater
Separating funnel

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

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20. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
NH2?
+4-covalent - +2-ionic
Experimental mass/theoretical mass X 100

21. What is Big K in terms of kf and kr?
-Ea/R
RCOR
Big K=kf/kr
Insoluble except for nitrate and acetate

22. Acids + Carbonates (bicarbonates) make?
Insoluble
do not change
Clear
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

23. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
bright yellow
Orange

24. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
do not change
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CO (poisonous)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

25. Are weak acids (and bases) written dissociated?

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26. group 1 ions/compounds
Ppt will NOT form (unsaturated)
Conjugate pair (one must be a weak base or acid)
CnH2n
Soluble

27. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

28. What is the formula for percent yield?
basic
Experimental mass/theoretical mass X 100
do not change
But S° of element is not zero (except at 0K)

29. Buffer capacity must contain decent amounts of a ________ ________
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Conjugate pair (one must be a weak base or acid)
no - they're written undissociated (HAaq)

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

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31. primary colors
Pale purple - (orange)-yellow - red - blue - green.
Orange
red - green - blue
No - it depends on the number of ions produced on dissolving.

32. chlorite
Acids; HCOOCH3 is an ester
are less dense than water
Salt and water
ClO2?

33. What is the sign of the anode in voltaic cells? in electrolytic cells?
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
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
voltaic: - electrolytic: +
Salt + water.

34. sulfate
OH?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
acids
SO4²?

35. silver iodide
Pale yellow
Mono; di; tri; tetra; penta; hexa.
red - green - blue
An active metal.

36. What is the general formula for an aldehyde?
T increases exponentially the proportion of molecules with E > Ea
Insoluble except nitrate and acetate
RCHO (carbonyl at end)
Soluble

37. Name six characteristics of transition elements (or their compounds)
?G=negative - E° must be positive
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)
Clear
Most are soluble except Ag - Pb

38. hypochlorite
do not change
Group 1 hydroxides (ex: NaOH)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
ClO?

39. How do you compute % dissociation?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
[A?]/[HA] x 100 or [BH?]/[B] x 100
ROR
zero

40. What two compounds are great oxidizing agents?

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41. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
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
Check for air bubbles in the buret and remove the buret funnel from the buret
red - green - blue

42. What is the word equation for addition polymerisation?
They stay the same.
Kc=Kp
Check for air bubbles in the buret and remove the buret funnel from the buret
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

43. Color is due to ______ _______ of light.
Filtration
Selective absorption
chemically (ex: with carbon)
bent

44. lead iodide
Insoluble except for nitrate and acetate
bright yellow
catalyst=conc H2SO4
The compound with the lowest Ksp value.

45. What is the formula for percent error?
CO2 and H2O
|experimental - accepted|/accepted X 100
Soluble
are less dense than water

46. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
catalyst=conc H2SO4
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
H+
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

47. chlorate
ClO3?
Disulfur dichloride
RCOOR
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

48. ammonium/ammonium compounds
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?)
ionic and form hydrogen and hydroxide
More chaotic (ex: gases made)
Soluble

49. Acid plus base make?
ns² electrons (first in-first out)
basic
Ksp = 108s5
Salt + water.

50. permanganate
hydroxides (ex: Ba(OH)2)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
MnO4?
S crystal at 0K=0