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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. chlorite
zero
ClO2?
CnH2n+1 often designated 'R' ex C3H7 is propyl
chemically (ex: with carbon)

2. Does Kw increase or decrease with T? Why?
Mono; di; tri; tetra; penta; hexa.
S crystal at 0K=0
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
lighted splint (positive result=pop)

3. What does a short - sharp melting point indicate?
H2PO4?
Iodine and CO2 (dry ice)
Salt + water
Identity and purity (impure compounds usually have broad & low melting points)

4. What type of compounds are almost always colored?
The dilution effect when the solutions mix. M1V1 = M2V2
Clear
K1 x K2
Transition element compounds (except if it has a full or empty d shell)

5. ________ are Lewis bases - because they can donate a lone pair of electrons.
ClO4?
OH- and NH3
fractional distillation
ethers

6. Color (absorbance) is proportional to ________
by electrolysis
Concentration
chemically (ex: with carbon)
The compound with the lowest Ksp value.

7. chromate ion (soln + most solids)
Cr2O7²?
CrO4²?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
yellow

8. What should you check for before you begin titrating?
Read the bottom of the meniscus
Check for air bubbles in the buret and remove the buret funnel from the buret
RCOR
Salt + water

9. How do you get the equation for a net electrolysis reaction?
Combine the equations for the half reactions in the non-spontaneous direction
NO3?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
proton donor base

10. ammonium/ammonium compounds
Increases down group 1 decreases down group 17
Soluble
CO2 and H2O
ClO3?

11. What are isotopes?
lighted splint (positive result=pop)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
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.
acid + alcohol

12. How do you heat a test tube?
Heat a test tube at an angle at the side of the tube (not bottom)
No - it depends on the number of ions produced on dissolving.
Salt + water
Evaporation

13. perchlorate
T increases exponentially the proportion of molecules with E > Ea
ClO4?
fruit - fish - bases
red - green - blue

14. What is the first law of thermodynamics?
CH3COO?
H3PO4
E=q + w (negative is by system - positive is on system)
A salt solution.

15. What is the sign of the anode in voltaic cells? in electrolytic cells?
Check for air bubbles in the buret and remove the buret funnel from the buret
non-metal oxides and hydrides are covalently bonded and are acidic.
voltaic: - electrolytic: +
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

16. How are metal oxides and hydrides bonded? are they acidic or basic?
metal oxides and hydrides are ionically bonded and basic
T increases exponentially the proportion of molecules with E > Ea
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

17. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
Tetrahedral
Separating funnel
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
?G= -ve - E°= +ve

18. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Synthesis - separation and purification of the product and its identification.
Reduction always takes place at the cathode (RED CAT) In both types of cell!
How grouped results are
Ksp = 27s4

19. Esters smell like _______ and amines smell like _______ and are ______.
Insoluble except group 1 and ammonium
fruit - fish - bases
methyl formate
+4-covalent - +2-ionic

20. Which value of R do you use for all energy and kinetics calculations?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
R=8.31 J/mol/K
It ceases - the circuit is broken.
Heat a test tube at an angle at the side of the tube (not bottom)

21. oxalate
C2O4²?
0 and 14
Both electrons come from the same atom (just as good as a regular bond)
Reduction always takes place at the cathode (RED CAT) In both types of cell!

22. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
zero
basic
?H formation of an element in standard state=0
PO4³?

23. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
zero
catalyst=conc H2SO4
Evaporation

24. 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
water and substances with (s) less dense than
OH- and NH3
CN?

25. What is the sign of the cathode in voltaic cells? in electrolytic cells?
Pale purple - (orange)-yellow - red - blue - green.
voltaic: + electrolytic: -
ClO4?
ClO?

26. What is H2CO3 (carbonate acid) usually written as?
RCOOR
H2O + CO2 (it decomposes readily)
The benzene ring (or more correctly the phenyl group - C6H5)
Orange

27. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
water and substances with (s) less dense than
?G= -ve - E°= +ve
Conjugate pair (one must be a weak base or acid)

28. chlorine
Ksp = 4s³
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Insoluble except for nitrate and acetate
Greenish-yellow gas

29. What type of metals don't react with water or acids to form H2?

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

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31. carbonates
q=mc?T q=mL (or n x ?h)
Insoluble (except group 1 ammonium and Ba)
Molecules with the same molecular formulas - but different structural formulas
Insoluble except group 1 and ammonium

32. lead iodide
bright yellow
CnH2n+1 often designated 'R' ex C3H7 is propyl
?H formation of an element in standard state=0
No - NH3 and HCl gases are extremely soluble

33. hydroxide
do not change
OH?
Clear
Group I metals (soft metals) are stored under oil

34. Acid plus base make?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Acid rain - dissolves marble buildings/statues and kills trees.
Salt + water.
fruit - fish - bases

35. What is the relationship in strength between sigma and pi bonds?
Group 1 hydroxides (ex: NaOH)
it's lower and occurs over less sharp a range
Sigma bonds are stronger than pi bonds
Decant

36. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
The compound with the lowest Ksp value.
Pour liquids using a funnel or down a glass rod
ion pairing

37. Acidic gases like SO2 in the atmosphere cause what environmental problems?
ion pairing
Acid rain - dissolves marble buildings/statues and kills trees.
Decant
NH4?

38. What are two substances that sublime at 1 atm when heated?
Perform ICE BOX calculation based on K1
No - it depends on the number of ions produced on dissolving.
Iodine and CO2 (dry ice)
Current - time and charge on ion (moles of e used in half cell reaction)

39. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
Kc=Kp
Initiation energy (NOT Ea)
They stay the same.
Increases.

40. What is the word equation for condensation polymerisation ?
H2PO4?
RCHO (carbonyl at end)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
R=8.31 J/mol/K

41. What is the general formula for alkyl halides?
H2PO4?
Soluble
RX
fractional distillation

42. What is HCOOCH3?
Acids; HCOOCH3 is an ester
At half equivalence - pH=pKa
Increases.
Making sigma bonds and holding lone pairs

43. What do acids plus active metals form?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
?H formation of an element in standard state=0
Check for air bubbles in the buret and remove the buret funnel from the buret

44. Which of the rates changes more when temperature is increased?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Ksp = 108s5
Monomer + monomer = polymer product + a simple molecule such as water or HCl
C2O4²?

45. What equipment do you need for a titration?
Ionic compounds
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
proton acceptor.
Synthetic condensation polymer (aka a polyamide)

46. What are allotropes?
blue (BTB)
C4H10
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
different forms of the same element

47. What is the formula for alkanes?
0 and 14
Salts (ex: CaO + SO2 ? CaSO3)
ionic and form hydrogen and hydroxide
CnH2n+2

48. Acids + Carbonates (bicarbonates) make?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
K1 x K2
The compound with the lowest Ksp value.

49. How does half life change for zero-th order - first order - and second order processes?
Decant
water and substances with (s) less dense than
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
zero-th: decreases - first: constant - second: increases

50. What are the signs of ?G and E° for spontaneous reactions?
Glowing splint (positive result=relights)
?G=negative - E° must be positive
a-IMFs - b-molecular volume
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)