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Covalent Bonds
Chapter 5 Section 3
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Covalent Bonds
Remember…covalent bonds form between two nonmetals
The bonds form when electrons are shared between atoms, not transferred
This happens because neither atom will take the electrons from the other, they attract them at the same time.
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Single Bonds
Ionic compounds only form single bonds when there are a pair of electrons between atoms
This molecule has 5 single bonds
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Single and Double/Triple Bonds
Covalent (molecular) compounds can form single, double, and triple bonds
Each bond has a pair of electrons between atoms
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Single and Double/Triple Bonds
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Covalent Bonds
The electrons are sometimes shared equally when the same element bonds with itself (BrINClHOF). This is called a nonpolar bond.
Sometimes they are shared unequally when one atom is slightly stronger than the other. This is called a polar bond.
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Covalent Bonds
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Properties of Molecular Compounds
Some form crystal shapes, most do notLow melting points compared to ionic
compoundsDo not conduct electricity in solution
(dissolved in water)
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Writing Covalent Formulas
Use the same procedure as for ionic formulas
Example: C Br C4+ Br1-
CBr4
Example: N S N5+ S2-
N2S5
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Naming Covalent Formulas
Use the same procedure as for ionic formulas
Add Latin prefix that matches the subscript for the element to each part of formula name1= mono 6= hexa
2= di 7= hepta
3= tri 8= octa
4= tetra 9= nona
5= penta 10= deca
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Naming Covalent Formulas
Example: CBr4
Carbon tetrabromideN2S5
Dinitrogen pentasulfideH2O
Dihydrogen monoxideCO2
Carbon dioxide