Chemical compounds nomenclature
Download
1 / 33

Chemical Compounds Nomenclature - PowerPoint PPT Presentation


  • 149 Views
  • Uploaded on

Chemical Compounds Nomenclature. All things have names, chemical compounds included. But whereas two people can have the same name, no two chemicals can have the same name.

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha
Download Presentation

PowerPoint Slideshow about ' Chemical Compounds Nomenclature' - aldon


An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
Chemical compounds nomenclature
Chemical Compounds Nomenclature


  • All things have names, chemical compounds included. But whereas two people can have the same name, no two chemicals can have the same name.

  • The system of chemical nomenclature will allow you to give any chemical its proper name and you will also be able to write the correct chemical formula.


Elements
Elements whereas two people can have the same name, no two chemicals can have the same name.

  • Most elements do not exist in nature in their pure form, as elements. Gold, Silver, and Platinum are three metals that can be found in the Earth’s crust as elements. They are called precious elements because their occurrence is so rare.

  • There are only 90 naturally occurring elements. Most of these elements are found in nature, only as compounds. Elements combine in may different ways to form the astonishing variety of natural and synthetic compounds that you see and use everyday.



Chemical and common names
Chemical and Common Names state. These elements are called diatomic molecules.


  • Because there are so many compounds, chemists have developed a classification system to organize them according to their properties (melting point, boiling point, hardness, conductivity, and solubility).

  • Based on their physical properties, compounds can be classified into two groups: ionic compounds and covalent compounds.


  • Ionic compounds and covalent compounds display distinct physical properties because of chemical bonding.

  • Bonding involves the interaction between the valence electrons of atoms.

  • Usually a the formation of a bond between atoms creates a compound that is more stable than either of the two atoms on their own.


Naming ions
Naming Ions physical properties because of chemical bonding

  • Naming monoatomic cations

    • To name a monoatomic cation, write the name of the element and add the word “ion” to it.

      • Be2+ is called the Beryllium Ion

  • Naming monoatomic anions

    • To name a monoatomic anion, write the name of the element and change the ending to ide. You can also include the word ion, but it is not necessary.

      • N3- is called Nitride (ion)


  • Transition metals
    Transition Metals physical properties because of chemical bonding

    • All of the transition elements form cations (positive ions).

    • To name a transition metal, write the name of the element then use a Roman numeral to identify the charge. Follow that with the word ion.

      • Fe1+ is the Iron (I) ion

      • Fe2+ is the Iron (II) ion

      • Fe3+ is the Iron (III) ion


    Polyatomic ions
    Polyatomic Ions physical properties because of chemical bonding

    • Polyatomic Ions are tightly bound groups of atoms that behave as a unit.

    • Use the chart provided to name a polyatomic ion.

      • (PO4)3- is the phosphate ion

      • (ClO2)- is the chlorite ion


    Compounds physical properties because of chemical bondingcan be divided into two basic categories, those which are true binary compounds (contain only two types of elements), and those which contain more than two different types of elements.


    Naming ionic compounds
    Naming Ionic Compounds: physical properties because of chemical bonding

    Monoatomic or simple ions

    Single atoms that have lost or gained one or more electrons

    Form binary ionic compounds (2 simple ions)

    Consist of cations and anions

    Eg. Sodium + chlorine Na+ Cl-


    Cations are written first, anions are second (name changes to “-ide” for the anion)

    The total charge must be zero

    Do not write charges in your final answer


    Writing formulas for ionic compounds
    Writing Formulas for Ionic Compounds to “-ide” for the anion)

    • In binary ionic compounds, the total number of positive charges must equal the total number of negative charges. Basically, the overall charge must be zero.

    • When writing binary ionic formulas, the cation always goes first.


    K to “-ide” for the anion)1+ and Br 1-

    Ca2+ and S2-

    Ca2+ and Cl1-

    Na1+ and P3-

    Fe3+ and O2-

    Form KBr

    Form CaS

    Form CaCl2

    Form Na3P

    Form Fe2O3


    The trick
    The Trick!! to “-ide” for the anion)

    • Write down the ions

    • Take the charge of the cation (just the number) and write it as the subscript on the anion.

    • Take the charge of the anion (just the number) and write it as the subscript on the cation.

    • This is called the cross over rule!

    • It works for polyatomic ions as well!


    Steps for writing binary ionic formulas when given the name
    Steps for Writing Binary Ionic Formulas When Given the Name to “-ide” for the anion)

    • Write the symbol for the elements involved with their charges. You can determine the charge based on their position on the periodic table;

      • Group 1 is 1+ - Group 5 is 3-

      • Group 2 is 2+ - Group 6 is 2-

      • Group 3 is 3+ - Group 7 is 1-

      • Group 4 is + or – 4 - Group 8 is 0

    • Once you have the symbols with the charges, combine the ions to make the formula.


