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ADV. INORG CHEM > MOLECULAR STRUCTURE AND BONDING > Flashcards

MOLECULAR STRUCTURE AND BONDING Flashcards

1
Q

refers to the attractive forces that hold atoms together in compounds

A

Chemical bonding

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2
Q

What are the types of chemical bonding?

A

Ionic bonding
Covalent bonding
*single and multiple bonds
* coordinate bond
Metallic bonding
Hydrogen bonding
Van der Waals
Intermolecular forces

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3
Q

a fundamental chemical property that describes the tendency of an atom to attract electrons in a chemical bond

higher EN attract electrons + participate in chemical reactions

values decrease moving down and to the left in the periodic table

A

Electronegativity

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4
Q

between atoms; predict the type of chemical bond (ionic/covalent) and polarity (polar/nonpolar, partial positive/partial negative charges)

A

Electronegativity differences

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5
Q

energetics of bond formation

A

Pauling

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6
Q

properties of individual atoms, electronvolts

A

Mulliken

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7
Q

Review on the Pauling, Mulliken, and Allred-Rochow table on ppt

A
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8
Q

electric field at the surface of an atom

A

Allred and Ruchow

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9
Q

ability of an atom (electron cloud) to be distorted by an electric field (such as that of a neighboring ion)

A

Polarizability

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10
Q

An atom or ion is highly polarizable if?

A

its electron distribution can be distorted readily

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11
Q

species that effectively distort the electron distribution of a neighboring atom or anion are described?

A

as having a polarizing ability

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12
Q

extensive polarization leads to covalency

A
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13
Q

What are Fajan’s rules:

A
  1. small, highly charged cations have polarizing ability
  2. large, highly charged anions are easily polarized (increases with the size of the atom)
  3. cations that do not have a noble-gas electron configuration are easily polarized.
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14
Q

Do all the electrons in an atom contribute equally to the polarizability?

A

Not all electrons in an atom contribute equally to polarizability. Core electrons, being tightly bound to the nucleus, contribute less, while valence electrons, which are more loosely bound, contribute more due to their higher susceptibility to external electric fields.

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15
Q

Which would be the more polarizable, an F−ion or an I− ion?

A

I− ion is larger than F –, thus, I– is likely to be more polarizable

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16
Q

Which would be more polarizing, Na+ or Cs+?

A

Na+ is smaller than Cs+, thus, Na+ is more polarizing

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17
Q

discovery of the covalent bond and his concept of electron pairs

his Lewis dot structures and other contributions to valence bond theory have shaped modern theories of chemical bonding

A

Gilbert Newton Lewis (1875-1946)

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18
Q

uses dots (or dots and crosses) to represent the number of valence electrons, and the nuclei are indicated by appropriate elemental symbols

A

Lewis structure (Electron dot structure)

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19
Q

each atom shares electrons with neighboring atoms to achieve a total of eight valence electrons (an octet)

A

Octet rule

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20
Q

Guide to Lewis structure is in your notebook ( *̀ ω *́ )✧

A
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21
Q

Lewis structure in three steps:

  1. Decide on the number of electrons that are to be included in the structure by adding together the numbers f all the valence electrons provided by the atoms.
  2. Write the chemical symbols of the atoms in the arrangement that shows which atoms are bonded together.
  3. Distribute the electrons in pairs.
A
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22
Q

yt on Lewis structures

A
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23
Q

the electrical charge difference between the valence electrons in an isolated atom and the number of electrons assigned to that atom in a Lewis structure

A

Formal charge

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24
Q

For molecules, a Lewis structure in which there are no formal charges is preferable to one in which formal charges are present.

A
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25
Q

Lewis structures with large formal charges are less plausible than those with small formal charges

A
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26
Q

Negative formal charges are placed on the most electronegative atoms.

A
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27
Q

Formula for formal charge:

Valence electrons - (Bonds + dots)

A
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28
Q

practice in drawing Lewis structures; this will appear on the exam for sure TT

A
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29
Q

Study on the formal charge and expanded counts on central atom

A
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30
Q

Study the structures of BeF2, BeCl2, and BF3

A
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31
Q

the actual structure of the molecule is a superposition, or average, of all the feasible Lewis structures corresponding to a given atomic arrangement.

A

Resonance

32
Q

practice on how to make resonance structures again

A
33
Q

QS asked during lecture:

  1. What is the main purpose/essence of resonance?
  2. Why are there molecules that can undergo/capable of resonance?
  3. Why is the average of these resonance structures more stable? - they want to share electrons and occupy a larger space (search and confirm)
A
34
Q

occurs between structures that differ only in the allocation of electrons; NOT between structures in which the atoms themselves lie in different positions

A

Resonance

35
Q

What are the two main effect of resonance?

