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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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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. Acid plus base make?
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Salt + water.
H2PO4?
OH- and NH3

2. How do you find the pH for a dibasic acid? (H2A)?
Perform ICE BOX calculation based on K1
ClO4?
Greenish-yellow gas
Purple

3. Ions are not ______.
Glacial acetic acid
bases
atoms
It ceases - the circuit is broken.

4. 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
CnH2n
Heat a test tube at an angle at the side of the tube (not bottom)
But S° of element is not zero (except at 0K)

5. What are allotropes?
do not change
ROH
different forms of the same element
Mono; di; tri; tetra; penta; hexa.

6. What shape is carbon dioxide?
look for changes in oxidation # - the one that goes up is oxidized and is the RA
Heat a test tube at an angle at the side of the tube (not bottom)
?H-kJ - ?S-J - ?G-kJ
linear

7. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B3 A3B2?
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.
Suniverse increases for spontaneous processes
ClO2?
Ksp = 108s5

8. mercury (I) ion
non-metal oxides and hydrides are covalently bonded and are acidic.
-Ea/R
Hg2²?
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?

9. The definition of acidic basic and neutral aqueous solutions is:
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
linear
zero
basic

10. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
Pour liquids using a funnel or down a glass rod
Heat a test tube at an angle at the side of the tube (not bottom)
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 benzene ring (or more correctly the phenyl group - C6H5)

11. What is the formula for summation?

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12. What causes the dramatic effect of T on rate?
Cu3(PO4)2
They decrease (or could be the same if the solid has ONLY JUST disappeared)
T increases exponentially the proportion of molecules with E > Ea
Soluble

13. chlorate
ClO3?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
OH- and NH3
redox reaction

14. sulfates
Hg2²?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Lack of rotation of groups around a double bond. (cis has groups on same side - trans on opposite sides)
Soluble except Ag - Pb - Ca - Sr Ba)

15. What is the pH of 1.0M HCl? 1M NaOH?
bent
CnH(2n+2)
0 and 14
Heat a test tube at an angle at the side of the tube (not bottom)

16. Nonmetals are good _____ agents. Metals are good _______ agents.
Heptane
oxidizing - (F2 is the best) - reducing (ex: Li - Na).
Distillation
RCOOR

17. When a cell is 'flat' What is its voltage?
No - NH3 and HCl gases are extremely soluble
[A?]/[HA] x 100 or [BH?]/[B] x 100
zero
red - green - blue

18. What do the 'a' and 'b' in Van Der Waal's equation allow for?
q=mc?T q=mL (or n x ?h)
Unsaturated - addition (ex: decolorize bromine solution)
RCOR
a-IMFs - b-molecular volume

19. What changes Keq?
Only temperature
Acidic is when [H?] > [OH?] - basic is when [H?] < [OH?] - acidic is when [H?] = [OH?]
ethers
water and substances with (s) less dense than

20. When combining half equations - what do you do to E° values when multiplying coefficients?
No - it depends on the number of ions produced on dissolving.
metal oxides and hydrides are ionically bonded and basic
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Nothing

21. What is the formula for alkynes?
Primary alcohols are partially oxidized to aldehydes and then totally oxidized to acids (wine to vinegar)
do not change
CnH2n-2
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

22. What does the solubility of organic compounds depend on?
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
Pale yellow
it reacts by substitution NOT addition
Ignore 'x' if its K is very small compared to [reactant] (5% rule)

23. What process do you use to obtain a solvent from a solution?
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)
Distillation
Two amino acids joined together; many amino acids joined together; lots of amino acids joined together
Exothermic (?H for ANY sa/sb = -57kJ/mol)

24. What is the name of S2Cl2? (Know how to name others like this - too)
Disulfur dichloride
benzene has a delocalized pi ring structure
proton acceptor.
?G is zero at equilibrium when spontaneity is the same in either direction (K=1)

25. What is the formula for obtaining charge flowing in a cell?
Group I metals (soft metals) are stored under oil
Increases.
Salt + water
Q=It (time in seconds)

26. 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
Add acid to water so that the acid doesn't boil and spit
Insoluble except nitrate and acetate
RCHO (carbonyl at end)

