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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. chlorate
CO3²?
blue
ClO3?
a-IMFs - b-molecular volume

2. What are isotopes?
Check for air bubbles in the buret and remove the buret funnel from the buret
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
acid + alcohol
E=q + w (negative is by system - positive is on system)

3. How does half life change for zero-th order - first order - and second order processes?
Concentration
zero-th: decreases - first: constant - second: increases
No - it depends on the number of ions produced on dissolving.
Greenish-yellow gas

4. What do hydrocarbons form when they burn in air (oxygen)?
Group 1 hydroxides (ex: NaOH)
Molecules with the same molecular formulas - but different structural formulas
CO2 and H2O
The Faraday or Faraday's constant.

5. What is the formula for alkanes?
CnH2n+2
Pale yellow
H2PO4?
CO2 and H2O

6. When can supercooling occur? What does it look like on a cooling curve?

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7. Name six characteristics of transition elements (or their compounds)
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
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)
Molecules with the same molecular formulas - but different structural formulas
are less dense than water

8. Give an example of a concentrated weak acid.
10?8
Tetrahedral
Glacial acetic acid
CO (poisonous)

9. What is the relative solubility of CO2 - HCl - NH3 - NO2 - O2 - and SO2?
An active metal.
C2O4²?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Separating funnel

10. Is the freezing of ice endothermic or exothermic?
Exothermic
allow for the vapor pressure of water and make sure to level levels
Decant
O2 needs 4F/mol H2 needs 2F/mol

11. What is the difference between equivalence point and end point of a titration.
OH?
different forms of the same element
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
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)

12. What is the general formula for an acid?
a-IMFs - b-molecular volume
0.10M HCl (more ions)
Unsaturated - addition (ex: decolorize bromine solution)
RCOOH

13. Metal hydrides are _____ and form _______ and _______ when added to water
ionic and form hydrogen and hydroxide
-Ea/R
same KE - but PEice<PEwater
A) any range. b) 8-10 c) 4-6

14. A Bronsted-Lowry base is...
metal oxides and hydrides are ionically bonded and basic
strong acids/bases are written as H+ or OH- ions
proton acceptor.
They decrease (or could be the same if the solid has ONLY JUST disappeared)

15. Which alkali metals float on water?
neutralization: high K - H2O product dissociation: low K - H2O reactant
All except for lithium
A) any range. b) 8-10 c) 4-6
0.10M HCl (more ions)

16. ammonium
left - ppt will form
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Purple
NH4?

17. What gases usually come off during the 'electrolysis of water?' At the anode? At the cathode?
Anode - oxygen. Cathode - hydrogen
T increases exponentially the proportion of molecules with E > Ea
+4-covalent - +2-ionic
Trigonal pyramidal

18. What is the formula for obtaining charge flowing in a cell?
Q=It (time in seconds)
H+
voltaic: + electrolytic: -
bright yellow

19. nitrates
Soluble
ionic and form hydrogen and hydroxide
Anode - oxygen. Cathode - hydrogen
no - they're written undissociated (HAaq)

20. acetates
Ksp = 27s4
CN?
Silvery gray solid - brown - purple
Soluble

21. Generally - which oxy acid is strongest?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
The dilution effect when the solutions mix. M1V1 = M2V2
acids
The one with most oxygen atoms (highest oxidation number)

22. What is the general formula for an ester?
zero
Cu3(PO4)2
RCOOR
blue

23. mercury (I) ion
metal oxides and hydrides are ionically bonded and basic
Check for air bubbles in the buret and remove the buret funnel from the buret
Hg2²?
zero

24. What are isomers?
Molecules with the same molecular formulas - but different structural formulas
Ksp = 108s5
Most INsoluble except group 1 and ammonium
it is lower and occurs over less sharp a range

25. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
zero
RCOR
neutralization: high K - H2O product dissociation: low K - H2O reactant
do not change

26. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Tetrahedral
ClO3?
Ksp = 4s³
zero

27. What value of R do you use for thermo calculations? gas calculations?
S crystal at 0K=0
?G=negative - E° must be positive
Selective absorption
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K

28. What should you check for before you begin titrating?
Saturated - Substitution (which requires more radical conditions)
Check for air bubbles in the buret and remove the buret funnel from the buret
hydroxides (ex: Ba(OH)2)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

29. What does the solubility of organic compounds depend on?
CH3COO?
Heptane
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
HClO4

30. What are the units of the first order rate constant?
Acidified
A) any range. b) 8-10 c) 4-6
Time?¹ - (ex. s?¹ - hr?¹ - etc)
Graduated cylinder

31. How do you compute % dissociation?
H2PO4?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Disulfur dichloride
ROR

32. What is reflux?
H2PO4?
Hg2²?
Insoluble except group 1 and ammonium
boiling without losing volatile solvents/reactants

33. potassium permanganate
Purple
?H formation of an element in standard state=0
left - ppt will form
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.

34. What process do you use to obtain the solute from a solution?
Increases.
Evaporation
zero
an oxidized and reduced substance

35. What are amphoteric oxides?
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?)
linear
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
0 and 14

36. Name some properties of Group 17
ionic and form hydrogen and hydroxide
look for changes in oxidation # - the one that goes up is oxidized and is the RA
K1 x K2
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

37. What apparatus do you use to pour liquids?
Identity and purity (impure compounds usually have broad & low melting points)
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Pour liquids using a funnel or down a glass rod
metal oxides and hydrides are ionically bonded and basic

38. What is the general formula for an amine?
RNH2
Iodine and CO2 (dry ice)
Molecules with the same molecular formulas - but different structural formulas
Exothermic (?H for ANY sa/sb = -57kJ/mol)

39. What is the sign of the anode in voltaic cells? in electrolytic cells?
redox reaction
Ksp = 27s4
voltaic: - electrolytic: +
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

40. How does group 1 metals' density compare to water's?
?G=negative - E° must be positive
are less dense than water
Soluble
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?)

41. silver iodide
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Synthesis - separation and purification of the product and its identification.
ion pairing
Pale yellow

42. Where are group I metals stored?
boiling without losing volatile solvents/reactants
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Decant
Group I metals (soft metals) are stored under oil

43. What is the formula for percent yield?
Experimental mass/theoretical mass X 100
Ksp = 27s4
Soluble
it's lower and occurs over less sharp a range

44. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
ClO3?
H+
zero-th: decreases - first: constant - second: increases
do not change

45. phosphates
All except for lithium
SO4²?
Most INsoluble except group 1 and ammonium
How close results are to the accepted value

46. Colorless doesn't mean ______
Clear
Products - reactants (except for BDE when it's reactants - products)
Disulfur dichloride
ion pairing

47. What is the general formula for alkyl halides?
RX
The one with most oxygen atoms (highest oxidation number)
A) any range. b) 8-10 c) 4-6
CnH2n

48. What is the charge on a chlorine atom?
RCOOH
zero
They stay the same.
Check for air bubbles in the buret and remove the buret funnel from the buret

49. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Mn²? - Cr³? - Cr³
a-IMFs - b-molecular volume
C4H10
PO4³?

50. What do metal oxides plus acids form?
Insoluble
Salt + water
PO4³?
They decrease (or could be the same if the solid has ONLY JUST disappeared)

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AP Chemistry 2

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