Chem - bonding and structure - covalent network Flashcards
What type of structure dose a covalent bond have
Covalent network - non metal - non metal
What are the particles and type of bond
Atoms - Covalent bond
What is the electrical conductivity
No charger particles therefore do not conduct elections apart from graphite as it has delocalized electrons between layers
What is its melting point and boiling point
High as it has strong covalent bonds
What are other properties you might be asked to account for
- Hard
- Graphite is slippery used as a lubricant due to weak attractive forces between layers
- Diamond and SiO2 has strong covalent bonds in 3D lattice
What is the structure of graphite
- Shape/ arrangement
- bonds
- properties of the substance
Graphite consists of C atoms covalently bonded to 3 other C atoms [ trigonal planar shape] in a 2D arrangement forming layers with weak intermolecular forces between them. The weak attractions between the layers of atoms are easily broken. Therefore graphite is soft and slippery and the layers can slide over each other.
What is the structure of diamond
- Shape/ arrangement
- bonds
- properties of the substance
Diamond is made from carbon atoms. Each carbon is covalently bonded to 4 other atoms in a tetrahedral arrangement, which forms a covalent network solid. The covalent bonds between the carbons are very strong and require a large amount of energy therefore explaining diamonds strength and high melting point.
What is silicon dioxide structure
- Shape/ arrangement
- bonds
- properties of the substance
SiO2 consists of silicon and oxygen atoms held together by covalent bonds in tetrahedral arrangement so that a 3D network exists
What is the melting point of all covalent bonds
In order to melt covalent network substances strong covalent bonds between atoms must be broken. A lot of energy is required to do so . Therefore melting points are high
