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. A Bronsted-Lowry acid is...
ROH
proton donor base
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Ppt will NOT form (unsaturated)

2. Why are noble gases stable?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Orange
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
0 and 14

3. What do group I/II metal oxides plus water form?
Iodine and CO2 (dry ice)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
OH- and NH3
bases

4. What is the sign of the cathode in voltaic cells? in electrolytic cells?
benzene has a delocalized pi ring structure
Increases down group 1 decreases down group 17
voltaic: + electrolytic: -
They decrease (or could be the same if the solid has ONLY JUST disappeared)

5. iodine - iodine solution - iodine vapor
CrO4²?
NH4?
ion pairing
Silvery gray solid - brown - purple

6. What is the formula for obtaining charge flowing in a cell?
hydroxides (ex: Ba(OH)2)
HClO4
Q=It (time in seconds)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

7. Does Benzene react by addition or substitution?
Evaporation
Salts (ex: CaO + SO2 ? CaSO3)
it reacts by substitution NOT addition
H3PO4

8. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
Perform ICE BOX calculation based on K1
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Concentration

9. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
A salt solution.
RCOOH
Silvery gray solid - brown - purple

10. What is the basic structure of an optical isomer?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
?G=negative - E° must be positive
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Iodine and CO2 (dry ice)

11. Name 2 ways in which you can create a buffer?
proton acceptor.
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)
Pour liquids using a funnel or down a glass rod
Soluble

12. Alcohols and _______ are FG isomers
blue (BTB)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
ethers
CrO4²?

13. What type of solutions do small - highly charged cations tend to form?
proton donor base
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
blue glass - it filters UV
Soluble

14. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Disulfur dichloride
CnH(2n+2)
water and substances with (s) less dense than
basic

15. What apparatus do you use to separate 2 immiscible liquids?
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)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Separating funnel
Pour liquids using a funnel or down a glass rod

16. What do the 'a' and 'b' in Van Der Waal's equation allow for?
|experimental - accepted|/accepted X 100
a-IMFs - b-molecular volume
CnH2n
bent

17. silver iodide
Pale yellow
ClO4?
Salts (ex: CaO + SO2 ? CaSO3)
Unsaturated - addition (ex: decolorize bromine solution)

18. How do you get Ecell for spontaneous reactions?
Iodine and CO2 (dry ice)
Insoluble (except group 1 ammonium and Ba)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Insoluble except group 1 and ammonium

19. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
Both electrons come from the same atom (just as good as a regular bond)
Perform ICE BOX calculation based on K1
ClO4?

20. ________ are Lewis bases - because they can donate a lone pair of electrons.
How close results are to the accepted value
Separating funnel
OH- and NH3
Monomer + monomer = polymer product + a simple molecule such as water or HCl

21. What is the general formula for a ketone?
Check for air bubbles in the buret and remove the buret funnel from the buret
methyl formate
Heat a test tube at an angle at the side of the tube (not bottom)
RCOR

22. What do you do to get rid of most of the solution from a precipitate?
Saturated - Substitution (which requires more radical conditions)
Most INsoluble except group 1 and ammonium
ethers
Decant

23. Both Acetic acid and ____________ are also functional isomers.
Unsaturated - addition (ex: decolorize bromine solution)
methyl formate
proton acceptor.
Making sigma bonds and holding lone pairs

24. Do anions flow to the cathode or anode?
Anode
Concentration
Purple
proton donor base

25. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Heat a test tube at an angle at the side of the tube (not bottom)
red - green - blue
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

26. 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?
C2O4²?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Mn²? - Cr³? - Cr³
The compound with the lowest Ksp value.

27. What is the slope of the graph of lnk vs. 1/T?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Ppt will NOT form (unsaturated)
Heptane
-Ea/R

28. What is the conjugate acid of H2PO4?
Iodine and CO2 (dry ice)
ethers
H3PO4
Salt and water

29. What type of compounds do metals/non metals form?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Ionic compounds
Soluble
methyl formate

30. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
Evaporation
Initiation energy (NOT Ea)
it is lower and occurs over less sharp a range

31. At what point during titration do you have the perfect buffer - and what is the pH at this point?
?G= -ve - E°= +ve
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
At half equivalence - pH=pKa
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

32. What is the formula for alkenes?
Cr2O7²?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
CnH2n
HClO4

33. How do you heat a test tube?
Pour liquids using a funnel or down a glass rod
do not change
Heat a test tube at an angle at the side of the tube (not bottom)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

34. What do acids plus active metals form?
They stay the same.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Tetrahedral
Ksp = s²

35. What process do you use to obtain a solvent from a solution?
It ceases - the circuit is broken.
red - green - blue
Distillation
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

36. What type of compounds do Group 14 form?
redox reaction
The compound with the lowest Ksp value.
+4-covalent - +2-ionic
Exothermic (?H for ANY sa/sb = -57kJ/mol)

37. Does Kw increase or decrease with T? Why?
?G=negative - E° must be positive
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
CnH2n

38. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Hg2²?
zero-th: decreases - first: constant - second: increases
P2O5

39. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
Ionic compounds
same KE - but PEice<PEwater
Hg²?

40. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
atoms
?G= -ve - E°= +ve
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Time?¹ - (ex. s?¹ - hr?¹ - etc)

41. mercury (I) ion
Hg2²?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
CnH(2n+2)
no - they're written undissociated (HAaq)

42. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
A salt solution.
hydroxides (ex: Ba(OH)2)
same KE - but PEice<PEwater
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

43. thiosulfate
no - they're written undissociated (HAaq)
S2O3²?
Eudiometer
Group I metals (soft metals) are stored under oil

44. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Greenish-yellow gas
water and substances with (s) less dense than
Sigma bonds are stronger than pi bonds
Acid rain - dissolves marble buildings/statues and kills trees.

45. chlorite
ion pairing
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.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ClO2?

46. What does the solubility of organic compounds depend on?
fruit - fish - bases
Group 1 hydroxides (ex: NaOH)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

47. What kind of bonding structure does benzene have?
Salt + water.
Hg²?
benzene has a delocalized pi ring structure
?G= -ve - E°= +ve

48. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
ROR
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
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)

49. Esters smell like _______ and amines smell like _______ and are ______.
Purple
fruit - fish - bases
Acids; HCOOCH3 is an ester
Heat a test tube at an angle at the side of the tube (not bottom)

50. bromine
brown volatile liquid
Glacial acetic acid
Orange
CO2 and H2O