Giant Covalent Structures Flashcards
What are the covalent bonds like between atoms?
Very strong
Which substances with covalent bonds have this structure?
Diamond, Graphite, Silicon Dioxide and Fullerene
What do diamond and graphite have in common?
They are both made up of carbon. They are Allotropes of carbon (different forms of the same element)
What are the differences of diamond and graphite?
-Different bonding arrangements
-Different giant structures
-Different properties
How many of the electrons in the outer shell of the diamond form covalent bonds?
All four of them
Is diamond hard?
Very hard- the hardest natural substance
What are the covalent bonds like in the rigid lattice structure of the diamond?
Strong
Why does diamond have a high melting and boiling point?
Because a lot of energy is needed to break the many covalent bonds in the giant covalent structure
Why can diamond not conduct electricity?
Because there are no freely mobile electrons or ions to carry a charge
How many of the electrons in the outer shell of graphite from covalent bonds?
Three or four
Why is graphite soft and slippery?
Because there are no covalent bonds between the layers, so layers can slide over each other easily
Why does Graphite conduct electricity?
Because it ha sone delocalized electron per carbon atom- delocalized electrons are free to move through the layers and carry currents
Why does graphite have a high melting/boiling point?
Because there are many strong covalent bonds in layers need large amounts of energy to break
What atoms are Silicon dioxide made up of?
Oxygen and Silicon
What is the electronic configuration of Silicon and Oxygen?
[2.8.4] and [2.6]
