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Chem 260 > Chapter 1 > Flashcards

Chapter 1 Flashcards

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1
Q

Shells

A

The probability of finding an electron inn various regions of space relative to the nucleus.

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2
Q

The energy of electron shells is _______.

A

Quantized

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3
Q

Quantization

A

Only specific values of energy are possible, rather than a continuum of values.

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4
Q

Delocalization

A

The spreading of electron density over a large volume of space.

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5
Q

Orbital

A

A region in space that can hold two electrons and has a specific quantized energy.

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6
Q

What orbitals does the first shell contain?

A

1s

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7
Q

What orbitals does the second shell contain?

A

One 2s and three 2p orbitals

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8
Q

Ground-state electron configuration

A

The electron configuration of lowest energy

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9
Q

Three rules for determining the ground-state electron configuration:

A
  1. The Aufbau (“build up”) principle
  2. The Pauli exclusion principle
  3. Hund’s rule
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10
Q

Aufbau principle

A

Orbitals fill in order of increasing energy, from lowest to highest,.

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11
Q

Pauli exclusion principle

A

Requires that only two electrons can occupy an orbital and their spins must be paired.

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12
Q

Paired spins

A

Two electrons with opposite spins

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13
Q

Hund’s rule

A

When orbitals of equal energy are available, but there are not enough electrons to fill all of them completely, then one electron is added to each orbital before a second electron is added to any of them. The spins of single electrons in the degenerate orbitals should be aligned.

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14
Q

Energy

A

The ability to do work

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15
Q

When a structure is higher in energy, the ____ energy it has stored.

A

more

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16
Q

Why does nature seek to reach it’s ground state?

A

When the electrons are rearranged back to the ground state, energy is released.

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17
Q

Ionization potential

A

The energy it takes to remove an electron from an atom or a molecule.

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18
Q

Covalent bond

A

A bond formed by the sharing of electron pairs between adjacent atoms

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19
Q

Electronegativity

A

A measure of the force of attraction by an atom for electrons it share in a chemical bond with another atom

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20
Q

Nonpolar covalent bond

A

A covalent bond in which the difference in electronegativity of the bonded atoms is less than 0.5

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21
Q

Polar covalent bond

A

A covalent bond in which the difference in electronegativity of the bonded atoms is between 0.5 and 1.9

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22
Q

What is the dipole moment of a polar bond equal to?

A

The product of the absolute value of the partial charge times the distance between the dipolar charges.

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23
Q

What is the Pauling scale?

A

A scale of electronegativity values

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24
Q

Electron Affinity

A

The energy released upon addition of an electron

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25
Q

Equation for formal charge

A

Valence e- in the neutral, unbonded atom - (all unshared e- + one half of all shared e-)

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26
Q

Alcohol

A

OH (hydroxyl) group bonded to a carbon atom.

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27
Q

Primary

A

The carbon bonded to the functional group is bonded to one carbon atom.

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28
Q

Secondary

A

The carbon bonded to the functional group is bonded to two carbon atoms

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29
Q

Tertiary

A

The carbon bonded to the functional group is bonded to three carbon atoms

30
Q

Another term for ester:

A

Carboxylic ester

31
Q

Can the nitrogen from an amide be bonded to other carbons?

A

Yes, there do not have to be hydrogens attached to the nitrogen. It can be contained within the molecule, rather than just at the end of it.

32
Q

Tetrahedral bond angle:

A

109.5

33
Q

Trigonal planar bond angle

A

120

34
Q

Linear bond angle

A

180

35
Q

Bent (3 regions of electron density). Description and bond angle

A

2 bonded pairs, 1 lone pair. <120

36
Q

Trigonal pyramidal. Description and bond angle

A

3 bonded pairs, 1 lone pair. <109.5

37
Q

Bent (4 regions of electron density). Description and bond angle.

A

2 bonded pairs, 2 lone pairs. <109.5

38
Q

Einstein proposed that light consists of:

A

photons of electromagnetic radiation

39
Q

The energy E of a photon =

A

hv

40
Q

h is:

A

Planck’s constant

41
Q

What did Louis de Broglie propose?

