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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. ammonium
Identity and purity (impure compounds usually have broad & low melting points)
Ksp = 4s
Making sigma bonds and holding lone pairs
NH4?

2. A geometric (or cis-trans) isomer exists due to.....
water and substances with (s) less dense than
Insoluble except group 1 and ammonium
ClO3?
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)

3. copper sulfate
Suniverse increases for spontaneous processes
C4H10
water and substances with (s) less dense than
blue

4. What are the formulas for q?
The dilution effect when the solutions mix. M1V1 = M2V2
q=mc?T q=mL (or n x ?h)
Disulfur dichloride
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

5. What is the formula for alkanes?
Orange
non-metal oxides and hydrides are covalently bonded and are acidic.
yellow
CnH2n+2

6. What apparatus do you use to separate 2 immiscible liquids?
Separating funnel
allow for the vapor pressure of water and make sure to level levels
Glacial acetic acid
Salts (ex: CaO + SO2 ? CaSO3)

7. When combining half equations - what do you do to E values when multiplying coefficients?
Insoluble
CO (poisonous)
#ligands=charge x2
Nothing

8. What equipment do you need for a titration?
MnO4?
Orange
benzene is less reactive than alkenes
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

9. chlorite
Ions go through the salt bridge - electrons go through metal wires in the external circuit
ClO2?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
lighted splint (positive result=pop)

10. What process do you use to obtain the solute from a solution?
Purple
Evaporation
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
zero-th: decreases - first: constant - second: increases

11. BaSO4
bright yellow
'non-active' metals such as Cu - Ag - Au - Pt - etc.
Insoluble
Orange

12. chromate ion (soln + most solids)
ClO4?
yellow
Iodine and CO2 (dry ice)
bright yellow

13. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
The Faraday or Faraday's constant.
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Salts (ex: CaO + SO2 ? CaSO3)

14. acetate
Soluble
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
CH3COO?
Identity and purity (impure compounds usually have broad & low melting points)

15. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Filtration

16. mercury (II) ion
No - it depends on the number of ions produced on dissolving.
Hg?
red - green - blue
NH2?

17. What are the units of the first order rate constant?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
q=mc?T q=mL (or n x ?h)
Time? - (ex. s? - hr? - etc)
voltaic: + electrolytic: -

18. ________ are Lewis bases - because they can donate a lone pair of electrons.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
OH- and NH3
Transition element compounds (except if it has a full or empty d shell)
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.

19. What is the general formula for an aldehyde?
They stay the same.
small size and high charge
RCHO (carbonyl at end)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

20. Alkanes are _________ and react by _________
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
NH4?
Saturated - Substitution (which requires more radical conditions)
yellow

21. What process do you use to separate two liquids with different boiling points?
fractional distillation
Iodine and CO2 (dry ice)
Saturated - Substitution (which requires more radical conditions)
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

22. Name C7H16
K1 x K2
Heptane
Synthetic condensation polymer (aka a polyamide)
Check for air bubbles in the buret and remove the buret funnel from the buret

23. What steps do organic labs consist of?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
zero
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Synthesis - separation and purification of the product and its identification.

24. How are non-metal oxides and hydrides bonded? are they acidic or basic?
R=8.31 J/mol/K
Sigma bonds are stronger than pi bonds
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
non-metal oxides and hydrides are covalently bonded and are acidic.

25. What type of compounds do metals/non metals form?
0.10M HCl (more ions)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
bases
Ionic compounds

26. Which value of R do you use for all energy and kinetics calculations?
Eudiometer
R=8.31 J/mol/K
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)
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)

27. nitrates
Orange
zero-th: decreases - first: constant - second: increases
Soluble
HClO4

28. What things should you remember to do when collecting gas over water?
acid + alcohol
allow for the vapor pressure of water and make sure to level levels
OH?
ROR

29. What causes the dramatic effect of T on rate?
S2O3?
T increases exponentially the proportion of molecules with E > Ea
RCHO (carbonyl at end)
ClO?

30. ammonium/ammonium compounds
CrO4?
Silvery gray solid - brown - purple
Soluble
The one with most oxygen atoms (highest oxidation number)

31. potassium permanganate
Hydrogen (active metals are metals with more negative reduction potentials in E chart)
different forms of the same element
Purple
Molecules with the same molecular formulas - but different structural formulas

32. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
strong acids/bases are written as H+ or OH- ions
4 sigma bonds-109 - sp - one double bond-120 - sp two double bonds-180 - sp one triple bond-180 - sp
ns electrons (first in-first out)

33. What is the general formula of an alkane?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Pale purple - (orange)-yellow - red - blue - green.
CnH(2n+2)
Read the bottom of the meniscus

34. halides
Most are soluble except Ag - Pb
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
non-metal oxides and hydrides are covalently bonded and are acidic.
ns electrons (first in-first out)

35. bromothymol
RCOR
ion pairing
an oxidized and reduced substance
blue (BTB)

36. lead iodide
ion pairing
proton donor base
bright yellow
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

37. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
H2O + CO2 (it decomposes readily)
methyl formate
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)
water and substances with (s) less dense than

38. What is the basic structure of an optical isomer?
P2O5
ion pairing
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

39. What is accuracy?
Pipette (burette if need repetition)
How close results are to the accepted value
HClO4
How grouped results are

40. carbonates
Insoluble except group 1 and ammonium
ionic and form hydrogen and hydroxide
|experimental - accepted|/accepted X 100
Silvery gray solid - brown - purple

41. What part of a liquid do you look at to measure its volume?
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Read the bottom of the meniscus
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

42. Which of the rates changes more when temperature is increased?
Unsaturated - addition (ex: decolorize bromine solution)
Read the bottom of the meniscus
Salts (ex: CaO + SO2 ? CaSO3)
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

43. How do you clean a buret/pipette for a titration?
no - they're written undissociated (HAaq)
Initiation energy (NOT 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.
it reacts by substitution NOT addition

44. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
different forms of the same element
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
H+
Big K=kf/kr

45. How does benzene compare in reactivity to alkenes?
benzene is less reactive than alkenes
Acids; HCOOCH3 is an ester
Heptane
allow for the vapor pressure of water and make sure to level levels

46. What is the general formula for an acid?
ion pairing
Soluble
RCOOH
Pipette (burette if need repetition)

47. dihydrogen phosphate
it is lower and occurs over less sharp a range
H2O + CO2 (it decomposes readily)
Heptane
H2PO4?

48. When can supercooling occur? What does it look like on a cooling curve?
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)
Separating funnel
C4H10

49. How can metals like iron and zinc be reduced?
chemically (ex: with carbon)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
ClO4?
CH3COO?

50. How are more active metals reduced?
different forms of the same element
A) any range. b) 8-10 c) 4-6
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
by electrolysis

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