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. Neutralization is an ________ reaction.
RNH2
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

2. Acids + Carbonates (bicarbonates) make?
+4-covalent - +2-ionic
Exothermic (?H for ANY sa/sb = -57kJ/mol)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Soluble except Ag - Pb - Ca - Sr Ba)

3. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
basic
different forms of the same element
proton acceptor.
Mn²? - Cr³? - Cr³

4. What is the conjugate acid of H2PO4?
H3PO4
Products - reactants (except for BDE when it's reactants - products)
hydroxides (ex: Ba(OH)2)
red - green - blue

5. Is a graduated cylinder or beaker more accurate?
?H-kJ - ?S-J - ?G-kJ
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
bright yellow
Graduated cylinder

6. What do nonmetal oxides plus water form?
water and substances with (s) less dense than
acids
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant
strong acids/bases are written as H+ or OH- ions

7. What changes Keq?
Only temperature
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Ionic compounds
CN?

8. What shape is methane?
Ppt will NOT form (unsaturated)
Tetrahedral
How grouped results are
10?8

9. What is the conjugate base of NH3?
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
RNH2
NH2?
hydroxides (ex: Ba(OH)2)

10. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
zero
The dilution effect when the solutions mix. M1V1 = M2V2
boiling without losing volatile solvents/reactants
Pale purple - (orange)-yellow - red - blue - green.

11. What is the slope of the graph of lnk vs. 1/T?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
PO4³?
-Ea/R
CnH(2n+2)

12. What measuring device would you use for very small volumes of liquids?
blue
Concentration
Pipette (burette if need repetition)
A) any range. b) 8-10 c) 4-6

13. What is the formula of butane?
small size and high charge
C4H10
Glacial acetic acid
Trigonal pyramidal

14. What do acids plus active metals form?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
water and substances with (s) less dense than
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
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)

15. When AB(s) and AC(s) are formed by adding A? ions to a mixture of 0.10M B? & 0.10M C? ions - which will precipitate first?
?H-kJ - ?S-J - ?G-kJ
H3PO4
The compound with the lowest Ksp value.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -

16. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
S crystal at 0K=0
ClO3?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
water and substances with (s) less dense than

17. How are metal oxides and hydrides bonded? are they acidic or basic?
bent
metal oxides and hydrides are ionically bonded and basic
H2O + CO2 (it decomposes readily)
The compound with the lowest Ksp value.

18. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Most are soluble except Ag - Pb
Reduction always takes place at the cathode (RED CAT) In both types of cell!
How close results are to the accepted value
hydroxides (ex: Ba(OH)2)

19. BaSO4
Insoluble
Both electrons come from the same atom (just as good as a regular bond)
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Big K=kf/kr

20. perchlorate
ClO4?
CO (poisonous)
?G= -ve - E°= +ve
Synthesis - separation and purification of the product and its identification.

21. What word is a clue for a redox reaction?
It ceases - the circuit is broken.
Acidified
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
Insoluble

22. What part of a liquid do you look at to measure its volume?
ion pairing
Most are soluble except Ag - Pb
Insoluble
Read the bottom of the meniscus

23. hydroxide
Salts (ex: CaO + SO2 ? CaSO3)
Sigma bonds are stronger than pi bonds
OH?
Identity and purity (impure compounds usually have broad & low melting points)

24. How does group 1 metals' density compare to water's?
Increases.
How close results are to the accepted value
ns² electrons (first in-first out)
are less dense than water

25. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
a-IMFs - b-molecular volume
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
Glacial acetic acid

26. Lattice energy is high for ions with _____ size and _____ charge
All except for lithium
CnH2n+1 often designated 'R' ex C3H7 is propyl
small size and high charge
are less dense than water

27. What is the formula for alkynes?
RCOR
chemically (ex: with carbon)
More chaotic (ex: gases made)
CnH2n-2

28. barium sulfate
ClO4?
Current - time and charge on ion (moles of e used in half cell reaction)
do not change
White precipitate

29. oxalate
SO4²?
Tetrahedral
C2O4²?
Identity and purity (impure compounds usually have broad & low melting points)

30. ammonium/ammonium compounds
Soluble
Separating funnel
Orange
Identity and purity (impure compounds usually have broad & low melting points)

31. What happens to the ion concentrations of a saturated solution when it is diluted and no solid solute remains?
Evaporation
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Concentration
They decrease (or could be the same if the solid has ONLY JUST disappeared)

32. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Anode - oxygen. Cathode - hydrogen
Cr2O7²?

33. chlorine
Greenish-yellow gas
zero-th: decreases - first: constant - second: increases
Filtration
Synthetic condensation polymer (aka a polyamide)

34. What is the pH of 1.0M HCl? 1M NaOH?
Kc=Kp
0 and 14
do not change
Eudiometer

35. What is the test for oxygen?
bent
Glowing splint (positive result=relights)
Soluble
How grouped results are

36. A Bronsted-Lowry base is...
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
ns² electrons (first in-first out)
Soluble
proton acceptor.

37. What is precision?
[A?]/[HA] x 100 or [BH?]/[B] x 100
How grouped results are
yellow
hydroxides (ex: Ba(OH)2)

38. 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

39. Alcohols and _______ are FG isomers
Greenish-yellow gas
bases
proton donor base
ethers

40. Buffer capacity must contain decent amounts of a ________ ________
Big K=kf/kr
P2O5
blue glass - it filters UV
Conjugate pair (one must be a weak base or acid)

41. What variables effect the moles of substance liberated in electrolysis. (a.k.a. Faraday's Laws)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
non-metal oxides and hydrides are covalently bonded and are acidic.
proton acceptor.
Current - time and charge on ion (moles of e used in half cell reaction)

42. What reacts with an acid to create hydrogen gas?
An active metal.
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Salt and water
Soluble

43. How do you compute % dissociation?
0 and 14
Group I metals (soft metals) are stored under oil
[A?]/[HA] x 100 or [BH?]/[B] x 100
Tetrahedral

44. What is the basic structure of an optical isomer?
Salt and water
are less dense than water
Pale purple - (orange)-yellow - red - blue - green.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.

45. What do you use to look at burning magnesium? why?
strong acids/bases are written as H+ or OH- ions
it reacts by substitution NOT addition
HClO4
blue glass - it filters UV

46. What is the sign of the anode in voltaic cells? in electrolytic cells?
Ionic compounds
ion pairing
E=q + w (negative is by system - positive is on system)
voltaic: - electrolytic: +

47. primary colors
NH4?
red - green - blue
it is lower and occurs over less sharp a range
S crystal at 0K=0

48. What is the general formula for alkyl halides?
RX
Salt + water.
Graduated cylinder
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus

49. What causes the dramatic effect of T on rate?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
different forms of the same element
T increases exponentially the proportion of molecules with E > Ea
do not change

50. halides
CnH2n+2
Most are soluble except Ag - Pb
bright yellow
Most INsoluble except group 1 and ammonium