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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. chromate ion (soln + most solids)
0.10M HCl (more ions)
lighted splint (positive result=pop)
non-metal oxides and hydrides are covalently bonded and are acidic.
yellow

2. What shape is methane?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Experimental mass/theoretical mass X 100
basic
Tetrahedral

3. How can metals like iron and zinc be reduced?
Exothermic
chemically (ex: with carbon)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Disulfur dichloride

4. What is the general formula for an acid?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Mono; di; tri; tetra; penta; hexa.
methyl formate
RCOOH

5. Alkenes are ________ and react by __________
The dilution effect when the solutions mix. M1V1 = M2V2
Increases down group 1 decreases down group 17
Insoluble except nitrate and acetate
Unsaturated - addition (ex: decolorize bromine solution)

6. Does Kw increase or decrease with T? Why?
Separating funnel
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
A) any range. b) 8-10 c) 4-6

7. Generally - which oxy acid is strongest?
?H formation of an element in standard state=0
Concentration
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
The one with most oxygen atoms (highest oxidation number)

8. What do you use to look at burning magnesium? why?
SO4²?
blue glass - it filters UV
blue (BTB)
How grouped results are

9. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Iodine and CO2 (dry ice)
water and substances with (s) less dense than
T increases exponentially the proportion of molecules with E > Ea

10. What is a dipeptide? polypeptide? protein?
S2O3²?
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
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

11. bromine
brown volatile liquid
H2PO4?
Distillation
All except for lithium

12. What is the charge on a chlorine atom?
benzene has a delocalized pi ring structure
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)
S crystal at 0K=0
zero

13. What is the conjugate acid of H2PO4?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
H3PO4
CO3²?
do not change

14. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
atoms
H3PO4
C2O4²?
same KE - but PEice<PEwater

15. How are metal oxides and hydrides bonded? are they acidic or basic?
P2O5
How close results are to the accepted value
metal oxides and hydrides are ionically bonded and basic
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.

16. A Bronsted-Lowry base is...
K1 x K2
Ksp = 4s³
The compound with the lowest Ksp value.
proton acceptor.

17. What process do you use to obtain the precipitate from a solution?
Filtration
Heptane
fractional distillation
More chaotic (ex: gases made)

18. silver iodide
Insoluble except group 1 and ammonium
Perform ICE BOX calculation based on K1
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Pale yellow

19. What are hybrid orbitals used for?
CnH2n+1 often designated 'R' ex C3H7 is propyl
The dilution effect when the solutions mix. M1V1 = M2V2
Making sigma bonds and holding lone pairs
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

20. What are the names and formulas of the 6 strong acids?
proton donor base
RCOOR
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Insoluble except nitrate and acetate

21. How many ligands attach to a central ion in a complex ion?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
#ligands=charge x2
water and substances with (s) less dense than
S crystal at 0K=0

22. carbonates
They stay the same.
blue
Insoluble except group 1 and ammonium
Experimental mass/theoretical mass X 100

23. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
a-IMFs - b-molecular volume
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
?G= -ve - E°= +ve

24. sulfate
fractional distillation
boiling without losing volatile solvents/reactants
SO4²?
CN?

25. What is the formula for alkynes?
S2O3²?
CnH2n-2
proton acceptor.
Salt + water.

26. 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?
-Ea/R
Greenish-yellow gas
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
benzene has a delocalized pi ring structure

27. sulfates
Soluble except Ag - Pb - Ca - Sr Ba)
K1 x K2
Selective absorption
C2O4²?

28. What are two substances that sublime at 1 atm when heated?
Insoluble except group 1 and ammonium
Iodine and CO2 (dry ice)
CH3COO?
CO2 and H2O

29. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
An active metal.

30. What do nonmetal oxides plus water form?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
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)
acids
linear

31. What are amphoteric oxides?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Add acid to water so that the acid doesn't boil and spit
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?)

32. What type of polymer is nylon?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
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)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Synthetic condensation polymer (aka a polyamide)

33. What do metal oxides plus non- metal oxides form?
same KE - but PEice<PEwater
Salts (ex: CaO + SO2 ? CaSO3)
Disulfur dichloride
Q=It (time in seconds)

34. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
How close results are to the accepted value
neutralization: high K - H2O product dissociation: low K - H2O reactant
Pour liquids using a funnel or down a glass rod
Salt + water.

35. phosphate
PO4³?
NH2?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Heat a test tube at an angle at the side of the tube (not bottom)

36. Alkanes are _________ and react by _________
A salt solution.
Saturated - Substitution (which requires more radical conditions)
bright yellow
All except for lithium

37. chlorate
ClO3?
Q=It (time in seconds)
Increases.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

38. What type of metals don't react with water or acids to form H2?

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39. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
All except for lithium
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

40. If Q < Ksp a ppt ______
Mn²? - Cr³? - Cr³
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Ppt will NOT form (unsaturated)
red - green - blue

41. What kind of bonding structure does benzene have?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
E=q + w (negative is by system - positive is on system)
bases
benzene has a delocalized pi ring structure

42. What are the common strong bases?
no - they're written undissociated (HAaq)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
zero
Group 1 hydroxides (ex: NaOH)

43. permanganate
'non-active' metals such as Cu - Ag - Au - Pt - etc.
But S° of element is not zero (except at 0K)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
MnO4?

44. What is the formula for summation?

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45. During a titration what is present in the beaker at the equivalence point?
A salt solution.
water and substances with (s) less dense than
metal oxides and hydrides are ionically bonded and basic
strong acids/bases are written as H+ or OH- ions

46. What do group I/II metal oxides and acids form?
Salt and water
The benzene ring (or more correctly the phenyl group - C6H5)
Iodine and CO2 (dry ice)
Time?¹ - (ex. s?¹ - hr?¹ - etc)

47. Color is due to ______ _______ of light.
Graduated cylinder
Selective absorption
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
basic

48. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Evaporation
#ligands=charge x2
Mono; di; tri; tetra; penta; hexa.
Ionic compounds

49. Do you use J or kJ for ?H - ?S - and ?G?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
But S° of element is not zero (except at 0K)
Ionic compounds
?H-kJ - ?S-J - ?G-kJ

50. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Glacial acetic acid
CnH(2n+2)
Products - reactants (except for BDE when it's reactants - products)