Molecular Compounds - Sciencepoint Cafe
Transcript of Molecular Compounds - Sciencepoint Cafe
Oct. 21, 2008
Review of Ionic Compounds
• Ionic compounds form when ions come together to balance out their overall charge.
• This way the atoms have a complete outer shell and have an overall charge of zero.
BUT, there is another way to attain a complete outer shell AND an overall charge of zero …
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Molecular Compounds
• Involve COVALENT BONDS (instead of Ionic Bonds)
• Electrons of neutral non-metal atoms are shared to form a molecule.
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Another Familiar Example • In order to create pure Water (H2O), Hydrogen
and Oxygen form covalent bonds by sharing electrons.
H
H
O
H
H
O
Both the Hydrogen and the Oxygen remain electrically neutral, AND have been able to completely fill their outer valence shell.
Shared electrons
Oct. 21, 2008
Formulas for Molecular Compounds
• The Combining Capacity is the number of covalent bonds that an atom would need to form a stable molecule.
H
H
O
H
H
O
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Example • Carbon has four electrons in its outer valence.
• It would need to share 4 more electrons with other atoms in order to fill its outer valence.
• Therefore it has a combining capacity of 4.
C
H
H
H
H
The molecule produced is Methane
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Chemical Formula
• Follow the same “shortcut” steps used for Ionic Compounds
• Use the COMBINING CAPACITY instead of the ionic charge.
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Example • How would you write the formula for a
compound formed between carbon and sulfur?
C S
1. Write the symbols for the two elements. Which one is written first this time?
2. Write the combining capacity of each element above the symbol.
4 2
3. Crisscross the combining capacity to produce subscripts.
The formula is C2S4
4. Reduce the subscripts if possible.
The correct formula is CS2
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Naming for Molecular Compounds
• Molecular compounds use prefixes to indicate the number of atoms in a molecule.
Prefix Number Example (formula)
mon(o) 1 carbon monoxide
di 2 carbon disulfide
tri 3 sulfur trioxide
tetra 4 carbon tetrafluoride
pent(a) 5 phosphorus pentabromide
CO
CS2
SO3
CF4
PBr5
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Practice
• Write the names for: – CO2
– PF3
– As2S3
• Write the formulas for: – Sulfur dichloride
– Boron triiodide
– Diphosphorus tetraoxide