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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. What is the difference between equivalence point and end point of a titration.
RCHO (carbonyl at end)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ion pairing
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

2. What apparatus do you use to separate 2 immiscible liquids?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
ionic and form hydrogen and hydroxide
Separating funnel
?H-kJ - ?S-J - ?G-kJ

3. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
q=mc?T q=mL (or n x ?h)
left - ppt will form
water and substances with (s) less dense than
They decrease (or could be the same if the solid has ONLY JUST disappeared)

4. What process do you use to obtain the precipitate from a solution?
Filtration
C2O4²?
Graduated cylinder
ethers

5. How can metals like iron and zinc be reduced?
methyl formate
K2
CO3²?
chemically (ex: with carbon)

6. Is a graduated cylinder or beaker more accurate?
Salt + water.
Pale yellow
Concentration
Graduated cylinder

7. What shape is ammonia?
left - ppt will form
fractional distillation
zero
Trigonal pyramidal

8. What changes Keq?
H+
Only temperature
Pour liquids using a funnel or down a glass rod
Soluble

9. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Heptane
Insoluble except group 1 and ammonium
They decrease (or could be the same if the solid has ONLY JUST disappeared)
neutralization: high K - H2O product dissociation: low K - H2O reactant

10. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
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.
Salts (ex: CaO + SO2 ? CaSO3)
water and substances with (s) less dense than
neutralization: high K - H2O product dissociation: low K - H2O reactant

11. What value of R do you use for thermo calculations? gas calculations?
ion pairing
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Ppt will NOT form (unsaturated)
Concentration

12. What does saturated mean? Unsaturated?
H3PO4
red - green - blue
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Hg2²?

13. What are two substances that sublime at 1 atm when heated?
MnO4?
Iodine and CO2 (dry ice)
CO2 and H2O
proton donor base

14. How do you get Ecell for spontaneous reactions?
no - they're written undissociated (HAaq)
Iodine and CO2 (dry ice)
are less dense than water
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

15. What is the conjugate base of NH3?
ClO2?
Suniverse increases for spontaneous processes
boiling without losing volatile solvents/reactants
NH2?

16. What is the formula for alkynes?
CnH2n-2
NO3?
RCOR
K1 x K2

17. What is accuracy?
How close results are to the accepted value
Iodine and CO2 (dry ice)
Kc=Kp
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

18. What are allotropes?
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
Heptane
It ceases - the circuit is broken.

19. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
A salt solution.

20. What element is used to vulcanize rubber?
atoms
NH2?
The one with most oxygen atoms (highest oxidation number)
Sulfur

21. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Glowing splint (positive result=relights)
do not change
Kc=Kp
At half equivalence - pH=pKa

22. What shape is carbon dioxide?
Evaporation
linear
small size and high charge
H2O + CO2 (it decomposes readily)

23. dichromate (soln + most solids)
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?)
Orange
CO3²?
-Ea/R

24. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Pour liquids using a funnel or down a glass rod
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
do not change
0.10M HCl (more ions)

25. Ca - Sr - Ba
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.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Check for air bubbles in the buret and remove the buret funnel from the buret
hydroxides (ex: Ba(OH)2)

26. 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?
no - they're written undissociated (HAaq)
bright yellow
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
Ksp = s²

27. What type of solutions do small - highly charged cations tend to form?
Silvery gray solid - brown - purple
Concentration
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
zero

28. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
allow for the vapor pressure of water and make sure to level levels
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Read the bottom of the meniscus
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

29. What type of metals don't react with water or acids to form H2?

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30. What do group I/II metal oxides plus water form?
it is lower and occurs over less sharp a range
bases
Salts (ex: CaO + SO2 ? CaSO3)
red - green - blue

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

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32. What is the pH of 1.0M HCl? 1M NaOH?
Both electrons come from the same atom (just as good as a regular bond)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
0 and 14
H2PO4?

33. Which value of R do you use for all energy and kinetics calculations?
different forms of the same element
benzene has a delocalized pi ring structure
R=8.31 J/mol/K
NH4?

34. What is the catalyst for this reaction Ester + ?
atoms
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
catalyst=conc H2SO4
Soluble

35. Buffer capacity must contain decent amounts of a ________ ________
?H formation of an element in standard state=0
Conjugate pair (one must be a weak base or acid)
it's lower and occurs over less sharp a range
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

36. Alkanes are _________ and react by _________
Increases down group 1 decreases down group 17
Iodine and CO2 (dry ice)
Saturated - Substitution (which requires more radical conditions)
Increases.

37. Lattice energy is high for ions with _____ size and _____ charge
#ligands=charge x2
small size and high charge
Most INsoluble except group 1 and ammonium
Insoluble except group 1 and ammonium

38. What two compounds are great oxidizing agents?

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39. What process do you use to obtain the solute from a solution?
CrO4²?
More chaotic (ex: gases made)
Evaporation
?G=negative - E° must be positive

40. What does a short - sharp melting point indicate?
zero
it reacts by substitution NOT addition
No - NH3 and HCl gases are extremely soluble
Identity and purity (impure compounds usually have broad & low melting points)

41. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
?H formation of an element in standard state=0
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Reduction always takes place at the cathode (RED CAT) In both types of cell!

42. acetate
CH3COO?
methyl formate
Decant
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

43. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Glowing splint (positive result=relights)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
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

44. What are two allotropes of carbon?
diamond and graphite
NO3?
More chaotic (ex: gases made)
Greenish-yellow gas

45. Which alkali metals float on water?
All except for lithium
T increases exponentially the proportion of molecules with E > Ea
C4H10
Molecules with the same molecular formulas - but different structural formulas

46. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
The dilution effect when the solutions mix. M1V1 = M2V2
Soluble
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
strong acids/bases are written as H+ or OH- ions

47. What is the general formula of an alkane?
atoms
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Time?¹ - (ex. s?¹ - hr?¹ - etc)
CnH(2n+2)

48. What type of compounds do metals/non metals form?
S crystal at 0K=0
OH?
Ionic compounds
acids

49. What do you use for an acid spill? base spill?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Iodine and CO2 (dry ice)
Soluble
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

50. perchlorate
C4H10
Q=It (time in seconds)
fruit - fish - bases
ClO4?