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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. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
strong acids/bases are written as H+ or OH- ions
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
same KE - but PEice<PEwater
CO (poisonous)

2. Which alkali metals float on water?
left - ppt will form
E=q + w (negative is by system - positive is on system)
A salt solution.
All except for lithium

3. What is the second law of thermodynamics?
Suniverse increases for spontaneous processes
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
hydroxides (ex: Ba(OH)2)
H+

4. How do you heat a test tube?
The Faraday or Faraday's constant.
Suniverse increases for spontaneous processes
Selective absorption
Heat a test tube at an angle at the side of the tube (not bottom)

5. What shape is methane?
Filtration
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Tetrahedral
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

6. What is the difference between equivalence point and end point of a titration.
look for changes in oxidation # - the one that goes up is oxidized and is the RA
C2O4²?
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
it is lower and occurs over less sharp a range

7. What does a short - sharp melting point indicate?
The dilution effect when the solutions mix. M1V1 = M2V2
Identity and purity (impure compounds usually have broad & low melting points)
Nothing
ClO2?

8. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
ionic and form hydrogen and hydroxide
Initiation energy (NOT Ea)
strong acids/bases are written as H+ or OH- ions
zero

9. What should you check for before you begin titrating?
Glowing splint (positive result=relights)
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
CnH2n+1 often designated 'R' ex C3H7 is propyl
Check for air bubbles in the buret and remove the buret funnel from the buret

10. What is the general formula for an alcohol?
ROH
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
basic
acids

11. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
T increases exponentially the proportion of molecules with E > Ea
Most are soluble except Ag - Pb
same KE - but PEice<PEwater
Anode - oxygen. Cathode - hydrogen

12. Lattice energy is high for ions with _____ size and _____ charge
ion pairing
How grouped results are
small size and high charge
an oxidized and reduced substance

13. How do you get Ecell for spontaneous reactions?
MnO4?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Pour liquids using a funnel or down a glass rod
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

14. hydroxide
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Making sigma bonds and holding lone pairs
Graduated cylinder
OH?

15. Give an example of a dilute strong acid.
C2O4²?
hydroxides (ex: Ba(OH)2)
HClO4
Pale purple - (orange)-yellow - red - blue - green.

16. hypochlorite
Hg²?
RCHO (carbonyl at end)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
ClO?

17. phosphates
chemically (ex: with carbon)
an oxidized and reduced substance
Ksp = 27s4
Most INsoluble except group 1 and ammonium

18. halides
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)
Acidified
CnH2n-2
Most are soluble except Ag - Pb

19. How does half life change for zero-th order - first order - and second order processes?
Only temperature
zero-th: decreases - first: constant - second: increases
metal oxides and hydrides are ionically bonded and basic
non-metal oxides and hydrides are covalently bonded and are acidic.

20. phosphate
fractional distillation
it reacts by substitution NOT addition
PO4³?
Monomer + monomer = polymer product + a simple molecule such as water or HCl

21. Does Benzene react by addition or substitution?
Trigonal pyramidal
it reacts by substitution NOT addition
Insoluble except for nitrate and acetate
Purple

22. Which of the rates changes more when temperature is increased?
CH3COO?
A) any range. b) 8-10 c) 4-6
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

23. What is the formula for obtaining charge flowing in a cell?
Filtration
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.
Q=It (time in seconds)
Insoluble

24. Give an example of a concentrated weak acid.
Ksp = 27s4
Glacial acetic acid
same KE - but PEice<PEwater
fractional distillation

25. cyanide
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Clear
RCOOH
CN?

26. ammonium
CrO4²?
Soluble
NH4?
+4-covalent - +2-ionic

27. Do anions flow to the cathode or anode?
Anode
ClO2?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Sulfur

28. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
OH?
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)
Insoluble
10?8

29. dichromate
?H formation of an element in standard state=0
acids
Insoluble (except group 1 ammonium and Ba)
Cr2O7²?

30. How do you dilute an acid?

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31. lead iodide
bright yellow
Acids; HCOOCH3 is an ester
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
H2O + CO2 (it decomposes readily)

32. How are metal oxides and hydrides bonded? are they acidic or basic?
CnH(2n+2)
metal oxides and hydrides are ionically bonded and basic
ROR
'non-active' metals such as Cu - Ag - Au - Pt - etc.

33. What is the first law of thermodynamics?
hydroxides (ex: Ba(OH)2)
Kc=Kp
Insoluble except group 1 and ammonium
E=q + w (negative is by system - positive is on system)

34. A geometric (or cis-trans) isomer exists due to.....
ROH
Glowing splint (positive result=relights)
allow for the vapor pressure of water and make sure to level levels
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

35. potassium permanganate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Purple
methyl formate
bases

36. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
E=q + w (negative is by system - positive is on system)
No - NH3 and HCl gases are extremely soluble
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

37. What are the common strong bases?
Salt and water
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
The benzene ring (or more correctly the phenyl group - C6H5)
Group 1 hydroxides (ex: NaOH)

38. mercury (II) ion
Hg²?
voltaic: - electrolytic: +
Perform ICE BOX calculation based on K1
Making sigma bonds and holding lone pairs

39. What process do you use to obtain the solute from a solution?
H2O + CO2 (it decomposes readily)
Evaporation
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

40. Color is due to ______ _______ of light.
Selective absorption
ROH
The one with most oxygen atoms (highest oxidation number)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

41. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Cu3(PO4)2
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Increases.
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)

42. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
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)
redox reaction
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

43. Acid plus base make?
bases
Salt + water.
zero
0 and 14

44. silver compounds
Hg2²?
Selective absorption
Add acid to water so that the acid doesn't boil and spit
Insoluble except for nitrate and acetate

45. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
SO4²?
No - it depends on the number of ions produced on dissolving.
H3PO4
no - they're written undissociated (HAaq)

46. Metal hydrides are _____ and form _______ and _______ when added to water
RCHO (carbonyl at end)
ionic and form hydrogen and hydroxide
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
H2O + CO2 (it decomposes readily)

47. What value of R do you use for thermo calculations? gas calculations?
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.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Soluble
Synthesis - separation and purification of the product and its identification.

48. What are isotopes?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
OH?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Making sigma bonds and holding lone pairs

49. What is the relationship in strength between sigma and pi bonds?
CH3COO?
Sigma bonds are stronger than pi bonds
Pour liquids using a funnel or down a glass rod
How close results are to the accepted value

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

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