27. What do you do to Keq when you combine 2 reactions - reverse an equation - or halve coefficients?
ROR
methyl formate
allow for the vapor pressure of water and make sure to level levels
Combine: multiply Keq - reverse: 1/Keq - Halve coefficients: Keq^(1/2)

28. What are two substances that sublime at 1 atm when heated?
K2
Most INsoluble except group 1 and ammonium
Increases for endo - (becomes more soluble) decreases (becomes less soluble) for exo.
Iodine and CO2 (dry ice)

29. barium sulfate
?H-kJ - ?S-J - ?G-kJ
H+
White precipitate
SO4²?

30. Is the freezing of ice endothermic or exothermic?
The dilution effect when the solutions mix. M1V1 = M2V2
ethers
Conjugate pair (one must be a weak base or acid)
Exothermic

31. What is the general formula for an ester?
White precipitate
it is lower and occurs over less sharp a range
They stay the same.
RCOOR

32. What is HCOOCH3?
Clear
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Separating funnel
Acids; HCOOCH3 is an ester

33. For what types of substances does the solid/liquid equilibrium line on a phase diagram slope LEFT?
Exothermic
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7
Filtration
water and substances with (s) less dense than

34. What reacts with an acid to create hydrogen gas?
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Insoluble except for nitrate and acetate
An active metal.
Kc=Kp

35. 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?)
Disulfur dichloride
Exothermic
redox reaction

36. Color is due to ______ _______ of light.
Increases.
it reacts by substitution NOT addition
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)
Selective absorption

37. What part of a liquid do you look at to measure its volume?
bright yellow
blue (BTB)
CH3COO?
Read the bottom of the meniscus

38. What is the second law of thermodynamics?
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?)
a-IMFs - b-molecular volume
Suniverse increases for spontaneous processes
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

39. What do the 'a' and 'b' in Van Der Waal's equation allow for?
a-IMFs - b-molecular volume
Concentration
But S° of element is not zero (except at 0K)
Group I metals (soft metals) are stored under oil

40. potassium permanganate
Synthetic condensation polymer (aka a polyamide)
small size and high charge
Purple
#ligands=charge x2

41. acetate
CH3COO?
Check for air bubbles in the buret and remove the buret funnel from the buret
Ksp = 108s5
Transition element compounds (except if it has a full or empty d shell)

42. Alkenes are ________ and react by __________
Add acid to water so that the acid doesn't boil and spit
Unsaturated - addition (ex: decolorize bromine solution)
Transition element compounds (except if it has a full or empty d shell)
ROR

43. How do you identify which is oxidized or otherwise?
benzene is less reactive than alkenes
basic
10?8
look for changes in oxidation # - the one that goes up is oxidized and is the RA

44. What is Ksp in terms of molar solubility ('s') for an electrolyte AB3 or A3B?
Ksp = 27s4
?H formation of an element in standard state=0
small size and high charge
ClO3?

45. Is the ?H formation of an element in standard state zero?
Both electrons come from the same atom (just as good as a regular bond)
S2O3²?
?H formation of an element in standard state=0
it's lower and occurs over less sharp a range

46. phosphate
Evaporation
PO4³?
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Hg2²?

47. mercury (II) ion
No - NH3 and HCl gases are extremely soluble
Glowing splint (positive result=relights)
NH4?
Hg²?

48. Which of the rates changes more when temperature is increased?
bent
it's lower and occurs over less sharp a range
Greenish-yellow gas
Temperature increase the endothermic k more (hence increasing T moves equilibrium in the endothermic direction)

49. What process takes place at the cathode in an electrochemical cell? In an electrolytic cell?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Iodine and CO2 (dry ice)
ClO4?
blue (BTB)

50. How are non-metal oxides and hydrides bonded? are they acidic or basic?
But S° of element is not zero (except at 0K)
States related to IMF magnitude (dispersion) - iodine-silvery grey solid - chlorine-yellowish green gas - bromine-brown volatile liquid - poisonous and reactive - good oxidizing agents -
non-metal oxides and hydrides are covalently bonded and are acidic.
ion pairing

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AP Chemistry 2

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