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AP Chemistry 2

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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 does a short - sharp melting point indicate?
strong acids/bases are written as H+ or OH- ions
Identity and purity (impure compounds usually have broad & low melting points)
Ksp = s²
NH4?

2. How do you explain trends in atomic properties using Coulomb's Law?
Ksp = 108s5
proton donor base
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
No - it depends on the number of ions produced on dissolving.

3. lead compounds
Insoluble except nitrate and acetate
CnH2n+1 often designated 'R' ex C3H7 is propyl
Sigma bonds are stronger than pi bonds
Insoluble (except group 1 ammonium and Ba)

4. What is the formula for alkenes?
CnH2n
boiling without losing volatile solvents/reactants
MnO4?
blue glass - it filters UV

5. What are the common strong bases?
an oxidized and reduced substance
Group 1 hydroxides (ex: NaOH)
fruit - fish - bases
Read the bottom of the meniscus

6. copper sulfate
blue
zero-th: decreases - first: constant - second: increases
?H-kJ - ?S-J - ?G-kJ
Soluble

7. What is the sign of the anode in voltaic cells? in electrolytic cells?
|experimental - accepted|/accepted X 100
Filtration
Silvery gray solid - brown - purple
voltaic: - electrolytic: +

8. potassium permanganate
proton donor base
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Silvery gray solid - brown - purple
Purple

9. perchlorate
Current - time and charge on ion (moles of e used in half cell reaction)
ClO4?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Ksp = 27s4

10. A geometric (or cis-trans) isomer exists due to.....
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
water and substances with (s) less dense than
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

11. An amphiprotic (amphoteric) species is...
Q=It (time in seconds)
H2O + CO2 (it decomposes readily)
Making sigma bonds and holding lone pairs
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

12. Do you use J or kJ for ?H - ?S - and ?G?
Insoluble except nitrate and acetate
?H-kJ - ?S-J - ?G-kJ
zero
White precipitate

13. How does group 1 metals' density compare to water's?
Hg2²?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
proton acceptor.
are less dense than water

14. Colorless doesn't mean ______
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Clear
K2
Separating funnel

15. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
CnH2n-2
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.

16. What are the products of the reaction between group 1 metals and water?

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17. What do group I/II metal oxides and acids form?
non-metal oxides and hydrides are covalently bonded and are acidic.
Making sigma bonds and holding lone pairs
Salt and water
redox reaction

18. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
S crystal at 0K=0
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
10?8
metal oxides and hydrides are ionically bonded and basic

19. Does Benzene react by addition or substitution?
it reacts by substitution NOT addition
CnH2n-2
At half equivalence - pH=pKa
strong acids/bases are written as H+ or OH- ions

20. What is the formula for percent error?
Mono; di; tri; tetra; penta; hexa.
acid + alcohol
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
|experimental - accepted|/accepted X 100

21. What do metal oxides plus non- metal oxides form?
redox reaction
CnH2n+1 often designated 'R' ex C3H7 is propyl
Salts (ex: CaO + SO2 ? CaSO3)
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia

22. If a weak acid is diluted more - what happens to its % dissociation value?
water and substances with (s) less dense than
it's lower and occurs over less sharp a range
Increases.
Mono; di; tri; tetra; penta; hexa.

23. What are isotopes?
H2PO4?
10?8
ion pairing
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

24. Are weak acids (and bases) written dissociated?

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25. What process do you use to obtain the solute from a solution?
do not change
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Evaporation
All except for lithium

26. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
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.
H+
Selective absorption
H2O + CO2 (it decomposes readily)

27. What type of compounds do Group 14 form?
H2PO4?
ClO2?
+4-covalent - +2-ionic
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

28. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Check for air bubbles in the buret and remove the buret funnel from the buret
Unsaturated - addition (ex: decolorize bromine solution)
Add acid to water so that the acid doesn't boil and spit

29. During a titration what is present in the beaker at the equivalence point?
A salt solution.
Identity and purity (impure compounds usually have broad & low melting points)
zero-th: decreases - first: constant - second: increases
Conjugate pair (one must be a weak base or acid)

30. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
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?)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
zero
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)

31. What is the pH of 1.0M HCl? 1M NaOH?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
0 and 14
?H formation of an element in standard state=0
non-metal oxides and hydrides are covalently bonded and are acidic.

32. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Cr2O7²?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Soluble
Reduction always takes place at the cathode (RED CAT) In both types of cell!

33. How does benzene compare in reactivity to alkenes?
no - they're written undissociated (HAaq)
benzene is less reactive than alkenes
But S° of element is not zero (except at 0K)
Pipette (burette if need repetition)

34. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Soluble
White precipitate
PO4³?

35. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
bright yellow
chemically (ex: with carbon)

36. What are two allotropes of carbon?
0.10M HCl (more ions)
Greenish-yellow gas
Graduated cylinder
diamond and graphite

37. dichromate
Salts (ex: CaO + SO2 ? CaSO3)
blue
Cr2O7²?
Heptane

38. chlorate
ClO3?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Check for air bubbles in the buret and remove the buret funnel from the buret
CnH2n-2

39. What is the difference between equivalence point and end point of a titration.
Check for air bubbles in the buret and remove the buret funnel from the buret
zero
it is lower and occurs over less sharp a range
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

40. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
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)
Iodine and CO2 (dry ice)
RCOOR

41. What do you need to make a polymer?
Pipette (burette if need repetition)
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)
Unsaturated - addition (ex: decolorize bromine solution)
H+

42. Where are group I metals stored?
Acids; HCOOCH3 is an ester
Iodine and CO2 (dry ice)
Group I metals (soft metals) are stored under oil
hydroxides (ex: Ba(OH)2)

43. lead iodide
Group 1 hydroxides (ex: NaOH)
bright yellow
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
The Faraday or Faraday's constant.

44. What is the general formula for an aldehyde?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
RCHO (carbonyl at end)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Both electrons come from the same atom (just as good as a regular bond)

45. What is reflux?
Pale purple - (orange)-yellow - red - blue - green.
boiling without losing volatile solvents/reactants
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Increases down group 1 decreases down group 17

46. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
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
Ksp = 27s4
The one with most oxygen atoms (highest oxidation number)
More chaotic (ex: gases made)

47. What process do you use to separate two liquids with different boiling points?
fractional distillation
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
An active metal.
Group I metals (soft metals) are stored under oil

48. What are hybrid orbitals used for?
A salt solution.
Conjugate pair (one must be a weak base or acid)
Making sigma bonds and holding lone pairs
bases

49. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Increases.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
an oxidized and reduced substance
a-IMFs - b-molecular volume

50. How do you clean a buret/pipette for a titration?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
PO4³?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

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AP Chemistry 2

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