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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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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. chlorate
Insoluble (except group 1 ammonium and Ba)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
How grouped results are
ClO3?

2. Ca - Sr - Ba
Suniverse increases for spontaneous processes
hydroxides (ex: Ba(OH)2)
left - ppt will form
S crystal at 0K=0

3. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Synthetic condensation polymer (aka a polyamide)
Synthesis - separation and purification of the product and its identification.

4. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
Insoluble except nitrate and acetate
basic
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

5. What is the formula of butane?
Insoluble except for nitrate and acetate
Increases.
Products - reactants (except for BDE when it's reactants - products)
C4H10

6. What type of compounds do Group 14 form?
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)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
+4-covalent - +2-ionic
Increases.

7. What is H2CO3 (carbonate acid) usually written as?
H2O + CO2 (it decomposes readily)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
water and substances with (s) less dense than
Anode

8. How do you get the equation for a net electrolysis reaction?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Ksp = 27s4
Combine the equations for the half reactions in the non-spontaneous direction
ionic and form hydrogen and hydroxide

9. What do ions and electrons travel through in a voltaic/electrolytic cell?
a-IMFs - b-molecular volume
Anode - oxygen. Cathode - hydrogen
Group I metals (soft metals) are stored under oil
Ions go through the salt bridge - electrons go through metal wires in the external circuit

10. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
benzene has a delocalized pi ring structure
Ksp = 27s4
Separating funnel
The benzene ring (or more correctly the phenyl group - C6H5)

11. What type of compounds do metals/non metals form?
Ionic compounds
Monomer + monomer = polymer product + a simple molecule such as water or HCl
?G= -ve - E°= +ve
Unsaturated - addition (ex: decolorize bromine solution)

12. permanganate
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
MnO4?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
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

13. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
No - it depends on the number of ions produced on dissolving.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
CnH(2n+2)
Increases down group 1 decreases down group 17

14. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
CnH2n+2
Cr2O7²?
benzene is less reactive than alkenes
same KE - but PEice<PEwater

15. When driving off water from a hydrate - how do you tell you're done?
CnH(2n+2)
H3PO4
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Soluble

16. What is the general formula for an aldehyde?
Hg²?
RCHO (carbonyl at end)
NO3?
RCOOH

17. What is the formula for obtaining charge flowing in a cell?
The compound with the lowest Ksp value.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Q=It (time in seconds)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

18. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
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
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

19. Which would cause the bulb in a conductivity apparatus to be brightest?
by electrolysis
0.10M HCl (more ions)
Greenish-yellow gas
Products - reactants (except for BDE when it's reactants - products)

20. What do metal oxides plus acids form?
But S° of element is not zero (except at 0K)
Salt + water
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

21. ammonium
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
NH4?
CnH2n

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

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23. What apparatus do you use to separate 2 immiscible liquids?
Nothing
Graduated cylinder
Separating funnel
?G= -ve - E°= +ve

24. What is the general formula for an alcohol?
do not change
Kc=Kp
ROH
Mono; di; tri; tetra; penta; hexa.

25. nitrate
NO3?
Filtration
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Acid rain - dissolves marble buildings/statues and kills trees.

26. What are two substances that sublime at 1 atm when heated?
Soluble
Disulfur dichloride
Iodine and CO2 (dry ice)
More chaotic (ex: gases made)

27. During a titration what is present in the beaker at the equivalence point?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
A salt solution.
Pale yellow
Ions go through the salt bridge - electrons go through metal wires in the external circuit

28. What is the test for oxygen?
Most are soluble except Ag - Pb
PO4³?
Pipette (burette if need repetition)
Glowing splint (positive result=relights)

29. Which of the rates changes more when temperature is increased?
0 and 14
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
it is lower and occurs over less sharp a range

30. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
ionic and form hydrogen and hydroxide
10?8
C2O4²?
Read the bottom of the meniscus

31. Name 2 ways in which you can create a buffer?
At half equivalence - pH=pKa
Soluble
do not change
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)

32. A geometric (or cis-trans) isomer exists due to.....
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
The one with most oxygen atoms (highest oxidation number)
Insoluble except for nitrate and acetate
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

33. What are the units of the first order rate constant?
acid + alcohol
No - it depends on the number of ions produced on dissolving.
Time?¹ - (ex. s?¹ - hr?¹ - etc)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

34. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
it reacts by substitution NOT addition
Most are soluble except Ag - Pb
allow for the vapor pressure of water and make sure to level levels

35. silver compounds
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Insoluble except for nitrate and acetate
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Ksp = 4s³

36. dichromate (soln + most solids)
Acid rain - dissolves marble buildings/statues and kills trees.
yellow
Orange
ns² electrons (first in-first out)

37. What type of solutions do small - highly charged cations tend to form?
water and substances with (s) less dense than
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
A salt solution.

38. What is the sign of the cathode in voltaic cells? in electrolytic cells?
[A?]/[HA] x 100 or [BH?]/[B] x 100
The benzene ring (or more correctly the phenyl group - C6H5)
do not change
voltaic: + electrolytic: -

39. What is precision?
All except for lithium
How grouped results are
S2O3²?
look for changes in oxidation # - the one that goes up is oxidized and is the RA

40. What element is used to vulcanize rubber?
?G=negative - E° must be positive
Sulfur
A) any range. b) 8-10 c) 4-6
metal oxides and hydrides are ionically bonded and basic

41. What is the third law of thermodynamics?
Separating funnel
S crystal at 0K=0
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
lighted splint (positive result=pop)

42. If a weak acid is diluted more - what happens to its % dissociation value?
Read the bottom of the meniscus
Increases.
Distillation
water and substances with (s) less dense than

43. What type of compounds are almost always colored?
NH4?
Transition element compounds (except if it has a full or empty d shell)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)

44. What is the name of S2Cl2? (Know how to name others like this - too)
Glowing splint (positive result=relights)
zero
R=8.31 J/mol/K
Disulfur dichloride

45. What is accuracy?
Hg2²?
How close results are to the accepted value
RX
red - green - blue

46. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
allow for the vapor pressure of water and make sure to level levels
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Anode - oxygen. Cathode - hydrogen
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

47. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
H+
ionic and form hydrogen and hydroxide
CH3COO?
acid + alcohol

48. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Insoluble except nitrate and acetate
Reduction always takes place at the cathode (RED CAT) In both types of cell!
zero-th: decreases - first: constant - second: increases

49. group 1 ions/compounds
fractional distillation
T increases exponentially the proportion of molecules with E > Ea
Soluble
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

50. How are non-metal oxides and hydrides bonded? are they acidic or basic?
voltaic: - electrolytic: +
The benzene ring (or more correctly the phenyl group - C6H5)
zero
non-metal oxides and hydrides are covalently bonded and are acidic.