Mind Map Gallery Structure and Bonding - Metallic Bonding Mind Map

Structure and Bonding - Metallic Bonding Mind Map

This mindmap is about metallic Bonding. It covers the following key topics: - Metallic structure - Physical properties of metals - Alloys The magnetic attraction between these free-moving (delocalized) electrons and the positive metal ions is known as the metallic bond. Metals often have high melting and boiling temperatures and can keep a consistent structure due to the strength of their metallic connections. Metals are efficient heat and electrical conductors. Hope you can find more interesting templates here in EdrawMind Gallery.

Edited at 2022-06-30 13:36:50

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Structure and Bonding - Metallic Bonding Mind Map

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Structure and Bonding - Metallic Bonding

metallic structure

subtances with metallic structure:

pure metals

aluminium

copper

potassium

sodium

Alloys - mixtures of metals

steel

brass

structure of a metal

positive metals ions surrounded by a 'sea of mobile delocalised electrons'

delocalised valnece electrons move freely like a cloud of negative charge

metallic bonding - strong electrostatic attraction between positive metal ions and the 'sea of delocalised electrons

attraction between the delocalised electrons and the metal cations is responsible for the strength of the metal lattice

arrangement

close together in a regular manner

known as metal lattice

Physical metal properties

metals have high density

majority of metals have higher densities than non-metals

group 1 metals, also known as light metals happen to be exceptions to this generelization

this is because of the tightly packed crystal lattice of the metallic structure

strength of metallic bonds for different metals reaches a maximum around the centre of the transition metal series as those elements have large amiunts od delocalised electrons in the metallic bonds

metals have high melting and boiling points

metal atoms are held together by strong metallic bonds

a lot of energy is required to overcome these bonds

explains the high melting and boiling points

metals are good electrical conductors

when a potential difference is applied across the ends of a metallic conductor,

delocalised electrons will be attracted and hence move towards the positive end

movement of charge known as electric current

metals are good conductors of electricity because they have delocalised mobile electrons that move towards the positive terminal when connected to a circuit

metals are good heat conductors

metal atoms are closely packed

heat can be transferred from one atom to the next by vibration as they are close together

the free electrons also suddenly acquire more energy

they move faster and collide with the other electrons, transferring part of the energy

thus heat is easily conducted from one end to the other end of the metal

Metals are malleable and ductile

malleable (can be rolled into sheets)

when a metal is bent

layers of cations in the metal lattice slide over one another easily and fit into new positions

the shape of the metal has changed but it does not break apart

ductile (can be pulled into wires)

when force is applied to 1 layer of cations

this layer easily slides over the other layers

makes the metal longer and flatter without breaking apart

this is possible because metallic bonding reamin largely undisrupted

metal cations are shielded from each other's repulsions by the 'sea of delocalised electrons' in between them

shielding is present no matter how much the lattice is distorted

bending and shearing forces can deform metal lattices without shattering them

Alloys

a homogenous mixture of a metal and another element

stronger and harder than pure metals

a metal can be made stronger and harder by the adding other elements into its structure

The presence of atoms of a different size disrupts the regular arrangement of the metal atoms

prevents the metal atoms from sliding over one another easily