Ionic And Metallic Bonding + Atoms Flashcards
Describe the structure of metals
Giant structure
Metal ions in layers
Delocalised electrons
Explain why pure metals have high melting and boiling points
Strong metallic bonds between metal ions and delocalised electrons
Require a lot of energy to overcome
Describe what happens to electrons in ionic bonding
Transferred from one atom to another
If a non metal forms an ion , will it have positive and negative charge
Negative
Explain why pure metals are malleable
Layers of metal ions are free to slide over each other
Explain why metals are good conductors of thermal energy
Delocalised electrons can move through the metal and transfer energy
Describe the structure of a typical alloy
Metallic structure
With atoms of different metals or carbon mixed in
Name the 2 different types of substances that form ionic bonds when they react together
Metals and non metals
Explain why metals are good conductors of electricity
Delocalised electrons can move through the metal and carry charge
If a metal forms an ion, will it have a positive or negative charge?
Positive
Ion
An atom with an overall charge
Explain why alloys can be harder than pure metals
They have atoms of different sizes
Which distorts the layers of the structure
And prevents them from sliding over each other easily
Give 4 typical properties of pure metals
High melting and boiling points
Malleable
God conductors of electricity
Good conductors of thermal energy
Give a reason for alloying a metal
To make it harder.
Explain in terms of electrons what occurs when magnesium reacts with chlorine to form magnesium chloride
One magnesium atom transfers one electron to one chlorine atom, and another electron to a second chlorine atom
The ions have full outer shells
The ions are then attracted to each other by the electrostatic force of attraction
