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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. What are two substances that sublime at 1 atm when heated?
blue (BTB)
Purple
Iodine and CO2 (dry ice)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

2. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Group 1 hydroxides (ex: NaOH)
strong acids/bases are written as H+ or OH- ions
Distillation
They stay the same.

3. What are the formulas for q?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Group 1 hydroxides (ex: NaOH)
q=mc?T q=mL (or n x ?h)
Distillation

4. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Current - time and charge on ion (moles of e used in half cell reaction)
Experimental mass/theoretical mass X 100
voltaic: + electrolytic: -
Molecules with the same molecular formulas - but different structural formulas

5. Name some properties of Group 17
Filtration
Distillation
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
RCOR

6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Transition element compounds (except if it has a full or empty d shell)

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

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8. How do you get Ecell for spontaneous reactions?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Decant
Ksp = 27s4

9. What things should you remember to do when collecting gas over water?
Sigma bonds are stronger than pi bonds
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
allow for the vapor pressure of water and make sure to level levels
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

10. What is the difference between equivalence point and end point of a titration.
NH2?
it's lower and occurs over less sharp a range
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
Acids; HCOOCH3 is an ester

11. What do group I/II metal oxides plus water form?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
bases
no - they're written undissociated (HAaq)
Q=It (time in seconds)

12. What electrons are lost/gained first in transition element ions?
|experimental - accepted|/accepted X 100
But S° of element is not zero (except at 0K)
A salt solution.
ns² electrons (first in-first out)

13. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
Eudiometer
Increases.
methyl formate

14. What are two substances that sublime at 1 atm when heated?
Heptane
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Iodine and CO2 (dry ice)
It ceases - the circuit is broken.

15. What is the general formula for a ketone?
Graduated cylinder
blue glass - it filters UV
RCOR
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

16. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
No - NH3 and HCl gases are extremely soluble
Group 1 hydroxides (ex: NaOH)
acids

17. chromate ion (soln + most solids)
It ceases - the circuit is broken.
Hg2²?
yellow
ROH

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

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19. Acids + Carbonates (bicarbonates) make?
Salt + water
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Anode
acids

20. What steps do organic labs consist of?
non-metal oxides and hydrides are covalently bonded and are acidic.
Synthesis - separation and purification of the product and its identification.
OH?
Insoluble

21. What is the conjugate acid of H2PO4?
CnH2n+2
Increases down group 1 decreases down group 17
H3PO4
Reduction always takes place at the cathode (RED CAT) In both types of cell!

22. What is the formula for obtaining charge flowing in a cell?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
But S° of element is not zero (except at 0K)
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)
Q=It (time in seconds)

23. What is the third law of thermodynamics?
Sulfur
S crystal at 0K=0
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
voltaic: - electrolytic: +

24. What is the general formula for an acid?
Graduated cylinder
C4H10
RCOOH
The one with most oxygen atoms (highest oxidation number)

25. When a cell is 'flat' What is its voltage?
zero
C4H10
it's lower and occurs over less sharp a range
Disulfur dichloride

26. A Bronsted-Lowry base is...
CnH2n+1 often designated 'R' ex C3H7 is propyl
Most are soluble except Ag - Pb
Tetrahedral
proton acceptor.

27. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
same KE - but PEice<PEwater
allow for the vapor pressure of water and make sure to level levels
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

28. What is the second law of thermodynamics?
NH4?
Most are soluble except Ag - Pb
Kc=Kp
Suniverse increases for spontaneous processes

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

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30. If ?S is positive - are the products more or less chaotic than the reactants?
Disulfur dichloride
Soluble
More chaotic (ex: gases made)
NH2?

31. What do acids plus active metals form?
chemically (ex: with carbon)
Anode
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
a-IMFs - b-molecular volume

32. What is the catalyst for this reaction Ester + ?
by electrolysis
Nothing
catalyst=conc H2SO4
ROH

33. How many faradays of electric charge do you need to produce one mole of O2? H2?
Salt and water
0.10M HCl (more ions)
H+
O2 needs 4F/mol H2 needs 2F/mol

34. What is the pH of 1.0M HCl? 1M NaOH?
Increases down group 1 decreases down group 17
Conjugate pair (one must be a weak base or acid)
chemically (ex: with carbon)
0 and 14

35. What are the prefixes for the naming of binary molecular compound formulas (up to six)
hydroxides (ex: Ba(OH)2)
Hg2²?
Acidified
Mono; di; tri; tetra; penta; hexa.

36. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Exothermic
H+
O2 needs 4F/mol H2 needs 2F/mol
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

37. lead compounds
Pour liquids using a funnel or down a glass rod
ClO2?
linear
Insoluble except nitrate and acetate

38. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
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
[A?]/[HA] x 100 or [BH?]/[B] x 100
Check for air bubbles in the buret and remove the buret funnel from the buret
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

39. What measuring device would you use for very small volumes of liquids?
RNH2
Ionic compounds
Pipette (burette if need repetition)
+4-covalent - +2-ionic

40. Name 2 ways in which you can create a buffer?
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)
The benzene ring (or more correctly the phenyl group - C6H5)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

41. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
ion pairing
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Iodine and CO2 (dry ice)

42. What are the signs for ?G and E° for spontaneous reactions?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
?G= -ve - E°= +ve
ClO2?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

43. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
RCOOH
Disulfur dichloride
Insoluble except group 1 and ammonium

44. If Q < Ksp a ppt ______
?G=negative - E° must be positive
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Ppt will NOT form (unsaturated)
ion pairing

45. What is the general formula for an ether?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
ROR
Suniverse increases for spontaneous processes
Trigonal pyramidal

46. How does benzene compare in reactivity to alkenes?
RCOOR
Distillation
do not change
benzene is less reactive than alkenes

47. What is the general formula of an alkane?
CnH(2n+2)
Increases.
benzene is less reactive than alkenes
CO3²?

48. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
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)
Group I metals (soft metals) are stored under oil
Synthesis - separation and purification of the product and its identification.

49. What reacts with an acid to create hydrogen gas?
An active metal.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
CO2 and H2O
OH?

50. acetate
CH3COO?
K2
ROH
Ions go through the salt bridge - electrons go through metal wires in the external circuit