chapter 7 ionic covalent and metal materials
DESCRIPTION
Chapter 7 Ionic Covalent and Metal Materials. Types of Atoms. Ionic Compounds: 1/3 page for each. Ions (Ca+ions & Anions). Covalent (Molecular Compounds):. Two or more nonmetals. Metallic Solids:. Only metal atoms. Electron Dot structures. - PowerPoint PPT PresentationTRANSCRIPT
Chapter 7
Ionic Covalent and Metal Materials
Types of AtomsIonic
Compounds:
Covalent
(Molecular Compounds):
Metallic Solids:
Ions
(Ca+ions
& Anions)
Two or more
nonmetal atoms
2 or more
metals atoms
Electron Dot structures
valence electrons: as dots around the atomic symbols EX. Ne
• Octet Rule - atoms react until contain 8 valence e-
F Ne_
(Fluorine) Ions achieve electron configuration as Noble Gas Neon
Halide Ions
halogen, become negative gaining 1 electron.
F I BrFluorin
e IodineBromine
__
_
Fl0urine, Iodine and Bromine are all halogens - Halide Ions.
+
Ionic Bonds• force binds oppositely charged
ions
Na
ClSodium (Cation) Chlorine
(Anion)
-
Sodium chloride
Sodium
Electrostatic Attraction
B. Two types of compounds
Ionic Ionic CompoundsCompoundsMade from Made from
IOIONSNSatoms w/ positive or negative charges.when an atom has lost or gained electrons.
• Good conductors when dissolved/melted.
ca+ion & anion
Electrically Electrically neuneutraltral
Na Na ++
Cl Cl --NaClNaCl
+Crystalline Solid -
Bond formationIonic Compounds:
Covalent (Molecular):
Metallic Solids:
Transfer of electrons
Sharing of electrons
Free moving valence e-
Bond formation
room temperature crystalline
Hard & Brittle, High Melting pt
solid, liquid or gas. soft & low melting point
Soft to very hard Higher valence # of e- , harder metal.
Electrostatic forces
Very Strong
Weak
Strong
How many Na+
surround Cl-?
Na+
Na+
Na+
Na+Na+
Na+
Na+
Na+Na+
Na+
Na+
Na+Na+
Na+
Na+
Na+
Cl-
Cl-
Cl-
Cl-Cl-
Cl-
Cl-
Cl-Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Na+
Na+
Na+
Na+Na+
Na+
Na+
Na+Na+
Na+
Na+
Na+Na+
Na+
Na+
Na+
Cl-
Cl-
Cl-
Cl-Cl-
Cl-
Cl-
Cl-Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Na+
Na+
Na+
Na+Na+
Na+
Na+
Na+Na+
Na+
Na+
Na+Na+
Na+
Na+
Na+
Cl-
Cl-
Cl-
Cl-Cl-
Cl-
Cl-
Cl-Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Cl-
Compound ArrangementIonic Compound
•Oppositely charged ions close packed layers.
Unit cell
repeating 3D pattern :
Crystal
Even at this point, there was still a Polar Covalent Bond between Sara, Johnny and Bill…
Johnny didn’t like the feeling of competing with Bill but he knew if he really wanted her,
he’d have to fight for her.
Stop in the name of Love, before You break my heart.
Covalent Compound
•nonmetals bonds between molecules are weak
Water molecules
Weak forces
•Low to high mt. pts.
•Ductile: can be
hammered into different shapes
•Malleable:
can be drawn into wires
•Metals:
e- e-
Form a bond
Electron cloud
ConductorsMetallic Solids:
Good conductors of heat
Why?
• Free-moving valence electrons
• Free-moving valence electrons
Why?
in the molten state.
or as electrolytes
Ionic Compounds:
Conductors
Bonds break (melt) or dissociate (dissolve).Ions separate - free to
move around.
Poor conductors
Molecular Compounds:
Don’t form ions
Network Solids• Consist of atoms held together by large network of covalent bonds.• Each atom is covalently bonded in a large chain or network.• There are NO molecules in a network solid, only atoms bonded together.Example: Diamond
• Bonds are very strong.
Network Solid
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