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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. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Distillation
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
basic
Check for air bubbles in the buret and remove the buret funnel from the buret

2. What is the third law of thermodynamics?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
S crystal at 0K=0
Acid rain - dissolves marble buildings/statues and kills trees.
Perform ICE BOX calculation based on K1

3. Acid plus base make?
Synthesis - separation and purification of the product and its identification.
benzene is less reactive than alkenes
Salt + water.
Ppt will NOT form (unsaturated)

4. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
NO3?
How close results are to the accepted value
strong acids/bases are written as H+ or OH- ions

5. What shape is water?
RCOOR
bent
blue glass - it filters UV
Salt + water

6. Color is due to ______ _______ of light.
Iodine and CO2 (dry ice)
H2O + CO2 (it decomposes readily)
Selective absorption
Cr2O7²?

7. During a titration what is present in the beaker at the equivalence point?
Mn²? - Cr³? - Cr³
A salt solution.
blue
More chaotic (ex: gases made)

8. What is the 'virtual' Ka for the complete dissociation of a dibasic acid?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
allow for the vapor pressure of water and make sure to level levels
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
K1 x K2

9. chromate ion (soln + most solids)
Salt + water.
No - it depends on the number of ions produced on dissolving.
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
yellow

10. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
atoms
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

11. Name some properties of Group 17
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Ions go through the salt bridge - electrons go through metal wires in the external circuit
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Pale yellow

12. What shape is carbon dioxide?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
blue
Pour liquids using a funnel or down a glass rod
linear

13. How many ligands attach to a central ion in a complex ion?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
#ligands=charge x2
an oxidized and reduced substance
P2O5

14. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
The one with most oxygen atoms (highest oxidation number)
Kc=Kp
SO4²?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

15. How are more active metals reduced?
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Salt + water
by electrolysis
neutralization: high K - H2O product dissociation: low K - H2O reactant

16. What is the formula for obtaining charge flowing in a cell?
RCOOH
Check for air bubbles in the buret and remove the buret funnel from the buret
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Q=It (time in seconds)

17. What type of compounds are almost always colored?
Transition element compounds (except if it has a full or empty d shell)
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?)
Pale purple - (orange)-yellow - red - blue - green.
acid + alcohol

18. What do you use to look at burning magnesium? why?
|experimental - accepted|/accepted X 100
CrO4²?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
blue glass - it filters UV

19. What is the difference between equivalence point and end point of a titration.
Separating funnel
linear
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
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

20. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
zero
Selective absorption
CO (poisonous)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

21. What is the formula for summation?

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22. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
RCOR
Pale purple - (orange)-yellow - red - blue - green.
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

23. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Nothing
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
voltaic: + electrolytic: -
+4-covalent - +2-ionic

24. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
red - green - blue
basic
P2O5

25. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Increases down group 1 decreases down group 17
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)
Nothing

26. Do anions flow to the cathode or anode?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
by electrolysis
Anode
Exothermic

27. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Greenish-yellow gas
a-IMFs - b-molecular volume
Soluble
C2O4²?

28. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Insoluble except for nitrate and acetate
different forms of the same element
Sigma bonds are stronger than pi bonds

29. What is the formula for alkynes?
Ksp = 4s³
Anode
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
CnH2n-2

30. Ions are not ______.
blue
atoms
Cu3(PO4)2
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

31. What things should you remember to do when collecting gas over water?
H2PO4?
acid + alcohol
allow for the vapor pressure of water and make sure to level levels
catalyst=conc H2SO4

32. 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.
E=q + w (negative is by system - positive is on system)
'non-active' metals such as Cu - Ag - Au - Pt - etc.

33. What effect does increasing the size/surface area of a voltaic cell have on the cell?
RCOOH
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
by electrolysis
do not change

34. What is the conjugate base of NH3?
NH2?
acid + alcohol
Salt + water
Conjugate pair (one must be a weak base or acid)

35. Give an example of a concentrated weak acid.
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CnH2n+1 often designated 'R' ex C3H7 is propyl
Glacial acetic acid
RNH2

36. Why are i factors (Van't Hoff factors) often less than ideal?
Insoluble except nitrate and acetate
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)
CrO4²?
ion pairing

37. What is reflux?
catalyst=conc H2SO4
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
boiling without losing volatile solvents/reactants
zero

38. What is the energy you must put into a reaction to make it start called?
Salt and water
Kc=Kp
Initiation energy (NOT Ea)
K2

39. How do you heat a test tube?
CrO4²?
ion pairing
Heat a test tube at an angle at the side of the tube (not bottom)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

40. What electrons are lost/gained first in transition element ions?
voltaic: + electrolytic: -
H3PO4
ns² electrons (first in-first out)
An active metal.

41. What is the test for hydrogen?
But S° of element is not zero (except at 0K)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
lighted splint (positive result=pop)

42. hypochlorite
Big K=kf/kr
Insoluble except group 1 and ammonium
C2O4²?
ClO?

43. What is the general formula of an alkane?
CnH(2n+2)
Insoluble except nitrate and acetate
T increases exponentially the proportion of molecules with E > Ea
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

44. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
Eudiometer
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
+4-covalent - +2-ionic

45. chlorate
ClO3?
But S° of element is not zero (except at 0K)
ethers
ionic and form hydrogen and hydroxide

46. What two types of substances are present in all redox reactions?
an oxidized and reduced substance
RCOR
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Salts (ex: CaO + SO2 ? CaSO3)

47. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Ksp = 4s³
SO4²?
Group 1 hydroxides (ex: NaOH)

48. iodine - iodine solution - iodine vapor
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
Silvery gray solid - brown - purple
White precipitate
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

49. What type of compounds do Group 14 form?
+4-covalent - +2-ionic
metal oxides and hydrides are ionically bonded and basic
Group 1 hydroxides (ex: NaOH)
same KE - but PEice<PEwater

50. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
it is lower and occurs over less sharp a range
Acid rain - dissolves marble buildings/statues and kills trees.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
No - it depends on the number of ions produced on dissolving.