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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. What things should you remember to do when collecting gas over water?
NO2 and SO2 are very soluble - CO2 and O2 are somewhat soluble
allow for the vapor pressure of water and make sure to level levels
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Trigonal pyramidal

2. What electrons are lost/gained first in transition element ions?
The dilution effect when the solutions mix. M1V1 = M2V2
Separating funnel
ns² electrons (first in-first out)
voltaic: - electrolytic: +

3. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
bright yellow
No - it depends on the number of ions produced on dissolving.
Potassium permanganate and potassium dichromate (they're clues that a reaction will be redox)
bases

4. What is the relationship between Rate and Molar Mass for two gases? Velocity and Temperature? Energy and Temperature?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Disulfur dichloride
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
boiling without losing volatile solvents/reactants

5. What measuring device would you use for very small volumes of liquids?
Pipette (burette if need repetition)
it reacts by substitution NOT addition
benzene is less reactive than alkenes
K1 x K2

6. Which value of R do you use for all energy and kinetics calculations?
Pale yellow
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
RX
R=8.31 J/mol/K

7. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
The dilution effect when the solutions mix. M1V1 = M2V2
RX
are less dense than water

8. What is the word equation for condensation polymerisation ?
Monomer + monomer = polymer product + a simple molecule such as water or HCl
acids
Both electrons come from the same atom (just as good as a regular bond)
S crystal at 0K=0

9. What are the prefixes for the naming of binary molecular compound formulas (up to six)
Mono; di; tri; tetra; penta; hexa.
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.
different forms of the same element
It ceases - the circuit is broken.

10. What are the products for these common oxidizing agents? MnO4? - CrO4²? - Cr2O7²?
Read the bottom of the meniscus
The compound with the lowest Ksp value.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Mn²? - Cr³? - Cr³

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?
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
benzene is less reactive than alkenes
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
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

12. What complex ion does ammonia form with silver? copper? cadmium? zinc?
redox reaction
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
Acidified
zero

13. What is the formula for alkanes?
CnH2n+2
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
The dilution effect when the solutions mix. M1V1 = M2V2
S crystal at 0K=0

14. ________ are Lewis bases - because they can donate a lone pair of electrons.
Pale yellow
OH- and NH3
But S° of element is not zero (except at 0K)
Synthetic condensation polymer (aka a polyamide)

15. What is the general formula for alkyl halides?
+4-covalent - +2-ionic
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
RX
Experimental mass/theoretical mass X 100

16. What is the general formula for a ketone?
zero
strong acids/bases are written as H+ or OH- ions
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
RCOR

17. How do you get the equation for a net electrolysis reaction?
CnH(2n+2)
Transition element compounds (except if it has a full or empty d shell)
Acidified
Combine the equations for the half reactions in the non-spontaneous direction

18. What is the general formula for an aldehyde?
RCOOH
NO3?
RCHO (carbonyl at end)
OH?

19. What is the basic structure of an optical isomer?
Acid rain - dissolves marble buildings/statues and kills trees.
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
Sigma bonds are stronger than pi bonds
NO3?

20. Ca - Sr - Ba
CO3²?
The dilution effect when the solutions mix. M1V1 = M2V2
hydroxides (ex: Ba(OH)2)
CnH2n+2

21. oxalate
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
C2O4²?
Synthetic condensation polymer (aka a polyamide)
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell

22. What is the conjugate base of NH3?
Ppt will NOT form (unsaturated)
NH2?
Making sigma bonds and holding lone pairs
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

23. What type of compounds do Group 14 form?
Sigma bonds are stronger than pi bonds
+4-covalent - +2-ionic
Mono; di; tri; tetra; penta; hexa.
CnH2n+1 often designated 'R' ex C3H7 is propyl

24. What process do you use to obtain the solute from a solution?
zero
Exothermic
metal oxides and hydrides are ionically bonded and basic
Evaporation

