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FDSCI 101 Day 15 W15

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Richard Datwyler

on 24 February 2015

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Transcript of FDSCI 101 Day 15 W15

Why is it important to understand the structure (bonding) of a molecule?
A.To know the boiling temperature of the molecule.
B.To know how explosive the molecule is.
C.To know how toxic the molecule is.
D.The structure determines the function of the molecule.
Chemist view the objects made from 3 main types of particulates, which is not one of the three?
A) Ions
B) Molecules
C) Atoms
D) Chemicals
E) all of these are correct
Which is not a Molecule under the standard definition in chemistry
A) Fats
B) Salts
C) Sugars
D) Amino Acids
Which are involved in making bonds between atoms
A) All atomic electrons
B) All valence electrons
C) All extra electrons
D) All protons
E) All neutrons
Covalent bonds form when atoms share electrons.
What would happen if the electrons were not evenly shared?

Sharing Electrons

Covalent Bonds

the branch of science that deals with the identification of the substances of which matter is composed;


Why do we care whether a bond is covalent or ionic?

Bonding patterns give us information about how molecules interact with each other.
Non-polar = hydrophobic
Polar = hydrophilic
Ionic = hydrophilic

Bond Properties

Nonpolar (pure) covalent
Equal sharing

Polar covalent
Unequal sharing

Electron stealing

and the use of these processes to form new substances.
the investigation of their properties and the ways in which they interact, combine, and change;
Keeping it together
What particles are on the outside of an atom?

Almost everything around us consists of atoms stuck together. Why do atoms stick together?
Would they be attracted to other similar particles?
What charge do these particles have?
Types of bonds
What would this do to the bond?
Consider an H-F molecule. To which atom would the bonding electrons be more attracted?
Ionic Bonds
When one substance has a strong affinity for an electron, and another has a weak affinity, so much so that the electron is 'stolen' then an ionic bond forms.

A cation is the atom that gives up the electrons ( thus is positively charged) and is usually a metal
An anion is the atom that steals the electron (thus is negatively charged) and is usually a non metal
Valence electrons
The valence electrons are those found in the outer most shells of atoms
These are the atoms that are responsible for bonding.
Most commonly used examples have 8 (2 also)
Lewis structures
Valence electrons
Bohr model
2 shell
8 shell

Forming bonds
rule of 8
Fill up the valence shell

Show example: Sodium + Chlorine
The number of bonds formed determines the shape of the molecule due to the forces of the valence electrons.

Nice examples are

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