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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 are strong ones written?
H3PO4
strong acids/bases are written as H+ or OH- ions
are less dense than water
boiling without losing volatile solvents/reactants

2. chlorate
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
ClO3?
ClO2?
Acidified

3. nitrate
Purple
Graduated cylinder
At half equivalence - pH=pKa
NO3?

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

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5. What measuring device would you use for very small volumes of liquids?
A) any range. b) 8-10 c) 4-6
Pipette (burette if need repetition)
ROH
no - they're written undissociated (HAaq)

6. sulfates
ns² electrons (first in-first out)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Most are soluble except Ag - Pb
Soluble except Ag - Pb - Ca - Sr Ba)

7. What is the third law of thermodynamics?
CrO4²?
left - ppt will form
Pipette (burette if need repetition)
S crystal at 0K=0

8. What should you check for before you begin titrating?
Soluble
Conjugate pair (one must be a weak base or acid)
Check for air bubbles in the buret and remove the buret funnel from the buret
Suniverse increases for spontaneous processes

9. How does the melting point of a mixture compare to the MP of a pure substance?

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10. What are amphoteric oxides?
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)
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?)
ion pairing
MnO4?

11. How many faradays of electric charge do you need to produce one mole of O2? H2?
OH- and NH3
O2 needs 4F/mol H2 needs 2F/mol
acid + alcohol
zero

12. What do nonmetal oxides plus water form?
Conjugate pair (one must be a weak base or acid)
RX
Ksp = 4s³
acids

13. 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
an oxidized and reduced substance
H3PO4
Disulfur dichloride

14. What two compounds are great oxidizing agents?

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15. What device would you use to measure a volume of gas?
Acids; HCOOCH3 is an ester
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
Eudiometer
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

16. What are the signs of ?G and E° for spontaneous reactions?
?G=negative - E° must be positive
strong acids/bases are written as H+ or OH- ions
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
bases

17. What effect does increasing the size/surface area of a voltaic cell have on the cell?
a-IMFs - b-molecular volume
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
P2O5
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

18. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
voltaic: + electrolytic: -
Exothermic
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

19. acetate
H2PO4?
CH3COO?
Heptane
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

20. Aromatic compounds contain what?
No - NH3 and HCl gases are extremely soluble
The benzene ring (or more correctly the phenyl group - C6H5)
Big K=kf/kr
Time?¹ - (ex. s?¹ - hr?¹ - etc)

21. 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
Concentration
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Filtration

22. What is a dipeptide? polypeptide? protein?
+4-covalent - +2-ionic
The compound with the lowest Ksp value.
zero
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

23. perchlorate
All except for lithium
proton donor base
Insoluble
ClO4?

24. What do you use for an acid spill? base spill?
Synthetic condensation polymer (aka a polyamide)
chemically (ex: with carbon)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

25. What is the formula of butane?
CO (poisonous)
Transition element compounds (except if it has a full or empty d shell)
C4H10
E=q + w (negative is by system - positive is on system)

26. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Products - reactants (except for BDE when it's reactants - products)
Insoluble (except group 1 ammonium and Ba)
non-metal oxides and hydrides are covalently bonded and are acidic.
SO4²?

27. Which of the rates changes more when temperature is increased?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
[A?]/[HA] x 100 or [BH?]/[B] x 100
bent
neutralization: high K - H2O product dissociation: low K - H2O reactant

28. permanganate
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
MnO4?
ClO4?

29. What do you use to look at burning magnesium? why?
lighted splint (positive result=pop)
Ksp = 4s³
blue glass - it filters UV
CN?

30. What shape is water?
bent
Selective absorption
Soluble
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

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

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32. What is the general formula for an amine?
K1 x K2
Pale yellow
RNH2
hydroxides (ex: Ba(OH)2)

33. How do you heat a test tube?
Acids; HCOOCH3 is an ester
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Heat a test tube at an angle at the side of the tube (not bottom)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

34. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
red - green - blue
RCOOR
Mn²? - Cr³? - Cr³
Trigonal pyramidal

35. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
P2O5
Big K=kf/kr
+4-covalent - +2-ionic
CnH(2n+2)

36. Do anions flow to the cathode or anode?
C4H10
Anode
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Reduction always takes place at the cathode (RED CAT) In both types of cell!

37. oxalate
C2O4²?
?H formation of an element in standard state=0
NO3?
benzene has a delocalized pi ring structure

38. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
Orange
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
The dilution effect when the solutions mix. M1V1 = M2V2

39. ammonium
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
CrO4²?
Only temperature
NH4?

40. acetates
Soluble
Purple
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

41. silver iodide
They stay the same.
Insoluble (except group 1 ammonium and Ba)
Pale yellow
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

42. Does Kw increase or decrease with T? Why?
neutralization: high K - H2O product dissociation: low K - H2O reactant
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
NO3?
10?8

43. What is the formula for percent error?
zero
zero-th: decreases - first: constant - second: increases
Hg2²?
|experimental - accepted|/accepted X 100

44. Color is due to ______ _______ of light.
H2PO4?
Selective absorption
CnH(2n+2)
ionic and form hydrogen and hydroxide

45. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
allow for the vapor pressure of water and make sure to level levels
Making sigma bonds and holding lone pairs
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

46. ________ are Lewis bases - because they can donate a lone pair of electrons.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
OH- and NH3
Distillation
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

47. 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
Reduction always takes place at the cathode (RED CAT) In both types of cell!
lighted splint (positive result=pop)
Heat a test tube at an angle at the side of the tube (not bottom)

48. When is ?G zero?
H3PO4
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
red - green - blue
C4H10

49. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
Greenish-yellow gas
Ionic compounds
metal oxides and hydrides are ionically bonded and basic

50. What do metal oxides plus acids form?
Salt + water
ethers
CO (poisonous)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).