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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 can metals like iron and zinc be reduced?
Molecules with the same molecular formulas - but different structural formulas
CO3²?
lighted splint (positive result=pop)
chemically (ex: with carbon)

2. What are isotopes?
Add acid to water so that the acid doesn't boil and spit
Products - reactants (except for BDE when it's reactants - products)
proton acceptor.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

3. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Molecules with the same molecular formulas - but different structural formulas
Disulfur dichloride

4. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
?G=negative - E° must be positive
bent
E=q + w (negative is by system - positive is on system)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

5. What part of a liquid do you look at to measure its volume?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Read the bottom of the meniscus
by electrolysis

6. A Bronsted-Lowry base is...
Sulfur
Graduated cylinder
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
proton acceptor.

7. Color is due to ______ _______ of light.
All except for lithium
Selective absorption
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
H2O + CO2 (it decomposes readily)

8. What is the word equation for addition polymerisation?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

9. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
Soluble except Ag - Pb - Ca - Sr Ba)
10?8
Group I metals (soft metals) are stored under oil
Mono; di; tri; tetra; penta; hexa.

10. carbonates
Insoluble except group 1 and ammonium
atoms
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Distillation

11. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
P2O5
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
S crystal at 0K=0

12. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Pale purple - (orange)-yellow - red - blue - green.
Soluble except Ag - Pb - Ca - Sr Ba)
it is lower and occurs over less sharp a range
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.

13. What does saturated mean? Unsaturated?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Exothermic
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

14. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
linear
catalyst=conc H2SO4
ClO?

15. What is an Alkyl group?

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16. What complex ion does ammonia form with silver? copper? cadmium? zinc?
zero
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Acid rain - dissolves marble buildings/statues and kills trees.
NH2?

17. When driving off water from a hydrate - how do you tell you're done?
No - it depends on the number of ions produced on dissolving.
Combine the equations for the half reactions in the non-spontaneous direction
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
left - ppt will form

18. How are metal oxides and hydrides bonded? are they acidic or basic?
Salt + water
red - green - blue
metal oxides and hydrides are ionically bonded and basic
The benzene ring (or more correctly the phenyl group - C6H5)

19. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
Soluble except Ag - Pb - Ca - Sr Ba)
Hg²?
Synthesis - separation and purification of the product and its identification.

20. dichromate
Cr2O7²?
Both electrons come from the same atom (just as good as a regular bond)
Acid rain - dissolves marble buildings/statues and kills trees.
CnH2n+2

21. phosphate
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
non-metal oxides and hydrides are covalently bonded and are acidic.
PO4³?
blue

22. Which of the rates changes more when temperature is increased?
C2O4²?
Filtration
Sigma bonds are stronger than pi bonds
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

23. What reacts with an acid to create hydrogen gas?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
do not change
An active metal.
Trigonal pyramidal

24. How are strong ones written?
strong acids/bases are written as H+ or OH- ions
+4-covalent - +2-ionic
Heptane
Identity and purity (impure compounds usually have broad & low melting points)

25. Buffer capacity must contain decent amounts of a ________ ________
left - ppt will form
Conjugate pair (one must be a weak base or acid)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
boiling without losing volatile solvents/reactants

26. What apparatus do you use to separate 2 immiscible liquids?
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.
Separating funnel
Pale yellow
Insoluble (except group 1 ammonium and Ba)

27. What is the relationship in strength between sigma and pi bonds?
HClO4
it's lower and occurs over less sharp a range
Sigma bonds are stronger than pi bonds
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

28. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
An active metal.
it is lower and occurs over less sharp a range
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

29. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
Acidified
Acid rain - dissolves marble buildings/statues and kills trees.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

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

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31. permanganate
Insoluble
+4-covalent - +2-ionic
Unsaturated - addition (ex: decolorize bromine solution)
MnO4?

32. What equipment do you need for a titration?
Glowing splint (positive result=relights)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
it is lower and occurs over less sharp a range

33. What is the pH of 1.0M HCl? 1M NaOH?
linear
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
acid + alcohol
0 and 14

34. Acid plus base make?
brown volatile liquid
are less dense than water
Salt + water.
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

35. Colorless doesn't mean ______
RX
zero
RCOR
Clear

36. nitrate
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
NO3?
H2PO4?

37. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
RCHO (carbonyl at end)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Anode - oxygen. Cathode - hydrogen

38. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Iodine and CO2 (dry ice)
redox reaction
Ksp = 4s³
H+

39. What is the general formula for an acid?
non-metal oxides and hydrides are covalently bonded and are acidic.
a-IMFs - b-molecular volume
RCOOH
q=mc?T q=mL (or n x ?h)

40. ammonium/ammonium compounds
The benzene ring (or more correctly the phenyl group - C6H5)
blue (BTB)
Soluble
Insoluble except for nitrate and acetate

41. What is the test for hydrogen?
do not change
?H formation of an element in standard state=0
lighted splint (positive result=pop)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

42. Give an example of a concentrated weak acid.
Soluble except Ag - Pb - Ca - Sr Ba)
same KE - but PEice<PEwater
Glacial acetic acid
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)

43. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
CO3²?
OH?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
0 and 14

44. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
Conjugate pair (one must be a weak base or acid)
Making sigma bonds and holding lone pairs
are less dense than water

45. 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.
A) any range. b) 8-10 c) 4-6
The compound with the lowest Ksp value.
zero-th: decreases - first: constant - second: increases
Distillation

46. chlorine
Most are soluble except Ag - Pb
E=q + w (negative is by system - positive is on system)
Greenish-yellow gas
Conjugate pair (one must be a weak base or acid)

47. What do you need to make a polymer?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
proton acceptor.
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)
CnH2n-2

48. What is the catalyst for this reaction Ester + ?
Perform ICE BOX calculation based on K1
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
RNH2
catalyst=conc H2SO4

49. group 1 ions/compounds
ion pairing
Soluble
Products - reactants (except for BDE when it's reactants - products)
Unsaturated - addition (ex: decolorize bromine solution)

50. What are the names and formulas of the 6 strong acids?
Salt and water
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
a-IMFs - b-molecular volume
Group I metals (soft metals) are stored under oil