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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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1. What are the signs for ?G and E° for spontaneous reactions?
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
?G= -ve - E°= +ve
SO4²?
Glacial acetic acid

2. Both Acetic acid and ____________ are also functional isomers.
methyl formate
same KE - but PEice<PEwater
'non-active' metals such as Cu - Ag - Au - Pt - etc.
red - green - blue

3. Alkanes are _________ and react by _________
Ksp = 4s³
Salt + water.
ion pairing
Saturated - Substitution (which requires more radical conditions)

4. What equipment do you need for a titration?
Ksp = s²
same KE - but PEice<PEwater
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
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.

5. What is the general formula for an acid?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
At half equivalence - pH=pKa
RCOOH
10?8

6. cyanide
CN?
Salt + water.
ClO2?
ns² electrons (first in-first out)

7. chlorate
ClO3?
are less dense than water
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
Suniverse increases for spontaneous processes

8. What causes the dramatic effect of T on rate?
an oxidized and reduced substance
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
T increases exponentially the proportion of molecules with E > Ea
different forms of the same element

9. carbonates
CN?
Insoluble except group 1 and ammonium
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Pale purple - (orange)-yellow - red - blue - green.

10. Esterification is...
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Ksp = 4s³
acid + alcohol
'non-active' metals such as Cu - Ag - Au - Pt - etc.

11. What apparatus do you use to separate 2 immiscible liquids?
S2O3²?
Separating funnel
Concentration
acids

12. lead iodide
bright yellow
ns² electrons (first in-first out)
P2O5
RCHO (carbonyl at end)

13. What reacts with an acid to create hydrogen gas?
ns² electrons (first in-first out)
T increases exponentially the proportion of molecules with E > Ea
An active metal.
Glowing splint (positive result=relights)

14. Does Kw increase or decrease with T? Why?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
0.10M HCl (more ions)
Heptane

15. What can form during the combustion of hydrocarbons in a limited supply of oxygen?
Selective absorption
Kc=Kp
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
CO (poisonous)

16. What part of a liquid do you look at to measure its volume?
Graduated cylinder
Greenish-yellow gas
Read the bottom of the meniscus
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

17. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Check for air bubbles in the buret and remove the buret funnel from the buret
a-IMFs - b-molecular volume
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Acid rain - dissolves marble buildings/statues and kills trees.

18. Aromatic compounds contain what?
C2O4²?
The benzene ring (or more correctly the phenyl group - C6H5)
Molecules with the same molecular formulas - but different structural formulas
Hg²?

19. What is the word equation for addition polymerisation?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
White precipitate
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
But S° of element is not zero (except at 0K)

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

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21. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
Exothermic (?H for ANY sa/sb = -57kJ/mol)
lighted splint (positive result=pop)
Combine the equations for the half reactions in the non-spontaneous direction

22. If Q < Ksp a ppt ______
#ligands=charge x2
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Ppt will NOT form (unsaturated)
Increases down group 1 decreases down group 17

23. How many faradays of electric charge do you need to produce one mole of O2? H2?
atoms
O2 needs 4F/mol H2 needs 2F/mol
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
proton acceptor.

24. Which alkali metals float on water?
Only temperature
All except for lithium
Evaporation
They stay the same.

25. oxalate
Exothermic
Experimental mass/theoretical mass X 100
C2O4²?
'non-active' metals such as Cu - Ag - Au - Pt - etc.

26. What is accuracy?
Unsaturated - addition (ex: decolorize bromine solution)
How close results are to the accepted value
#ligands=charge x2
ionic and form hydrogen and hydroxide

27. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
ClO3?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Soluble
Pale purple - (orange)-yellow - red - blue - green.

28. lead compounds
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
allow for the vapor pressure of water and make sure to level levels
Insoluble except nitrate and acetate
CH3COO?

29. phosphates
Ksp = s²
Group I metals (soft metals) are stored under oil
Most INsoluble except group 1 and ammonium
But S° of element is not zero (except at 0K)

30. How does the KE and PE of ice at 0°C compare to the KE and PE of water at 0°C?
Purple
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
same KE - but PEice<PEwater
-Ea/R

31. Neutralization is an ________ reaction.
Soluble except Ag - Pb - Ca - Sr Ba)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
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

32. acetates
NH4?
The Faraday or Faraday's constant.
RCOOH
Soluble

33. Lattice energy is high for ions with _____ size and _____ charge
small size and high charge
Tetrahedral
Pale yellow
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

34. What do you do to get rid of most of the solution from a precipitate?
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)
Decant
ClO3?
voltaic: + electrolytic: -

35. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
ROH
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Big K=kf/kr
Soluble

36. Name some properties of Group 17
CO2 and H2O
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Anode - oxygen. Cathode - hydrogen

37. What is the word equation for condensation polymerisation ?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Monomer + monomer = polymer product + a simple molecule such as water or HCl
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
Salt + water.

38. permanganate
non-metal oxides and hydrides are covalently bonded and are acidic.
ClO?
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
MnO4?

39. State whether K is high or low and whether H2O a product or reactant for the following reactions: a) neutralization. b) dissociation in water.
neutralization: high K - H2O product dissociation: low K - H2O reactant
R=8.31 J/mol/K
[A?]/[HA] x 100 or [BH?]/[B] x 100
Check for air bubbles in the buret and remove the buret funnel from the buret

40. What is the general formula for a ketone?
It ceases - the circuit is broken.
Conjugate pair (one must be a weak base or acid)
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)
RCOR

41. What is H2CO3 (carbonate acid) usually written as?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Ppt will NOT form (unsaturated)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
H2O + CO2 (it decomposes readily)

42. When the salt bridge is removed what happens to the cell reaction?
Soluble
Ksp = 4s³
It ceases - the circuit is broken.
left - ppt will form

43. Why are noble gases stable?
Orange
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
CnH(2n+2)
Exothermic

44. Which value of R do you use for all energy and kinetics calculations?
brown volatile liquid
R=8.31 J/mol/K
OH- and NH3
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

45. What is the formula of butane?
Glowing splint (positive result=relights)
C4H10
red - green - blue
do not change

46. What range of indicator would you use for the following titrations. a) s.a. + s.b. b) w.a. + s.b. c) w.b. + s.a.
boiling without losing volatile solvents/reactants
CO3²?
CnH2n-2
A) any range. b) 8-10 c) 4-6

47. What process do you use to obtain the precipitate from a solution?
Filtration
same KE - but PEice<PEwater
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Insoluble except group 1 and ammonium

48. Acidic gases like SO2 in the atmosphere cause what environmental problems?
Tetrahedral
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Acid rain - dissolves marble buildings/statues and kills trees.
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)

49. If ?S is positive - are the products more or less chaotic than the reactants?
brown volatile liquid
Tetrahedral
Increases.
More chaotic (ex: gases made)

50. chlorine
Greenish-yellow gas
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
voltaic: - electrolytic: +
Salts (ex: CaO + SO2 ? CaSO3)

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AP Chemistry 2

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