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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 effect does increasing the size/surface area of a voltaic cell have on the cell?
Pour liquids using a funnel or down a glass rod
Ions go through the salt bridge - electrons go through metal wires in the external circuit
C2O4²?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

2. How can metals like iron and zinc be reduced?
Group 1 hydroxides (ex: NaOH)
chemically (ex: with carbon)
Ksp = 27s4
They decrease (or could be the same if the solid has ONLY JUST disappeared)

3. How do you identify which is oxidized or otherwise?
Graduated cylinder
non-metal oxides and hydrides are covalently bonded and are acidic.
Purple
look for changes in oxidation # - the one that goes up is oxidized and is the RA

4. What shape is ammonia?
Trigonal pyramidal
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
no - they're written undissociated (HAaq)

5. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Group 1 hydroxides (ex: NaOH)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
H+

6. What do group I/II metal oxides plus water form?
Disulfur dichloride
Orange
bases
Cu3(PO4)2

7. Alkanes are _________ and react by _________
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)
zero
Saturated - Substitution (which requires more radical conditions)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

8. Name C7H16
allow for the vapor pressure of water and make sure to level levels
No - it depends on the number of ions produced on dissolving.
Heptane
Iodine and CO2 (dry ice)

9. How do you get Ecell for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Add acid to water so that the acid doesn't boil and spit
C2O4²?
Separating funnel

10. What is the word equation for condensation polymerisation ?
Soluble
Nothing
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Soluble

11. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
The dilution effect when the solutions mix. M1V1 = M2V2
ion pairing
Nothing

12. What is an Alkyl group?

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13. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
CO3²?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
do not change

14. How do you compute % dissociation?
CnH2n+1 often designated 'R' ex C3H7 is propyl
[A?]/[HA] x 100 or [BH?]/[B] x 100
brown volatile liquid
same KE - but PEice<PEwater

15. During a titration what is present in the beaker at the equivalence point?
A salt solution.
Ksp = 4s³
Salt + water.
CnH2n-2

16. What do metal oxides plus acids form?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
it reacts by substitution NOT addition
Salt + water
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

17. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
acids
Ksp = 4s³
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

18. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Insoluble except for nitrate and acetate
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
different forms of the same element

19. When a cell is 'flat' What is its voltage?
Exothermic
Insoluble
zero
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

20. Nonmetals are good _____ agents. Metals are good _______ agents.
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
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Eudiometer
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

21. Neutralization is an ________ reaction.
E=q + w (negative is by system - positive is on system)
acid + alcohol
Most INsoluble except group 1 and ammonium
Exothermic (?H for ANY sa/sb = -57kJ/mol)

22. BaSO4
Cr2O7²?
Insoluble
do not change
Tetrahedral

23. What is the general formula for an aldehyde?
NO3?
Synthesis - separation and purification of the product and its identification.
neutralization: high K - H2O product dissociation: low K - H2O reactant
RCHO (carbonyl at end)

24. primary colors
red - green - blue
Monomer + monomer = polymer product + a simple molecule such as water or HCl
zero
Exothermic (?H for ANY sa/sb = -57kJ/mol)

25. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
C2O4²?
Ksp = s²
The dilution effect when the solutions mix. M1V1 = M2V2
The Faraday or Faraday's constant.

26. acetate
Silvery gray solid - brown - purple
CH3COO?
ethers
Conjugate pair (one must be a weak base or acid)

27. 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)
by electrolysis
Insoluble
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.

28. Both Acetic acid and ____________ are also functional isomers.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
?G= -ve - E°= +ve
zero-th: decreases - first: constant - second: increases
methyl formate

29. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
+4-covalent - +2-ionic
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

30. A Bronsted-Lowry acid is...
Anode
Nothing
fruit - fish - bases
proton donor base

31. What is the formula of copper (II) phosphate?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Cu3(PO4)2
hydroxides (ex: Ba(OH)2)
Cr2O7²?

32. When is ?G zero?
Molecules with the same molecular formulas - but different structural formulas
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
it reacts by substitution NOT addition
ion pairing

33. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
Concentration
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
bright yellow

34. Does Kw increase or decrease with T? Why?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Selective absorption
Distillation
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

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

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36. mercury (I) ion
voltaic: - electrolytic: +
Hg2²?
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?)
methyl formate

37. cyanide
Anode - oxygen. Cathode - hydrogen
CN?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Unsaturated - addition (ex: decolorize bromine solution)

38. What are the common strong bases?
Both electrons come from the same atom (just as good as a regular bond)
Ksp = 108s5
Group 1 hydroxides (ex: NaOH)
CnH2n-2

39. acetates
Insoluble except for nitrate and acetate
Soluble
ROH
HClO4

40. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
ClO?
non-metal oxides and hydrides are covalently bonded and are acidic.
fruit - fish - bases

41. mercury (II) ion
Hg²?
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.
Identity and purity (impure compounds usually have broad & low melting points)
T increases exponentially the proportion of molecules with E > Ea

42. bromine
CnH2n+1 often designated 'R' ex C3H7 is propyl
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
brown volatile liquid
T increases exponentially the proportion of molecules with E > Ea

43. What two types of substances are present in all redox reactions?
NH2?
|experimental - accepted|/accepted X 100
an oxidized and reduced substance
do not change

44. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
fractional distillation
zero
same KE - but PEice<PEwater

45. What is a coordinate covalent bond?
Perform ICE BOX calculation based on K1
Both electrons come from the same atom (just as good as a regular bond)
blue (BTB)
allow for the vapor pressure of water and make sure to level levels

46. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
zero

47. dichromate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Cr2O7²?
Clear
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

48. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
fruit - fish - bases
it reacts by substitution NOT addition
Anode
water and substances with (s) less dense than

49. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
K1 x K2
red - green - blue
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?)
zero-th: decreases - first: constant - second: increases

50. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
basic
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
CnH2n+1 often designated 'R' ex C3H7 is propyl