chapter 7. chemical bonds
DESCRIPTION
Chapter 7. Chemical Bonds. Chemical bonds are the attractive forces that hold atoms together in a complex unit. Types of Bonds. Ionic bonds are electrostatic forces between ions. Oppositely charged ions attract one another. Covalent bonds form when atoms share electrons. - PowerPoint PPT PresentationTRANSCRIPT
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Chapter 7.
Chemical Bonds
Chemical bonds are the attractive forces that hold atoms together in a
complex unit.
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Types of Bonds
Ionic bonds are electrostatic forces between ions.
Oppositely charged ions attract one another.
Covalent bonds form when atoms share electrons.
Bonds give shapes to molecules
Atoms are not charged
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Valence Electrons
Valence electrons are the electrons in the outermost s sub-shell and electrons in any other unfilled subshell.
Valence electrons are the least tightly held electrons in an atom, and they are the ones that "do chemistry".
An element's position on the Periodic Table shows how many valence electrons it has.
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Valence Electrons
Representative elements (Groups 1A – 7A) have 1 to 7 electrons.
We can represent them as dots around the element's symbol.
These are called Lewis Symbols.
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Lewis Symbols of 1st 20 Elements
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Stable Electron Configurations
Atoms are most stable when they have filled valence shells.
For representative elements, each atom wants 8 electrons surrounding it.
Transition metals are most stable with filled or half-filled outer s and d subshells.
Atoms will lose, gain or share electrons to reach these stable configurations.
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The Octet RuleRepresentative elements want 8 electrons in
their valence shells.
Noble gases have filled valence shells.
Group 6A and 7A nonmetals gain elec-trons to fill their valence shells.
Become anions
Group 1A, 2A, and 3A metals lose elec-trons to fill their valence shells.
Become cations
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Predict Charges
For ions of the following metals:
Na, Ca, Al
For ions of the following nonmetals:
F, O, P
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Ionic Bonds
Ionic bonds are chemical bonds that result from the attraction of positive and negative ions for each other.
Metal cation(s) and nonmetal anion(s)
Higher charges, stronger bonds
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Ionic Bonds
Ionic compounds are chemical compounds characterized by ionic bonds between atoms.
An ionic compound will have a formula such that charge neutrality is achieved.
Na1+ + Cl1- NaCl
Mg2+ + 2 Cl1- MgCl2
Al3+ + 3 Cl1- AlCl3
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Structures of Ionic Compounds
Ionic bonds are non-directional electrostatic forces
Ions arrange themselves in an array (usually a crystal lattice) that
Maximizes interactions between oppositely charged ions
Minimizes interactions between ions of like charge
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Structure of NaCl(2 dimensions)
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Structure of NaCl(3 dimensions)
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Other Crystal Structures
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Details about Ionization
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Ionization Energy
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Electron Affinity
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Covalent Bonds
Covalent bonds are chemical bonds that result when two nuclei attract and share the same electrons.
Covalent bonds form between atoms of nonmetals.
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Covalent Bonds
Covalent compounds are characterized by covalent bonds between atoms.
A covalent compound will have a formula such that all the atoms share electrons in such a way that the octet rule is satisfied.
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Lewis Structures
Lewis Structures are groupings of Lewis symbols that show transfer of electrons in ionic compounds or sharing of electrons in covalent compounds.
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Lewis Structure of H2
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Bond Distance
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Lewis Structures of Diatomic Molecules
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Lewis Structure for Ammonia (NH3)
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Multiple Covalent Bonds
Two atoms can share more than two electrons.
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Drawing Lewis Structures
Determine the number of electrons
A. Needed to give each atom an octet
except hydrogen, which needs two
B. Available (all valence electrons for
all atoms in structure)
C. Shared = Needed Available
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Drawing Lewis Structures
Choose the central atom for the structure
A. NEVER hydrogen
B. CARBON if it's in the formula
C. Choose atom furthest left and/or down
on the Periodic Table
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Drawing Lewis Structures
Draw structure
A. Write symbol of central atom
B. Arrange other atoms around it
C. Show shared electrons as dots between atoms
D. Show other available electrons as dots around atoms
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Drawing Lewis Structures
Check structure
A. Is the right atom in the center?
B. Have the correct number of electrons
been shared?
C. Are all available electrons shown?
D. Is the octet rule satisfied?
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Drawing Lewis Structures
Examples:
H2O
CO2
HCN
SO3
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Drawing Lewis Structures
Resonance Structures are two or more Lewis Structures for the same species that differ only in the position of the electrons.
