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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 relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Insoluble (except group 1 ammonium and Ba)
CnH2n+1 often designated 'R' ex C3H7 is propyl
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
zero

2. When combining half equations - what do you do to E° values when multiplying coefficients?
proton acceptor.
Heptane
|experimental - accepted|/accepted X 100
Nothing

3. mercury (I) ion
Hg2²?
Graduated cylinder
Big K=kf/kr
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

4. How are strong ones written?
Selective absorption
Synthetic condensation polymer (aka a polyamide)
strong acids/bases are written as H+ or OH- ions
Eudiometer

5. Does reactivity increase/decrease going down group 1 and group 17?
it is lower and occurs over less sharp a range
Increases down group 1 decreases down group 17
Salt + water
Sigma bonds are stronger than pi bonds

6. ammonium/ammonium compounds
Eudiometer
Soluble
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
ROH

7. Esterification is...
Ksp = 108s5
acid + alcohol
Nothing
zero-th: decreases - first: constant - second: increases

8. 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?
fruit - fish - bases
redox reaction
CnH2n
The compound with the lowest Ksp value.

9. What are the names and formulas of the 6 strong acids?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
The compound with the lowest Ksp value.
Eudiometer
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

10. What type of compounds do metals/non metals form?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Ionic compounds
Pipette (burette if need repetition)
Identity and purity (impure compounds usually have broad & low melting points)

11. Which of the rates changes more when temperature is increased?
Heat a test tube at an angle at the side of the tube (not bottom)
Insoluble except group 1 and ammonium
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
left - ppt will form

12. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
OH?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
S2O3²?

13. What process do you use to obtain a solvent from a solution?
ClO3?
Distillation
Q=It (time in seconds)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

14. What are amphoteric oxides?
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?)
Distillation
Ions go through the salt bridge - electrons go through metal wires in the external circuit
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)

15. Ca - Sr - Ba
PO4³?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
basic
hydroxides (ex: Ba(OH)2)

16. What is the second law of thermodynamics?
Suniverse increases for spontaneous processes
an oxidized and reduced substance
CH3COO?
Heat a test tube at an angle at the side of the tube (not bottom)

17. What does the solubility of organic compounds depend on?
Purple
H2O + CO2 (it decomposes readily)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

18. potassium permanganate
Purple
Soluble
Identity and purity (impure compounds usually have broad & low melting points)
Insoluble except group 1 and ammonium

19. When driving off water from a hydrate - how do you tell you're done?
SO4²?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
ion pairing

20. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
boiling without losing volatile solvents/reactants
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
RCHO (carbonyl at end)

21. A geometric (or cis-trans) isomer exists due to.....
Most are soluble except Ag - Pb
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
ns² electrons (first in-first out)
#ligands=charge x2

22. What things should you remember to do when collecting gas over water?
a-IMFs - b-molecular volume
look for changes in oxidation # - the one that goes up is oxidized and is the RA
allow for the vapor pressure of water and make sure to level levels
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

23. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
CO (poisonous)
E=q + w (negative is by system - positive is on system)
0.10M HCl (more ions)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

24. What type of compounds are almost always colored?
Pale purple - (orange)-yellow - red - blue - green.
Transition element compounds (except if it has a full or empty d shell)
Pour liquids using a funnel or down a glass rod
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

25. What does a short - sharp melting point indicate?
Most are soluble except Ag - Pb
Identity and purity (impure compounds usually have broad & low melting points)
Hg2²?
Acids; HCOOCH3 is an ester

26. A Bronsted-Lowry acid is...
Iodine and CO2 (dry ice)
Saturated - Substitution (which requires more radical conditions)
Orange
proton donor base

27. What is the word equation for condensation polymerisation ?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Monomer + monomer = polymer product + a simple molecule such as water or HCl
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

28. Where are group I metals stored?
Sigma bonds are stronger than pi bonds
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Group I metals (soft metals) are stored under oil
Identity and purity (impure compounds usually have broad & low melting points)

29. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
q=mc?T q=mL (or n x ?h)
CO3²?
Exothermic
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

30. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
+4-covalent - +2-ionic
#ligands=charge x2
blue (BTB)
Kc=Kp

31. If Q > Ksp - then system shifts _______ and ppt ______
Salt + water
left - ppt will form
Synthetic condensation polymer (aka a polyamide)
acid + alcohol

32. Color (absorbance) is proportional to ________
neutralization: high K - H2O product dissociation: low K - H2O reactant
Suniverse increases for spontaneous processes
zero
Concentration

33. What is the general formula for an alcohol?
0 and 14
ROH
Trigonal pyramidal
E=q + w (negative is by system - positive is on system)

34. Name 2 ways in which you can create a buffer?
P2O5
Sigma bonds are stronger than pi bonds
red - green - blue
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)

35. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
RCOOR
Pipette (burette if need repetition)

36. What should you check for before you begin titrating?
zero
Check for air bubbles in the buret and remove the buret funnel from the buret
It ceases - the circuit is broken.
S2O3²?

37. What do the 'a' and 'b' in Van Der Waal's equation allow for?
ClO3?
The dilution effect when the solutions mix. M1V1 = M2V2
R=8.31 J/mol/K
a-IMFs - b-molecular volume

38. What is HCOOCH3?
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
acid + alcohol
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Acids; HCOOCH3 is an ester

39. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
At half equivalence - pH=pKa
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Increases.

40. carbonate
CO3²?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Ppt will NOT form (unsaturated)
RCOOH

41. What are the signs of ?G and E° for spontaneous reactions?
The Faraday or Faraday's constant.
OH?
?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

42. How are non-metal oxides and hydrides bonded? are they acidic or basic?
ClO2?
non-metal oxides and hydrides are covalently bonded and are acidic.
voltaic: - electrolytic: +
0.10M HCl (more ions)

43. hydroxides
CnH2n+2
same KE - but PEice<PEwater
Insoluble (except group 1 ammonium and Ba)
fruit - fish - bases

44. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
RCHO (carbonyl at end)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
blue

45. Is the standard entropy (S°) of an element zero?
Read the bottom of the meniscus
But S° of element is not zero (except at 0K)
a-IMFs - b-molecular volume
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

46. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
Purple
CO (poisonous)
Both electrons come from the same atom (just as good as a regular bond)

47. 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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48. carbonates
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Insoluble except group 1 and ammonium
left - ppt will form
Group I metals (soft metals) are stored under oil

49. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
atoms
chemically (ex: with carbon)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Conjugate pair (one must be a weak base or acid)

50. What is the catalyst for this reaction Ester + ?
catalyst=conc H2SO4
CO (poisonous)
Insoluble (except group 1 ammonium and Ba)
But S° of element is not zero (except at 0K)