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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.
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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 do you identify which is oxidized or otherwise?
CH3COO?
C2O4²?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Anode - oxygen. Cathode - hydrogen

2. What do you use to look at burning magnesium? why?
Suniverse increases for spontaneous processes
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Soluble
blue glass - it filters UV

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

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4. Do you use J or kJ for ?H - ?S - and ?G?
acid + alcohol
?H-kJ - ?S-J - ?G-kJ
it reacts by substitution NOT addition
Current - time and charge on ion (moles of e used in half cell reaction)

5. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
|experimental - accepted|/accepted X 100
10?8
Saturated - Substitution (which requires more radical conditions)
ion pairing

6. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
A salt solution.
Decant
zero

7. Metal hydrides are _____ and form _______ and _______ when added to water
diamond and graphite
ionic and form hydrogen and hydroxide
red - green - blue
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

8. What is Big K in terms of kf and kr?
Identity and purity (impure compounds usually have broad & low melting points)
Increases down group 1 decreases down group 17
Big K=kf/kr
basic

9. dihydrogen phosphate
|experimental - accepted|/accepted X 100
RCOOR
H2PO4?
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

10. How do you get the equation for a net electrolysis reaction?
O2 needs 4F/mol H2 needs 2F/mol
Combine the equations for the half reactions in the non-spontaneous direction
RCHO (carbonyl at end)
Glacial acetic acid

11. What is the formula of butane?
Molecules with the same molecular formulas - but different structural formulas
C4H10
K1 x K2
hydroxides (ex: Ba(OH)2)

12. If a free element is involved - what type of reaction must be involved?
Initiation energy (NOT Ea)
redox reaction
Anode - oxygen. Cathode - hydrogen
Perform ICE BOX calculation based on K1

13. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
10?8
?G=negative - E° must be positive
Salts (ex: CaO + SO2 ? CaSO3)

14. Acid plus base make?
Hg2²?
ClO?
Salt + water.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

15. What reacts with an acid to create hydrogen gas?
An active metal.
CnH2n+2
Time?¹ - (ex. s?¹ - hr?¹ - etc)
red - green - blue

16. What does the solubility of organic compounds depend on?
do not change
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)
P2O5
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

17. What changes Keq?
NO3?
Only temperature
water and substances with (s) less dense than
a-IMFs - b-molecular volume

18. How do you dilute an acid?

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19. If ?S is positive - are the products more or less chaotic than the reactants?
strong acids/bases are written as H+ or OH- ions
Insoluble (except group 1 ammonium and Ba)
More chaotic (ex: gases made)
Greenish-yellow gas

20. 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
bright yellow
Increases.
fruit - fish - bases

21. What is the general formula for an amine?
OH- and NH3
Ksp = 4s³
ionic and form hydrogen and hydroxide
RNH2

22. Color is due to ______ _______ of light.
Selective absorption
Disulfur dichloride
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
H2O + CO2 (it decomposes readily)

23. What is the test for oxygen?
RX
Molecules with the same molecular formulas - but different structural formulas
Glowing splint (positive result=relights)
zero

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

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25. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Synthetic condensation polymer (aka a polyamide)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

26. Can you collect soluble gases over water?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
No - NH3 and HCl gases are extremely soluble
Insoluble except nitrate and acetate
boiling without losing volatile solvents/reactants

27. What two compounds are great oxidizing agents?

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28. For a dibasic acid (H2A) - [A²?]= ____ ?
basic
It ceases - the circuit is broken.
K2
RCOOR

29. Esters smell like _______ and amines smell like _______ and are ______.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
fruit - fish - bases
same KE - but PEice<PEwater
Sulfur

30. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
More chaotic (ex: gases made)
zero
Products - reactants (except for BDE when it's reactants - products)
Ksp = 27s4

31. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
basic
10?8
an oxidized and reduced substance

32. acetates
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Soluble
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
C4H10

33. What is H2CO3 (carbonate acid) usually written as?
it's lower and occurs over less sharp a range
Anode - oxygen. Cathode - hydrogen
H2O + CO2 (it decomposes readily)
Insoluble

34. When driving off water from a hydrate - how do you tell you're done?
Combine the equations for the half reactions in the non-spontaneous direction
brown volatile liquid
E=q + w (negative is by system - positive is on system)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

35. 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
Tetrahedral
Time?¹ - (ex. s?¹ - hr?¹ - etc)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

36. What do you use for an acid spill? base spill?
do not change
proton acceptor.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
E=q + w (negative is by system - positive is on system)

37. What are the common strong bases?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
The benzene ring (or more correctly the phenyl group - C6H5)
Group 1 hydroxides (ex: NaOH)

38. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Transition element compounds (except if it has a full or empty d shell)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Current - time and charge on ion (moles of e used in half cell reaction)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

39. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
CO2 and H2O
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Kc=Kp
water and substances with (s) less dense than

40. A geometric (or cis-trans) isomer exists due to.....
Pour liquids using a funnel or down a glass rod
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
methyl formate
voltaic: - electrolytic: +

41. lead iodide
Experimental mass/theoretical mass X 100
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
allow for the vapor pressure of water and make sure to level levels
bright yellow

42. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Experimental mass/theoretical mass X 100
HClO4
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

43. nitrates
it is lower and occurs over less sharp a range
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Soluble
Saturated - Substitution (which requires more radical conditions)

44. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Most are soluble except Ag - Pb
same KE - but PEice<PEwater
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Initiation energy (NOT Ea)

45. What do hydrocarbons form when they burn in air (oxygen)?
CO2 and H2O
The compound with the lowest Ksp value.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
allow for the vapor pressure of water and make sure to level levels

46. What is the general formula for an acid?
Ksp = s²
RCOOH
basic
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

47. What are the signs of ?G and E° for spontaneous reactions?
acid + alcohol
?G=negative - E° must be positive
Q=It (time in seconds)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

48. How many ligands attach to a central ion in a complex ion?
by electrolysis
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
neutralization: high K - H2O product dissociation: low K - H2O reactant
#ligands=charge x2

49. What do acids plus active metals form?
Acidified
Kc=Kp
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

50. How are more active metals reduced?
by electrolysis
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Ksp = 27s4
White precipitate

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AP Chemistry 2

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