There must be at least one double bond in the structure for there to be resonance.
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Drawing Lewis Structures
Polyatomic Ions are charged groups of atoms, held together by covalent bonds.
They often appear in parentheses in chemical formulas, e.g. Al2(SO4)3.
Draw their structures in the usual way, but account for the charge in the available electrons.
Examples:
PO43 NH4
1+ CO32
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Drawing Lewis Structures
Acids of Polyatomic Anions:
Draw the structure of the anion, with hydrogen atoms bonded to the oxygen atoms.
Examples:
H3PO4
H2CO3
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Molecular Geometry
Lewis Structures give numbers and types of bonds in molecules and polyatomic ions.
Lewis Structures do not convey information about the shapes of the molecules and ions.
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Molecular Geometry
VSEPR:
Valence Shell Electron Pair Repulsion Theory.
VSEPR theory is an explanation of the shapes of simple molecules that uses Lewis Struc-tures. It is based on the fact that electrons repel each other, and groups of electrons will get as far away from each other as possible in a molecule or polyatomic ion.
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Molecular Geometry
VSEPR electron groups are groups of valence electrons that are present in a localized region in a molecule.
Each bond is a group (single or multiple)
Each non-bonded pair is a group
If the central atom follows the octet rule, there can be 2, 3, or 4 electron groups around it.
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Molecular Geometry
Electronic geometries are descriptions of the arrangement of electrons about the central atom in a molecule or ion.
# of Electron Regions Electronic about Central Atom Geometry
2 Linear
3 Trigonal Planar
4 Tetrahedral
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Molecular Geometry
The Three Possible Electronic Geometries (where the electrons are)
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Molecular GeometryWhat? That's not where you told me the
atomic orbitals were!
Nope! Now we're looking at molecules, with hybrid orbitals.
Hybrid orbitals are combinations of atomic orbitals. These give rise to the shapes of molecules and polyatomic ions.
A specific type of hybrid orbital is associated with each electronic geometry.
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Linear Electronic Geometry, sp Hybridization
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Trigonal Planar Electronic Geometry, sp2 Hybridization
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Tetrahedral Electronic Geometry, sp3 Hybridization
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Molecules with Linear Electronic Geometry, sp Hybridization
Molecular Geometry is Linear
CO2 (carbon dioxide)
HCN (hydrogen cyanide)
C2H2 (acetylene)
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Molecules with Trigonal Planar Electronic Geometry, sp2
Hybridization
Molecular Geometry
SO3 (sulfur trioxide) Trigonal Planar
SO2 (sulfur dioxide) Angular/Bent
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Molecules with Tetrahedral Electronic Geometry, sp3 Hybridization
Molecular Geometry
CH4 (methane) Tetrahedral
NH3 (ammonia) Trigonal Pyramidal
H2O (water) Angular/Bent
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Molecular Geometry
Examples:
CCl4 (carbon tetrachloride)
H3O1+ (hydronium ion)
C2H4 (ethylene)
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Types of Bonds (sigma) bonds result from end-to-end overlap
of orbitals, electron density is on bond axis.
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Types of Bonds (pi) bonds result from parallel overlap of orbit-
als; there is no electron density on bond axis.
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Types of Bonds
There can be more than one bond between two atoms.
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Types of BondsResonance is really a bond distributed over
several bonds, as in the carbonate anion
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Bond PolarityWe've looked at ionic bonds and covalent
bonds. Actually, there's a continuum, and most bonds fall in the middle.
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Bond Polarity
Representing bond polarity:
+
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Electronegativities
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Bond Classification
Look up electronegativities of atoms, calculate difference between them
Difference: Bond Type:
0.0 to 0.4 Nonpolar covalent
0.5 to 1.9 Polar covalent
2.0 Ionic
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Polarity of Molecules
A nonpolar molecule or ion has a symmet-rical distribution of electrical charge.
A polar molecule or ion has an unsymmet-rical distribution of electrical charge.
Look at polarities of individual bonds. If the polarities cancel out, the molecule is not polar. If they don't, the molecule is polar.
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Polarity of Molecules
Rule:
If all the electron regions around the central atom in a simple structure are bonds,
and
all the substituent (surrounding) atoms are the same
the molecule or ion is not polar.
In any other case, it is polar.
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Polarity of Molecules
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Polarity of Molecules
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Polarity of Molecules
Examples:
SO3 SO2
NH3 H2O
CH2O NO31