Bonding Flashcards
Learning (22 cards)
What are ions?
Charged particles
What are anions?
Negative ions
What are cations?
Positive ions
What is metallic bonding?
Strong electrostatic forces of attraction between positive metal ions and delocalised electrons.
Why do metals have high melting/boiling points?
Strong electrostatic forces of attraction between metal ions and delocalised electrons, in a giant metallic lattice so lots of energy needed to break them.
Why do metals conduct electricity?
Delocalised electrons which are free to move.
Why are metals malleable and ductile?
They have layers of cations which can slide over each other.
What is ionic bonding?
The strong electrostatic forces of attraction between oppositely charged ions.
Why do ionic compound have high melting/boiling points?
There are strong electrostatic forces of attraction between oppositely charged ions in a giant lattice, where a lot of energy is needed to break the bonds
In what state do ionic compounds conduct electricity?
In Liquid because ions can flow.
In what state do ionic compounds not conduct electricity?
In solid because ions are in fixed position and cannot flow.
Why are ionic compounds brittle?
When force is applied, ions shift and line up. Ions repel, so crystal structure breaks apart.
What is giant covalent bonding?
Strong electrostatic forces of attraction between a shared pair of electrons and positive nuclei of 2 atoms.
Why do giant covalent structure have high melting/boiling points?
They have a giant structure with strong electrostatic forces of attraction between shared pair of electrons and nuclei which require ahigh amount of energy to break the strong covalent bonds.
Why does diamond not conduct electricity?
All electrons used up in covalent bonds so no delocalised electrons to flow.
Why do graphene and graphite conduct electricity?
Each cation forms 3 covalent bonds, so there is a delocalised electron free to move.
Why is diamond hard?
Diamond is tetrahedral, with many strong covalent bonds, requiring much energy to break.
Why is graphite soft?
Graphite has hexagonal layers, with weak forces which break easily so layers can slide over each other.
What is simple molecular covalent bonding?
Strong electrostatic forces of attraction between a shared pair of electrons and 2 positive nuclei.
Why do simple molecular covalent structures have low melting/boiling points?
A small amount of energy is required to overcome the weak intermolecular forces between the nuclei.
Do simple molecular structures conduct electricity?
No because no delocalised electrons are free to move.
