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AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
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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. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
redox reaction
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
water and substances with (s) less dense than
0 and 14

2. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
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.
proton donor base
Eudiometer

3. If Q > Ksp - then system shifts _______ and ppt ______
No - NH3 and HCl gases are extremely soluble
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Salts (ex: CaO + SO2 ? CaSO3)
left - ppt will form

4. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
zero-th: decreases - first: constant - second: increases
Nothing
Pale purple - (orange)-yellow - red - blue - green.
linear

5. If a free element is involved - what type of reaction must be involved?
redox reaction
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
H2O + CO2 (it decomposes readily)
NO3?

6. What do group I/II metal oxides plus water form?
bases
White precipitate
Anode - oxygen. Cathode - hydrogen
?G=negative - E° must be positive

7. Ca - Sr - Ba
hydroxides (ex: Ba(OH)2)
Products - reactants (except for BDE when it's reactants - products)
Check for air bubbles in the buret and remove the buret funnel from the buret
Salt and water

8. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
They stay the same.
Cr2O7²?
ROH

9. What equipment do you need for a titration?
Tetrahedral
Experimental mass/theoretical mass X 100
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
More chaotic (ex: gases made)

10. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Glacial acetic acid
CH3COO?
K2
Reduction always takes place at the cathode (RED CAT) In both types of cell!

11. Name six characteristics of transition elements (or their compounds)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Q=It (time in seconds)
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)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

12. What are two substances that sublime at 1 atm when heated?
Ionic compounds
do not change
Iodine and CO2 (dry ice)
boiling without losing volatile solvents/reactants

13. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Exothermic
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
neutralization: high K - H2O product dissociation: low K - H2O reactant
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

14. Give an example of a dilute strong acid.
Soluble
HClO4
Most INsoluble except group 1 and ammonium
E=q + w (negative is by system - positive is on system)

15. What type of compounds do Group 14 form?
Check for air bubbles in the buret and remove the buret funnel from the buret
Heat a test tube at an angle at the side of the tube (not bottom)
+4-covalent - +2-ionic
OH- and NH3

16. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Synthetic condensation polymer (aka a polyamide)
Mono; di; tri; tetra; penta; hexa.
Concentration
Mn²? - Cr³? - Cr³

17. What is H2CO3 (carbonate acid) usually written as?
Salt and water
CO (poisonous)
H2O + CO2 (it decomposes readily)
are less dense than water

18. carbonates
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Ionic compounds
Insoluble (except group 1 ammonium and Ba)
Insoluble except group 1 and ammonium

19. What are two allotropes of carbon?
proton donor base
Mn²? - Cr³? - Cr³
small size and high charge
diamond and graphite

20. What are the prefixes for the naming of binary molecular compound formulas (up to six)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
strong acids/bases are written as H+ or OH- ions
Mono; di; tri; tetra; penta; hexa.
Conjugate pair (one must be a weak base or acid)

21. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
Salt + water.
zero
lighted splint (positive result=pop)

22. What is the general formula for an ether?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
ROR
Increases.
by electrolysis

23. What is the general formula for an aldehyde?
Tetrahedral
?G=negative - E° must be positive
Anode
RCHO (carbonyl at end)

24. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
CH3COO?
do not change
Saturated - Substitution (which requires more radical conditions)
E=q + w (negative is by system - positive is on system)

25. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
The dilution effect when the solutions mix. M1V1 = M2V2
Soluble
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
q=mc?T q=mL (or n x ?h)

26. What is the test for hydrogen?
Ionic compounds
Acid rain - dissolves marble buildings/statues and kills trees.
lighted splint (positive result=pop)
Pipette (burette if need repetition)

27. What shape is water?
Disulfur dichloride
Most INsoluble except group 1 and ammonium
bent
Exothermic

28. What is the formula for summation?

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29. What is the general formula for an acid?
neutralization: high K - H2O product dissociation: low K - H2O reactant
RCOOH
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
an oxidized and reduced substance

30. Alkenes are ________ and react by __________
C4H10
Unsaturated - addition (ex: decolorize bromine solution)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
acids

31. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
small size and high charge
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

32. How does half life change for zero-th order - first order - and second order processes?
Suniverse increases for spontaneous processes
Sigma bonds are stronger than pi bonds
zero-th: decreases - first: constant - second: increases
methyl formate

33. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
CO2 and H2O
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
bright yellow
Synthetic condensation polymer (aka a polyamide)

34. What do metal oxides plus non- metal oxides form?
NH2?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
ns² electrons (first in-first out)
Salts (ex: CaO + SO2 ? CaSO3)

35. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
it reacts by substitution NOT addition
allow for the vapor pressure of water and make sure to level levels
RNH2
Anode - oxygen. Cathode - hydrogen

36. ammonium/ammonium compounds
Reduction always takes place at the cathode (RED CAT) In both types of cell!
P2O5
Soluble
metal oxides and hydrides are ionically bonded and basic

37. What is the general formula for an ester?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
RCOOR
Q=It (time in seconds)

38. What shape is carbon dioxide?
linear
by electrolysis
zero
10?8

39. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
#ligands=charge x2
?G=negative - E° must be positive
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
K1 x K2

40. What is the relationship in strength between sigma and pi bonds?
C2O4²?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Sigma bonds are stronger than pi bonds
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

41. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
allow for the vapor pressure of water and make sure to level levels
H2PO4?
Acid rain - dissolves marble buildings/statues and kills trees.

42. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
same KE - but PEice<PEwater
zero
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
lighted splint (positive result=pop)

43. When driving off water from a hydrate - how do you tell you're done?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
boiling without losing volatile solvents/reactants
Hg2²?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

44. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
H3PO4
Add acid to water so that the acid doesn't boil and spit
C4H10

45. What is the second law of thermodynamics?
zero
voltaic: - electrolytic: +
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Suniverse increases for spontaneous processes

46. What is a dipeptide? polypeptide? protein?
No - it depends on the number of ions produced on dissolving.
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Hg²?
PO4³?

47. What steps do organic labs consist of?
it's lower and occurs over less sharp a range
Synthesis - separation and purification of the product and its identification.
hydroxides (ex: Ba(OH)2)
bright yellow

48. dihydrogen phosphate
H2PO4?
Both electrons come from the same atom (just as good as a regular bond)
Iodine and CO2 (dry ice)
Hg2²?

49. During a titration what is present in the beaker at the equivalence point?
RX
Orange
A salt solution.
How grouped results are

50. How many ligands attach to a central ion in a complex ion?
Pipette (burette if need repetition)
#ligands=charge x2
They stay the same.
No - NH3 and HCl gases are extremely soluble