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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. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
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-2
benzene has a delocalized pi ring structure
H+

2. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
boiling without losing volatile solvents/reactants
Ksp = 27s4
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

3. What is the slope of the graph of lnk vs. 1/T?
Group 1 hydroxides (ex: NaOH)
Perform ICE BOX calculation based on K1
-Ea/R
allow for the vapor pressure of water and make sure to level levels

4. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
benzene has a delocalized pi ring structure
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
neutralization: high K - H2O product dissociation: low K - H2O reactant
CrO4²?

5. How do you get Ecell for spontaneous reactions?
Increases down group 1 decreases down group 17
Products - reactants (except for BDE when it's reactants - products)
The compound with the lowest Ksp value.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

6. silver compounds
NH2?
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
Insoluble except for nitrate and acetate
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

7. What do metal oxides plus acids form?
water and substances with (s) less dense than
Insoluble
Salt + water
hydroxides (ex: Ba(OH)2)

8. What is the formula of copper (II) phosphate?
diamond and graphite
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.
Cu3(PO4)2
T increases exponentially the proportion of molecules with E > Ea

9. Where are group I metals stored?
different forms of the same element
The Faraday or Faraday's constant.
Group I metals (soft metals) are stored under oil
CnH2n

10. dichromate (soln + most solids)
CO (poisonous)
Orange
allow for the vapor pressure of water and make sure to level levels
It ceases - the circuit is broken.

11. carbonate
basic
redox reaction
CO3²?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

12. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Nothing
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Evaporation
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

13. What is the formula for alkynes?
Soluble
Pour liquids using a funnel or down a glass rod
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
CnH2n-2

14. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Big K=kf/kr
At half equivalence - pH=pKa
But S° of element is not zero (except at 0K)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

15. What is the general formula for an aldehyde?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
RCHO (carbonyl at end)
O2 needs 4F/mol H2 needs 2F/mol
E=q + w (negative is by system - positive is on system)

16. What is the sign of the anode in voltaic cells? in electrolytic cells?
Disulfur dichloride
0.10M HCl (more ions)
voltaic: - electrolytic: +
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

17. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
fruit - fish - bases
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Ppt will NOT form (unsaturated)
10?8

18. nitrates
acid + alcohol
small size and high charge
Soluble
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

19. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Ksp = 108s5
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
CnH2n+2

20. How many faradays of electric charge do you need to produce one mole of O2? H2?
Salts (ex: CaO + SO2 ? CaSO3)
bright yellow
O2 needs 4F/mol H2 needs 2F/mol
Anode - oxygen. Cathode - hydrogen

21. mercury (II) ion
Hg²?
are less dense than water
Ions go through the salt bridge - electrons go through metal wires in the external circuit
lighted splint (positive result=pop)

22. primary colors
water and substances with (s) less dense than
red - green - blue
0.10M HCl (more ions)
Read the bottom of the meniscus

23. lead iodide
linear
bright yellow
A) any range. b) 8-10 c) 4-6
it's lower and occurs over less sharp a range

24. What type of compounds are almost always colored?
Separating funnel
No - NH3 and HCl gases are extremely soluble
Transition element compounds (except if it has a full or empty d shell)
'non-active' metals such as Cu - Ag - Au - Pt - etc.

25. What is the general formula for an acid?
CnH2n+2
RCOOH
Iodine and CO2 (dry ice)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

26. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

27. What does the solubility of organic compounds depend on?
acid + alcohol
diamond and graphite
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Kc=Kp

28. What is the formula for percent error?
it is lower and occurs over less sharp a range
-Ea/R
|experimental - accepted|/accepted X 100
Most INsoluble except group 1 and ammonium

29. Is a graduated cylinder or beaker more accurate?
Synthetic condensation polymer (aka a polyamide)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
CO (poisonous)
Graduated cylinder

30. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
ion pairing
hydroxides (ex: Ba(OH)2)
zero

31. What is the name of S2Cl2? (Know how to name others like this - too)
zero
allow for the vapor pressure of water and make sure to level levels
Disulfur dichloride
H2O + CO2 (it decomposes readily)

32. The oxidation # for acid base reactions...
Molecules with the same molecular formulas - but different structural formulas
do not change
Most INsoluble except group 1 and ammonium
small size and high charge

33. What do metal oxides plus non- metal oxides form?
Clear
Evaporation
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Salts (ex: CaO + SO2 ? CaSO3)

34. What is the charge on a chlorine atom?
zero
It ceases - the circuit is broken.
Ppt will NOT form (unsaturated)
H3PO4

35. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
CnH2n+2
brown volatile liquid
bright yellow

36. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
ClO3?
Big K=kf/kr
'non-active' metals such as Cu - Ag - Au - Pt - etc.

37. copper sulfate
P2O5
strong acids/bases are written as H+ or OH- ions
[A?]/[HA] x 100 or [BH?]/[B] x 100
blue

38. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
How close results are to the accepted value
Disulfur dichloride
ionic and form hydrogen and hydroxide
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

39. What is the formula for alkenes?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
same KE - but PEice<PEwater
Initiation energy (NOT Ea)
CnH2n

40. What two types of substances are present in all redox reactions?
brown volatile liquid
an oxidized and reduced substance
Hg2²?
Pipette (burette if need repetition)

41. Esters smell like _______ and amines smell like _______ and are ______.
Concentration
fruit - fish - bases
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)
lighted splint (positive result=pop)

42. chlorite
Insoluble (except group 1 ammonium and Ba)
Iodine and CO2 (dry ice)
Pale purple - (orange)-yellow - red - blue - green.
ClO2?

43. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Insoluble except nitrate and acetate
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
bright yellow

44. What do group I/II metal oxides and acids form?
Anode - oxygen. Cathode - hydrogen
Salt and water
Evaporation
Filtration

45. What is accuracy?
do not change
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
How close results are to the accepted value
They stay the same.

46. What is HCOOCH3?
Acids; HCOOCH3 is an ester
White precipitate
are less dense than water
No - it depends on the number of ions produced on dissolving.

47. What do hydrocarbons form when they burn in air (oxygen)?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
CO2 and H2O
Tetrahedral
Ksp = 27s4

48. ________ are Lewis bases - because they can donate a lone pair of electrons.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
OH- and NH3
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
How close results are to the accepted value

49. Color is due to ______ _______ of light.
+4-covalent - +2-ionic
0 and 14
Selective absorption
Iodine and CO2 (dry ice)

50. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
Purple
ethers
RCOR