More on Ions
Record into your notes
Achieving Noble Gas
Electron Configuration
An ion forms when an atom
• loses electrons (OIL, oxidation) or gains
electrons (RIG, reduction) to achieve noble
gas electron configuration
Recognize the appearance of Bohr’s Model
after an atom loses or gains electrons to form
ions and/or how two atom share their electrons
covalently to achieve noble gas electron
configuration.
1
Supplemental packet page 50
Atomic Number: 11
sodium-23 ion
Name:
23
Symbol:
1+
Na
11
mass # 23
#p
______
11
#n
12
______
#e
10
______
Physical Properties: Atomic Number: 17
••
•• •• ••
•••
More protons than
electrons
Electronic
Configuration:
1s2 2s2 2p6 3s0
Atomic Number: 12
magnesium-24 ion
Name:
24
Symbol:
2+
Mg
12
mass # 24
#p
12
______
#n
12
______
#e
10
______
1s2 2s2 2p6 3s0
Configuration:
Supplemental packet page 50
Atomic Number: 11
sodium-23 ion
Name:
23
Symbol:
1+
11Na
mass # 23
#p
______
11
#n
12
______
#e
10
______
Electronic
1s2 2s2 2p6 3s0
Atomic Number: 12
24
Symbol:
12Mg
mass # 24
#p
12
______
#n
12
______
10
______
#e
2+
Electronic
Configuration:
Properties:
mass # 35
combines w/
anions
Lewis Dot:
[Na]1+
Physical Properties:
Symbol:
•
Chemical
Properties:
#p
______
#n
______
#e
______
Lewis Dot:
Electronic
Configuration:
metal cation
positive ion
2+ charge
Physical Properties:
Name:
Symbol:
•
Chemical
Properties:
combines w/
anions
Lewis Dot:
[Mg]2+
Chemical
mass # 16
Properties:
#p
______
#n
______
#e
______
Lewis Dot:
Electronic
Configuration:
Ionic Structure
Name:
Properties:
mass # 35
combines w/
anions
Lewis Dot:
[Na]1+
••
•••
•
•• • • •• ••
•••
••
Physical Properties:
chloride-35 ion
metal cation
positive ion
1+ charge
Chemical
35
Symbol:
1-
17Cl
#p
______
17
#n
18
______
#e
18
______
nonmetal anion
negative ion
1- charge
Chemical
Properties:
combines w/
cations
Lewis Dot:
More electrons than
protons
Electronic
Configuration:
1s2 2s2 2p6
•• •Cl• ••]1[
3s 3p
••
2
6
Physical Properties: Atomic Number: 8
magnesium-24 ion
Name:
Name:
Physical Properties: Atomic Number: 17
••
•• •• ••
•••
More protons than
electrons
Configuration:
metal cation
positive ion
1+ charge
Chemical
Physical Properties: Atomic Number: 8
••
•• •• ••
•••
More protons than
electrons
Electronic
Ionic Structure
••
•• •• ••
•••
More protons than
electrons
1s2 2s2 2p6 3s2
metal cation
positive ion
2+ charge
Name: oxygen-16
Symbol:
8
Chemical
Properties:
combines w/
anions
Lewis Dot:
[Mg]2+
16
2-
O
mass # 16
Physical Properties:
ion
••
•• •• ••
•••
#p
8
______
#n
8
______
10
______ More electrons than
#e
Electronic
Configuration:
protons
1s2 2s2 2p6 3s0
nonmetal anion
negative ion
2- charge
Chemical
Properties:
combines w/
cations
Lewis Dot:
[•• ••O•• ••]2-
2
Please note the movement of the red colored valence (outermost) electron
on sodium. It is transferred over to the fluorine atom.
Bohr Models
Lewis dot structures
Please note the movement of the red colored valence (outermost) electron
on the 1) _______ atom. It is transferred over to the 2) ________ atom.
Fill in the blanks
ANS. 1)Mg, 2)Cl
3
Record into your notes
Ions isoelectronic (“same electronic configuration”) with noble gases
[Ne]
••
• ]1[•• Cl
• ••
[Na]1+
1s2 2s2 2p6
[Ne]
[Ar]
1s2 2s2 2p6 3s2 3p6
[•• ••O•• ••]2-
[Mg]2+
1s2 2s2 2p6
[Ne]
1s2 2s2 2p6
Please note the addition of the red colored valence (outermost) electrons
to each atom listed. Recognize boron, B, is a semimetal, not a nonmetal.
Draw the following into your notes opposite page 64
nonmetals gain just enough electrons to achieve noble gas
e- configuration of the noble gas in their period (row)
••
• • •
•
• •
••
•
••
••
••
••
•
•
• •
• •
• • ••
•
••
•
•
•
•
• •
• •
• •
•
•
•
•
•
••
••
••
••
10 Ne
5B
6C
7N
8O
9F
N 3–
O 2–
F–
nitride ion
oxide ion
fluoride ion
nonmetals ions
Please Note: the nonmetals like to gain electrons & the stability of these
ions is associated with 8 valence electrons (an octet)
semimetal
C 4–
carbide ion
4
Chapter 5 - Introduction to Chemical Bonding
Ions isoelectronic (“same electronic configuration”) with noble gases
[Ne]
[Na]1+
••
• ]1[•• Cl
• ••
[Ar]
[•• ••O•• ••]2-
[Ne]
Electrostatic repulsions
Like charges repel
[Ne]
[Mg]2+
Electrostatic attractions
Opposites attract
5
Ionic Bonding (transferring electrons to achieve noble gas electron configuration)
[Na]1+
1.Opposites attract (cation attracts an anion)
2.Brought together by electrostatics
3.Ions coming together to balance charge
••
• ]1[•• Cl
• ••
sodium chloride
• • 1[•• •Cl
]
• ••
[Mg]2+
• • 1[•• •Cl
]
• ••
magnesium chloride
[Mg]2+
[•• ••O•• ••]2-
magnesium oxide
Looking ahead to Chapter 6
Covalent Bonding (sharing electrons to achieve noble gas electron configuration)
1. Bonding for FONCl BrISCH nonmetals
2. Brought together by sharing of electrons
3. Achieving an OCTET of valence electrons
versus Chapter 5 - Ionic Bonding
Ionic Bonding (transferring electrons to achieve noble gas electron configuration)
1. Opposites attract (cation attracts an anion)
2. Brought together by electrostatics
3. Ions coming together to balance charge
6
Please note the addition of the red colored valence (outermost) electron
by the in coming hydrogen atom which will be shared by both atoms.
Covalent Bonding (sharing electrons to achieve noble gas electron configuration)
nonmetals bond to hydrogen to achieve noble gas e- configuration
of the noble gas in their period (row)
••
•
H
•
•
•
•
•
•
Addition of hydrogen
Achieving an OCTET valence
•
•
•
••
•H•
••
••
•
H• •
H• •
H• •
• • ••H
•
•
•
•
•
•
•H •
•H •
•H •
•
•
•
•
•
••
••
••
••
H
H
1H
5B
10 Ne
7N
6C
CH4
methane gas
8O
NH3
ammonia gas
H2O
water
molecules of nonmetals hydrides
9F
HF
hydrogen
fluoride
Looking ahead to Chapter 6
[Na]1+
••
• Cl •
• •
••
[
]
Ionic substances
Supplemental packet page 64
Ionic compounds are held together by strong electrical forces between oppositely charged ions (e.g., Na+ , Cl – ). These forces are referred
as ionic bonds . Typically, ionic compounds (ionic salts) have relative high melting points (mp NaCl = 801 °C).and exist
1- to
physically as solids at room temperature. It takes a lot of energy to break an ionic bond. Can you give additional examples of ionic
compounds?
Molecular compounds . Two or more atoms may combine with one another to form an uncharged molecule. The atoms involved are
unusually those of nonmetallic elements. Within the molecule, atoms are held to one another by strong forces called covalent bonds.
diatomic molecules - there are seven diatomic molecules that behave as discrete units.
room temperature are variable.
The physical states for these molecules at
H H gas
NN
O O
gas
gas
F gas
F
Cl Cl gas
Br Br liquid
I solid
I
molecules with multiple bonding patterns
H
molecules of nonmetals hydrides
H C
••
H
H
O
H
H
H
H
Si H
P
S
H
H
H
H
H
H
H
H
••
H
H
N
••••
••••
H
•• •
•• •
F
•• •
•• •
Cl
Summary
What is the favorite charge of these elements as ions? Indicate charge. Is there a relationship
between the type of element that likes to have positive charge? a negative charge?
Li
Be
B
C
N
O
F
ion charge:
1+ 2+ 3+ 4- 3- 2- 1-
How many atoms will each element bond to in order to be stable?
of bonds that each element will make.
Li
number of bonds:
1
Be
B
C
2 3 4
N
O
3 2
Indicate the number
F
1
Is there a relationship between ion charge and the number of bonds an element will make?
If so, describe the relationship.
7
Supplemental packet page 64
H
•• N
N
••
gas
•O• •O•
•gas
• ••
To these molecules,
Add missing
nonbonding pair of electrons
•••F•
••
•
••Cl•
••
•••Br•
••
•
•• I•
••
H
gas
•F• •
gas
• ••
•Cl• •
gas
• ••
•Br• • liquid
• ••
•I• •
solid
• ••
Favorite bonding modes for
nonmetals C, N,O, halogen, H
•Know the preferred total number
of bonds to these elements
CNOFH
4 3 211
•N O , nitrogen and oxygen may
have variable number of bonds
(2) (1)
(4) (3)
8
Supplemental packet page 68
valence ________
shell electron
________
VSEPR = ________
pair ________
repulsion
________
Determine the angles between bonds, name the geometry about the central atom and give the its hybridization.
IdealIdeal
bonding
for carbon = Four bonds to carbon - Four bonding modes
Geometries
bond angles
geometric name
H
120 H
C 120
120
H
120
H
H
109.5 109.5
109.5 H109.5
H
C
tetrahedral
Non-Ideal Geometries
C
H
180
H
trigonal planar
C
C H
linear
O
180 O
C
linear
Ideal bonding angles for carbon
:
:
:
bond angles
H
N
H
107.5 107.5
H
geometric name
pyramidal or
trigonal pyramid
N
θ<120
bent
H
:
O
H
104.5
H
O
:
:
N
N
H
:
bond angles
:
N
H
Bond angles are less than ideal angle
Electron pair occupies a lot of space &
is held close to nucleus of central atom
C
H
geometric name
bent
9