Part 1: Covalent Bonds And Molecules. Objectives Explain what a covalent bond is and what type of...
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Transcript of Part 1: Covalent Bonds And Molecules. Objectives Explain what a covalent bond is and what type of...
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Part 1: Covalent BondsAnd Molecules
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Objectives
• Explain what a covalent bond is and what type of elements form them
• Describe how molecules with covalent bonds are named
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Octet Rule
• Atoms want to achieve a noble gas electron configuration – s2p6 – 8 valence electrons in dot structure
• Exception is hydrogen wants to have two valence electrons to be like helium (“duet rule”)
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Ionic Compounds• Ex.) NaCl• Na achieves octet rule by losing 1
electron and Cl achieves octet rule by gaining 1 electron
• Valence electrons get transferred from metal to nonmetal
• Ionic compounds contain ions (cation + anion) held together by ionic bonds
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• Some nonmetals are unlikely to lose or gain electrons
• Ex. Nonmetal elements in Group 4 have four electrons in their outer levels
• To gain or lose four electrons is highly unlikely due to their protons’ attraction
Covalent Bonds
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Molecular Compounds
• Ex.) H2O• No ions!!!• All atoms are held together by
covalent bonds• Electrons get shared so the octet
rule can be met for all atoms• Two non-metals
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• The stable attraction that forms between nonmetal atoms when they share electrons is known as a covalent bond • The neutral particle that forms due to electron sharing is called a molecule
• Use Lewis Dot structures for clarity
Covalent Bonds
A water molecule
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• A single covalent bond is made up of two shared electrons
• A water molecule containstwo single bonds in which each atom contributes one electron to the other in the bond• The result: a stable outer energy level for each atom in the molecule:
• 2 for H and 8 for O
Covalent Bonds
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Molecule Example (water)
Molecule- Smallest part of molecular compound held together by covalent bonds
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• A covalent bond also can contain more than one pair of electrons
• An example of this is the bond in oxygen (O2) or nitrogen (N2)
Covalent Bonds
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Molecular Formula
Structural Formula
Molecule Representation
H2O
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Naming Molecular (Covalent) Compounds
• No molecular compounds will ever contain metals or contain ions
• You need to forget about charges when naming molecular compounds
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Rules for Naming Molecular Compounds
1. Use full name of first element2. Second element uses the “root” name of
the element + the “ide” suffix. 3. Use hydrate prefixes to denote how many
atoms of each are in the compound.Ex.) CO2 = Carbon dioxide
4. Prefix “mono” is never used in front of the 1st element and the 2nd element only uses the prefix “mono” if it is oxygen. Ex.) carbon monoxide
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Examples of Naming Molecules…
• OF2
• CO• NH3
• P2I5
• H2O
• Oxygen difluoride• Carbon monoxide NOT
monooxide• Nitrogen trihydride• Diphosphorus pentiodide (drop
“a” from penta)• Dihydrogen monoxide
• NONE OF THESE COMPOUNDS CONTAIN METALS!!!
• HYDROGEN = NOT A METAL!!!
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Objectives
• Explain what a covalent bond is and what type of elements form them
• Describe how molecules with covalent bonds are named
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