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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 is HCOOCH3?
Insoluble (except group 1 ammonium and Ba)
Acids; HCOOCH3 is an ester
Salt + water.
Silvery gray solid - brown - purple

2. Ions are not ______.
atoms
it is lower and occurs over less sharp a range
Insoluble except for nitrate and acetate
red - green - blue

3. What is the formula for alkynes?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
CO3²?
CnH2n-2
it's lower and occurs over less sharp a range

4. What is the general formula for an alcohol?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Heat a test tube at an angle at the side of the tube (not bottom)
CnH2n+2
ROH

5. What shape is methane?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Transition element compounds (except if it has a full or empty d shell)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Tetrahedral

6. What do you need to make a polymer?
Soluble
CnH2n
non-metal oxides and hydrides are covalently bonded and are acidic.
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)

7. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
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
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
?H formation of an element in standard state=0
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

8. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
No - it depends on the number of ions produced on dissolving.
zero
ROH
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

9. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Hg2²?
The dilution effect when the solutions mix. M1V1 = M2V2
The compound with the lowest Ksp value.
Add acid to water so that the acid doesn't boil and spit

10. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Eudiometer
Combine the equations for the half reactions in the non-spontaneous direction

11. What part of a liquid do you look at to measure its volume?
A) any range. b) 8-10 c) 4-6
Read the bottom of the meniscus
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

12. bromothymol
It ceases - the circuit is broken.
Anode - oxygen. Cathode - hydrogen
Glowing splint (positive result=relights)
blue (BTB)

13. What is the general formula for an ester?
RCOOR
Experimental mass/theoretical mass X 100
bases
an oxidized and reduced substance

14. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
ns² electrons (first in-first out)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
q=mc?T q=mL (or n x ?h)

15. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Reduction always takes place at the cathode (RED CAT) In both types of cell!
allow for the vapor pressure of water and make sure to level levels
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

16. How does benzene compare in reactivity to alkenes?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
benzene is less reactive than alkenes
atoms

17. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Pipette (burette if need repetition)
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
metal oxides and hydrides are ionically bonded and basic

18. What two compounds are great oxidizing agents?

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19. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Silvery gray solid - brown - purple
ROH
same KE - but PEice<PEwater

20. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
zero
S2O3²?
C4H10

21. How are metal oxides and hydrides bonded? are they acidic or basic?
No - NH3 and HCl gases are extremely soluble
diamond and graphite
Current - time and charge on ion (moles of e used in half cell reaction)
metal oxides and hydrides are ionically bonded and basic

22. What do the 'a' and 'b' in Van Der Waal's equation allow for?
ns² electrons (first in-first out)
a-IMFs - b-molecular volume
Ppt will NOT form (unsaturated)
Suniverse increases for spontaneous processes

23. What is the relationship in strength between sigma and pi bonds?
RX
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Sigma bonds are stronger than pi bonds
Ksp = s²

24. What is the name of S2Cl2? (Know how to name others like this - too)
Most INsoluble except group 1 and ammonium
Disulfur dichloride
The compound with the lowest Ksp value.
Orange

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

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26. nitrates
do not change
Unsaturated - addition (ex: decolorize bromine solution)
Soluble
Exothermic (?H for ANY sa/sb = -57kJ/mol)

27. halides
Most are soluble except Ag - Pb
zero
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.
Heptane

28. What is a coordinate covalent bond?
Synthesis - separation and purification of the product and its identification.
OH- and NH3
Both electrons come from the same atom (just as good as a regular bond)
Soluble

29. Color (absorbance) is proportional to ________
#ligands=charge x2
neutralization: high K - H2O product dissociation: low K - H2O reactant
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
Concentration

30. Name six characteristics of transition elements (or their compounds)
ethers
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)
|experimental - accepted|/accepted X 100
Synthesis - separation and purification of the product and its identification.

31. Why are i factors (Van't Hoff factors) often less than ideal?
boiling without losing volatile solvents/reactants
blue
Nothing
ion pairing

32. At what point during titration do you have the perfect buffer - and what is the pH at this point?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
At half equivalence - pH=pKa
ClO2?
Q=It (time in seconds)

33. What is the third law of thermodynamics?
Soluble
Hg²?
S crystal at 0K=0
RCOOR

34. What are isotopes?
are less dense than water
bent
The Faraday or Faraday's constant.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

35. Both Acetic acid and ____________ are also functional isomers.
H2O + CO2 (it decomposes readily)
MnO4?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
methyl formate

36. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
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.
ROR
No - it depends on the number of ions produced on dissolving.

37. What reacts with an acid to create hydrogen gas?
An active metal.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Pale yellow
Trigonal pyramidal

38. What is the general formula for an ether?
ROR
They decrease (or could be the same if the solid has ONLY JUST disappeared)
PO4³?
ion pairing

39. What is the word equation for condensation polymerisation ?
OH?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Pour liquids using a funnel or down a glass rod
Insoluble except for nitrate and acetate

40. How do you explain trends in atomic properties using Coulomb's Law?
CO2 and H2O
Decant
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
CO (poisonous)

41. What is the difference between equivalence point and end point of a titration.
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
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.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

42. silver compounds
Salt + water
Experimental mass/theoretical mass X 100
allow for the vapor pressure of water and make sure to level levels
Insoluble except for nitrate and acetate

43. ________ are Lewis bases - because they can donate a lone pair of electrons.
Iodine and CO2 (dry ice)
OH- and NH3
Ionic compounds
CrO4²?

44. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
Trigonal pyramidal
redox reaction
Ppt will NOT form (unsaturated)

45. An amphiprotic (amphoteric) species is...
Glowing splint (positive result=relights)
Q=It (time in seconds)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
CnH2n-2

46. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
CO (poisonous)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Q=It (time in seconds)
Decant

47. What changes Keq?
OH?
Hg2²?
Only temperature
Most are soluble except Ag - Pb

48. What is the pH of 1.0M HCl? 1M NaOH?
ClO2?
same KE - but PEice<PEwater
0 and 14
blue

49. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Increases.
NO3?
Purple
Acid rain - dissolves marble buildings/statues and kills trees.

50. nitrate
Acid rain - dissolves marble buildings/statues and kills trees.
NO3?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
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.