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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. ammonium
zero-th: decreases - first: constant - second: increases
Both electrons come from the same atom (just as good as a regular bond)
S2O3²?
NH4?

2. During a titration what is present in the beaker at the equivalence point?
A salt solution.
Molecules with the same molecular formulas - but different structural formulas
Ksp = 108s5
yellow

3. hydroxides
brown volatile liquid
Conjugate pair (one must be a weak base or acid)
Insoluble (except group 1 ammonium and Ba)
allow for the vapor pressure of water and make sure to level levels

4. What is reflux?
boiling without losing volatile solvents/reactants
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
redox reaction
Ksp = 108s5

5. What is the formula for obtaining charge flowing in a cell?
RNH2
Both electrons come from the same atom (just as good as a regular bond)
Q=It (time in seconds)
CH3COO?

6. What is the general formula for a ketone?
zero-th: decreases - first: constant - second: increases
Sigma bonds are stronger than pi bonds
RCOR
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

7. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
voltaic: - electrolytic: +
basic
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Kc=Kp

8. A Bronsted-Lowry base is...
proton acceptor.
PO4³?
Ksp = 4s³
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

9. What process do you use to obtain the precipitate from a solution?
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.
Acids; HCOOCH3 is an ester
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Filtration

10. How do you heat a test tube?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Heat a test tube at an angle at the side of the tube (not bottom)
Graduated cylinder

11. How do you get Ecell for spontaneous reactions?
acid + alcohol
Transition element compounds (except if it has a full or empty d shell)
H2O + CO2 (it decomposes readily)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)

12. How does the melting point of a mixture compare to the MP of a pure substance?

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13. What is the formula for alkynes?
The dilution effect when the solutions mix. M1V1 = M2V2
O2 needs 4F/mol H2 needs 2F/mol
red - green - blue
CnH2n-2

14. What is the charge on a chlorine atom?
zero
10?8
Purple
Ions go through the salt bridge - electrons go through metal wires in the external circuit

15. phosphate
do not change
PO4³?
chemically (ex: with carbon)
by electrolysis

16. Why are noble gases stable?
ROH
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ns² electrons (first in-first out)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

17. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
neutralization: high K - H2O product dissociation: low K - H2O reactant
Disulfur dichloride
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.

18. What are two substances that sublime at 1 atm when heated?
Glacial acetic acid
Iodine and CO2 (dry ice)
H2PO4?
allow for the vapor pressure of water and make sure to level levels

19. cyanide
q=mc?T q=mL (or n x ?h)
H3PO4
CN?
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

20. primary colors
red - green - blue
Silvery gray solid - brown - purple
an oxidized and reduced substance
do not change

21. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
0 and 14
They decrease (or could be the same if the solid has ONLY JUST disappeared)
ClO4?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

22. What is the conjugate acid of H2PO4?
allow for the vapor pressure of water and make sure to level levels
q=mc?T q=mL (or n x ?h)
H3PO4
Unsaturated - addition (ex: decolorize bromine solution)

23. Neutralization is an ________ reaction.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Big K=kf/kr
RCOOR

24. Generally - which oxy acid is strongest?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
The one with most oxygen atoms (highest oxidation number)
blue (BTB)

25. What are the signs for ?G and E° for spontaneous reactions?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
bent
White precipitate
?G= -ve - E°= +ve

26. Acid plus base make?
Initiation energy (NOT Ea)
Salt + water.
RCOOH
Big K=kf/kr

27. What shape is ammonia?
non-metal oxides and hydrides are covalently bonded and are acidic.
Trigonal pyramidal
Silvery gray solid - brown - purple
CO3²?

28. What kind of bonding structure does benzene have?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
diamond and graphite
yellow
benzene has a delocalized pi ring structure

29. What type of compounds do Group 14 form?
Heptane
Increases.
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
+4-covalent - +2-ionic

30. The oxidation # for acid base reactions...
do not change
redox reaction
Synthesis - separation and purification of the product and its identification.
diamond and graphite

31. What do metal oxides plus acids form?
Salt + water
strong acids/bases are written as H+ or OH- ions
How grouped results are
At half equivalence - pH=pKa

32. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Sigma bonds are stronger than pi bonds
Read the bottom of the meniscus
HClO4

33. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
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.
Suniverse increases for spontaneous processes
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

34. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
Unsaturated - addition (ex: decolorize bromine solution)
Filtration
Orange

35. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
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?)
Anode - oxygen. Cathode - hydrogen
Insoluble except group 1 and ammonium
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

36. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Silvery gray solid - brown - purple
voltaic: + electrolytic: -
bent
linear

37. What are hybrid orbitals used for?
Making sigma bonds and holding lone pairs
10?8
bright yellow
Check for air bubbles in the buret and remove the buret funnel from the buret

38. What is the formula of butane?
RCOR
do not change
C4H10
OH?

39. What does saturated mean? Unsaturated?
water and substances with (s) less dense than
Soluble
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

40. Name six characteristics of transition elements (or their compounds)
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)
Anode
left - ppt will form
?G=negative - E° must be positive

41. What process do you use to obtain a solvent from a solution?
ns² electrons (first in-first out)
Anode - oxygen. Cathode - hydrogen
Clear
Distillation

42. What is the third law of thermodynamics?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
A) any range. b) 8-10 c) 4-6
Monomer + monomer = polymer product + a simple molecule such as water or HCl
S crystal at 0K=0

43. What is the formula for percent yield?
Identity and purity (impure compounds usually have broad & low melting points)
Products - reactants (except for BDE when it's reactants - products)
Exothermic
Experimental mass/theoretical mass X 100

44. silver iodide
bright yellow
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
basic
Pale yellow

45. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
CO3²?
Pale purple - (orange)-yellow - red - blue - green.
Tetrahedral

46. What are isotopes?
10?8
S2O3²?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
hydroxides (ex: Ba(OH)2)

47. What is HCOOCH3?
Acids; HCOOCH3 is an ester
NH2?
Identity and purity (impure compounds usually have broad & low melting points)
0 and 14

48. Alkanes are _________ and react by _________
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Saturated - Substitution (which requires more radical conditions)
CnH2n+1 often designated 'R' ex C3H7 is propyl
'non-active' metals such as Cu - Ag - Au - Pt - etc.

49. Do anions flow to the cathode or anode?
Selective absorption
RCOOR
Anode
An active metal.

50. What do acids plus active metals form?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
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.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Filtration