Test your basic knowledge |

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?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
same KE - but PEice<PEwater
Anode - oxygen. Cathode - hydrogen
Distillation

2. mercury (I) ion
boiling without losing volatile solvents/reactants
Hg2²?
allow for the vapor pressure of water and make sure to level levels
C4H10

3. What type of compounds do metals/non metals form?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Ionic compounds
Acid rain - dissolves marble buildings/statues and kills trees.
Experimental mass/theoretical mass X 100

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

5. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Acid rain - dissolves marble buildings/statues and kills trees.
Molecules with the same molecular formulas - but different structural formulas
'non-active' metals such as Cu - Ag - Au - Pt - etc.

6. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
diamond and graphite
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Trigonal pyramidal

7. What is the basic structure of an optical isomer?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
The benzene ring (or more correctly the phenyl group - C6H5)
A) any range. b) 8-10 c) 4-6
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

8. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
q=mc?T q=mL (or n x ?h)
ethers
Reduction always takes place at the cathode (RED CAT) In both types of cell!
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

9. chlorite
Nothing
Synthesis - separation and purification of the product and its identification.
ClO2?
CnH2n+1 often designated 'R' ex C3H7 is propyl

10. primary colors
White precipitate
Only temperature
red - green - blue
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

11. When the salt bridge is removed what happens to the cell reaction?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
yellow
linear
It ceases - the circuit is broken.

12. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
redox reaction
The benzene ring (or more correctly the phenyl group - C6H5)
Salts (ex: CaO + SO2 ? CaSO3)
basic

13. What kind of bonding structure does benzene have?
[A?]/[HA] x 100 or [BH?]/[B] x 100
benzene has a delocalized pi ring structure
RCHO (carbonyl at end)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

15. hydroxide
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Experimental mass/theoretical mass X 100
a-IMFs - b-molecular volume
OH?

16. How do you identify which is oxidized or otherwise?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
CO2 and H2O
look for changes in oxidation # - the one that goes up is oxidized and is the RA
An active metal.

17. What two types of substances are present in all redox reactions?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
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?)
an oxidized and reduced substance
Suniverse increases for spontaneous processes

18. acetate
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
?G= -ve - E°= +ve
Exothermic
CH3COO?

19. nitrate
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
allow for the vapor pressure of water and make sure to level levels
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)
NO3?

20. Why are i factors (Van't Hoff factors) often less than ideal?
q=mc?T q=mL (or n x ?h)
Soluble
ion pairing
non-metal oxides and hydrides are covalently bonded and are acidic.

21. What is the general formula for an ester?
catalyst=conc H2SO4
ethers
different forms of the same element
RCOOR

22. Color is due to ______ _______ of light.
Selective absorption
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?)
Cu3(PO4)2
Soluble

23. What do hydrocarbons form when they burn in air (oxygen)?
RX
MnO4?
CO2 and H2O
How close results are to the accepted value

24. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Heptane
Add acid to water so that the acid doesn't boil and spit
?G=negative - E° must be positive

25. lead iodide
0 and 14
Iodine and CO2 (dry ice)
Big K=kf/kr
bright yellow

26. chlorine
Greenish-yellow gas
CO2 and H2O
SO4²?
Read the bottom of the meniscus

27. How are more active metals reduced?
by electrolysis
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
But S° of element is not zero (except at 0K)
Insoluble (except group 1 ammonium and Ba)

28. dihydrogen phosphate
H2PO4?
Greenish-yellow gas
bright yellow
brown volatile liquid

29. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
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.
T increases exponentially the proportion of molecules with E > Ea
blue (BTB)

30. Does Kw increase or decrease with T? Why?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
different forms of the same element
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

31. Metal hydrides are _____ and form _______ and _______ when added to water
Insoluble except group 1 and ammonium
HClO4
ionic and form hydrogen and hydroxide
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)

32. acetates
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Unsaturated - addition (ex: decolorize bromine solution)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Soluble

33. barium sulfate
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
linear
ClO2?
White precipitate

34. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
boiling without losing volatile solvents/reactants
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)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

35. If a free element is involved - what type of reaction must be involved?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
redox reaction
Nothing
H2O + CO2 (it decomposes readily)

36. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
CnH2n
hydroxides (ex: Ba(OH)2)
zero
Unsaturated - addition (ex: decolorize bromine solution)

37. What does the solubility of organic compounds depend on?
Nothing
red - green - blue
by electrolysis
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

38. What element is used to vulcanize rubber?
Sulfur
Insoluble except nitrate and acetate
Tetrahedral
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

39. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Perform ICE BOX calculation based on K1
Insoluble except nitrate and acetate

40. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
CnH2n+2
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
The Faraday or Faraday's constant.

41. Both Acetic acid and ____________ are also functional isomers.
methyl formate
It ceases - the circuit is broken.
ClO3?
Read the bottom of the meniscus

42. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

43. What is a coordinate covalent bond?
Decant
Both electrons come from the same atom (just as good as a regular bond)
Big K=kf/kr
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?)

44. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Salt + water
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

46. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
CnH2n+1 often designated 'R' ex C3H7 is propyl
Concentration
The benzene ring (or more correctly the phenyl group - C6H5)

47. cyanide
Increases.
RNH2
CN?
Identity and purity (impure compounds usually have broad & low melting points)

48. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
diamond and graphite
Add acid to water so that the acid doesn't boil and spit
Making sigma bonds and holding lone pairs

49. What is HCOOCH3?
Big K=kf/kr
ion pairing
Acids; HCOOCH3 is an ester
OH- and NH3

50. Name C7H16
RCHO (carbonyl at end)
C2O4²?
Heptane
NH2?