1.3 Bonding
No description yet. This curated deck is ready for daily study.
Card preview (24)
What is ionic bonding
Strong electrostatic forces of attraction between oppositely charged ions held in a lattice
Give an example of an ionically bonded substance
NaCl
How high are ionically bonded substances mp and bp? Why?
High - takes lots of energy to break strong electrostatic forces of attraction between oppositely charged ions
Do ionic compounds conduct electricity? Why?
Yes, when molten / in solution as the ions are free to move and carry charge (don’t conduct when solid)
What is simple molecular covalent bonding?
Strong covalent bonds between atoms, weak Van de Waals forces of attraction between molecules
Are there any lone electrons in simple covalent bonding
No - all involved in bonding
Can simple molecular covalent molecules conduct electricity? Why?
No - all electrons used in bonding and aren’t free to move
Do simple molecular substances have a high/low mpt and bpt? Why?
Low - weak van de Waals forces of attraction between molecules that don’t take much energy to overcome (these are overcome rather than covalent bonds)
Describe macromolecular covalent bonding
Lattice of many atoms held together by strong covalent bonds
Do substances with macromolecular covalent bonds have high/low mpt and bpt ? Why?
High, as it takes a lot of energy to overcome many strong covalent bonds
Do substances with macromolecular covalent bonds conduct electricity?
Most don’t as all electrons are used in bonding
Describe the structure of diamond
3D tetrahedral structure of C atoms with each C atom bonded to 4 others
Describe the structure of graphite
Similar to diamond but each atom is only bonded to 3 others so it is in layers Weak van de Waals forces of attraction between layers allow them to Slide Over each other —> soft and slippery One electron of each carbon is delocalised and can carry charge —> can conduct electricity
Describe metallic bonding
Lattice of positive metals ions strongly attracted to a sea of delocalised electrons. Layers slide over each other - malleable
Do metallic compounds have high mpt / bpt ? Why ?
High as strong forces of attraction between positive metal ions and negatively charged sea of delocalised electrons
Do metallic compounds conduct electricity ? Why?
Yes as delocalised electrons can move throughout the metal to carry charges
How does the strength of metallic bonding change across the periodic table? Why?
Increases - higher mpt and bpt, stronger Higher charge on metal ions More delocalised electrons per metal ion Stronger forces of attraction between
Define electronegativity
The ability of an atom to attract a pair of electrons in a covalent bond
What affects electronegativity ? (3)
Atomic radius Nuclear charge Electron shielding
What is the most electronegative element?
Fluorine (F) - 4.0 on paulings scale Largest nuclear charge for its electron shielding, smallest atomic radius
How do you get a non-polar bond?
Both bonding elements have the same electronegativity
When do you get a polar bond?
When both bonding atoms have different electronegativity
What is the strongest form of inter-molecular force?
Hydrogen bonding
What is the weakest form of intermolecular force?
Van de Waals forces