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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. What are hybrid orbitals used for?
RCHO (carbonyl at end)
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)
ClO2?
Making sigma bonds and holding lone pairs

2. What do you use to look at burning magnesium? why?
Ppt will NOT form (unsaturated)
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
blue glass - it filters UV
lighted splint (positive result=pop)

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

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4. Do you use J or kJ for ?H - ?S - and ?G?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Increases.
Concentration
?H-kJ - ?S-J - ?G-kJ

5. 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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6. What is the test for oxygen?
MnO4?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
H2O + CO2 (it decomposes readily)
Glowing splint (positive result=relights)

7. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Transition element compounds (except if it has a full or empty d shell)
Mn²? - Cr³? - Cr³
Insoluble
Graduated cylinder

8. What two types of substances are present in all redox reactions?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
a-IMFs - b-molecular volume
Anode - oxygen. Cathode - hydrogen
an oxidized and reduced substance

9. What do metal oxides plus non- metal oxides form?
boiling without losing volatile solvents/reactants
Salts (ex: CaO + SO2 ? CaSO3)
OH?
Ksp = 108s5

10. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
left - ppt will form
The benzene ring (or more correctly the phenyl group - C6H5)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

11. When combining half equations - what do you do to E° values when multiplying coefficients?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Nothing
Mono; di; tri; tetra; penta; hexa.
P2O5

12. What do hydrocarbons form when they burn in air (oxygen)?
Trigonal pyramidal
CO2 and H2O
Anode - oxygen. Cathode - hydrogen
The benzene ring (or more correctly the phenyl group - C6H5)

13. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
Synthetic condensation polymer (aka a polyamide)
10?8
basic

14. What is the second law of thermodynamics?
R=8.31 J/mol/K
methyl formate
They stay the same.
Suniverse increases for spontaneous processes

15. What steps do organic labs consist of?
R=8.31 J/mol/K
brown volatile liquid
Synthesis - separation and purification of the product and its identification.
it's lower and occurs over less sharp a range

16. What is the conjugate base of NH3?
C4H10
Perform ICE BOX calculation based on K1
Hg²?
NH2?

17. phosphate
SO4²?
They stay the same.
Acidified
PO4³?

18. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
redox reaction
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
The one with most oxygen atoms (highest oxidation number)

19. Acids + Carbonates (bicarbonates) make?
P2O5
basic
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

20. Color (absorbance) is proportional to ________
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Concentration
Ksp = 4s³
Saturated - Substitution (which requires more radical conditions)

21. Ca - Sr - Ba
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
hydroxides (ex: Ba(OH)2)
H2O + CO2 (it decomposes readily)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

22. What is the charge on a chlorine atom?
water and substances with (s) less dense than
benzene is less reactive than alkenes
zero
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

23. permanganate
#ligands=charge x2
MnO4?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
hydroxides (ex: Ba(OH)2)

24. chlorine
CO (poisonous)
Greenish-yellow gas
HClO4
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

25. What is the formula of butane?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
ClO4?
C4H10

26. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
are less dense than water
ROR
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Pour liquids using a funnel or down a glass rod

27. During a titration what is present in the beaker at the equivalence point?
non-metal oxides and hydrides are covalently bonded and are acidic.
The one with most oxygen atoms (highest oxidation number)
redox reaction
A salt solution.

28. If a weak acid is diluted more - what happens to its % dissociation value?
No - NH3 and HCl gases are extremely soluble
Increases.
CnH2n-2
chemically (ex: with carbon)

29. What is accuracy?
How close results are to the accepted value
'non-active' metals such as Cu - Ag - Au - Pt - etc.
MnO4?
Big K=kf/kr

30. What type of solutions do small - highly charged cations tend to form?
Identity and purity (impure compounds usually have broad & low melting points)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
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
Soluble except Ag - Pb - Ca - Sr Ba)

31. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Kc=Kp
It ceases - the circuit is broken.
An active metal.

32. What is Big K in terms of kf and kr?
CnH(2n+2)
Big K=kf/kr
C2O4²?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

33. nitrate
Transition element compounds (except if it has a full or empty d shell)
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?
Current - time and charge on ion (moles of e used in half cell reaction)

34. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
allow for the vapor pressure of water and make sure to level levels
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

35. Does reactivity increase/decrease going down group 1 and group 17?
They stay the same.
Increases down group 1 decreases down group 17
Pale yellow
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

36. What changes Keq?
RCOOH
Only temperature
Monomer + monomer = polymer product + a simple molecule such as water or HCl
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

37. What shape is water?
RCOOH
Iodine and CO2 (dry ice)
different forms of the same element
bent

38. What are the products of the reaction between group 1 metals and water?

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39. What word is a clue for a redox reaction?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
H2PO4?
Acidified
proton donor base

40. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
RX
zero
NO3?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

41. Aromatic compounds contain what?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Q=It (time in seconds)
The benzene ring (or more correctly the phenyl group - C6H5)
PO4³?

42. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
acid + alcohol
Soluble

43. What are amphoteric oxides?
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?)
T increases exponentially the proportion of molecules with E > Ea
Group 1 hydroxides (ex: NaOH)
Sigma bonds are stronger than pi bonds

44. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
NH2?
Acidified
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

45. silver compounds
Insoluble except for nitrate and acetate
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
More chaotic (ex: gases made)
How grouped results are

46. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
zero-th: decreases - first: constant - second: increases
acid + alcohol
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

47. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Increases.
CnH(2n+2)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
The one with most oxygen atoms (highest oxidation number)

48. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
At half equivalence - pH=pKa
|experimental - accepted|/accepted X 100
?G= -ve - E°= +ve
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

49. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
fractional distillation
#ligands=charge x2
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

50. What is the general formula for a ketone?
RCOR
chemically (ex: with carbon)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
White precipitate