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Understanding Electron-Dot Notation and Valence Electrons in Atoms

This guide explains the concept of electron-dot notation, focusing on the distinction between valence and non-bonding electrons in atoms. It details how only the outermost electrons, known as valence electrons, participate in bonding, while inner electrons do not. The guide also covers the periodic table's groupings concerning valence electron counts, the formation of cations and anions, and how to predict ion formation. Diagrams for electron-dot representations of ions and periodic modifications are included for clarity.

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Understanding Electron-Dot Notation and Valence Electrons in Atoms

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  1. Depicting Electrons ELECTRON-DOT NOTATION

  2. Atoms consist of inner and outer electrons. • Only the outermost electrons in an atom can participate in bonding. • Called valence electrons. • The inner electrons do not participate in bonding. • Called non-bonding electrons. Inner & Outer Electrons

  3. Each group on the periodic table has a set number of valence electrons. • Group 1 elements have 1 valence electron. • Group 2 elements have 2 valence electrons. • Group 13 elements have 3 valence electrons. • Group 14 elements have 4 valence electrons. • Group 15 elements have 5 valence electrons. • Group 16 elements have 6 valence electrons. • Group 17 elements have 7 valence electrons. • Group 18 elements have 8 valence electrons. Determining Number of Valence Electrons

  4. Depiction of the valence electrons of an atom. • Valence electrons are represented as dots surrounding the elemental symbol. • Fill in the blank periodic table with electron-dot notations. USE PENCIL. Electron-Dot Notation

  5. Ions form when atoms gain or lose electrons. • Cations form when electrons are lost. • Positively charged. • Charge is determined by number of electrons lost. • Anions form when electrons are gained. • Negatively charged. • Charge is determined by number of electrons gained. • Octet rule: atoms will gain or lose electrons so that they have 8 valence electrons. Ions

  6. Atoms with fewer than four valence electrons will lose electrons to form cations. • A group 1 atom will lose 1 electron to form a 1+cation. • A group 2 atom will lose 2 electrons to form a 2+cation. • A group 13 atom will lose 3 electrons to form a 3+cation. • Atoms with more than four valence electrons will gain electrons to form anions. • A group 15 atom will gain 3 electrons to form a 3- anion. • A group 16 atom will gain 2 electrons to form a 2- anion. • A group 17 atom will gain 1 electron to form a 1- anion. Predicting Ions

  7. Certain groups do not form ions. • Group 14 (carbon group). • Group 18 (noble gases). Predicting Ions

  8. Cation formation: • Remove the number of electrons appropriate for the group. • Charge is positive and equal to the number of electrons lost. • Anion formation: • Add the number of electrons appropriate for the group. • Charge is negative and equal to the number of electrons gained. • Edit your periodic table to show ion formation by removing or adding electrons to the electron-dot notation. Be sure to indicate the charge of the ions. Electron-Dot Notation of Ions

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