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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. cyanide
Ksp = 108s5
CN?
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.
How grouped results are

2. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
How close results are to the accepted value
0 and 14
no - they're written undissociated (HAaq)

3. sulfate
SO4²?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
ROR
ionic and form hydrogen and hydroxide

4. What do group I/II metal oxides plus water form?
CO3²?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
bases

5. acetate
Identity and purity (impure compounds usually have broad & low melting points)
RCHO (carbonyl at end)
Acid rain - dissolves marble buildings/statues and kills trees.
CH3COO?

6. ammonium/ammonium compounds
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
The one with most oxygen atoms (highest oxidation number)
Distillation
Soluble

7. What type of compounds do metals/non metals form?
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.
Ionic compounds
Kc=Kp
-Ea/R

8. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
RCOOH
basic
How close results are to the accepted value
a-IMFs - b-molecular volume

9. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
[A?]/[HA] x 100 or [BH?]/[B] x 100
CN?
SO4²?
CO (poisonous)

10. Does Benzene react by addition or substitution?
Saturated - Substitution (which requires more radical conditions)
it reacts by substitution NOT addition
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
strong acids/bases are written as H+ or OH- ions

11. phosphate
RCOR
metal oxides and hydrides are ionically bonded and basic
PO4³?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

12. What process do you use to obtain the precipitate from a solution?
Mn²? - Cr³? - Cr³
Filtration
it's lower and occurs over less sharp a range
K1 x K2

13. An amphiprotic (amphoteric) species is...
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
MnO4?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
H2PO4?

14. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
OH?
chemically (ex: with carbon)
RCOR

15. What is the general formula for an ether?
ROR
Purple
O2 needs 4F/mol H2 needs 2F/mol
Sulfur

16. What is reflux?
No - it depends on the number of ions produced on dissolving.
Making sigma bonds and holding lone pairs
boiling without losing volatile solvents/reactants
Acidified

17. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
Anode - oxygen. Cathode - hydrogen
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
Insoluble except nitrate and acetate

18. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Only temperature
Hg²?
Most INsoluble except group 1 and ammonium

19. What effect does increasing the size/surface area of a voltaic cell have on the cell?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
P2O5
Unsaturated - addition (ex: decolorize bromine solution)
Q=It (time in seconds)

20. What is the general formula for alkyl halides?
RX
ion pairing
ns² electrons (first in-first out)
Insoluble

21. What does the solubility of organic compounds depend on?
Concentration
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

22. For a dibasic acid (H2A) - [A²?]= ____ ?
allow for the vapor pressure of water and make sure to level levels
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
The one with most oxygen atoms (highest oxidation number)
K2

23. chromate
CrO4²?
bent
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

24. When combining half equations - what do you do to E° values when multiplying coefficients?
blue glass - it filters UV
No - it depends on the number of ions produced on dissolving.
At half equivalence - pH=pKa
Nothing

25. What is the formula for percent error?
|experimental - accepted|/accepted X 100
Reduction always takes place at the cathode (RED CAT) In both types of cell!
hydroxides (ex: Ba(OH)2)
Combine the equations for the half reactions in the non-spontaneous direction

26. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Current - time and charge on ion (moles of e used in half cell reaction)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
basic

27. What is a coordinate covalent bond?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Unsaturated - addition (ex: decolorize bromine solution)
Both electrons come from the same atom (just as good as a regular bond)
acids

28. How many faradays of electric charge do you need to produce one mole of O2? H2?
a-IMFs - b-molecular volume
atoms
CnH2n
O2 needs 4F/mol H2 needs 2F/mol

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

30. Nonmetals are good _____ agents. Metals are good _______ agents.
Ksp = 27s4
ion pairing
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
No - it depends on the number of ions produced on dissolving.

31. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
?G=negative - E° must be positive
blue (BTB)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
same KE - but PEice<PEwater

32. lead iodide
T increases exponentially the proportion of molecules with E > Ea
strong acids/bases are written as H+ or OH- ions
benzene is less reactive than alkenes
bright yellow

33. chromate ion (soln + most solids)
Salt + water.
yellow
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)

34. What are isomers?
Heptane
Glacial acetic acid
Molecules with the same molecular formulas - but different structural formulas
#ligands=charge x2

35. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
water and substances with (s) less dense than
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
At half equivalence - pH=pKa

36. What do you need to make a polymer?
CrO4²?
do not change
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)
Graduated cylinder

37. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
non-metal oxides and hydrides are covalently bonded and are acidic.
ns² electrons (first in-first out)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

38. What are isotopes?
neutralization: high K - H2O product dissociation: low K - H2O reactant
water and substances with (s) less dense than
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Filtration

39. Name C7H16
water and substances with (s) less dense than
Combine the equations for the half reactions in the non-spontaneous direction
brown volatile liquid
Heptane

40. What is the formula for alkynes?
An active metal.
zero
bent
CnH2n-2

41. What do ions and electrons travel through in a voltaic/electrolytic cell?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Identity and purity (impure compounds usually have broad & low melting points)
acid + alcohol
Ions go through the salt bridge - electrons go through metal wires in the external circuit

42. What do nonmetal oxides plus water form?
acids
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Silvery gray solid - brown - purple
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

43. What do you use to look at burning magnesium? why?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
blue glass - it filters UV
Monomer + monomer = polymer product + a simple molecule such as water or HCl
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

44. The definition of acidic basic and neutral aqueous solutions is:
Synthetic condensation polymer (aka a polyamide)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

45. If a weak acid is diluted more - what happens to its % dissociation value?
Salts (ex: CaO + SO2 ? CaSO3)
Products - reactants (except for BDE when it's reactants - products)
Increases.
Cu3(PO4)2

46. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
Mn²? - Cr³? - Cr³
RCOOR
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

47. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
same KE - but PEice<PEwater
zero
CO2 and H2O
blue glass - it filters UV

48. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
Ppt will NOT form (unsaturated)
Salt and water
metal oxides and hydrides are ionically bonded and basic

49. When can supercooling occur? What does it look like on a cooling curve?

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