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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. How do you get Ecell for spontaneous reactions?
Increases down group 1 decreases down group 17
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Glowing splint (positive result=relights)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

2. Acid plus base make?
Salt + water.
allow for the vapor pressure of water and make sure to level levels
Experimental mass/theoretical mass X 100
CO2 and H2O

3. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
ionic and form hydrogen and hydroxide
Ionic compounds
water and substances with (s) less dense than

4. Color is due to ______ _______ of light.
allow for the vapor pressure of water and make sure to level levels
Exothermic
CH3COO?
Selective absorption

5. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
ClO2?
a-IMFs - b-molecular volume
Cu3(PO4)2
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

6. When combining half equations - what do you do to E° values when multiplying coefficients?
Group I metals (soft metals) are stored under oil
Nothing
basic
Q=It (time in seconds)

7. If Q < Ksp a ppt ______
lighted splint (positive result=pop)
Ppt will NOT form (unsaturated)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
NH2?

8. What do you need to make a polymer?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Separating funnel
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)
RCOR

9. When a cell is 'flat' What is its voltage?
zero
basic
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
benzene is less reactive than alkenes

10. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
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
ns² electrons (first in-first out)
do not change

11. What is the charge on a chlorine atom?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
zero
water and substances with (s) less dense than
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

12. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

13. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
MnO4?
At half equivalence - pH=pKa

14. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
CN?
Ionic compounds
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

15. silver iodide
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
acids
Anode
Pale yellow

16. What part of a liquid do you look at to measure its volume?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Acid rain - dissolves marble buildings/statues and kills trees.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Read the bottom of the meniscus

17. mercury (II) ion
Hg²?
Insoluble
blue glass - it filters UV
Only temperature

18. What is the word equation for addition polymerisation?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Anode
#ligands=charge x2
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

19. What do the 'a' and 'b' in Van Der Waal's equation allow for?
zero
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.
a-IMFs - b-molecular volume
Clear

20. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
Group I metals (soft metals) are stored under oil
R=8.31 J/mol/K
blue

21. How do you compute % dissociation?
Distillation
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
[A?]/[HA] x 100 or [BH?]/[B] x 100
Silvery gray solid - brown - purple

22. What is the general formula for an ether?
ROR
It ceases - the circuit is broken.
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Acids; HCOOCH3 is an ester

23. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
OH- and NH3
do not change
Orange

24. What are the units of the first order rate constant?
Pale purple - (orange)-yellow - red - blue - green.
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Salts (ex: CaO + SO2 ? CaSO3)
Current - time and charge on ion (moles of e used in half cell reaction)

25. What is an Alkyl group?

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26. nitrates
Pale purple - (orange)-yellow - red - blue - green.
Soluble
atoms
allow for the vapor pressure of water and make sure to level levels

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
Unsaturated - addition (ex: decolorize bromine solution)
NH4?
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.

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

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29. How are metal oxides and hydrides bonded? are they acidic or basic?
NO3?
Heptane
Conjugate pair (one must be a weak base or acid)
metal oxides and hydrides are ionically bonded and basic

30. What is the catalyst for this reaction Ester + ?
catalyst=conc H2SO4
allow for the vapor pressure of water and make sure to level levels
Graduated cylinder
NH2?

31. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
Soluble except Ag - Pb - Ca - Sr Ba)
Pour liquids using a funnel or down a glass rod
CrO4²?

32. ammonium
They stay the same.
NH4?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Selective absorption

33. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
Initiation energy (NOT Ea)
RX
H2O + CO2 (it decomposes readily)

34. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Add acid to water so that the acid doesn't boil and spit

35. How do you find the pH for a dibasic acid? (H2A)?
are less dense than water
it reacts by substitution NOT addition
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Perform ICE BOX calculation based on K1

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

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37. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
K1 x K2
water and substances with (s) less dense than
Q=It (time in seconds)
|experimental - accepted|/accepted X 100

38. What do you use to look at burning magnesium? why?
Check for air bubbles in the buret and remove the buret funnel from the buret
blue glass - it filters UV
Acids; HCOOCH3 is an ester
hydroxides (ex: Ba(OH)2)

39. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
CrO4²?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
non-metal oxides and hydrides are covalently bonded and are acidic.
CnH2n-2

40. mercury (I) ion
Hg2²?
Most INsoluble except group 1 and ammonium
Iodine and CO2 (dry ice)
Trigonal pyramidal

41. How can metals like iron and zinc be reduced?
A salt solution.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
brown volatile liquid
chemically (ex: with carbon)

42. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
yellow
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
10?8
Insoluble except for nitrate and acetate

43. How does the melting point of a mixture compare to the MP of a pure substance?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Perform ICE BOX calculation based on K1
ns² electrons (first in-first out)
it is lower and occurs over less sharp a range

44. Generally - which oxy acid is strongest?
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
do not change
The one with most oxygen atoms (highest oxidation number)
Concentration

45. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Initiation energy (NOT Ea)
Ksp = 27s4

46. nitrate
K2
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
CO (poisonous)
NO3?

47. What is the third law of thermodynamics?
CnH2n+1 often designated 'R' ex C3H7 is propyl
S crystal at 0K=0
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
NH4?

48. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
blue glass - it filters UV
T increases exponentially the proportion of molecules with E > Ea
Salt and water

49. What things should you remember to do when collecting gas over water?
basic
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)
allow for the vapor pressure of water and make sure to level levels
Silvery gray solid - brown - purple

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

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