CHEMICAL NAMES AND FORMULAS naming and presentation
- 1. CHEMICAL NAMES AND FORMULAS Naming Binary Molecular Compounds
- 2. MOLECULAR COMPOUNDS Molecular compounds are inorganic compounds that take the form of discrete molecules. Examples include such familiar substances as water (H2O) and carbon dioxide (CO2). These compounds are very different from ionic compounds like sodium chloride (NaCl). Ionic compounds are formed when metal atoms lose one or more of their electrons to nonmetal atoms. The resulting cations and anions are electrostatically attracted to each other.
- 3. MOLECULAR COMPOUNDS So what holds the atoms of a molecule together? Rather than forming ions, the atoms of a molecule share their electrons in such a way that a bond forms between a pair of atoms. In a carbon dioxide molecule, there are two of these bonds, each occurring between the carbon atom and one of the two oxygen atoms
- 4. CARBON DIOXIDE Carbon dioxide molecules consist of a central carbon atom bonded to 2 oxygen atoms.
- 5. NAMING BINARY MOLECULAR COMPOUNDS Recall that a molecular formula shows the number of atoms of each element that a molecule contains. A molecule of water contains two hydrogen atoms and one oxygen atom, so its formula is H2O. A molecule of octane, which is a component of gasoline, contains 8 atoms of carbon and 18 atoms of hydrogen. The molecular formula of octane is C8H18C8H18
- 6. NAMING BINARY MOLECULAR COMPOUNDS Naming binary (two-element) molecular compounds is similar to naming simple ionic compounds. The first element in the formula is simply listed using the name of the element. The second element is named by taking the stem of the element name and adding the suffix -ide. A system of numerical prefixes is used to specify the number of atoms in a molecule.
- 7. Numerical Prefixes for Naming Binary Covalent Compounds Number of Atoms in Compound Prefix on the Name of the Element 1 mono-* 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca- *This prefix is not used for the first element’s name
- 9. Generally, the less electronegative element is written first in the formula, though there are a few exceptions. Carbon is always first in a formula and hydrogen is after nitrogen in a formula such as NH3. The order of common nonmetals in binary compound formulas is CC, PP, NN, HH, SS, II, BrBr, ClCl, OO, FF
- 10. The a or o at the end of a prefix is usually dropped from the name when the name of the element begins with a vowel. As an example, four oxygen atoms, is tetroxide instead of tetraoxide
- 11. The prefix is "mono" is not added to the first element’s name if there is only one atom of the first element in a molecule.
- 12. SOME EXAMPLES OF MOLECULAR COMPOUNDS Formula Name NO nitrogen monoxide N2O dinitrogen monoxide S2Cl2 disulfur dichloride Cl2O7 dichlorine heptoxide
- 13. Notice that the mono- prefix is not used with the nitrogen in the first compound, but is used with the oxygen in both of the first two examples. The S2Cl2 emphasizes that the formulas for molecular compounds are not reduced to their lowest ratios. The o of the mono- and the a of hepta-are dropped from the name when paired with oxide.
- 14. SIMPLE MOLECULA R COMPOUNDS W IT H COMMON NA MES For some simple covalent compounds, we use common names rather than systematic names. We have already encountered these compounds, but we list them here explicitly: H2O: water NH3: ammonia CH4: methane H2O2: hydrogen peroxide
- 15. Methane is the simplest organic compound. Organic compounds are compounds with carbon atoms and are named by a separate nomenclature system. Some Compounds Have Both Covalent and Ionic Bonds
- 16. 1. CO2 2. SO2 3. CS2 4. CF4 5. SeCl2 6. SO3 7. SF6 8. Cl2O 9. ClF 10.ClF5