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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 many ligands attach to a central ion in a complex ion?
Hydrogen (active metals are metals with more negative reduction potentials in E° chart)
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
A salt solution.
#ligands=charge x2

2. Ions are not ______.
Suniverse increases for spontaneous processes
atoms
O2 needs 4F/mol H2 needs 2F/mol
There's one normal boiling point (1 atm) - but many boiling points (P dependent)

3. nitrates
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)
Soluble
Initiation energy (NOT Ea)
allow for the vapor pressure of water and make sure to level levels

4. What are the prefixes used to name organic alkanes with varying number of carbon atoms? (Up to ten carbons)
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
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
benzene is less reactive than alkenes

5. What is the sign of the cathode in voltaic cells? in electrolytic cells?
voltaic: + electrolytic: -
Soluble
No - it depends on the number of ions produced on dissolving.
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

6. What are the signs of ?G and E° for spontaneous reactions?
Time?¹ - (ex. s?¹ - hr?¹ - etc)
by electrolysis
?G=negative - E° must be positive
They decrease (or could be the same if the solid has ONLY JUST disappeared)

7. What is the general formula for alkyl halides?
q=mc?T q=mL (or n x ?h)
Soluble
CnH2n
RX

8. What is the general formula for a ketone?
Reduction always takes place at the cathode (RED CAT) In both types of cell!
Products - reactants (except for BDE when it's reactants - products)
RCOR
Kc=Kp

9. Why are i factors (Van't Hoff factors) often less than ideal?
ion pairing
#ligands=charge x2
R=8.31 J/mol/K
Alkali ion - OH? - and H2 (phenolphthalein goes pink - thus 'alkali' metals)

10. What is the solubility of AgF - AgCl - AgBr - and AgI in water and ammonia?
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
They have high ionization energies (due to high nuclear charge and no shielding) and cannot add electrons due to full valence shell
Meth - eth - prop - but - pent - hex - hept - oct - non - dec
Glacial acetic acid

11. silver iodide
zero-th: decreases - first: constant - second: increases
Pale yellow
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
ion pairing

12. What do group I/II metal oxides and acids form?
Salt and water
Q=It (time in seconds)
?H-kJ - ?S-J - ?G-kJ
Increases.

13. How do you explain trends in atomic properties using Coulomb's Law?
it is lower and occurs over less sharp a range
bases
Mention effective nuclear charge (shielding) and distance of outer electrons from the nucleus
-Ea/R

14. nitrate
NO3?
NH2?
RCOOH
[A?]/[HA] x 100 or [BH?]/[B] x 100

15. What are the bond angles and hybridization for a carbon with 4 sigma bonds? one double bond? two double bonds? one triple bond?
4 sigma bonds-109° - sp³ - one double bond-120° - sp² two double bonds-180° - sp one triple bond-180° - sp
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
Orange
K2

16. What are the names and formulas of the 6 strong acids?
red - green - blue
?H-kJ - ?S-J - ?G-kJ
K2
HNO3 - (nitric) H2SO4 -(sulfuric) HCl -(hydrochloric) HBr -(hydrobromic) HI - (hydroiodic) HClO4 (perchloric)

17. acetate
PO4³?
blue
CH3COO?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)

18. 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)
There's one normal boiling point (1 atm) - but many boiling points (P dependent)
basic
Salts (ex: CaO + SO2 ? CaSO3)

19. What do ions and electrons travel through in a voltaic/electrolytic cell?
Ions go through the salt bridge - electrons go through metal wires in the external circuit
Thermo: R=8.31J/mol/K - gas calculations: R=.0821 L atm/mol/K or 62.4L mmHg/mol/K
HClO4
WA/SB: pH>7 SA/WB: pH<7 SA/SB: pH=7

20. At what point during titration do you have the perfect buffer - and what is the pH at this point?
At half equivalence - pH=pKa
fractional distillation
basic
hydroxides (ex: Ba(OH)2)

21. phosphates
Most INsoluble except group 1 and ammonium
Cu3(PO4)2
linear
it's lower and occurs over less sharp a range

22. What do metal oxides plus acids form?
No - it depends on the number of ions produced on dissolving.
ROH
Salt + water
#ligands=charge x2

23. How many faradays of electric charge do you need to produce one mole of O2? H2?
Transition element compounds (except if it has a full or empty d shell)
bright yellow
O2 needs 4F/mol H2 needs 2F/mol
Hg²?

24. Generally - which oxy acid is strongest?
The one with most oxygen atoms (highest oxidation number)
it reacts by substitution NOT addition
diamond and graphite
#ligands=charge x2

25. How many normal boiling points and boiling points are there?

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26. What complex ion does ammonia form with silver? copper? cadmium? zinc?
RCOOR
Combine the equations for the half reactions in the non-spontaneous direction
[Ag(NH3)2]? - [Cu(NH3)4]²? - [Cd(NH3)4]²? - [Zn(NH3)4]²?
The compound with the lowest Ksp value.

