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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. Name C7H16
P2O5
ROH
Perform ICE BOX calculation based on K1
Heptane

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

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3. hydroxides
Decant
Insoluble (except group 1 ammonium and Ba)
It ceases - the circuit is broken.
zero

4. What does a short - sharp melting point indicate?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
CO2 and H2O
ionic and form hydrogen and hydroxide
Identity and purity (impure compounds usually have broad & low melting points)

5. For a dibasic acid (H2A) - [A²?]= ____ ?
CnH2n-2
K2
More chaotic (ex: gases made)
voltaic: + electrolytic: -

6. What is the charge on a chlorine atom?
NH4?
same KE - but PEice<PEwater
zero
Most INsoluble except group 1 and ammonium

7. What two types of substances are present in all redox reactions?
CnH2n+1 often designated 'R' ex C3H7 is propyl
a-IMFs - b-molecular volume
Heat a test tube at an angle at the side of the tube (not bottom)
an oxidized and reduced substance

8. A Bronsted-Lowry base is...
proton acceptor.
Trigonal pyramidal
allow for the vapor pressure of water and make sure to level levels
benzene has a delocalized pi ring structure

9. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
?G= -ve - E°= +ve
ClO2?
0 and 14
basic

10. What is the formula for summation?

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11. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
CO (poisonous)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
?G=negative - E° must be positive
NH4?

12. What do acids plus active metals form?
Concentration
PO4³?
The benzene ring (or more correctly the phenyl group - C6H5)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

13. Metal hydrides are _____ and form _______ and _______ when added to water
an oxidized and reduced substance
ionic and form hydrogen and hydroxide
Glacial acetic acid
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)

14. What are hybrid orbitals used for?
Making sigma bonds and holding lone pairs
C2O4²?
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
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

15. dihydrogen phosphate
H2PO4?
acid + alcohol
CN?
Orange

16. What steps do organic labs consist of?
proton acceptor.
Synthesis - separation and purification of the product and its identification.
Iodine and CO2 (dry ice)
Salt + water.

17. What type of solutions do small - highly charged cations tend to form?
Transition element compounds (except if it has a full or empty d shell)
Pale yellow
H2O + CO2 (it decomposes readily)
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

18. Color is due to ______ _______ of light.
But S° of element is not zero (except at 0K)
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Selective absorption
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

19. What type of compounds do metals/non metals form?
ClO4?
do not change
redox reaction
Ionic compounds

20. In equilibrium calculations for weak acids/bases - when should you ignore 'x' with respect to initial concentration of acid or base

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21. If a free element is involved - what type of reaction must be involved?
H3PO4
A salt solution.
redox reaction
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

22. 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?
0.10M HCl (more ions)
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
The compound with the lowest Ksp value.
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)

23. How do you clean a buret/pipette for a titration?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
allow for the vapor pressure of water and make sure to level levels
Insoluble except nitrate and acetate

24. What is accuracy?
Distillation
Silvery gray solid - brown - purple
CO3²?
How close results are to the accepted value

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

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26. BaSO4
E=q + w (negative is by system - positive is on system)
chemically (ex: with carbon)
Insoluble
Time?¹ - (ex. s?¹ - hr?¹ - etc)

27. What is a coordinate covalent bond?
RCOOH
Mn²? - Cr³? - Cr³
diamond and graphite
Both electrons come from the same atom (just as good as a regular bond)

28. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
an oxidized and reduced substance
CO2 and H2O

29. ________ are Lewis bases - because they can donate a lone pair of electrons.
Silvery gray solid - brown - purple
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
Initiation energy (NOT Ea)
OH- and NH3

30. What are the names and formulas of the 6 strong acids?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
proton acceptor.
yellow
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

31. What is a dipeptide? polypeptide? protein?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
C2O4²?
[A?]/[HA] x 100 or [BH?]/[B] x 100
diamond and graphite

32. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Exothermic
Glacial acetic acid

33. chlorate
ClO3?
Saturated - Substitution (which requires more radical conditions)
Orange
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)

34. Ions are not ______.
atoms
The one with most oxygen atoms (highest oxidation number)
CO3²?
K1 x K2

35. carbonates
They decrease (or could be the same if the solid has ONLY JUST disappeared)
acids
Unsaturated - addition (ex: decolorize bromine solution)
Insoluble except group 1 and ammonium

36. Both Acetic acid and ____________ are also functional isomers.
voltaic: + electrolytic: -
Increases.
methyl formate
Pale yellow

37. 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
CnH2n+2
a-IMFs - b-molecular volume
Read the bottom of the meniscus

38. When a cell is 'flat' What is its voltage?
MnO4?
Hg2²?
CO3²?
zero

39. chromate
The dilution effect when the solutions mix. M1V1 = M2V2
CnH2n-2
An active metal.
CrO4²?

40. What do hydrocarbons form when they burn in air (oxygen)?
Filtration
blue glass - it filters UV
CO2 and H2O
Hg2²?

41. Why are i factors (Van't Hoff factors) often less than ideal?
H2PO4?
zero-th: decreases - first: constant - second: increases
ion pairing
Soluble except Ag - Pb - Ca - Sr Ba)

42. When the salt bridge is removed what happens to the cell reaction?
Insoluble except group 1 and ammonium
S crystal at 0K=0
Saturated - Substitution (which requires more radical conditions)
It ceases - the circuit is broken.

43. What is the basic structure of an optical isomer?
Clear
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Conjugate pair (one must be a weak base or acid)
Molecules with the same molecular formulas - but different structural formulas

44. Aromatic compounds contain what?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
The benzene ring (or more correctly the phenyl group - C6H5)
C4H10
water and substances with (s) less dense than

45. How are primary alcohols turned into acids?
Ksp = 4s³
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Pale purple - (orange)-yellow - red - blue - green.
'non-active' metals such as Cu - Ag - Au - Pt - etc.

46. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
catalyst=conc H2SO4
?H-kJ - ?S-J - ?G-kJ
They decrease (or could be the same if the solid has ONLY JUST disappeared)
RCOR

47. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Both electrons come from the same atom (just as good as a regular bond)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
0 and 14
Synthetic condensation polymer (aka a polyamide)

48. What is the formula for percent yield?
0 and 14
brown volatile liquid
Experimental mass/theoretical mass X 100
Graduated cylinder

49. What is the conjugate base of NH3?
a-IMFs - b-molecular volume
it's lower and occurs over less sharp a range
NH2?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

50. Which of the rates changes more when temperature is increased?
zero
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
proton donor base
Molecules with the same molecular formulas - but different structural formulas