Metallic Bonding Flashcards
What does chemical bonding involve?
An attraction between atoms to form chemical substances containing two or more atoms
What is all bonding in nature?
Electrostatic, which means between opposite charges
What is the difference between intermolecular and intramolecular bonds?
Intramolecular bonds are within molecules whereas intermolecular bonds are between molecules
What are the three major types of intramolecular bonds?
Metallic, ionic and covalent
What are the four major types of intermolecular bonds?
Ion-dipole, dipole-dipole, hydrogen bonding and dispersion forces
What are the two metals which are not solids at room temperature?
Mercury and gallium
What are the key properties of metals?
Solid at room temperature, high melting point, good conductors of heat/electricity, malleable, ductile, strong, dense and sonorous
What is an example of metallic bonding?
Sodium which is held together with metallic bonds in a giant lattice structure
What is an example of ionic bonding?
Sodium chloride which exists as giant lattices of ions, held together by ionic bonds
What is an example of covalent bonding?
Chlorine is covalently bonded within discrete, separate molecules
How are the atoms in pure metals packed together?
In tightly packed layers which form a regular lattice structure
Explain how metallic bonding works?
The outer electrons of the atoms seperate and create a sea of delocalised electrons which are free to move throughout the whole structure.
The metal atoms than exist as cations and are attracted to the sea of electrons
What do delocalised electrons in metallic bonding allow?
Metals to conduct heat and electricity
When a metal is heated, what happens to the delocalised electrons?
They gain kinetic energy, thus move faster and make heat/electricity transfer very efficient
Why are metals lustrous?
Delocalised electrons reflect light
What happens when a metal is hit?
The layers of metal ions are able to slide over each other, thus the structure does not shatter
Why do the metallic bonds not break when a metal is hit and what does this explain?
The delocalised electrons are free to move, thus metals are malleable, ductile and strong
Why can metals conduct electricity?
They have electrons that are delocalised and can migrate to a positive electrode
What is the structure of a metal?
A sea of free moving electrons surrounding a lattice of cations
What is the structure normally associated with metallic bonding?
A regular arrangement of ions surrounded by a sea of electrons
