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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. Name some properties of Group 17
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Disulfur dichloride

2. Is the ?H formation of an element in standard state zero?
zero
?H formation of an element in standard state=0
O2 needs 4F/mol H2 needs 2F/mol
Reduction always takes place at the cathode (RED CAT) In both types of cell!

3. What type of polymer is nylon?
Sigma bonds are stronger than pi bonds
Distillation
Synthetic condensation polymer (aka a polyamide)
zero

4. What is the formula for alkenes?
strong acids/bases are written as H+ or OH- ions
Soluble
Acids; HCOOCH3 is an ester
CnH2n

5. What is the word equation for condensation polymerisation ?
Ksp = 108s5
Monomer + monomer = polymer product + a simple molecule such as water or HCl
H2PO4?
Separating funnel

6. What element is used to vulcanize rubber?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Silvery gray solid - brown - purple
Sulfur
-Ea/R

7. 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
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
NH4?
But S° of element is not zero (except at 0K)

8. What is H2CO3 (carbonate acid) usually written as?
Kc=Kp
H2O + CO2 (it decomposes readily)
Mn²? - Cr³? - Cr³
It ceases - the circuit is broken.

9. What is the general formula for an amine?
lighted splint (positive result=pop)
diamond and graphite
RNH2
redox reaction

10. What is the general formula for an ether?
?H formation of an element in standard state=0
Check for air bubbles in the buret and remove the buret funnel from the buret
water and substances with (s) less dense than
ROR

11. lead compounds
ns² electrons (first in-first out)
Insoluble except nitrate and acetate
R=8.31 J/mol/K
Insoluble (except group 1 ammonium and Ba)

12. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Ksp = s²
Clear
methyl formate
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

13. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
Ksp = 108s5
Unsaturated - addition (ex: decolorize bromine solution)
K1 x K2
Pale yellow

14. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Time?¹ - (ex. s?¹ - hr?¹ - etc)
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.
Graduated cylinder

15. What are the prefixes for the naming of binary molecular compound formulas (up to six)
OH- and NH3
Mono; di; tri; tetra; penta; hexa.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
The compound with the lowest Ksp value.

16. chlorite
Group 1 hydroxides (ex: NaOH)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
ClO2?
?H formation of an element in standard state=0

17. Which value of R do you use for all energy and kinetics calculations?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
RCOR
by electrolysis
R=8.31 J/mol/K

18. Alkanes are _________ and react by _________
Ksp = 108s5
Group 1 hydroxides (ex: NaOH)
Saturated - Substitution (which requires more radical conditions)
it's lower and occurs over less sharp a range

19. What is the formula of copper (II) phosphate?
Cu3(PO4)2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Hg²?
?H formation of an element in standard state=0

20. What electrons are lost/gained first in transition element ions?
boiling without losing volatile solvents/reactants
They stay the same.
Pour liquids using a funnel or down a glass rod
ns² electrons (first in-first out)

21. What two types of substances are present in all redox reactions?
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
Ksp = 27s4
Hg2²?
an oxidized and reduced substance

22. What is a dipeptide? polypeptide? protein?
CO2 and H2O
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together

23. hypochlorite
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Hg²?
catalyst=conc H2SO4
ClO?

24. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Soluble
Sulfur
P2O5
Anode - oxygen. Cathode - hydrogen

25. What is the difference between equivalence point and end point of a titration.
P2O5
Separating funnel
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
different forms of the same element

26. ammonium/ammonium compounds
RCOR
The Faraday or Faraday's constant.
Hg2²?
Soluble

27. chlorate
benzene is less reactive than alkenes
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?)
ClO3?
Silvery gray solid - brown - purple

28. nitrate
NO3?
White precipitate
red - green - blue
?G= -ve - E°= +ve

29. What are isotopes?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
benzene is less reactive than alkenes
Mn²? - Cr³? - Cr³
ClO4?

30. How does the melting point of a mixture compare to the MP of a pure substance?

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31. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
?G=negative - E° must be positive
blue (BTB)
CO3²?

32. Is the freezing of ice endothermic or exothermic?
zero
Exothermic
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Suniverse increases for spontaneous processes

33. acetate
Experimental mass/theoretical mass X 100
yellow
voltaic: + electrolytic: -
CH3COO?

34. What is the slope of the graph of lnk vs. 1/T?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Most are soluble except Ag - Pb
-Ea/R
Soluble

35. What causes the dramatic effect of T on rate?
T increases exponentially the proportion of molecules with E > Ea
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Insoluble except for nitrate and acetate
Big K=kf/kr

36. What do group I/II metal oxides plus water form?
hydroxides (ex: Ba(OH)2)
bases
brown volatile liquid
HClO4

37. What device would you use to measure a volume of gas?
Clear
How close results are to the accepted value
Eudiometer
-Ea/R

38. permanganate
CrO4²?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Separating funnel
MnO4?

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

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40. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Disulfur dichloride
a-IMFs - b-molecular volume
CO (poisonous)
Selective absorption

41. Generally - which oxy acid is strongest?
Transition element compounds (except if it has a full or empty d shell)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
The one with most oxygen atoms (highest oxidation number)
ion pairing

42. What is Big K in terms of kf and kr?
left - ppt will form
Big K=kf/kr
Iodine and CO2 (dry ice)
|experimental - accepted|/accepted X 100

43. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
How grouped results are
it reacts by substitution NOT addition
Ions go through the salt bridge - electrons go through metal wires in the external circuit

44. What type of compounds are almost always colored?
C2O4²?
RCHO (carbonyl at end)
Transition element compounds (except if it has a full or empty d shell)
Saturated - Substitution (which requires more radical conditions)

45. What is the formula for alkanes?
Insoluble except nitrate and acetate
CnH2n+2
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Insoluble except group 1 and ammonium

46. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
allow for the vapor pressure of water and make sure to level levels
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Purple

47. hydroxides
Anode
ns² electrons (first in-first out)
blue
Insoluble (except group 1 ammonium and Ba)

48. What do metal oxides plus acids form?
R=8.31 J/mol/K
Salt + water
strong acids/bases are written as H+ or OH- ions
by electrolysis

49. What complex ion does ammonia form with silver? copper? cadmium? zinc?
hydroxides (ex: Ba(OH)2)
Insoluble except for nitrate and acetate
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

50. If ?S is positive - are the products more or less chaotic than the reactants?
More chaotic (ex: gases made)
T increases exponentially the proportion of molecules with E > Ea
Q=It (time in seconds)
NH2?