C2-Bonding, structure and properties of matter Flashcards
What are ions
They are charged particles
What happens to metals and nonmetals to form ions
Metals have to lose electrons from the outer shell to form positive ions
Nonmetals have to gain electrons to the outer shell to form negative ions
What is ionic bonding
Transfer of electrons
Why do ionic structures have a high melting/boiling point
There is a giant structure and they have many electrostatic bonds of attraction between opposite Lee charged ions. This requires a large amount of energy to overcome the strong forces of attraction between ions. It is also a giant lattice so there are many forces of attraction
Why can ionic Aqueous solutions carry a charge
Because in an aqueous solution the bonds are broken and ions are free to move and carry charge
What are traits of an ionic bond
High melting and boiling point
– conducts electricity in molten or Aqueous solutions
What is a covalent bond
Bonding between nonmetals
- Sharing electrons
Bonds within the atoms are held together by very strong covalent bonds however they have a low melting point because the intermolecular force of attraction are weak
Why do covalent bonds have low melting/boiling points
Because covalent bonds have weak forces of Intermolecular forces of attraction meaning it requires a little energy to overcome the week bonds
Why do covalent bonds not conduct electricity
Because they have no free electrons or ions to carry the charge
– they also have no charge
Why are metals malleable
Because metals consist of giant structures that are arranged in a regular pattern which allow atoms to slide over each other
Why can a metal carry a charge
Metals have a giant structure which each metal atom has a delocalised electrons which are free to move and carry charge through the whole structure
Why do metals have a high melting point
Because the electrostatic forces of attraction between metal atoms and the delocalise sea of electrons are very strong And therefore need loads of energy to be broken
Why are normal metals softer than alloys
Metals are arranged in order grows so when a force is exerted I can easily slide over each other. Alloys have a mixture of elements so therefore cannot slide over each other with much ease
What are the properties of a solid
Strong forces of attraction between particles which hold them close together in fixed positions to form a regular lattice arrangement
– they don’t move from their positions and keep a defined shape
– the particles vibrate about their positions – the hotter the solid becomes the more they vibrate
What is the properties of a liquid
In liquids, there are weak forces of attraction between the particles. They randomly arranged and free to move past each other however they tend to stick closely together
– They have a definite volume but don’t keep to a defined shape
– they will move constantly at random motion – the hotter the liquid it gets the faster they move
What are the properties of a gas
The force of attraction is a very weak therefore they can move around freely far apart from each other
– gases don’t keep in shape and volume am always feel any container
– the particles move constantly with random motion – the hotter it Gets the faster they move
Why do you larger covalent molecules have a higher melting and boiling point
Because the intermolecular forces increase of the size of the molecules
What are polymers
Very large molecules that are linked to other atoms by strong covalent forces
What is the structure and bonding of diamond
Enjoyment, each carbon atom has for covalent bonds with other carbon atoms in a giant covalent structure, so the diamond is very hard, also has a very high melting point and does not conduct electricity
What is the bonding and structure of graphite
I fight, each carbon atom forms three covalent bonds With other carbon atoms, forming layers of hexagonally rings which have no covalent bonds between the layers
– one electron from each carbon atom is the localised
What is graphene
Grapheme is a single layer of graphite and has properties that make it useful in electronics
What are fullerenes
They are Look use of carbon atoms with hollow shapes. They are generally have the structure of hexagonally rings
- They have a large surface area so they can help make great catalysts
– e.g. nanotubes – which have a high length to diameter ratio
What is silicon dioxide
Sand
