Bonding
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Define ionic bonding
Ionic bonding involves electrostatic attraction between oppositely charged ions in a lattice
What is the compound formula for sulfate?
SO4^2-
What is the compound formula for sulfate?
SO4^2-
What is the formula for hydroxide ?
OH-
What is the formula for carbonate ?
CO3^2-
What is the formula for ammonium?
NH+4
Define covalent bonding
A single covalent bond contains a shared pair of electrons Held by electrostatic attraction
What do multiple bonds contain ?
Multiple bonds contain multiple pairs of electrons
Define a coordinate /dative covalent bond
Contains a shared pair of electrons with both electrons supplied by one atom
What happens in a coordinate covalent bond ?
-atom accepts the electron pair is an atom that doesn’t have a filled outer main level of electrons-atom is electron deficient -the atom is donating the electrons has a pair of electrons that is not being used in a bond called a lone pair
What are the similarities with an ordinary covalent bond and coordinate bonds?
Coordinate bonds have exactly the same strength and length as ordinary covalent bonds between the same pair of atoms
Define metallic bonding
Metallic bonding involves attraction between delocalised electrons and positive ions arranged in a lattice
What does the number of delocalised electrons depend on ?
Number of delocalised electrons depends on how many electrons have been lost by each metal atom
What are the properties of metals?
Good conductors of electricity Good conductors of heat Malleable Ductile High mpg and bpt
Why are metals good conductors of electricity?
Delocalised electrons move freely throughout the structure enabling current to flow
Why are metals good conductors of heat?
Closely packed ions enables efficient spread of energy through vibrations
Why are metals malleable and ductile ?
Layers of positive ions can slide over each other
Why do metals have high mpt and bpt?
Strong electrostatic attraction between positive ions and delocalised electrons
Define electronegativity
Electronegativity is the power of an atom to draw electron density in a covalent bond towards itself
What scale shows how electronegative an atom is?
Pauling scale=0-4 the greater the number the more electronegativite the atom the noble gases have no number because they do not in general form covalent bonds
What does electronegativity depend on?
Nuclear charge Distance between the nucleus and the outer shell electrons Shielding of nuclear charge by electrons in inner shell
Describe nuclear charge in electronegativity terms
Attraction between positive protons in the nucleus and electrons .an increase in protons means increased attraction for electron number in outer shells thus increased nuclear charge means increased electronegativity
Describe atomic radii in terms of electronegativity
Electrons closer to nucleus are more strongly attracted to positive nucleus electrons further away are less attracted so higher atomic radii means decreased electronegativity
Describe shielding of nuclear charge by electrons in inner shells through electronegativity
Filled energy levels can shield the effects of nuclear charge outer electrons are less attracted to nucleus thus adding extra shells/sub shells in atom will cause electrons to feel less attractive force higher number of inner shells and sub shells decreases electronegativity