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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 is Big K in terms of kf and kr?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Big K=kf/kr
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
hydroxides (ex: Ba(OH)2)

2. Color (absorbance) is proportional to ________
Most INsoluble except group 1 and ammonium
O2 needs 4F/mol H2 needs 2F/mol
left - ppt will form
Concentration

3. What is precision?
How grouped results are
blue (BTB)
Insoluble
Monomer + monomer = polymer product + a simple molecule such as water or HCl

4. Why are noble gases stable?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Transition element compounds (except if it has a full or empty d shell)
H+
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

5. Do anions flow to the cathode or anode?
allow for the vapor pressure of water and make sure to level levels
water and substances with (s) less dense than
Evaporation
Anode

6. How can metals like iron and zinc be reduced?
Insoluble
allow for the vapor pressure of water and make sure to level levels
CH3COO?
chemically (ex: with carbon)

7. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
RCOOR
10?8
More chaotic (ex: gases made)
Sulfur

8. dichromate
CO3²?
ROR
Cr2O7²?
Soluble

9. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
a-IMFs - b-molecular volume
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
0.10M HCl (more ions)

10. What type of compounds do metals/non metals form?
Ionic compounds
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
lighted splint (positive result=pop)

11. Is the freezing of ice endothermic or exothermic?
Exothermic
chemically (ex: with carbon)
same KE - but PEice<PEwater
Evaporation

12. 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
Read the bottom of the meniscus
Monomer + monomer = polymer product + a simple molecule such as water or HCl
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

13. What is the general formula for an acid?
blue
RCOOH
zero
Mono; di; tri; tetra; penta; hexa.

14. sulfates
RNH2
a-IMFs - b-molecular volume
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
Soluble except Ag - Pb - Ca - Sr Ba)

15. What measuring device would you use for very small volumes of liquids?
it's lower and occurs over less sharp a range
Pipette (burette if need repetition)
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
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)

16. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Increases down group 1 decreases down group 17
?G=negative - E° must be positive
H+
-Ea/R

17. What are two substances that sublime at 1 atm when heated?
red - green - blue
Acidified
Iodine and CO2 (dry ice)
Pour liquids using a funnel or down a glass rod

18. What is the formula for alkanes?
+4-covalent - +2-ionic
blue
Iodine and CO2 (dry ice)
CnH2n+2

19. What is the sign of the anode in voltaic cells? in electrolytic cells?
blue
Insoluble
Saturated - Substitution (which requires more radical conditions)
voltaic: - electrolytic: +

20. What is the general formula for an amine?
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.
RNH2
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)
acids

21. What is the general formula for an aldehyde?
fruit - fish - bases
RCHO (carbonyl at end)
it is lower and occurs over less sharp a range
redox reaction

22. What is the sign of the cathode in voltaic cells? in electrolytic cells?
O2 needs 4F/mol H2 needs 2F/mol
bright yellow
voltaic: + electrolytic: -
Big K=kf/kr

23. How do you get the equation for a net electrolysis reaction?
H2O + CO2 (it decomposes readily)
CnH(2n+2)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Combine the equations for the half reactions in the non-spontaneous direction

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

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25. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
The one with most oxygen atoms (highest oxidation number)
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)
Only temperature

26. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Sigma bonds are stronger than pi bonds
diamond and graphite
ClO?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

27. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

28. What value of R do you use for thermo calculations? gas calculations?
No - NH3 and HCl gases are extremely soluble
proton acceptor.
Hg2²?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

29. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
CnH2n
Reduction always takes place at the cathode (RED CAT) In both types of cell!
H3PO4
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.

30. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
Nothing
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Soluble
ClO2?

31. When the salt bridge is removed what happens to the cell reaction?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
It ceases - the circuit is broken.
Salt + water.
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.

32. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Anode
K1 x K2
allow for the vapor pressure of water and make sure to level levels
Salt and water

33. What are allotropes?
different forms of the same element
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
CrO4²?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

34. What is the test for hydrogen?
?H formation of an element in standard state=0
?H-kJ - ?S-J - ?G-kJ
lighted splint (positive result=pop)
[A?]/[HA] x 100 or [BH?]/[B] x 100

35. barium sulfate
White precipitate
Synthesis - separation and purification of the product and its identification.
More chaotic (ex: gases made)
Making sigma bonds and holding lone pairs

36. If Q > Ksp - then system shifts _______ and ppt ______
blue glass - it filters UV
left - ppt will form
ethers
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

37. How does the melting point of a mixture compare to the MP of a pure substance?
No - it depends on the number of ions produced on dissolving.
S2O3²?
it is lower and occurs over less sharp a range
Glowing splint (positive result=relights)

38. What is accuracy?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
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)
How close results are to the accepted value
Ionic compounds

39. Alcohols and _______ are FG isomers
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
ethers
Mono; di; tri; tetra; penta; hexa.

40. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
lighted splint (positive result=pop)
allow for the vapor pressure of water and make sure to level levels
Kc=Kp

41. What are the common strong bases?
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?)
?G=negative - E° must be positive
Group 1 hydroxides (ex: NaOH)
RCOR

42. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
H2PO4?
it is lower and occurs over less sharp a range
Selective absorption

43. carbonate
Glowing splint (positive result=relights)
CO3²?
Soluble
They stay the same.

44. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
Ksp = 4s³
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
RCHO (carbonyl at end)

45. How does benzene compare in reactivity to alkenes?
brown volatile liquid
Perform ICE BOX calculation based on K1
benzene is less reactive than alkenes
HClO4

46. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Saturated - Substitution (which requires more radical conditions)

47. Acids + Carbonates (bicarbonates) make?
same KE - but PEice<PEwater
fruit - fish - bases
different forms of the same element
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

48. Is the ?H formation of an element in standard state zero?
RCHO (carbonyl at end)
?H formation of an element in standard state=0
Filtration
MnO4?

49. What do you use to look at burning magnesium? why?
blue glass - it filters UV
A) any range. b) 8-10 c) 4-6
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)
The dilution effect when the solutions mix. M1V1 = M2V2

50. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
Products - reactants (except for BDE when it's reactants - products)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
ns² electrons (first in-first out)

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AP Chemistry 2

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