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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. barium sulfate
Pale purple - (orange)-yellow - red - blue - green.
atoms
White precipitate
Insoluble (except group 1 ammonium and Ba)

2. phosphates
proton donor base
?G=negative - E° must be positive
chemically (ex: with carbon)
Most INsoluble except group 1 and ammonium

3. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H2O + CO2 (it decomposes readily)
Glowing splint (positive result=relights)
H+
Heat a test tube at an angle at the side of the tube (not bottom)

4. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
HClO4
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Synthetic condensation polymer (aka a polyamide)
Molecules with the same molecular formulas - but different structural formulas

5. What is the general formula for an amine?
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.
Orange
RNH2
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

6. How does benzene compare in reactivity to alkenes?
Orange
Synthesis - separation and purification of the product and its identification.
Decant
benzene is less reactive than alkenes

7. What changes Keq?
Tetrahedral
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Anode - oxygen. Cathode - hydrogen
Only temperature

8. What is the second law of thermodynamics?
acid + alcohol
Suniverse increases for spontaneous processes
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)
ethers

9. Color is due to ______ _______ of light.
Selective absorption
zero
Mono; di; tri; tetra; penta; hexa.
a-IMFs - b-molecular volume

10. chromate
Q=It (time in seconds)
CrO4²?
Insoluble except nitrate and acetate
SO4²?

11. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
CH3COO?

12. The oxidation # for acid base reactions...
do not change
Ionic compounds
#ligands=charge x2
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

13. What do ions and electrons travel through in a voltaic/electrolytic cell?
Q=It (time in seconds)
OH- and NH3
Ions go through the salt bridge - electrons go through metal wires in the external circuit
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

14. What is the first law of thermodynamics?
No - it depends on the number of ions produced on dissolving.
do not change
E=q + w (negative is by system - positive is on system)
Ksp = 108s5

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

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16. Buffer capacity must contain decent amounts of a ________ ________
?G= -ve - E°= +ve
It ceases - the circuit is broken.
Conjugate pair (one must be a weak base or acid)
Glacial acetic acid

17. A Bronsted-Lowry acid is...
proton donor base
Insoluble except group 1 and ammonium
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
H3PO4

18. Colorless doesn't mean ______
same KE - but PEice<PEwater
Clear
#ligands=charge x2
Salt + water.

19. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
Orange
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
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

20. Which alkali metals float on water?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
same KE - but PEice<PEwater
Kc=Kp
All except for lithium

21. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
proton donor base

22. What do the 'a' and 'b' in Van Der Waal's equation allow for?
|experimental - accepted|/accepted X 100
a-IMFs - b-molecular volume
-Ea/R
The one with most oxygen atoms (highest oxidation number)

23. What is a coordinate covalent bond?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
NH2?
Both electrons come from the same atom (just as good as a regular bond)
E=q + w (negative is by system - positive is on system)

24. Do anions flow to the cathode or anode?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
-Ea/R
Anode
Experimental mass/theoretical mass X 100

25. acetates
Mono; di; tri; tetra; penta; hexa.
Selective absorption
Soluble
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

26. What things should you remember to do when collecting gas over water?
Anode
allow for the vapor pressure of water and make sure to level levels
Increases.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

27. Metal hydrides are _____ and form _______ and _______ when added to water
Sigma bonds are stronger than pi bonds
Anode - oxygen. Cathode - hydrogen
ionic and form hydrogen and hydroxide
PO4³?

28. What shape is carbon dioxide?
linear
by electrolysis
Salt + water.
Most are soluble except Ag - Pb

29. What is the general formula for an aldehyde?
RCHO (carbonyl at end)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
RX
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

30. How are metal oxides and hydrides bonded? are they acidic or basic?
metal oxides and hydrides are ionically bonded and basic
A salt solution.
NO3?
The one with most oxygen atoms (highest oxidation number)

31. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
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.
C4H10
ionic and form hydrogen and hydroxide
Mn²? - Cr³? - Cr³

32. A geometric (or cis-trans) isomer exists due to.....
Group 1 hydroxides (ex: NaOH)
Anode
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
At half equivalence - pH=pKa

33. Is the ?H formation of an element in standard state zero?
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
?H formation of an element in standard state=0
The dilution effect when the solutions mix. M1V1 = M2V2
ClO2?

34. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Soluble
?G=negative - E° must be positive

35. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
RCOOH
no - they're written undissociated (HAaq)

36. Ions are not ______.
boiling without losing volatile solvents/reactants
?H formation of an element in standard state=0
Pale purple - (orange)-yellow - red - blue - green.
atoms

37. What do you use to look at burning magnesium? why?
CnH2n-2
blue glass - it filters UV
Selective absorption
+4-covalent - +2-ionic

38. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
CO (poisonous)
C4H10
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
CnH2n+2

39. For a dibasic acid (H2A) - [A²?]= ____ ?
OH- and NH3
K2
H2PO4?
ClO4?

40. What process do you use to obtain the precipitate from a solution?
non-metal oxides and hydrides are covalently bonded and are acidic.
ClO3?
Filtration
Most INsoluble except group 1 and ammonium

41. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Decant
Insoluble (except group 1 ammonium and Ba)

42. What shape is water?
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)
bent
CnH2n+2
Most INsoluble except group 1 and ammonium

43. primary colors
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?)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
HClO4
red - green - blue

44. What does saturated mean? Unsaturated?
Glowing splint (positive result=relights)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
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.
benzene is less reactive than alkenes

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

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46. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
No - it depends on the number of ions produced on dissolving.
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

47. What process do you use to obtain the solute from a solution?
voltaic: - electrolytic: +
Evaporation
NO3?
Heptane

48. silver compounds
NH4?
Read the bottom of the meniscus
Separating funnel
Insoluble except for nitrate and acetate

49. carbonates
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Heat a test tube at an angle at the side of the tube (not bottom)
ROH
Insoluble except group 1 and ammonium

50. What do group I/II metal oxides and acids form?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
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)
Salt and water
The benzene ring (or more correctly the phenyl group - C6H5)

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AP Chemistry 2

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