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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.
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 find the pH for a dibasic acid? (H2A)?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Glacial acetic acid
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Perform ICE BOX calculation based on K1

2. phosphates
Most INsoluble except group 1 and ammonium
-Ea/R
strong acids/bases are written as H+ or OH- ions
The dilution effect when the solutions mix. M1V1 = M2V2

3. Alkanes are _________ and react by _________
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Salts (ex: CaO + SO2 ? CaSO3)
Saturated - Substitution (which requires more radical conditions)
No - it depends on the number of ions produced on dissolving.

4. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Group I metals (soft metals) are stored under oil
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)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

5. bromine
methyl formate
Saturated - Substitution (which requires more radical conditions)
brown volatile liquid
Selective absorption

6. What steps do organic labs consist of?
ClO?
Synthesis - separation and purification of the product and its identification.
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Decant

7. How many ligands attach to a central ion in a complex ion?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
#ligands=charge x2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
CN?

8. Aromatic compounds contain what?
The benzene ring (or more correctly the phenyl group - C6H5)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
A) any range. b) 8-10 c) 4-6
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

9. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Group 1 hydroxides (ex: NaOH)
Graduated cylinder
P2O5
H3PO4

10. What changes Keq?
Only temperature
bright yellow
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

11. bromothymol
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
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
blue (BTB)
Iodine and CO2 (dry ice)

12. Name some properties of Group 17
it is lower and occurs over less sharp a range
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Clear
q=mc?T q=mL (or n x ?h)

13. What do hydrocarbons form when they burn in air (oxygen)?
small size and high charge
Distillation
CO2 and H2O
Time?¹ - (ex. s?¹ - hr?¹ - etc)

14. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
All except for lithium
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
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)
Pale purple - (orange)-yellow - red - blue - green.

15. Why are i factors (Van't Hoff factors) often less than ideal?
Big K=kf/kr
Insoluble except nitrate and acetate
The Faraday or Faraday's constant.
ion pairing

16. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Evaporation
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)
Perform ICE BOX calculation based on K1

17. How can metals like iron and zinc be reduced?
ionic and form hydrogen and hydroxide
Identity and purity (impure compounds usually have broad & low melting points)
chemically (ex: with carbon)
Separating funnel

18. What two compounds are great oxidizing agents?

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

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20. What do metal oxides plus acids form?
Salt + water
ROR
red - green - blue
Group I metals (soft metals) are stored under oil

21. Name C7H16
Heptane
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Monomer + monomer = polymer product + a simple molecule such as water or HCl
ns² electrons (first in-first out)

22. What do metal oxides plus non- metal oxides form?
K1 x K2
proton donor base
H2O + CO2 (it decomposes readily)
Salts (ex: CaO + SO2 ? CaSO3)

23. hydroxides
it is lower and occurs over less sharp a range
Insoluble (except group 1 ammonium and Ba)
CnH2n+1 often designated 'R' ex C3H7 is propyl
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

24. What complex ion does ammonia form with silver? copper? cadmium? zinc?
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.
RCHO (carbonyl at end)
Acids; HCOOCH3 is an ester
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

25. If Q < Ksp a ppt ______
CH3COO?
Current - time and charge on ion (moles of e used in half cell reaction)
Ppt will NOT form (unsaturated)
RCHO (carbonyl at end)

26. What word is a clue for a redox reaction?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
strong acids/bases are written as H+ or OH- ions
ClO3?
Acidified

27. How do you get the equation for a net electrolysis reaction?
More chaotic (ex: gases made)
Identity and purity (impure compounds usually have broad & low melting points)
Combine the equations for the half reactions in the non-spontaneous direction
RCHO (carbonyl at end)

28. hydroxide
R=8.31 J/mol/K
OH?
ClO4?
small size and high charge

29. At what point during titration do you have the perfect buffer - and what is the pH at this point?
Trigonal pyramidal
At half equivalence - pH=pKa
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Acids; HCOOCH3 is an ester

30. Name six characteristics of transition elements (or their compounds)
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)
bright yellow
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

31. silver iodide
chemically (ex: with carbon)
Evaporation
bright yellow
Pale yellow

32. What is the formula for alkanes?
H3PO4
CnH2n+2
MnO4?
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.

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

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34. During a titration what is present in the beaker at the equivalence point?
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
boiling without losing volatile solvents/reactants
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
A salt solution.

35. How are strong ones written?
Graduated cylinder
strong acids/bases are written as H+ or OH- ions
ROH
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

36. BaSO4
CH3COO?
zero
An active metal.
Insoluble

37. What equipment do you need for a titration?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
No - NH3 and HCl gases are extremely soluble
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
E=q + w (negative is by system - positive is on system)

38. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
strong acids/bases are written as H+ or OH- ions
water and substances with (s) less dense than
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
CN?

39. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
Exothermic (?H for ANY sa/sb = -57kJ/mol)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Current - time and charge on ion (moles of e used in half cell reaction)

40. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
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.

41. hypochlorite
ClO?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Initiation energy (NOT Ea)
Group 1 hydroxides (ex: NaOH)

42. chlorite
ClO2?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
ROR
At half equivalence - pH=pKa

43. Ca - Sr - Ba
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
ion pairing
NH2?
hydroxides (ex: Ba(OH)2)

44. How do you heat a test tube?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Heat a test tube at an angle at the side of the tube (not bottom)
H2PO4?
Iodine and CO2 (dry ice)

45. If a weak acid is diluted more - what happens to its % dissociation value?
0.10M HCl (more ions)
Increases.
Sigma bonds are stronger than pi bonds
Reduction always takes place at the cathode (RED CAT) In both types of cell!

46. Esters smell like _______ and amines smell like _______ and are ______.
Pour liquids using a funnel or down a glass rod
fruit - fish - bases
How grouped results are
|experimental - accepted|/accepted X 100

47. phosphate
Making sigma bonds and holding lone pairs
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Soluble
PO4³?

48. What process do you use to obtain the precipitate from a solution?
Filtration
basic
do not change
Acids; HCOOCH3 is an ester

49. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
ionic and form hydrogen and hydroxide
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Glowing splint (positive result=relights)
allow for the vapor pressure of water and make sure to level levels

50. What is the word equation for condensation polymerisation ?
C2O4²?
Iodine and CO2 (dry ice)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
ethers