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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 precipitate from a solution?
Insoluble (except group 1 ammonium and Ba)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Filtration
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

2. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
?G=negative - E° must be positive
Iodine and CO2 (dry ice)
|experimental - accepted|/accepted X 100
water and substances with (s) less dense than

3. What is the general formula for a ketone?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
diamond and graphite
RCOR
Decant

4. What are two allotropes of carbon?
P2O5
diamond and graphite
Hg²?
blue (BTB)

5. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
HClO4
ROR
T increases exponentially the proportion of molecules with E > Ea

6. How are more active metals reduced?
Hg²?
by electrolysis
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Iodine and CO2 (dry ice)

7. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
a-IMFs - b-molecular volume
it is lower and occurs over less sharp a range
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

8. What shape is water?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Big K=kf/kr
Current - time and charge on ion (moles of e used in half cell reaction)
bent

9. Ca - Sr - Ba
Most are soluble except Ag - Pb
hydroxides (ex: Ba(OH)2)
Concentration
acid + alcohol

10. mercury (II) ion
Molecules with the same molecular formulas - but different structural formulas
Glacial acetic acid
Hg²?
yellow

11. Esters smell like _______ and amines smell like _______ and are ______.
They stay the same.
fruit - fish - bases
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Selective absorption

12. How do you get the equation for a net electrolysis reaction?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Ksp = s²
Combine the equations for the half reactions in the non-spontaneous direction
neutralization: high K - H2O product dissociation: low K - H2O reactant

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

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14. dichromate
Pale yellow
S crystal at 0K=0
Cr2O7²?
#ligands=charge x2

15. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
do not change
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Anode - oxygen. Cathode - hydrogen
The one with most oxygen atoms (highest oxidation number)

16. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
water and substances with (s) less dense than
Kc=Kp
Acids; HCOOCH3 is an ester
basic

17. At what point during titration do you have the perfect buffer - and what is the pH at this point?
zero
fractional distillation
At half equivalence - pH=pKa
small size and high charge

18. If Q < Ksp a ppt ______
H3PO4
Ppt will NOT form (unsaturated)
Insoluble except group 1 and ammonium
Sulfur

19. What is the energy you must put into a reaction to make it start called?
The dilution effect when the solutions mix. M1V1 = M2V2
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
The compound with the lowest Ksp value.
Initiation energy (NOT Ea)

20. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
0.10M HCl (more ions)
The compound with the lowest Ksp value.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Big K=kf/kr

21. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
?G=negative - E° must be positive
strong acids/bases are written as H+ or OH- ions
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)

22. iodine - iodine solution - iodine vapor
ion pairing
Hg2²?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Silvery gray solid - brown - purple

23. Alkanes are _________ and react by _________
Ksp = 108s5
Saturated - Substitution (which requires more radical conditions)
no - they're written undissociated (HAaq)
An active metal.

24. How do you dilute an acid?

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25. Esterification is...
acid + alcohol
?H formation of an element in standard state=0
Eudiometer
Ions go through the salt bridge - electrons go through metal wires in the external circuit

26. chlorine
C2O4²?
Greenish-yellow gas
by electrolysis
Pipette (burette if need repetition)

27. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
blue (BTB)
ion pairing
Monomer + monomer = polymer product + a simple molecule such as water or HCl

28. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
CnH2n+2
Pipette (burette if need repetition)
RCHO (carbonyl at end)

29. What are two substances that sublime at 1 atm when heated?
Insoluble (except group 1 ammonium and Ba)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Soluble except Ag - Pb - Ca - Sr Ba)
Iodine and CO2 (dry ice)

30. What device would you use to measure a volume of gas?
No - it depends on the number of ions produced on dissolving.
Tetrahedral
Eudiometer
H2O + CO2 (it decomposes readily)

31. dichromate (soln + most solids)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Pale purple - (orange)-yellow - red - blue - green.
Orange
E=q + w (negative is by system - positive is on system)

32. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
water and substances with (s) less dense than
neutralization: high K - H2O product dissociation: low K - H2O reactant
0 and 14
Pour liquids using a funnel or down a glass rod

33. How does group 1 metals' density compare to water's?
Insoluble
are less dense than water
fractional distillation
Synthetic condensation polymer (aka a polyamide)

34. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Acidified
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
OH?
Salt + water.

35. Nonmetals are good _____ agents. Metals are good _______ agents.
Group 1 hydroxides (ex: NaOH)
Conjugate pair (one must be a weak base or acid)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

36. Color is due to ______ _______ of light.
Selective absorption
H2O + CO2 (it decomposes readily)
ethers
Insoluble except nitrate and acetate

37. What is the difference between equivalence point and end point of a titration.
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
They stay the same.
Selective absorption
zero-th: decreases - first: constant - second: increases

38. What is the first law of thermodynamics?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
E=q + w (negative is by system - positive is on system)
Clear
MnO4?

39. What is the formula of copper (II) phosphate?
water and substances with (s) less dense than
Cu3(PO4)2
Mn²? - Cr³? - Cr³
Ksp = s²

40. Ions are not ______.
atoms
yellow
H2O + CO2 (it decomposes readily)
RCHO (carbonyl at end)

41. What measuring device would you use for very small volumes of liquids?
atoms
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Pipette (burette if need repetition)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

42. What is the conjugate acid of H2PO4?
brown volatile liquid
H3PO4
Salt + water.
Only temperature

43. What type of compounds do metals/non metals form?
Ionic compounds
Distillation
acid + alcohol
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

44. A Bronsted-Lowry base is...
?H formation of an element in standard state=0
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
red - green - blue
proton acceptor.

45. If a free element is involved - what type of reaction must be involved?
Big K=kf/kr
#ligands=charge x2
redox reaction
No - it depends on the number of ions produced on dissolving.

46. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
chemically (ex: with carbon)
SO4²?
P2O5

47. What are the units of the first order rate constant?
water and substances with (s) less dense than
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.
Sigma bonds are stronger than pi bonds
Time?¹ - (ex. s?¹ - hr?¹ - etc)

48. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
brown volatile liquid
Increases.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
ethers

49. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
Molecules with the same molecular formulas - but different structural formulas
hydroxides (ex: Ba(OH)2)
voltaic: + electrolytic: -

50. What do metal oxides plus acids form?
Ksp = 4s³
It ceases - the circuit is broken.
fractional distillation
Salt + water