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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.
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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 do nonmetal oxides plus water form?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
'non-active' metals such as Cu - Ag - Au - Pt - etc.
acids
allow for the vapor pressure of water and make sure to level levels

2. How are metal oxides and hydrides bonded? are they acidic or basic?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
an oxidized and reduced substance
metal oxides and hydrides are ionically bonded and basic
How close results are to the accepted value

3. What is the formula for obtaining charge flowing in a cell?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
PO4³?
Q=It (time in seconds)
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)

4. What causes the dramatic effect of T on rate?
bases
T increases exponentially the proportion of molecules with E > Ea
No - NH3 and HCl gases are extremely soluble
Group 1 hydroxides (ex: NaOH)

5. Why are noble gases stable?
S2O3²?
Increases down group 1 decreases down group 17
Big K=kf/kr
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

6. What is the second law of thermodynamics?
The Faraday or Faraday's constant.
Insoluble
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Suniverse increases for spontaneous processes

7. What is the energy you must put into a reaction to make it start called?
no - they're written undissociated (HAaq)
Initiation energy (NOT Ea)
zero-th: decreases - first: constant - second: increases
P2O5

8. Where are group I metals stored?
Group I metals (soft metals) are stored under oil
small size and high charge
OH- and NH3
All except for lithium

9. What is the formula for alkynes?
chemically (ex: with carbon)
RCHO (carbonyl at end)
voltaic: + electrolytic: -
CnH2n-2

10. How do you heat a test tube?
OH?
Heat a test tube at an angle at the side of the tube (not bottom)
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?)
Acids; HCOOCH3 is an ester

11. Is the ?H formation of an element in standard state zero?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Most are soluble except Ag - Pb
?H formation of an element in standard state=0
Synthesis - separation and purification of the product and its identification.

12. dihydrogen phosphate
S2O3²?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
E=q + w (negative is by system - positive is on system)
H2PO4?

13. How do you explain trends in atomic properties using Coulomb's Law?
Making sigma bonds and holding lone pairs
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
Sulfur
ClO4?

14. dichromate (soln + most solids)
P2O5
Orange
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Trigonal pyramidal

15. What shape is ammonia?
an oxidized and reduced substance
Trigonal pyramidal
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.

16. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
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.
bright yellow
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

17. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
Current - time and charge on ion (moles of e used in half cell reaction)
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
look for changes in oxidation # - the one that goes up is oxidized and is the RA

18. Which would cause the bulb in a conductivity apparatus to be brightest?
ethers
P2O5
H3PO4
0.10M HCl (more ions)

19. What type of compounds do metals/non metals form?
Soluble
|experimental - accepted|/accepted X 100
basic
Ionic compounds

20. What are the signs for ?G and E° for spontaneous reactions?
?G= -ve - E°= +ve
neutralization: high K - H2O product dissociation: low K - H2O reactant
0.10M HCl (more ions)
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

21. What are the products of the reaction between group 1 metals and water?

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22. Color is due to ______ _______ of light.
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.
Big K=kf/kr
Selective absorption
bright yellow

23. chlorite
?H formation of an element in standard state=0
The compound with the lowest Ksp value.
Q=It (time in seconds)
ClO2?

24. silver compounds
White precipitate
K2
Insoluble except for nitrate and acetate
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

25. What is the formula for percent error?
Salt + water.
RCOOR
water and substances with (s) less dense than
|experimental - accepted|/accepted X 100

26. Name some properties of Group 17
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
A salt solution.
atoms
RCOOR

27. How can metals like iron and zinc be reduced?
RCOOH
?G= -ve - E°= +ve
chemically (ex: with carbon)
Acids; HCOOCH3 is an ester

28. copper sulfate
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.
left - ppt will form
blue
Sigma bonds are stronger than pi bonds

29. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
same KE - but PEice<PEwater

30. What effect does increasing the size/surface area of a voltaic cell have on the cell?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
CH3COO?
0.10M HCl (more ions)
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?)

31. What type of compounds are almost always colored?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
Transition element compounds (except if it has a full or empty d shell)
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
CO (poisonous)

32. phosphates
Acids; HCOOCH3 is an ester
Greenish-yellow gas
Increases down group 1 decreases down group 17
Most INsoluble except group 1 and ammonium

33. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
a-IMFs - b-molecular volume
brown volatile liquid
ClO?

34. What does the solubility of organic compounds depend on?
do not change
Acids; HCOOCH3 is an ester
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
How close results are to the accepted value

35. carbonate
acid + alcohol
CO3²?
#ligands=charge x2
proton donor base

36. What word is a clue for a redox reaction?
Salts (ex: CaO + SO2 ? CaSO3)
Acidified
ns² electrons (first in-first out)
CO3²?

37. sulfate
SO4²?
Decant
boiling without losing volatile solvents/reactants
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

38. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Nothing
Read the bottom of the meniscus
T increases exponentially the proportion of molecules with E > Ea
No - it depends on the number of ions produced on dissolving.

39. What are isotopes?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
CO3²?
Purple
same KE - but PEice<PEwater

40. What is the difference between equivalence point and end point of a titration.
Experimental mass/theoretical mass X 100
yellow
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
Heptane

41. What are isomers?
?G= -ve - E°= +ve
HClO4
Making sigma bonds and holding lone pairs
Molecules with the same molecular formulas - but different structural formulas

42. If Q > Ksp - then system shifts _______ and ppt ______
Sigma bonds are stronger than pi bonds
left - ppt will form
Group 1 hydroxides (ex: NaOH)
NH2?

43. dichromate
Cr2O7²?
Ksp = 108s5
strong acids/bases are written as H+ or OH- ions
PO4³?

44. lead iodide
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
bright yellow
Current - time and charge on ion (moles of e used in half cell reaction)
White precipitate

45. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
Only temperature
Concentration
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

46. What is the general formula for an ether?
CnH2n+1 often designated 'R' ex C3H7 is propyl
ROR
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
same KE - but PEice<PEwater

47. How does group 1 metals' density compare to water's?
are less dense than water
?G= -ve - E°= +ve
acid + alcohol
CN?

48. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
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
Transition element compounds (except if it has a full or empty d shell)
All except for lithium
Insoluble except group 1 and ammonium

49. perchlorate
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
ClO4?
same KE - but PEice<PEwater
voltaic: - electrolytic: +

50. What is the general formula for an ester?
S crystal at 0K=0
RCOOR
Experimental mass/theoretical mass X 100
RCOR

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AP Chemistry 2

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