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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. mercury (I) ion
Read the bottom of the meniscus
?G= -ve - E°= +ve
CO (poisonous)
Hg2²?

2. During a titration what is present in the beaker at the equivalence point?
A salt solution.
ClO3?
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
Hg2²?

3. What do group I/II metal oxides plus water form?
q=mc?T q=mL (or n x ?h)
Pour liquids using a funnel or down a glass rod
bases
proton acceptor.

4. How are strong ones written?
hydroxides (ex: Ba(OH)2)
strong acids/bases are written as H+ or OH- ions
fractional distillation
CnH(2n+2)

5. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
CH3COO?
C2O4²?
P2O5
Disulfur dichloride

6. chlorine
ClO3?
Hg²?
Greenish-yellow gas
Soluble

7. At what point during titration do you have the perfect buffer - and what is the pH at this point?
RCHO (carbonyl at end)
At half equivalence - pH=pKa
Anode
an oxidized and reduced substance

8. What does a short - sharp melting point indicate?
different forms of the same element
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
Kc=Kp
Identity and purity (impure compounds usually have broad & low melting points)

9. What are two allotropes of carbon?
Pale yellow
Check for air bubbles in the buret and remove the buret funnel from the buret
ns² electrons (first in-first out)
diamond and graphite

10. If a free element is involved - what type of reaction must be involved?
The Faraday or Faraday's constant.
a-IMFs - b-molecular volume
redox reaction
Mn²? - Cr³? - Cr³

11. What is a coordinate covalent bond?
Iodine and CO2 (dry ice)
T increases exponentially the proportion of molecules with E > Ea
Heat a test tube at an angle at the side of the tube (not bottom)
Both electrons come from the same atom (just as good as a regular bond)

12. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
Selective absorption
The Faraday or Faraday's constant.
Heat a test tube at an angle at the side of the tube (not bottom)

13. Which value of R do you use for all energy and kinetics calculations?
Soluble
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Salt + water
R=8.31 J/mol/K

14. What are the common strong bases?
chemically (ex: with carbon)
Group 1 hydroxides (ex: NaOH)
hydroxides (ex: Ba(OH)2)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

15. What are two substances that sublime at 1 atm when heated?
Pale yellow
O2 needs 4F/mol H2 needs 2F/mol
Glacial acetic acid
Iodine and CO2 (dry ice)

16. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
H3PO4
Unsaturated - addition (ex: decolorize bromine solution)
ns² electrons (first in-first out)

17. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
HClO4
Insoluble except nitrate and acetate
same KE - but PEice<PEwater
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

18. carbonates
Insoluble except group 1 and ammonium
allow for the vapor pressure of water and make sure to level levels
RCHO (carbonyl at end)
Purple

19. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Initiation energy (NOT Ea)
Molecules with the same molecular formulas - but different structural formulas
red - green - blue

20. Ions are not ______.
Saturated - Substitution (which requires more radical conditions)
zero
non-metal oxides and hydrides are covalently bonded and are acidic.
atoms

21. silver iodide
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)
an oxidized and reduced substance
Pale yellow
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)

22. sulfates
An active metal.
Soluble except Ag - Pb - Ca - Sr Ba)
red - green - blue
zero

23. The oxidation # for acid base reactions...
yellow
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
do not change
Anode

24. What is the third law of thermodynamics?
It ceases - the circuit is broken.
S crystal at 0K=0
PO4³?
Perform ICE BOX calculation based on K1

25. What is the formula for alkenes?
Distillation
CnH2n
blue glass - it filters UV
SO4²?

26. dichromate (soln + most solids)
CN?
Orange
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
They decrease (or could be the same if the solid has ONLY JUST disappeared)

27. What is the general formula for an aldehyde?
?H-kJ - ?S-J - ?G-kJ
RCHO (carbonyl at end)
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.
NO3?

28. dichromate
CO (poisonous)
diamond and graphite
Cr2O7²?
Unsaturated - addition (ex: decolorize bromine solution)

29. A Bronsted-Lowry acid is...
proton donor base
Time?¹ - (ex. s?¹ - hr?¹ - etc)
zero
Mono; di; tri; tetra; penta; hexa.

30. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Silvery gray solid - brown - purple
Mono; di; tri; tetra; penta; hexa.
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
ClO2?

31. What electrons are lost/gained first in transition element ions?
RCOOH
ion pairing
ns² electrons (first in-first out)
ROR

32. chromate
Purple
C4H10
methyl formate
CrO4²?

33. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Check for air bubbles in the buret and remove the buret funnel from the buret
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
H+

34. What changes Keq?
voltaic: + electrolytic: -
Only temperature
an oxidized and reduced substance
They decrease (or could be the same if the solid has ONLY JUST disappeared)

35. What are the units of the first order rate constant?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Time?¹ - (ex. s?¹ - hr?¹ - etc)
CnH2n+2
Salt and water

36. primary colors
red - green - blue
Purple
Orange
are less dense than water

37. What causes the dramatic effect of T on rate?
?G=negative - E° must be positive
catalyst=conc H2SO4
Cu3(PO4)2
T increases exponentially the proportion of molecules with E > Ea

38. What is the general formula for a ketone?
RCOR
Group I metals (soft metals) are stored under oil
H2PO4?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

39. silver compounds
Anode - oxygen. Cathode - hydrogen
0 and 14
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Insoluble except for nitrate and acetate

40. thiosulfate
S2O3²?
allow for the vapor pressure of water and make sure to level levels
blue glass - it filters UV
RX

41. What is the formula for alkynes?
same KE - but PEice<PEwater
At half equivalence - pH=pKa
CnH2n-2
ROH

42. What things should you remember to do when collecting gas over water?
Pale yellow
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
allow for the vapor pressure of water and make sure to level levels
CO2 and H2O

43. What measuring device would you use for very small volumes of liquids?
OH- and NH3
Pipette (burette if need repetition)
?H formation of an element in standard state=0
allow for the vapor pressure of water and make sure to level levels

44. What device would you use to measure a volume of gas?
Evaporation
CH3COO?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Eudiometer

45. lead compounds
Insoluble except nitrate and acetate
Heat a test tube at an angle at the side of the tube (not bottom)
Soluble
OH- and NH3

46. How do you get the equation for a net electrolysis reaction?
linear
ROH
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Combine the equations for the half reactions in the non-spontaneous direction

47. phosphate
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Synthesis - separation and purification of the product and its identification.
PO4³?
Graduated cylinder

48. Are weak acids (and bases) written dissociated?

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49. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
HClO4
Sulfur
do not change

50. 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?
a-IMFs - b-molecular volume
ClO2?
All except for lithium
The compound with the lowest Ksp value.