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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. cyanide
CnH2n+1 often designated 'R' ex C3H7 is propyl
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
CN?
PO4³?

2. mercury (I) ion
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ppt will NOT form (unsaturated)
Pale purple - (orange)-yellow - red - blue - green.
Hg2²?

3. What is the general formula for a ketone?
RCOR
Concentration
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Evaporation

4. Esters smell like _______ and amines smell like _______ and are ______.
S2O3²?
fruit - fish - bases
blue (BTB)
CnH2n

5. chlorine
Greenish-yellow gas
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.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Both electrons come from the same atom (just as good as a regular bond)

6. What are amphoteric oxides?
S2O3²?
The benzene ring (or more correctly the phenyl group - C6H5)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
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?)

7. How are metal oxides and hydrides bonded? are they acidic or basic?
[A?]/[HA] x 100 or [BH?]/[B] x 100
metal oxides and hydrides are ionically bonded and basic
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

8. Aromatic compounds contain what?
Check for air bubbles in the buret and remove the buret funnel from the buret
Reduction always takes place at the cathode (RED CAT) In both types of cell!
same KE - but PEice<PEwater
The benzene ring (or more correctly the phenyl group - C6H5)

9. What is the pH of 1.0M HCl? 1M NaOH?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
brown volatile liquid
0 and 14
Trigonal pyramidal

10. copper sulfate
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
blue
It ceases - the circuit is broken.
Synthesis - separation and purification of the product and its identification.

11. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Suniverse increases for spontaneous processes
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
K1 x K2

12. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
RCHO (carbonyl at end)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

13. barium sulfate
White precipitate
ion pairing
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Insoluble

14. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Exothermic
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
same KE - but PEice<PEwater

15. Colorless doesn't mean ______
Clear
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
chemically (ex: with carbon)
H3PO4

16. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
?G=negative - E° must be positive
neutralization: high K - H2O product dissociation: low K - H2O reactant
RX
Pale purple - (orange)-yellow - red - blue - green.

17. How are more active metals reduced?
Most INsoluble except group 1 and ammonium
#ligands=charge x2
bases
by electrolysis

18. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Saturated - Substitution (which requires more radical conditions)
q=mc?T q=mL (or n x ?h)
Ksp = 4s³
Sulfur

19. What is the formula for alkanes?
metal oxides and hydrides are ionically bonded and basic
CnH2n+2
ClO4?
The one with most oxygen atoms (highest oxidation number)

20. What are hybrid orbitals used for?
Soluble
Making sigma bonds and holding lone pairs
Pale yellow
Tetrahedral

21. carbonate
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Silvery gray solid - brown - purple
it's lower and occurs over less sharp a range
CO3²?

22. What is the conjugate acid of H2PO4?
zero
a-IMFs - b-molecular volume
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
H3PO4

23. Does reactivity increase/decrease going down group 1 and group 17?
How close results are to the accepted value
ClO3?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Increases down group 1 decreases down group 17

24. When is ?G zero?
Cu3(PO4)2
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.
?H-kJ - ?S-J - ?G-kJ
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

25. What is reflux?
boiling without losing volatile solvents/reactants
it's lower and occurs over less sharp a range
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Synthesis - separation and purification of the product and its identification.

26. What is the formula for alkenes?
#ligands=charge x2
The compound with the lowest Ksp value.
CnH2n
But S° of element is not zero (except at 0K)

27. potassium permanganate
ion pairing
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Check for air bubbles in the buret and remove the buret funnel from the buret
Purple

28. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
Soluble
do not change
Ksp = 27s4

29. chromate
do not change
CrO4²?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Both electrons come from the same atom (just as good as a regular bond)

30. What is the general formula of an alkane?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
CnH(2n+2)
No - NH3 and HCl gases are extremely soluble
Nothing

31. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
NO3?
Eudiometer
non-metal oxides and hydrides are covalently bonded and are acidic.

32. Does Kw increase or decrease with T? Why?
Separating funnel
diamond and graphite
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

33. Alkanes are _________ and react by _________
MnO4?
Saturated - Substitution (which requires more radical conditions)
Acidified
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

34. What device would you use to measure a volume of gas?
red - green - blue
basic
Eudiometer
allow for the vapor pressure of water and make sure to level levels

35. The definition of acidic basic and neutral aqueous solutions is:
?G= -ve - E°= +ve
Cu3(PO4)2
Mono; di; tri; tetra; penta; hexa.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

36. A geometric (or cis-trans) isomer exists due to.....
Cu3(PO4)2
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Unsaturated - addition (ex: decolorize bromine solution)
Acidified

37. What are allotropes?
Acids; HCOOCH3 is an ester
10?8
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
different forms of the same element

38. What are the products of the reaction between group 1 metals and water?

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39. What is the charge on a chlorine atom?
zero
Conjugate pair (one must be a weak base or acid)
Acidified
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.

40. What is the formula for alkynes?
a-IMFs - b-molecular volume
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
CnH2n-2
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

41. What is the third law of thermodynamics?
Cr2O7²?
a-IMFs - b-molecular volume
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
S crystal at 0K=0

42. During a titration what is present in the beaker at the equivalence point?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CO (poisonous)
A salt solution.
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

43. What is the formula for percent yield?
ClO2?
SO4²?
Experimental mass/theoretical mass X 100
NO3?

44. What is the general formula for an alcohol?
do not change
are less dense than water
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)
ROH

45. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Insoluble (except group 1 ammonium and Ba)
All except for lithium
a-IMFs - b-molecular volume
Soluble

46. phosphate
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)
Insoluble except nitrate and acetate
Eudiometer
PO4³?

47. What do you need to make a polymer?
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)
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?)
redox reaction

48. What are two substances that sublime at 1 atm when heated?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Iodine and CO2 (dry ice)
neutralization: high K - H2O product dissociation: low K - H2O reactant
Increases.

49. Name some properties of Group 17
Ksp = 4s³
Soluble
Synthetic condensation polymer (aka a polyamide)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

50. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Orange
Pour liquids using a funnel or down a glass rod
10?8