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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. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
voltaic: + electrolytic: -
Iodine and CO2 (dry ice)
bent

2. Color is due to ______ _______ of light.
Selective absorption
water and substances with (s) less dense than
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
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

3. What effect does increasing the size/surface area of a voltaic cell have on the cell?
bent
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Heptane
Increases.

4. What is the difference between equivalence point and end point of a titration.
Nothing
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
Acid rain - dissolves marble buildings/statues and kills trees.
CO2 and H2O

5. Which alkali metals float on water?
it reacts by substitution NOT addition
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.
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)
All except for lithium

6. What is the general formula for alkyl halides?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Mn²? - Cr³? - Cr³
RX
The one with most oxygen atoms (highest oxidation number)

7. What is the first law of thermodynamics?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Pour liquids using a funnel or down a glass rod
E=q + w (negative is by system - positive is on system)
But S° of element is not zero (except at 0K)

8. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
?H formation of an element in standard state=0
water and substances with (s) less dense than

9. What do hydrocarbons form when they burn in air (oxygen)?
Sulfur
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Glacial acetic acid
CO2 and H2O

10. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
bright yellow
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
The dilution effect when the solutions mix. M1V1 = M2V2

11. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Acidified
Both electrons come from the same atom (just as good as a regular bond)
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)
Anode - oxygen. Cathode - hydrogen

12. What kind of bonding structure does benzene have?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
benzene has a delocalized pi ring structure
ClO4?
CH3COO?

13. lead compounds
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
?H formation of an element in standard state=0
Insoluble except nitrate and acetate
hydroxides (ex: Ba(OH)2)

14. What two types of substances are present in all redox reactions?
MnO4?
S crystal at 0K=0
an oxidized and reduced substance
OH?

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

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16. What type of compounds do metals/non metals form?
Ionic compounds
Insoluble except group 1 and ammonium
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
T increases exponentially the proportion of molecules with E > Ea

17. primary colors
How close results are to the accepted value
red - green - blue
it reacts by substitution NOT addition
CH3COO?

18. Esters smell like _______ and amines smell like _______ and are ______.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
fruit - fish - bases
bases
zero

19. Name some properties of Group 17
O2 needs 4F/mol H2 needs 2F/mol
left - ppt will form
ClO4?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

20. Ions are not ______.
atoms
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Initiation energy (NOT Ea)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

21. How do you get Ecell for spontaneous reactions?
E=q + w (negative is by system - positive is on system)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
CH3COO?
Soluble

22. What type of compounds are almost always colored?
Insoluble except for nitrate and acetate
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Transition element compounds (except if it has a full or empty d shell)
Mono; di; tri; tetra; penta; hexa.

23. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
Filtration
?G=negative - E° must be positive
Selective absorption

24. What do you do to get rid of most of the solution from a precipitate?
Decant
S2O3²?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
do not change

25. How many normal boiling points and boiling points are there?

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26. An amphiprotic (amphoteric) species is...
Suniverse increases for spontaneous processes
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

27. sulfates
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
K1 x K2
Soluble except Ag - Pb - Ca - Sr Ba)
boiling without losing volatile solvents/reactants

28. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
R=8.31 J/mol/K
Filtration
H+

29. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Salt + water.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Decant
RCOR

30. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
#ligands=charge x2
The dilution effect when the solutions mix. M1V1 = M2V2
yellow
White precipitate

31. Which value of R do you use for all energy and kinetics calculations?
Kc=Kp
But S° of element is not zero (except at 0K)
Salt + water.
R=8.31 J/mol/K

32. What device would you use to measure a volume of gas?
chemically (ex: with carbon)
ion pairing
voltaic: + electrolytic: -
Eudiometer

33. 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?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
The compound with the lowest Ksp value.
Increases down group 1 decreases down group 17
At half equivalence - pH=pKa

34. oxalate
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
H3PO4
Group 1 hydroxides (ex: NaOH)
C2O4²?

35. What measuring device would you use for very small volumes of liquids?
RCOOR
Pipette (burette if need repetition)
NH4?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

36. Is the ?H formation of an element in standard state zero?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
by electrolysis
?H formation of an element in standard state=0
Pale yellow

37. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Big K=kf/kr
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
metal oxides and hydrides are ionically bonded and basic

38. carbonate
CO3²?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
methyl formate
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

39. What is the charge on a chlorine atom?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Mono; di; tri; tetra; penta; hexa.
yellow
zero

40. What is H2CO3 (carbonate acid) usually written as?
Glowing splint (positive result=relights)
Mono; di; tri; tetra; penta; hexa.
H2O + CO2 (it decomposes readily)
it's lower and occurs over less sharp a range

41. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
acids
They decrease (or could be the same if the solid has ONLY JUST disappeared)
same KE - but PEice<PEwater

42. bromine
More chaotic (ex: gases made)
brown volatile liquid
non-metal oxides and hydrides are covalently bonded and are acidic.
look for changes in oxidation # - the one that goes up is oxidized and is the RA

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

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44. What is the conjugate base of NH3?
NH2?
+4-covalent - +2-ionic
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Anode

45. Acids + Carbonates (bicarbonates) make?
CN?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
C4H10
Sigma bonds are stronger than pi bonds

46. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
They stay the same.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Ksp = 4s³
#ligands=charge x2

47. chlorite
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Disulfur dichloride
ClO2?
voltaic: - electrolytic: +

48. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
No - it depends on the number of ions produced on dissolving.
E=q + w (negative is by system - positive is on system)
bright yellow

49. hydroxide
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Insoluble except for nitrate and acetate
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
OH?

50. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Current - time and charge on ion (moles of e used in half cell reaction)
Big K=kf/kr