2.4 Giant Structures Flashcards
What is the structure of Graphite?
Each carbon atom is bonded to 3 others, forming layers of hexagons
Describe the bonds WITHIN the hexagon layers (Graphite)
They are strong as they are covalently bonded
Describe the bonds of the hexagon layers ATRACTED to each other (Graphite)
They are weak as they are attracted via weak intermolecular forces
Describe the structure of diamond
Tetrahedral/Tetrahedron
Describe the bonds between carbons in diamond
All covalent bonds are identical, very strong and no intermolecular forces
List 2 uses of graphite?
- Industrial Lubricant
- Pencils
Why can graphite be used as an industrial lubricant?
Because graphite is slippery, as the layers of graphite have weak intermolecular forces, thus they slide over each other.
Why is graphite a conductor of electricity?
Each carbon atom is bonded to 3 others, one free electron is left, thus graphite has delocalized electrons to freely move
Why does graphite have a high melting point?
It has a giant covalent structure, and covalent bonds require high energy to break
List a use of diamond
- Cutting Tools (eg. Drills)
Why can diamond not conduct electricity?
No delocalized electrons
Why does diamond have a high melting point?
It has a giant covalent structure, and covalent bonds require high energy to break
What is the structure of Silicon(IV) Oxide
A macromolecular compound in a tetrahedron structure
List 2 Uses of Silicon(IV) Oxide SiO₂
- Sandpaper
- Lining inside of furnances
What is Silicon(IV) Oxide similar to?
Diamond
Metals consist of ___ structures
Giant Structures
Within the metal lattice, atoms lose their outer electrons and become ____ charged metal ions
Positively
Most metals have ___ melting and boiling points
High
Metals are ___ conductors of electricity and heat
Good
Define Malleable
Can be hamered into shape
Are most metals malleable?
Yes
Define ductile
Can be pulled into wires
Are most metals Ductile?
Yes