A

If light exhibits properties of particles in motion, then a particle in motion exhibits the properties of a wave. He proposed that a particle of mass m and velocity v has an associated wavelength.

42
Q

The sign of the numerical value of the wave equation is called the ______, and changes in sign are referred to as _______.

A

phase, phase changes.

43
Q

Node

A

Any point where the value of a solution of a wave equation is zero. Where phase changes occur.

44
Q

A nodal plane

A

Any plane perpendicular to the direction of propagation that runs through a node.

45
Q

Quantum mechanics

A

The branch of science that studies particles and their associated waves,

46
Q

A wave function occupies _______ and is called ______.

A

3-dimensional space, an orbital

47
Q

The value of 𝜑^2 is proportional to:

A

The probability of finding an electron at a given point in space, and the electron density at that point.

48
Q

s orbital shape:

A

sphere

49
Q

p orbital shape

A

peanut

50
Q

Molecular orbital theory

A

A combination of n atomic orbital gives n molecular orbitals.

51
Q

Sigma orbitals

A

Characterized by head-head overlap. Cylindrical symmetry of electron density about the internuclear axis. Primary bond type between two atoms. Typically made using hybrid orbitals.

52
Q

pi orbitals

A

Characterized by sideways overlap. Electron density above and below the internuclear axis. Additional bonds found in double and triple bonds. Almost always made using atomic p-orbitals.

53
Q

Valence bond theory

A

Involves the combination of atomic orbitals on each atoms before considering bonding. This combination is called hybridization, and the resulting atomic orbitals are called hybrid orbitals

54
Q

Hybrid orbitals

A

Formed by the “mixing” of atomic orbitals to create new orbitals of equal energy, called degenerate orbitals.

55
Q

Bonding molecular orbital

A

An orbital in which electrons have a lower energy in which they would in the isolated atomic orbitals

56
Q

Combination of two 1s orbitals by addition of their wave functions

A

Sigma bonding orbital

57
Q

Combination of two 1s orbitals by subtraction o their wave functions

A

Sigma anti-bonding orbital

58
Q

Anti-bonding molecular orbital

A

An orbital in which the electrons in it have a higher energy than they would be in the isolated atomic orbitals. Causes repulsion of the nuclei involved

59
Q

In VB theory, the bonds are localized:

A

between adjacent atoms rather than delocalized over several atoms as is MO theory

60
Q

sp3 hybrid orbitals

A

The mathematical combination of the 2s atomic orbital and three 2p atomic orbitals. 25% s-character, 75% p-character

61
Q

sp2 hybrid orbitals

A

The mathematical combination of one 2s atomic orbital and two 2p atomic orbitals. 33% s-character, 67% p-character.

62
Q

sp hybrid orbitals

A

The mathematical combination of one 2s orbital and one 2p atomic orbital. 50% s-character, 50% p-character

63
Q

How are S and P though of regarding hybridization?

A

sp3 hybridized with a formal charge, rather than involving 3d orbitals

64
Q

Theory of Resonance

A

Many molecules and ions are best described by writing two or more Lewis structures and considering the real molecule or ion to be a composite of these structures.

65
Q

Individual Lewis structures are called:

A

contributing structures

66
Q

Rules for writing acceptable contributing structures:

A
  1. All contributing structures must have the same number of valence electrons
  2. Must obey the rules of covalent bonding
  3. Same atom connectivity
  4. Same number of valence electrons
67
Q

Preferences for estimating the relative important of contributing structures

A

1: filled valence shells
2: least separation of unlike charges
3: negative charge on a more electronegative atom

68
Q

How is charge delocalization depicted?

A

Dashed lines (the second line) between the atoms the charge can be on and a 1/2 charge on each atom.

69
Q

Conjugation

A

A lack of an intervening atom between pi bonds or between pi bonds and lone-pair electrons

70
Q

Delocalization occurs in _______ systems.

A

conjugated

71
Q

To picture the orbitals involved in delocalized systems, use only ____ theory.

A

molecular orbital

72
Q

The shorter the bond, the _______ the bond.

A

stronger

Chem 260 (5 decks)

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