Bonding Properties Flashcards
Monatomic properties and what group do they appear
Noble gasses
Low melting and boiling points due to the van der Wahls between the atoms which take very little energy to overcome
Poor conductors of electricity because these atoms are neutral and therefore have no delocalised electrons
How are the size of van der Wahls forces effected ?
Number of electrons
Atomic radius
If more electrons and larger atomic radius the size of the van der Wahls forces will increase
What are iodines properties ?
Simple molecular
Low melting and boiling point
Because of weak intermolecular forces, which are van der Wahls which takes little energy to overcome
Poor conductor of electricity
Because the molecules are neutral and have no delocalised electrons
What are the properties of Ice ?
Simple molecular
Low melting and boiling point
Because of the weak intermolecular forces, which are Van der Wahls, dipole-dipole and hydrogen bonding
Water has a higher melting point point than other simple molecules because of the hydrogen bonding
Poor conductor of electricity because the molecules are neutral and have no delocalised electrons
What are the properties of Diamond ?
Giant covalent lattice
High melting and boiling point
Because of the strong covalent bonds between atoms which take a lot of energy to overcome
Poor conductor of electricity as all electrons are involved in bonding so no delocalised electrons
What are the properties of Graphite ?
Giant covalent lattice
High melting and boiling point because of the strong covalent bonds between atoms. These take a lot of energy to overcome
Good conductor of electricity because each carbon is joined to 3 others and there is one delocalised electron per atom. Electrons are free to move through the structure and carry charge
What are the properties of Sodium Chloride ?
Giant ionic lattice
High melting and boiling point
Because of strong electrostatic forces of attraction between oppositely charged ions which take a lot of energy to overcome
Conducts when molten or in aqueous solution because ions are free to move and carry charge through the structure.
Poor conductor in solids as the ions are fixed in position and unable to move
What are the properties of Magnesium ?
Giant metallic lattice
High melting and boiling point
Strong electrostatic forces of attraction between positive ions and delocalised electrons, these take a lot of energy to overcome
Good conductor of electricity because the outer shell electrons are delocalised and electrons are free to move through the structure and carry charge
Give the order of the strength of intermolecular forces from highest to lowest
Hydrogen bonding, dipole-dipole, Van der Wahls
Explain why HF has a higher boiling point than NH3
There is a greater difference in electronegativity between H and F than the H and N
This results in a stronger dipole moment in HF
Explain why some molecules have polar bonds but do not have a permanent dipole
For example: CO2 and CCl4
Polar bonds cancel each other out if the molecule is symmetrical
How is the strength of ionic bonding affected ?
Size of atom - smaller the ion the stronger the ionic bonding
Charge - the greater the charge on the ion the stronger the ionic bonding
Ions get bigger down the group
How is the strength of metallic bonding affected ?
Size of atoms - the smaller the atom the stronger the metallic bonding
Nuclear charge - the greater the number of protons the stronger the metallic bonding
Number of delocalised electrons - the more delocalised electrons the stronger the metallic bonding
What is the definition of Electronegativity ?
The power of an atom to attract the pair of electrons in a covalent bond
