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. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
it's lower and occurs over less sharp a range
acids
Iodine and CO2 (dry ice)

2. What is the formula for alkynes?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
acids
CnH2n-2
a-IMFs - b-molecular volume

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

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

4. Does Benzene react by addition or substitution?
water and substances with (s) less dense than
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
it reacts by substitution NOT addition
PO4³?

5. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
water and substances with (s) less dense than
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Both electrons come from the same atom (just as good as a regular bond)
Disulfur dichloride

6. What device would you use to measure a volume of gas?
same KE - but PEice<PEwater
Eudiometer
ClO3?
O2 needs 4F/mol H2 needs 2F/mol

7. What do group I/II metal oxides plus water form?
ion pairing
bases
An active metal.
CnH(2n+2)

8. What things should you remember to do when collecting gas over water?
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)
Soluble
CnH2n+1 often designated 'R' ex C3H7 is propyl
allow for the vapor pressure of water and make sure to level levels

9. What is the general formula for alkyl halides?
RX
Mono; di; tri; tetra; penta; hexa.
?G=negative - E° must be positive
Q=It (time in seconds)

10. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
benzene has a delocalized pi ring structure
H+
Anode - oxygen. Cathode - hydrogen

11. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
Making sigma bonds and holding lone pairs
Initiation energy (NOT Ea)
-Ea/R

12. What shape is methane?
Tetrahedral
proton acceptor.
SO4²?
A) any range. b) 8-10 c) 4-6

13. What type of solutions do small - highly charged cations tend to form?
Acid rain - dissolves marble buildings/statues and kills trees.
RCHO (carbonyl at end)
R=8.31 J/mol/K
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

14. Why are i factors (Van't Hoff factors) often less than ideal?
Suniverse increases for spontaneous processes
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
ion pairing
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

15. Name six characteristics of transition elements (or their compounds)
Synthetic condensation polymer (aka a polyamide)
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)
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
Exothermic (?H for ANY sa/sb = -57kJ/mol)

16. What apparatus do you use to separate 2 immiscible liquids?
voltaic: + electrolytic: -
Suniverse increases for spontaneous processes
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Separating funnel

17. What are the names and formulas of the 6 strong acids?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Sulfur
Soluble

18. Acids + Carbonates (bicarbonates) make?
Salt and water
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Exothermic
CnH2n-2

19. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
ROR
MnO4?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
same KE - but PEice<PEwater

20. How are more active metals reduced?
zero
Tetrahedral
by electrolysis
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

21. Where are group I metals stored?
Only temperature
Group I metals (soft metals) are stored under oil
OH?
How grouped results are

22. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
RCOR
Salt + water
strong acids/bases are written as H+ or OH- ions

23. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
CnH2n
P2O5
?G= -ve - E°= +ve
|experimental - accepted|/accepted X 100

24. chlorate
ClO3?
CnH2n-2
It ceases - the circuit is broken.
CnH(2n+2)

25. How do you explain trends in atomic properties using Coulomb's Law?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
?H-kJ - ?S-J - ?G-kJ
Check for air bubbles in the buret and remove the buret funnel from the buret

26. hydroxides
same KE - but PEice<PEwater
Acidified
Insoluble (except group 1 ammonium and Ba)
bent

27. Why are i factors (Van't Hoff factors) often less than ideal?
same KE - but PEice<PEwater
Check for air bubbles in the buret and remove the buret funnel from the buret
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
ion pairing

28. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
ClO4?
Add acid to water so that the acid doesn't boil and spit
same KE - but PEice<PEwater

29. What is the third law of thermodynamics?
CN?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
S crystal at 0K=0
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

30. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Salt and water
same KE - but PEice<PEwater
Iodine and CO2 (dry ice)
No - NH3 and HCl gases are extremely soluble

31. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Kc=Kp
OH- and NH3
White precipitate
methyl formate

32. nitrate
Glowing splint (positive result=relights)
NO3?
But S° of element is not zero (except at 0K)
ionic and form hydrogen and hydroxide

33. What apparatus do you use to pour liquids?
q=mc?T q=mL (or n x ?h)
Soluble except Ag - Pb - Ca - Sr Ba)
Pour liquids using a funnel or down a glass rod
Synthesis - separation and purification of the product and its identification.

34. Give an example of a dilute strong acid.
CnH2n+1 often designated 'R' ex C3H7 is propyl
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.
CN?
HClO4

35. sulfates
Exothermic
atoms
Soluble except Ag - Pb - Ca - Sr Ba)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

36. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
Synthesis - separation and purification of the product and its identification.
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Conjugate pair (one must be a weak base or acid)

37. Nonmetals are good _____ agents. Metals are good _______ agents.
Pale purple - (orange)-yellow - red - blue - green.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Most INsoluble except group 1 and ammonium

38. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Ionic compounds
voltaic: + electrolytic: -
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
They stay the same.

39. carbonate
The one with most oxygen atoms (highest oxidation number)
C4H10
CO3²?
RCOOR

40. What type of compounds do Group 14 form?
allow for the vapor pressure of water and make sure to level levels
Nothing
same KE - but PEice<PEwater
+4-covalent - +2-ionic

41. barium sulfate
Reduction always takes place at the cathode (RED CAT) In both types of cell!
fractional distillation
White precipitate
fruit - fish - bases

42. What two compounds are great oxidizing agents?

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

43. Esters smell like _______ and amines smell like _______ and are ______.
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
CnH2n
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
fruit - fish - bases

44. Esterification is...
Disulfur dichloride
ClO3?
acid + alcohol
The dilution effect when the solutions mix. M1V1 = M2V2

45. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
All except for lithium
Salt + water
A) any range. b) 8-10 c) 4-6
The dilution effect when the solutions mix. M1V1 = M2V2

46. mercury (II) ion
Hg²?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
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
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

47. How many ligands attach to a central ion in a complex ion?
blue (BTB)
#ligands=charge x2
T increases exponentially the proportion of molecules with E > Ea
OH- and NH3

48. iodine - iodine solution - iodine vapor
a-IMFs - b-molecular volume
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.
The benzene ring (or more correctly the phenyl group - C6H5)
Silvery gray solid - brown - purple

49. What should you check for before you begin titrating?
K2
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Check for air bubbles in the buret and remove the buret funnel from the buret
Heptane

50. What are two allotropes of carbon?
Anode - oxygen. Cathode - hydrogen
diamond and graphite
Concentration
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]