Elements can bond together to form large structures and crystal arrangements. But all have a similarity in the type of bonds formed. Very often the bonds form determine the physical properties of the elements and there is variety within the same types of bonding due to the position of the elements in different groups and periods.
Bonding describes how metallic and non metallic elements of the periodic table exist as elements or combined together to form new compounds with different properties
Malleable describes when layers in a solid can slide over each other when a force is applied
Ductile is a term used to describe when layers in a metal can be pressured down into smaller layers that are next to each other turning them into a wire
A crystal has a 3d arrangement of atoms highly ordered to produce 3d structures which have straight edges and flat faces
Metallic bonding is the bonding between metallic ions where the metallic atoms lose their electrons and form positive metal ions
Transition metals are the central section of the periodic table containing the majority of the metals. Also have d sub orbitals producing certain chemical properties
Delocalised electrons is the term used to describe electrons when they leave their shells and move between positive ions and are free to move
Metals are located on the left hand side of the periodic table and comprising a large part of the periodic table. Metal elements have metallic bonding where positive ions are held in sea of delocalized electrons.
An ion forms when an atom loses or gains electrons to form a positive or negative particles due to the unbalanced number of protons
An atom is the smallest particle that makes up all matter
The electron is the smallest sub atomic particle that make up the atom. Has a negative charge and is located in shells that orbit the nucleus
The shell is the path that electrons follow outside the nucleus. Shells can be considered as energy levels and the further away from the nucleus the higher in energy.