12287146
Description
Mind Map by Dominic Weston, updated more than 1 year ago
|
Created by Dominic Weston
about 6 years ago
|
|
Bonding
- Ionic
- Structure
- Ionic crystals are giant lattices of ions
- "Giant" as made up of many repeating units
- "Giant" as made up of many repeating units
- Ionic crystals are giant lattices of ions
- Properties
- Conduct electricity when molten or dissolved
- Ions are free to move and carry a charge
- Ions are free to move and carry a charge
- High melting points
- Strong electrostatic forces need lots of energy to break bonds
- Strong electrostatic forces need lots of energy to break bonds
- Tend to dissolve in water
- Polar water molecules pull ions aways from lattice causing it to dissolve
- Polar water molecules pull ions aways from lattice causing it to dissolve
- Conduct electricity when molten or dissolved
- Bonding
- Strong electrostatic forces of attraction between oppositley charged ions
- Electrons transfered between one atom to another forming ions
- Not just atons, compounds can form compound ions
- Sulfate SO4 ^2-
- Hydroxide OH-
- Nitrate NO3 ^-
- Carbonate CO3 ^2-
- Ammonium NH4 ^+
- Compounds have overall neutral charge
- Sulfate SO4 ^2-
- Not just atons, compounds can form compound ions
- Electrons transfered between one atom to another forming ions
- Strong electrostatic forces of attraction between oppositley charged ions
- Structure
- Covalent
- Molecules held together by strong covalent bonds
- Atoms share electrons to fully saturate both outer shells
- Both nuclei attact to shared electrons electrostatically
- Double or triple covalent bonds share multiple pairs or electrons
- Covalent bonds shown by 'dash' e.g. C-H
- Covalent bonds don't break during melting or boiling, other than giant covalent substances
- To melt or boil, just overcome the intermolecular forces, dont need break covalent bonds
- Gives simple covalent compounds relatively low melting / boiling points
- So Cl2 is gas at room temp has low MP and BP
- Diamond does need the covalent bonds broken, sublimes at 3600 cel
- Diamond does need the covalent bonds broken, sublimes at 3600 cel
- MP and BP determined by strength of attraction between particles
- So Cl2 is gas at room temp has low MP and BP
- Gives simple covalent compounds relatively low melting / boiling points
- To melt or boil, just overcome the intermolecular forces, dont need break covalent bonds
- Covalent bonds don't break during melting or boiling, other than giant covalent substances
- Covalent bonds shown by 'dash' e.g. C-H
- Double or triple covalent bonds share multiple pairs or electrons
- Dative covalent bond
- Covalent bond in which both electrons come from the same atom
- Shown by an arrow to replace the 'dash' N-->H
- Shown by an arrow to replace the 'dash' N-->H
- Covalent bond in which both electrons come from the same atom
- Both nuclei attact to shared electrons electrostatically
- Atoms share electrons to fully saturate both outer shells
- Giant Covalent structures (Macromolecular)
- Many atoms covalently bonded
- Diamond
- Hardest known substance
- Made of carbon, each bonded covalently with 4 other carbon atoms
- Forms a tetrahedral shape with very strong covalent bonds
- High melting point, extremely hard, good thermal conductor
- Cannot conduct electricty (all e- held in bonds), cannot dissolve, refracts light
- Cannot conduct electricty (all e- held in bonds), cannot dissolve, refracts light
- High melting point, extremely hard, good thermal conductor
- Forms a tetrahedral shape with very strong covalent bonds
- Made of carbon, each bonded covalently with 4 other carbon atoms
- Hardest known substance
- Graphite
- Carbon arranged in sheets of flat hexagons with delocalised e-
- Weak bonds between layers causes them to slide in pencils
- Delocalised eletrons can move to carry a charge
- Layers far apart compared to covalent bonds - gives a low density makes strong and lightweight
- Strong covalent bonds in hexagon sheets causes high melting point
- Completely insoluble
- Completely insoluble
- Strong covalent bonds in hexagon sheets causes high melting point
- Layers far apart compared to covalent bonds - gives a low density makes strong and lightweight
- Delocalised eletrons can move to carry a charge
- Weak bonds between layers causes them to slide in pencils
- one carbon bonded to 3 others
- Carbon arranged in sheets of flat hexagons with delocalised e-
- Many atoms covalently bonded
- Molecules held together by strong covalent bonds
- Shape of molecules
- Shape of a molecule depends on the number or pairs of electrons
- Electron pairs exist as charged clouds - there is a high probability of electron pair
- As the clouds are all negative they repel each other
- Shape affects how much it repels other clouds
- LP:LP strongest repulsion, biggest angles
- LP:BP Strong
- BP:BP Weakest repulsion, smallest angles
- Can work out the shape of molecule using VSEPR
- Find number of electrons on the outer shell of central atom
- Find how many electrons are used in bonding pairs
- Check for charge - positive = less electrons
- Sort any left over electrons as lone pairs
- Sort any left over electrons as lone pairs
- Check for charge - positive = less electrons
- Find how many electrons are used in bonding pairs
