Chemical Bonding #6

Vocabulary flashcards covering chemical bonding (metallic, ionic, covalent, polar/non-polar) and periodic trends based on lecture notes.

Atomic Radius

The distance between the centre of the nucleus and the outermost electrons.

Ionisation Energy

The energy required to remove an electron from an atom.

Electronegativity

A measure of how strongly an atom attracts bonding electrons.

Octet Rule

The principle stating that atoms are most stable when they have a full outer shell of valence electrons.

Valence Electrons

The electrons located in the outermost shell of an atom.

Metallic Bonding

A type of chemical bonding occurring between metal atoms where valence electrons are delocalised and shared across a lattice structure.

Delocalised Electrons

Electrons that move freely throughout a metallic lattice and are not bound to any specific parent atom.

Ionic Bonding

The electrostatic attraction between positive ions (cations) and negative ions (anions) formed when electrons are completely transferred due to a large difference in electronegativity.

Covalent Bonding

A chemical bond formed when nonmetal atoms with similar electronegativities share pairs of valence electrons.

Polar Covalent Bond

A covalent bond in which electrons are shared unequally between atoms with moderate electronegativity differences, creating partial charges ($\delta+$ and $\delta-$).

Non-Polar Covalent Bond

A covalent bond where bonding electrons are shared equally between two atoms with very small or zero electronegativity difference.

Partial Charges ($\delta+$ / $\delta-$)

Fractional electric charges that arise on atoms in a molecule due to the unequal distribution of shared bonding electrons.

Giant Ionic Lattice

A regular three-dimensional structure composed of alternating positive and negative ions held together by strong electrostatic forces of attraction.

Giant Metallic Lattice

A regular three-dimensional arrangement of positive metal ions surrounded by a sea of mobile, delocalised electrons.

Periodic Trends Overview

A summary chart displaying how atomic radius decreases across a period and increases down a group, while ionisation energy and electron affinity increase across a period and decrease down a group.

Electronegativity Difference Classification Table

A table outlining bond classifications based on electronegativity difference: values $< 1.0$ indicate covalent bonds, $1.0 - 2.0$ indicate polar covalent bonds, and $> 2.0$ indicate ionic bonds.

Ionic Bonding Shell Diagram in Sodium Chloride

An electron shell diagram showing the sodium ion ($Na^+$) with configuration 2,8 and the chloride ion ($Cl^-$) with configuration 2,8,8 formed after electron transfer.

Sodium Chloride Crystal Structure

A 3D lattice representation of sodium chloride showing alternating sodium ($Na^+$) and chloride ($Cl^-$) ions bound together by electrostatic attraction.

Polar Molecule Charge Distribution (Hydrogen Fluoride)

A diagram demonstrating fluorine's higher electronegativity ($4.0$) compared to hydrogen ($2.1$), resulting in a greater attraction for the shared electron pair and generating partial charges ($\delta+$ and $\delta-$).

Metallic Bonding Lattice Model

A schematic diagram showing fixed positive metal ions surrounded by mobile, delocalised electrons.