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. primary colors
Separating funnel
red - green - blue
H3PO4
No - it depends on the number of ions produced on dissolving.

2. How are more active metals reduced?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
by electrolysis
Mono; di; tri; tetra; penta; hexa.

3. What is the word equation for condensation polymerisation ?
metal oxides and hydrides are ionically bonded and basic
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Exothermic (?H for ANY sa/sb = -57kJ/mol)
The one with most oxygen atoms (highest oxidation number)

4. ________ are Lewis bases - because they can donate a lone pair of electrons.
basic
by electrolysis
Insoluble (except group 1 ammonium and Ba)
OH- and NH3

5. How do you identify which is oxidized or otherwise?
Anode
RX
Insoluble except group 1 and ammonium
look for changes in oxidation # - the one that goes up is oxidized and is the RA

6. What should you check for before you begin titrating?
Check for air bubbles in the buret and remove the buret funnel from the buret
bright yellow
Experimental mass/theoretical mass X 100
Monomer + monomer = polymer product + a simple molecule such as water or HCl

7. Give an example of a concentrated weak acid.
No - NH3 and HCl gases are extremely soluble
Glacial acetic acid
Anode - oxygen. Cathode - hydrogen
Salt and water

8. What word is a clue for a redox reaction?
an oxidized and reduced substance
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Acidified
zero

9. If ?S is positive - are the products more or less chaotic than the reactants?
methyl formate
How grouped results are
More chaotic (ex: gases made)
Synthesis - separation and purification of the product and its identification.

10. Esterification is...
CnH2n
Mono; di; tri; tetra; penta; hexa.
acid + alcohol
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)

11. Name six characteristics of transition elements (or their compounds)
How grouped results are
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
look for changes in oxidation # - the one that goes up is oxidized and is the RA
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)

12. When combining half equations - what do you do to E° values when multiplying coefficients?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Ksp = 108s5
Nothing
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

13. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Separating funnel
Exothermic
White precipitate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

14. What causes the dramatic effect of T on rate?
Salt and water
methyl formate
T increases exponentially the proportion of molecules with E > Ea
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.

15. lead compounds
Making sigma bonds and holding lone pairs
ion pairing
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Insoluble except nitrate and acetate

16. What process do you use to obtain a solvent from a solution?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Orange
Distillation
?G=negative - E° must be positive

17. What type of compounds do metals/non metals form?
Ionic compounds
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
?H-kJ - ?S-J - ?G-kJ
0.10M HCl (more ions)

18. What changes Keq?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
bent
Only temperature

19. chlorine
ROR
CnH(2n+2)
Selective absorption
Greenish-yellow gas

20. Give an example of a dilute strong acid.
blue
E=q + w (negative is by system - positive is on system)
Soluble
HClO4

21. What type of compounds are almost always colored?
do not change
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Unsaturated - addition (ex: decolorize bromine solution)
Transition element compounds (except if it has a full or empty d shell)

22. What shape is ammonia?
do not change
Trigonal pyramidal
zero
Sigma bonds are stronger than pi bonds

23. How can metals like iron and zinc be reduced?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Pale yellow
chemically (ex: with carbon)
same KE - but PEice<PEwater

24. What are the formulas for q?
Q=It (time in seconds)
q=mc?T q=mL (or n x ?h)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
Ksp = 108s5

25. When driving off water from a hydrate - how do you tell you're done?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

26. What type of compounds do Group 14 form?
NH4?
ClO3?
diamond and graphite
+4-covalent - +2-ionic

27. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
?H formation of an element in standard state=0
Evaporation

28. What effect does increasing the size/surface area of a voltaic cell have on the cell?
#ligands=charge x2
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CnH2n-2

29. What is accuracy?
Ksp = 4s³
How close results are to the accepted value
water and substances with (s) less dense than
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

30. What is reflux?
different forms of the same element
boiling without losing volatile solvents/reactants
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
atoms

31. What is a coordinate covalent bond?
Both electrons come from the same atom (just as good as a regular bond)
|experimental - accepted|/accepted X 100
fractional distillation
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

32. What is the general formula for an alcohol?
How grouped results are
Kc=Kp
Conjugate pair (one must be a weak base or acid)
ROH

33. Alkenes are ________ and react by __________
Most INsoluble except group 1 and ammonium
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Soluble
Unsaturated - addition (ex: decolorize bromine solution)

34. Why are i factors (Van't Hoff factors) often less than ideal?
T increases exponentially the proportion of molecules with E > Ea
The one with most oxygen atoms (highest oxidation number)
Soluble
ion pairing

35. barium sulfate
redox reaction
Salt and water
White precipitate
strong acids/bases are written as H+ or OH- ions

36. What is the general formula of an alkane?
CnH(2n+2)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Pale purple - (orange)-yellow - red - blue - green.
Transition element compounds (except if it has a full or empty d shell)

37. Can you collect soluble gases over water?
No - NH3 and HCl gases are extremely soluble
it's lower and occurs over less sharp a range
Heptane
Pale purple - (orange)-yellow - red - blue - green.

38. 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?
The compound with the lowest Ksp value.
#ligands=charge x2
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Separating funnel

39. What is the basic structure of an optical isomer?
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
benzene is less reactive than alkenes
Ksp = 108s5
Making sigma bonds and holding lone pairs

40. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Exothermic
RX

41. What is the charge on a chlorine atom?
zero
Exothermic
-Ea/R
Salts (ex: CaO + SO2 ? CaSO3)

42. How many faradays of electric charge do you need to produce one mole of O2? H2?
O2 needs 4F/mol H2 needs 2F/mol
fruit - fish - bases
OH?
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.

43. What element is used to vulcanize rubber?
Synthetic condensation polymer (aka a polyamide)
White precipitate
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Sulfur

44. What are two substances that sublime at 1 atm when heated?
Graduated cylinder
Evaporation
do not change
Iodine and CO2 (dry ice)

45. What is the conjugate base of NH3?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
NH2?
Soluble
same KE - but PEice<PEwater

46. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
The dilution effect when the solutions mix. M1V1 = M2V2
H2PO4?
Insoluble except for nitrate and acetate
allow for the vapor pressure of water and make sure to level levels

47. What do nonmetal oxides plus water form?
CnH2n-2
atoms
acids
Clear

48. When is ?G zero?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
q=mc?T q=mL (or n x ?h)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
do not change

49. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
H2O + CO2 (it decomposes readily)
No - it depends on the number of ions produced on dissolving.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Purple

50. What are the signs for ?G and E° for spontaneous reactions?
brown volatile liquid
blue glass - it filters UV
Insoluble (except group 1 ammonium and Ba)
?G= -ve - E°= +ve