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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 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?
Separating funnel
zero
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
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

2. perchlorate
H2PO4?
ClO4?
Clear
boiling without losing volatile solvents/reactants

3. Which value of R do you use for all energy and kinetics calculations?
metal oxides and hydrides are ionically bonded and basic
R=8.31 J/mol/K
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
C4H10

4. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
The dilution effect when the solutions mix. M1V1 = M2V2
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
It ceases - the circuit is broken.

5. What shape is water?
bent
The one with most oxygen atoms (highest oxidation number)
Current - time and charge on ion (moles of e used in half cell reaction)
basic

6. What is the test for oxygen?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
left - ppt will form
Glowing splint (positive result=relights)
are less dense than water

7. For a dibasic acid (H2A) - [A²?]= ____ ?
Eudiometer
hydroxides (ex: Ba(OH)2)
H2O + CO2 (it decomposes readily)
K2

8. What apparatus do you use to pour liquids?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
an oxidized and reduced substance
Pour liquids using a funnel or down a glass rod
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

9. silver iodide
Pale yellow
hydroxides (ex: Ba(OH)2)
Concentration
CrO4²?

10. What is the general formula for an ester?
H2PO4?
RCOOR
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
0 and 14

11. Does Kw increase or decrease with T? Why?
ROR
Pour liquids using a funnel or down a glass rod
+4-covalent - +2-ionic
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

12. What do you do to get rid of most of the solution from a precipitate?
Decant
Separating funnel
left - ppt will form
CH3COO?

13. Acids + Carbonates (bicarbonates) make?
[A?]/[HA] x 100 or [BH?]/[B] x 100
zero
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
it's lower and occurs over less sharp a range

14. What do you need to make a polymer?
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)
O2 needs 4F/mol H2 needs 2F/mol
No - NH3 and HCl gases are extremely soluble
How close results are to the accepted value

15. What value of R do you use for thermo calculations? gas calculations?
White precipitate
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
CnH2n+2
Salt + water

16. How do you get the equation for a net electrolysis reaction?
?G= -ve - E°= +ve
methyl formate
Combine the equations for the half reactions in the non-spontaneous direction
Monomer + monomer = polymer product + a simple molecule such as water or HCl

17. What shape is methane?
CO2 and H2O
Combine the equations for the half reactions in the non-spontaneous direction
Tetrahedral
Clear

18. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
voltaic: + electrolytic: -
ClO3?
Heat a test tube at an angle at the side of the tube (not bottom)

19. hypochlorite
MnO4?
Filtration
RCOOH
ClO?

20. Metal hydrides are _____ and form _______ and _______ when added to water
P2O5
linear
ionic and form hydrogen and hydroxide
CnH2n+2

21. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Kc=Kp
NO3?

22. What is the conjugate acid of H2PO4?
H3PO4
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Initiation energy (NOT Ea)
CH3COO?

23. dichromate
Mono; di; tri; tetra; penta; hexa.
Hg²?
Experimental mass/theoretical mass X 100
Cr2O7²?

24. chromate
ClO?
CrO4²?
Distillation
same KE - but PEice<PEwater

25. Why are i factors (Van't Hoff factors) often less than ideal?
At half equivalence - pH=pKa
ion pairing
SO4²?
No - NH3 and HCl gases are extremely soluble

26. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Ksp = 108s5
Both electrons come from the same atom (just as good as a regular bond)
Distillation
a-IMFs - b-molecular volume

27. oxalate
Orange
red - green - blue
zero
C2O4²?

28. What is the formula for alkenes?
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)
Hg2²?
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
CnH2n

29. What things should you remember to do when collecting gas over water?
Glowing splint (positive result=relights)
non-metal oxides and hydrides are covalently bonded and are acidic.
blue (BTB)
allow for the vapor pressure of water and make sure to level levels

30. What is the formula of butane?
Orange
C4H10
How grouped results are
Acids; HCOOCH3 is an ester

31. How does group 1 metals' density compare to water's?
Soluble
CnH2n+1 often designated 'R' ex C3H7 is propyl
K2
are less dense than water

32. Does Benzene react by addition or substitution?
10?8
No - NH3 and HCl gases are extremely soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
it reacts by substitution NOT addition

33. 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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34. What are the formulas for q?
ion pairing
Add acid to water so that the acid doesn't boil and spit
ClO4?
q=mc?T q=mL (or n x ?h)

35. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Exothermic
Insoluble except nitrate and acetate
S crystal at 0K=0
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

36. Color is due to ______ _______ of light.
Selective absorption
RNH2
No - it depends on the number of ions produced on dissolving.
Current - time and charge on ion (moles of e used in half cell reaction)

37. What do group I/II metal oxides plus water form?
ethers
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Only temperature
bases

38. phosphate
PO4³?
red - green - blue
CO (poisonous)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

39. What element is used to vulcanize rubber?
Sulfur
Acids; HCOOCH3 is an ester
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Add acid to water so that the acid doesn't boil and spit

40. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
HClO4
CnH2n-2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Current - time and charge on ion (moles of e used in half cell reaction)

41. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
basic
Ksp = 108s5
ns² electrons (first in-first out)

42. What is the general formula for an aldehyde?
Acid rain - dissolves marble buildings/statues and kills trees.
H3PO4
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
RCHO (carbonyl at end)

43. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
Soluble
Purple
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

44. What process do you use to obtain the precipitate from a solution?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CnH2n+1 often designated 'R' ex C3H7 is propyl
Filtration
neutralization: high K - H2O product dissociation: low K - H2O reactant

45. Esterification is...
No - NH3 and HCl gases are extremely soluble
no - they're written undissociated (HAaq)
Cu3(PO4)2
acid + alcohol

46. How do you compute % dissociation?
CnH2n-2
Salt + water.
H2PO4?
[A?]/[HA] x 100 or [BH?]/[B] x 100

47. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
zero-th: decreases - first: constant - second: increases
blue
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
neutralization: high K - H2O product dissociation: low K - H2O reactant

48. When driving off water from a hydrate - how do you tell you're done?
The dilution effect when the solutions mix. M1V1 = M2V2
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Molecules with the same molecular formulas - but different structural formulas
ionic and form hydrogen and hydroxide

49. What are the common strong bases?
They stay the same.
Check for air bubbles in the buret and remove the buret funnel from the buret
it reacts by substitution NOT addition
Group 1 hydroxides (ex: NaOH)

50. 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
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
H2PO4?
Read the bottom of the meniscus