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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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1. Does Kw increase or decrease with T? Why?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
bases
Molecules with the same molecular formulas - but different structural formulas
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

2. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Ksp = 27s4
AgF-soluble in water - other silver halides insoluble in water - AgCl-soluble in excess ammonia - AgBr-somewhat soluble - AgI (yellow)-somewhat soluble in excess ammonia
Soluble
CnH2n-2

3. What is the general formula for an alcohol?
ROH
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)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

4. What is the test for oxygen?
Insoluble except nitrate and acetate
Glowing splint (positive result=relights)
CnH2n
The dilution effect when the solutions mix. M1V1 = M2V2

5. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
T increases exponentially the proportion of molecules with E > Ea
chemically (ex: with carbon)
Hg2²?

6. What do the 'a' and 'b' in Van Der Waal's equation allow for?
hydroxides (ex: Ba(OH)2)
ion pairing
a-IMFs - b-molecular volume
are less dense than water

7. What is the energy you must put into a reaction to make it start called?
Tetrahedral
Initiation energy (NOT Ea)
it's lower and occurs over less sharp a range
zero-th: decreases - first: constant - second: increases

8. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
?H formation of an element in standard state=0
voltaic: + electrolytic: -
Ksp = 108s5
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

9. Name six characteristics of transition elements (or their compounds)
RX
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
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)

10. What part of a liquid do you look at to measure its volume?
The compound with the lowest Ksp value.
Acid rain - dissolves marble buildings/statues and kills trees.
Read the bottom of the meniscus
CnH2n+1 often designated 'R' ex C3H7 is propyl

11. chlorite
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Hg²?
ClO2?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

12. What do nonmetal oxides plus water form?
Insoluble
CO2 and H2O
acids
CN?

13. What are the prefixes for the naming of binary molecular compound formulas (up to six)
But S° of element is not zero (except at 0K)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
ion pairing
Mono; di; tri; tetra; penta; hexa.

14. dichromate
At half equivalence - pH=pKa
red - green - blue
Acids; HCOOCH3 is an ester
Cr2O7²?

15. dichromate (soln + most solids)
Soluble
Orange
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
ion pairing

16. oxalate
CH3COO?
C2O4²?
Insoluble (except group 1 ammonium and Ba)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

17. What is the slope of the graph of lnk vs. 1/T?
Ksp = s²
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
-Ea/R
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

18. What process do you use to obtain the solute from a solution?
Evaporation
Combine the equations for the half reactions in the non-spontaneous direction
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Check for air bubbles in the buret and remove the buret funnel from the buret

19. acetates
acid + alcohol
Soluble
PO4³?
fruit - fish - bases

20. phosphates
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Most INsoluble except group 1 and ammonium
Saturated - Substitution (which requires more radical conditions)
Cu3(PO4)2

21. What is the general formula of an alkane?
Decant
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
CnH(2n+2)

22. What is the relationship in strength between sigma and pi bonds?
T increases exponentially the proportion of molecules with E > Ea
Sigma bonds are stronger than pi bonds
Soluble
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

23. What is the general formula for an ether?
bases
ROR
OH?
it reacts by substitution NOT addition

24. What is the first law of thermodynamics?
|experimental - accepted|/accepted X 100
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)
Pale purple - (orange)-yellow - red - blue - green.

25. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
Saturated - Substitution (which requires more radical conditions)
water and substances with (s) less dense than
Ksp = s²
A salt solution.

26. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Mn²? - Cr³? - Cr³
Transition element compounds (except if it has a full or empty d shell)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

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

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28. 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.
redox reaction
red - green - blue

29. Color is due to ______ _______ of light.
O2 needs 4F/mol H2 needs 2F/mol
RCOOH
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Selective absorption

30. An amphiprotic (amphoteric) species is...
Disulfur dichloride
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
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
All except for lithium

31. How does half life change for zero-th order - first order - and second order processes?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Transition element compounds (except if it has a full or empty d shell)
boiling without losing volatile solvents/reactants
zero-th: decreases - first: constant - second: increases

32. What is the conjugate acid of H2PO4?
CnH2n+2
Salts (ex: CaO + SO2 ? CaSO3)
?G=negative - E° must be positive
H3PO4

33. mercury (I) ion
Hg2²?
redox reaction
No - it depends on the number of ions produced on dissolving.
Saturated - Substitution (which requires more radical conditions)

34. What type of metals don't react with water or acids to form H2?

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35. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
-Ea/R
OH?
proton acceptor.

36. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
Anode
redox reaction
H2O + CO2 (it decomposes readily)
do not change

37. What is the sign of the anode in voltaic cells? in electrolytic cells?
CrO4²?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
voltaic: - electrolytic: +
CO3²?

38. dihydrogen phosphate
ethers
?G=negative - E° must be positive
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
H2PO4?

39. How does group 1 metals' density compare to water's?
R=8.31 J/mol/K
ClO2?
are less dense than water
catalyst=conc H2SO4

40. barium sulfate
Insoluble except group 1 and ammonium
zero
Mono; di; tri; tetra; penta; hexa.
White precipitate

41. Ca - Sr - Ba
hydroxides (ex: Ba(OH)2)
Molecules with the same molecular formulas - but different structural formulas
fruit - fish - bases
CnH2n-2

42. What is a dipeptide? polypeptide? protein?
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)
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
HClO4

43. chlorate
ClO3?
Combine the equations for the half reactions in the non-spontaneous direction
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)
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

44. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
acids
it's lower and occurs over less sharp a range
Insoluble except group 1 and ammonium

45. What device would you use to measure a volume of gas?
Eudiometer
Soluble
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Iodine and CO2 (dry ice)

46. What measuring device would you use for very small volumes of liquids?
brown volatile liquid
fruit - fish - bases
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Pipette (burette if need repetition)

47. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Nothing
fruit - fish - bases
Ksp = 108s5

48. carbonate
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
CO3²?
blue (BTB)
?G=negative - E° must be positive

49. If Q < Ksp a ppt ______
Ppt will NOT form (unsaturated)
bright yellow
More chaotic (ex: gases made)
Time?¹ - (ex. s?¹ - hr?¹ - etc)

50. How does the melting point of a mixture compare to the MP of a pure substance?
Hg²?
left - ppt will form
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
it is lower and occurs over less sharp a range