Chemical bonds in substances
- molecular compounds (covalent)
- ie: h2O, nh3, hf. Usually made up of nonmetals
- structure and bonding
- attractive force that holds bonds together are
covalent bonds
- attractive force originates from sharing of electrons
- water moleculares are held together by covalent
bonds
- intermolecular forces responsible for molecules
staying together in condensed together. Only for
molecular compounds
- intramolecular forces = covalent bonding.
- intermolecular forces = h-bonding, dipole dipole,
London Forces
-Network Covalent Compounds
- ie: diamond, graphite, silicon dioxide held together by
network of covalent bonds and sometimes intermolecular
forces too
- in a diamond, carbon bonded to 4 others
tetrahedrally. Held together by interlocking
covalent bonds
- Bucky Ball compounds consists of c60 clusters held by
intermolecular forces.
- strongest to weakest: covalent bonds, intermolecular
forces
- ionic compounds
-solid ionic compounds consists of enormous array of
cations and anions
- no distinction between intermolecular forces vs.
intramolecular forces
, - unlike molecular substances, ionic substances don’t
contain groups of atoms that function as unit. They stay
together because of electrostatic attraction
- attractive forces between cations and anions called
ionic bonds
- Metals
-structure and bonding
- each atom donates its valence electrons for form
pool of electrons. Cations held together by their
attractions to “sea/pool of electrons”. This
attractive force referred to as metallic bond
- no distinction between intra and inter forces
Types of intermolecular forces
- imf consists of Dipole Dipole, London forces and H-bonding
dipole dipole interaction
- polar molecules with partial positive charge on 1 end
and partial negative charge on other tend to line up so
positive end of 1 dipole is near negative end.
- dipole is when one end is negative, other positive. IE:
HF, HCL, etc. I
- stronger electronegativity, stronger dipole
attraction
Hydrogen bonding
- When H is bonded to one of the small, electronegative
atoms, n, o, f, the positive h will attract the lone pair of
electroneg atoms
- each water molecule can form up to 2 other
hydrogen molecules • c-
1 lone pair
•
le : Ntfs H N t
- -
1- 1 Of the ✓Malli
atoms
+1 electroneg
- molecular compounds (covalent)
- ie: h2O, nh3, hf. Usually made up of nonmetals
- structure and bonding
- attractive force that holds bonds together are
covalent bonds
- attractive force originates from sharing of electrons
- water moleculares are held together by covalent
bonds
- intermolecular forces responsible for molecules
staying together in condensed together. Only for
molecular compounds
- intramolecular forces = covalent bonding.
- intermolecular forces = h-bonding, dipole dipole,
London Forces
-Network Covalent Compounds
- ie: diamond, graphite, silicon dioxide held together by
network of covalent bonds and sometimes intermolecular
forces too
- in a diamond, carbon bonded to 4 others
tetrahedrally. Held together by interlocking
covalent bonds
- Bucky Ball compounds consists of c60 clusters held by
intermolecular forces.
- strongest to weakest: covalent bonds, intermolecular
forces
- ionic compounds
-solid ionic compounds consists of enormous array of
cations and anions
- no distinction between intermolecular forces vs.
intramolecular forces
, - unlike molecular substances, ionic substances don’t
contain groups of atoms that function as unit. They stay
together because of electrostatic attraction
- attractive forces between cations and anions called
ionic bonds
- Metals
-structure and bonding
- each atom donates its valence electrons for form
pool of electrons. Cations held together by their
attractions to “sea/pool of electrons”. This
attractive force referred to as metallic bond
- no distinction between intra and inter forces
Types of intermolecular forces
- imf consists of Dipole Dipole, London forces and H-bonding
dipole dipole interaction
- polar molecules with partial positive charge on 1 end
and partial negative charge on other tend to line up so
positive end of 1 dipole is near negative end.
- dipole is when one end is negative, other positive. IE:
HF, HCL, etc. I
- stronger electronegativity, stronger dipole
attraction
Hydrogen bonding
- When H is bonded to one of the small, electronegative
atoms, n, o, f, the positive h will attract the lone pair of
electroneg atoms
- each water molecule can form up to 2 other
hydrogen molecules • c-
1 lone pair
•
le : Ntfs H N t
- -
1- 1 Of the ✓Malli
atoms
+1 electroneg
