Reactivity and structure 2
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Why is a metallic bond non-directional?
Electrons shared with every cation
Lattice
3D repeating structure
Properties of metals
Good thermal and electrical conductors melleable strength
Can two metals bond together?
Yes but most likely through an alloy (multiple metals). Brass contains copper and zinc
Ionic bond
A strong electrostatic attraction between positive and negative ions
Binary ionic compound
A binary ionic compound is composed of ions of two different elements like sodium iodide and sodium chloride. A non binary ionic bond is NaNO₃.
Monatomic ion
A monatomic ion is a ion that consists of only one atom “Monobrow”
Polyatomic ion
A polyatomic ion is an ion that consists of two or more atoms such as sulphate.
Ionic lattice
An ionic lattice is a regular repeating structure consisting of alternating cations and anions. Also 3D.
Bonding of ionic compound
Electrostatic attraction between cations and anions. Ionic bond
Characteristics of ionic bonding
Not volatile Soluble in water Brittle
Covalent bond
Bonds form to form a stable electron configuration and release energy. Electrons are shared
Octet rule
Tendency of atoms to prefer to have 8 electrons in the valence shell
What is the duplet rule and what elements does it apply to?
Same as octet rule except it’s a tendency to have 2 electrons in valence shell. This applies to hydrogen
Difference between lone pair and bonding pair of electrons?
Lone pair - not bonded to another element Bonded pair - bonded to another element
Sigma bond
Caused by direct overlap of two orbitals and is stronger than pi bonds. Every covalent bond has a sigma bond.
Pi bond
Caused by sideways overlap of two orbitals and is much weaker than sigma bonds.
Coordination bond
Both electrons shared from same atom. Often shown by an arrow pointing from the atom which donates the lone pair to the atom which receives it.
Resonance
Molecule or polyatomic ion for which two possible Lewis formula’s can be drawn.
Resonance hybrid
More stable than Lewis structures and is when more than two possible Lewis structures.
Electronegativity
Ability of an atom to attract a bonding pair of electrons in a covalent bond.
Dipole moment
Measure of net polarity which is the magnitude of charge at either end of the molecular dipole times the distance between charges.
London forces
• Exist in all molecules • May also be known as dispersion forces or instantaneous induced dipole-dipole forces More info in revision book
What affects the magnitude of London forces?
• Number of electrons • Size of electron cloud • Shapes of molecules