11. Bonding & Molecular Structure

Lewis Dot Structures: Exceptions

Lewis Structures   Octet Exceptions

Draw the Lewis Dot Structure for POCl3.

Consider the following XF4 ions: PF4-, BrF4-, ClF4+, and AlF4-.
(a) Which of the ions have more than an octet of electrons
around the central atom?

Radical compounds always have an odd number of total valence electrons.

How to draw Lewis structures for covalent compounds - Dr K

Write Lewis structures for each molecule or ion. Use expanded 
octets as necessary. 
a. PF5

Molecules with an odd number of electrons are called radicals.

This exception to the octet rules occurs with odd-numbers of electrons.

It is possible for stable compounds to have less than an octet of electrons.

Atoms such as H and B have less than an octet in stable compounds.

Elements in period three and below (n < 3) may expand their octets into the d-subshell.

Correct, n must equal to or greater than 3.

Elements in period three have energetically accessible d orbitals.

This exception to the octet rule results in an expanded octet on the central atom.

 Think about the possible exceptions to the octet rule. 

Lewis Structures for Covalent Molecules: Step-by-Step

Exceptions To The Octet Rule - Lewis Dot Diagrams

Use Lewis structures to explain why Br3- and I3- are stable, while F3- is not.

8.2 How to Draw Lewis Dot Structures | Complete Guide | General Chemistry

Free radicals are important in many environmentally significant
reactions (see the Chemistry in the Environment box on free
radicals in this chapter). For example, photochemical smog—
smog that results from the action of sunlight on air pollutants—
forms in part by these two steps:
NO2 UV light NO + O
O + O2 O3
The product of this reaction, ozone, is a pollutant in the lower
atmosphere. (Upper atmospheric ozone is a natural part of the
atmosphere that protects life on Earth from ultraviolet light.)
Ozone is an eye and lung irritant and also accelerates the weathering
of rubber products. Rewrite the given reactions using the
Lewis structure of each reactant and product. Identify the free
radicals.

Write the Lewis structure for each molecule (octet rule not
followed).
a. BBr3
b. NO
c. ClO2

Lewis Dot Structures: Exceptions Example 1

Draw the Lewis Dot Structure for the radical hydroxide, OH.

Some theories of aging suggest that free radicals cause certain 
diseases and perhaps aging in general. As you know from the 
Lewis model, such molecules are not chemically stable and will 
quickly react with other molecules. According to certain theories, 
free radicals may attack molecules within the cell, such as 
DNA, changing them and causing cancer or other diseases. Free 
radicals may also attack molecules on the surfaces of cells, making 
them appear foreign to the body’s immune system. The immune 
system then attacks the cells and destroys them, 
weakening the body. Draw Lewis structures for each free radical 
implicated in this theory of aging. 
c. OH

Using Lewis symbols and Lewis structures, diagram the formation
of BF3 from B and F atoms, showing valence-shell
electrons. (e) Does BF3 obey the octet rule?

Draw Lewis structures for the following: (c) AsF5

Determine the Lewis Dot Structure for the following compound:SOCl2

Group 2A and 3A elements have incomplete octets. Group 5A-8A elements can have expanded octets.

Draw the Lewis structures for each of the following molecules
or ions. Identify instances where the octet rule is not
obeyed; state which atom in each compound does not follow
the octet rule; and state how many electrons surround these
atoms: (a) PF6-, (b) BeCl2, (c) NH3, (d) XeF2O (the Xe is the
central atom), (e) SO42 - .

(b) Which of these compounds or ions is an exception to the octet rule: borohydride (BH4-), borazine (B3N3H6, which is analogous
to benzene with alternating B and N in the ring), or boron
trichloride

Exceptions to the Octet Rule

Although I3- is a known ion, F3- is not. (c) Another classmate says F3- does not exist because it would violate the octet rule.
Is this classmate possibly correct?

Lewis Dot Structures: Exceptions Example 2

Metalloids can sometimes adopt the bonding preferences of similar nonmetals. Based on your knowledge of expanded octets, draw the Lewis Dot Structure for the following ion, SiF62–.

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Lewis Dot Structures: Neutral Compounds

Lewis Dot Structures or Electron Dot Structures&nbsp;are diagrams that show how elements in a molecule use their valence electrons to form bonds.&nbsp;

Average Bond Order

Average Bond Order represents the average number of chemical bonds between a pair of bond elements.

Lewis Dot Structures: Ions

Lewis Dot Structures of Ions involves losing or gaining valence electrons to draw the most likely structure.&nbsp;

Octet Rule

The&nbsp;Octet Rule states that main-group elements will generally form enough bonds to obtain 8 electrons in their valence shell.&nbsp;

Lewis Dot Symbols

Lewis Dot Symbols represent the outer shell electrons of an element.&nbsp;

Lewis Dot Structures: Sigma & Pi Bonds

Sigma Bonds directly connect element together, while Pi Bonds provide insulation and protection for those bonds.&nbsp;

Lewis Dot Structure Exceptions&nbsp;happen when the central element violates the Octet Rule.

Born Haber Cycle

In the Born-Haber Cycle, ionic solids are created through the ionization and eventual combination of elements.&nbsp;

Coulomb's Law

Coulomb's Law is used to determine the forces experienced by charged particles.&nbsp;

Chemical Bonds

A chemical bond is the connection&nbsp;of different elements through the sharing, transferring or pooling of electrons.&nbsp;

Resonance Structures

Resonance Structures are used to represent the different possible bonding arrangements of a molecule.

Lewis Dot Structures: Acids

Drawing the Lewis Dot Structure of Acids&nbsp;involves first drawing the polyatomic anion and then attaching the H+ ion.&nbsp;

Formal Charge

Formal Charge is the charge given to an element within a molecule when assuming equal sharing of electrons between bonded elements.&nbsp;

Bond Energy

Bond Energy is the amount of energy stored within a chemical bond.

Lattice Energy

Lattice Energy&nbsp;is the estimate for the strength of ionic bonds.&nbsp;

Dipole Moment

Dipole arrows are used anytime a molecule possesses a dipole moment, which happens when a molecule is polar.&nbsp;