A
  1. resonance averages the bond characteristics over the molecule (search more on this)
  2. the energy of a resonance hybrid structure is lower than that of any single contributing structure
36
Q

Resonance structures that contribute more to the electronic ground state of the species, generally,

A

a. have smaller magnitudes of formal charges

b. place negative formal charges on more electronegative elements

c. have smaller separation of charges what does this mean again TT)

37
Q

ask about the bond lengths on ppt

A
38
Q

Study the formation of covalent bond between two hydrogen atoms up to the graph

A
39
Q

internuclear distance at which the attractive and repulsive forces balance and the bond is most stable

A

Bond length

40
Q

Note that a C=C double bond is not twice as strong as a single bond. Similarly, a triple bond is not three
times as strong as a single bond.

A
41
Q

molecules and ions that contain only single bonds, the approximate shape can be predicted from the number of electron pairs in the outer or valence shell of the central atom

A

Sidgwick-Powell theory

42
Q
  1. If there are two pairs of electrons in the valence shell of the central atom, the
    orbitals containing them will be oriented at 180° to each other. It follows that if
    these orbitals overlap with orbitals from other atoms to form bonds, then the
    molecule formed will be linear.
  2. If there are three electron pairs on the central atom, they will be at 120° to each
    other, giving a plane triangular structure.
  3. For four electron pairs the angle is 109°28, and the shape is tetrahedral.
  4. For five pairs, the shape is a trigonal bipyramid. For six pairs the angles are 90° and
    the shape is octahedral.
A
43
Q

predicts the spatial arrangement of atoms in a polyatomic molecules or ion.

A

Valence shell electron-pair repulsion (VSEPR)

44
Q

shows where the bonding occurs and where lone pairs of valence shell electrons are directed

A

Valence shell electron-pair repulsion (VSEPR)

45
Q

describes how the bonding takes place, in terms of overlapping atomic orbitals

A

Valence bond theory

46
Q

atomic orbitals are often “mixed,” or hybridized, to form new orbitals with different spatial orientations

A

Valence bond theory

47
Q

The method for predicting molecular shapes is based on “electron-pair electrostatic repulsion”. It states that molecules adopt geometries that position valence electron pairs as far apart as possible to minimize electron-electron repulsion. This theory, known as “VSEPR (Valence Shell Electron Pair Repulsion)”, provides approximate molecular shapes that generally agree with experimental observations.

A
48
Q

the total number of positions occupied by atoms or lone pairs around a central atom; lone pairs and bonding pairs both influence the molecular shape

A

Steric number

49
Q

the VSEPT model predicts that electron-pair repulsions involving lone pairs (lp) are stronger than those involving bonding pairs (bp) in the order…

A

lp-lp repulsion > lp-bp repulsion > bp-bp repulsion

50
Q

READ EBOOK BEFORE U SLEEP SO NO MORE INSOMNIA AGAIN

A
51
Q

The VSEPR model assumes that all lone pairs are stereochemically active and therefore do affect the molecular geometry.

A
52
Q

common mistake in exam is not knowing the difference between valence bond theory and VSEPR

A
53
Q

read about octahedral and distorted pentagonal bipyramidal

A
54
Q

possible qs in exam: describe the bond angle i.e is it greater than 90 degrees or less or is it in the equatorial or axial position

A
55
Q

study on how to predict the structure and shape of a molecule/ion + practice, practice, practice

A
56
Q

Do multiple bonds influence the molecular geometry of a molecule/ion?

A

The VSEPR model considers double and triple bonds to have
slightly greater repulsive effects than single bonds because
of the repulsive effect of pie electrons that increase the
electron density between the bonded atoms beyond that
present in an s bond.

57
Q

study + read on the structure containing multiple bonds

A
58
Q

Multiple bonds:

  1. tend to occupy the same positions as lone pairs
  2. like lone pairs, they also occupy more space than ingle bonds, causing distortions that squeeze the rest of the molecule together
A
59
Q

lone pairs often have a greater influence than multiple bonds dictating molecular geometry

A
60
Q

What are the conditions that must be met for a molecule to be polar?

A
  1. There must be at least one polar bond or one lone pair on the central atom
  2. a. the polar bonds, if there are more than one, must be arranged so that their polarities (bond dipoles) do not cancel

b. If there are two or more lone pirs on the central atom, they must be arranged so that their polarities do not cancel.

