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Why Atoms Seek Stability; Valence Electrons & The Octet Rule; How Ions Form: Cations & Anions; Valency and Periodic Table Patterns; The Importance of Ions in Our World

Valency and Ions

Chemistry

Valency and Ions

Understanding how atoms become stable and form charged particles.

Agenda

• Why Atoms Seek Stability

• Valence Electrons & The Octet Rule

• How Ions Form: Cations & Anions

• Valency and Periodic Table Patterns

• The Importance of Ions in Our World

Atoms: Stable or Not?

Atoms aren't always stable in their natural state. They strive to achieve a full outer electron shell, also known as a stable octet, to become more balanced. This is why elements like Sodium (Na) and Chlorine (Cl) react readily, unlike stable noble gases such as Neon (Ne) or Argon (Ar).

Atom model with nucleus and orbiting electrons, illustrating stability.

Outer Shell Electrons

Valence electrons are the electrons found in the outermost energy shell of an atom. These electrons are key to how an atom will react with other atoms, determining its chemical behavior. For instance, sodium (Na) has one valence electron, making it highly reactive, while neon (Ne) has a full outer shell, making it stable.

Bohr model illustrates electrons in orbits around the nucleus.

Atom's nucleus and orbiting electrons, representing chemical behavior.

The Octet Rule

• Atoms aim for eight valence electrons.

• This makes them stable, like noble gases.

• They gain, lose, or share electrons.

• Example: Sodium loses, chlorine gains an electron.

Atoms with a Charge

When atoms gain or lose electrons, they become electrically charged particles called ions. Losing electrons, like a sodium atom (Na) forming Na+, results in a positive charge (cation). Gaining electrons, such as a chlorine atom (Cl) forming Cl-, creates a negative charge (anion).

Sodium and chlorine atoms form ions through electron transfer.

Losing Electrons: Cations

When a neutral atom loses one or more negatively charged electrons, it transforms into a positively charged ion, known as a cation. This occurs because the atom now has more protons (positive charges) than electrons. A common example is sodium (Na), which readily loses one electron to become a sodium ion (Na+), carrying a +1 charge.

Gaining Electrons: Anions

Anions are negatively charged ions formed when a neutral atom gains one or more electrons. For instance, a Chlorine atom (Cl) gains one electron to become a chloride ion (Cl-). This gain of negative charge makes it an anion.

What is Valency?

• It's an element's combining power.

• Determined by electrons gained, lost, or shared.

• Goal: achieve a stable outer shell.

• Example: Hydrogen (valency 1), Oxygen (valency 2).

Group 1: One Valence Electron

Forming +1 Ions (Cations)

Elements in Group 1 of the periodic table, such as Lithium (Li) and Potassium (K), are known as alkali metals. They all share a key characteristic: they have only one electron in their outermost energy shell. This single electron is called a valence electron and largely determines their chemical behavior.

To achieve a stable electron configuration, similar to noble gases, Group 1 elements readily lose this single valence electron. When an atom loses an electron, it forms a positively charged ion, known as a cation. For example, Lithium loses its one electron to become Li+, and Potassium becomes K+, both with a +1 charge.

Valency and Ions

Why Atoms Seek Stability; Valence Electrons & The Octet Rule; How Ions Form: Cations & Anions; Valency and Periodic Table Patterns; The Importance of Ions in Our World

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