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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.
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. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Cu3(PO4)2
E=q + w (negative is by system - positive is on system)
water and substances with (s) less dense than

2. The oxidation # for acid base reactions...
Transition element compounds (except if it has a full or empty d shell)
do not change
allow for the vapor pressure of water and make sure to level levels
diamond and graphite

3. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
0.10M HCl (more ions)
CrO4²?
#ligands=charge x2

4. group 1 ions/compounds
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Soluble
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
PO4³?

5. How do you explain trends in atomic properties using Coulomb's Law?
ns² electrons (first in-first out)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
H+
Suniverse increases for spontaneous processes

6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
An active metal.
Ksp = 108s5
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.
ionic and form hydrogen and hydroxide

7. What process do you use to separate two liquids with different boiling points?
Mn²? - Cr³? - Cr³
fractional distillation
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Nothing

8. silver iodide
Most are soluble except Ag - Pb
Pale yellow
PO4³?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

9. If a free element is involved - what type of reaction must be involved?
An active metal.
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)
redox reaction
CH3COO?

10. Alcohols and _______ are FG isomers
ethers
blue (BTB)
Unsaturated - addition (ex: decolorize bromine solution)
ROR

11. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
S2O3²?
Purple
Pour liquids using a funnel or down a glass rod
neutralization: high K - H2O product dissociation: low K - H2O reactant

12. What is the formula for percent error?
How grouped results are
OH?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
|experimental - accepted|/accepted X 100

13. Color is due to ______ _______ of light.
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Selective absorption
metal oxides and hydrides are ionically bonded and basic
NH4?

14. What is the name of S2Cl2? (Know how to name others like this - too)
Decant
?H formation of an element in standard state=0
Acid rain - dissolves marble buildings/statues and kills trees.
Disulfur dichloride

15. What is the formula for obtaining charge flowing in a cell?
acids
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
HClO4
Q=It (time in seconds)

16. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
Synthetic condensation polymer (aka a polyamide)
Pour liquids using a funnel or down a glass rod
it is lower and occurs over less sharp a range

17. What is the first law of thermodynamics?
White precipitate
strong acids/bases are written as H+ or OH- ions
ClO3?
E=q + w (negative is by system - positive is on system)

18. Ions are not ______.
atoms
it is lower and occurs over less sharp a range
Tetrahedral
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

19. Colorless doesn't mean ______
different forms of the same element
brown volatile liquid
Clear
Q=It (time in seconds)

20. What are the signs of ?G and E° for spontaneous reactions?
CN?
-Ea/R
ion pairing
?G=negative - E° must be positive

21. What is the general formula for an ether?
Insoluble except for nitrate and acetate
ROR
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Ksp = 27s4

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

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23. Name some properties of Group 17
proton donor base
red - green - blue
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
voltaic: - electrolytic: +

24. How are non-metal oxides and hydrides bonded? are they acidic or basic?
strong acids/bases are written as H+ or OH- ions
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Concentration
non-metal oxides and hydrides are covalently bonded and are acidic.

25. What does a short - sharp melting point indicate?
Filtration
Hg2²?
blue
Identity and purity (impure compounds usually have broad & low melting points)

26. mercury (II) ion
Hg²?
Big K=kf/kr
Insoluble except group 1 and ammonium
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

27. acetates
All except for lithium
Soluble
Graduated cylinder
K2

28. A geometric (or cis-trans) isomer exists due to.....
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
But S° of element is not zero (except at 0K)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
CnH2n+1 often designated 'R' ex C3H7 is propyl

29. What do you use to look at burning magnesium? why?
Synthesis - separation and purification of the product and its identification.
Cu3(PO4)2
blue glass - it filters UV
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

30. What does the solubility of organic compounds depend on?
Products - reactants (except for BDE when it's reactants - products)
proton acceptor.
lighted splint (positive result=pop)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

31. How are more active metals reduced?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
CnH2n+1 often designated 'R' ex C3H7 is propyl
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)
by electrolysis

32. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
bright yellow
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)
ROH

33. What is the formula of copper (II) phosphate?
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)
Tetrahedral
brown volatile liquid
Cu3(PO4)2

34. What is the second law of thermodynamics?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Suniverse increases for spontaneous processes
Soluble
0 and 14

35. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Selective absorption
Saturated - Substitution (which requires more radical conditions)
ionic and form hydrogen and hydroxide
Mono; di; tri; tetra; penta; hexa.

36. What is the general formula for an amine?
RNH2
bases
Insoluble except for nitrate and acetate
Evaporation

37. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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38. oxalate
Trigonal pyramidal
SO4²?
C2O4²?
The compound with the lowest Ksp value.

39. ammonium/ammonium compounds
Soluble
catalyst=conc H2SO4
no - they're written undissociated (HAaq)
benzene has a delocalized pi ring structure

40. Acid plus base make?
Most INsoluble except group 1 and ammonium
Salt + water.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
water and substances with (s) less dense than

41. Metal hydrides are _____ and form _______ and _______ when added to water
Tetrahedral
No - it depends on the number of ions produced on dissolving.
ionic and form hydrogen and hydroxide
Synthetic condensation polymer (aka a polyamide)

42. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Most INsoluble except group 1 and ammonium
CnH2n+1 often designated 'R' ex C3H7 is propyl
They decrease (or could be the same if the solid has ONLY JUST disappeared)

43. How does benzene compare in reactivity to alkenes?
Iodine and CO2 (dry ice)
by electrolysis
benzene is less reactive than alkenes
chemically (ex: with carbon)

44. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Sigma bonds are stronger than pi bonds
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Insoluble except for nitrate and acetate
CnH(2n+2)

45. When combining half equations - what do you do to E° values when multiplying coefficients?
atoms
White precipitate
Anode
Nothing

46. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Acids; HCOOCH3 is an ester
Ksp = s²
C2O4²?
Products - reactants (except for BDE when it's reactants - products)

47. Give an example of a concentrated weak acid.
Glacial acetic acid
PO4³?
blue (BTB)
Hg2²?

48. How do you get Ecell for spontaneous reactions?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
An active metal.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Sigma bonds are stronger than pi bonds

49. What is the general formula for an acid?
RCOOH
bright yellow
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
HClO4

50. What reacts with an acid to create hydrogen gas?
Pipette (burette if need repetition)
An active metal.
A salt solution.
Mn²? - Cr³? - Cr³