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AP Chemistry 2

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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. What are two allotropes of carbon?
small size and high charge
diamond and graphite
MnO4?
it reacts by substitution NOT addition

2. If a free element is involved - what type of reaction must be involved?
Transition element compounds (except if it has a full or empty d shell)
Decant
?H formation of an element in standard state=0
redox reaction

3. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
It ceases - the circuit is broken.
Decant
CO (poisonous)
An active metal.

4. What is HCOOCH3?
Acids; HCOOCH3 is an ester
ethers
allow for the vapor pressure of water and make sure to level levels
Hg²?

5. What shape is carbon dioxide?
?G=negative - E° must be positive
linear
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
They stay the same.

6. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Molecules with the same molecular formulas - but different structural formulas
Soluble
No - it depends on the number of ions produced on dissolving.
Ksp = 27s4

7. What is the general formula for an amine?
RNH2
voltaic: + electrolytic: -
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Acid rain - dissolves marble buildings/statues and kills trees.

8. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Insoluble except group 1 and ammonium
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
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

9. Does reactivity increase/decrease going down group 1 and group 17?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Glacial acetic acid
Increases down group 1 decreases down group 17
Acid rain - dissolves marble buildings/statues and kills trees.

10. How many ligands attach to a central ion in a complex ion?
Ksp = 4s³
Synthesis - separation and purification of the product and its identification.
#ligands=charge x2
O2 needs 4F/mol H2 needs 2F/mol

11. Do you use J or kJ for ?H - ?S - and ?G?
ethers
[A?]/[HA] x 100 or [BH?]/[B] x 100
different forms of the same element
?H-kJ - ?S-J - ?G-kJ

12. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Ksp = 4s³
acids
Purple

13. A Bronsted-Lowry base is...
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
proton acceptor.
PO4³?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

14. What is H2CO3 (carbonate acid) usually written as?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
ethers
Initiation energy (NOT Ea)
H2O + CO2 (it decomposes readily)

15. What is the catalyst for this reaction Ester + ?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
catalyst=conc H2SO4
H3PO4

16. Which would cause the bulb in a conductivity apparatus to be brightest?
bases
0.10M HCl (more ions)
Group 1 hydroxides (ex: NaOH)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

17. How do you compute % dissociation?
[A?]/[HA] x 100 or [BH?]/[B] x 100
fractional distillation
Insoluble
Acid rain - dissolves marble buildings/statues and kills trees.

18. sulfates
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)
Soluble except Ag - Pb - Ca - Sr Ba)
It ceases - the circuit is broken.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

19. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Separating funnel
?H formation of an element in standard state=0
redox reaction

20. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Q=It (time in seconds)
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
P2O5
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)

21. acetates
Soluble
Salts (ex: CaO + SO2 ? CaSO3)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
CrO4²?

22. When driving off water from a hydrate - how do you tell you're done?
H2PO4?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
OH- and NH3

23. What are the signs of ?G and E° for spontaneous reactions?
Ppt will NOT form (unsaturated)
ROH
?G=negative - E° must be positive
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

24. carbonates
Identity and purity (impure compounds usually have broad & low melting points)
Insoluble except group 1 and ammonium
Trigonal pyramidal
Insoluble

25. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Soluble except Ag - Pb - Ca - Sr Ba)
neutralization: high K - H2O product dissociation: low K - H2O reactant
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
Unsaturated - addition (ex: decolorize bromine solution)

26. 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?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
The compound with the lowest Ksp value.
acid + alcohol

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

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28. What process do you use to obtain the precipitate from a solution?
RCOOH
Filtration
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
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.

29. mercury (I) ion
Hg2²?
Kc=Kp
Ksp = 4s³
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

30. oxalate
C2O4²?
NO3?
ClO2?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

31. What is the charge on a chlorine atom?
Glowing splint (positive result=relights)
At half equivalence - pH=pKa
zero
an oxidized and reduced substance

32. What is the formula of butane?
CnH2n+2
Hg²?
Orange
C4H10

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

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34. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
acid + alcohol
Transition element compounds (except if it has a full or empty d shell)
HClO4
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

35. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Pipette (burette if need repetition)
The dilution effect when the solutions mix. M1V1 = M2V2
Group 1 hydroxides (ex: NaOH)

36. Which of the rates changes more when temperature is increased?
same KE - but PEice<PEwater
Soluble
Hg2²?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

37. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
Ppt will NOT form (unsaturated)
#ligands=charge x2
Transition element compounds (except if it has a full or empty d shell)

38. What electrons are lost/gained first in transition element ions?
Ksp = s²
ns² electrons (first in-first out)
Most are soluble except Ag - Pb
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

39. What is the general formula for an aldehyde?
Molecules with the same molecular formulas - but different structural formulas
SO4²?
But S° of element is not zero (except at 0K)
RCHO (carbonyl at end)

40. What two compounds are great oxidizing agents?

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41. What type of compounds are almost always colored?
Purple
Transition element compounds (except if it has a full or empty d shell)
bases
zero

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.
Glacial acetic acid
chemically (ex: with carbon)
Sulfur

43. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Pour liquids using a funnel or down a glass rod
Hg2²?
Time?¹ - (ex. s?¹ - hr?¹ - etc)

44. Lattice energy is high for ions with _____ size and _____ charge
q=mc?T q=mL (or n x ?h)
Suniverse increases for spontaneous processes
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
small size and high charge

45. How are strong ones written?
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)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
strong acids/bases are written as H+ or OH- ions
q=mc?T q=mL (or n x ?h)

46. Nonmetals are good _____ agents. Metals are good _______ agents.
non-metal oxides and hydrides are covalently bonded and are acidic.
CN?
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)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

47. For a dibasic acid (H2A) - [A²?]= ____ ?
ClO3?
ionic and form hydrogen and hydroxide
K2
ROH

48. ammonium/ammonium compounds
Soluble
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
allow for the vapor pressure of water and make sure to level levels

49. BaSO4
CnH2n+2
Cu3(PO4)2
Insoluble
benzene has a delocalized pi ring structure

50. nitrate
NO3?
Insoluble except for nitrate and acetate
strong acids/bases are written as H+ or OH- ions
Heptane

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AP Chemistry 2

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