Test your basic knowledge |

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 part of a liquid do you look at to measure its volume?
R=8.31 J/mol/K
Read the bottom of the meniscus
Salt and water
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

2. copper sulfate
blue
no - they're written undissociated (HAaq)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Most INsoluble except group 1 and ammonium

3. What process do you use to obtain a solvent from a solution?
CnH(2n+2)
Increases down group 1 decreases down group 17
Separating funnel
Distillation

4. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Concentration
H+
lighted splint (positive result=pop)

5. halides
Soluble
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Experimental mass/theoretical mass X 100
Most are soluble except Ag - Pb

6. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
do not change
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Current - time and charge on ion (moles of e used in half cell reaction)
An active metal.

7. Acids + Carbonates (bicarbonates) make?
Ppt will NOT form (unsaturated)
yellow
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
A salt solution.

8. Where are group I metals stored?
Soluble
Group I metals (soft metals) are stored under oil
Glowing splint (positive result=relights)
Monomer + monomer = polymer product + a simple molecule such as water or HCl

9. Which would cause the bulb in a conductivity apparatus to be brightest?
Clear
0.10M HCl (more ions)
Mono; di; tri; tetra; penta; hexa.
Separating funnel

10. What is the general formula for an ester?
CnH2n+1 often designated 'R' ex C3H7 is propyl
zero-th: decreases - first: constant - second: increases
[A?]/[HA] x 100 or [BH?]/[B] x 100
RCOOR

11. How do you dilute an acid?

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

13. mercury (I) ion
Ionic compounds
strong acids/bases are written as H+ or OH- ions
Hg2²?
A salt solution.

14. What complex ion does ammonia form with silver? copper? cadmium? zinc?
small size and high charge
Only temperature
CN?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

15. What is the conjugate base of NH3?
NH2?
A) any range. b) 8-10 c) 4-6
Insoluble except for nitrate and acetate
same KE - but PEice<PEwater

16. dichromate (soln + most solids)
Orange
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
O2 needs 4F/mol H2 needs 2F/mol

17. mercury (II) ion
Hg²?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Conjugate pair (one must be a weak base or acid)
CnH2n+2

18. Neutralization is an ________ reaction.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Q=It (time in seconds)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Soluble

19. What do you do to get rid of most of the solution from a precipitate?
Decant
RCOR
Selective absorption
-Ea/R

20. What are two allotropes of carbon?
Increases.
diamond and graphite
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CN?

21. How does group 1 metals' density compare to water's?
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)
Salt + water
voltaic: + electrolytic: -
are less dense than water

22. What are two substances that sublime at 1 atm when heated?
White precipitate
by electrolysis
Iodine and CO2 (dry ice)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

23. A Bronsted-Lowry base is...
proton acceptor.
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
blue
They decrease (or could be the same if the solid has ONLY JUST disappeared)

24. What is the formula for percent error?
Perform ICE BOX calculation based on K1
Selective absorption
ClO4?
|experimental - accepted|/accepted X 100

25. chlorine
More chaotic (ex: gases made)
Transition element compounds (except if it has a full or empty d shell)
Greenish-yellow gas
P2O5

26. How do you identify which is oxidized or otherwise?
water and substances with (s) less dense than
look for changes in oxidation # - the one that goes up is oxidized and is the RA
CnH2n+1 often designated 'R' ex C3H7 is propyl
Suniverse increases for spontaneous processes

27. What electrons are lost/gained first in transition element ions?
Purple
ns² electrons (first in-first out)
OH- and NH3
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

28. What is a coordinate covalent 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)
Big K=kf/kr
Both electrons come from the same atom (just as good as a regular bond)
Anode

29. perchlorate
Molecules with the same molecular formulas - but different structural formulas
Glacial acetic acid
ClO4?
yellow

30. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
-Ea/R
Soluble

31. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Hg2²?
Ksp = 4s³
NO3?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

32. bromine
A salt solution.
brown volatile liquid
CN?
K1 x K2

33. Why are i factors (Van't Hoff factors) often less than ideal?
diamond and graphite
Suniverse increases for spontaneous processes
Products - reactants (except for BDE when it's reactants - products)
ion pairing

34. What is the general formula for an acid?
RCOOH
Insoluble (except group 1 ammonium and Ba)
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
O2 needs 4F/mol H2 needs 2F/mol

35. Does Benzene react by addition or substitution?
Tetrahedral
it reacts by substitution NOT addition
ROR
RNH2

36. What type of compounds do metals/non metals form?
CH3COO?
redox reaction
Q=It (time in seconds)
Ionic compounds

37. silver iodide
it's lower and occurs over less sharp a range
CnH2n-2
an oxidized and reduced substance
Pale yellow

38. Give an example of a concentrated weak acid.
zero
At half equivalence - pH=pKa
#ligands=charge x2
Glacial acetic acid

39. hypochlorite
ClO?
ion pairing
Heptane
metal oxides and hydrides are ionically bonded and basic

40. carbonates
Salt and water
CnH2n+2
chemically (ex: with carbon)
Insoluble except group 1 and ammonium

41. dichromate
Only temperature
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Cr2O7²?
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)

42. How are metal oxides and hydrides bonded? are they acidic or basic?
Ksp = 108s5
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.
But S° of element is not zero (except at 0K)
metal oxides and hydrides are ionically bonded and basic

43. If a weak acid is diluted more - what happens to its % dissociation value?
0 and 14
Increases.
It ceases - the circuit is broken.
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

44. What is an Alkyl group?

45. For a dibasic acid (H2A) - [A²?]= ____ ?
K2
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.
it reacts by substitution NOT addition
[A?]/[HA] x 100 or [BH?]/[B] x 100

46. sulfate
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Soluble
SO4²?
Transition element compounds (except if it has a full or empty d shell)

47. cyanide
CN?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Synthetic condensation polymer (aka a polyamide)
+4-covalent - +2-ionic

48. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Pale yellow
Eudiometer

49. sulfates
bent
PO4³?
Soluble except Ag - Pb - Ca - Sr Ba)
OH- and NH3

50. What do hydrocarbons form when they burn in air (oxygen)?
Heptane
0.10M HCl (more ions)
CO2 and H2O
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask