STRUCTURE AND BONDING NOTES
Bonds between atoms are called atomic bonds.
Forces between molecules are called intermolecular forces.
o Intermolecular forces are broken and formed when molecular
substances change state (solid, liquid and gas).
Full Notes Bonding
There are only 118 elements in the periodic table, yet there are millions of different
substances on planet earth. The abilities of elements to react together and
‘combine’ with each other give rise to these millions of different substances.
Atoms ‘combine’ by forming bonds between themselves. A small group of atoms
(two or more) bonded together in a unit forms a molecule. When atoms of different
elements combine and bond, a compound is formed.
Atomic bonds are bonds that exist between atoms.
Intermolecular forces are forces that arise between molecules. These forces ‘hold’
molecules together and cause them to exist in either a solid or liquid state.
, THERE ARE THREE TYPES OF ATOMIC BONDING:
Covalent
Ionic
Metallic
There are three key types of intermolecular forces:
Instantaneous, temporary induced, dipole-dipole
Permanent dipole-dipole
Hydrogen bonding
Molecular substances are made of molecules (small groups of atoms covalently
bonded together). When molecular substances melt or boil, it is intermolecular
forces between the molecules that are broken. The atomic bonds within the
molecules remain unchanged.
, QUICK NOTES COVALENT BONDING
A covalent bond is the sharing of one pair of electrons between two atoms.
o Two atomic orbitals from two atoms overlap and create a new area of
electron density between the two atoms.
o The positively charged nuclei of both atoms get attracted to the shared
pair of negatively charged electrons and this pulls them closer
together.
The distance between the centre of each nuclei is called a ‘bond length’.
Non-metal atoms form covalent bonds with other non-metal atoms.
As covalent bonds occur between atoms, they are atomic bonds.
Atomic Structure Recap
Atoms have electrons that travel around a nucleus in ‘orbitals’. Each orbital can
have a maximum of one pair of electrons in. These orbitals exist in shells, and each
Bonds between atoms are called atomic bonds.
Forces between molecules are called intermolecular forces.
o Intermolecular forces are broken and formed when molecular
substances change state (solid, liquid and gas).
Full Notes Bonding
There are only 118 elements in the periodic table, yet there are millions of different
substances on planet earth. The abilities of elements to react together and
‘combine’ with each other give rise to these millions of different substances.
Atoms ‘combine’ by forming bonds between themselves. A small group of atoms
(two or more) bonded together in a unit forms a molecule. When atoms of different
elements combine and bond, a compound is formed.
Atomic bonds are bonds that exist between atoms.
Intermolecular forces are forces that arise between molecules. These forces ‘hold’
molecules together and cause them to exist in either a solid or liquid state.
, THERE ARE THREE TYPES OF ATOMIC BONDING:
Covalent
Ionic
Metallic
There are three key types of intermolecular forces:
Instantaneous, temporary induced, dipole-dipole
Permanent dipole-dipole
Hydrogen bonding
Molecular substances are made of molecules (small groups of atoms covalently
bonded together). When molecular substances melt or boil, it is intermolecular
forces between the molecules that are broken. The atomic bonds within the
molecules remain unchanged.
, QUICK NOTES COVALENT BONDING
A covalent bond is the sharing of one pair of electrons between two atoms.
o Two atomic orbitals from two atoms overlap and create a new area of
electron density between the two atoms.
o The positively charged nuclei of both atoms get attracted to the shared
pair of negatively charged electrons and this pulls them closer
together.
The distance between the centre of each nuclei is called a ‘bond length’.
Non-metal atoms form covalent bonds with other non-metal atoms.
As covalent bonds occur between atoms, they are atomic bonds.
Atomic Structure Recap
Atoms have electrons that travel around a nucleus in ‘orbitals’. Each orbital can
have a maximum of one pair of electrons in. These orbitals exist in shells, and each
