Naming Compounds 1. Molecules and Molecular Compounds (Covalent Compounds) Two or more atoms tightly...
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Transcript of Naming Compounds 1. Molecules and Molecular Compounds (Covalent Compounds) Two or more atoms tightly...
Molecules and Molecular Compounds (Covalent Compounds)
•Two or more atoms tightly bound together •Bond by a covalent bond – the sharing of electrons
•Usually nonmetals bonded to other nonmetals
•Elements found in nature in molecular form – N2, O2, F2, Cl2, Br2, I2, H2
• Aka diatomic elements
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•Molecular formulas – indicate actual numbers of and types of atoms in a molecule
•Term “molecule” refers only to covalently bonded substances.
•Empirical formulas – smallest possible whole number subscripts
•Use the Greek prefixes to name binary covalent compounds
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Prefixes Used in Naming Molecular Compounds
Number Prefix
1 mono-
2 di-
3 tri-
4 tetra-
5 penta-
6 hexa-
7 hepta-
8 octa- ExampleGive the chemical formula for the following: silicon tetrachloride
disulfur dichloride
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Ions and Ionic Compounds(Formula Units)
•Ion – formed when electrons are added or removed from an atom
•Cation – ion with a positive charge – typically metals
•Anion – ion with a negative charge – typically non-metals
•Ionic Compounds are always a metal bonded to a metal
•Compounds formed when cations and anions are attracted to each other
•Formed by the transfer of electrons 5
Naming Ionic Compounds
•Cations – (the metals) – have the same name as the metal
•Must use roman numerals if dealing with a metal that can have more than one charge – i.e. the transition metals
•One-atom anions – (the nonmetals) – • Their ending changes to –ide
e.g. NaCl is sodium chloride
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ExampleGive the chemical formula for the following:
magnesium sulfate
silver sulfide
lead(II)nitrate
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Naming acids
I –ate it and it was –ic
I caught –ite –ous
Binary AcidsHydro ……. -ic
ExampleGive the formulas for the following:
1. hydrobromic acid
2. carbonic acid
3. Sulfurous acid
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