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Periodic Table: Atomic Structure, Valence Electrons & Element Properties, Summaries of Chemistry

Adrian CollegeChemistry

An overview of the periodic table, explaining how elements are arranged based on atomic number, the concept of periods and groups, and the significance of valence electrons in determining the properties of elements. It also introduces the three basic categories of elements: metals, non-metals, and semi-metals or metalloids.

Typology: Summaries

2021/2022

Uploaded on 09/12/2022

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The Periodic Table
•Elements in the periodic table are arranged
according to atomic number
•Remember: atomic number determines the
identity of the element
•The horizontal rows of the elements on the
periodic table are called periods
•The columns are called groups
•The group number tells the valence electrons
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The Periodic Table

  • (^) Elements in the periodic table are arranged according to atomic number
  • (^) Remember: atomic number determines the identity of the element
  • (^) The horizontal rows of the elements on the periodic table are called periods
  • (^) The columns are called groups
  • (^) The group number tells the valence electrons

The Periodic Table

  • (^) The table is set up such that it indicates the number of electron shells in each atom
  • (^) The number of valence electrons
  • (^) As you go down the rows, the number of shells increases
  • (^) As you move from left to right in any row, the number of valence electrons increases
  • (^) So you can predict the structure of the next atom

Categories of Elements

  • (^) Elements of the periodic table belong to 3 basic categories - (^) Metals - (^) Non-metals - (^) Semi-metals or metalloids
  • (^) Majority of elements in the periodic table are considered metals
  • (^) These metals in the periodic table are divided into groups

Groups of Metals

  • (^) Alkali metals
    • (^) Group I
    • (^) Form salts and many other compounds
    • (^) Highly reactive
  • (^) Alkaline Earth metals
    • (^) Group II
  • (^) Transition metals
    • (^) Very hard
    • (^) High melting and boiling points
  • (^) Using the periodic table rows and groups one can predict a number of properties of atoms
  • (^) This is true for metals, non-metals and semi- metals
  • (^) In transition metals this simplified explanation of the properties of elements does not work

Importance of Valence Electrons

  • (^) They are electrons in the highest energy level
  • (^) They are exposed
  • (^) They are electrons that get most involved in chemical reaction
  • (^) Electron dot diagrams are used to show valence electrons
  • (^) Drawn around the symbol of the atom as if there is a square around it – with up to two dots per side

Effective Nuclear Charge

  • (^) The nuclear charge felt by the valence electrons after you have taken into account the number of shielding electrons surrounding the nucleus
  • (^) Let us take an example of Beryllium:
  • (^) The nucleus itself has a +4 charge and anything near to it feels that charge
  • (^) The two electrons in the first energy level feel that charge
  • (^) The electrons that are in the valency energy level would be shielded from the nucleus by the two first energy level electrons - (^) The +4 nuclear charge is shielded by 2 electrons - (^) That gives and effective nuclear charge of +2 felt by valency electrons