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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. How does the melting point of a mixture compare to the MP of a pure substance?
Both electrons come from the same atom (just as good as a regular bond)
Heat a test tube at an angle at the side of the tube (not bottom)
it is lower and occurs over less sharp a range
?G= -ve - E°= +ve

2. Ca - Sr - Ba
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
hydroxides (ex: Ba(OH)2)
NO3?
CrO4²?

3. lead iodide
Q=It (time in seconds)
bright yellow
bent
methyl formate

4. dichromate (soln + most solids)
Salt + water.
fractional distillation
Orange
small size and high charge

5. primary colors
0.10M HCl (more ions)
It ceases - the circuit is broken.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
red - green - blue

6. What shape is water?
bent
Purple
The compound with the lowest Ksp value.
Initiation energy (NOT Ea)

7. 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?
#ligands=charge x2
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
H3PO4
catalyst=conc H2SO4

8. silver iodide
CN?
?H formation of an element in standard state=0
Pale yellow
voltaic: + electrolytic: -

9. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Hg2²?
T increases exponentially the proportion of molecules with E > Ea
Experimental mass/theoretical mass X 100
Anode - oxygen. Cathode - hydrogen

10. Esters smell like _______ and amines smell like _______ and are ______.
Soluble
CrO4²?
fruit - fish - bases
RX

11. 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?
Most are soluble except Ag - Pb
+4-covalent - +2-ionic
The compound with the lowest Ksp value.
Suniverse increases for spontaneous processes

12. cyanide
CN?
same KE - but PEice<PEwater
a-IMFs - b-molecular volume
K2

13. The oxidation # for acid base reactions...
Only temperature
bases
ethers
do not change

14. mercury (I) ion
Hg2²?
Filtration
S crystal at 0K=0
Exothermic

15. Ions are not ______.
atoms
Pale purple - (orange)-yellow - red - blue - green.
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?)
CnH(2n+2)

16. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
Salt and water
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
?H formation of an element in standard state=0

17. What do ions and electrons travel through in a voltaic/electrolytic cell?
Cu3(PO4)2
Ions go through the salt bridge - electrons go through metal wires in the external circuit
CO (poisonous)
At half equivalence - pH=pKa

18. 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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19. If a weak acid is diluted more - what happens to its % dissociation value?
it reacts by substitution NOT addition
no - they're written undissociated (HAaq)
Increases.
benzene is less reactive than alkenes

20. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
SO4²?
Glowing splint (positive result=relights)
a-IMFs - b-molecular volume

21. One mole of electrons carries 96500Coulombs - what is this quantity called?

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22. If Q > Ksp - then system shifts _______ and ppt ______
left - ppt will form
Both electrons come from the same atom (just as good as a regular bond)
Q=It (time in seconds)
NH4?

23. What changes Keq?
H2PO4?
Only temperature
Exothermic (?H for ANY sa/sb = -57kJ/mol)
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.

24. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pale purple - (orange)-yellow - red - blue - green.
Acidified
Silvery gray solid - brown - purple
Current - time and charge on ion (moles of e used in half cell reaction)

25. What is the test for hydrogen?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
lighted splint (positive result=pop)
Disulfur dichloride
Mono; di; tri; tetra; penta; hexa.

26. Is a graduated cylinder or beaker more accurate?
zero
Separating funnel
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Graduated cylinder

27. Neutralization is an ________ reaction.
Kc=Kp
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Iodine and CO2 (dry ice)

28. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
P2O5
No - it depends on the number of ions produced on dissolving.
red - green - blue
by electrolysis

29. BaSO4
do not change
Increases.
H2PO4?
Insoluble

30. What apparatus do you use to pour liquids?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Cr2O7²?
At half equivalence - pH=pKa
Pour liquids using a funnel or down a glass rod

31. What are hybrid orbitals used for?
blue
acid + alcohol
Making sigma bonds and holding lone pairs
E=q + w (negative is by system - positive is on system)

32. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
Cr2O7²?
ionic and form hydrogen and hydroxide
it reacts by substitution NOT addition
A) any range. b) 8-10 c) 4-6

33. A geometric (or cis-trans) isomer exists due to.....
Soluble
Ionic compounds
Glowing splint (positive result=relights)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

34. How does half life change for zero-th order - first order - and second order processes?
hydroxides (ex: Ba(OH)2)
water and substances with (s) less dense than
zero-th: decreases - first: constant - second: increases
Cr2O7²?

35. What does a short - sharp melting point indicate?
Pale purple - (orange)-yellow - red - blue - green.
E=q + w (negative is by system - positive is on system)
Increases.
Identity and purity (impure compounds usually have broad & low melting points)

36. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Cu3(PO4)2
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CrO4²?

37. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO3?
Insoluble except nitrate and acetate
More chaotic (ex: gases made)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

38. nitrates
Separating funnel
Soluble
Silvery gray solid - brown - purple
Synthesis - separation and purification of the product and its identification.

39. What are two allotropes of carbon?
All except for lithium
diamond and graphite
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

40. 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
zero
Add acid to water so that the acid doesn't boil and spit
Pale purple - (orange)-yellow - red - blue - green.

41. 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
zero
Sulfur
yellow

42. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Big K=kf/kr
boiling without losing volatile solvents/reactants
PO4³?

43. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
10?8
zero-th: decreases - first: constant - second: increases
bases
More chaotic (ex: gases made)

44. chromate
White precipitate
?G=negative - E° must be positive
CrO4²?
are less dense than water

45. Do anions flow to the cathode or anode?
Anode
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
No - NH3 and HCl gases are extremely soluble

46. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
H+
-Ea/R
fruit - fish - bases
Ksp = 27s4

47. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Soluble
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
diamond and graphite
fractional distillation

48. What process do you use to separate two liquids with different boiling points?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
ROH
+4-covalent - +2-ionic
fractional distillation

49. Is the freezing of ice endothermic or exothermic?
Sigma bonds are stronger than pi bonds
Insoluble except for nitrate and acetate
RCOOH
Exothermic

50. Generally - which oxy acid is strongest?
allow for the vapor pressure of water and make sure to level levels
Increases down group 1 decreases down group 17
Monomer + monomer = polymer product + a simple molecule such as water or HCl
The one with most oxygen atoms (highest oxidation number)