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CCP 3 > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

Definitions

1
Q
  • protons and neutrons
  • electron cloud
  • mass (nucleus)
  • volume (electron)
A

Atomic Structure

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2
Q

two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons

A

Isotopes

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3
Q

electron location unknown but electron density is known

A

Quantum Mechanical Model

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4
Q

electron will be in a certain region of space (orbital) at a given instant

A

Electron Density

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5
Q

Electrons do not circle around the nucleus in fixed orbits but rather,
in ________.

A

Orbitals

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6
Q

Each orbital has a characteristic _____and ____ (energy).

A

Shape and Size

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7
Q

used to described orbitals

A

Quantum Numbers

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8
Q

lowest-energy orbitals fill up first

A

Aufbau Principle

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9
Q

If two or more empty orbitals of equal energy are available, one electron occupies each with spins parallel until all orbitals are half-full,

A

Hund’s Rule

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10
Q

Only two electrons can occupy an orbital, and they must
have opposite spins

A

Pauli’ Exclusion Principle

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11
Q

there is a limit to the precision with which certain pairs of physical properties can be simultaneously known

A

Heisenberg’s Uncertainty Principle

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12
Q

Electron BELOW the outermost shell

A

Core Electrons

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13
Q

Electrons IN the outermost shell

A

Valence Electrons

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14
Q

An attractive force between two ions or between two atoms

A

Chemical bond

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15
Q

Why do chemical bonds form?

A

more stable and lower in energy

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16
Q

How do chemical bonds form?

A

Octet Rule

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17
Q

Chemistry of main-group elements is governed by their tendency to
take on the electron configuration of the nearest noble gas.

A

Octet Rule

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18
Q

Attractive forces between opposite charges

A

Electrostatic Attraction

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19
Q

formed in electrostatic attraction
formed in transfer of electrons
reaction of metals with nonmetals

A

Ionic Bond

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20
Q

Compounds formed by ionic bonds

A

Ionic Compound

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21
Q

Bond formed as a result of sharing electrons between two nuclei

A

Covalent Bond

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22
Q

Compounds formed by covalent bonds

A

Molecular compounds

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23
Q

Measure of the ability of an atom to pull the bonding electrons toward itself

A

Electronegativity

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24
Q

covalent bond between atoms with SAME electronegativity

A

Nonpolar covalent bond

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25
Q

covalent bond between atoms with DIFFERENT ELECTRONEGATIVITIES

A

Polar covalent bond

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26
Q

< 0.4

A

pure covalent

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27
Q

between 0.4 and 1.8

A

Polar covalent

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28
Q

> 1.8

A

ionic

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29
Q

a pair of equal and oppositely charged poles separated by a DISTANCE

A

Dipole

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30
Q

Measure of Dipole

A

Dipole moment

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31
Q

magnitude of the charge on either atom x distance between the two charges

A

Dipole moment

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32
Q

electron-dot structures

A

Lewis Structures

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33
Q

line-bond structures

A

Kekule Structures

34
Q

not an actual charge, used for bookkeeping of electrons

A

Formal charge

35
Q

charge if each bonding electron pair in the molecule were shared equally between atoms

A

Formal Charge

36
Q

Difference VE when it is not bonded and VE when it is bonded

A

Formal Charge

37
Q

OMITTING OF THE COVALENT bonds and listing
atoms bonded to a particular carbon (or nitrogen or oxygen) next toit (with a subscript if there is more than one of a particular atom)

A

Condensed structures

38
Q

C atoms aren’t shown
C atoms are assume in the lines
H atoms aren’t shown
Atoms other than C and H are shown

A

Skeletal structures

39
Q

Shows 3D shape

A

Perspective Drawing

40
Q

Show bond angles accurately

A

Ball-and-Stick Model

41
Q

Shows atoms in scale

A

Space-filling Model

42
Q

Bond lies in the plane of the paper

A

Normal Bond

43
Q

Bond extends backwards, away from the viewer

A

Dashed bond

44
Q

Bond protudes forwards, toward the viewer

A

Wedged bond

45
Q

Geometry based on arrangement of atoms in a molecule + defined by bond angles

A

Molecular Geometry

46
Q

Geometry based on valence electron pairs around a central atom + Defined by bond angles

A

Electron pair geometry

47
Q

A model for the prediction of molecular geometry based on the MINIMIZATION OF ELECTRON REPULSION between regions of eelctron density around an atom

A

Valence-Shell Electron-Pair Repulsion Model (VSEPR)

48
Q

The best arrangement of a given number of electron pairs (bonding and nonbonding) is the one that minimizes the repulsions among them.

A

Valence-Shell Electron-Pair Repulsion Model (VSEPR)

49
Q

Without lone pairs:

A

Electron Pair Geometry and Molecular Geometry is equal

50
Q

assumes that the electrons in a molecule occupy OVERLAPPING atomic orbitals of the individual atoms

A

Valence Bond Theory

51
Q

Assumes the formation of molecular orbitals from the atomic orbitals

A

Molecular Orbital Theory

52
Q

How is covalent bonds formed?

A

When atomic orbitals on neighboring atoms overlap one another

53
Q

head-on overlap of atomic orbitals; stronger

A

Sigma σ

54
Q

sideway overlap of atomic orbitals; weaker

A

PI BONDS (π)

55
Q

atomic orbitals obtained when TWO OR MORE NONEQUIVALENT ORBITALS of the SAME ATOM combine for covalent bond formation

A

Hybrid Orbitals

56
Q

Produces the molecular geometry of the molecule.

A

Hybridization

57
Q

The greater the electron density in the gregion of orbital overlap

A

The stronger and shorter the bond

58
Q

As s character increases, bond angle _______

A

Increases

59
Q

Describes a region of space in a molecule where electrons are most likely to be found

A

Molecular Orbital

60
Q

2 ways to combine atomic orbitals into molecular orbitals

A

Additive and Subtractive

61
Q

2 ways to combine atomic orbitals into molecular orbitals

? - Lower energy, bonding molecular oribtal

A

Additive

62
Q

2 ways to combine atomic orbitals into molecular orbitals

? - higher energy, antibonding molecular orbital

A

Subtractive

63
Q

occurs when an electron is shared by more than 2 atoms with π bonds (p orbitals)

A

π ELECTRON DELOCALIZATION

64
Q

Structures are represented by resonance contributors

A

π ELECTRON DELOCALIZATION

65
Q

Some substances can’t be represented by a single line-bond structure and must be considered as a resonance hybrid of two or more structures.

A

Resonance

66
Q

two individual line-bond structures

A

Resonance forms

67
Q

indicated by the double-
headed arrow between them.

A

Special Resonance Relationship

68
Q

What is the different between resonance forms?

A

Placement of the π BOND and NONBONDING VALENCE ELECTRONS

69
Q

single unchanging structure

A

Resonance Hybrid

70
Q

two individual forms and has characteristics of both

A

Resonance Hybrid

71
Q

Between resonance forms

A

Double headed arrow

72
Q

Movement of electrons

A

Curly Arrow

73
Q

From electron-rich species

A

Tail

74
Q

To electron-deficient specials

A

Head

75
Q

Double bonds separated by single bonds

A

Conjugation

76
Q

Refers to a system that has a p orbital adjacent to a π bond allowing delocalization of π electrons

A

Conjugation

77
Q

Compounds with isolated double bonds (___________)

A

Higher energy

78
Q

Special kind of conjugation and cyclic unsaturated molecules with unusual stability

A

Aromaticity

79
Q

Originally used to classify benzene and its derivatives because
many of them have distinctive odors

A

Aromaticity

80
Q
A

CCP 3 (4 decks)

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