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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. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
?H formation of an element in standard state=0
The dilution effect when the solutions mix. M1V1 = M2V2
acid + alcohol
left - ppt will form

2. If Q < Ksp a ppt ______
It ceases - the circuit is broken.
Ppt will NOT form (unsaturated)
acid + alcohol
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

3. What are the signs of ?G and E° for spontaneous reactions?
?G=negative - E° must be positive
blue glass - it filters UV
zero
CnH2n-2

4. What is the formula for alkynes?
Purple
CnH2n-2
ClO3?
allow for the vapor pressure of water and make sure to level levels

5. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
zero
neutralization: high K - H2O product dissociation: low K - H2O reactant
ClO4?

6. Acid plus base make?
fruit - fish - bases
Cu3(PO4)2
diamond and graphite
Salt + water.

7. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
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)
atoms

8. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
SO4²?
yellow
Ionic compounds

9. Do anions flow to the cathode or anode?
left - ppt will form
Soluble
water and substances with (s) less dense than
Anode

10. What is the formula for obtaining charge flowing in a cell?
Insoluble except nitrate and acetate
C2O4²?
Q=It (time in seconds)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

11. Both Acetic acid and ____________ are also functional isomers.
Clear
Filtration
methyl formate
hydroxides (ex: Ba(OH)2)

12. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Kc=Kp
Pale yellow
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Insoluble (except group 1 ammonium and Ba)

13. nitrates
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
it's lower and occurs over less sharp a range
Soluble
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

14. What is the energy you must put into a reaction to make it start called?
Exothermic
allow for the vapor pressure of water and make sure to level levels
Initiation energy (NOT Ea)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

15. How do you explain trends in atomic properties using Coulomb's Law?
Ksp = s²
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Exothermic (?H for ANY sa/sb = -57kJ/mol)
non-metal oxides and hydrides are covalently bonded and are acidic.

16. Does Benzene react by addition or substitution?
Salt + water
it reacts by substitution NOT addition
Greenish-yellow gas
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

17. Which alkali metals float on water?
benzene has a delocalized pi ring structure
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
All except for lithium
Unsaturated - addition (ex: decolorize bromine solution)

18. group 1 ions/compounds
C4H10
Distillation
Soluble
How grouped results are

19. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Ksp = 4s³
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
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
are less dense than water

20. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Unsaturated - addition (ex: decolorize bromine solution)
voltaic: + electrolytic: -
Soluble

21. Name 2 ways in which you can create a buffer?
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)
Heat a test tube at an angle at the side of the tube (not bottom)
Identity and purity (impure compounds usually have broad & low melting points)
Iodine and CO2 (dry ice)

22. acetate
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)
CH3COO?
NO3?
ns² electrons (first in-first out)

23. During a titration what is present in the beaker at the equivalence point?
A salt solution.
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
Heat a test tube at an angle at the side of the tube (not bottom)
Cu3(PO4)2

24. How does half life change for zero-th order - first order - and second order processes?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
acid + alcohol
zero-th: decreases - first: constant - second: increases
left - ppt will form

25. Name C7H16
blue glass - it filters UV
Concentration
Heptane
Exothermic (?H for ANY sa/sb = -57kJ/mol)

26. ammonium/ammonium compounds
ethers
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Soluble
Salt + water.

27. What is the difference between equivalence point and end point of a titration.
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)
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
look for changes in oxidation # - the one that goes up is oxidized and is the RA
SO4²?

28. What type of solutions do small - highly charged cations tend to form?
Making sigma bonds and holding lone pairs
Add acid to water so that the acid doesn't boil and spit
Synthetic condensation polymer (aka a polyamide)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

29. How do you find the pH for a dibasic acid? (H2A)?
Perform ICE BOX calculation based on K1
All except for lithium
No - it depends on the number of ions produced on dissolving.
The Faraday or Faraday's constant.

30. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Cr2O7²?
no - they're written undissociated (HAaq)
bent
Reduction always takes place at the cathode (RED CAT) In both types of cell!

31. A Bronsted-Lowry base is...
E=q + w (negative is by system - positive is on system)
proton acceptor.
Decant
PO4³?

32. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
RCHO (carbonyl at end)
CO (poisonous)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

33. What is the general formula for alkyl halides?
CH3COO?
RX
bent
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

34. What process do you use to obtain a solvent from a solution?
it reacts by substitution NOT addition
Ions go through the salt bridge - electrons go through metal wires in the external circuit
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Distillation

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

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36. potassium permanganate
Purple
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)
proton donor base
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

37. What shape is carbon dioxide?
10?8
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
H2PO4?
linear

38. Esterification is...
zero
Kc=Kp
acid + alcohol
OH- and NH3

39. What is the pH of 1.0M HCl? 1M NaOH?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Kc=Kp
They decrease (or could be the same if the solid has ONLY JUST disappeared)
0 and 14

40. What are hybrid orbitals used for?
Making sigma bonds and holding lone pairs
Reduction always takes place at the cathode (RED CAT) In both types of cell!
diamond and graphite
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

41. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Identity and purity (impure compounds usually have broad & low melting points)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Clear
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

42. iodine - iodine solution - iodine vapor
Graduated cylinder
Mono; di; tri; tetra; penta; hexa.
strong acids/bases are written as H+ or OH- ions
Silvery gray solid - brown - purple

43. What do metal oxides plus acids form?
bent
Salt + water
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
small size and high charge

44. When driving off water from a hydrate - how do you tell you're done?
Sigma bonds are stronger than pi bonds
T increases exponentially the proportion of molecules with E > Ea
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

45. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
Pale purple - (orange)-yellow - red - blue - green.
10?8
The compound with the lowest Ksp value.
benzene is less reactive than alkenes

46. When the salt bridge is removed what happens to the cell reaction?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
acid + alcohol
Disulfur dichloride
It ceases - the circuit is broken.

47. What reacts with an acid to create hydrogen gas?
?G= -ve - E°= +ve
K2
same KE - but PEice<PEwater
An active metal.

48. Alcohols and _______ are FG isomers
OH- and NH3
ethers
diamond and graphite
Heptane

49. phosphate
Clear
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
NH4?
PO4³?

50. What are the products of the reaction between group 1 metals and water?

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