Structure and Bonding Flashcards
Definition of a compound
Two or more elements which are chemically combined
Definition of Covalent Bonding
Shared pair of electrons
Definition of Ionic Bonding
(electrostatic) attraction between oppositely charged ions
Describe the structure of NaCl
Giant ionic lattic (structure) electrostatic attraction Between Na+ and Cl-
Type of bonding in graphite
Covalent
Describe the structure of diamond
Giant covalent structure where each carbon has 4 bonds
Describe the structure of graphite
Giant covalent structure where each carbon has 3 bonds. It is arranged in layers.
Definition of Metallic Bonding
(electrostatic) attraction between positive metal ions and the delocalised electrons
Type of bonding in CO2
Covalent
Describe the structure of CO2
Simple molecular
Identify the bonding in H2O and describe its structure
Covalent Simple molecular
Identify the type of bonding in copper and describe its structure
Metallic Giant metallic lattice
Identify the type of bonding in sodium and describe its structure
Ionic Giant ionic lattice
Identify the type of bonding in Ca(OH)2 and describe its structure
Ionic Giant ionic lattice
Identify the type of bonding in SiO2 and describe its structure
Covalent Giant covalent lattice/structure (giant molecular)
Graphite, diamond, nanotubes and fullerenes are all _________________ of carbon
allotropes
Explain why NaCl is a solid at room temperature
It has a giant ionic lattice It is held together by ionic bonds which are very strong Therefore it has a high melting point
Explain why oxygen is a gas at room temperature
It has a simple molecular structure It is held together by weak intermolecular forces Therefore it has a low melting point
Explain why iron is a solid at room temperature
It has a giant metallic structure It is held together by strong metallic bonds Therefore it has a high melting point
Explain why iron conducts electricity as a solid and liquid
It has delocalised electrons which are free to move throughout the metal structure
Explain why graphite conducts electricity
Each carbon has only 3 bonds. This leaves one delocalised electron Which is free to move throughout the structure
Explain why diamond doesn’t conduct electricity
Each carbon has 4 bonds. It has no free electrons
Explain why sodium chloride doesn’t conduct electricity as a solid
The ions can’t move and carry the charge
Explain why sodium chloride conducts electricity when dissolved
The ions are free to move and carry the charge
Explain why carbon dioxide doesn’t conduct electricity
Its electrons aren’t free to move and carry the charge
Explain why molten magnesium chloride can conduct electricity
The ions are free to move and carry the charge
Explain why methane is a gas at room temperature
It is a simple molecular substance It is held together by weak intermolecular forces Therefore it has a low melting point
Explain why graphite has a very high melting point
It has a giant covalent structure which is held together by strong covalent bonds which require a lot of energy to break
What property makes diamond useful for sharpening knives
It is very hard
Explain why diamond is so hard
It is arranged in a giant lattice Each carbon has 4 bonds The lattice is rigid
Explain why thermosetting polymers have high melting points
They have crosslinks between the chains made with covalent bonds which are strong
What conditions can be changed to make high density polyethene instead of low density polyethene?
Temperature
Pressure
What is a nanoparticle
a particle between 1nm and 100nm in size
Why do nanoparticles have different properties?
Because they have a much bigger surface area
What are the risks of nanoparticles?
Their large surface area makes them very reactive/explosive (nano aluminium) Nanoparticles are easily absorbed by the lungs and there is little research into the long term health risks.
Explain why copper is used to make wires rather than graphite
Copper and graphite both conduct electricity
Copper and graphite both have a high melting point
Graphite is soft and brittle
Copper is strong and ductile
Name properties you would expect of an ionic compound?
High melting point
Doesn’t conduct electricity when solid
Conducts electricity when molten or in solution
Name properties you’d expect of a simple covalent solid
Low melting point
Brittle
Dull
Soft
Name properties you’d expect of a metal
High melting point
Conducts heat and electricity
Hard
Lustrous (shiny)
Malleable (can be hammered into shape)
Ductile ( can be drawn into wires)
What is meant by the term diatomic?
molecule containing two atoms
Name the diatomic elements
Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine
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