Test your basic knowledge |

AP Chemistry 2

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
bent
Separating funnel
The one with most oxygen atoms (highest oxidation number)

2. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Perform ICE BOX calculation based on K1
Only temperature
water and substances with (s) less dense than
same KE - but PEice<PEwater

3. Do anions flow to the cathode or anode?
[A?]/[HA] x 100 or [BH?]/[B] x 100
Anode
zero
Transition element compounds (except if it has a full or empty d shell)

4. What process do you use to obtain the solute from a solution?
Evaporation
Salt + water
OH?
How grouped results are

5. halides
Most are soluble except Ag - Pb
NO3?
Sulfur
Group I metals (soft metals) are stored under oil

6. nitrates
Soluble
a-IMFs - b-molecular volume
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
an oxidized and reduced substance

7. What do you use for an acid spill? base spill?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
CO3²?
Heptane
bright yellow

8. What is the third law of thermodynamics?
Pale purple - (orange)-yellow - red - blue - green.
Ppt will NOT form (unsaturated)
S crystal at 0K=0
Synthesis - separation and purification of the product and its identification.

9. What is the general formula for an amine?
SO4²?
Greenish-yellow gas
RNH2
?G= -ve - E°= +ve

10. How many normal boiling points and boiling points are there?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

11. mercury (II) ion
ClO4?
Hg²?
S2O3²?
OH?

12. What process do you use to obtain the precipitate from a solution?
proton acceptor.
Filtration
allow for the vapor pressure of water and make sure to level levels
RCOOH

13. What is the general formula for an ester?
RCOOR
Silvery gray solid - brown - purple
Increases down group 1 decreases down group 17
Graduated cylinder

14. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
non-metal oxides and hydrides are covalently bonded and are acidic.
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Increases down group 1 decreases down group 17

15. What do hydrocarbons form when they burn in air (oxygen)?
voltaic: + electrolytic: -
CO2 and H2O
NH4?
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.

16. Both Acetic acid and ____________ are also functional isomers.
methyl formate
Synthesis - separation and purification of the product and its identification.
Pour liquids using a funnel or down a glass rod
Unsaturated - addition (ex: decolorize bromine solution)

17. dichromate
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
+4-covalent - +2-ionic
it is lower and occurs over less sharp a range
Cr2O7²?

18. What is the formula for alkynes?
CnH2n-2
10?8
Tetrahedral
Disulfur dichloride

19. acetates
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
small size and high charge
Soluble
are less dense than water

20. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
CH3COO?
Pipette (burette if need repetition)
Pale yellow

21. What does the solubility of organic compounds depend on?
RCOOH
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Acid rain - dissolves marble buildings/statues and kills trees.
different forms of the same element

22. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
Only temperature
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
An active metal.

23. What do nonmetal oxides plus water form?
Group 1 hydroxides (ex: NaOH)
CH3COO?
Saturated - Substitution (which requires more radical conditions)
acids

24. Neutralization is an ________ reaction.
metal oxides and hydrides are ionically bonded and basic
NO3?
yellow
Exothermic (?H for ANY sa/sb = -57kJ/mol)

25. Does reactivity increase/decrease going down group 1 and group 17?
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)
Increases down group 1 decreases down group 17
proton acceptor.
CnH2n-2

26. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
blue glass - it filters UV
The dilution effect when the solutions mix. M1V1 = M2V2
ClO3?
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

27. What two compounds are great oxidizing agents?

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

28. Do you use J or kJ for ?H - ?S - and ?G?
?H-kJ - ?S-J - ?G-kJ
White precipitate
Hg2²?
S2O3²?

29. Esterification is...
Hg2²?
acid + alcohol
RCOR
zero

30. What is the formula of copper (II) phosphate?
But S° of element is not zero (except at 0K)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
CN?
Cu3(PO4)2

31. Acids + Carbonates (bicarbonates) make?
zero-th: decreases - first: constant - second: increases
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
#ligands=charge x2
non-metal oxides and hydrides are covalently bonded and are acidic.

32. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
-Ea/R
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
NH2?
Ksp = 27s4

33. 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)
K2
linear
Trigonal pyramidal

34. What part of a liquid do you look at to measure its volume?
ClO3?
NO3?
Read the bottom of the meniscus
SO4²?

35. Is the ?H formation of an element in standard state zero?
?H formation of an element in standard state=0
RCOR
-Ea/R
Greenish-yellow gas

36. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
RCOOH
Hg²?
CO (poisonous)
ethers

37. When the salt bridge is removed what happens to the cell reaction?
10?8
S crystal at 0K=0
It ceases - the circuit is broken.
Orange

38. acetate
CH3COO?
Separating funnel
Molecules with the same molecular formulas - but different structural formulas
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)

39. What is the conjugate acid of H2PO4?
CnH2n+2
proton donor base
H3PO4
The compound with the lowest Ksp value.

40. What process do you use to obtain a solvent from a solution?
Distillation
Ions go through the salt bridge - electrons go through metal wires in the external circuit
H3PO4
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

41. What is accuracy?
Silvery gray solid - brown - purple
MnO4?
Glowing splint (positive result=relights)
How close results are to the accepted value

42. How does half life change for zero-th order - first order - and second order processes?
zero-th: decreases - first: constant - second: increases
RCOR
CnH2n+1 often designated 'R' ex C3H7 is propyl
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

43. Why are noble gases stable?
Eudiometer
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

44. What is the sign of the anode in voltaic cells? in electrolytic cells?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Initiation energy (NOT Ea)
voltaic: - electrolytic: +
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

45. What is the formula for percent yield?
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Experimental mass/theoretical mass X 100
Add acid to water so that the acid doesn't boil and spit
ionic and form hydrogen and hydroxide

46. What steps do organic labs consist of?
Combine the equations for the half reactions in the non-spontaneous direction
Synthetic condensation polymer (aka a polyamide)
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Synthesis - separation and purification of the product and its identification.

47. What type of solutions do small - highly charged cations tend to form?
basic
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Most INsoluble except group 1 and ammonium
The Faraday or Faraday's constant.

48. What is the formula for obtaining charge flowing in a cell?
Salts (ex: CaO + SO2 ? CaSO3)
Q=It (time in seconds)
+4-covalent - +2-ionic
Synthetic condensation polymer (aka a polyamide)

49. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
same KE - but PEice<PEwater
Salt + water
H3PO4

50. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
CO2 and H2O
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Read the bottom of the meniscus
neutralization: high K - H2O product dissociation: low K - H2O reactant