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AP Chemistry 2

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Answer 50 questions in 15 minutes.
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1. What do metal oxides plus acids form?
CnH2n
Kc=Kp
Insoluble except group 1 and ammonium
Salt + water

2. Give an example of a concentrated weak acid.
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Glacial acetic acid
Tetrahedral

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

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4. ammonium
NH4?
CnH2n+2
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
Most INsoluble except group 1 and ammonium

5. What things should you remember to do when collecting gas over water?
allow for the vapor pressure of water and make sure to level levels
proton acceptor.
ethers
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

6. What do nonmetal oxides plus water form?
atoms
acids
Silvery gray solid - brown - purple
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?)

7. Color (absorbance) is proportional to ________
Soluble
Concentration
Soluble
Insoluble except for nitrate and acetate

8. What do ions and electrons travel through in a voltaic/electrolytic cell?
Sulfur
Distillation
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Ksp = 27s4

9. What happens to the ion concentrations of a saturated solution when it is diluted and allowed to reach equilibrium - with solid solute still present?
acid + alcohol
They stay the same.
CnH2n-2
non-metal oxides and hydrides are covalently bonded and are acidic.

10. When a cell is 'flat' What is its voltage?
it is lower and occurs over less sharp a range
Exothermic
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
zero

11. 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?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
redox reaction
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
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

12. To decide if a ppt forms when solutions are mixed - what is the first thing you have to remember?
allow for the vapor pressure of water and make sure to level levels
Pour liquids using a funnel or down a glass rod
Evaporation
The dilution effect when the solutions mix. M1V1 = M2V2

13. What are the formulas for q?
bent
q=mc?T q=mL (or n x ?h)
Insoluble except for nitrate and acetate
The dilution effect when the solutions mix. M1V1 = M2V2

14. What is the relationship in strength between sigma and pi bonds?
bright yellow
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)
Cu3(PO4)2
Sigma bonds are stronger than pi bonds

15. What are two substances that sublime at 1 atm when heated?
red - green - blue
RCHO (carbonyl at end)
It ceases - the circuit is broken.
Iodine and CO2 (dry ice)

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

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17. What is the test for hydrogen?
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)
Most are soluble except Ag - Pb
lighted splint (positive result=pop)
RCOOR

18. chlorate
ClO3?
it's lower and occurs over less sharp a range
Ignore 'x' if its K is very small compared to [reactant] (5% rule)
Salts (ex: CaO + SO2 ? CaSO3)

19. Buffer capacity must contain decent amounts of a ________ ________
Suniverse increases for spontaneous processes
brown volatile liquid
Disulfur dichloride
Conjugate pair (one must be a weak base or acid)

20. bromine
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
brown volatile liquid
ion pairing
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask

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

22. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
neutralization: high K - H2O product dissociation: low K - H2O reactant
Hg2²?
Glowing splint (positive result=relights)

23. What is accuracy?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
How close results are to the accepted value
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Sigma bonds are stronger than pi bonds

24. What are the names and formulas of the 6 strong acids?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Orange
RX

25. What do the 'a' and 'b' in Van Der Waal's equation allow for?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
a-IMFs - b-molecular volume
Pour liquids using a funnel or down a glass rod
H2O + CO2 (it decomposes readily)

26. hydroxides
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Orange
Insoluble (except group 1 ammonium and Ba)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

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

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28. Neutralization is an ________ reaction.
Perform ICE BOX calculation based on K1
Exothermic (?H for ANY sa/sb = -57kJ/mol)
ClO?
PO4³?

29. Can you collect soluble gases over water?
OH?
Add acid to water so that the acid doesn't boil and spit
No - NH3 and HCl gases are extremely soluble
ClO?

30. What kind of bonding structure does benzene have?
benzene has a delocalized pi ring structure
Selective absorption
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Molecules with the same molecular formulas - but different structural formulas

31. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
ethers
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
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
Trigonal pyramidal

32. What is the general formula for an amine?
Group 1 hydroxides (ex: NaOH)
RNH2
OH?
Time?¹ - (ex. s?¹ - hr?¹ - etc)

33. What is Ksp in terms of molar solubility ('s') for an electrolyte AB?
are less dense than water
Glacial acetic acid
Ksp = s²
Acid rain - dissolves marble buildings/statues and kills trees.

34. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
How grouped results are
ionic and form hydrogen and hydroxide
Monomer + monomer = polymer product + a simple molecule such as water or HCl

35. How does benzene compare in reactivity to alkenes?
OH?
T increases exponentially the proportion of molecules with E > Ea
benzene is less reactive than alkenes
Insoluble

36. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Making sigma bonds and holding lone pairs
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Purple
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)

37. What complex ion does ammonia form with silver? copper? cadmium? zinc?
Molecules with the same molecular formulas - but different structural formulas
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Products - reactants (except for BDE when it's reactants - products)
An active metal.

38. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
H2O + CO2 (it decomposes readily)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
P2O5
zero

39. Generally - which oxy acid is strongest?
NH2?
The one with most oxygen atoms (highest oxidation number)
Silvery gray solid - brown - purple
Big K=kf/kr

40. What is the general formula for an ester?
Soluble
The compound with the lowest Ksp value.
Cr2O7²?
RCOOR

41. How does group 1 metals' density compare to water's?
are less dense than water
White precipitate
More chaotic (ex: gases made)
Current - time and charge on ion (moles of e used in half cell reaction)

42. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Soluble except Ag - Pb - Ca - Sr Ba)
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Glowing splint (positive result=relights)

43. How do you heat a test tube?
allow for the vapor pressure of water and make sure to level levels
Glowing splint (positive result=relights)
Kc=Kp
Heat a test tube at an angle at the side of the tube (not bottom)

44. What is the general formula for an aldehyde?
Filtration
RCHO (carbonyl at end)
ROR
brown volatile liquid

45. What shape is water?
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
bright yellow
bent
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

46. If a free element is involved - what type of reaction must be involved?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
redox reaction
Eudiometer

47. What value of R do you use for thermo calculations? gas calculations?
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
?H formation of an element in standard state=0
SO4²?
All except for lithium

48. How does the melting point of a mixture compare to the MP of a pure substance?
Insoluble except for nitrate and acetate
it is lower and occurs over less sharp a range
CnH2n+1 often designated 'R' ex C3H7 is propyl
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

49. If Q > Ksp - then system shifts _______ and ppt ______
Products - reactants (except for BDE when it's reactants - products)
left - ppt will form
Tetrahedral
Check for air bubbles in the buret and remove the buret funnel from the buret

50. What is the relationship between Kc and Kp if there's no ?n (gaseous molecules)?
Tetrahedral
Kc=Kp
A salt solution.
Unsaturated - addition (ex: decolorize bromine solution)

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AP Chemistry 2

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