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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. copper sulfate
blue
diamond and graphite
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
No - it depends on the number of ions produced on dissolving.

2. What are two substances that sublime at 1 atm when heated?
Iodine and CO2 (dry ice)
proton donor base
Add acid to water so that the acid doesn't boil and spit
blue (BTB)

3. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
Distillation
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
linear

4. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
look for changes in oxidation # - the one that goes up is oxidized and is the RA
PO4³?

5. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ClO4?
Glacial acetic acid
an oxidized and reduced substance

6. phosphate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Insoluble except for nitrate and acetate
Check for air bubbles in the buret and remove the buret funnel from the buret
PO4³?

7. When can supercooling occur? What does it look like on a cooling curve?

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8. What kind of bonding structure does benzene have?
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
benzene has a delocalized pi ring structure
Increases down group 1 decreases down group 17
q=mc?T q=mL (or n x ?h)

9. Acids + Carbonates (bicarbonates) make?
Insoluble (except group 1 ammonium and Ba)
?G=negative - E° must be positive
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

10. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
H2O + CO2 (it decomposes readily)
Eudiometer
CN?

11. What are the signs of ?G and E° for spontaneous reactions?
Nothing
?G=negative - E° must be positive
MnO4?
Exothermic (?H for ANY sa/sb = -57kJ/mol)

12. How are metal oxides and hydrides bonded? are they acidic or basic?
Insoluble
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
metal oxides and hydrides are ionically bonded and basic

13. How are primary alcohols turned into acids?
No - NH3 and HCl gases are extremely soluble
acid + alcohol
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

14. ammonium
Ksp = s²
NH4?
Current - time and charge on ion (moles of e used in half cell reaction)
Salt + water

15. Generally - which oxy acid is strongest?
Suniverse increases for spontaneous processes
Ksp = 4s³
The one with most oxygen atoms (highest oxidation number)
Ionic compounds

16. 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?
PO4³?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
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

17. What is H2CO3 (carbonate acid) usually written as?
Making sigma bonds and holding lone pairs
ClO3?
left - ppt will form
H2O + CO2 (it decomposes readily)

18. permanganate
P2O5
boiling without losing volatile solvents/reactants
MnO4?
Ionic compounds

19. Why are noble gases stable?
NH4?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
ClO2?

20. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
A) any range. b) 8-10 c) 4-6
Clear
K1 x K2

21. How do you explain trends in atomic properties using Coulomb's Law?
ClO3?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Glowing splint (positive result=relights)

22. What two types of substances are present in all redox reactions?
basic
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
an oxidized and reduced substance
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

23. What are hybrid orbitals used for?
Acid rain - dissolves marble buildings/statues and kills trees.
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Making sigma bonds and holding lone pairs
Soluble

24. acetate
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Trigonal pyramidal
CH3COO?
proton acceptor.

25. Alcohols and _______ are FG isomers
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
ethers
Anode - oxygen. Cathode - hydrogen
acids

26. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Molecules with the same molecular formulas - but different structural formulas
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
a-IMFs - b-molecular volume
Ksp = s²

27. What do ions and electrons travel through in a voltaic/electrolytic cell?
Exothermic
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Ions go through the salt bridge - electrons go through metal wires in the external circuit

28. Esters smell like _______ and amines smell like _______ and are ______.
do not change
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
No - NH3 and HCl gases are extremely soluble
fruit - fish - bases

29. Where are group I metals stored?
CO2 and H2O
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)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Group I metals (soft metals) are stored under oil

30. What is HCOOCH3?
Filtration
Acids; HCOOCH3 is an ester
Trigonal pyramidal
But S° of element is not zero (except at 0K)

31. Which value of R do you use for all energy and kinetics calculations?
ClO4?
Heptane
R=8.31 J/mol/K
Salts (ex: CaO + SO2 ? CaSO3)

32. What is the catalyst for this reaction Ester + ?
K2
catalyst=conc H2SO4
it reacts by substitution NOT addition
K1 x K2

33. chlorine
HClO4
Greenish-yellow gas
RX
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)

34. Nonmetals are good _____ agents. Metals are good _______ agents.
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Current - time and charge on ion (moles of e used in half cell reaction)
Experimental mass/theoretical mass X 100
#ligands=charge x2

35. What is the general formula for alkyl halides?
linear
redox reaction
RX
OH- and NH3

36. What is a coordinate covalent bond?
Soluble
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
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
Both electrons come from the same atom (just as good as a regular bond)

37. What are two substances that sublime at 1 atm when heated?
Conjugate pair (one must be a weak base or acid)
H3PO4
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Iodine and CO2 (dry ice)

38. What type of polymer is nylon?
Synthetic condensation polymer (aka a polyamide)
it's lower and occurs over less sharp a range
Group I metals (soft metals) are stored under oil
H+

39. A geometric (or cis-trans) isomer exists due to.....
do not change
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Tetrahedral
Big K=kf/kr

40. What is the sign of the anode in voltaic cells? in electrolytic cells?
blue (BTB)
Orange
voltaic: - electrolytic: +
Filtration

41. Is the standard entropy (S°) of an element zero?
Synthetic condensation polymer (aka a polyamide)
But S° of element is not zero (except at 0K)
Increases down group 1 decreases down group 17
10?8

42. What process do you use to obtain the precipitate from a solution?
it is lower and occurs over less sharp a range
H2O + CO2 (it decomposes readily)
Synthesis - separation and purification of the product and its identification.
Filtration

43. Give an example of a dilute strong acid.
neutralization: high K - H2O product dissociation: low K - H2O reactant
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
HClO4

44. What are the units of the first order rate constant?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Soluble except Ag - Pb - Ca - Sr Ba)
RX
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

45. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Mono; di; tri; tetra; penta; hexa.
H+
Ionic compounds
The compound with the lowest Ksp value.

46. What are isotopes?
Insoluble except group 1 and ammonium
Heat a test tube at an angle at the side of the tube (not bottom)
Salt + water
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

47. What does a short - sharp melting point indicate?
OH- and NH3
fractional distillation
Identity and purity (impure compounds usually have broad & low melting points)
Soluble

48. How does half life change for zero-th order - first order - and second order processes?
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.
ethers
zero-th: decreases - first: constant - second: increases
CnH2n+1 often designated 'R' ex C3H7 is propyl

49. How do you heat a test tube?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Tetrahedral
ClO3?
Heat a test tube at an angle at the side of the tube (not bottom)

50. Which alkali metals float on water?
All except for lithium
Iodine and CO2 (dry ice)
zero
Soluble except Ag - Pb - Ca - Sr Ba)