Bonding, Structure, and Properties of Metallic Bonds

These flashcards cover key concepts related to metallic bonding, ionic bonding, covalent bonding, and their properties.

Metallic Bonding

The bonding that occurs when metal atoms bond to each other.

Delocalized Electrons

Electrons from the outer shell of atoms that are free to move throughout the entire structure.

Strength of Metallic Bond

Arises from the attraction between metal ions and delocalized electrons.

Properties of Metals

Good conductors of electricity and heat, malleable, and ductile.

High Melting and Boiling Points

Require large amounts of energy to break the strong metallic bonds.

Ionic Bonding

The bonding that occurs between metal and non-metal atoms due to the transfer of electrons.

Ion

A charged particle that has a different number of protons and electrons.

Covalent Bonding

The bonding that occurs between non-metal atoms by sharing electrons.

Simple Molecular Structures

Composed of a small number of atoms held together by covalent bonds.

Weak Intermolecular Forces

Forces between individual molecules that lead to low melting and boiling points.

Giant Covalent Structures

Composed of many atoms held together by covalent bonds in a large network.

Diamond

A material where each carbon atom is bonded to four other carbon atoms.

Graphite

A form of carbon that conducts electricity due to delocalized electrons between layers.