Topic 2 The periodic table and bonding

Periodic Table

A tabular arrangement of elements organized by their atomic number, electron configuration, and recurring chemical properties.

Groups

Vertical columns in the periodic table, where elements have similar properties and the same number of electrons in their outer shell.

Periods

Horizontal rows in the periodic table where properties of elements change as you move across.

Electron Shells

Energy levels surrounding the nucleus of an atom, where electrons reside.

Electron Configuration

The distribution of electrons in an atom's electron shells.

Metallic Properties

Characteristics of metals including conductivity of electricity and heat, malleability, and ductility.

Metals

Elements located on the left of the zigzag line in the periodic table that conduct electricity and tend to lose electrons.

Non-Metals

Elements located on the right of the zigzag line in the periodic table that are poor conductors of electricity and typically gain electrons.

Noble Gases (Group 0)

Colorless, inert gases that do not react easily with other elements due to their full outer electron shells.

Ionic Bonding

The attraction between oppositely charged ions formed when electrons are transferred from one atom to another.

Cation

A positively charged ion that is formed when an atom loses electrons.

Anion

A negatively charged ion that is formed when an atom gains electrons.

Electrostatic Force

The force of attraction between oppositely charged ions in ionic compounds.

Ionic Compounds

Compounds formed from ionic bonds that have a lattice structure.

Lattice Structure

The organized, repetitive three-dimensional arrangement of ions in ionic compounds.

Melting Point

The temperature at which a solid turns into a liquid; ionic compounds have high melting points due to strong ionic bonds.

Covalent Bonding

A type of bonding where atoms share pairs of electrons.

Intermolecular Forces

Forces of attraction between molecules that are generally weaker than covalent bonds.

Simple Molecular Substances

Substances made up of molecules held together by covalent bonds with low melting and boiling points.

Giant Covalent Structures

Large networks of atoms bonded together covalently, resulting in high melting and boiling points.

Graphite

A form of carbon where each atom forms three covalent bonds, arranged in layers, which makes it soft and slippery.

Diamond

A form of carbon where each atom forms four covalent bonds, resulting in a hard structure with a high melting point.

Fullerene

A molecular form of carbon where atoms are arranged in a hollow sphere, consisting of 60 carbon atoms.

Electrical Conductivity

The ability of a material to conduct electricity, largely produced by the movement of electrons.

Electrolyte

A substance that produces an electrically conducting solution when dissolved in water or melted.

Metallic Bonding

The attraction between free electrons and metal ions that leads to the electrical conductivity of metals.

pH of Metal Oxides

Basic metal oxides have a pH greater than 7 and can neutralize acids.

pH of Non-Metal Oxides

Non-metal oxides are acidic and have a pH of less than 7, neutralizing bases.

Noble Gas Inertness

The reluctance of noble gases to react due to their full outer electron shells.

Energy Required for Bond Breakage

Significant energy is needed to break strong covalent bonds in giant covalent structures.

Delocalized Electrons

Electrons that are free to move between atoms in structures like graphite, allowing electrical conductivity.

Electrical Current

The flow of electrons or ions that results in the conduction of electricity.

Conditions for Ionic Conductivity

Ionic compounds conduct electricity only when melted or dissolved in water due to the mobility of ions.

Electrons in Ionic Compounds

Electrons are tightly bound in solid ionic compounds, preventing conductivity.