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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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1. phosphate
catalyst=conc H2SO4
?H-kJ - ?S-J - ?G-kJ
PO4³?
?G=negative - E° must be positive

2. What process do you use to obtain the precipitate from a solution?
RNH2
Filtration
Sulfur
Glacial acetic acid

3. Acids + Carbonates (bicarbonates) make?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
C2O4²?
Salt + water
H2PO4?

4. iodine - iodine solution - iodine vapor
Sigma bonds are stronger than pi bonds
Silvery gray solid - brown - purple
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

5. Neutralization is an ________ reaction.
Suniverse increases for spontaneous processes
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Orange
T increases exponentially the proportion of molecules with E > Ea

6. What are two allotropes of carbon?
'non-active' metals such as Cu - Ag - Au - Pt - etc.
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)
diamond and graphite
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

7. ammonium/ammonium compounds
Soluble
Read the bottom of the meniscus
Anode
voltaic: + electrolytic: -

8. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
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
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

9. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
a-IMFs - b-molecular volume
HClO4
Ksp = 27s4

10. What is the general formula for an alcohol?
It ceases - the circuit is broken.
ROH
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?)
C2O4²?

11. Buffer capacity must contain decent amounts of a ________ ________
boiling without losing volatile solvents/reactants
catalyst=conc H2SO4
Conjugate pair (one must be a weak base or acid)
CnH2n-2

12. What do you use to look at burning magnesium? why?
blue glass - it filters UV
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.
Increases.
CrO4²?

13. What is the general formula of an alkane?
CnH2n+1 often designated 'R' ex C3H7 is propyl
Conjugate pair (one must be a weak base or acid)
CnH(2n+2)
Insoluble except group 1 and ammonium

14. What is the energy you must put into a reaction to make it start called?
Big K=kf/kr
Disulfur dichloride
How close results are to the accepted value
Initiation energy (NOT Ea)

15. Both Acetic acid and ____________ are also functional isomers.
E=q + w (negative is by system - positive is on system)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
methyl formate
White precipitate

16. Do anions flow to the cathode or anode?
Mono; di; tri; tetra; penta; hexa.
benzene is less reactive than alkenes
Perform ICE BOX calculation based on K1
Anode

17. What is the first law of thermodynamics?
E=q + w (negative is by system - positive is on system)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Soluble
Group I metals (soft metals) are stored under oil

18. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
Disulfur dichloride
benzene is less reactive than alkenes
Exothermic (?H for ANY sa/sb = -57kJ/mol)

19. What is the test for oxygen?
Disulfur dichloride
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Silvery gray solid - brown - purple
Glowing splint (positive result=relights)

20. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Glowing splint (positive result=relights)
CnH2n
Mn²? - Cr³? - Cr³
No - it depends on the number of ions produced on dissolving.

21. How are primary alcohols turned into acids?
Suniverse increases for spontaneous processes
Separating funnel
Experimental mass/theoretical mass X 100
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

22. thiosulfate
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
S2O3²?
CO3²?

23. What is the formula for alkynes?
Ionic compounds
O2 needs 4F/mol H2 needs 2F/mol
CnH2n-2
[A?]/[HA] x 100 or [BH?]/[B] x 100

24. Which would cause the bulb in a conductivity apparatus to be brightest?
0.10M HCl (more ions)
CO3²?
Acid rain - dissolves marble buildings/statues and kills trees.
red - green - blue

25. barium sulfate
Ions go through the salt bridge - electrons go through metal wires in the external circuit
White precipitate
Mn²? - Cr³? - Cr³
Most INsoluble except group 1 and ammonium

26. How do you find the pH for a dibasic acid? (H2A)?
Perform ICE BOX calculation based on K1
Soluble
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Graduated cylinder

27. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
C4H10
Molecules with the same molecular formulas - but different structural formulas
The compound with the lowest Ksp value.
Disulfur dichloride

28. hydroxides
Insoluble (except group 1 ammonium and Ba)
Q=It (time in seconds)
NH4?
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

29. One mole of electrons carries 96500Coulombs - what is this quantity called?

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30. A Bronsted-Lowry base is...
Most are soluble except Ag - Pb
Increases down group 1 decreases down group 17
proton acceptor.
bent

31. What is accuracy?
Soluble
benzene is less reactive than alkenes
How close results are to the accepted value
ion pairing

32. lead compounds
RCOOR
Synthetic condensation polymer (aka a polyamide)
Insoluble except nitrate and acetate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

33. Why are noble gases stable?
No - it depends on the number of ions produced on dissolving.
Salt + water.
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Pour liquids using a funnel or down a glass rod

34. How does benzene compare in reactivity to alkenes?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Pale purple - (orange)-yellow - red - blue - green.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
benzene is less reactive than alkenes

35. What is Big K in terms of kf and kr?
Big K=kf/kr
Cu3(PO4)2
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
S2O3²?

36. How many normal boiling points and boiling points are there?

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37. chlorite
Tetrahedral
The dilution effect when the solutions mix. M1V1 = M2V2
ClO2?
bright yellow

38. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
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)
benzene has a delocalized pi ring structure
same KE - but PEice<PEwater
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

39. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Concentration
an oxidized and reduced substance
non-metal oxides and hydrides are covalently bonded and are acidic.
CnH2n+1 often designated 'R' ex C3H7 is propyl

40. chromate
Making sigma bonds and holding lone pairs
voltaic: - electrolytic: +
CrO4²?
zero

41. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Distillation
RX

42. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
zero
q=mc?T q=mL (or n x ?h)
10?8

43. How many faradays of electric charge do you need to produce one mole of O2? H2?
T increases exponentially the proportion of molecules with E > Ea
P2O5
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
O2 needs 4F/mol H2 needs 2F/mol

44. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Ksp = 4s³
NH2?
T increases exponentially the proportion of molecules with E > Ea

45. What is the general formula for an ester?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
RCOOR
Distillation
But S° of element is not zero (except at 0K)

46. What type of compounds are almost always colored?
Synthetic condensation polymer (aka a polyamide)
?G=negative - E° must be positive
fruit - fish - bases
Transition element compounds (except if it has a full or empty d shell)

47. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Anode - oxygen. Cathode - hydrogen
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
voltaic: - electrolytic: +

48. How do you heat a test tube?
Cr2O7²?
Synthetic condensation polymer (aka a polyamide)
benzene is less reactive than alkenes
Heat a test tube at an angle at the side of the tube (not bottom)

49. bromine
S2O3²?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
brown volatile liquid
Soluble

50. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
A salt solution.
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)