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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 name of S2Cl2? (Know how to name others like this - too)
Ppt will NOT form (unsaturated)
yellow
Disulfur dichloride
boiling without losing volatile solvents/reactants

2. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Products - reactants (except for BDE when it's reactants - products)
Anode - oxygen. Cathode - hydrogen
It ceases - the circuit is broken.
Hg2²?

3. If a weak acid is diluted more - what happens to its % dissociation value?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Increases.
PO4³?
Insoluble

4. What are isomers?
ionic and form hydrogen and hydroxide
Molecules with the same molecular formulas - but different structural formulas
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
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

5. What is H2CO3 (carbonate acid) usually written as?
Pipette (burette if need repetition)
H2O + CO2 (it decomposes readily)
Graduated cylinder
red - green - blue

6. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
Acids; HCOOCH3 is an ester
CO3²?
fractional distillation

7. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
How grouped results are
Salt and water
H2O + CO2 (it decomposes readily)

8. Which of the rates changes more when temperature is increased?
SO4²?
CnH2n-2
diamond and graphite
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

9. What do metal oxides plus non- metal oxides form?
Salts (ex: CaO + SO2 ? CaSO3)
blue
Pale yellow
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

10. The oxidation # for acid base reactions...
Filtration
do not change
Pipette (burette if need repetition)
Suniverse increases for spontaneous processes

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

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12. What steps do organic labs consist of?
methyl formate
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Synthesis - separation and purification of the product and its identification.
non-metal oxides and hydrides are covalently bonded and are acidic.

13. Give an example of a dilute strong acid.
an oxidized and reduced substance
Soluble
HClO4
ionic and form hydrogen and hydroxide

14. Ions are not ______.
a-IMFs - b-molecular volume
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
atoms
ionic and form hydrogen and hydroxide

15. When the salt bridge is removed what happens to the cell reaction?
voltaic: + electrolytic: -
linear
It ceases - the circuit is broken.
Making sigma bonds and holding lone pairs

16. What are the common strong bases?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Group 1 hydroxides (ex: NaOH)
it is lower and occurs over less sharp a range
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

17. Name some properties of Group 17
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Glowing splint (positive result=relights)
proton donor base

18. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
The Faraday or Faraday's constant.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
neutralization: high K - H2O product dissociation: low K - H2O reactant
Experimental mass/theoretical mass X 100

19. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
RX
Kc=Kp
Molecules with the same molecular formulas - but different structural formulas
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

20. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
q=mc?T q=mL (or n x ?h)
Soluble
-Ea/R

21. What does saturated mean? Unsaturated?
Orange
They stay the same.
RCHO (carbonyl at end)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

22. What do acids plus active metals form?
ion pairing
RCOR
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
do not change

23. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Graduated cylinder
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.
ClO4?

24. What is the formula for alkynes?
zero
T increases exponentially the proportion of molecules with E > Ea
Graduated cylinder
CnH2n-2

25. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Glacial acetic acid
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
K1 x K2
Pale purple - (orange)-yellow - red - blue - green.

26. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
atoms
benzene has a delocalized pi ring structure
Nothing

27. What is an Alkyl group?

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28. What do the 'a' and 'b' in Van Der Waal's equation allow for?
allow for the vapor pressure of water and make sure to level levels
a-IMFs - b-molecular volume
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Cu3(PO4)2

29. What is HCOOCH3?
Cr2O7²?
Current - time and charge on ion (moles of e used in half cell reaction)
Cu3(PO4)2
Acids; HCOOCH3 is an ester

30. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
NH2?
Transition element compounds (except if it has a full or empty d shell)
'non-active' metals such as Cu - Ag - Au - Pt - etc.

31. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
by electrolysis
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
R=8.31 J/mol/K

32. What is the conjugate acid of H2PO4?
O2 needs 4F/mol H2 needs 2F/mol
H3PO4
ion pairing
do not change

33. lead iodide
How close results are to the accepted value
Unsaturated - addition (ex: decolorize bromine solution)
ns² electrons (first in-first out)
bright yellow

34. For a dibasic acid (H2A) - [A²?]= ____ ?
Tetrahedral
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
How close results are to the accepted value
K2

35. Ca - Sr - Ba
boiling without losing volatile solvents/reactants
hydroxides (ex: Ba(OH)2)
ClO3?
it reacts by substitution NOT addition

36. Acid plus base make?
Salt + water.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
linear
zero

37. chlorine
Greenish-yellow gas
The dilution effect when the solutions mix. M1V1 = M2V2
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

38. What do hydrocarbons form when they burn in air (oxygen)?
C2O4²?
Cu3(PO4)2
CO2 and H2O
bent

39. What process do you use to obtain the solute from a solution?
Soluble
Cu3(PO4)2
Heat a test tube at an angle at the side of the tube (not bottom)
Evaporation

40. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Hg2²?
CO (poisonous)
Q=It (time in seconds)

41. Which would cause the bulb in a conductivity apparatus to be brightest?
Soluble except Ag - Pb - Ca - Sr Ba)
Pale purple - (orange)-yellow - red - blue - green.
0.10M HCl (more ions)
Orange

42. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
fractional distillation
ionic and form hydrogen and hydroxide
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

43. What part of a liquid do you look at to measure its volume?
it's lower and occurs over less sharp a range
Mono; di; tri; tetra; penta; hexa.
?H formation of an element in standard state=0
Read the bottom of the meniscus

44. Name 2 ways in which you can create a buffer?
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)
Add acid to water so that the acid doesn't boil and spit
voltaic: - electrolytic: +
Only temperature

45. Is a graduated cylinder or beaker more accurate?
Graduated cylinder
H2O + CO2 (it decomposes readily)
Salts (ex: CaO + SO2 ? CaSO3)
Filtration

46. When a cell is 'flat' What is its voltage?
Insoluble except for nitrate and acetate
Tetrahedral
The dilution effect when the solutions mix. M1V1 = M2V2
zero

47. bromine
Salt and water
Hg2²?
RNH2
brown volatile liquid

48. What is the word equation for condensation polymerisation ?
different forms of the same element
Monomer + monomer = polymer product + a simple molecule such as water or HCl
benzene has a delocalized pi ring structure
Synthetic condensation polymer (aka a polyamide)

49. hypochlorite
How grouped results are
ClO?
Experimental mass/theoretical mass X 100
strong acids/bases are written as H+ or OH- ions

50. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Ppt will NOT form (unsaturated)
No - it depends on the number of ions produced on dissolving.
NH4?
do not change