25. What type of compounds do metals/non metals form?
Cu3(PO4)2
Reverse most negative E° and add voltages to get Ecell (or take absolute difference between Ered values)
Ionic compounds
Sulfur

26. When driving off water from a hydrate - how do you tell you're done?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Group I metals (soft metals) are stored under oil
CO3²?
Heat to constant mass-weigh - reheat - cool - and weigh again until mass is constant

27. What word is a clue for a redox reaction?
Heat a test tube at an angle at the side of the tube (not bottom)
Acidified
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]

28. What shape is methane?
Pipette (burette if need repetition)
Tetrahedral
Iodine and CO2 (dry ice)
left - ppt will form

29. What do you use for an acid spill? base spill?
fruit - fish - bases
ClO2?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
yellow

30. When the salt bridge is removed what happens to the cell reaction?
It ceases - the circuit is broken.
Hg²?
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

31. What is a coordinate covalent bond?
Most are soluble except Ag - Pb
Both electrons come from the same atom (just as good as a regular bond)
They stay the same.
S crystal at 0K=0

32. What type of compounds are almost always colored?
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
Transition element compounds (except if it has a full or empty d shell)
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)

33. Which of the rates changes more when temperature is increased?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
methyl formate
Read the bottom of the meniscus

34. What two types of substances are present in all redox reactions?
non-metal oxides and hydrides are covalently bonded and are acidic.
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
Eudiometer
an oxidized and reduced substance

35. What is the energy you must put into a reaction to make it start called?
Initiation energy (NOT Ea)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
voltaic: - electrolytic: +
Exothermic (?H for ANY sa/sb = -57kJ/mol)

36. How do you find the pH for a dibasic acid? (H2A)?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
RNH2
Perform ICE BOX calculation based on K1
Q=It (time in seconds)

37. What is the word equation for addition polymerisation?
K1 x K2
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Only temperature
Initiation energy (NOT Ea)

38. The oxidation # for acid base reactions...
Insoluble except for nitrate and acetate
Optical isomers contain at least one chiral (asymmetric) C atom which is a C atom that has four different groups attached to it.
do not change
Sigma bonds are stronger than pi bonds

39. What is the general formula for an ether?
Group I metals (soft metals) are stored under oil
CN?
ROR
Unsaturated - addition (ex: decolorize bromine solution)

40. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
basic
CnH2n+2
water and substances with (s) less dense than
HClO4

41. What are two substances that sublime at 1 atm when heated?
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
CrO4²?
Iodine and CO2 (dry ice)
An active metal.

42. What do hydrocarbons form when they burn in air (oxygen)?
CO2 and H2O
No - it depends on the number of ions produced on dissolving.
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Sigma bonds are stronger than pi bonds

43. What apparatus do you use to pour liquids?
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
Synthetic condensation polymer (aka a polyamide)
Pour liquids using a funnel or down a glass rod
Meth - eth - prop - but - pent - hex - hept - oct - non - dec

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

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45. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
CnH2n-2
Pale purple - (orange)-yellow - red - blue - green.
Q=It (time in seconds)

46. What should you check for before you begin titrating?
ns² electrons (first in-first out)
Check for air bubbles in the buret and remove the buret funnel from the buret
acid + alcohol
No - it depends on the number of ions produced on dissolving.

47. What is an Alkyl group?

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48. If a weak acid is diluted more - what happens to its % dissociation value?
metal oxides and hydrides are ionically bonded and basic
Increases.
bases
?G= -ve - E°= +ve

49. Esters smell like _______ and amines smell like _______ and are ______.
fruit - fish - bases
NO3?
ethers
neutralization: high K - H2O product dissociation: low K - H2O reactant

50. Is magnesium oxide (and other main group metal oxides) likely to be acidic - basic or neutral?
voltaic: + electrolytic: -
Soluble except Ag - Pb - Ca - Sr Ba)
acid + alcohol
basic