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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. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pipette (burette if need repetition)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
The dilution effect when the solutions mix. M1V1 = M2V2
Pale purple - (orange)-yellow - red - blue - green.

2. hydroxides
Insoluble (except group 1 ammonium and Ba)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Evaporation
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

3. Aromatic compounds contain what?
blue (BTB)
Trigonal pyramidal
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
The benzene ring (or more correctly the phenyl group - C6H5)

4. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
acid + alcohol
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CnH(2n+2)

5. What is the word equation for addition polymerisation?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
no - they're written undissociated (HAaq)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
The compound with the lowest Ksp value.

6. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
0.10M HCl (more ions)
bright yellow
Time?¹ - (ex. s?¹ - hr?¹ - etc)

7. Nonmetals are good _____ agents. Metals are good _______ agents.
Soluble
Making sigma bonds and holding lone pairs
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

8. lead compounds
The one with most oxygen atoms (highest oxidation number)
Sigma bonds are stronger than pi bonds
allow for the vapor pressure of water and make sure to level levels
Insoluble except nitrate and acetate

9. What are the signs of ?G and E° for spontaneous reactions?
CO2 and H2O
?G=negative - E° must be positive
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
A salt solution.

10. thiosulfate
The benzene ring (or more correctly the phenyl group - C6H5)
ion pairing
S2O3²?
They decrease (or could be the same if the solid has ONLY JUST disappeared)

11. What type of solutions do small - highly charged cations tend to form?
PO4³?
Hg2²?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Equivalence point is the titrant volume when the moles of acid and base are stoichiometrically equal; end point is the titrant volume when the color of the indicator permanently changes. If you choose the correct indicator - they should occur at the

12. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Hg2²?
do not change
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
A salt solution.

13. Color is due to ______ _______ of light.
ion pairing
Selective absorption
water and substances with (s) less dense than
left - ppt will form

14. What do metal oxides plus non- metal oxides form?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Saturated - Substitution (which requires more radical conditions)
Read the bottom of the meniscus
Salts (ex: CaO + SO2 ? CaSO3)

15. What do ions and electrons travel through in a voltaic/electrolytic cell?
Concentration
CnH2n-2
same KE - but PEice<PEwater
Ions go through the salt bridge - electrons go through metal wires in the external circuit

16. What is the formula for summation?

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17. How are non-metal oxides and hydrides bonded? are they acidic or basic?
no - they're written undissociated (HAaq)
Suniverse increases for spontaneous processes
H+
non-metal oxides and hydrides are covalently bonded and are acidic.

18. What is the test for hydrogen?
yellow
Products - reactants (except for BDE when it's reactants - products)
lighted splint (positive result=pop)
H2PO4?

19. What is the conjugate acid of H2PO4?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Concentration
H3PO4
blue

20. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
SO4²?
a-IMFs - b-molecular volume
zero
Reduction always takes place at the cathode (RED CAT) In both types of cell!

21. What is the sign of the anode in voltaic cells? in electrolytic cells?
it's lower and occurs over less sharp a range
PO4³?
CO3²?
voltaic: - electrolytic: +

22. What is the test for oxygen?
Glowing splint (positive result=relights)
?G=negative - E° must be positive
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
it reacts by substitution NOT addition

23. Name six characteristics of transition elements (or their compounds)
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.
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
chemically (ex: with carbon)

24. Acids + Carbonates (bicarbonates) make?
PO4³?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Decant
Soluble

25. What are two allotropes of carbon?
They stay the same.
are less dense than water
diamond and graphite
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

26. Alkanes are _________ and react by _________
Ppt will NOT form (unsaturated)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
non-metal oxides and hydrides are covalently bonded and are acidic.
Saturated - Substitution (which requires more radical conditions)

27. What equipment do you need for a titration?
linear
non-metal oxides and hydrides are covalently bonded and are acidic.
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Insoluble except for nitrate and acetate

28. How do you compute % dissociation?
Ksp = 27s4
it is lower and occurs over less sharp a range
[A?]/[HA] x 100 or [BH?]/[B] x 100
q=mc?T q=mL (or n x ?h)

29. Esterification is...
acid + alcohol
fractional distillation
catalyst=conc H2SO4
Eudiometer

30. Which alkali metals float on water?
RX
All except for lithium
No - it depends on the number of ions produced on dissolving.
ClO3?

31. What is the slope of the graph of lnk vs. 1/T?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
by electrolysis
Ionic compounds
-Ea/R

32. Give an example of a concentrated weak acid.
Glacial acetic acid
-Ea/R
0 and 14
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

33. mercury (I) ion
Tetrahedral
Soluble except Ag - Pb - Ca - Sr Ba)
Q=It (time in seconds)
Hg2²?

34. sulfates
ethers
Soluble except Ag - Pb - Ca - Sr Ba)
acid + alcohol
K1 x K2

35. 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.
Greenish-yellow gas
ion pairing
A) any range. b) 8-10 c) 4-6
But S° of element is not zero (except at 0K)

36. What do you use to look at burning magnesium? why?
bases
chemically (ex: with carbon)
?H-kJ - ?S-J - ?G-kJ
blue glass - it filters UV

37. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
CO (poisonous)
RCOOH
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Anode

38. dichromate
Cr2O7²?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

39. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Only temperature
Mono; di; tri; tetra; penta; hexa.
ns² electrons (first in-first out)

40. Does reactivity increase/decrease going down group 1 and group 17?
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
ClO?
Hg²?
Increases down group 1 decreases down group 17

41. What value of R do you use for thermo calculations? gas calculations?
Group I metals (soft metals) are stored under oil
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Hg2²?
NH2?

42. phosphate
H2PO4?
At half equivalence - pH=pKa
RCOOH
PO4³?

43. 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?
ClO?
Pale purple - (orange)-yellow - red - blue - green.
'non-active' metals such as Cu - Ag - Au - Pt - etc.
The compound with the lowest Ksp value.

44. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
It ceases - the circuit is broken.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
no - they're written undissociated (HAaq)

45. Give an example of a dilute strong acid.
ClO2?
10?8
Reduction always takes place at the cathode (RED CAT) In both types of cell!
HClO4

46. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
Soluble
Products - reactants (except for BDE when it's reactants - products)
A salt solution.

47. If Q > Ksp - then system shifts _______ and ppt ______
H2PO4?
hydroxides (ex: Ba(OH)2)
Pale yellow
left - ppt will form

48. What steps do organic labs consist of?
The one with most oxygen atoms (highest oxidation number)
RCOOR
Iodine and CO2 (dry ice)
Synthesis - separation and purification of the product and its identification.

49. How are primary alcohols turned into acids?
-Ea/R
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Making sigma bonds and holding lone pairs
HClO4

50. The definition of acidic basic and neutral aqueous solutions is:
Silvery gray solid - brown - purple
Ksp = s²
H2O + CO2 (it decomposes readily)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]