Ionic And Metallic Bonding Flashcards
What are Ions
when a particle looses or gains an electron , its balance with the protons is lost, making it either positively charger if electron was lost or negatively charged if it was gained.
If a particle looses an electron it would have a + symbol as its now positively charged.
Explain Ionic Bonding
When metal atoms react with non metal atoms, they transfer electrons to the non metal atom ( instead of sharing like covalent )
Non metal + metal = Ionic As electrons are transferred
What is One Ionic structure
Giant ionic lattice
Explain how a giant ionic lattice is formed
When metal atoms transferrer electrons to non metals, you end up with positive and negative ions
These positive and negative atoms are attracted to each other by the strong ELECTROSSTATIC FORCE of attraction . This attraction is ionic bonding
Electrostatic attraction between oppositely charger ions
Explain 2 Ionic Properties
- melting points and why
- conductivity and why
Melting Points- Ionic substances have a high MP because the electrostatic force of attraction between oppositely charged ions are strong and require a lot of energy to break
Conductivity- Solid ionic substances do not conduct because the ions are fixed in position and are not free to carry charge.
However when melted or dissolved in water, ionic substances conduct as the ions are free to move around and carry charge
This happens as in water the ions are separated so the negative ions move toward the positive electrode and the positive ions move toward the negative electrode
why are ionic structures strong
Ionic structures are strong because of the number of ionic bonds
Explain metallic structure
Atoms that make up metals, form layers. The electrons on the outermost energy level are delocalised and can move through the whole structure.
So in short the metallic structure is layered positive ions in a “sea” of delocalised electrons
What is the force present in metallic structures
A strong electrostatic attraction between the sea of delocalised electrons(negative) and positive metal Ions
Give 3 metallic properties and explain
Malleable- Pure metals are malleable as the layers can slide over each other
Conduction- metals are good electric and thermal conductors as they have delocalised electrons.
High Melting point - Due to the strong electrostatic force of attraction between the sea of delocalised electrons and positive ions
What is an alloy
An alloy is a pure metal mixed with small portions of other metals.
why is an alloys useful in comparison to pure metals
An alloy is a mixture of metals that are harder than pure metals as the layers in the structure are distorted
Alloys are more useful than pure metals as their physical properties can be altered to fit a purpose
What makes a pure metal strong
The amount of delocalised electrons relate to its tensile strength, as the more delocalised electrons there are, the stronger the metal is.
