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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.
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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. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Insoluble except group 1 and ammonium
non-metal oxides and hydrides are covalently bonded and are acidic.
SO4²?

2. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
CnH2n+1 often designated 'R' ex C3H7 is propyl
Unsaturated - addition (ex: decolorize bromine solution)
proton acceptor.

3. hypochlorite
RCOOH
A salt solution.
metal oxides and hydrides are ionically bonded and basic
ClO?

4. What is the charge on a chlorine atom?
ClO2?
lighted splint (positive result=pop)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
zero

5. What do group I/II metal oxides plus water form?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Mono; di; tri; tetra; penta; hexa.
bases
benzene is less reactive than alkenes

6. What is the first law of thermodynamics?
q=mc?T q=mL (or n x ?h)
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?)
ns² electrons (first in-first out)
E=q + w (negative is by system - positive is on system)

7. When the salt bridge is removed what happens to the cell reaction?
Greenish-yellow gas
Trigonal pyramidal
It ceases - the circuit is broken.
But S° of element is not zero (except at 0K)

8. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
left - ppt will form
Anode - oxygen. Cathode - hydrogen
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

9. What does a short - sharp melting point indicate?
Exothermic
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Initiation energy (NOT Ea)
Identity and purity (impure compounds usually have broad & low melting points)

10. How does half life change for zero-th order - first order - and second order processes?
Salt + water
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Ksp = s²
zero-th: decreases - first: constant - second: increases

11. acetate
CH3COO?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Heat a test tube at an angle at the side of the tube (not bottom)
Pale purple - (orange)-yellow - red - blue - green.

12. What is the general formula for alkyl halides?
Acids; HCOOCH3 is an ester
left - ppt will form
RX
blue (BTB)

13. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
?G= -ve - E°= +ve
Evaporation

14. lead iodide
bright yellow
different forms of the same element
R=8.31 J/mol/K
?H formation of an element in standard state=0

15. What are allotropes?
same KE - but PEice<PEwater
ionic and form hydrogen and hydroxide
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
different forms of the same element

16. Do you use J or kJ for ?H - ?S - and ?G?
?H-kJ - ?S-J - ?G-kJ
are less dense than water
acids
Heptane

17. A Bronsted-Lowry base is...
proton acceptor.
q=mc?T q=mL (or n x ?h)
Transition element compounds (except if it has a full or empty d shell)
Kc=Kp

18. What is the conjugate acid of H2PO4?
ethers
H3PO4
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
bright yellow

19. What equipment do you need for 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
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
T increases exponentially the proportion of molecules with E > Ea

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

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21. Color (absorbance) is proportional to ________
Most are soluble except Ag - Pb
O2 needs 4F/mol H2 needs 2F/mol
Concentration
Anode

22. phosphates
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
How grouped results are
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Most INsoluble except group 1 and ammonium

23. dichromate (soln + most solids)
linear
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)
Orange
acids

24. What is the formula for summation?

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25. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Suniverse increases for spontaneous processes
?G=negative - E° must be positive
Selective absorption

26. For a dibasic acid (H2A) - [A²?]= ____ ?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
K2
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
+4-covalent - +2-ionic

27. What is the word equation for addition polymerisation?
acid + alcohol
At half equivalence - pH=pKa
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)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

28. Why are noble gases stable?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Glowing splint (positive result=relights)
Ksp = 27s4
K1 x K2

29. Does reactivity increase/decrease going down group 1 and group 17?
Purple
Increases down group 1 decreases down group 17
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Acid rain - dissolves marble buildings/statues and kills trees.

30. Name C7H16
Check for air bubbles in the buret and remove the buret funnel from the buret
Greenish-yellow gas
Heptane
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

31. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Making sigma bonds and holding lone pairs
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Heat a test tube at an angle at the side of the tube (not bottom)

32. potassium permanganate
Big K=kf/kr
Greenish-yellow gas
Purple
lighted splint (positive result=pop)

33. What apparatus do you use to pour liquids?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Pour liquids using a funnel or down a glass rod
Insoluble
Sulfur

34. What two types of substances are present in all redox reactions?
OH?
Purple
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)
an oxidized and reduced substance

35. nitrate
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Anode
Silvery gray solid - brown - purple
NO3?

36. What is the formula for alkenes?
Add acid to water so that the acid doesn't boil and spit
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
CnH2n

37. What measuring device would you use for very small volumes of liquids?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Pipette (burette if need repetition)
All except for lithium
SO4²?

38. chlorite
Anode
Acids; HCOOCH3 is an ester
ClO2?
Insoluble except for nitrate and acetate

39. Name 2 ways in which you can create a buffer?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
OH?
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)

40. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
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
same KE - but PEice<PEwater
CnH2n+2

41. acetates
They stay the same.
zero
Soluble
ClO3?

42. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Soluble except Ag - Pb - Ca - Sr Ba)
But S° of element is not zero (except at 0K)
Ksp = 4s³

43. ammonium/ammonium compounds
K1 x K2
Mono; di; tri; tetra; penta; hexa.
Soluble
Monomer + monomer = polymer product + a simple molecule such as water or HCl

44. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
How grouped results are
Purple
RNH2

45. What do acids plus active metals form?
Selective absorption
Disulfur dichloride
S2O3²?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

46. What shape is water?
CnH2n+1 often designated 'R' ex C3H7 is propyl
fractional distillation
catalyst=conc H2SO4
bent

47. sulfate
?H formation of an element in standard state=0
+4-covalent - +2-ionic
SO4²?
zero

48. 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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49. An amphiprotic (amphoteric) species is...
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Glowing splint (positive result=relights)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

50. What do group I/II metal oxides and acids form?
CO3²?
HClO4
Graduated cylinder
Salt and water