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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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1. How does half life change for zero-th order - first order - and second order processes?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Iodine and CO2 (dry ice)
CO3²?
zero-th: decreases - first: constant - second: increases

2. How do you find the pH for a dibasic acid? (H2A)?
are less dense than water
fruit - fish - bases
Perform ICE BOX calculation based on K1
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.

3. Diphosphorus pentoxide is a typical molecular binary compound. What is its formula?
Glacial acetic acid
atoms
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
P2O5

4. chlorate
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
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)
ClO3?
Salt + water

5. Does Kw increase or decrease with T? Why?
proton acceptor.
Ksp = 108s5
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
bright yellow

6. Acid plus base make?
Salt + water.
a-IMFs - b-molecular volume
CO2 and H2O
H+

7. Name 2 ways in which you can create a buffer?
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)
blue (BTB)
redox reaction
Acidified

8. One mole of electrons carries 96500Coulombs - what is this quantity called?

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9. nitrates
Soluble
10?8
H2O + CO2 (it decomposes readily)
boiling without losing volatile solvents/reactants

10. What apparatus do you use to pour liquids?
CnH2n+2
?G= -ve - E°= +ve
Pour liquids using a funnel or down a glass rod
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties

11. What do you use for an acid spill? base spill?
C2O4²?
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
H2O + CO2 (it decomposes readily)

12. 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
CO2 and H2O
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)
CH3COO?

13. ____ is a Lewis acid - since it can accept a lone pair - completing its stable form - which requires two electrons.
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
hydroxides (ex: Ba(OH)2)
H+
it is lower and occurs over less sharp a range

14. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
basic
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
do not change

15. What two compounds are great oxidizing agents?

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16. What are two substances that sublime at 1 atm when heated?
Making sigma bonds and holding lone pairs
Suniverse increases for spontaneous processes
Iodine and CO2 (dry ice)
Synthetic condensation polymer (aka a polyamide)

17. How are metal oxides and hydrides bonded? are they acidic or basic?
a-IMFs - b-molecular volume
metal oxides and hydrides are ionically bonded and basic
Concentration
allow for the vapor pressure of water and make sure to level levels

18. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
E=q + w (negative is by system - positive is on system)
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
ClO4?

19. What type of compounds are almost always colored?
P2O5
Combine the equations for the half reactions in the non-spontaneous direction
strong acids/bases are written as H+ or OH- ions
Transition element compounds (except if it has a full or empty d shell)

20. halides
no - they're written undissociated (HAaq)
Salt - Carbon dioxide and water.(latter also known as carbonic acid H2CO3)
Most are soluble except Ag - Pb
10?8

21. hydroxide
Soluble
are less dense than water
OH?
S2O3²?

22. What are two allotropes of carbon?
benzene is less reactive than alkenes
linear
Graduated cylinder
diamond and graphite

23. What is the general formula for a ketone?
Hg2²?
Iodine and CO2 (dry ice)
P2O5
RCOR

24. Color (absorbance) is proportional to ________
MnO4?
Mn²? - Cr³? - Cr³
Concentration
catalyst=conc H2SO4

25. What electrons are lost/gained first in transition element ions?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
ns² electrons (first in-first out)
[A?]/[HA] x 100 or [BH?]/[B] x 100
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)

26. Does reactivity increase/decrease going down group 1 and group 17?
Increases down group 1 decreases down group 17
Increase - the dissociation of water is endothermic so increasing T favors forward direction - thus more ions.
S crystal at 0K=0
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

27. Which of the rates changes more when temperature is increased?
Exothermic
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
bright yellow
?G= -ve - E°= +ve

28. Colorless doesn't mean ______
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.
ns² electrons (first in-first out)
Clear
Increases down group 1 decreases down group 17

29. When gas is collected over water - we must allow for leveling the water levels and for the V.P. of water. Why?
ion pairing
SO4²?
Insoluble except group 1 and ammonium
To ensure Ptot = Plab and that Pgas = Ptot-PH2O

30. What is the general formula for an amine?
Add acid to water so that the acid doesn't boil and spit
chemically (ex: with carbon)
RNH2
It ceases - the circuit is broken.

31. What is the general formula for an alcohol?
non-metal oxides and hydrides are covalently bonded and are acidic.
ROH
an oxidized and reduced substance
Kc=Kp

32. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
H+
non-metal oxides and hydrides are covalently bonded and are acidic.
?H formation of an element in standard state=0

33. What is the pH of a salt made from a WA/SB? SA/WB? SA/SB?
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
Ksp = s²

34. Color is due to ______ _______ of light.
do not change
strong acids/bases are written as H+ or OH- ions
Selective absorption
yellow

35. Name some properties of Group 17
small size and high charge
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
C2O4²?
CnH2n+2

36. Which value of R do you use for all energy and kinetics calculations?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
No effect on Voltage (hetero) but will increase current possible (surface area increases rate of reaction)
R=8.31 J/mol/K
Tetrahedral

37. What kind of bonding structure does benzene have?
R=8.31 J/mol/K
benzene has a delocalized pi ring structure
Greenish-yellow gas
Ksp = 108s5

38. What is the formula for percent error?
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)
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)
Eudiometer
|experimental - accepted|/accepted X 100

39. bromothymol
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
blue (BTB)
They decrease (or could be the same if the solid has ONLY JUST disappeared)
look for changes in oxidation # - the one that goes up is oxidized and is the RA

40. How does group 1 metals' density compare to water's?
same KE - but PEice<PEwater
are less dense than water
Acid rain - dissolves marble buildings/statues and kills trees.
CO2 and H2O

41. nitrate
Mn²? - Cr³? - Cr³
The compound with the lowest Ksp value.
NO3?
allow for the vapor pressure of water and make sure to level levels

42. What are the formulas for q?
q=mc?T q=mL (or n x ?h)
Time?¹ - (ex. s?¹ - hr?¹ - etc)
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
No - it depends on the number of ions produced on dissolving.

43. Does the electrolyte with the lowest Ksp value have to be the least soluble? Why?
benzene has a delocalized pi ring structure
No - it depends on the number of ions produced on dissolving.
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
strong acids/bases are written as H+ or OH- ions

44. Group 14 shows non-metal and metal characteristics. What two oxidation states do the elements in group 14 exist in?
+4 and +2 (+4 dominates top of group and +2 at bottom of group)
Combine the equations for the half reactions in the non-spontaneous direction
bright yellow
Mn²? - Cr³? - Cr³

45. What is a coordinate covalent bond?
small size and high charge
?H formation of an element in standard state=0
P2O5
Both electrons come from the same atom (just as good as a regular bond)

46. phosphates
voltaic: + electrolytic: -
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
At half equivalence - pH=pKa
Most INsoluble except group 1 and ammonium

47. Alkenes are ________ and react by __________
Unsaturated - addition (ex: decolorize bromine solution)
How close results are to the accepted value
Current - time and charge on ion (moles of e used in half cell reaction)
proton acceptor.

48. What is the formula for alkynes?
CnH2n-2
Products - reactants (except for BDE when it's reactants - products)
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
ion pairing

49. What type of compounds do metals/non metals form?
H+
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Pipette (burette if need repetition)
Ionic compounds

50. Which would cause the bulb in a conductivity apparatus to be brightest?
RNH2
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
+4-covalent - +2-ionic
0.10M HCl (more ions)

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AP Chemistry 2

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