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Bonding Unit
Learning Goal #2: Compare covalent, ionic, and metallic bonds with respect to electron behavior and relative bond strength.
The type of bond can The type of bond can usuallyusually be calculated by be calculated by finding the difference in electronegativity of the finding the difference in electronegativity of the
two atoms that are going together.two atoms that are going together.This table is found on page 304 of the text.This table is found on page 304 of the text.
Electronegativity Difference
• If the difference in electronegativities is between:– 1.7 to 4.0: Ionic– 0.3 to 1.7: Polar Covalent– 0.0 to 0.3: Non-Polar Covalent
Example: NaClNa = 0.8, Cl = 3.0Difference is 2.2, sothis is an ionic bond!
Bonding spectrum100% covalent 100% ionic
A+ B-A B A B
Increasing EN
Increasing polarity Transfer
IONIC BONDbond formed
between two ions by the
transfer of electrons
Metal + Nonmetal
Opposites Attract!
Ionic Bond Characteristics
One atom gains, one loses electrons. Produce charged ions in all states. Electrical attraction between ions of
opposite charge. Between atoms of metals and nonmetals
with very different electronegativity Strong Bond but not as strong as a covalent
bond.
Ionic Bond CharacteristicsCrystalline solid.Very high melting point.Soluble in H2O.Insoluble in nonpolar solvents.Nonconductor of heat and electricity in solid form.Conducts electricity in aqueous solutions or when melted.Examples: NaCl, CaCO3
Ionic Bond
COVALENT BONDbond formed by the sharing of electrons
Nonmetal + Nonmetal
Covalent Bond• Atoms can form molecules by sharing electrons
in the covalent bond. This is done only among non-metal atoms.
Covalent Bond Characteristics
Between nonmetallic elements of similar electronegativity.
Formed by sharing electron pairs Stable non-ionizing particles Strongest bond type
Gas, liquid, or a soft solid at room temperature.Low melting point and low boiling point.Most are Insoluble in H2OSoluble in nonpolar solvents.Nonconductor of heat and electricity.Nonlustrous
Covalent Bond Characteristics
The Covalent Bond• Shared electrons are attracted to the nuclei of
both atoms.
• They move back and forth between the outer energy levels of each atom in the covalent bond.
• So, each atom has a stable outer energy level some of the time.
when electrons are shared equally
NONPOLAR COVALENT BONDS
H2 or Cl2
Nonpolar Covalent Molecules
• Equal distribution of charge around a central atom.
• Molecule has a symmetrical shape
when electrons are shared but shared unequally
POLAR COVALENT BONDS
OH-
Polar Covalent Molecules
• Electrons are shared, but not equally.
• Some atoms have a stronger pull for the electrons.
• Molecule not symmetrical in shape (unbalanced).
METALLIC BONDbond found in
metals; holds metal atoms together
very stronglyMetal + Metal
Metallic Bond Characteristics
• Formed between atoms of metallic elements• Electron cloud around atoms
• In metals, valence electrons are shared, free to move about.
• Good conductors of heat and electricity in all states.
• Strong bond, but weakest of the three bond types.
Metallic Bond Characteristics
• Malleable solid• High melting point and boiling
point.• Insoluble in H2O.• Insoluble in nonpolar solvents.• Lustrous• Examples: gold, copper
Metals Form Alloys
Metals do not combine with metals. They form Alloys which is a solution of a metal in a metal.Examples are steel, brass, bronze and pewter.
Bond Type
Review
Na Cl
NaCl
+-
electron transferand the formation of ions
This is the formation of an ionic bondionic bond.
This is the formation of a covalent bondcovalent bond.
Cl2
Cl Cl
sharing of a pair of electronsand the formation of molecules
Metallic Bonds
Fe
Positive Nuclei
Electrons Freely Moving
Metal atoms tightly packed with electrons
moving freely around the positive nuclei.
Covalent Bonds Ionic Bonds Metallic Bonds
Shape Definite Shape No Definite Shape
Definite Shape
Boiling Point Low High High
Examples Methane (CH4) Sodium Chloride (NaCl)
Iron Metal
Occurs Between 2 Non-Metals Metal and Non-metal
2 Metals
Formation Sharing of Electrons
Transfer of Electrons
The valence electrons are detached from the atoms but not held by any of the
other atoms.
Polarity Low High ----------
Melting Point Low High High
Electronegativity Difference
Low High Low
State at Room Temperature
Liquid Or Gaseous
Solid Solid
1. Explain how gaining, losing or sharing valence electrons will help predict the type of bond between two elements?
2. How does a bond type describe what behavior the valence electrons are exhibiting?
3. Which are the strongest and weakest types of bonds?
Essential Questions