Types of bonding Flashcards
What are the 5 giant covalent structures?
Diamond, graphite, silicone, silicone dioxide and boron
What is ionic bonding?
The electrostatic attraction between positive and negative ions
What is a covalent bond?
Strong electrostatic attraction between a shared pair of electrons and nuclei of the bond
What is metallic bonding?
The electrostatic attraction between positive metal ions and delocalised electrons
What are lone pairs?
Pairs of electrons not involved in bonding
How are dative bonds drawn?
With an arrow
What is a dative covalent bond?
Shared pair of electrons which the bonding pair has been provided by one of the bonding atoms only
How do you write about melting point?
- type of bonding
- force
- between _____ particles
- energy
With ion in a period, which ion has the stronger charge?
The ion with the greatest charge
With ions in the same group, which ion will have stronger attraction?
The smallest ion
How does attraction effect melting point?
The greater the attraction, the greater the melting point
What affects the melting point of metals?
Ionic charge and ionic radius of metal cations and number of delocalised electrons per cation
How does charge affect melting point of metals?
An atoms with a higher charge (e.g. 3+ vs 1+) has greater attraction
How does atomic radius effect melting point?
An atom with a smaller atomic radius will have greater attraction
How does number of delocalised electrons affect melting point?
Atoms with more delocalised electrons per cation will have greater attraction
What is the bonding inside metallic structures?
Electrostatic attractions between cations and electrons
What is the bonding inside ionic structures?
The electrostatic attraction between cations and anions
What do you include when writing about conductivity?
- Type of bonding
- Mobile charge carriers.
- Charged particles
What is the conductivity of metals?
In a solid, delocalised electrons can move and act as mobile charge carries but when molten, both delocalised electrons and positive metal cations can move so conducts better as liquid
What is the conductivity of ionic compounds?
When solid, ions are in fixed positions in lattice and can’t conduct electricity. When molten, the lattice is broke down and ions are free to move and act as mobile charge carriers so can only conduct as liquid
What is the conductivity of covalent compounds?
Simple molecular structure consisting of neutral molecules held together by intermolecular forces with no charged particles which can move so cannot conduct
How does delocalised electrons affect melting points?
The more delocalised electrons per cation, the higher the conductivity.
