section 5.2— drawing molecules objectives: use the periodic table to identify the number of...
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Section 5.2—Drawing Molecules
Objectives: •use the periodic table to identify the number of valence electrons in an atom•draw Lewis Dot structures for ionic and covalent compounds•introduce the idea of isomers
Drawing Molecules on Paper
Lewis Structures (or Dot Structures) are one way we draw compounds on paper
Since paper is 2-D and compounds aren’t, it’s not a perfect way to represent how atoms bond…but it’s a good way to begin to visualize compounds
How do we determine the number of valence electrons in an atom?
The number found with the “A” in the group number IS the number of valence electrons.
1 2 3 4 5 6 7 8
Remember:
Put electrons on each side of the element’s symbol.
Put one in each spot before doubling up!
O
Oxygen is in group VIA or 6A.
There are 6 valence electrons.
Example:Draw the
Lewis Structure for an oxygen
atom
Practice: Oxygen
To Draw Ionic Compounds
Draw each atomTransfer electrons from metal atoms to
non-metal atoms, keeping track of their new charge
Practice: KCl
ClK
Potassium has 1 electron
Chlorine has 7 electrons
Example:Draw the
Lewis Structure for
KCl
FBa
Barium has 2 electrons
Fluorine has 7 electrons
Example:Draw the
Lewis Structure the
ionic compound of
Barium fluoride
The fluorine is full, but the Barium isn’t!
FBa
Example:Draw the
Lewis Structure the
ionic compound of
Barium fluoride F
Another fluorine atom is needed!
FBa
Example:Draw the
Lewis Structure the
ionic compound of
Barium fluoride
F
+2 -1
-1
Now all have full valence shells and the charges are balanced, just as when you learned to write in BaF2 in Chapter 2!
A note about Ionic Dot Structures
The atoms are not sharing the electrons—make sure you clearly draw the atoms separate!
Practice Problems
Draw Lewis Dot Structures for compounds that form between the following atoms. What are the formulas for the compounds?
1.Al and Cl
2.Ba and O
3.Na and P
Arrange the Atoms Atoms found in the middle of covalent
compounds are the atoms with the LEAST electron affinity.
Hydrogen & Halogens (F, Cl, Br, I) can only bond with one other atom—they can’t go in the middle of a molecules
Always put them around the outside
In general, write out the atoms in the same order as they appear in the chemical formula
Use the periodic table to decide how many electrons are around each atom
Write the electrons around each atom
Next:
H
HExample:Draw the
Lewis Structure for
CH4 C HH
Carbon is in the middle – the H’s are around it.Carbon has 4 electronsEach hydrogen has 1
Practice: CH4
H
H
Any electron that is being shared between two atoms gets to be counted by both atoms!
All atoms are “full” with 8 valence electrons (except H—it can only hold 2)
Each pair of electrons shared by two atoms forms a bond
A bond can also be represented by a single dash
C HH
Sometimes . . .
Sometimes, you don’t end up having a full valence shells for all atoms in the compound.
Example:Draw the
Lewis Structure for
CH2O
HC OH
•C has to go in the middle – the O and 2 H’s are around it.•C has 4 electrons, oxygen has 6 and each H has 1.
Practice: CH2O
Note: the carbon and oxygen only have 7 each However, they each have a single, unshared
electron. They could share those with each other!
Example:Draw the
Lewis Structure for
CH2O
HC OH
Example:Draw the
Lewis Structure for
CH2O
HC OH
Now the carbon and oxygen both have8 valence electrons! (And the H’s have 2!)
Double Bonds
Double bonds are when 2 pairs of electrons are shared between the same two atoms
Double Bond
And when a double bond isn’t enough…
Sometimes forming a double bond still isn’t enough to have all the valence shells full
Practice: C2H2
Both C’s go in the middle and 1 H goes on each side.
The C’s have 4 electrons each; the H’s have 1.
Example:Draw the
Lewis Structure for
C2H2
HC CH
Each carbon atom only has 7 electrons…not a full set of 8!
But they each have an un-paired electron left!
Example:Draw the
Lewis Structure for
C2H2
HC CH
Each carbon atom only has 7 electrons…not a full set of 8!
But they each have an un-paired electron left!
Example:Draw the
Lewis Structure for
C2H2
HC CH
Now they each have 8 electrons!
Properties of multiple bonds
Single Bond
Double Bond
Triple Bond
Shorter bonds (atoms closer together)
Stronger bonds (takes more energy to break)
Polyatomic Ions
They are a group of atoms bonded together that have an overall charge
Polyatomic ions have a covalent bond within themselves…
But an ionic bond with other ions
Isomers
For many compounds, there is more than one correct way to draw a Lewis Dot Structure
HC CH CHH
HC CH CH
H
Chemical Formula: C3H4
Chemical Formula: C3H4
Contains 2 sets of double bonds between carbons
Contains 1 triple bond and 1 single bond between carbons
Both structures have full valence shells!
Both are “correct”
The chemical formula alone does not give you enough information to differentiate between the two structures
HC CH CHH
HC CH CH
H
Chemical Formula: C3H4