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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. 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
Ksp = 27s4
NO3?
Combine the equations for the half reactions in the non-spontaneous direction

2. What part of a liquid do you look at to measure its volume?
Read the bottom of the meniscus
A) any range. b) 8-10 c) 4-6
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
RCOOR

3. What is precision?
Transition element compounds (except if it has a full or empty d shell)
small size and high charge
How grouped results are
Soluble

4. What is the charge on a chlorine atom?
ROH
A salt solution.
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
zero

5. When the salt bridge is removed what happens to the cell reaction?
Decant
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
Disulfur dichloride
It ceases - the circuit is broken.

6. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Suniverse increases for spontaneous processes
Acid rain - dissolves marble buildings/statues and kills trees.
No - it depends on the number of ions produced on dissolving.

7. How are primary alcohols turned into acids?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CnH2n-2
OH?

8. acetate
CH3COO?
OH?
Transition element compounds (except if it has a full or empty d shell)
do not change

9. How do you heat a test tube?
chemically (ex: with carbon)
Heat a test tube at an angle at the side of the tube (not bottom)
zero-th: decreases - first: constant - second: increases
NH2?

10. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
linear
Perform ICE BOX calculation based on K1
do not change

11. What is the basic structure of an optical isomer?
a-IMFs - b-molecular volume
Insoluble except for nitrate and acetate
fruit - fish - bases
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

12. What is the formula of copper (II) phosphate?
Cu3(PO4)2
ClO4?
The one with most oxygen atoms (highest oxidation number)
acid + alcohol

13. bromine
zero-th: decreases - first: constant - second: increases
brown volatile liquid
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

14. What is the formula for alkynes?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CnH2n-2
ROR
strong acids/bases are written as H+ or OH- ions

15. What shape is water?
Identity and purity (impure compounds usually have broad & low melting points)
Clear
No - it depends on the number of ions produced on dissolving.
bent

16. What apparatus do you use to separate 2 immiscible liquids?
q=mc?T q=mL (or n x ?h)
Group I metals (soft metals) are stored under oil
Separating funnel
Purple

17. What type of solutions do small - highly charged cations tend to form?
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
No - it depends on the number of ions produced on dissolving.
CnH2n
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)

18. What is the pH of 1.0M HCl? 1M NaOH?
Read the bottom of the meniscus
Heptane
0 and 14
Acid rain - dissolves marble buildings/statues and kills trees.

19. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Big K=kf/kr
The benzene ring (or more correctly the phenyl group - C6H5)
The dilution effect when the solutions mix. M1V1 = M2V2
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

20. Color is due to ______ _______ of light.
Selective absorption
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
OH?

21. mercury (I) ion
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Hg2²?
CO (poisonous)
Trigonal pyramidal

22. How do you find the pH for a dibasic acid? (H2A)?
voltaic: + electrolytic: -
Ksp = s²
Perform ICE BOX calculation based on K1
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

23. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Acid rain - dissolves marble buildings/statues and kills trees.
Suniverse increases for spontaneous processes
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
White precipitate

24. Do you use J or kJ for ?H - ?S - and ?G?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Disulfur dichloride
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
?H-kJ - ?S-J - ?G-kJ

25. What is the general formula for an amine?
-Ea/R
CnH2n-2
HClO4
RNH2

26. What process do you use to obtain the precipitate from a solution?
Greenish-yellow gas
Clear
Filtration
Ksp = 4s³

27. barium sulfate
White precipitate
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Soluble
Monomer + monomer = polymer product + a simple molecule such as water or HCl

28. What do group I/II metal oxides and acids form?
Salt and water
Concentration
by electrolysis
Iodine and CO2 (dry ice)

29. What value of R do you use for thermo calculations? gas calculations?
CO3²?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Only temperature

30. 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?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Disulfur dichloride
NO3?
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

31. What things should you remember to do when collecting gas over water?
Exothermic (?H for ANY sa/sb = -57kJ/mol)
HClO4
zero
allow for the vapor pressure of water and make sure to level levels

32. What is the relationship in strength between sigma and pi bonds?
Sigma bonds are stronger than pi bonds
Insoluble (except group 1 ammonium and Ba)
voltaic: - electrolytic: +
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

33. What do nonmetal oxides plus water form?
acids
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
CnH2n-2
The one with most oxygen atoms (highest oxidation number)

34. ________ are Lewis bases - because they can donate a lone pair of electrons.
Combine the equations for the half reactions in the non-spontaneous direction
Pipette (burette if need repetition)
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
OH- and NH3

35. What is the formula for alkanes?
yellow
CnH2n+2
ethers
Salt and water

36. iodine - iodine solution - iodine vapor
Ppt will NOT form (unsaturated)
Selective absorption
Silvery gray solid - brown - purple
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

37. ammonium
NO3?
CO (poisonous)
NH4?
Heptane

38. What is the energy you must put into a reaction to make it start called?
Identity and purity (impure compounds usually have broad & low melting points)
Initiation energy (NOT Ea)
CrO4²?
Salt + water.

39. How are metal oxides and hydrides bonded? are they acidic or basic?
basic
Synthesis - separation and purification of the product and its identification.
Synthetic condensation polymer (aka a polyamide)
metal oxides and hydrides are ionically bonded and basic

40. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Purple
Ksp = s²
More chaotic (ex: gases made)

41. What word is a clue for a redox reaction?
Mn²? - Cr³? - Cr³
Acidified
An active metal.
a-IMFs - b-molecular volume

42. What is the sign of the anode in voltaic cells? in electrolytic cells?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
voltaic: - electrolytic: +
Insoluble
HClO4

43. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
Suniverse increases for spontaneous processes
acids
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

44. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
+4-covalent - +2-ionic
Combine the equations for the half reactions in the non-spontaneous direction
RCHO (carbonyl at end)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

45. What element is used to vulcanize rubber?
Pale purple - (orange)-yellow - red - blue - green.
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
fruit - fish - bases
Sulfur

46. What is the formula of butane?
H2PO4?
Anode
C4H10
How grouped results are

47. How does the melting point of a mixture compare to the MP of a pure substance?

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48. Alkenes are ________ and react by __________
H2PO4?
Unsaturated - addition (ex: decolorize bromine solution)
HClO4
RX

49. carbonate
-Ea/R
CO3²?
Soluble
'non-active' metals such as Cu - Ag - Au - Pt - etc.

50. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
different forms of the same element
it reacts by substitution NOT addition
Molecules with the same molecular formulas - but different structural formulas
Pale purple - (orange)-yellow - red - blue - green.

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AP Chemistry 2

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