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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. Generally - which oxy acid is strongest?
Cu3(PO4)2
Ionic compounds
The one with most oxygen atoms (highest oxidation number)
Insoluble (except group 1 ammonium and Ba)

2. What word is a clue for a redox reaction?
Acidified
The dilution effect when the solutions mix. M1V1 = M2V2
Disulfur dichloride
Group 1 hydroxides (ex: NaOH)

3. What is the formula for alkenes?
are less dense than water
Transition element compounds (except if it has a full or empty d shell)
Ksp = 27s4
CnH2n

4. 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
Products - reactants (except for BDE when it's reactants - products)
Glowing splint (positive result=relights)
T increases exponentially the proportion of molecules with E > Ea

5. Neutralization is an ________ reaction.
allow for the vapor pressure of water and make sure to level levels
left - ppt will form
Exothermic (?H for ANY sa/sb = -57kJ/mol)
different forms of the same element

6. What is the general formula for an acid?
fruit - fish - bases
RCOOH
it's lower and occurs over less sharp a range
NO3?

7. When combining half equations - what do you do to E° values when multiplying coefficients?
Nothing
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
do not change
ethers

8. What is the third law of thermodynamics?
The one with most oxygen atoms (highest oxidation number)
S crystal at 0K=0
How grouped results are
CnH2n-2

9. What should you check for before you begin titrating?
Greenish-yellow gas
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.
0.10M HCl (more ions)
Check for air bubbles in the buret and remove the buret funnel from the buret

10. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
NO3?
are less dense than water

11. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Eudiometer
NH2?

12. Both Acetic acid and ____________ are also functional isomers.
Hg2²?
methyl formate
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Pour liquids using a funnel or down a glass rod

13. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
More chaotic (ex: gases made)
neutralization: high K - H2O product dissociation: low K - H2O reactant
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.
blue glass - it filters UV

14. hypochlorite
ClO?
Iodine and CO2 (dry ice)
Read the bottom of the meniscus
Oxides that react with both acids (make salts + water) AND bases (forms complex ion - ex: ZnO and Al2O3 in bases make Zn(OH)4²? and Al(OH)4? or Al(OH)6³?)

15. mercury (I) ion
Hg2²?
Increases.
Making sigma bonds and holding lone pairs
The benzene ring (or more correctly the phenyl group - C6H5)

16. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
They stay the same.
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
catalyst=conc H2SO4
CnH2n-2

17. How do you dilute an acid?

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18. What is the general formula for alkyl halides?
Sulfur
?H-kJ - ?S-J - ?G-kJ
RX
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

19. What shape is water?
More chaotic (ex: gases made)
RNH2
bent
But S° of element is not zero (except at 0K)

20. What is the charge on a chlorine atom?
?H formation of an element in standard state=0
zero
The dilution effect when the solutions mix. M1V1 = M2V2
Ksp = 108s5

21. If a weak acid is diluted more - what happens to its % dissociation value?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Increases.
Check for air bubbles in the buret and remove the buret funnel from the buret
OH- and NH3

22. hydroxide
Pipette (burette if need repetition)
Glowing splint (positive result=relights)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
OH?

23. One mole of electrons carries 96500Coulombs - what is this quantity called?

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24. copper sulfate
blue
fractional distillation
CO (poisonous)
ionic and form hydrogen and hydroxide

25. What kind of bonding structure does benzene have?
Check for air bubbles in the buret and remove the buret funnel from the buret
benzene has a delocalized pi ring structure
Ksp = 4s³
Trigonal pyramidal

26. What is reflux?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Anode - oxygen. Cathode - hydrogen
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
boiling without losing volatile solvents/reactants

27. If a free element is involved - what type of reaction must be involved?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
redox reaction
ion pairing
Only temperature

28. What is an Alkyl group?

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29. What do group I/II metal oxides and acids form?
q=mc?T q=mL (or n x ?h)
RNH2
redox reaction
Salt and water

30. bromothymol
blue (BTB)
do not change
-Ea/R
RCOOR

31. What is a coordinate covalent bond?
Making sigma bonds and holding lone pairs
Both electrons come from the same atom (just as good as a regular bond)
Unsaturated - addition (ex: decolorize bromine solution)
proton donor base

32. iodine - iodine solution - iodine vapor
Silvery gray solid - brown - purple
Hg²?
E=q + w (negative is by system - positive is on system)
Check for air bubbles in the buret and remove the buret funnel from the buret

33. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
The dilution effect when the solutions mix. M1V1 = M2V2
Purple
HClO4

34. Does Kw increase or decrease with T? Why?
voltaic: + electrolytic: -
acid + alcohol
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

35. bromine
brown volatile liquid
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Saturated - Substitution (which requires more radical conditions)
neutralization: high K - H2O product dissociation: low K - H2O reactant

36. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
CN?
left - ppt will form
Kc=Kp
Transition element compounds (except if it has a full or empty d shell)

37. Where are group I metals stored?
It ceases - the circuit is broken.
Group I metals (soft metals) are stored under oil
Orange
Hg²?

38. 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?
E=q + w (negative is by system - positive is on system)
water and substances with (s) less dense than
hydroxides (ex: Ba(OH)2)
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

39. 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
C2O4²?
The compound with the lowest Ksp value.
P2O5

40. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
It ceases - the circuit is broken.
basic
redox reaction
Time?¹ - (ex. s?¹ - hr?¹ - etc)

41. What is the slope of the graph of lnk vs. 1/T?
Sulfur
-Ea/R
by electrolysis
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

42. What do acids plus active metals form?
zero-th: decreases - first: constant - second: increases
HClO4
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
No - NH3 and HCl gases are extremely soluble

43. oxalate
C2O4²?
ClO?
White precipitate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

44. cyanide
a-IMFs - b-molecular volume
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Increases.
CN?

45. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
CrO4²?
CnH2n-2
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)

46. How do you clean a buret/pipette for a titration?
Heptane
Pipette (burette if need repetition)
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

47. What changes Keq?
Evaporation
Only temperature
Time?¹ - (ex. s?¹ - hr?¹ - etc)
ROH

48. A Bronsted-Lowry acid is...
ROH
The benzene ring (or more correctly the phenyl group - C6H5)
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
proton donor base

49. Why are noble gases stable?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Heptane
ClO2?
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

50. How are primary alcohols turned into acids?
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
No - NH3 and HCl gases are extremely soluble
RCOR
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)