Chemical Names and Formulas

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Chemical Names and Formulas

• By Philip Wolf, Tom Rains,
• Stacey Shank, and Aubrey Chester

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Table of Contents

• Periodic table
• J.J. Berzelius
• Naming ions
• Nomenclature
• Binary compounds
• Polyatomic
• Acids
• Oxidation number
• Chemical formulas
• Laws

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Periodic Table

• Period- a horizontal row which consists of seven
  different rows, in order of atomic mass from
  least to the greatest.

• Group- vertical column with three different types
  of elements.
• Metals- left side of the periodic table. Ex. (Sn)
  tin
• Nonmetals- right side of periodic table. (H)
  Helium
• Metalloids- along the staircase on the periodic
  table. (B) Boron

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Periodic Table (continued)

• Consists of two main groups
• Main group elements- the elements in groups 1,
  12, and 13-18.
• Transition group elements- elements that are
  within groups 3-12.

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J.J. Berzelius

• Berzelius was a Swedish chemists who created the
  modern symbols for elements.
• Berzeliuz developedthe ion and ionic co-mpound
  concepts.
• He is known as the father of chemistry.
• More on Berzelius

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Naming Ions

• Mono-atomic anions are named by adding ide to
  the end of an element name after dropping the
  ending off of the elements original name.
• Ex. H-1 Hydride ion

• Mono-atomic cations are named by just simply
  using the elements name.
• Ex. H1 Hydrogen ion
• More on Ions

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Naming Anions

• Anion- term used to describe a negatively charged
  ion.
• Anions always have the same charge, the charge is
  written as a superscript on the right, and to
  change an element to an anion, the ending ide
  must be added.

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Nomenclature

• Nomenclature- rules for naming compounds. Binary
  ionic, Binary covalent (molecular), Polyatomic
  ionic, or Acidic based ionic are the
  possibilities for naming a compound.
• More on nomenclature

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Binary Ionic

• Two monatomic ions, cation name is the element
  name, anion name ends with ide, cations with
  multi charges use Roman numerals in naming.
• Ex. FeCl3 Iron (III) chloride

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Binary Covalent (Molecular)

• Two nonmetals, first element name is same, second
  element name ends with an ide, and prefix is
  used to represent the number of atoms.
• Ex. CO2 Carbon Dioxide

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Polyatomic Ionic

• Many atoms with a collective charge and most are
  called oxyanions.
• Ex. Al(OH)3 Aluminum Hydroxide
• Ex2. Ca(NO3)2 Calcium Nitrate

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Acids

• Contains a free H1 ion in water, naming based on
  oxygen.
• Binary Acid
• Name starts with hydro- and ends with ic
• Some positive elements may have more than one
  positive charge, so they may form more than one
  compound with an element.
• Note this difference by writing the oxidation
  number of positively charged element as a Roman
  numeral in parentheses.
• Ex. H3P Hydrophosphoric acid

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Oxidation Number

• Chemists have determined ration in which most
  elements combine.
• Ratios depend on structure of the atom.
• When atom reacts to form ion, stability of the
  octet of electrons allows prediction of number of
  electrons gained or lost.
• More on oxidation number

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Oxidation Number (Continued)

• You can then predict the charge of ion formed.
• When single ion takes on a charge, it is called a
  monatomic ion.
• Charge of this monatomic ion is called oxidation
  number, the ion ends with ide.

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Chemical Formulas

• Three main parts
• Writing formulas
• Properties of chemical formulas
• Laws

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Writing Formulas

• Atom made of more than one atoms is called a
  polyatomic ion.
• A way to determine ratio of elements or
  polyatomic ions in a compound is to add the
  charges algebraically. If charges add up to
  zero, the formula is written correctly.

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Properties of Chemical Formulas

• Shows the kind and number of atoms in the
  smallest piece of a substance.
• Molecular formula, number, and kinds of atoms in
  a molecule CO2C6H12O6
• If there is more than one atom, use a subscript.
  Ex. H2O

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Properties of Chemical Formulas (Cnt.)

• There are seven diatomic elements
• Hydrogen (H2)
• Nitrogen (N2)
• Oxygen (O2)
• Fluorine (F2)
• Chlorine (Cl2)
• Bromine (Br2)
• Iodine (I2)

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Laws

• Law of definite proportions
• The elements composing a compound are always
  found in the same ratio by mass.
• Law of multiple proportions
• The masses of one element that combine with a
  fixed amount of another element to form more that
  one compound are in the same ratio of small,
  whole numbers.
• More on Laws