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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.
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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. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Conjugate pair (one must be a weak base or acid)
bent
a-IMFs - b-molecular volume

2. silver compounds
Insoluble except for nitrate and acetate
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
R=8.31 J/mol/K
blue (BTB)

3. When combining half equations - what do you do to E° values when multiplying coefficients?
They stay the same.
Nothing
Increases.
S2O3²?

4. Ions are not ______.
atoms
Insoluble except group 1 and ammonium
same KE - but PEice<PEwater
They decrease (or could be the same if the solid has ONLY JUST disappeared)

5. A geometric (or cis-trans) isomer exists due to.....
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
fruit - fish - bases
Ksp = 27s4
ClO4?

6. What complex ion does ammonia form with silver? copper? cadmium? zinc?
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)
zero
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Heat a test tube at an angle at the side of the tube (not bottom)

7. What are hybrid orbitals used for?
RCOR
Only temperature
Making sigma bonds and holding lone pairs
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

8. Esters smell like _______ and amines smell like _______ and are ______.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
a-IMFs - b-molecular volume
Group 1 hydroxides (ex: NaOH)
fruit - fish - bases

9. How does the melting point of a mixture compare to the MP of a pure substance?
H2PO4?
C2O4²?
it is lower and occurs over less sharp a range
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

10. During a titration what is present in the beaker at the equivalence point?
A salt solution.
fruit - fish - bases
CnH2n
The one with most oxygen atoms (highest oxidation number)

11. nitrate
no - they're written undissociated (HAaq)
NO3?
PO4³?
Ions go through the salt bridge - electrons go through metal wires in the external circuit

12. For a dibasic acid (H2A) - [A²?]= ____ ?
RNH2
Silvery gray solid - brown - purple
K2
-Ea/R

13. How many normal boiling points and boiling points are there?

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14. mercury (I) ion
Add acid to water so that the acid doesn't boil and spit
Hg2²?
Insoluble
RCOR

15. What shape is ammonia?
Insoluble
Trigonal pyramidal
it is lower and occurs over less sharp a range
yellow

16. What is the general formula for alkyl halides?
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)
RX
RNH2
Concentration

17. An amphiprotic (amphoteric) species is...
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
RCHO (carbonyl at end)
C2O4²?

18. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
Pipette (burette if need repetition)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
fractional distillation

19. Acid plus base make?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
CnH(2n+2)
Ksp = 27s4
Salt + water.

20. What are two substances that sublime at 1 atm when heated?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Soluble except Ag - Pb - Ca - Sr Ba)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Iodine and CO2 (dry ice)

21. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Making sigma bonds and holding lone pairs
CO2 and H2O
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Experimental mass/theoretical mass X 100

22. What does a short - sharp melting point indicate?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Identity and purity (impure compounds usually have broad & low melting points)
Salts (ex: CaO + SO2 ? CaSO3)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

23. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
CrO4²?
Anode
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

24. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Glacial acetic acid
PO4³?
O2 needs 4F/mol H2 needs 2F/mol

25. How does the melting point of a mixture compare to the MP of a pure substance?

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26. What are isotopes?
The one with most oxygen atoms (highest oxidation number)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Nothing
allow for the vapor pressure of water and make sure to level levels

27. How many faradays of electric charge do you need to produce one mole of O2? H2?
MnO4?
OH?
O2 needs 4F/mol H2 needs 2F/mol
Ksp = 4s³

28. What are allotropes?
different forms of the same element
RCHO (carbonyl at end)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
NH2?

29. What is the general formula for an amine?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
atoms
Insoluble except for nitrate and acetate
RNH2

30. chromate
CrO4²?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
The dilution effect when the solutions mix. M1V1 = M2V2
Initiation energy (NOT Ea)

31. What do you use to look at burning magnesium? why?
OH?
blue glass - it filters UV
Ionic compounds
?H formation of an element in standard state=0

32. How are more active metals reduced?
by electrolysis
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Ppt will NOT form (unsaturated)
Decant

33. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Heat a test tube at an angle at the side of the tube (not bottom)
?H-kJ - ?S-J - ?G-kJ
neutralization: high K - H2O product dissociation: low K - H2O reactant
zero

34. Give an example of a dilute strong acid.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
H+
HClO4

35. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
zero
Insoluble (except group 1 ammonium and Ba)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

36. What is the pH of 1.0M HCl? 1M NaOH?
No - NH3 and HCl gases are extremely soluble
0 and 14
Only temperature
ClO2?

37. ammonium/ammonium compounds
Soluble
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.
q=mc?T q=mL (or n x ?h)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

38. Which alkali metals float on water?
All except for lithium
Ksp = s²
Ions go through the salt bridge - electrons go through metal wires in the external circuit
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)

39. What changes Keq?
Only temperature
acid + alcohol
benzene has a delocalized pi ring structure
All except for lithium

40. What electrons are lost/gained first in transition element ions?
ns² electrons (first in-first out)
CN?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
0.10M HCl (more ions)

41. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pale purple - (orange)-yellow - red - blue - green.
Check for air bubbles in the buret and remove the buret funnel from the buret
Both electrons come from the same atom (just as good as a regular bond)
CnH2n+2

42. perchlorate
ClO4?
E=q + w (negative is by system - positive is on system)
?G= -ve - E°= +ve
Exothermic

43. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
It ceases - the circuit is broken.
HClO4
They stay the same.
A) any range. b) 8-10 c) 4-6

44. A Bronsted-Lowry base is...
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
proton acceptor.
zero
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

45. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
RNH2
Group I metals (soft metals) are stored under oil
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
HClO4

46. How does half life change for zero-th order - first order - and second order processes?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Salt + water.
zero-th: decreases - first: constant - second: increases
proton donor base

47. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
CnH2n+1 often designated 'R' ex C3H7 is propyl
Ionic compounds
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

48. What are the signs for ?G and E° for spontaneous reactions?
Saturated - Substitution (which requires more radical conditions)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
OH- and NH3
?G= -ve - E°= +ve

49. What do group I/II metal oxides and acids form?
S2O3²?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Salt and water
Making sigma bonds and holding lone pairs

50. potassium permanganate
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Purple
Most INsoluble except group 1 and ammonium
Most are soluble except Ag - Pb