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. What type of compounds do metals/non metals form?
Soluble
S crystal at 0K=0
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Ionic compounds

2. What is precision?
How grouped results are
Pale yellow
CnH2n+2
Synthetic condensation polymer (aka a polyamide)

3. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Disulfur dichloride
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Current - time and charge on ion (moles of e used in half cell reaction)
non-metal oxides and hydrides are covalently bonded and are acidic.

4. ammonium/ammonium compounds
NH4?
Soluble
same KE - but PEice<PEwater
Experimental mass/theoretical mass X 100

5. How many ligands attach to a central ion in a complex ion?
water and substances with (s) less dense than
are less dense than water
acid + alcohol
#ligands=charge x2

6. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ksp = 108s5
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Initiation energy (NOT Ea)

7. Ca - Sr - Ba
hydroxides (ex: Ba(OH)2)
it reacts by substitution NOT addition
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
allow for the vapor pressure of water and make sure to level levels

8. What is the formula for alkenes?
CnH2n
allow for the vapor pressure of water and make sure to level levels
At half equivalence - pH=pKa
Sigma bonds are stronger than pi bonds

9. How does group 1 metals' density compare to water's?
ns² electrons (first in-first out)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
are less dense than water
Most are soluble except Ag - Pb

10. mercury (I) ion
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Hg2²?
Making sigma bonds and holding lone pairs

11. 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?
P2O5
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
same KE - but PEice<PEwater
Eudiometer

12. What are isomers?
red - green - blue
Molecules with the same molecular formulas - but different structural formulas
Iodine and CO2 (dry ice)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

13. halides
OH?
Most are soluble except Ag - Pb
Transition element compounds (except if it has a full or empty d shell)
[A?]/[HA] x 100 or [BH?]/[B] x 100

14. Metal hydrides are _____ and form _______ and _______ when added to water
HClO4
ionic and form hydrogen and hydroxide
RCHO (carbonyl at end)
Mono; di; tri; tetra; penta; hexa.

15. 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.
CO3²?
small size and high charge
Current - time and charge on ion (moles of e used in half cell reaction)
A) any range. b) 8-10 c) 4-6

16. If a weak acid is diluted more - what happens to its % dissociation value?
Products - reactants (except for BDE when it's reactants - products)
?G=negative - E° must be positive
Sulfur
Increases.

17. What measuring device would you use for very small volumes of liquids?
Ionic compounds
metal oxides and hydrides are ionically bonded and basic
Pipette (burette if need repetition)
Big K=kf/kr

18. 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

19. 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
do not change
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
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

20. iodine - iodine solution - iodine vapor
C4H10
an oxidized and reduced substance
Silvery gray solid - brown - purple
it's lower and occurs over less sharp a range

21. What is the slope of the graph of lnk vs. 1/T?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Cr2O7²?
benzene is less reactive than alkenes
-Ea/R

22. How many faradays of electric charge do you need to produce one mole of O2? H2?
RNH2
R=8.31 J/mol/K
O2 needs 4F/mol H2 needs 2F/mol
non-metal oxides and hydrides are covalently bonded and are acidic.

23. What is the formula for percent yield?
All except for lithium
Iodine and CO2 (dry ice)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Experimental mass/theoretical mass X 100

24. The definition of acidic basic and neutral aqueous solutions is:
CnH2n+2
small size and high charge
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

25. Name C7H16
10?8
Heptane
small size and high charge
Perform ICE BOX calculation based on K1

26. What process do you use to obtain the solute from a solution?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Evaporation
a-IMFs - b-molecular volume
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)

27. What are the common strong bases?
RNH2
Increases.
Group 1 hydroxides (ex: NaOH)
Read the bottom of the meniscus

28. How do you explain trends in atomic properties using Coulomb's Law?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
brown volatile liquid
Salt + water.
0 and 14

29. primary colors
RX
Ppt will NOT form (unsaturated)
fractional distillation
red - green - blue

30. What is the energy you must put into a reaction to make it start called?
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.
Initiation energy (NOT Ea)
?G= -ve - E°= +ve

31. Does reactivity increase/decrease going down group 1 and group 17?
Mn²? - Cr³? - Cr³
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Increases down group 1 decreases down group 17
Anode

32. What complex ion does ammonia form with silver? copper? cadmium? zinc?
it is lower and occurs over less sharp a range
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
strong acids/bases are written as H+ or OH- ions
RCOOR

33. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
The compound with the lowest Ksp value.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Pale purple - (orange)-yellow - red - blue - green.
Unsaturated - addition (ex: decolorize bromine solution)

34. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Decant
Sulfur
Suniverse increases for spontaneous processes
Current - time and charge on ion (moles of e used in half cell reaction)

35. What is the general formula for an amine?
fractional distillation
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.
RNH2
NH4?

36. What are isotopes?
RCOOR
CO3²?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

37. Acidic gases like SO2 in the atmosphere cause what environmental problems?
C4H10
Acid rain - dissolves marble buildings/statues and kills trees.
metal oxides and hydrides are ionically bonded and basic
Anode - oxygen. Cathode - hydrogen

38. What is an Alkyl group?

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

39. nitrate
Pour liquids using a funnel or down a glass rod
Insoluble except group 1 and ammonium
NO3?
White precipitate

40. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Big K=kf/kr
no - they're written undissociated (HAaq)
Mn²? - Cr³? - Cr³
blue

41. Acids + Carbonates (bicarbonates) make?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
ethers
zero
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

42. Lattice energy is high for ions with _____ size and _____ charge
catalyst=conc H2SO4
Only temperature
small size and high charge
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

43. permanganate
MnO4?
They stay the same.
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
E=q + w (negative is by system - positive is on system)

44. hydroxide
yellow
Big K=kf/kr
Sulfur
OH?

45. How does benzene compare in reactivity to alkenes?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
benzene is less reactive than alkenes
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
No - it depends on the number of ions produced on dissolving.

46. Buffer capacity must contain decent amounts of a ________ ________
NO3?
Conjugate pair (one must be a weak base or acid)
Q=It (time in seconds)
Insoluble (except group 1 ammonium and Ba)

47. When is ?G zero?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Acidified
same KE - but PEice<PEwater
Synthetic condensation polymer (aka a polyamide)

48. What is the name of S2Cl2? (Know how to name others like this - too)
Combine the equations for the half reactions in the non-spontaneous direction
Disulfur dichloride
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Salt + water.

49. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Current - time and charge on ion (moles of e used in half cell reaction)
Reduction always takes place at the cathode (RED CAT) In both types of cell!
0.10M HCl (more ions)
Salts (ex: CaO + SO2 ? CaSO3)

50. What is the general formula of an alkane?
Insoluble except for nitrate and acetate
CnH(2n+2)
allow for the vapor pressure of water and make sure to level levels
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)