Bonding Flashcards
What is ionic bonding and give an example
Strong electrostatic forces between oppositely charged ions in a lattice
E.g NaCl (salt)
Describe and explain why ionic bonding has its properties?
High m.p. and b.p. —> requires lots of energy to break electrostatic forces
Conducts electricity —> when in solution ions are free to carry charge
What is simple molecular covalent bonding?
Give some of its properties
Strong covalent bonds between atoms but weak Van der Waals
Cannot conduct electricity (electrons aren’t free to move)
Has a low m.p. and b.p. (weak VdW)
Describe macromolecular bonding and give some of its properties
Lattice of many atoms held together by covalent bonds
High m.p. and b.p.
Doesn’t conduct electricity
Compare and contrast the structure of diamond and graphite
Both have a macromolecular covalent structure
Each C in diamond is bonded to 4 others
In graphite each C is only bonded to 3
Describe metallic bonding
Lattice of +ve metal ions strongly attracted to a sea of delocalised electrons
Explain the trends and properties of metallic bonding
High m.p. and b.p. —> strong attraction betwenn +ve ions and -ve electrons
Conduct electricity —> delocalised electrons can carry charge
Strength of bond increases across the period —> more delocalised electrons which means a stronger force between them
Define electronegativity (EN)
Ability of an atom to attract the pair of electrons in a covalent bond
What affects EN?
Nuclear charge
Atomic radius
Electron shielding
What’s the difference between a non-polar and polar bond?
Non-polar = both bonding atoms have the same EN
Polar = bonding atoms have different EN
Describe Van der Waals force of interaction
Random movement of electrons creates temporary dipoles
Induces dipole in neighbouring molecule
Temporary induced dipole-dipole (VdW)
Describe a permanent dipole-dipole attraction
Molecules with polar bonds have permanent dipoles
Attraction between those dipoles and neighbouring molecules
What is a dative/co-ordinate covalent bond?
When an electro deficient atom accepts a lone pair of electrons from another atom
Name the shape, bond angle and how many bonded and lone pairs there are
Linear = 180 —> 2b, 0l
Trigonal Planar = 120 —> 3b, 0l
Tetrahedral = 109.5 —> 4b, 0l
Trigonal bypyramid = 90 and 120 —> 5b, 0l
Octahedral = 90 —> 6b, 0l