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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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 happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
a-IMFs - b-molecular volume
ClO2?
They decrease (or could be the same if the solid has ONLY JUST disappeared)

2. What is Big K in terms of kf and kr?
ionic and form hydrogen and hydroxide
Big K=kf/kr
RCHO (carbonyl at end)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

3. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
fruit - fish - bases
Acids; HCOOCH3 is an ester
Synthetic condensation polymer (aka a polyamide)

4. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Purple
Anode - oxygen. Cathode - hydrogen
Current - time and charge on ion (moles of e used in half cell reaction)
Making sigma bonds and holding lone pairs

5. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
Soluble
Glowing splint (positive result=relights)
CnH2n

6. carbonates
allow for the vapor pressure of water and make sure to level levels
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Insoluble except group 1 and ammonium
Insoluble (except group 1 ammonium and Ba)

7. The oxidation # for acid base reactions...
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.
fractional distillation
do not change
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

8. Aromatic compounds contain what?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
ion pairing
The benzene ring (or more correctly the phenyl group - C6H5)
different forms of the same element

9. Can you collect soluble gases over water?
same KE - but PEice<PEwater
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
No - NH3 and HCl gases are extremely soluble
it reacts by substitution NOT addition

10. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
are less dense than water
Clear
same KE - but PEice<PEwater
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

11. 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?
No - it depends on the number of ions produced on dissolving.
CnH2n+2
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
NO3?

12. Which of the rates changes more when temperature is increased?
yellow
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
How close results are to the accepted value
Ppt will NOT form (unsaturated)

13. At what point during titration do you have the perfect buffer - and what is the pH at this point?
?G= -ve - E°= +ve
benzene is less reactive than alkenes
At half equivalence - pH=pKa
Iodine and CO2 (dry ice)

14. How does the melting point of a mixture compare to the MP of a pure substance?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
CnH2n+1 often designated 'R' ex C3H7 is propyl
it is lower and occurs over less sharp a range
White precipitate

15. BaSO4
ClO2?
Insoluble except group 1 and ammonium
it is lower and occurs over less sharp a range
Insoluble

16. Colorless doesn't mean ______
Most INsoluble except group 1 and ammonium
Clear
it is lower and occurs over less sharp a range
S crystal at 0K=0

17. How does benzene compare in reactivity to alkenes?
How close results are to the accepted value
benzene is less reactive than alkenes
?H formation of an element in standard state=0
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

18. What is the energy you must put into a reaction to make it start called?
Pipette (burette if need repetition)
ethers
Initiation energy (NOT Ea)
Big K=kf/kr

19. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
R=8.31 J/mol/K
K2
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

20. What equipment do you need for a titration?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
acids
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

21. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
H+
Ionic compounds
PO4³?

22. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
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
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Most are soluble except Ag - Pb
CO3²?

23. What shape is ammonia?
Trigonal pyramidal
SO4²?
OH- and NH3
blue

24. The definition of acidic basic and neutral aqueous solutions is:
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
fruit - fish - bases

25. A Bronsted-Lowry base is...
CO (poisonous)
proton acceptor.
Check for air bubbles in the buret and remove the buret funnel from the buret
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

26. What is the formula for alkenes?
basic
Nothing
E=q + w (negative is by system - positive is on system)
CnH2n

27. perchlorate
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Suniverse increases for spontaneous processes
Graduated cylinder
ClO4?

28. Give an example of a dilute strong acid.
HClO4
White precipitate
Conjugate pair (one must be a weak base or acid)
The compound with the lowest Ksp value.

29. What type of compounds do Group 14 form?
Heat a test tube at an angle at the side of the tube (not bottom)
At half equivalence - pH=pKa
Read the bottom of the meniscus
+4-covalent - +2-ionic

30. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
White precipitate
P2O5
Experimental mass/theoretical mass X 100
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

31. What is the conjugate acid of H2PO4?
Products - reactants (except for BDE when it's reactants - products)
Insoluble except group 1 and ammonium
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
H3PO4

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

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33. How do you get the equation for a net electrolysis reaction?
proton acceptor.
proton donor base
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Combine the equations for the half reactions in the non-spontaneous direction

34. What process do you use to separate two liquids with different boiling points?
blue glass - it filters UV
fractional distillation
bases
basic

35. What apparatus do you use to pour liquids?
Experimental mass/theoretical mass X 100
Pour liquids using a funnel or down a glass rod
Kc=Kp
it's lower and occurs over less sharp a range

36. What do you need to make a polymer?
by electrolysis
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)
White precipitate
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

37. What shape is carbon dioxide?
linear
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Acid rain - dissolves marble buildings/statues and kills trees.
Conjugate pair (one must be a weak base or acid)

38. What is HCOOCH3?
Group 1 hydroxides (ex: NaOH)
Suniverse increases for spontaneous processes
Insoluble (except group 1 ammonium and Ba)
Acids; HCOOCH3 is an ester

39. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
bright yellow
Mono; di; tri; tetra; penta; hexa.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Most are soluble except Ag - Pb

40. primary colors
zero
Glowing splint (positive result=relights)
small size and high charge
red - green - blue

41. What is the formula of butane?
White precipitate
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Molecules with the same molecular formulas - but different structural formulas
C4H10

42. hypochlorite
NO3?
ClO?
benzene has a delocalized pi ring structure
do not change

43. What is the test for hydrogen?
lighted splint (positive result=pop)
Nothing
ethers
Monomer + monomer = polymer product + a simple molecule such as water or HCl

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

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45. What does saturated mean? Unsaturated?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
MnO4?
Disulfur dichloride
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

46. What steps do organic labs consist of?
Combine the equations for the half reactions in the non-spontaneous direction
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?)
Synthesis - separation and purification of the product and its identification.
Cr2O7²?

47. chromate ion (soln + most solids)
Salt and water
yellow
CnH2n+1 often designated 'R' ex C3H7 is propyl
benzene has a delocalized pi ring structure

48. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
allow for the vapor pressure of water and make sure to level levels
+4-covalent - +2-ionic
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

49. permanganate
Add acid to water so that the acid doesn't boil and spit
Experimental mass/theoretical mass X 100
It ceases - the circuit is broken.
MnO4?

50. If a free element is involved - what type of reaction must be involved?
Cr2O7²?
Insoluble except nitrate and acetate
redox reaction
Pale yellow

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AP Chemistry 2

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