27. Both Acetic acid and ____________ are also functional isomers.
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
The compound with the lowest Ksp value.
Decant
methyl formate

28. When a cell is 'flat' What is its voltage?
Decant
zero
Whether or not they can form H-bonds with water (ex: Ethyl alcohol is soluble but dimethyl ether is not)
SO4²?

29. What do you use to look at burning magnesium? why?
Iodine and CO2 (dry ice)
Soluble except Ag - Pb - Ca - Sr Ba)
an oxidized and reduced substance
blue glass - it filters UV

30. What is a coordinate covalent bond?
MnO4?
Both electrons come from the same atom (just as good as a regular bond)
water and substances with (s) less dense than
Filtration

31. What is the word equation for condensation polymerisation ?
Cold beaker=endothermic - ?H=positive (hot beaker=exothermic - ?H=negative)
Monomer + monomer = polymer product + a simple molecule such as water or HCl
Cu3(PO4)2
Pale purple - (orange)-yellow - red - blue - green.

32. ammonium/ammonium compounds
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)
Soluble
Iodine and CO2 (dry ice)
different forms of the same element

33. When a cell is 'flat' a.k.a 'reached equilibrium' - what is its ?G value?
zero
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
But S° of element is not zero (except at 0K)

34. What type of solutions do small - highly charged cations tend to form?
Acidic solutions (Ex: [Fe(H2O)6]³? + H2O = Fe(H2O)5OH]²? + H3O?)
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
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)
by electrolysis

35. What changes Keq?
buret - pipette - pipette filler - Erlenmeyer flask - volumetric flask
Only temperature
0.10M HCl (more ions)
#ligands=charge x2

36. Flame tests for certain metal ions (simple emission spectra) gives which colors for potassium - sodium - lithium - copper - barium
Ksp = s²
'non-active' metals such as Cu - Ag - Au - Pt - etc.
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Pale purple - (orange)-yellow - red - blue - green.

37. How are non-metal oxides and hydrides bonded? are they acidic or basic?
Iodine and CO2 (dry ice)
Exothermic (?H for ANY sa/sb = -57kJ/mol)
non-metal oxides and hydrides are covalently bonded and are acidic.
fruit - fish - bases

38. What is the formula for summation?

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39. 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
ns² electrons (first in-first out)
Two forms of the same element (same Z) with different # of neutrons and similar chemical properties
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2

40. What is Ksp in terms of molar solubility ('s') for an electrolyte A2B or AB2?
Ksp = 4s³
do not change
Products - reactants (except for BDE when it's reactants - products)
C2O4²?

41. 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?
metal oxides and hydrides are ionically bonded and basic
The compound with the lowest Ksp value.
P2O5
Filtration

42. What shape is methane?
Conjugate pair (one must be a weak base or acid)
Tetrahedral
Group I metals (soft metals) are stored under oil
Soluble

43. What is an Alkyl group?

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44. What is the word equation for addition polymerisation?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
are less dense than water
ClO3?
Q=It (time in seconds)

45. How do you compute % dissociation?
Insoluble
[A?]/[HA] x 100 or [BH?]/[B] x 100
diamond and graphite
ClO3?

46. What is the energy you must put into a reaction to make it start called?
zero
r1/r2=(M2/M1)^½ - v1/v2=(T1/T2)^½ - E1/E2=T1/T2
Initiation energy (NOT Ea)
Most are soluble except Ag - Pb

47. What is the conjugate acid of H2PO4?
1. Rinse the buret/pipette with deionized water - 2. Rinse the buret/pipette with the solution you plan on filling the buret/pipette with.
atoms
A substance that can act as an acid or a base. ex. water - HCO3? ion etc.
H3PO4

48. What do you need to make a polymer?
ClO2?
it is lower and occurs over less sharp a range
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)
Pale purple - (orange)-yellow - red - blue - green.

49. What do you use for an acid spill? base spill?
n(unsaturated monomer) = polymer (no loss in material) ex. n(C2H4) = (C2H4)n (polyethylene)
Heat a test tube at an angle at the side of the tube (not bottom)
redox reaction
Acid spill-NaHCO3 (baking soda) base spill-acetic acid (vinegar)

50. What does saturated mean? Unsaturated?
Saturated organic compounds contain single bonds in their carbon skeleton. Unsaturated have at least one double or triple bond.
allow for the vapor pressure of water and make sure to level levels
Greenish-yellow gas
oxidizing - (F2 is the best) - reducing (ex: Li - Na).

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AP Chemistry 2

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