Test your basic knowledge |

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. A geometric (or cis-trans) isomer exists due to.....
CnH2n
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
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.
linear

2. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
it's lower and occurs over less sharp a range
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Molecules with the same molecular formulas - but different structural formulas

3. What is the formula for percent error?
|experimental - accepted|/accepted X 100
q=mc?T q=mL (or n x ?h)
S2O3²?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

4. What is the test for hydrogen?
OH- and NH3
lighted splint (positive result=pop)
Check for air bubbles in the buret and remove the buret funnel from the buret
Pipette (burette if need repetition)

5. Name 2 ways in which you can create a buffer?
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)
Salts (ex: CaO + SO2 ? CaSO3)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
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)

6. Lattice energy is high for ions with _____ size and _____ charge
ionic and form hydrogen and hydroxide
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
small size and high charge
Iodine and CO2 (dry ice)

7. What is the sign of the cathode in voltaic cells? in electrolytic cells?
S crystal at 0K=0
Anode - oxygen. Cathode - hydrogen
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)
voltaic: + electrolytic: -

8. Do anions flow to the cathode or anode?
CO3²?
Anode
Molecules with the same molecular formulas - but different structural formulas
bent

9. chlorite
More chaotic (ex: gases made)
ClO2?
brown volatile liquid
blue glass - it filters UV

10. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Pale yellow
Combine the equations for the half reactions in the non-spontaneous direction
a-IMFs - b-molecular volume
Mn²? - Cr³? - Cr³

11. ammonium/ammonium compounds
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
ion pairing
are less dense than water
Soluble

12. How does half life change for zero-th order - first order - and second order processes?
H3PO4
RNH2
zero-th: decreases - first: constant - second: increases
water and substances with (s) less dense than

13. What are the common strong bases?
Ppt will NOT form (unsaturated)
do not change
Group 1 hydroxides (ex: NaOH)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

14. Why are i factors (Van't Hoff factors) often less than ideal?
acids
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
ion pairing
O2 needs 4F/mol H2 needs 2F/mol

15. Name some properties of Group 17
ethers
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Unsaturated - addition (ex: decolorize bromine solution)
Hg2²?

16. What is the general formula for an amine?
CnH(2n+2)
RNH2
blue glass - it filters UV
T increases exponentially the proportion of molecules with E > Ea

17. Does reactivity increase/decrease going down group 1 and group 17?
strong acids/bases are written as H+ or OH- ions
allow for the vapor pressure of water and make sure to level levels
Increases down group 1 decreases down group 17
it is lower and occurs over less sharp a range

18. What is Big K in terms of kf and kr?
Increases.
NH2?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Big K=kf/kr

19. chromate
CrO4²?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
it's lower and occurs over less sharp a range
ClO4?

20. When a cell is 'flat' What is its voltage?
Disulfur dichloride
zero-th: decreases - first: constant - second: increases
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
zero

21. copper sulfate
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
?G=negative - E° must be positive
blue
Insoluble

22. What is reflux?
bright yellow
A salt solution.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
boiling without losing volatile solvents/reactants

23. What is the general formula for an alcohol?
Acid rain - dissolves marble buildings/statues and kills trees.
ROH
Pale yellow
Mn²? - Cr³? - Cr³

24. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Soluble
0.10M HCl (more ions)

25. What does a short - sharp melting point indicate?
Cu3(PO4)2
?H formation of an element in standard state=0
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Identity and purity (impure compounds usually have broad & low melting points)

26. Acids + Carbonates (bicarbonates) make?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Pour liquids using a funnel or down a glass rod
RCHO (carbonyl at end)

27. carbonate
Purple
Iodine and CO2 (dry ice)
Concentration
CO3²?

28. What two types of substances are present in all redox reactions?
H2O + CO2 (it decomposes readily)
an oxidized and reduced substance
They stay the same.
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?)

29. What is the general formula for an acid?
Salt and water
RCOOH
ROR
At half equivalence - pH=pKa

30. What is the charge on a chlorine atom?
Decant
The compound with the lowest Ksp value.
zero
?G= -ve - E°= +ve

31. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Kc=Kp
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

32. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
H2O + CO2 (it decomposes readily)
zero
basic
CO (poisonous)

33. iodine - iodine solution - iodine vapor
CnH(2n+2)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Silvery gray solid - brown - purple
metal oxides and hydrides are ionically bonded and basic

34. During a titration what is present in the beaker at the equivalence point?
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)
S crystal at 0K=0
A salt solution.
Unsaturated - addition (ex: decolorize bromine solution)

35. What is precision?
R=8.31 J/mol/K
water and substances with (s) less dense than
How grouped results are
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

36. What process do you use to obtain a solvent from a solution?
Distillation
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)
Identity and purity (impure compounds usually have broad & low melting points)
Big K=kf/kr

37. What is accuracy?
Mono; di; tri; tetra; penta; hexa.
The one with most oxygen atoms (highest oxidation number)
How close results are to the accepted value
different forms of the same element

38. What are two substances that sublime at 1 atm when heated?
S crystal at 0K=0
Increases.
Iodine and CO2 (dry ice)
left - ppt will form

39. What is the second law of thermodynamics?
Heptane
Suniverse increases for spontaneous processes
by electrolysis
Soluble

40. What is the name of S2Cl2? (Know how to name others like this - too)
Check for air bubbles in the buret and remove the buret funnel from the buret
Pipette (burette if need repetition)
ion pairing
Disulfur dichloride

41. What shape is ammonia?
methyl formate
0.10M HCl (more ions)
Trigonal pyramidal
OH?

42. What are the names and formulas of the 6 strong acids?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Increases.
RCOOR

43. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
it reacts by substitution NOT addition
Group I metals (soft metals) are stored under oil
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

44. Give an example of a dilute strong acid.
Acid rain - dissolves marble buildings/statues and kills trees.
Nothing
HClO4
Soluble except Ag - Pb - Ca - Sr Ba)

45. 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?
Experimental mass/theoretical mass X 100
The compound with the lowest Ksp value.
Distillation
R=8.31 J/mol/K

46. ammonium
+4-covalent - +2-ionic
NH4?
Synthetic condensation polymer (aka a polyamide)
Decant

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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

48. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
H+
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

49. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
The dilution effect when the solutions mix. M1V1 = M2V2
Salt + water
+4-covalent - +2-ionic
White precipitate

50. Are weak acids (and bases) written dissociated?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183