Upload
nora-turpin
View
214
Download
1
Tags:
Embed Size (px)
Citation preview
Lewis Structures and Chemical Bonds
Chapter 7
Suggested HW7.1, 7.3, 7.7, 7.15, 7.17, 7.23, 7.31, 7.37, 7.39, 7.59, 7.61, 7.63,
7.67, 7.69, 7.73, 7.75, 7.77, 7.81, 7.97, 7.99, 7.101, 7.105, 7.107, 7.109, 7.111, 7.115, 7.119, 7.121, 7.125, 7.127, 7.129,
7.139, 7.143, 7.145, 7.147
Lecture 4
1
• Electrons dictate the chemistry of an atom• Electrons fill orbitals in order or increasing energy
1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p …
• We can represent the electron configuration of an element by showing the orbital designation or orbital configuration
Review
2
1s2 2s22p6 3s23p4
[Ne]3s23p4
1s1
Shell
subshell
Number of electron in subshell
S
Octet Rule and Ions
3
• An ion is an atom that has gained or lost electrons– This results in a net charge on the atom
• If an ion has a net (+) charge cation• If an ion has a net (-) charge anion
Ions tend to form such that they satisfy the Octet Rule
The Octet Rule – Atoms prefer to have 8 electrons in their outer shell
(or dublet for H and He).
Valence electrons = outer shell
Forming Ions
4
Na (Z = 11) [Ne] 3s1
Noble gas configuration ALWAYS satisfy the octet rule
Mg (Z = 12) [Ne] 3s2
Cl (Z = 17) [Ne] 3s2 3p5 S (Z = 17) [Ne] 3s2 3p4
Lewis Representation
5
• American chemist G.N. Lewis had a profound impact on our understanding of chemical bonding. One of his many contributions was a simple way to represent chemical bonds. We call these Lewis Symbols.
– Valence Electrons are represented by dots.– A single dot represents an electron– A pair of dots represents two paired electrons sharing an orbital
H He N O
O2- K Mg2+ I-
1s1 1s2 2s22p3 2s22p4
2s22p6 3s1 [Ne] 5s25p6
Compound
6
Compounds
Organic Compound
Inorganic Compound
Contains Carbon
Composed of Charged
components
Cations Anions
Covalent
Ionic Bonds
Bond Type
Electronegativity
7
Some atoms attract electrons more than others
Electronegativity difference
2 Ionic Bond< 2 Covalent
X-Y
Ionic Bonds
9
Ion Na+ Cl-
Electron Configuration [Ne] [Ne]2s22p6
Lewis Symbol
Ionic bonds do not share electrons – bond forms through charge attraction
NaCl
CaCl2
Ion Ca2+ Cl-
Electron Configuration [Ar] [Ne]2s22p6
Lewis Symbol
Covalent Bonds
10
Covalent bonds electrons shared between two atoms. This involves an overlap of atomic orbitals
Let’s consider H2 - two hydrogen atoms share electrons.
H H
Commonly represented as:
Solid line represents covalent bond
Octet Rule NOT satisfied! Electrons pair and are shared between both
atoms
Covalent Bonding – Fluorine (F2)
12
Energy
2s2
Fluorine
Energy
2s2
Fluorine
Atomic Orbitals are NOT optimized for bonding
2p5 2p5
sp3 sp3
VSEPR
23
Valence Shell Electron Pair Repulsion
• Each region of electrons (bond or lone pair) counts as a balloon• Balloons want to spread out as much as possible