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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. ammonium/ammonium compounds
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Soluble

2. Colorless doesn't mean ______
Clear
Ksp = 4s³
ClO?
CH3COO?

3. How are metal oxides and hydrides bonded? are they acidic or basic?
metal oxides and hydrides are ionically bonded and basic
Separating funnel
chemically (ex: with carbon)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

4. What does saturated mean? Unsaturated?
Pale yellow
CnH2n
do not change
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

5. A Bronsted-Lowry base is...
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
The compound with the lowest Ksp value.
White precipitate
proton acceptor.

6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
No - it depends on the number of ions produced on dissolving.
Ksp = 4s³
Unsaturated - addition (ex: decolorize bromine solution)
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)

7. How does half life change for zero-th order - first order - and second order processes?
ClO2?
OH?
zero-th: decreases - first: constant - second: increases
-Ea/R

8. What is the general formula for an alcohol?
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?)
Selective absorption
ROH
No - NH3 and HCl gases are extremely soluble

9. What type of compounds do metals/non metals form?
|experimental - accepted|/accepted X 100
Ionic compounds
CnH2n
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.

10. What is the hybridization for a given atom with four single bonds? one double and two single bonds? two double bonds? one triple and one single bond? two single bonds and two lone pairs? three single bonds and one lone pair?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Only temperature
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
Pale purple - (orange)-yellow - red - blue - green.

11. What is the third law of thermodynamics?
RCOR
look for changes in oxidation # - the one that goes up is oxidized and is the RA
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
S crystal at 0K=0

12. chromate ion (soln + most solids)
OH- and NH3
Pipette (burette if need repetition)
yellow
Pale purple - (orange)-yellow - red - blue - green.

13. chlorate
Glowing splint (positive result=relights)
ClO3?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Hg²?

14. Alcohols and _______ are FG isomers
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)
ethers
Insoluble except nitrate and acetate
it's lower and occurs over less sharp a range

15. Alkenes are ________ and react by __________
an oxidized and reduced substance
Unsaturated - addition (ex: decolorize bromine solution)
water and substances with (s) less dense than
It ceases - the circuit is broken.

16. oxalate
CN?
different forms of the same element
zero-th: decreases - first: constant - second: increases
C2O4²?

17. potassium permanganate
Ions go through the salt bridge - electrons go through metal wires in the external circuit
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Purple
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

18. How can metals like iron and zinc be reduced?
Acids; HCOOCH3 is an ester
left - ppt will form
It ceases - the circuit is broken.
chemically (ex: with carbon)

19. What equipment do you need for a titration?
linear
10?8
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
ionic and form hydrogen and hydroxide

20. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Iodine and CO2 (dry ice)
Insoluble except group 1 and ammonium
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Big K=kf/kr

21. How does the melting point of a mixture compare to the MP of a pure substance?
it is lower and occurs over less sharp a range
same KE - but PEice<PEwater
Graduated cylinder
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

22. primary colors
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
methyl formate
red - green - blue
zero

23. The definition of acidic basic and neutral aqueous solutions is:
RCOOR
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Unsaturated - addition (ex: decolorize bromine solution)
acids

24. What is the general formula for an acid?
RCOOH
Ksp = 27s4
Iodine and CO2 (dry ice)
A) any range. b) 8-10 c) 4-6

25. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Ksp = s²
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Combine the equations for the half reactions in the non-spontaneous direction
MnO4?

26. acetates
Clear
Products - reactants (except for BDE when it's reactants - products)
Anode
Soluble

27. carbonates
Combine the equations for the half reactions in the non-spontaneous direction
Acid rain - dissolves marble buildings/statues and kills trees.
Insoluble except group 1 and ammonium
different forms of the same element

28. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
redox reaction
it is lower and occurs over less sharp a range
How grouped results are
do not change

29. hydroxide
OH?
neutralization: high K - H2O product dissociation: low K - H2O reactant
The benzene ring (or more correctly the phenyl group - C6H5)
Salt + water

30. What changes Keq?
Only temperature
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
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
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

31. What is the test for hydrogen?
lighted splint (positive result=pop)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Identity and purity (impure compounds usually have broad & low melting points)

32. What is the general formula of an alkane?
blue
benzene is less reactive than alkenes
CnH(2n+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 -

33. What shape is methane?
CnH2n+1 often designated 'R' ex C3H7 is propyl
Experimental mass/theoretical mass X 100
Tetrahedral
Ksp = 27s4

34. What are two substances that sublime at 1 atm when heated?
E=q + w (negative is by system - positive is on system)
Iodine and CO2 (dry ice)
voltaic: + electrolytic: -
ClO?

35. What is a dipeptide? polypeptide? protein?
Tetrahedral
same KE - but PEice<PEwater
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
CO2 and H2O

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

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37. How do you clean a buret/pipette for a titration?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
RCOR
Salt + water.

38. What does a short - sharp melting point indicate?
Identity and purity (impure compounds usually have broad & low melting points)
RX
How grouped results are
Pale yellow

39. chlorine
a-IMFs - b-molecular volume
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Greenish-yellow gas
ROH

40. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
strong acids/bases are written as H+ or OH- ions
Experimental mass/theoretical mass X 100
Suniverse increases for spontaneous processes
zero

41. Where are group I metals stored?
a-IMFs - b-molecular volume
H2O + CO2 (it decomposes readily)
Acidified
Group I metals (soft metals) are stored under oil

42. Is the standard entropy (S°) of an element zero?
+4-covalent - +2-ionic
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
No - NH3 and HCl gases are extremely soluble
But S° of element is not zero (except at 0K)

43. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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44. What are two allotropes of carbon?
Products - reactants (except for BDE when it's reactants - products)
same KE - but PEice<PEwater
hydroxides (ex: Ba(OH)2)
diamond and graphite

45. bromothymol
Ksp = s²
[A?]/[HA] x 100 or [BH?]/[B] x 100
Separating funnel
blue (BTB)

46. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
same KE - but PEice<PEwater
0 and 14
R=8.31 J/mol/K
Salt + water.

47. What element is used to vulcanize rubber?
Evaporation
Sulfur
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
CO2 and H2O

48. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
Big K=kf/kr
Soluble
Heptane

49. silver iodide
ionic and form hydrogen and hydroxide
voltaic: - electrolytic: +
Pale yellow
An active metal.

50. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
blue (BTB)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
acids