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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. What process do you use to obtain the precipitate from a solution?
C4H10
Filtration
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

2. Nonmetals are good _____ agents. Metals are good _______ agents.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
ionic and form hydrogen and hydroxide
benzene has a delocalized pi ring structure
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

3. Does Kw increase or decrease with T? Why?
acid + alcohol
Increases.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

4. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
NH2?

5. What do nonmetal oxides plus water form?
zero
Insoluble
acids
Acidified

6. How do you clean a buret/pipette for a titration?
non-metal oxides and hydrides are covalently bonded and are acidic.
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
S crystal at 0K=0
zero

7. What are amphoteric oxides?
Salt + water
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?)
blue (BTB)
catalyst=conc H2SO4

8. What is the formula for summation?

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9. silver compounds
Insoluble except for nitrate and acetate
ClO3?
White precipitate
CnH2n-2

10. sulfate
blue glass - it filters UV
SO4²?
CrO4²?
Initiation energy (NOT Ea)

11. dichromate
Ksp = 27s4
Cr2O7²?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
RX

12. What are the common strong bases?
Group 1 hydroxides (ex: NaOH)
blue
Synthesis - separation and purification of the product and its identification.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

13. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Pale yellow
ClO2?

14. Is the standard entropy (S°) of an element zero?
Selective absorption
But S° of element is not zero (except at 0K)
Check for air bubbles in the buret and remove the buret funnel from the buret
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

15. How do you get the equation for a net electrolysis reaction?
Pale purple - (orange)-yellow - red - blue - green.
red - green - blue
non-metal oxides and hydrides are covalently bonded and are acidic.
Combine the equations for the half reactions in the non-spontaneous direction

16. What is the slope of the graph of lnk vs. 1/T?
ion pairing
Synthetic condensation polymer (aka a polyamide)
-Ea/R
proton acceptor.

17. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
Ionic compounds
benzene has a delocalized pi ring structure
voltaic: + electrolytic: -

18. What is the relationship in strength between sigma and pi bonds?
Glowing splint (positive result=relights)
Disulfur dichloride
a-IMFs - b-molecular volume
Sigma bonds are stronger than pi bonds

19. copper sulfate
Purple
Insoluble
0 and 14
blue

20. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Concentration
NH4?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

21. For a dibasic acid (H2A) - [A²?]= ____ ?
ROR
Salts (ex: CaO + SO2 ? CaSO3)
K2
CnH(2n+2)

22. Name some properties of Group 17
fruit - fish - bases
Insoluble except nitrate and acetate
K2
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

23. 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
CO2 and H2O
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

24. What two compounds are great oxidizing agents?

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25. What is the name of S2Cl2? (Know how to name others like this - too)
non-metal oxides and hydrides are covalently bonded and are acidic.
Disulfur dichloride
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
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)

26. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Greenish-yellow gas
redox reaction
non-metal oxides and hydrides are covalently bonded and are acidic.
'non-active' metals such as Cu - Ag - Au - Pt - etc.

27. What does saturated mean? Unsaturated?
ionic and form hydrogen and hydroxide
Soluble
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

28. What is the formula for alkynes?
Soluble
Saturated - Substitution (which requires more radical conditions)
linear
CnH2n-2

29. If ?S is positive - are the products more or less chaotic than the reactants?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
More chaotic (ex: gases made)
Tetrahedral
zero

30. What is the general formula for alkyl halides?
allow for the vapor pressure of water and make sure to level levels
?H-kJ - ?S-J - ?G-kJ
RX
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

31. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
ion pairing
Big K=kf/kr
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

32. What is the charge on a chlorine atom?
zero
RCOOR
Acids; HCOOCH3 is an ester
Time?¹ - (ex. s?¹ - hr?¹ - etc)

33. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
RCHO (carbonyl at end)
CnH(2n+2)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
ethers

34. barium sulfate
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Concentration
Time?¹ - (ex. s?¹ - hr?¹ - etc)
White precipitate

35. How are strong ones written?
it is lower and occurs over less sharp a range
strong acids/bases are written as H+ or OH- ions
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Disulfur dichloride

36. Why are noble gases stable?
Molecules with the same molecular formulas - but different structural formulas
Acid rain - dissolves marble buildings/statues and kills trees.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Kc=Kp

37. During a titration what is present in the beaker at the equivalence point?
A salt solution.
voltaic: - electrolytic: +
Molecules with the same molecular formulas - but different structural formulas
Ksp = 4s³

38. bromine
brown volatile liquid
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Increases down group 1 decreases down group 17
The benzene ring (or more correctly the phenyl group - C6H5)

39. What is the formula for obtaining charge flowing in a cell?
Insoluble (except group 1 ammonium and Ba)
Glowing splint (positive result=relights)
K2
Q=It (time in seconds)

40. What do acids plus active metals form?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
ClO?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
OH?

41. How many ligands attach to a central ion in a complex ion?
At half equivalence - pH=pKa
neutralization: high K - H2O product dissociation: low K - H2O reactant
Heat a test tube at an angle at the side of the tube (not bottom)
#ligands=charge x2

42. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
bent
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Initiation energy (NOT Ea)

43. What is the catalyst for this reaction Ester + ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
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)
catalyst=conc H2SO4
Molecules with the same molecular formulas - but different structural formulas

44. What are the signs for ?G and E° for spontaneous reactions?
CnH2n+2
?G= -ve - E°= +ve
OH?
Soluble

45. How do you find the pH for a dibasic acid? (H2A)?
water and substances with (s) less dense than
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Perform ICE BOX calculation based on K1
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

46. What are two substances that sublime at 1 atm when heated?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Iodine and CO2 (dry ice)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

47. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
Suniverse increases for spontaneous processes
Ppt will NOT form (unsaturated)
Initiation energy (NOT Ea)

48. How do you get Ecell for spontaneous reactions?
[A?]/[HA] x 100 or [BH?]/[B] x 100
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
S crystal at 0K=0
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

49. mercury (II) ion
Kc=Kp
Heptane
Ksp = 27s4
Hg²?

50. hypochlorite
ClO?
Soluble
White precipitate
CO2 and H2O