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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. Color (absorbance) is proportional to ________
brown volatile liquid
Concentration
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)
Identity and purity (impure compounds usually have broad & low melting points)

2. What is the first law of thermodynamics?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Group 1 hydroxides (ex: NaOH)
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)
E=q + w (negative is by system - positive is on system)

3. What element is used to vulcanize rubber?
red - green - blue
Sulfur
'non-active' metals such as Cu - Ag - Au - Pt - etc.
PO4³?

4. What is the third law of thermodynamics?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
S crystal at 0K=0
+4-covalent - +2-ionic
Ksp = 4s³

5. group 1 ions/compounds
PO4³?
Synthesis - separation and purification of the product and its identification.
Group I metals (soft metals) are stored under oil
Soluble

6. ammonium/ammonium compounds
Products - reactants (except for BDE when it's reactants - products)
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.
Hg2²?
Soluble

7. Does reactivity increase/decrease going down group 1 and group 17?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Separating funnel
Ionic compounds
Increases down group 1 decreases down group 17

8. Aromatic compounds contain what?
The benzene ring (or more correctly the phenyl group - C6H5)
ClO?
Products - reactants (except for BDE when it's reactants - products)
MnO4?

9. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Molecules with the same molecular formulas - but different structural formulas
voltaic: - electrolytic: +
zero
blue (BTB)

10. During a titration what is present in the beaker at the equivalence point?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
proton donor base
A salt solution.

11. BaSO4
methyl formate
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
Insoluble
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

12. Does Kw increase or decrease with T? Why?
CnH2n-2
ClO2?
RX
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

13. If Q > Ksp - then system shifts _______ and ppt ______
water and substances with (s) less dense than
Acidified
Separating funnel
left - ppt will form

14. iodine - iodine solution - iodine vapor
All except for lithium
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)
Silvery gray solid - brown - purple

15. The definition of acidic basic and neutral aqueous solutions is:
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)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Molecules with the same molecular formulas - but different structural formulas

16. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
CH3COO?
#ligands=charge x2
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

17. What shape is ammonia?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Trigonal pyramidal
voltaic: + electrolytic: -

18. How many ligands attach to a central ion in a complex ion?
Salt + water
#ligands=charge x2
small size and high charge
proton donor base

19. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
Group I metals (soft metals) are stored under oil
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Sulfur

20. dichromate (soln + most solids)
Orange
Group 1 hydroxides (ex: NaOH)
At half equivalence - pH=pKa
Acidified

21. What is the general formula for an acid?
CnH2n-2
OH?
RCOOH
benzene is less reactive than alkenes

22. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
O2 needs 4F/mol H2 needs 2F/mol
Acid rain - dissolves marble buildings/statues and kills trees.
metal oxides and hydrides are ionically bonded and basic

23. What is HCOOCH3?
Acids; HCOOCH3 is an ester
boiling without losing volatile solvents/reactants
PO4³?
Pipette (burette if need repetition)

24. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
Initiation energy (NOT Ea)
Most are soluble except Ag - Pb
Evaporation

25. chlorite
Transition element compounds (except if it has a full or empty d shell)
It ceases - the circuit is broken.
Evaporation
ClO2?

26. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
fractional distillation
Heat a test tube at an angle at the side of the tube (not bottom)
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)

27. Which of the rates changes more when temperature is increased?
?H formation of an element in standard state=0
do not change
a-IMFs - b-molecular volume
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

28. When combining half equations - what do you do to E° values when multiplying coefficients?
Q=It (time in seconds)
CO3²?
Nothing
They decrease (or could be the same if the solid has ONLY JUST disappeared)

29. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
RCOR
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

30. When driving off water from a hydrate - how do you tell you're done?
Insoluble except group 1 and ammonium
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
blue
#ligands=charge x2

31. Esters smell like _______ and amines smell like _______ and are ______.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Pour liquids using a funnel or down a glass rod
chemically (ex: with carbon)
fruit - fish - bases

32. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Soluble
Current - time and charge on ion (moles of e used in half cell reaction)
More chaotic (ex: gases made)
ion pairing

33. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
Eudiometer
Synthetic condensation polymer (aka a polyamide)
Kc=Kp

34. What do you use for an acid spill? base spill?
Acids; HCOOCH3 is an ester
Transition element compounds (except if it has a full or empty d shell)
RCOOH
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

35. Acidic gases like SO2 in the atmosphere cause what environmental problems?
The Faraday or Faraday's constant.
Acid rain - dissolves marble buildings/statues and kills trees.
Greenish-yellow gas
Iodine and CO2 (dry ice)

36. What process do you use to separate two liquids with different boiling points?
A salt solution.
White precipitate
are less dense than water
fractional distillation

37. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
SO4²?
ion pairing
The Faraday or Faraday's constant.
same KE - but PEice<PEwater

38. perchlorate
Anode
ClO4?
Glowing splint (positive result=relights)
Purple

39. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
same KE - but PEice<PEwater
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Concentration

40. What is the slope of the graph of lnk vs. 1/T?
-Ea/R
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
CO2 and H2O
it's lower and occurs over less sharp a range

41. Does Benzene react by addition or substitution?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Anode
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)
it reacts by substitution NOT addition

42. What do the 'a' and 'b' in Van Der Waal's equation allow for?
red - green - blue
a-IMFs - b-molecular volume
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

43. nitrate
NO3?
a-IMFs - b-molecular volume
The Faraday or Faraday's constant.
OH- and NH3

44. What does a short - sharp melting point indicate?
They stay the same.
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Identity and purity (impure compounds usually have broad & low melting points)
'non-active' metals such as Cu - Ag - Au - Pt - etc.

45. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Identity and purity (impure compounds usually have broad & low melting points)
fruit - fish - bases
Increases.

46. What is the word equation for condensation polymerisation ?
are less dense than water
PO4³?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

47. What changes Keq?
Only temperature
benzene has a delocalized pi ring structure
Nothing
CnH2n

48. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
SO4²?
CnH2n
yellow

49. What do metal oxides plus non- metal oxides form?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
K1 x K2
Heptane
Salts (ex: CaO + SO2 ? CaSO3)

50. oxalate
C2O4²?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Q=It (time in seconds)
H3PO4