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AP Chemistry 2

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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. Neutralization is an ________ reaction.
Exothermic (?H for ANY sa/sb = -57kJ/mol)
CO2 and H2O
Orange
Mn²? - Cr³? - Cr³

2. What is the charge on a chlorine atom?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
zero
Check for air bubbles in the buret and remove the buret funnel from the buret
White precipitate

3. What is the difference between equivalence point and end point of a titration.
no - they're written undissociated (HAaq)
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
ion pairing
Synthesis - separation and purification of the product and its identification.

4. If a weak acid is diluted more - what happens to its % dissociation value?
Salts (ex: CaO + SO2 ? CaSO3)
Purple
Increases.
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

5. permanganate
acids
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Heptane
MnO4?

6. nitrates
Soluble
Making sigma bonds and holding lone pairs
Acidified
RCOR

7. 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?
+4-covalent - +2-ionic
The compound with the lowest Ksp value.
OH- and NH3
redox reaction

8. How do you identify which is oxidized or otherwise?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Saturated - Substitution (which requires more radical conditions)
Pipette (burette if need repetition)
Hg2²?

9. Alcohols and _______ are FG isomers
ethers
White precipitate
Soluble
Acid rain - dissolves marble buildings/statues and kills trees.

10. What apparatus do you use to separate 2 immiscible liquids?
It ceases - the circuit is broken.
lighted splint (positive result=pop)
Separating funnel
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)

11. What effect does increasing the size/surface area of a voltaic cell have on the cell?
Conjugate pair (one must be a weak base or acid)
Nothing
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Soluble

12. What is the slope of the graph of lnk vs. 1/T?
CO (poisonous)
-Ea/R
blue
different forms of the same element

13. What is the formula for obtaining charge flowing in a cell?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Q=It (time in seconds)
Orange
ROH

14. What things should you remember to do when collecting gas over water?
Ppt will NOT form (unsaturated)
metal oxides and hydrides are ionically bonded and basic
allow for the vapor pressure of water and make sure to level levels
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

15. What complex ion does ammonia form with silver? copper? cadmium? zinc?
ethers
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
zero
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

16. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
Nothing
H3PO4
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp

17. What is the pH of 1.0M HCl? 1M NaOH?
0 and 14
Exothermic
Orange
No - NH3 and HCl gases are extremely soluble

18. perchlorate
ClO4?
A) any range. b) 8-10 c) 4-6
CnH(2n+2)
Soluble

19. What are the names and formulas of the 6 strong acids?
Increases down group 1 decreases down group 17
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
Pale purple - (orange)-yellow - red - blue - green.
Identity and purity (impure compounds usually have broad & low melting points)

20. A geometric (or cis-trans) isomer exists due to.....
non-metal oxides and hydrides are covalently bonded and are acidic.
Clear
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

21. Colorless doesn't mean ______
Clear
are less dense than water
Initiation energy (NOT Ea)
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)

22. Name six characteristics of transition elements (or their compounds)
Soluble
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)
Graduated cylinder
Unsaturated - addition (ex: decolorize bromine solution)

23. carbonate
CO3²?
zero
But S° of element is not zero (except at 0K)
zero

24. Buffer capacity must contain decent amounts of a ________ ________
Conjugate pair (one must be a weak base or acid)
Initiation energy (NOT Ea)
NH4?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

25. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
Synthesis - separation and purification of the product and its identification.
basic
Q=It (time in seconds)
Silvery gray solid - brown - purple

26. Name 2 ways in which you can create a buffer?
NH4?
1) Add together a weak base with a salt of that base made with a strong acid. (or visa versa) 2) by partially neutralizing a weak base with a strong acid or weak acid with a strong base. (Ex: 0.2 mol NH3 + 0.1 mol HCl)
hydroxides (ex: Ba(OH)2)
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.

27. oxalate
C2O4²?
zero
Filtration
Insoluble (except group 1 ammonium and Ba)

28. 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?
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
CH3COO?
different forms of the same element
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

29. phosphate
10?8
PO4³?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
no - they're written undissociated (HAaq)

30. If a free element is involved - what type of reaction must be involved?
P2O5
Both electrons come from the same atom (just as good as a regular bond)
redox reaction
?H formation of an element in standard state=0

31. hydroxide
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
OH?
diamond and graphite
Soluble

32. How are primary alcohols turned into acids?
different forms of the same element
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

33. What apparatus do you use to pour liquids?
CnH2n+1 often designated 'R' ex C3H7 is propyl
Pour liquids using a funnel or down a glass rod
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

34. What are the units of the first order rate constant?
H2PO4?
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)
CnH(2n+2)
Time?¹ - (ex. s?¹ - hr?¹ - etc)

35. What reacts with an acid to create hydrogen gas?
An active metal.
How close results are to the accepted value
The Faraday or Faraday's constant.
Perform ICE BOX calculation based on K1

36. What is HCOOCH3?
Add acid to water so that the acid doesn't boil and spit
Acids; HCOOCH3 is an ester
Silvery gray solid - brown - purple
no - they're written undissociated (HAaq)

37. Alkenes are ________ and react by __________
it's lower and occurs over less sharp a range
Unsaturated - addition (ex: decolorize bromine solution)
zero
CnH2n+1 often designated 'R' ex C3H7 is propyl

38. What is reflux?
boiling without losing volatile solvents/reactants
Current - time and charge on ion (moles of e used in half cell reaction)
ClO2?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble

39. What is the general formula for an amine?
S crystal at 0K=0
Soluble
CO3²?
RNH2

40. silver compounds
To ensure Ptot = Plab and that Pgas = Ptot-PH2O
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
Insoluble except for nitrate and acetate
CnH(2n+2)

41. How do you find the pH for a dibasic acid? (H2A)?
|experimental - accepted|/accepted X 100
Perform ICE BOX calculation based on K1
Ppt will NOT form (unsaturated)
CH3COO?

42. What is the formula of copper (II) phosphate?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
But S° of element is not zero (except at 0K)
Cu3(PO4)2
Making sigma bonds and holding lone pairs

43. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
C2O4²?
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
voltaic: - electrolytic: +

44. mercury (I) ion
ROH
fruit - fish - bases
Hg2²?
by electrolysis

45. What is the general formula for an aldehyde?
+4-covalent - +2-ionic
ethers
CO3²?
RCHO (carbonyl at end)

46. What should you check for before you begin titrating?
do not change
Check for air bubbles in the buret and remove the buret funnel from the buret
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

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
SO4²?
Current - time and charge on ion (moles of e used in half cell reaction)
CO3²?

48. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
q=mc?T q=mL (or n x ?h)
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)
OH?
neutralization: high K - H2O product dissociation: low K - H2O reactant

49. Which value of R do you use for all energy and kinetics calculations?
R=8.31 J/mol/K
HClO4
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)
Separating funnel

50. What do hydrocarbons form when they burn in air (oxygen)?
RCHO (carbonyl at end)
methyl formate
CO2 and H2O
'non-active' metals such as Cu - Ag - Au - Pt - etc.

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AP Chemistry 2

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