Valence Electrons & Ionic Compounds (College Board AP Chemistry)

• Valence electrons are the electrons present in the outermost shell of an atom
• Valence electrons dictate an atom's reactivity and ability to form bonds
• The number of valence electrons can be obtained from the electron configuration of an atom

The Beryllium Atom

Beryllium electron configuration and valence electrons

• The interactions between the valence electrons and nuclei of elements determine if two elements are likely to form a chemical bond
• There are two types of chemical bonds depending on the elements that take part in the bonding process: ionic bond and covalent bond
  • An ionic bond occurs between a metal and a nonmetal
  • A covalent bond occurs between two nonmetals

Valence Electrons and the Periodic Table

• Elements in the same group (columns) of the periodic table have the same number of electrons in their valence shell
• The valence electrons determine the chemical behavior
• As you move across a period from left to right, without counting the transition metals, the number of valence electrons increases by one

Formation of Ions

• Ions are atoms that have lost or gained electrons
• Atoms form ions to achieve the electron configuration of their closest noble gas
• Noble gasses have a stable electron configuration because of their full outer shell
• Atoms lose electrons to form cations
  • Since a cation has more protons than electrons, it has a positive charge
  • Cations are formed by elements metals which have few valence electrons

Sodium Atom Becoming a Sodium Ion

Formation of positively charged sodium ion - sodium loses 1 electron to become a sodium ion

• Atoms gain electrons to form anions
  • Since an anion has less protons than electrons, it has a negative charge
  • Anions are formed by non-metals which are elements that lack a few electrons
• The electrostatic attraction between a positive ion (cation) and a negative ion (anion) is defined as an ionic bond

Chlorine Atom Becoming a Chloride Ion

Formation of negatively charged chloride ion - it gains 1 electron to become a chloride ion

Common ions and the Periodic Table

• The periodic table can help you to identify the typical charges of cations or ions
• Elements in Group 1 tend to lose their lonely electron from their valence shell, therefore, the common charge for all the elements is 1+
  • E.g. Sodium (Na) tend to form Na⁺ cation
• Elements in Group 2 tend to lose two electrons from their valence shell, therefore, the common charge for all the elements is 2+
  • E.g. Magnesium (Mg) tend to form Mg²⁺ cation
• Elements in the Group 3 (skipping the transition metals) tend to lose three electrons from their valence shell, therefore, the common charge for all the elements is 3+
  • E.g. Aluminum (Al) tend to form Al³⁺ cation
• Elements in the Group 5 (skipping the transition metals) tend to gain three valence electrons, therefore, the common charge for all the elements is 3-
  • E.g. Nitrogen (N) tend to form N^3- anion
• Elements in the Group 6 (skipping the transition metals) tend to gain two valence electrons, therefore, the common charge for all the elements is 2-
  • E.g. Oxygen (O) tend to form O^2- anion
• Elements in the Group 7 (skipping the transition metals) tend to gain one valence electron, therefore, the common charge for all the elements is 1-
  • E.g. Fluorine (F) tend to form F^- anion
• Atoms in Group 4 tend not form ions, therefore it is not possible to form ionic compounds with those elements