chemical bonding i. introduction to bonding. 2.4.1 define chemical bond 2.4.2 explain why most atoms...
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Chemical Bonding
I. Introduction toBonding
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2.4.1 Define chemical bond
2.4.2 Explain why most atoms form chemical bonds.
2.4.3 Describe ionic and covalent bonding.
2.4.4 Classify bonding type according to electronegativity differences
2.4.5 Define molecule and molecular formula.
OBJECTIVES OBJECTIVES
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Review
We can also predict what ions an element will form.
+1
+2 +3
+/-
4 -3 -2 -10
multiple cations
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Vocabulary
Chemical Bond
electrical attraction between nuclei and valence e- of neighboring atoms that binds the atoms together
bonds form in order to…increase stability
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Vocabulary
Octet Rule:Atoms will transfer or share electrons in order to have 8 electrons in their highest energy level.
• This makes it like a noble gas
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Vocabulary
CHEMICAL FORMULA
MolecularFormula
FormulaUnit
IONIC COVALENT
COCO22NaClNaCl
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Vocabulary
COMPOUND
TernaryCompound
BinaryCompound
2 elementsmore than 2
elements
NaNONaNO33NaClNaCl
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Vocabulary
ION
PolyatomicIon
MonatomicIon
1 atom 2 or more atoms
NONO33--NaNa++
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IONIC COVALENTBond Formation
Type of Structure
Solubility in Water
Electrical Conductivity
OtherProperties
e- are transferred from metal to nonmetal
high
yes (solution or liquid)
yes
e- are shared between two nonmetals
low
no
usually not
MeltingPoint
crystal lattice true molecules
Types of Bonds
Physical State solid liquid or gas
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“electron sea”
METALLICBond Formation
Type of Structure
Solubility in Water
Electrical Conductivity
OtherProperties
MeltingPoint
Types of Bonds
Physical State
e- are delocalized among metal atoms
very high
yes (any form)
no
malleable, ductile, lustrous
solid
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Quick Hint
All All covalent bondscovalent bonds are between are between two non-metalstwo non-metals
All All ionic bondsionic bonds are between a are between a metalmetal (cation) and a (cation) and a nonmetalnonmetal (anion). (anion).
All All metallic bondsmetallic bonds are between are between two metalstwo metals
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Lewis Structure
Covalent – show sharing of electronsIonic – show transfer of electrons
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Lewis Structures
Covalent – show sharing of electronsIonic – show transfer of electrons
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Ionic Nomenclature – Ionic Formulas
Write each ion, cation first. Don’t show charges in the final formula.
Overall charge must equal zero. If charges cancel, just write symbols. If not, use subscripts to balance charges.
Use parentheses to show more than one polyatomic ion.
Stock System – Roman numerals indicate the ion’s charge
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Ionic Nomenclature – Ionic Names
Write the names of both ions, cation first.
Change ending of monatomic ions to –ide.
Polyatomic ions have special names.
Stock System – Use Roman numerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.
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Ionic Nomenclature
Consider the following: Does it contain a polyatomic ion?
-ide, 2 elements no-ate or –ite, 3+ elements yes
Does it contain a Roman numeral?Check the table for metals not in Groups 1 or 2.
No prefixes.
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Ionic Nomenclature
Potassium chloride K+ Cl- KCl
Magnesium nitrate Mg2+ NO- Mg(NO3)2
Copper (ii) chloride Cu2+ Cl- CuCl2
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Ionic Nomenclature
NaBr Sodium bromide
Na2CO3
Sodium carbonate
FeCl3 Iron (III) chloride
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Covalent Bonding
• Covalent bonds can have multiple bonds.• Single Covalent Bond
– Chemical bond resulting from sharing of an electron pair between two atoms
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Double Covalent Bond Chemical bond resulting from sharing of
two electron pairs between two atoms
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Triple Covalent Bonds Chemical bond resulting from sharing of
three electron pairs between two atoms
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Molecular Nomenclature
Prefix System (Binary system)
1.Less electronegative atom comes first.
2.Add prefixes to indicate number of atoms. Omit mono- prefix on first element.
3.Change the ending of the second element to –ide.
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Molecular Nomenclature Prefixes
Mono- 1Di- 2Tri- 3Tetra- 4Penta- 5
Hexa- 6Hepta- 7Octa- 8Nona- 9Deca- 10
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Molecular Nomenclature
CCl4 Carbon tetrachloride
N2O
Dinitrogen monoxideSF6
Sulfur hexaflouride
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Molecular Nomenclature
Arsenic trichloride AsCl3
Dinitrogen monoxide N2O5
Tetraphosphorus decoxide P4O10
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Bond Polarity
Most bonds are a blend of ionic and covalent characteristics.
Differences in electronegativity determines bond type.
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Bond Polarity
Electronegativity Attraction an atom has for a shared pair
of electrons. higher e-neg atom -
lower e-neg atom +
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Dipole Movement
Dipole Moment - a measure of the polarity of a bond. Is often represented by a special arrow. Arrow points to more EN atom.
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Bond Polarity
Electronegativity Trend (p. 151) Increases up and to the right.
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Nonpolar Covalent Bond e- are shared equally symmetrical e- density usually identical atoms
Bond Polarity
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+ -
Bond Polarity
Polar Covalent Bond e- are shared unequally asymmetrical e- density results in partial charges (dipole)
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Bond Polarity
Ionic Bond e- are not shared results in charged particles opposite charges attract
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Determining Type, EN0.3
1.7
5% 50%
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Determining Type, EN
Ionic, Polar or Nonpolar Covalent Compounds: The difference in electronegativity between bonding atoms leads to the type of compound.
Example:O2 , O=O ENO = 3.5 EN = 0 NO , N=O ENN = 3.0, ENO = 3.5 EN = .5 CO , C= ENC = 2.5, ENO = 3.5 EN = 1.0 NaCl , Na+Cl- ENNa = 0.9, ENCl = 3.0 EN = 2.1
Nonpolar Covalent
Polar Covalent
Ionic
Polar Covalent
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Sample Problem
Use electronegativity differences to classify bonding between sulfur, S, and the following elements: hydrogen, H; cesium, Cs; and chlorine, Cl. In each pair, which atom will be more negative?Bonding between sulfur and
Electronegativity difference Bond
type
More-negative atom
hydrogen 2.5 – 2.1 = 0.4 Polar-covalent
sulfur
cesium 2.5 – 0.7 = 1.8 Ionic sulfur
chlorine 3.0 – 2.5 = 0.5 Polar-covalent
chlorine
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Additional Sample Problems
Complete the following chart:
Elements bonded
Electronegativity difference Bond
type
More-negative atom
a. C and H 2.5 – 2.1 = 0.4 Polar-covalent
carbon
b. C and S 2.5 – 2.5 = 0 Nonpolar covalent
Same electronegativityc. O and H 3.5 – 2.1 = 1.4 Polar-
covalentoxygen
d. Na and Cl
3.0 – 0.9 = 2.1 Ionic chlorine
e. Cs and S
2.5 – 0.7 = 1.8 Ionic sulfur