Chemical Bonds
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Chemical Bonds
+
proton
neutron
-
electron
Orbital Notation
Electron Configuration
Electron-Dot (Lewis-Dot) Structure
Chemical Bonds
Be
+
Name
Atomic Number
Symbol
Atomic Mass
proton
neutron
-
electron
Orbital Notation
Be
Electron Configuration
Be
Electron-Dot (Lewis-Dot) Structure
Be
Chemical Bonds
Name
Atomic Number
Symbol
Atomic Mass
O
+
proton
neutron
-
electron
Orbital Notation
O
Electron Configuration
O
Electron-Dot (Lewis-Dot) Structure
O
Draw orbital notations
for the following:
Draw electron configurations
for the following:
C
C
C
Ne
Ne
Ne
Mg
P
Ca
Draw electron-dot (Lewis-Dot)
structures for the following:
Mg
Mg
P
P
Ca
Ca
Forming an Ionic Bond
Na
1s
2s
2p
2s
2p
Na
Cl
Cl
3s
Cl
1s
Na
3s
3p
Forming an Ionic Bond
Na
1s
2s
2p
2s
2p
Be
1s
Cl
Cl
3s
Be
Be
O
O
3p
2s
O
1s
Na
3s
Cl
1s
Na
2s
2p
Chemical Bond
A. Ionic Bond
A. Ionic Bond
Properties of Ionic Compounds -when ionic compounds form, they form
a _____________, a ________________
_________ arrangement of _______ and
________ ions
-the energy required to separate _______
(6.02 x 1023) of ions from each other is
called the ________________, the more
________ the lattice energy, the ______
the attraction between ions
-the strength of the attraction between
ions affects the compound’s __________
_________
Properties of Ionic Compounds
A. Lattice Energy
Compound
Lattice Energy
Properties of Ionic Compounds
A. Lattice Energy
0
-200
-400
F
Cl
Br
I
-600
-800
-1000
-1200
Li
Na
K
Properties of Ionic Compounds
A. Lattice Energy
-the lattice energy is more negative in ionic
compounds that have ____________________,
because the ions are ___________________ to
each other
B. Melting and
Boiling Points
Compound
Melting Point (°C)
Boiling Point (°C)
Properties of Ionic Compounds
B. Melting and
Boiling Points
-ionic compounds with higher lattice energies
have _________melting and boiling points temps.
-smaller ions are more ________ attracted to each
other, because the _______ is closer to the
_______ _________, while ions with larger
positive and negative charges are more
________ attracted to each other
C. Electrical Conductivity -to conduct electricity, charged particles
must be _________________, so ionic
compounds generally do not conduct
electricity as a _____, but generally do
as a ______ or when ______________
_______________
Properties of Ionic Compounds
D. Hardness -the ions in ionic compounds with _______________
lattice energies are more _________ attracted to each
other, so they tend to be ________
For Review
1. Rank the following ionic compounds, in order, from most negative
to least negative lattice energy: RbCl, RbF, RbBr, RbI
2. Rank the following ionic compounds, in order, from highest to lowest
melting point temperature: NaCl, MgCl2, MgO
3. Rank the following ionic compounds, in order, from softest to
hardest: Li2O, Li2S, Li2Te, Li2Se
4. Rank the following ionic compounds, in order, from ions most strongly
to ions least strongly attracted to each other: MgF2, RbCl, CaF2,
CaCl2, MgO