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. How many ligands attach to a central ion in a complex ion?
#ligands=charge x2
Distillation
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)
voltaic: + electrolytic: -

2. For a weak acid solution in water - Ka = 10?6 what is Kb for its conjugate base?
An active metal.
SO4²?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
10?8

3. What is the general formula for an ester?
RCOOR
voltaic: + electrolytic: -
?H formation of an element in standard state=0
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.

4. Why are noble gases stable?
Insoluble except for nitrate and acetate
chemically (ex: with carbon)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
voltaic: - electrolytic: +

5. What is the general formula for alkyl halides?
RX
are less dense than water
proton donor base
blue

6. What are hybrid orbitals used for?
S2O3²?
+4-covalent - +2-ionic
Making sigma bonds and holding lone pairs
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

7. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
linear
S2O3²?
CO3²?

8. What are allotropes?
diamond and graphite
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
different forms of the same element

9. 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?
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
Salt + water
Nothing
OH?

10. What two compounds are great oxidizing agents?

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

11. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
yellow
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

12. Does reactivity increase/decrease going down group 1 and group 17?
At half equivalence - pH=pKa
The benzene ring (or more correctly the phenyl group - C6H5)
Glacial acetic acid
Increases down group 1 decreases down group 17

13. When driving off water from a hydrate - how do you tell you're done?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Group 1 hydroxides (ex: NaOH)
Decant
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

14. What is the general formula for an aldehyde?
A monomer with a double bond OR two monomers with an arrangement of FGs that allows them to react repeatedly with one another (ex. OH and COOH)
Soluble
RCHO (carbonyl at end)
chemically (ex: with carbon)

15. Is the freezing of ice endothermic or exothermic?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Exothermic
neutralization: high K - H2O product dissociation: low K - H2O reactant
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

16. permanganate
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Unsaturated - addition (ex: decolorize bromine solution)
MnO4?

17. What shape is carbon dioxide?
RCOOR
NH4?
linear
Saturated - Substitution (which requires more radical conditions)

18. What is the sign of the cathode in voltaic cells? in electrolytic cells?
+4-covalent - +2-ionic
voltaic: + electrolytic: -
Insoluble except group 1 and ammonium
Eudiometer

19. What is the general formula for an alcohol?
strong acids/bases are written as H+ or OH- ions
ROH
A salt solution.
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)

20. lead iodide
All except for lithium
bright yellow
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Current - time and charge on ion (moles of e used in half cell reaction)

21. silver iodide
They decrease (or could be the same if the solid has ONLY JUST disappeared)
ClO3?
Clear
Pale yellow

22. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
water and substances with (s) less dense than
Ksp = s²
chemically (ex: with carbon)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

23. What does saturated mean? Unsaturated?
ClO2?
CnH2n+2
Acids; HCOOCH3 is an ester
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.

24. How do you explain trends in atomic properties using Coulomb's Law?
How close results are to the accepted value
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
A) any range. b) 8-10 c) 4-6
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

25. What is the conjugate acid of H2PO4?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Acids; HCOOCH3 is an ester
Iodine and CO2 (dry ice)
H3PO4

26. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Only temperature
non-metal oxides and hydrides are covalently bonded and are acidic.
bases
They stay the same.

27. What do hydrocarbons form when they burn in air (oxygen)?
CnH2n-2
CO2 and H2O
No - it depends on the number of ions produced on dissolving.
neutralization: high K - H2O product dissociation: low K - H2O reactant

28. What is the formula of copper (II) phosphate?
Transition element compounds (except if it has a full or empty d shell)
Products - reactants (except for BDE when it's reactants - products)
Cu3(PO4)2
Mn²? - Cr³? - Cr³

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

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

30. Colorless doesn't mean ______
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Evaporation
atoms
Clear

31. If a free element is involved - what type of reaction must be involved?
CO (poisonous)
Conjugate pair (one must be a weak base or acid)
redox reaction
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

32. acetates
Most are soluble except Ag - Pb
CN?
Soluble
C4H10

33. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
benzene is less reactive than alkenes
left - ppt will form
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Soluble except Ag - Pb - Ca - Sr Ba)

34. iodine - iodine solution - iodine vapor
q=mc?T q=mL (or n x ?h)
Silvery gray solid - brown - purple
OH?
S2O3²?

35. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
Transition element compounds (except if it has a full or empty d shell)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
C2O4²?

36. What is the general formula for an acid?
Kc=Kp
Time?¹ - (ex. s?¹ - hr?¹ - etc)
RCOOH
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

37. What is the catalyst for this reaction Ester + ?
catalyst=conc H2SO4
proton acceptor.
proton donor base
linear

38. What is the difference between equivalence point and end point of a titration.
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
CrO4²?
The Faraday or Faraday's constant.
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)

39. How are metal oxides and hydrides bonded? are they acidic or basic?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Making sigma bonds and holding lone pairs
Exothermic (?H for ANY sa/sb = -57kJ/mol)
metal oxides and hydrides are ionically bonded and basic

40. chlorate
Heat a test tube at an angle at the side of the tube (not bottom)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Unsaturated - addition (ex: decolorize bromine solution)
ClO3?

41. Give an example of a concentrated weak acid.
Transition element compounds (except if it has a full or empty d shell)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
a-IMFs - b-molecular volume
Glacial acetic acid

42. How do you dilute an acid?

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

43. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
Sulfur
Identity and purity (impure compounds usually have broad & low melting points)
blue

44. Is a graduated cylinder or beaker more accurate?
Transition element compounds (except if it has a full or empty d shell)
Graduated cylinder
strong acids/bases are written as H+ or OH- ions
It ceases - the circuit is broken.

45. The oxidation numbers of the metals or nonmetals ___________ during such a reaction
#ligands=charge x2
do not change
OH?
Tetrahedral

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

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

47. How does half life change for zero-th order - first order - and second order processes?
Unsaturated - addition (ex: decolorize bromine solution)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Insoluble
zero-th: decreases - first: constant - second: increases

48. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
RNH2
[A?]/[HA] x 100 or [BH?]/[B] x 100
blue (BTB)

49. Color (absorbance) is proportional to ________
Concentration
blue glass - it filters UV
redox reaction
ion pairing

50. lead compounds
Graduated cylinder
Filtration
ion pairing
Insoluble except nitrate and acetate