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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. Is a graduated cylinder or beaker more accurate?
T increases exponentially the proportion of molecules with E > Ea
it's lower and occurs over less sharp a range
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Graduated cylinder

2. What is the conjugate base of NH3?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
NH2?
Increases down group 1 decreases down group 17

3. Name some properties of Group 17
Orange
T increases exponentially the proportion of molecules with E > Ea
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

4. What effect does increasing the size/surface area of a voltaic cell have on the cell?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
The compound with the lowest Ksp value.
More chaotic (ex: gases made)
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.

5. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
-Ea/R
Experimental mass/theoretical mass X 100
Monomer + monomer = polymer product + a simple molecule such as water or HCl

6. hydroxide
Mn²? - Cr³? - Cr³
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
OH?
'non-active' metals such as Cu - Ag - Au - Pt - etc.

7. bromothymol
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
?G=negative - E° must be positive
CnH2n-2
blue (BTB)

8. Ions are not ______.
They stay the same.
Distillation
An active metal.
atoms

9. 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?)
#ligands=charge x2
More chaotic (ex: gases made)
Orange

10. acetate
?G=negative - E° must be positive
CH3COO?
No - it depends on the number of ions produced on dissolving.
OH?

11. When can supercooling occur? What does it look like on a cooling curve?

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12. What type of polymer is nylon?
Cu3(PO4)2
?H-kJ - ?S-J - ?G-kJ
Synthetic condensation polymer (aka a polyamide)
Soluble

13. What is the word equation for addition polymerisation?
ClO3?
voltaic: - electrolytic: +
zero
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

14. BaSO4
Insoluble
no - they're written undissociated (HAaq)
RCOOR
Salt + water

15. What is the pH of 1.0M HCl? 1M NaOH?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Salts (ex: CaO + SO2 ? CaSO3)
Synthesis - separation and purification of the product and its identification.
0 and 14

16. chromate
CrO4²?
Acidified
All except for lithium
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

17. What is the formula of butane?
water and substances with (s) less dense than
Clear
C4H10
CnH2n+2

18. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Heat a test tube at an angle at the side of the tube (not bottom)
Making sigma bonds and holding lone pairs
Ksp = 4s³

19. What is the second law of thermodynamics?
it is lower and occurs over less sharp a range
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Separating funnel
Suniverse increases for spontaneous processes

20. Name 2 ways in which you can create a buffer?
[A?]/[HA] x 100 or [BH?]/[B] x 100
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)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
The dilution effect when the solutions mix. M1V1 = M2V2

21. Why are noble gases stable?
Pipette (burette if need repetition)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
SO4²?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

22. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Trigonal pyramidal
neutralization: high K - H2O product dissociation: low K - H2O reactant
same KE - but PEice<PEwater
ClO3?

23. What is Big K in terms of kf and kr?
water and substances with (s) less dense than
Big K=kf/kr
S crystal at 0K=0
Acids; HCOOCH3 is an ester

24. Acid plus base make?
Acids; HCOOCH3 is an ester
Distillation
Salt + water.
CnH2n-2

25. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
It ceases - the circuit is broken.
Pale purple - (orange)-yellow - red - blue - green.

26. What do group I/II metal oxides plus water form?
0.10M HCl (more ions)
no - they're written undissociated (HAaq)
Q=It (time in seconds)
bases

27. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
Check for air bubbles in the buret and remove the buret funnel from the buret
Selective absorption
Silvery gray solid - brown - purple

28. What is the formula for alkanes?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Acid rain - dissolves marble buildings/statues and kills trees.
Tetrahedral
CnH2n+2

29. What do group I/II metal oxides and acids form?
Salt and water
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
OH?
CnH2n+2

30. What is the general formula for an amine?
Salt + water
RNH2
They stay the same.
Ppt will NOT form (unsaturated)

31. How do you find the pH for a dibasic acid? (H2A)?
H2PO4?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Perform ICE BOX calculation based on K1

32. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
ion pairing
water and substances with (s) less dense than
same KE - but PEice<PEwater

33. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
A salt solution.
do not change
same KE - but PEice<PEwater
O2 needs 4F/mol H2 needs 2F/mol

34. What do you do to get rid of most of the solution from a precipitate?
The Faraday or Faraday's constant.
no - they're written undissociated (HAaq)
CnH2n-2
Decant

35. What are the signs of ?G and E° for spontaneous reactions?
Soluble
?G=negative - E° must be positive
CnH2n-2
are less dense than water

36. cyanide
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Anode
same KE - but PEice<PEwater
CN?

37. What is the energy you must put into a reaction to make it start called?
proton acceptor.
White precipitate
Initiation energy (NOT Ea)
allow for the vapor pressure of water and make sure to level levels

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

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39. carbonates
redox reaction
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Insoluble except group 1 and ammonium
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

40. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Ionic compounds
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Anode
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

41. chromate ion (soln + most solids)
?G=negative - E° must be positive
RCHO (carbonyl at end)
proton donor base
yellow

42. What are allotropes?
ClO3?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
different forms of the same element
Soluble except Ag - Pb - Ca - Sr Ba)

43. What is the sign of the anode in voltaic cells? in electrolytic cells?
Salt + water
voltaic: - electrolytic: +
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
blue

44. What changes Keq?
Only temperature
Q=It (time in seconds)
NH2?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

45. An amphiprotic (amphoteric) species is...
Greenish-yellow gas
methyl formate
no - they're written undissociated (HAaq)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

46. What value of R do you use for thermo calculations? gas calculations?
Pipette (burette if need repetition)
How grouped results are
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

47. group 1 ions/compounds
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
RX
Ksp = s²
Soluble

48. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Current - time and charge on ion (moles of e used in half cell reaction)
do not change
Identity and purity (impure compounds usually have broad & low melting points)
diamond and graphite

49. What are isomers?
allow for the vapor pressure of water and make sure to level levels
Most are soluble except Ag - Pb
Products - reactants (except for BDE when it's reactants - products)
Molecules with the same molecular formulas - but different structural formulas

50. acetates
Soluble
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
CnH2n+1 often designated 'R' ex C3H7 is propyl
Mono; di; tri; tetra; penta; hexa.