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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. What process do you use to obtain a solvent from a solution?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Distillation
?G=negative - E° must be positive
H2O + CO2 (it decomposes readily)

2. When driving off water from a hydrate - how do you tell you're done?
Ksp = 27s4
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
But S° of element is not zero (except at 0K)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

3. What is the formula for percent error?
Silvery gray solid - brown - purple
|experimental - accepted|/accepted X 100
Most are soluble except Ag - Pb
non-metal oxides and hydrides are covalently bonded and are acidic.

4. primary colors
red - green - blue
linear
Pour liquids using a funnel or down a glass rod
proton donor base

5. Colorless doesn't mean ______
Concentration
by electrolysis
Initiation energy (NOT Ea)
Clear

6. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Most INsoluble except group 1 and ammonium
do not change
Selective absorption

7. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
Hg2²?
S2O3²?
ethers

8. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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9. Which value of R do you use for all energy and kinetics calculations?
White precipitate
a-IMFs - b-molecular volume
Anode - oxygen. Cathode - hydrogen
R=8.31 J/mol/K

10. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
Mn²? - Cr³? - Cr³
Glacial acetic acid
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

11. What complex ion does ammonia form with silver? copper? cadmium? zinc?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
basic
ClO?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

12. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Iodine and CO2 (dry ice)
K1 x K2
Suniverse increases for spontaneous processes
a-IMFs - b-molecular volume

13. What is the conjugate base of NH3?
NH2?
S2O3²?
Distillation
boiling without losing volatile solvents/reactants

14. Alkenes are ________ and react by __________
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Unsaturated - addition (ex: decolorize bromine solution)
neutralization: high K - H2O product dissociation: low K - H2O reactant
boiling without losing volatile solvents/reactants

15. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
HClO4
water and substances with (s) less dense than
acid + alcohol
by electrolysis

16. BaSO4
RCOOH
How grouped results are
Pale yellow
Insoluble

17. ammonium/ammonium compounds
ClO4?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Soluble
Most are soluble except Ag - Pb

18. What process do you use to separate two liquids with different boiling points?
fractional distillation
Exothermic
Products - reactants (except for BDE when it's reactants - products)
NH2?

19. During a titration what is present in the beaker at the equivalence point?
A salt solution.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
different forms of the same element
Acidified

20. Name 2 ways in which you can create a buffer?
neutralization: high K - H2O product dissociation: low K - H2O reactant
zero-th: decreases - first: constant - second: increases
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)
Time?¹ - (ex. s?¹ - hr?¹ - etc)

21. How does benzene compare in reactivity to alkenes?
Pale purple - (orange)-yellow - red - blue - green.
Conjugate pair (one must be a weak base or acid)
Initiation energy (NOT Ea)
benzene is less reactive than alkenes

22. sulfates
Kc=Kp
Soluble except Ag - Pb - Ca - Sr Ba)
linear
Most are soluble except Ag - Pb

23. What part of a liquid do you look at to measure its volume?
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
water and substances with (s) less dense than
K2
Read the bottom of the meniscus

24. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
it is lower and occurs over less sharp a range
No - NH3 and HCl gases are extremely soluble
Time?¹ - (ex. s?¹ - hr?¹ - etc)

25. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
CnH2n+2
ionic and form hydrogen and hydroxide

26. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
NH4?
Soluble
same KE - but PEice<PEwater
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

27. What do group I/II metal oxides and acids form?
Salt and water
CnH2n-2
O2 needs 4F/mol H2 needs 2F/mol
No - NH3 and HCl gases are extremely soluble

28. Which of the rates changes more when temperature is increased?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
benzene is less reactive than alkenes

29. What is the general formula of an alkane?
CnH(2n+2)
More chaotic (ex: gases made)
Both electrons come from the same atom (just as good as a regular bond)
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)

30. What is the formula of butane?
C4H10
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Ksp = 108s5
CnH2n+1 often designated 'R' ex C3H7 is propyl

31. potassium permanganate
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Purple
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Tetrahedral

32. Name C7H16
H+
Heptane
blue (BTB)
H2PO4?

33. When combining half equations - what do you do to E° values when multiplying coefficients?
C4H10
RCOOR
0 and 14
Nothing

34. What are two allotropes of carbon?
CN?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Soluble
diamond and graphite

35. What do metal oxides plus non- metal oxides form?
Synthetic condensation polymer (aka a polyamide)
They stay the same.
Salts (ex: CaO + SO2 ? CaSO3)
Sigma bonds are stronger than pi bonds

36. What is the formula for alkynes?
acids
Anode
CnH2n-2
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

37. Aromatic compounds contain what?
The benzene ring (or more correctly the phenyl group - C6H5)
hydroxides (ex: Ba(OH)2)
It ceases - the circuit is broken.
Current - time and charge on ion (moles of e used in half cell reaction)

38. What electrons are lost/gained first in transition element ions?
brown volatile liquid
ns² electrons (first in-first out)
allow for the vapor pressure of water and make sure to level levels
boiling without losing volatile solvents/reactants

39. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Soluble
RCHO (carbonyl at end)
Anode - oxygen. Cathode - hydrogen
Disulfur dichloride

40. A geometric (or cis-trans) isomer exists due to.....
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
fruit - fish - bases
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

41. What is the test for hydrogen?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
q=mc?T q=mL (or n x ?h)
lighted splint (positive result=pop)

42. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
Soluble
Identity and purity (impure compounds usually have broad & low melting points)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

43. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Mn²? - Cr³? - Cr³
They stay the same.

44. When a cell is 'flat' What is its voltage?
atoms
Selective absorption
Molecules with the same molecular formulas - but different structural formulas
zero

45. What are the signs for ?G and E° for spontaneous reactions?
No - it depends on the number of ions produced on dissolving.
ionic and form hydrogen and hydroxide
?G= -ve - E°= +ve
Graduated cylinder

46. What changes Keq?
S crystal at 0K=0
Only temperature
Exothermic (?H for ANY sa/sb = -57kJ/mol)
ion pairing

47. Name six characteristics of transition elements (or their compounds)
Group 1 hydroxides (ex: NaOH)
hydroxides (ex: Ba(OH)2)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
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)

48. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Silvery gray solid - brown - purple
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
No - it depends on the number of ions produced on dissolving.
zero

49. chlorate
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
ClO3?
Kc=Kp
They decrease (or could be the same if the solid has ONLY JUST disappeared)

50. What type of compounds do metals/non metals form?
Ionic compounds
ROR
Saturated - Substitution (which requires more radical conditions)
Unsaturated - addition (ex: decolorize bromine solution)