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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. If a weak acid is diluted more - what happens to its % dissociation value?
Salt + water.
Salts (ex: CaO + SO2 ? CaSO3)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Increases.

2. How do you identify which is oxidized or otherwise?
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.
look for changes in oxidation # - the one that goes up is oxidized and is the RA
CnH2n+2
Only temperature

3. What do metal oxides plus non- metal oxides form?
E=q + w (negative is by system - positive is on system)
ns² electrons (first in-first out)
Salts (ex: CaO + SO2 ? CaSO3)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

4. Does reactivity increase/decrease going down group 1 and group 17?
Hg²?
Increases down group 1 decreases down group 17
Distillation
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

5. Why are i factors (Van't Hoff factors) often less than ideal?
Cu3(PO4)2
How close results are to the accepted value
Sulfur
ion pairing

6. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Heptane
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Exothermic
Current - time and charge on ion (moles of e used in half cell reaction)

7. What is the general formula of an alkane?
CnH(2n+2)
ClO3?
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
Exothermic

8. What shape is carbon dioxide?
Salt and water
linear
Ions go through the salt bridge - electrons go through metal wires in the external circuit
?H formation of an element in standard state=0

9. Where are group I metals stored?
diamond and graphite
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Big K=kf/kr
Group I metals (soft metals) are stored under oil

10. What is the general formula for an aldehyde?
chemically (ex: with carbon)
K1 x K2
They stay the same.
RCHO (carbonyl at end)

11. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
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
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
All except for lithium

12. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
Increases.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

13. What is the formula for alkenes?
ROR
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
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
CnH2n

14. What complex ion does ammonia form with silver? copper? cadmium? zinc?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
An active metal.
CO3²?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

15. An amphiprotic (amphoteric) species is...
Tetrahedral
RCOOR
Mono; di; tri; tetra; penta; hexa.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

16. Buffer capacity must contain decent amounts of a ________ ________
brown volatile liquid
Q=It (time in seconds)
Conjugate pair (one must be a weak base or acid)
ion pairing

17. Aromatic compounds contain what?
Orange
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
They stay the same.
The benzene ring (or more correctly the phenyl group - C6H5)

18. Is a graduated cylinder or beaker more accurate?
R=8.31 J/mol/K
Graduated cylinder
chemically (ex: with carbon)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

19. How many faradays of electric charge do you need to produce one mole of O2? H2?
ns² electrons (first in-first out)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
O2 needs 4F/mol H2 needs 2F/mol
Unsaturated - addition (ex: decolorize bromine solution)

20. What type of solutions do small - highly charged cations tend to form?
|experimental - accepted|/accepted X 100
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
H+

21. What do ions and electrons travel through in a voltaic/electrolytic cell?
blue (BTB)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Decant
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

22. silver iodide
The dilution effect when the solutions mix. M1V1 = M2V2
an oxidized and reduced substance
Pale yellow
Insoluble

23. sulfate
it's lower and occurs over less sharp a range
SO4²?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
chemically (ex: with carbon)

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

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25. Do you use J or kJ for ?H - ?S - and ?G?
?H-kJ - ?S-J - ?G-kJ
ClO3?
Orange
same KE - but PEice<PEwater

26. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
H+
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
proton donor base

27. What does the solubility of organic compounds depend on?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Eudiometer
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
They decrease (or could be the same if the solid has ONLY JUST disappeared)

28. What shape is methane?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Greenish-yellow gas
Ppt will NOT form (unsaturated)
Tetrahedral

29. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
allow for the vapor pressure of water and make sure to level levels
Increases down group 1 decreases down group 17

30. mercury (II) ion
Ksp = 27s4
Sigma bonds are stronger than pi bonds
Evaporation
Hg²?

31. How many normal boiling points and boiling points are there?

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32. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
it reacts by substitution NOT addition
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
zero

33. Esters smell like _______ and amines smell like _______ and are ______.
O2 needs 4F/mol H2 needs 2F/mol
Most INsoluble except group 1 and ammonium
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
fruit - fish - bases

34. What is the pH of 1.0M HCl? 1M NaOH?
HClO4
0 and 14
K2
Salt + water

35. copper sulfate
H3PO4
blue
PO4³?
RCOR

36. What is the test for hydrogen?
a-IMFs - b-molecular volume
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
lighted splint (positive result=pop)
Current - time and charge on ion (moles of e used in half cell reaction)

37. What changes Keq?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Only temperature
K2

38. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
How close results are to the accepted value
Group I metals (soft metals) are stored under oil
a-IMFs - b-molecular volume

39. What is the formula of copper (II) phosphate?
Initiation energy (NOT Ea)
How close results are to the accepted value
Cu3(PO4)2
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

40. What do you use for an acid spill? base spill?
O2 needs 4F/mol H2 needs 2F/mol
Sulfur
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
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

41. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
C2O4²?
blue glass - it filters UV
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
boiling without losing volatile solvents/reactants

42. What is the general formula for an acid?
Silvery gray solid - brown - purple
RCOOH
Clear
Salt + water

43. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
basic
Anode - oxygen. Cathode - hydrogen
atoms
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

44. carbonates
voltaic: - electrolytic: +
boiling without losing volatile solvents/reactants
Insoluble except group 1 and ammonium
Distillation

45. potassium permanganate
linear
Purple
Clear
Ionic compounds

46. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Ksp = 108s5
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
small size and high charge
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

47. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
Glowing splint (positive result=relights)
A) any range. b) 8-10 c) 4-6
?G=negative - E° must be positive
Monomer + monomer = polymer product + a simple molecule such as water or HCl

48. Is the ?H formation of an element in standard state zero?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
No - it depends on the number of ions produced on dissolving.
?H formation of an element in standard state=0
Monomer + monomer = polymer product + a simple molecule such as water or HCl

49. What is the sign of the anode in voltaic cells? in electrolytic cells?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Iodine and CO2 (dry ice)
yellow
voltaic: - electrolytic: +

50. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
H3PO4
ClO2?
metal oxides and hydrides are ionically bonded and basic