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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. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
do not change
The benzene ring (or more correctly the phenyl group - C6H5)
Evaporation

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

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3. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
it is lower and occurs over less sharp a range
CnH2n+1 often designated 'R' ex C3H7 is propyl
Mono; di; tri; tetra; penta; hexa.

4. What apparatus do you use to pour liquids?
Filtration
Pour liquids using a funnel or down a glass rod
neutralization: high K - H2O product dissociation: low K - H2O reactant
a-IMFs - b-molecular volume

5. Metal hydrides are _____ and form _______ and _______ when added to water
Check for air bubbles in the buret and remove the buret funnel from the buret
ionic and form hydrogen and hydroxide
MnO4?
zero

6. What is an Alkyl group?

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7. What is the formula for percent yield?
The benzene ring (or more correctly the phenyl group - C6H5)
Experimental mass/theoretical mass X 100
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?)
Mono; di; tri; tetra; penta; hexa.

8. How are non-metal oxides and hydrides bonded? are they acidic or basic?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Iodine and CO2 (dry ice)
non-metal oxides and hydrides are covalently bonded and are acidic.
K1 x K2

9. What is the general formula for alkyl halides?
RX
CN?
zero-th: decreases - first: constant - second: increases
OH- and NH3

10. Why are noble gases stable?
Acidified
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Soluble
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

11. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Add acid to water so that the acid doesn't boil and spit
a-IMFs - b-molecular volume
S2O3²?
?G=negative - E° must be positive

12. How do you identify which is oxidized or otherwise?
OH?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Add acid to water so that the acid doesn't boil and spit
linear

13. silver compounds
Reduction always takes place at the cathode (RED CAT) In both types of cell!
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.
Insoluble except for nitrate and acetate
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

14. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
zero
NH2?

15. What is the formula of copper (II) phosphate?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
SO4²?
Cu3(PO4)2
Insoluble except for nitrate and acetate

16. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
Kc=Kp
zero
HClO4
an oxidized and reduced substance

17. Do you use J or kJ for ?H - ?S - and ?G?
Saturated - Substitution (which requires more radical conditions)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
?H-kJ - ?S-J - ?G-kJ

18. iodine - iodine solution - iodine vapor
?G=negative - E° must be positive
How close results are to the accepted value
Silvery gray solid - brown - purple
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

19. Which value of R do you use for all energy and kinetics calculations?
[A?]/[HA] x 100 or [BH?]/[B] x 100
zero-th: decreases - first: constant - second: increases
zero
R=8.31 J/mol/K

20. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Insoluble (except group 1 ammonium and Ba)
Pale purple - (orange)-yellow - red - blue - green.
Trigonal pyramidal
are less dense than water

21. Does reactivity increase/decrease going down group 1 and group 17?
Current - time and charge on ion (moles of e used in half cell reaction)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
it reacts by substitution NOT addition
Increases down group 1 decreases down group 17

22. bromothymol
blue (BTB)
benzene is less reactive than alkenes
Group I metals (soft metals) are stored under oil
They stay the same.

23. Is the standard entropy (S°) of an element zero?
But S° of element is not zero (except at 0K)
Combine the equations for the half reactions in the non-spontaneous direction
do not change
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

24. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
C2O4²?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Salt + water

25. 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
Concentration
basic
S crystal at 0K=0

26. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
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)
zero

27. What is the formula of butane?
q=mc?T q=mL (or n x ?h)
Increases down group 1 decreases down group 17
Insoluble except nitrate and acetate
C4H10

28. potassium permanganate
A salt solution.
R=8.31 J/mol/K
Purple
CN?

29. sulfates
Big K=kf/kr
Soluble except Ag - Pb - Ca - Sr Ba)
NH4?
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?)

30. The definition of acidic basic and neutral aqueous solutions is:
H2PO4?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Ppt will NOT form (unsaturated)
O2 needs 4F/mol H2 needs 2F/mol

31. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
same KE - but PEice<PEwater
How grouped results are
CnH2n-2

32. What is reflux?
Sigma bonds are stronger than pi bonds
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
boiling without losing volatile solvents/reactants
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

33. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
brown volatile liquid
PO4³?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Eudiometer

34. What measuring device would you use for very small volumes of liquids?
More chaotic (ex: gases made)
Combine the equations for the half reactions in the non-spontaneous direction
Pipette (burette if need repetition)
It ceases - the circuit is broken.

35. What is the name of S2Cl2? (Know how to name others like this - too)
CrO4²?
Ppt will NOT form (unsaturated)
ClO2?
Disulfur dichloride

36. What shape is carbon dioxide?
CrO4²?
linear
RCOOR
Ksp = 108s5

37. What element is used to vulcanize rubber?
Sulfur
Conjugate pair (one must be a weak base or acid)
fruit - fish - bases
Hg2²?

38. What is the general formula of an alkane?
Silvery gray solid - brown - purple
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
CnH(2n+2)
CO (poisonous)

39. carbonates
no - they're written undissociated (HAaq)
Increases.
Insoluble except group 1 and ammonium
non-metal oxides and hydrides are covalently bonded and are acidic.

40. What is the pH of 1.0M HCl? 1M NaOH?
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?)
Check for air bubbles in the buret and remove the buret funnel from the buret
K2
0 and 14

41. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
CN?
Pale purple - (orange)-yellow - red - blue - green.
Q=It (time in seconds)

42. What causes the dramatic effect of T on rate?
Transition element compounds (except if it has a full or empty d shell)
?H-kJ - ?S-J - ?G-kJ
T increases exponentially the proportion of molecules with E > Ea
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

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

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44. Ions are not ______.
The dilution effect when the solutions mix. M1V1 = M2V2
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
atoms
RCOOR

45. What is Big K in terms of kf and kr?
Big K=kf/kr
Purple
?G= -ve - E°= +ve
RCOOR

46. Which would cause the bulb in a conductivity apparatus to be brightest?
Synthesis - separation and purification of the product and its identification.
0.10M HCl (more ions)
An active metal.
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)

47. hypochlorite
ClO?
blue (BTB)
|experimental - accepted|/accepted X 100
HClO4

48. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Filtration
NO3?
Current - time and charge on ion (moles of e used in half cell reaction)
Sigma bonds are stronger than pi bonds

49. permanganate
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Separating funnel
Insoluble except group 1 and ammonium
MnO4?

50. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Insoluble (except group 1 ammonium and Ba)
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?)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp