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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 the formula of copper (II) phosphate?
Cu3(PO4)2
K1 x K2
zero-th: decreases - first: constant - second: increases
proton donor base

2. What is the test for hydrogen?
acid + alcohol
lighted splint (positive result=pop)
R=8.31 J/mol/K
look for changes in oxidation # - the one that goes up is oxidized and is the RA

3. What type of compounds do Group 14 form?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
chemically (ex: with carbon)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
+4-covalent - +2-ionic

4. How are more active metals reduced?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Graduated cylinder
by electrolysis
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

5. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
More chaotic (ex: gases made)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Mono; di; tri; tetra; penta; hexa.

6. What is the general formula for an aldehyde?
Salt + water
RCHO (carbonyl at end)
blue
Monomer + monomer = polymer product + a simple molecule such as water or HCl

7. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
yellow
Graduated cylinder
acids

8. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Mn²? - Cr³? - Cr³
Hg2²?

9. Nonmetals are good _____ agents. Metals are good _______ agents.
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)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Sulfur
Both electrons come from the same atom (just as good as a regular bond)

10. acetates
Soluble
bright yellow
Heat a test tube at an angle at the side of the tube (not bottom)
ROH

11. When can supercooling occur? What does it look like on a cooling curve?

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12. Esters smell like _______ and amines smell like _______ and are ______.
Most are soluble except Ag - Pb
fruit - fish - bases
Salt + water
bent

13. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Graduated cylinder

14. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
H2O + CO2 (it decomposes readily)
[A?]/[HA] x 100 or [BH?]/[B] x 100
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

15. What equipment do you need for a titration?
RCOR
Filtration
Acidified
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

16. Is the standard entropy (S°) of an element zero?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
But S° of element is not zero (except at 0K)
fractional distillation
-Ea/R

17. What is the pH of 1.0M HCl? 1M NaOH?
More chaotic (ex: gases made)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
0 and 14
T increases exponentially the proportion of molecules with E > Ea

18. What device would you use to measure a volume of gas?
Insoluble except for nitrate and acetate
boiling without losing volatile solvents/reactants
Eudiometer
basic

19. oxalate
H3PO4
different forms of the same element
?H-kJ - ?S-J - ?G-kJ
C2O4²?

20. What electrons are lost/gained first in transition element ions?
R=8.31 J/mol/K
Both electrons come from the same atom (just as good as a regular bond)
Hg²?
ns² electrons (first in-first out)

21. phosphates
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Most INsoluble except group 1 and ammonium
Check for air bubbles in the buret and remove the buret funnel from the buret
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

22. What is accuracy?
basic
How close results are to the accepted value
Soluble
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

23. What is the charge on a chlorine atom?
zero
Glacial acetic acid
?G=negative - E° must be positive
different forms of the same element

24. What is the name of S2Cl2? (Know how to name others like this - too)
left - ppt will form
proton donor base
Anode - oxygen. Cathode - hydrogen
Disulfur dichloride

25. What are two substances that sublime at 1 atm when heated?
Anode
Disulfur dichloride
Separating funnel
Iodine and CO2 (dry ice)

26. How do you get the equation for a net electrolysis reaction?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Combine the equations for the half reactions in the non-spontaneous direction
benzene is less reactive than alkenes
Salts (ex: CaO + SO2 ? CaSO3)

27. What is the first law of thermodynamics?
Purple
E=q + w (negative is by system - positive is on system)
S2O3²?
Concentration

28. What is the conjugate base of NH3?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Nothing
Salt + water.
NH2?

29. What are the signs for ?G and E° for spontaneous reactions?
diamond and graphite
?G= -ve - E°= +ve
No - NH3 and HCl gases are extremely soluble
Salt and water

30. halides
Glowing splint (positive result=relights)
Most are soluble except Ag - Pb
K2
ClO4?

31. Give an example of a dilute strong acid.
Both electrons come from the same atom (just as good as a regular bond)
Kc=Kp
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
HClO4

32. hydroxide
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
no - they're written undissociated (HAaq)
redox reaction
OH?

33. phosphate
Sigma bonds are stronger than pi bonds
a-IMFs - b-molecular volume
Ksp = s²
PO4³?

34. What is the general formula of an alkane?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Insoluble (except group 1 ammonium and Ba)
CnH(2n+2)
Making sigma bonds and holding lone pairs

35. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
voltaic: + electrolytic: -
same KE - but PEice<PEwater
RNH2
Unsaturated - addition (ex: decolorize bromine solution)

36. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
RX
K1 x K2
Initiation energy (NOT Ea)
Pour liquids using a funnel or down a glass rod

37. potassium permanganate
Increases down group 1 decreases down group 17
Purple
strong acids/bases are written as H+ or OH- ions
ClO4?

38. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Iodine and CO2 (dry ice)
S crystal at 0K=0
Mono; di; tri; tetra; penta; hexa.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

39. What reacts with an acid to create hydrogen gas?
An active metal.
Soluble
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Pale purple - (orange)-yellow - red - blue - green.

40. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
S2O3²?
Kc=Kp
S crystal at 0K=0
CO (poisonous)

41. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
it's lower and occurs over less sharp a range
lighted splint (positive result=pop)
No - it depends on the number of ions produced on dissolving.
They stay the same.

42. If a weak acid is diluted more - what happens to its % dissociation value?
Increases.
Sigma bonds are stronger than pi bonds
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Combine the equations for the half reactions in the non-spontaneous direction

43. What is the general formula for an acid?
RCOOH
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
NH2?
Molecules with the same molecular formulas - but different structural formulas

44. What do group I/II metal oxides plus water form?
No - it depends on the number of ions produced on dissolving.
bases
do not change
PO4³?

45. Generally - which oxy acid is strongest?
CH3COO?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
The one with most oxygen atoms (highest oxidation number)
no - they're written undissociated (HAaq)

46. dichromate (soln + most solids)
Orange
Salt + water.
hydroxides (ex: Ba(OH)2)
Salt and water

47. Name C7H16
Filtration
No - it depends on the number of ions produced on dissolving.
MnO4?
Heptane

48. What is the slope of the graph of lnk vs. 1/T?
a-IMFs - b-molecular volume
-Ea/R
Trigonal pyramidal
fruit - fish - bases

49. thiosulfate
fruit - fish - bases
S2O3²?
?H-kJ - ?S-J - ?G-kJ
Add acid to water so that the acid doesn't boil and spit

50. What is the general formula for an alcohol?
Ksp = 108s5
More chaotic (ex: gases made)
ROH
allow for the vapor pressure of water and make sure to level levels