6.2 covalent bonds
TRANSCRIPT
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6.2 Covalent Bonding
Covalent Bonding
You Will Need:iNotebookAt least 2pgs of CN
Agenda:Covalent Bonding LectureChemical Bonding VideoChemical Bonding QuizCovalent Bonding Wksht
Opener:
What is the difference between an anion and a cation?
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6.2 Covalent Bonding
How are atoms held together in a covalent bond?
Covalent Bonds
The attractions between the shared electrons and the protons in each nucleus hold the atoms together in a covalent bond.
A covalent bond is a chemical bond in which two atoms share a pair of valence electrons.
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6.2 Covalent Bonding
Sharing Electrons
When two atoms share one pair of electrons, the bond is called a single bond.
Covalent Bonds
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6.2 Covalent Bonding
Molecules of Elements
Two hydrogen atoms bonded together form a unit called a molecule.
A molecule is a neutral group of atoms that are joined together by one or more covalent bonds.
Covalent Bonds
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6.2 Covalent Bonding
Multiple Covalent Bonds
When two atoms share three pairs of electrons, the bond is called a triple bond. When two atoms share two pairs of electrons, the bond is called a double bond.
Each pair of shared electrons is represented by a long dash in the structural formula NN.
Covalent Bonds
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6.2 Covalent Bonding
When atoms form a polar covalent bond, the atom with the greater attraction for electrons has a partial negative charge. The other atom has a partial positive charge.
Unequal Sharing of Electrons
The type of atoms in a molecule and its shape are factors that determine whether a molecule is polar or nonpolar.
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6.2 Covalent Bonding
A covalent bond in which electrons are not shared equally is called a polar covalent bond.
Unequal Sharing of Electrons
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6.2 Covalent Bonding
Shared electrons in a hydrogen chloride molecule spend less time near the hydrogen atom than near the chlorine atom.
Unequal Sharing of Electrons
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6.2 Covalent Bonding
How do attractions between polar molecules compare to attractions between nonpolar molecules?
Attraction Between Molecules
Attractions between polar molecules are stronger than attractions between nonpolar molecules.