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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. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Synthetic condensation polymer (aka a polyamide)
fractional distillation
by electrolysis

2. When a cell is 'flat' What is its voltage?
zero
Soluble
No - NH3 and HCl gases are extremely soluble
How close results are to the accepted value

3. 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?
metal oxides and hydrides are ionically bonded and basic
blue
RCOOR
The compound with the lowest Ksp value.

4. group 1 ions/compounds
|experimental - accepted|/accepted X 100
Soluble
Kc=Kp
No - it depends on the number of ions produced on dissolving.

5. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
proton acceptor.
Kc=Kp
Making sigma bonds and holding lone pairs
Trigonal pyramidal

6. What is the catalyst for this reaction Ester + ?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
?G=negative - E° must be positive
catalyst=conc H2SO4
They stay the same.

7. Where are group I metals stored?
red - green - blue
Mono; di; tri; tetra; penta; hexa.
Group I metals (soft metals) are stored under oil
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

8. phosphates
Most INsoluble except group 1 and ammonium
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
The compound with the lowest Ksp value.
ClO?

9. How many ligands attach to a central ion in a complex ion?
Insoluble (except group 1 ammonium and Ba)
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
#ligands=charge x2
NO3?

10. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Greenish-yellow gas
water and substances with (s) less dense than
yellow
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

11. At what point during titration do you have the perfect buffer - and what is the pH at this point?
blue
Selective absorption
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
At half equivalence - pH=pKa

12. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
proton acceptor.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Purple

13. acetates
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
K1 x K2
Soluble except Ag - Pb - Ca - Sr Ba)
Soluble

14. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
are less dense than water
Pale purple - (orange)-yellow - red - blue - green.
K1 x K2
red - green - blue

15. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
-Ea/R
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
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

16. hydroxide
Soluble
voltaic: - electrolytic: +
OH?
Heat a test tube at an angle at the side of the tube (not bottom)

17. What is the general formula for a ketone?
RCOR
Insoluble except nitrate and acetate
Salt and water
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

18. What do metal oxides plus acids form?
ClO2?
+4-covalent - +2-ionic
Salt + water
Unsaturated - addition (ex: decolorize bromine solution)

19. Is the freezing of ice endothermic or exothermic?
RCOOH
Exothermic
CnH2n+2
it reacts by substitution NOT addition

20. bromine
Insoluble (except group 1 ammonium and Ba)
P2O5
brown volatile liquid
NH2?

21. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
Increases.
strong acids/bases are written as H+ or OH- ions
PO4³?

22. What two types of substances are present in all redox reactions?
Check for air bubbles in the buret and remove the buret funnel from the buret
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Perform ICE BOX calculation based on K1
an oxidized and reduced substance

23. What reacts with an acid to create hydrogen gas?
An active metal.
Exothermic
ionic and form hydrogen and hydroxide
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

24. oxalate
0 and 14
C2O4²?
No - it depends on the number of ions produced on dissolving.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

25. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Mn²? - Cr³? - Cr³
voltaic: + electrolytic: -
same KE - but PEice<PEwater
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

26. How can metals like iron and zinc be reduced?
Pipette (burette if need repetition)
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?)
CrO4²?
chemically (ex: with carbon)

27. What are the units of the first order rate constant?
Add acid to water so that the acid doesn't boil and spit
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)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Group I metals (soft metals) are stored under oil

28. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
zero
neutralization: high K - H2O product dissociation: low K - H2O reactant
blue glass - it filters UV
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. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
OH?
q=mc?T q=mL (or n x ?h)
White precipitate

30. dichromate (soln + most solids)
hydroxides (ex: Ba(OH)2)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Orange
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

31. What is the difference between equivalence point and end point of a titration.
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
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Group I metals (soft metals) are stored under oil
Soluble

32. What is the general formula for an aldehyde?
Heat a test tube at an angle at the side of the tube (not bottom)
RCHO (carbonyl at end)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ClO?

33. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
hydroxides (ex: Ba(OH)2)
Heat a test tube at an angle at the side of the tube (not bottom)
Ionic compounds
Mn²? - Cr³? - Cr³

34. What are the prefixes for the naming of binary molecular compound formulas (up to six)
proton donor base
More chaotic (ex: gases made)
Mono; di; tri; tetra; penta; hexa.
White precipitate

35. Color is due to ______ _______ of light.
PO4³?
Soluble
Selective absorption
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

36. The definition of acidic basic and neutral aqueous solutions is:
Eudiometer
Read the bottom of the meniscus
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
basic

37. nitrates
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
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.
Soluble
How grouped results are

38. dichromate
Cr2O7²?
Most are soluble except Ag - Pb
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
RNH2

39. During a titration what is present in the beaker at the equivalence point?
no - they're written undissociated (HAaq)
The compound with the lowest Ksp value.
A salt solution.
allow for the vapor pressure of water and make sure to level levels

40. Acids + Carbonates (bicarbonates) make?
brown volatile liquid
No - NH3 and HCl gases are extremely soluble
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

41. How do you get the equation for a net electrolysis reaction?
0.10M HCl (more ions)
Combine the equations for the half reactions in the non-spontaneous direction
MnO4?
Ksp = s²

42. What is the formula for percent error?
hydroxides (ex: Ba(OH)2)
|experimental - accepted|/accepted X 100
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Products - reactants (except for BDE when it's reactants - products)

43. chlorite
T increases exponentially the proportion of molecules with E > Ea
Acidified
ClO2?
CrO4²?

44. How are primary alcohols turned into acids?
zero
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
ion pairing
NH4?

45. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Anode
Ksp = 108s5
Acid rain - dissolves marble buildings/statues and kills trees.
Q=It (time in seconds)

46. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Separating funnel
it's lower and occurs over less sharp a range
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

47. What is the second law of thermodynamics?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
SO4²?
Suniverse increases for spontaneous processes
Soluble

48. What are amphoteric oxides?
left - ppt will form
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?)
Insoluble except for nitrate and acetate
voltaic: + electrolytic: -

49. What word is a clue for a redox reaction?
Acidified
no - they're written undissociated (HAaq)
Suniverse increases for spontaneous processes
Making sigma bonds and holding lone pairs

50. chlorate
methyl formate
Unsaturated - addition (ex: decolorize bromine solution)
Selective absorption
ClO3?