Bonding Flashcards
Define Ionic Bonding [2]
Transfer of Electrons from metal to non-metal
Metals lose electrons to form [2]
positive ions
Non-metals gain electrons to form [2]
negative ions
‘_______ force of attraction between opposite charged ions’ [1]
electrostatic
Define Covalent bonds [1]
A shared pair of electrons
Steps to covalent bonds [3]
- Write the atoms
- Number of valence electrons
- How many electrons it wants to gain (number of electrons shared)
define Ion [1]
A charged particle (through bonding)
define Atom [1]
Neutrally charged particle which makes up everything
Ionic bonding has a ____ melting point [1]
high melting point
Ionic bonding is held together by [1]
Electrostatic force of attraction
Describe ionic bonding [5]
*Between metals + non-metals
*Metals lose e- to from positive ions
*Non-metals gain e- to form negative ions
*transfer of electrons
*Electrostatic force of attraction holds ions together
Describe and explain the properties of diamonds [5]
*Giant Covalent
*Carbon atoms
*Held together by lots of covalent bonds
*High melting point
Because lots of covalent bonds that require a
lot of energy to break
*Doesn’t conduct electricity
Because no mobile charged carriers
Describe and explain Graphite [4]
*Giant Covalent
*lots of strong covalent bonds
*Carbon atoms form 3 bonds that require a lot of energy to break
*conducts electricity
Carbon atoms form 3 bonds so it has delocalised electrons between layers
Describe Covalent bonds [5]
*Shared pair of electrons
*Between non-metals
*Small molecule
*Held together by strong covalent bonds
Weak intermolecule forces
*Does not conduct electricity
Because there are no mobile charged carriers
Ionic bonding has a high melting point because… [2]
A lot of energy is required to WEAKEN the electrostatic force of attraction
Describe and explain the melting point of a giant ionic substances [3]
*high melting point
*because strong electrostatic force of attraction between oppositely charged ions
*that require a lot of energy to overcome
Describe and explain the melting point of simple covalent substances [3]
*small molecules
*weak intermolecular forces
*that require a small amount of energy to overcome
Describe and explain the melting point of giant metallic substances [3]
*high melting point
*because strong electrostatic force of attraction between positive metal ions and delocalised electrons
*That require a lot of energy to overcome
Describe and explain the melting point of giant covalent substances [3]
*high melting point
*because lots of strong covalent bonds
*that require a lot of energy to overcome
Describe and explain conductivity of giant ionic substances [4]
*doesn’t conduct when solid
*because the ions are fixed in position
*conducts when molten or aqueous
*because the ions can move and carry charge
Describe and explain the conductivity of simple covalent substances [2]
*doesn’t conduct
*no free electrons
Describe and explain the conductivity of giant metallic substances [3]
*conducts electricity
*because delocalised electrons
*can move and carry charge through the structure
Describe and explain the conductivity of a giant covalent substances [5]
*Diamond and silica don’t conduct
*Because no free electrons
*graphite does conduct
*carbon in graphite only forms 3 bonds
*so, there are free electrons that can move and carry charge through the structure
Name three giant covalent substances [3]
*diamond
*graphite
*silica (silicon Dioxide)
describe a lattice structure [2]
Strong electrostatic force of attraction that holds together opposite charged ions in fixed position (uniform) OoOoO
