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MCAT - Chemistry > Class 2 > Flashcards

Class 2 Flashcards

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1
Q

When determining ideal structure what things should you look for?

A
  1. Atoms obey octet rule 2. Formal charge = overall charge 3. Smallest set of formal charges 4. Posiitve formal charges on less EN atoms 5. Negative formal charges on more EN atoms
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2
Q

When drawing a Lewis structure, what atom should be central?

A

The least electronegative atom or carbon if there is one.

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3
Q

Formal charge must always equal what?

A

The overall charge!

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4
Q

What orbital geometric configuration is sp?

A

Linear

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5
Q

What orbital geometric configuration is sp2?

A

Trigonal planar

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6
Q

What orbital geometric configuration is sp3?

A

Tetrahedral

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7
Q

How does orbital geometry differ from molecular geometry/shape?

A

Oribtal geometry is solely based on sp level. Shape considers lone pairs/bonds.

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8
Q

What are the possible molecular geometries for sp hybridized molecules?

A

There is none! Same as orbital geometry

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9
Q

What are the possible molecular geometries for sp2 hybridized molecules?

A

bent (one lone pair)

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10
Q

What are the possible molecular geometries for sp3 hybridized molecules?

A

trigonal pyramid or bent (two lone pairs)

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11
Q

_____ bonds = stronger bonds = ______ bond dissociation energies.

A

Shorter bonds = stronger bonds = higher BDE

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12
Q

Breaking bonds is always what kind of process?

A

ENDOTHERMIC!

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13
Q

What kind of elements typically form covalent bonds?

A

High electronegative atoms (e.g. nonmetals with nonmetals).

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14
Q

Describe covalent bonds

A
  1. Electrons are localized between the two atoms. 2. Inflexible, hard, rigid compounds 3. Act as insulators
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15
Q

What is the difference between a polar covalent bond and a nonpolar covalent bond?

A

Nonpolar covalent = difference in EN of 0 Polar covalent = difference in EN > 0 but only slightly. A huge difference would result in an ionic bond.

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16
Q

How do you calculate the molecular dipole?

A

Add up all the bond dipoles.

17
Q

Do metals strongly or weakly attract their electrons?

A

Weakly (they have low electronegativities!)

18
Q

Describe metallic bonds

A
  1. Electrons are delocalized between the two atoms 2. Soft compounds 3. Act as conductors
19
Q

What is a coordinate covalent bond?

A

Lone pairs from a nucleophile/ligand “bond” with electron-deficient species. Electrons are localized If the nucleophile shares more than 2 electrons, it is considered a chelate.

20
Q

How does a coordinate covalent complex act? What is an example of one?

A

It is transient interaction, easily broken Iron atom in the heme unit

21
Q

What’s a weird thing about Boron?

A

It is cool with 3 bonds.

22
Q

What part of the heme unit does oxygen interact with? how?

A

Coordinates (forms a coordinate complex) with the iron.

23
Q

What forms ionic bonds?

A

Electrostatic interaction between atoms of opposite charge (anion and cation)

24
Q

Are ionic bonds insulators or conductors? Why?

A

Insulators because electrons are localized, and thus are rigid.

25
Q

The larger the ionic charge, the _________ the ionic dipole force

A

larger

26
Q

What is another term for dispersion forces?

A

diploe-induced dipole forces

27
Q

What are dispersion forces?

A

Collisions within the electron cloud cause temporary but small dipoles deforming the cloud. More electrons will create a stronger force (more polarizable). Think of it like throwing clay against a wall-> temporarily deforms and sticks to the wall.

28
Q

What is the weakest intermolecular force

A

(London) dispersion forces

29
Q

Hydrogen bonds are formed between molecules that are very very ________.

A

Polar!

30
Q

What is required to form a hydrogen bond?

A

A donor (N-H, O-H, F-H) and an acceptor (O: N: F:)

31
Q

What three things can increase entropy?

A
  1. increase number of particles 2. increase the volume it occupies 3. increase the temperature Rearrangement does NOT affect entropy
32
Q

What is the unit of entropy?

A

Joules/mol Kelvin

33
Q

What is the eqn for entropy?

A

change in entropy = moles x entropy of products - molez s entropy of reactants

34
Q

What is the (delta)H for an endothermic reaction?

A

positive

35
Q

What is the (delta)H for an exothermic reaction?

A

negative

36
Q

What is the difference between endergoinc and endothermic?

A

EnderGonic refers to (delta)G EnotHermic refers to (delta)H

37
Q

ATP dephosphorylation is an _________ process.

A

Endothermic! Breaking bonds! BUT at high temps, it is EXERGONIC!! (and thus spontaneous)!

MCAT - Chemistry (7 decks)

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