Bonding, Structure And Property Of Matter Flashcards
How are ions made
When electrons are transferred between elements
What are ions
Charged particles they can single or groups of atoms they can gain and lose electrons to form ions
If 2 ions are gained what is the charge
2-
If 2 ions are lost what is the charge
2+
What do group 1 and 2 metals do
They lose electrons and form positive ions
What do group 6 and 7 elements do
They gain electrons to form negative ions
What is an ionic compound
A compound that only contains ionic bonds
What is the structure of an ionic compound
Giant ionic lattice
What are the properties of an ionic compound
High melting point needs lots of electricity to overcome
High boiling point needs lots of electricity to overcome
Solid and can’t conduct electricity
Carry current when they melt
Dissolve in water to carry current
What’s the use of a dot and cross diagram
So you can count up the amount of atoms in an element
What is a covalent bond
When atoms share electrons so that they both have full outer shells
Why are the bonds strong
The atoms are attracted by electrostatic forces
Properties of a covalent bond
Strong covalent bonds with weak attraction between molecules.
Low melting and boiling points as they are easily parted.
Liquid or gas at room temperature.
If the molecule is bigger it needs more energy to break.
They don’t conduct electricity so they don’t have free electrons.
What is a polymer
A long molecule with repeating structure and are joined by covalent bonds
Why is more energy needed to break polymers
The intermolecular forces are larger meaning they are solid at room temperature
What are giant covalent structures
Structures where all atoms are bonded by strong covalent bonds
Properties of giant covalent structures
Very high boiling point and lots of energy is needed to break the bonds.
Don’t conduct electricity (except graphite)
What is the structure of diamond
Each carbon atom forms four covalent bonds in a rigid giant covalent structure
What is the structure of graphite
Each carbon atom forms 3 layers of covalent bonds. Each carbon has atom has one free electron (so can act as charge carrier)
What is the state of carbon
Giant covalent structure made of 4 covalent bonds making it really hard.
The strong bonds take lots of energy to break the the diamond.
Doesn’t conduct electricity because it has no free electrons or ions.
What is the state of graphite
Three covalent bonds creating three sheets.
Aren’t any bonds between layers so this is weak bonding so they can move move on each other this makes it soft and slippery.
Has a high melting point and needs lots of energy to break.
One electron is free so can act as a charge carrier.
State of graphene (one layer of graphite)
Sheet of carbon atoms joined together.
Very strong and light can be added to composite materials to improve strength without weight.
Has a free electron.
Most metals are
Solid at room temperature.
Good conductors if electricity and heat.
Malleable.
What is metallic bonding
The structure of of electrons which involves all of those which are free