- Shapes
- 2 Pairs
- 2 BP Linear
- 2 BP Linear
- 3 Pairs
- 3 BP Trigonal Planar
- 3 BP Trigonal Planar
- 4 Pairs
- 4 BP Tetrahedral
- 3BP 1LP Trigonal Pyramidal
- 2BP 2LP Bent
- 4 BP Tetrahedral
- 5 Pairs
- 5 BP Trigonal Bipyramidal
- 4BP 1LP Seesaw
- 3BP 2LP T-shaped
- 5 BP Trigonal Bipyramidal
- 6 Pairs
- 6 BP Octahedral
- 4BP 2LP Square Planar
- 6 BP Octahedral
- 2 Pairs
- Find number of electrons on the outer shell of central atom
- LP:LP strongest repulsion, biggest angles
- Shape affects how much it repels other clouds
- As the clouds are all negative they repel each other
- Electron pairs exist as charged clouds - there is a high probability of electron pair
- Shape of a molecule depends on the number or pairs of electrons
- Polarisation and Forces
- Intermolecular forces hold molecules together
- Electrogenativity is the ablility of an atom to attact an electron pair
- Fluorine, oxygen, chlorine all strongly electronegative
- Fluorine, oxygen, chlorine all strongly electronegative
- These forces are very weak, weaker than covalent, ionic and metallic bonds
- vann der Waals
- Perm. Dipole-Dipole
- Hydrogen
- Only happens between FON elements when covalently bonded to hydrogen
- FON very electrogenative, draws BP electrons from H
- As polar bond and Hydrogen high charge density, hydrogen can form bonds with lone pairs on FON atoms
- Increases boiling, melting points. Water, HF higher boiling point in halides cause of h-bonds
- Increases boiling, melting points. Water, HF higher boiling point in halides cause of h-bonds
- As polar bond and Hydrogen high charge density, hydrogen can form bonds with lone pairs on FON atoms
- FON very electrogenative, draws BP electrons from H
- Only happens between FON elements when covalently bonded to hydrogen
- Polar Bonds
- Causing weak electrostatic fordes of attaction between partial charges
- Causing weak electrostatic fordes of attaction between partial charges
- Hydrogen
- Cause all atoms and molecules to attract to each other
- At any moment electrons likely to be on one side of the atom causing a temp. dipole
- This can cause another temp. dipole opposite charged on the next atom, 2 dipoles attracted to each other
- Temp. dipoles constantly created/destroyed overall attraction though
- Temp. dipoles constantly created/destroyed overall attraction though
- This can cause another temp. dipole opposite charged on the next atom, 2 dipoles attracted to each other
- At any moment electrons likely to be on one side of the atom causing a temp. dipole
- Perm. Dipole-Dipole
- vann der Waals
- Electrogenativity is the ablility of an atom to attact an electron pair
- Covalent bonds polarised by differences in electronegativity
- Covalent bonds between the same element are non-polar as same electronegativity
- Water is polar and substances that are polar will dissolved well in it
- Water is polar and substances that are polar will dissolved well in it
- Covalent bonds between the same element are non-polar as same electronegativity
- Difference in electronegativity causes polar bond and a permanent dipole
- Dipole is a difference in charge between 2 by shift in electron density
- Dipole is a difference in charge between 2 by shift in electron density
- Intermolecular forces hold molecules together
- Metallic
- Metals exist in giant metallic lattice structures
- Outer most shell of electrons is delocalised
- Leaving a positive metal ion that is attracted to d.electrons
- Forms a lattice of closely packed positive ions
- In a sea of delocalised electrons (metalic bonding)
- Properties
- High melting points as strong electrostatic attraction between electrons and ions
- More delocalised electrons per atom, stronger bonding, so higher melting point
- D.electrons can pass kinetic energy to each other making them good thermal conductors
- Good electrical conductors as d.electrons can move to carry a current / charge
- Insoluble (except liquid metals)
- Insoluble (except liquid metals)
- Good electrical conductors as d.electrons can move to carry a current / charge
- D.electrons can pass kinetic energy to each other making them good thermal conductors
- More delocalised electrons per atom, stronger bonding, so higher melting point
- High melting points as strong electrostatic attraction between electrons and ions
- Materials (NOT RELATED TO METALLIC)
- Covalent bonds don't break during melting or boiling
- To melt or boil, only break bond between molecules, inter force
- Simple covalent, easy to overcome these forces
- Giant covalent need to break covalent bonds
- thats why it never really melts, only sublimes at 3600 cel
- thats why it never really melts, only sublimes at 3600 cel
- Giant covalent need to break covalent bonds
- Simple covalent, easy to overcome these forces
- To melt or boil, only break bond between molecules, inter force
- Covalent bonds don't break during melting or boiling
- Properties
- In a sea of delocalised electrons (metalic bonding)
- Forms a lattice of closely packed positive ions
- Leaving a positive metal ion that is attracted to d.electrons
- Outer most shell of electrons is delocalised
- Metals exist in giant metallic lattice structures
Want to create your own Mind Maps for free with GoConqr? Learn more.