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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. nitrate
NO3?
Kc=Kp
Sulfur
But S° of element is not zero (except at 0K)

2. What steps do organic labs consist of?
Ksp = 108s5
S crystal at 0K=0
Synthesis - separation and purification of the product and its identification.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

3. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
blue glass - it filters UV
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
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
Nothing

4. halides
CH3COO?
Current - time and charge on ion (moles of e used in half cell reaction)
Greenish-yellow gas
Most are soluble except Ag - Pb

5. How are primary alcohols turned into acids?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
do not change

6. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Nothing
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
A salt solution.
left - ppt will form

7. Alkenes are ________ and react by __________
benzene is less reactive than alkenes
RCOOH
Unsaturated - addition (ex: decolorize bromine solution)
allow for the vapor pressure of water and make sure to level levels

8. What shape is ammonia?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Trigonal pyramidal
brown volatile liquid
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

9. What is precision?
Acid rain - dissolves marble buildings/statues and kills trees.
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.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
How grouped results are

10. bromothymol
proton donor base
CO2 and H2O
?H formation of an element in standard state=0
blue (BTB)

11. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
CnH2n
Heptane
allow for the vapor pressure of water and make sure to level levels

12. What is the test for hydrogen?
lighted splint (positive result=pop)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Insoluble
NO3?

13. How does group 1 metals' density compare to water's?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
do not change
ROH
are less dense than water

14. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Glacial acetic acid
it is lower and occurs over less sharp a range
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

15. What is the formula of butane?
zero
C4H10
Conjugate pair (one must be a weak base or acid)
OH?

16. What is the slope of the graph of lnk vs. 1/T?
ClO?
-Ea/R
zero-th: decreases - first: constant - second: increases
boiling without losing volatile solvents/reactants

17. What does saturated mean? Unsaturated?
CnH2n
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
|experimental - accepted|/accepted X 100
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

18. Are weak acids (and bases) written dissociated?

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19. If a beaker gets cold - is the reaction endothermic or exothermic? is ?H positive or negative?
K1 x K2
benzene has a delocalized pi ring structure
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Both electrons come from the same atom (just as good as a regular bond)

20. What things should you remember to do when collecting gas over water?
Cr2O7²?
allow for the vapor pressure of water and make sure to level levels
benzene is less reactive than alkenes
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

21. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
zero
But S° of element is not zero (except at 0K)

22. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
CnH2n+2
Eudiometer
Nothing

23. Give an example of a dilute strong acid.
Hg2²?
an oxidized and reduced substance
Tetrahedral
HClO4

24. sulfate
White precipitate
Salt + water.
same KE - but PEice<PEwater
SO4²?

25. What do the 'a' and 'b' in Van Der Waal's equation allow for?
C2O4²?
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 -
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

26. What is the formula for summation?

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27. Color is due to ______ _______ of light.
Selective absorption
Experimental mass/theoretical mass X 100
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

28. How are strong ones written?
lighted splint (positive result=pop)
Filtration
strong acids/bases are written as H+ or OH- ions
Sigma bonds are stronger than pi bonds

29. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
NO3?
Cr2O7²?
Big K=kf/kr

30. 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.
Hg2²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
A) any range. b) 8-10 c) 4-6
RCOR

31. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Synthetic condensation polymer (aka a polyamide)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
do not change
They stay the same.

32. lead compounds
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Nothing
Insoluble except nitrate and acetate

33. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
SO4²?
S2O3²?
Anode - oxygen. Cathode - hydrogen
Sulfur

34. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
blue (BTB)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

35. acetate
Both electrons come from the same atom (just as good as a regular bond)
0.10M HCl (more ions)
CH3COO?
+4-covalent - +2-ionic

36. What type of metals don't react with water or acids to form H2?

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37. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
?G=negative - E° must be positive
a-IMFs - b-molecular volume
water and substances with (s) less dense than

38. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
#ligands=charge x2
Both electrons come from the same atom (just as good as a regular bond)
Cr2O7²?

39. Name some properties of Group 17
E=q + w (negative is by system - positive is on system)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
?G= -ve - E°= +ve
left - ppt will form

40. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
No - NH3 and HCl gases are extremely soluble
strong acids/bases are written as H+ or OH- ions
Insoluble except group 1 and ammonium
Pale purple - (orange)-yellow - red - blue - green.

41. What changes Keq?
Separating funnel
The compound with the lowest Ksp value.
allow for the vapor pressure of water and make sure to level levels
Only temperature

42. What is the general formula for an acid?
fractional distillation
CO (poisonous)
RCOOH
look for changes in oxidation # - the one that goes up is oxidized and is the RA

43. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
a-IMFs - b-molecular volume
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
E=q + w (negative is by system - positive is on system)
ClO4?

44. Metal hydrides are _____ and form _______ and _______ when added to water
Evaporation
0.10M HCl (more ions)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ionic and form hydrogen and hydroxide

45. What word is a clue for a redox reaction?
Acidified
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Pale yellow
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

46. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
|experimental - accepted|/accepted X 100
Cr2O7²?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

47. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
ROR
brown volatile liquid
They decrease (or could be the same if the solid has ONLY JUST disappeared)
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

48. What is the general formula for an ester?
Disulfur dichloride
Sulfur
RCOOR
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

49. What is accuracy?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Ksp = 27s4
How close results are to the accepted value
Ksp = 4s³

50. Esters smell like _______ and amines smell like _______ and are ______.
Filtration
q=mc?T q=mL (or n x ?h)
Combine the equations for the half reactions in the non-spontaneous direction
fruit - fish - bases