Bonding Flashcards
Ionic bonds
a strong electrostatic
attraction between oppositely charged ions
Covalent bond
when a pair of electrons is shared between two non-metal atoms leading to noble gas electronic configurations
Metallic bonding
the strong electrostatic attraction between the positive ions (metal name) in a giant
metallic lattice and a ‘sea’ of delocalised electrons
Diamond bond
Each carbon atom forms
4 strong covalent rigid bonds with each other
forming a tetrahederal arrangement
giving rise to a 3-dimensional macromolecular structure
Graphite bond
Each carbon atoms forms
3 strong covalent bonds with each other
forming layers of flat hexagonal rings
Silicon Dioxide bond
Each silicon atom is covalenty bonded to 4 Oxygen atoms
Each oxygen atom is bonded to 2 silicon atoms by strong rigid covalent bonds
forming a tetrehedral arrangement
giving rise to a 3-dimensional macromolecular structure
intermolecular forces def
and property
forces of attraction between molecules e.g Van der Waals
they are weak and easy to overcome at lower temperatures
intramolecular forces def
and property
forces of attraction found inside molecules
e.g covalent bonds
strong, do not break during melting or boiling
Diamond properties
High melting and boiling point (strong intramolecular)
Very Hard
Poor electrical conductor
Graphite properties
Electrical conductor
Lubricant (weak van der waals layer slide over each other)
Diamond vs Graphite
properties and uses
Properties of diamond:
- Does not conduct electricity
- very hard substance
- transparent crystal which sparkles in light
(Silicon oxide has same properties)
Uses of diamond:
- Used for cutting rocks
Properties of Graphite:
- Conducts electricity
- Soft and slippery
- A grey-black shiny solid
Uses of Graphite:
- Used as a lubricant
- Used as an electrode
Properties of metals
High melting points
Hard
Usually high density
Goold electrical conductivity as molten, aqueous or solid
Malleable and ductile
Simple molecular covalent bonds properties
Low melting and boiling points (weak intermolecular)
Poor electrical conductor
Ionic compounds properties
(physical)
- Good electrical conductivity when aqueous or molten but poor when solid
- High melting and boiling points
- Soluble in water
- Brittle
What is arrangement in ionic compound:
Giant ionic crystal lattice:
Regular arrangement of
alternating positive and negative ions held together by strong electrostatic forces of attraction