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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.
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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. During a titration what is present in the beaker at the equivalence point?
A salt solution.
ClO?
OH- and NH3
non-metal oxides and hydrides are covalently bonded and are acidic.

2. How are non-metal oxides and hydrides bonded? are they acidic or basic?
non-metal oxides and hydrides are covalently bonded and are acidic.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
A salt solution.
Concentration

3. What shape is ammonia?
Increases down group 1 decreases down group 17
Trigonal pyramidal
water and substances with (s) less dense than
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

4. How do you identify which is oxidized or otherwise?
0 and 14
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
10?8
look for changes in oxidation # - the one that goes up is oxidized and is the RA

5. What process do you use to obtain the precipitate from a solution?
Most are soluble except Ag - Pb
CN?
allow for the vapor pressure of water and make sure to level levels
Filtration

6. What measuring device would you use for very small volumes of liquids?
allow for the vapor pressure of water and make sure to level levels
An active metal.
basic
Pipette (burette if need repetition)

7. What are the signs for ?G and E° for spontaneous reactions?
K2
?G= -ve - E°= +ve
Most are soluble except Ag - Pb
S crystal at 0K=0

8. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
Heptane
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

9. What is the general formula for alkyl halides?
But S° of element is not zero (except at 0K)
RX
acid + alcohol
atoms

10. Why are i factors (Van't Hoff factors) often less than ideal?
Separating funnel
a-IMFs - b-molecular volume
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
ion pairing

11. What do you need to make a polymer?
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)
A salt solution.
No - it depends on the number of ions produced on dissolving.
Filtration

12. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Experimental mass/theoretical mass X 100
CnH(2n+2)
CnH2n
H+

13. What are two substances that sublime at 1 atm when heated?
zero
CH3COO?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Iodine and CO2 (dry ice)

14. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
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.
metal oxides and hydrides are ionically bonded and basic
Soluble
10?8

15. What things should you remember to do when collecting gas over water?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
A salt solution.
allow for the vapor pressure of water and make sure to level levels
ion pairing

16. phosphate
Read the bottom of the meniscus
Suniverse increases for spontaneous processes
Nothing
PO4³?

17. dihydrogen phosphate
H2PO4?
Suniverse increases for spontaneous processes
neutralization: high K - H2O product dissociation: low K - H2O reactant
Unsaturated - addition (ex: decolorize bromine solution)

18. How can metals like iron and zinc be reduced?
Hg²?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
chemically (ex: with carbon)
Ksp = 108s5

19. What type of polymer is nylon?
Insoluble (except group 1 ammonium and Ba)
Ionic compounds
Synthetic condensation polymer (aka a polyamide)
Hg2²?

20. Esterification is...
acid + alcohol
Insoluble except group 1 and ammonium
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Acid rain - dissolves marble buildings/statues and kills trees.

21. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
methyl formate
?G= -ve - E°= +ve
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Ksp = 27s4

22. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
Acids; HCOOCH3 is an ester
Experimental mass/theoretical mass X 100
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)

23. What is the charge on a chlorine atom?
NH2?
T increases exponentially the proportion of molecules with E > Ea
Ksp = s²
zero

24. How do you dilute an acid?

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25. Name 2 ways in which you can create a buffer?
H2PO4?
Ksp = 27s4
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)
Transition element compounds (except if it has a full or empty d shell)

26. One mole of electrons carries 96500Coulombs - what is this quantity called?

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27. How many ligands attach to a central ion in a complex ion?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
How grouped results are
#ligands=charge x2
Hg2²?

28. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Filtration
Group I metals (soft metals) are stored under oil
zero
K1 x K2

29. How do you get the equation for a net electrolysis reaction?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Acid rain - dissolves marble buildings/statues and kills trees.
Combine the equations for the half reactions in the non-spontaneous direction
bases

30. When combining half equations - what do you do to E° values when multiplying coefficients?
#ligands=charge x2
Pour liquids using a funnel or down a glass rod
Insoluble except nitrate and acetate
Nothing

31. dichromate
P2O5
Cr2O7²?
Only temperature
Separating funnel

32. What are the names and formulas of the 6 strong acids?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
allow for the vapor pressure of water and make sure to level levels
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
RCOR

33. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
allow for the vapor pressure of water and make sure to level levels
|experimental - accepted|/accepted X 100
a-IMFs - b-molecular volume

34. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
RCOR
?G= -ve - E°= +ve

35. What is HCOOCH3?
Acids; HCOOCH3 is an ester
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
The benzene ring (or more correctly the phenyl group - C6H5)
Distillation

36. If a free element is involved - what type of reaction must be involved?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
redox reaction
S2O3²?
Q=It (time in seconds)

37. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
?H formation of an element in standard state=0

38. Alcohols and _______ are FG isomers
ethers
Glacial acetic acid
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.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

39. Acid plus base make?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Hg2²?
Salt + water.
look for changes in oxidation # - the one that goes up is oxidized and is the RA

40. perchlorate
lighted splint (positive result=pop)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
K2
ClO4?

41. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
proton donor base
voltaic: + electrolytic: -
Pale purple - (orange)-yellow - red - blue - green.

42. Which of the rates changes more when temperature is increased?
CrO4²?
Salt + water
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
basic

43. Nonmetals are good _____ agents. Metals are good _______ agents.
acid + alcohol
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Acidified
Ksp = 108s5

44. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)
Mono; di; tri; tetra; penta; hexa.
CO (poisonous)

45. chromate
CrO4²?
Group 1 hydroxides (ex: NaOH)
Sigma bonds are stronger than pi bonds
Filtration

46. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Salt + water.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
How close results are to the accepted value
yellow

47. Generally - which oxy acid is strongest?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Tetrahedral
The one with most oxygen atoms (highest oxidation number)
Heptane

48. How are primary alcohols turned into acids?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
S2O3²?
R=8.31 J/mol/K

49. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
zero
linear
Suniverse increases for spontaneous processes

50. What does saturated mean? Unsaturated?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CnH2n
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Selective absorption