61
Q

linear molecule: bond dipoles cancel; nonpolar

angular molecule: bond dipoles do not cancel; polar

A
62
Q

mixing of pure atomic orbitals of comparable energy

A

Hybridization

63
Q

Features of hybrid orbitals:

  1. The number of hybrid orbitals of equal energy formed is the same as the number of atomic orbitals that are mixed. All the hybrid
    orbitals formed have identical characteristics.
  2. The shape of each hybrid orbital is such that one lobe is small and the other lobe is large.
  3. As the % s character increases in a hybrid orbital, the hybrid orbital become bulkier and shorter. On the other hand, as the % p or % d character increases, the orbital becomes longer and thinner.
  4. As the % s character increases, the energy of the hybrid orbital
    decreases and as the % p or % d character increases, the energy of the hybrid orbital increases.
  5. The s, p, and d orbitals involved in the different types of hybridization are as follows: this part is in your nb lol
A
64
Q

familiarize on the relation between electronic geometries and hybridization (if your brainpower can, memorize it, force it idk just do something about it TT)

A
65
Q

What are the procedure for hybridizing atomic orbitals?

A
  1. Draw the Lewis structure of the molecule.
  2. Predict the overall arrangement of the electron pairs (both bp and lp) using the VSEPR.
  3. Deduce the hybridization of the central atom by matching the arrangement of the electron pairs with those of the hybrid orbitals.
66
Q

TETRAHEDRAL ELECTRONIC GEOMETRY: AXE3 (3 LP)

  1. Each Group 7A element has 7 electrons in its highest occupied energy level. Group 7A elements form molecules such as H-F, Hi-Cl, Cl-Cl, and I-I by sharing one of their electrons with another atom. The other atom contributes one electron to the bonding.
  2. Lewis formulas for these molecules are shown in the margin. Any diatomic molecule must be linear.
  3. Neither VSEPR theory nor VB theory add anything to what we already know about the molecular geometry of such molecules.
A
67
Q

TRIGONAL BIPYRAMIDAL ELECTRON GEOMETRY: AX5

Valence bond theory
The heavier Group 5A elements—P, As, and Sb—can form five
covalent bonds using this hybridization. But nitrogen, also in
Group 5A, cannot form five covalent bonds because the valence
shell of N has no d orbitals (only one s and three p orbitals).

A
68
Q

a bond resulting from a head-in overlap of atomic orbitals

The region of electron sharing is along and cylindrically around an imaginary line connecting the bonded atoms

A

Sigma bond

69
Q

a bond resulting from side-on overlap of atomic orbitals.

The regions of electron sharing are on opposite sides of an imaginary line connecting the bonded atoms and parallel to this line

A

Pi bond

70
Q

A double bond consists of one sigma bond
and one pi bond.

A
71
Q

How to analyze the structure and bonding in any structure

  1. Write Lewis formula and identify a central atom.
  2. Count electron groups (bonded atoms & lone pairs) on that central atom.
  3. Determine electronic geometry around that central atom.
  4. Determine molecular geometry around that central atom.
  5. Adjust the molecular geometry for any lone pairs.
  6. Determine hybrid orbitals, describe bonding
  7. Can another central atom be identified?
    * YES = go back to step 2
    * NO = proceed to step 8
  8. Determine whether molecule is polar or nonpolar.
A
72
Q

When there are two electron groups around the central atom, it is sp hybridized. AB2
molecules and ions with no lone pairs on the central atom have linear electronic
geometry, linear molecular geometry, and sp hybridization on the central atom.

A
73
Q

When there are three electron groups around the central atom, it is sp2 hybridized. AB3
molecules and ions with no lone pairs on the central atom have trigonal planar electronic
geometry, trigonal planar molecular geometry, and sp2 hybridization on the central atom.

A
74
Q

When a molecule or polyatomic ion has no lone pairs of valence electrons on the central
atom, the molecular geometry is the same as the electronic geometry

A
75
Q

AB2U2 molecules and ions, each having four electron groups around the central atom,
usually have tetrahedral electronic geometry, angular molecular geometry, and sp3
hybridization on the central atom

A
76
Q

When there are five electron groups around the central atom, it is sp3d hybridized. AB5
molecules and ions with no lone pairs on the central atom have trigonal bipyramidal electronic geometry, trigonal bipyramidal molecular geometry, and sp3
d hybridization on the
central atom.

A

ADV. INORG CHEM (4 decks)

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