    Examples
    Examples to “-ide” for the anion)

    • Sodium Oxide

      • Na1+ and O2-

        • Na2O

  • Calcium Phosphide

    • Ca2+ and P3-

      • Ca3P2

  • Iron (III) Sulfide

    • Fe3+ and S2-

    • Fe2S3

  • Calcium Nitrate

    • Ca2+ and NO3-

    • Ca(NO3)2


  • Naming binary ionic compounds
    Naming Binary Ionic Compounds to “-ide” for the anion)

    • A compound is an inorganic compound that contains two elements.

    • Binary compounds may contain a metal and a non metal. These would be binary ionic compounds.

    • To name a binary ionic compound, name the cation first and then the anion.


    Examples1
    Examples to “-ide” for the anion)

    • CaS

      • Calcium ion

      • Sulfide ion

        • Calcium Sulfide

  • BeCl2

    • Beryllium ion

    • Chloride ion

      • Beryllium Chloride


  • Rules for formulas
    Rules for formulas: to “-ide” for the anion)

    Write the symbols for the ions involved

    eg. Silver and chlorine

    Ag+ and Cl-

    Determine the lowest whole number ratio of ions which will provide an overall net charge of zero

    Ag1+ Cl1- becomes AgCl (silver chloride)


    Example potassium and oxygen
    Example: potassium and oxygen to “-ide” for the anion)

    potassium - K+

    oxygen - O2-

    K2+ O12-

    becomes K2O potassium oxide


    Naming ionic compounds1
    Naming Ionic Compounds to “-ide” for the anion)

    Cation is named first

    Anion is named second

    Ending of anion is changed to “ide”

    Practice:

    NaCl BaCl2 Al2O3


    Multivalent ions
    Multivalent ions to “-ide” for the anion)

    - certain transition metals can form more than one type of ion, each with a different charge.

    • eg. Cu2+ - copper (II)

      Cu+ - copper (I)


    Multivalent ions continued
    Multivalent ions (continued) to “-ide” for the anion)

    • The transition metals have various electron configurations that will make them stable

    • Use a roman numeral after the cation to specify its charge (Stock naming system).

    • Eg. Iron (ii) oxide FeO

      Iron (iii) oxide Fe2O3


    Stock vs classical
    Stock vs. Classical to “-ide” for the anion)

    FormulaStock NameClassical Name

    Cu+ copper(I) ion Cuprous ion

    Cu2+ copper(II) ion Cupric ion

    Fe2+ iron(II) ion Ferrous ion

    Fe3+ iron(III) ion Ferric ion


    Fe to “-ide” for the anion)2+ so this is Iron (II) oxide

    • FeO

      • Iron ion

      • Oxide ion

        • Iron oxide

  • Fe2O3

    • Iron ion

    • Oxide ion

      • Iron oxide

  • No two compounds can have the same name, so the charge on the cation is included in the name as a Roman Numeral.

  • Fe3+ so this is Iron (III) oxide


    Naming of polyatomic compounds
    Naming of Polyatomic Compounds to “-ide” for the anion)

    • Identify the cation and the anion. (Use the polyatomic chart to identify the polyatomic ion).

    • Mg(NO3)2

      • Magnesium ion

      • Nitrate ion

        • Magnesium Nitrate


    • (NH to “-ide” for the anion)4)2(CO3)

      • Ammonium ion

      • Carbonate ion

        • Ammonium carbonate

  • Fe3(PO4)

    • Iron (I) ion

    • Phosphate ion

      • Iron (I) phosphate


  • Summary of ionic bonding
    Summary of Ionic Bonding… to “-ide” for the anion)

    • You have learned what happens when the EN difference between atoms is greater than 1.7 – you get an ionic bond.

    • The atom with the higher EN gains the electrons from the atoms with the lower EN, causing the atoms to become charged.

    • Oppositely charged ions attract and that is how the ionic bond is formed.


    Naming molecular compounds
    Naming Molecular Compounds: to “-ide” for the anion)

    Use prefixes to specify number of atoms of each element in the molecule

    Second element ends with “-ide”

    No charges used in formula

    The prefix “mono-” should not be used on the first element

    • mono

    • di

    • tri

    • tetra

    • penta

    • hexa

    • hepta

    • octa

    • nona

    • deca


    Exceptions
    Exceptions to “-ide” for the anion)

    • The prefix “mono” is attached to the name of the second element in the molecule when there is only one atom of that element present.

    • It is not used in the name if the first element if there is only one atom of that element present.


    Examples2
    Examples to “-ide” for the anion)

    • N2O5

      • 2 N is dintrogen

      • 5 O is pentaoxide

        • Dinitrogen pentaoxide

  • SF6

    • 1 S is monosulfur, except it is first, so just sulfur

    • 6 F is hexafluoride

      • Sulfur hexafluoride


  • ad