Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

AP Chemistry Mr. Slaven > Final Exam > Flashcards

Final Exam Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What tells you a molecule has ionic bonding as an intermolecular force?

A

Has ions, not polar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What tells you a molecule has ion-dipole forces as an intermolecular force?

A

Has ions involved, is polar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What tells you a molecule has hydrogen bonding as an intermolecular force?

A

NO ions involved, IS polar, has hydrogen bonded to N, O, or F atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What tells you a molecule has dipole-dipole forces as an intermolecular force?

A

No ions involed, IS polar, does NOT have hydrogen bonded to N, O, or F atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What tells you a molecule has london dispersion forces as an intermolecular force?

A

No ions involved, no polar molecules involved

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What are the oxidation rules for alkali metals and alkaline earth metals in compounds?

A

Alkali metal=+1
Alkaline Earth=+2
IN A COMPOUND, not alone

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the rule for the oxidation number of hydrogen in compounds?

A

It is +1, except it is -1 when combined with metals or boron in binary compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the oxidation rule with halogens?

A

-1, except when combined with a halogen above them on the periodic table or with oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is the oxidation rule for oxygen?

A

-2, except it’s -1 in peroxides

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Explain the relationship between effective nuclear charge, atom size, and the shielding effect.

A

Effective nuclear charge causes the overall attraction an electron experiences. Electrons between the nucleus and atom being considered lessens, or shields the atom from full nuclear charge. More electron shells=larger atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the trend with atom size in the periodic table and why?

A

Increases going from top to bottom in a group because of an increasing number of electron cells

Decreases going from left to right because of an increasing number of protons, meaning more attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is ionization energy? What needs to be overcome to remove an electron?

A

The energy needed to completely remove an electron from an atom. Energy must overcome the attraction between the nucleus and electron.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What factors effect the magnitude of ionization energy and why? What does it contribute to the trend of ionization energy?

A
  1. Size of the atom-the closer the electron is to the nucleus, the harder it is to remove. Ionization energy decreases from top to bottom, since valence electrons get further from nucleus
  2. Effective nuclear charge-Greater effective nuclear charge means it’s harder to remove. Ionization increases from left to right since effective nuclear energies do
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is electron affinity and its trend?

A

Electron affinity is the energy change that results from adding an electron to an ion or atom. It increases from left to right owing to increased effective nuclear charge, and decreases from top to bottom within a group owing to increased size

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

How are ionic and covalent bonds different physically? (3)

A
  1. Ionic bonds have higher melting points than covalent bonds
  2. Ionic bonds have higher electrical conductivity than covalent bonds
  3. Covalent bonds have shared electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is an electrolyte?

A

A substance that when dissolved in water produces a solution that can conduct an electric current.

17
Q

Which types of electrolytes conduct electricity effectively and ineffectively?

A

Strong electrolytes conduct electricity very efficiently

Weak electrolytes conduct only a small current

Nonelectrolytes conduct no current at all

18
Q

When are ionic substances good and bad conductors? Why?

A

Conduct well when melted, poorly when solid. When melted, the crystal lattice is broken and ions can move

19
Q

What happens if you add or remove something from an equation?(Lechateliers)

A

Add: Shift away from the side where the addition occurred

Remove: shift towards removal

20
Q

What is Le Chatelier’s rules with pressure/volume

A

If pressure increases/volume decreases, rxn will shift to the side with the fewest moles to relieve stress

21
Q

What does a positive, negative, and 0 value of 🔼G* indicate?

A

🔼G<0: Spontaneous in forward reaction

🔼G>0: Not spontaneous in forward direction

🔼G=0: System is at equilibrium

22
Q

What do positive and negative values of 🔼S tell us?

A

🔼S>0: disorder increases

🔼S<0: disorder decreases

23
Q

What do negative and positive 🔼H values represent?

A

🔼H>0: Reaction absorbed heat, it is endothermic

🔼H<0: Reaction released heat, it is exothermic

24
Q

What is molality?

A

The number of moles of solute per kilogram of solvent

25
Q

How can you distinguish an acid-base reaction?

A

They involve the transfer of one or more protons and often produce H2O

26
Q

What is an ideal gas?

A

A gas in which the particles

  1. Are very small
  2. Have negligible volume
  3. Are in constant emotion and colliding
  4. Neither attract nor repel each other
  5. Have an average kinetic energy equal to kelvin temperature
27
Q

Under what conditions are gasses ideal or closest to being ideal?

A

Non-polar gasses at a low pressure and a high temperature

28
Q

What is the purpose of van der waal’s equation?

A

It is a modification of the ideal gas law, it is meant to take into account molecular size and molecular interaction forces

29
Q

What are the a and b variable for in Van der waals equation?

A

The constant a provides a correction for the intermolecular forces. Constant b is a correction for finite molecular size and its value is the volume of one mole of the atoms or molecules.

30
Q

What is a titration?

A

A procedure for determining the unknown concentration of a solution using a solution with a known concentration, and an acid is paired with a base

31
Q

What is the end point of a titration?

A

The point where the solution changes color

32
Q

What is the equivalence point of a titration?

A

The point where moles of acid=moles of base

33
Q

What is the pH value at equivalence point in strong acid and strong base, weak acid strong base, and strong acid weak base titrations?

A

Strong acid+Strong base: pH=7 at equivalence point

Weak acid+Strong base: pH>7 at equivalence point

Weak base+Strong acid: pH<7 at equivalence point

34
Q

What do different values of K tell us?

A

K > 1 means that the reaction favors the products at equilibrium

K < 1 means that the reaction favors the reactants at equilibrium

35
Q

What does comparing Q and K tell us?

A

Q < K: Reactants must go to products for equilibrium

Q = K: the system is at equilibrium.

Q > K: Products must go to reactants for equilibrium

36
Q

How are mass and effusion related?

A

Lighter gases have higher speeds

AP Chemistry Mr. Slaven (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions