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Naming Ionic Compounds

Ionic Nomenclature, or. Naming Ionic Compounds. Ionic Compound Nomenclature. Naming ionic compounds is normally straight forward. We need to focus on the two parts of the compound: The cation and the anion. Decisions, decisions.

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Naming Ionic Compounds

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  1. Ionic Nomenclature, or Naming Ionic Compounds

  2. Ionic Compound Nomenclature • Naming ionic compounds is normally straight forward. We need to focus on the two parts of the compound: The cation and the anion.

  3. Decisions, decisions • When naming chemical compounds, one of the first things that needs to be done is to identify whether they are ionic or covalent in nature. • Remember, ionic compounds will contain a cation and an anion. The cation will come first in the formula and is usually a metal, so watch for that. • If you see no metal, then it is likely covalent. • Each of these types of compounds have slightly different naming rules.

  4. Naming the cation • In naming the cation, there is no change in the standard name of the metal. This is because metals usually have known charges, so we often do not need any more information. • So, the sodium ion (Na+) is simply named ‘sodium’. • Magnesium ions (Mg2+) are simply named ‘magnesium’. • An aluminum ion would be simply ‘aluminum’.

  5. Naming the cation, extended • The metals in groups 1, 2 and 13 typically have only one common charge. However, many transition metals, and even metals in groups 13 and 14 towards the bottom of the table can have more than a single charge available to them. • For these particular metals, we need to give more information than just the name. We also need to identify which charge the ion has.

  6. Naming the cation, extended II • To identify the charge, we write a roman numeral in parenthesis after the name of the metal. The roman numeral tells us the charge. • For example, iron has two common charges, 2+ and 3+, so we would name these as ‘Iron (II)’ (Fe2+) and ‘Iron (III)’ (Fe3+). • The most common metals that we will use are the two forms of iron, copper (I) and (II), gold (I) and (III), tin (II) and (IV), lead (II) and (IV), and nickel (II) and (III).

  7. Naming the anion • Naming anions is fairly straightforward as well. We need to know if the anion is made from a single element or is a ‘complex’ ion made of two or more elements covalently bonded together.

  8. Single element anions • Single element anions are named by taking the root of the element and changing the ending to ‘ide’. • Since most non-metal anions have a single common charge, we do not need any more information than the identity of the element. • Examples: ‘oxygen’ becomes ‘oxide’. ‘chlorine’ becomes ‘chloride’. ‘nitrogen’ becomes ‘nitride’.

  9. Complex anions • The nice thing about complex ions is that they have their own names, so you do not have to change a thing. • Most complex anions have an ending other than ‘ide’. Two important exceptions are ‘hydroxide (OH-)’ and ‘peroxide (O22-)’. • Most other complex ions end with either ‘ate’ or ‘ite’. • Examples: ‘nitrate (NO3-)’, ‘nitrite (NO2-)’ ‘sulfate (SO42-)’, ‘carbonate (CO32-)’, and ‘chlorite (ClO2-)’

  10. Examples – binary (2 elements) • Here are some binary ionic formulas. See if you can name them. CationAnion Sodium Magnesium Aluminum Calcium Iron (III) Copper (I) Chloride Oxide Fluoride Nitride Bromide Oxide • NaCl • MgO • AlF3 • Ca3N2 • FeBr3 • Cu2O

  11. Examples – polyatomic ionic • Here are some more complex ionic formulas. See if you can name them. CationAnion Sodium Magnesium Aluminum Calcium Iron (III) Copper (I) nitrate sulfate hydroxide carbonate chlorite carbonate • NaNO3 • MgSO4 • Al(OH)3 • CaCO3 • Fe(ClO2)3 • Cu2CO3

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