Test your basic knowledge |

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. Neutralization is an ________ reaction.
a-IMFs - b-molecular volume
Exothermic (?H for ANY sa/sb = -57kJ/mol)
0.10M HCl (more ions)
fruit - fish - bases

2. hydroxide
Monomer + monomer = polymer product + a simple molecule such as water or HCl
S2O3²?
Silvery gray solid - brown - purple
OH?

3. What type of compounds are almost always colored?
diamond and graphite
Salt + water
blue glass - it filters UV
Transition element compounds (except if it has a full or empty d shell)

4. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
Filtration
?H-kJ - ?S-J - ?G-kJ
CnH2n-2

5. carbonate
CO3²?
Cr2O7²?
brown volatile liquid
left - ppt will form

6. What do metal oxides plus non- metal oxides form?
RCHO (carbonyl at end)
Initiation energy (NOT Ea)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Salts (ex: CaO + SO2 ? CaSO3)

7. Metal hydrides are _____ and form _______ and _______ when added to water
Iodine and CO2 (dry ice)
ionic and form hydrogen and hydroxide
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
A) any range. b) 8-10 c) 4-6

8. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
An active metal.
0 and 14
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

9. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
zero
bases
Iodine and CO2 (dry ice)

10. Ca - Sr - Ba
MnO4?
brown volatile liquid
hydroxides (ex: Ba(OH)2)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

11. What is H2CO3 (carbonate acid) usually written as?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
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)
H2O + CO2 (it decomposes readily)

12. What type of compounds do Group 14 form?
White precipitate
+4-covalent - +2-ionic
lighted splint (positive result=pop)
Soluble

13. Which value of R do you use for all energy and kinetics calculations?
redox reaction
Group I metals (soft metals) are stored under oil
R=8.31 J/mol/K
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

14. What is the conjugate acid of H2PO4?
Anode
H3PO4
Filtration
Kc=Kp

15. ________ are Lewis bases - because they can donate a lone pair of electrons.
OH- and NH3
Anode
-Ea/R
fruit - fish - bases

16. Alcohols and _______ are FG isomers
ethers
brown volatile liquid
allow for the vapor pressure of water and make sure to level levels
PO4³?

17. cyanide
a-IMFs - b-molecular volume
red - green - blue
CN?
Transition element compounds (except if it has a full or empty d shell)

18. Alkanes are _________ and react by _________
Saturated - Substitution (which requires more radical conditions)
metal oxides and hydrides are ionically bonded and basic
Ksp = 27s4
Iodine and CO2 (dry ice)

19. How are more active metals reduced?
CO3²?
by electrolysis
T increases exponentially the proportion of molecules with E > Ea
E=q + w (negative is by system - positive is on system)

20. What process do you use to separate two liquids with different boiling points?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
fractional distillation
ClO4?
S crystal at 0K=0

21. What does a short - sharp melting point indicate?
Increases down group 1 decreases down group 17
OH?
Soluble
Identity and purity (impure compounds usually have broad & low melting points)

22. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
Mono; di; tri; tetra; penta; hexa.
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Experimental mass/theoretical mass X 100
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

23. What are two substances that sublime at 1 atm when heated?
H2O + CO2 (it decomposes readily)
Iodine and CO2 (dry ice)
water and substances with (s) less dense than
blue

24. chlorite
ClO2?
No - NH3 and HCl gases are extremely soluble
No - it depends on the number of ions produced on dissolving.
acid + alcohol

25. 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?
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
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
zero

26. What do ions and electrons travel through in a voltaic/electrolytic cell?
More chaotic (ex: gases made)
acids
Ions go through the salt bridge - electrons go through metal wires in the external circuit
small size and high charge

27. primary colors
red - green - blue
No - NH3 and HCl gases are extremely soluble
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Salts (ex: CaO + SO2 ? CaSO3)

28. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
CrO4²?
Separating funnel
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

29. How do you identify which is oxidized or otherwise?
allow for the vapor pressure of water and make sure to level levels
red - green - blue
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

30. bromothymol
Mono; di; tri; tetra; penta; hexa.
CN?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
blue (BTB)

31. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
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
Group 1 hydroxides (ex: NaOH)
Anode - oxygen. Cathode - hydrogen

32. If an electrolyte has an endothermic heat of solution - what will happen to its Ksp value when the temperature is raised? What about exothermic?
bright yellow
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Ionic compounds

33. What is an Alkyl group?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

34. hypochlorite
Glowing splint (positive result=relights)
ClO?
Iodine and CO2 (dry ice)
Products - reactants (except for BDE when it's reactants - products)

35. At what point during titration do you have the perfect buffer - and what is the pH at this point?
PO4³?
At half equivalence - pH=pKa
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Ksp = 108s5

36. For a dibasic acid (H2A) - [A²?]= ____ ?
But S° of element is not zero (except at 0K)
K2
Insoluble (except group 1 ammonium and Ba)
Pour liquids using a funnel or down a glass rod

37. chlorate
linear
ClO3?
zero
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

38. What is the relationship in strength between sigma and pi bonds?
do not change
Insoluble except for nitrate and acetate
P2O5
Sigma bonds are stronger than pi bonds

39. ammonium/ammonium compounds
Glacial acetic acid
Soluble
Experimental mass/theoretical mass X 100
Read the bottom of the meniscus

40. What is the formula for summation?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

41. Generally - which oxy acid is strongest?
RCOOH
The one with most oxygen atoms (highest oxidation number)
CnH(2n+2)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

42. What do the 'a' and 'b' in Van Der Waal's equation allow for?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
a-IMFs - b-molecular volume
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Glacial acetic acid

43. dihydrogen phosphate
H2PO4?
H3PO4
voltaic: + electrolytic: -
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

44. Does reactivity increase/decrease going down group 1 and group 17?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
methyl formate
Increases down group 1 decreases down group 17
Orange

45. If a free element is involved - what type of reaction must be involved?
Saturated - Substitution (which requires more radical conditions)
Purple
redox reaction
by electrolysis

46. When the salt bridge is removed what happens to the cell reaction?
NO3?
Glowing splint (positive result=relights)
metal oxides and hydrides are ionically bonded and basic
It ceases - the circuit is broken.

47. What word is a clue for a redox reaction?
zero
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Acidified
K1 x K2

48. How do you clean a buret/pipette for a titration?
Kc=Kp
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Group 1 hydroxides (ex: NaOH)

49. What complex ion does ammonia form with silver? copper? cadmium? zinc?
An active metal.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
The compound with the lowest Ksp value.
Tetrahedral

50. 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
voltaic: - electrolytic: +
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
proton donor base