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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 process do you use to obtain the solute from a solution?
Greenish-yellow gas
The dilution effect when the solutions mix. M1V1 = M2V2
The one with most oxygen atoms (highest oxidation number)
Evaporation

2. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
More chaotic (ex: gases made)
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.
Evaporation

3. Which alkali metals float on water?
H+
10?8
CH3COO?
All except for lithium

4. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
P2O5
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
H+
Insoluble (except group 1 ammonium and Ba)

5. If ?S is positive - are the products more or less chaotic than the reactants?
P2O5
Disulfur dichloride
Salts (ex: CaO + SO2 ? CaSO3)
More chaotic (ex: gases made)

6. sulfate
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
SO4²?
RCOOR

7. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
yellow
+4-covalent - +2-ionic
[A?]/[HA] x 100 or [BH?]/[B] x 100

8. Ions are not ______.
atoms
Acidified
red - green - blue
same KE - but PEice<PEwater

9. What do you do to get rid of most of the solution from a precipitate?
left - ppt will form
All except for lithium
Decant
boiling without losing volatile solvents/reactants

10. What is the formula for alkanes?
acids
CnH2n+2
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)
metal oxides and hydrides are ionically bonded and basic

11. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
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
voltaic: - electrolytic: +
q=mc?T q=mL (or n x ?h)

12. mercury (I) ion
CnH2n+2
A) any range. b) 8-10 c) 4-6
Hg2²?
The Faraday or Faraday's constant.

13. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Conjugate pair (one must be a weak base or acid)
Separating funnel
metal oxides and hydrides are ionically bonded and basic

14. What are the prefixes for the naming of binary molecular compound formulas (up to six)
left - ppt will form
At half equivalence - pH=pKa
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Mono; di; tri; tetra; penta; hexa.

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

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16. What is the conjugate base of NH3?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
NH2?
RCHO (carbonyl at end)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

17. When can supercooling occur? What does it look like on a cooling curve?

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

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19. How are metal oxides and hydrides bonded? are they acidic or basic?
White precipitate
Silvery gray solid - brown - purple
S crystal at 0K=0
metal oxides and hydrides are ionically bonded and basic

20. What should you check for before you begin titrating?
zero-th: decreases - first: constant - second: increases
Check for air bubbles in the buret and remove the buret funnel from the buret
Monomer + monomer = polymer product + a simple molecule such as water or HCl
RCOOH

21. Esterification is...
HClO4
Add acid to water so that the acid doesn't boil and spit
acid + alcohol
water and substances with (s) less dense than

22. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
diamond and graphite
non-metal oxides and hydrides are covalently bonded and are acidic.
CO2 and H2O

23. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
NO3?
Increases down group 1 decreases down group 17
Unsaturated - addition (ex: decolorize bromine solution)

24. What is the formula for percent error?
|experimental - accepted|/accepted X 100
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)
0 and 14
Decant

25. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Soluble
Sigma bonds are stronger than pi bonds
K2

26. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Transition element compounds (except if it has a full or empty d shell)
E=q + w (negative is by system - positive is on system)
Insoluble except group 1 and ammonium

27. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Products - reactants (except for BDE when it's reactants - products)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Soluble
q=mc?T q=mL (or n x ?h)

28. Give an example of a dilute strong acid.
Silvery gray solid - brown - purple
PO4³?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
HClO4

29. hydroxides
Insoluble (except group 1 ammonium and Ba)
metal oxides and hydrides are ionically bonded and basic
Both electrons come from the same atom (just as good as a regular bond)
Eudiometer

30. How many faradays of electric charge do you need to produce one mole of O2? H2?
methyl formate
It ceases - the circuit is broken.
strong acids/bases are written as H+ or OH- ions
O2 needs 4F/mol H2 needs 2F/mol

31. What shape is methane?
Anode - oxygen. Cathode - hydrogen
K2
CO2 and H2O
Tetrahedral

32. How are primary alcohols turned into acids?
catalyst=conc H2SO4
ClO3?
Big K=kf/kr
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

33. A Bronsted-Lowry base is...
Ksp = 108s5
Soluble
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
proton acceptor.

34. What do metal oxides plus non- metal oxides form?
water and substances with (s) less dense than
voltaic: - electrolytic: +
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Salts (ex: CaO + SO2 ? CaSO3)

35. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Soluble
do not change
a-IMFs - b-molecular volume
CO3²?

36. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
Soluble
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Iodine and CO2 (dry ice)

37. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
CH3COO?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

38. ammonium/ammonium compounds
proton acceptor.
Soluble
zero
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

39. What shape is ammonia?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CnH2n-2
Pale yellow
Trigonal pyramidal

40. silver compounds
OH- and NH3
Insoluble except for nitrate and acetate
0.10M HCl (more ions)
Insoluble except group 1 and ammonium

41. What is the formula for percent yield?
ethers
Ionic compounds
Experimental mass/theoretical mass X 100
Orange

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

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43. For a dibasic acid (H2A) - [A²?]= ____ ?
Insoluble except group 1 and ammonium
ethers
K2
Ksp = 4s³

44. halides
At half equivalence - pH=pKa
Most are soluble except Ag - Pb
OH- and NH3
non-metal oxides and hydrides are covalently bonded and are acidic.

45. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
CO2 and H2O
Tetrahedral
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

46. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
K1 x K2
redox reaction
same KE - but PEice<PEwater

47. acetates
Soluble
CN?
ion pairing
it's lower and occurs over less sharp a range

48. hydroxide
Clear
OH?
Trigonal pyramidal
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

49. What shape is carbon dioxide?
redox reaction
linear
Big K=kf/kr
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

50. What is the third law of thermodynamics?
Distillation
Acid rain - dissolves marble buildings/statues and kills trees.
CN?
S crystal at 0K=0