Bonding Flashcards
What are the limitations of the particle model?
Particles on solid since atoms are mostly empty Space many particles aren’t spherical.
What happens in ionic bonding?
Metals lose electrons to perform positively charged ions and nonmetals gain electrons to form negatively charged ions
Why positive ions positive?
Because they have more protons than electrons
Why are negative ions negative?
Because they have more electrons and protons
How doYou get from a liquid to a gas?
Evaporating or boiling
How do you get a liquid from a gas?
Condensing
Describe The structure of an ionic lattice
And ionic compound is a giant structure of ions. They have a regular repeating arrangement called an ionic lattice. The lattice has formed because the ions attract each other.
Name the properties of an ionic bond
They are held together by strong electrostatic forces of attraction between oppositely charged ions. They have a high boiling and melting point because the energy needed to break the electric static forces of attraction are high.
When can ionic bonds conduct electricity and why?
They can only conduct electricity when it is melted to form a liquid or dissolved in water to form an aqueous solution. This is because the particles are charged and free to move.
What is a covalent bond?
When two atoms share a pair of electrons, it occurs in nonmetals
What do covalent bonds have?
Weak intermolecular forces
Why do covalent bonds have low boiling and melting points?
Because they are held gather with weak into molecular forces and they need little energy to overcome these forces
Why can’t covalent bonds conduct electricity
Because they have no charged particles
What are giant covalent substances joined by?
Many atoms joined by covalent bonds
Why do giant covalent substances have a high melting and boiling point?
Because they are held together by strong covalent bonds that need a lot of energy to overcome
What are diamond and graphite?
Different forms of carbon giant structures of carbon atoms joined together by Covalent bonds
Give the structure of diamond
It is a giant covalent structure and each carbon atom is joined to four other carbon atoms by strong bonds
What network structure do carbon atoms and diamond form?
A regular tetrahedral
Give the properties of diamond
There are no free electrons and it is very hard due to a rigid network of carbon atoms held together by strong covalent bonds. It has a high melting point and doesn’t conduct electricity.
What is the structure of graphite?
It is a giant covalent structure and each carbon atom forms three covalent bonds with other carbon atoms
What are the layers like in graphite?
They form layers of hexagonal rings however there are no covalent bond between layers and there is one non-bonded or delocalised electron from each atom
Name the properties of graphite
Has delocalised electrons that are free to move between the layers and therefore they can conduct electricity
What is graphite useful for?
Electrodes and electrolysis
Why is graphite a good lubricant?
Because the forces between the layers are weak and they can slide over each other easily making it slippery
