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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. lead iodide
CnH(2n+2)
small size and high charge
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
bright yellow

2. How do you dilute an acid?

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3. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
ion pairing
Exothermic

4. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
Disulfur dichloride
Products - reactants (except for BDE when it's reactants - products)
redox reaction

5. What is the charge on a chlorine atom?
SO4²?
No - NH3 and HCl gases are extremely soluble
zero
PO4³?

6. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
CO3²?
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
Hg2²?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

7. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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8. How does half life change for zero-th order - first order - and second order processes?
Hg²?
zero-th: decreases - first: constant - second: increases
C4H10
q=mc?T q=mL (or n x ?h)

9. Esterification is...
bright yellow
Perform ICE BOX calculation based on K1
acid + alcohol
CO3²?

10. What are the signs of ?G and E° for spontaneous reactions?
it reacts by substitution NOT addition
Disulfur dichloride
?G=negative - E° must be positive
Acids; HCOOCH3 is an ester

11. When a cell is 'flat' What is its voltage?
Making sigma bonds and holding lone pairs
it's lower and occurs over less sharp a range
allow for the vapor pressure of water and make sure to level levels
zero

12. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Salt + water.
Experimental mass/theoretical mass X 100
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

13. What is the sign of the anode in voltaic cells? in electrolytic cells?
a-IMFs - b-molecular volume
RX
zero
voltaic: - electrolytic: +

14. What is reflux?
C2O4²?
How close results are to the accepted value
Q=It (time in seconds)
boiling without losing volatile solvents/reactants

15. What is the general formula for an ether?
O2 needs 4F/mol H2 needs 2F/mol
ROR
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

16. What is the third law of thermodynamics?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
No - it depends on the number of ions produced on dissolving.
S crystal at 0K=0
Ksp = 4s³

17. For a dibasic acid (H2A) - [A²?]= ____ ?
NH2?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
K2
bases

18. 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
The Faraday or Faraday's constant.
Hg²?
Soluble

19. What measuring device would you use for very small volumes of liquids?
Heptane
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Pipette (burette if need repetition)
ClO3?

20. ________ are Lewis bases - because they can donate a lone pair of electrons.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
OH- and NH3
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Cr2O7²?

21. What shape is carbon dioxide?
linear
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
bases

22. When is ?G zero?
bright yellow
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
H+
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

23. Is a graduated cylinder or beaker more accurate?
PO4³?
Graduated cylinder
At half equivalence - pH=pKa
do not change

24. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
+4-covalent - +2-ionic
Transition element compounds (except if it has a full or empty d shell)
The one with most oxygen atoms (highest oxidation number)

25. chromate ion (soln + most solids)
blue (BTB)
methyl formate
yellow
red - green - blue

26. 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?
Iodine and CO2 (dry ice)
The compound with the lowest Ksp value.
ion pairing
P2O5

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

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28. What is H2CO3 (carbonate acid) usually written as?
zero
H2O + CO2 (it decomposes readily)
Insoluble except group 1 and ammonium
chemically (ex: with carbon)

29. sulfate
?G=negative - E° must be positive
O2 needs 4F/mol H2 needs 2F/mol
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
SO4²?

30. What do you use for an acid spill? base spill?
Salts (ex: CaO + SO2 ? CaSO3)
White precipitate
Concentration
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

31. carbonate
q=mc?T q=mL (or n x ?h)
CO3²?
+4-covalent - +2-ionic
Salts (ex: CaO + SO2 ? CaSO3)

32. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Mono; di; tri; tetra; penta; hexa.
Pale purple - (orange)-yellow - red - blue - green.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

33. How does the melting point of a mixture compare to the MP of a pure substance?
A) any range. b) 8-10 c) 4-6
Most are soluble except Ag - Pb
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
it is lower and occurs over less sharp a range

34. Aromatic compounds contain what?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Increases down group 1 decreases down group 17
The benzene ring (or more correctly the phenyl group - C6H5)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

35. bromothymol
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Concentration
blue (BTB)

36. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
Iodine and CO2 (dry ice)
basic
Nothing

37. A Bronsted-Lowry base is...
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
ClO3?
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.
proton acceptor.

38. Which alkali metals float on water?
All except for lithium
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
proton acceptor.
Soluble except Ag - Pb - Ca - Sr Ba)

39. Color is due to ______ _______ of light.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
different forms of the same element
Selective absorption
Eudiometer

40. What process do you use to obtain the precipitate from a solution?
CN?
Ksp = s²
Filtration
Ksp = 4s³

41. perchlorate
a-IMFs - b-molecular volume
ClO4?
by electrolysis
Iodine and CO2 (dry ice)

42. What is the formula of copper (II) phosphate?
Cu3(PO4)2
Iodine and CO2 (dry ice)
R=8.31 J/mol/K
Tetrahedral

43. How do you clean a buret/pipette for a titration?
different forms of the same element
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
same KE - but PEice<PEwater
The dilution effect when the solutions mix. M1V1 = M2V2

44. What is the conjugate acid of H2PO4?
Trigonal pyramidal
Acidified
Conjugate pair (one must be a weak base or acid)
H3PO4

45. primary colors
OH?
red - green - blue
Orange
metal oxides and hydrides are ionically bonded and basic

46. What are isomers?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Mn²? - Cr³? - Cr³
Anode - oxygen. Cathode - hydrogen
Molecules with the same molecular formulas - but different structural formulas

47. What things should you remember to do when collecting gas over water?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
allow for the vapor pressure of water and make sure to level levels
same KE - but PEice<PEwater

48. Acidic gases like SO2 in the atmosphere cause what environmental problems?
0.10M HCl (more ions)
Acid rain - dissolves marble buildings/statues and kills trees.
Saturated - Substitution (which requires more radical conditions)
Products - reactants (except for BDE when it's reactants - products)

49. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Decant
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
T increases exponentially the proportion of molecules with E > Ea
same KE - but PEice<PEwater

50. What is precision?
How grouped results are
Salt + water.
S2O3²?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).