Covalent, Ionic and Metallic Bonding Flashcards
Structure between metals?
Giant metallic structure
Bonding between metals?
Metallic bonding
What is metallic bonding?
Electrostatic attraction between positive ions and delocalised electrons in a layered structure
Trend in melting points in metals
Al3+ is stronger than Mg2+ which is stronger than Na+ as it has more protons and more delocalised electrons so a stronger metallic bond
Are metals malleable/ ductile and if yes why?
Yes, because layers of ions can slide over each other
Why are metals electrical conductors?
The delocalised electrons can travel through the layers
Drawing silver as a metal in the mark scheme
6 same sized particles attached , each with a single + in the centre
Group 4 NON-METALS: structure?
Giant macromolecular structure
Group 4 NON-METALS: bonding?
Covalent bonding
What is covalent bonding?
Electrostatic attraction between a shared pair of electrons and a positive nucleus
What is the melting point of group 4 non-metals?
High because very strong covalent bonds must be broken between atoms
Electrical conductivity of silicon dioxide and diamond (group 4)
None as no delocalised electrons or free ions
Electrical conductivity of graphite (group 4)
Can conduct as delocalised electrons between layers can move
Structure of diamond
4 carbon atoms covalently bonded in tetrahedral structure 109.5 degree bond angle
Structure of graphite
3 Carbon atoms covalently bonded in a hexagonal layered structure, 4th electron delocalised between the layers. Bond angle 120 degrees between carbon atoms
Why can graphite act as a lubricant?
Weak van der waal forces between the layers allows the layers to slide past each other
Group 5,6,7,8 non metals structure?
Simple molecular structure
Group 5,6,7,8 non metals bonding?
Covalent bonding
Group 5,6,7,8 non metals melting point?
Low because of weak IMF between molecules so they are easily broken.
Group 5,6,7,8 non metals electrical conductivity?
None due to no free electrons
Why is the melting point of S8 higher than P4 than Cl2?
S8 has more electrons/ is a bigger molecule than P4, than Cl2 than a noble gas do it has more intermolecular forces so needs more energy to break the weak forces
When discussing simple molecular structures what should you talk about to get marks?
IMF
Metals and non-metals structure?
Giant ionic structure
Metals and non-metals bonding?
Ionic bonding
What is ionic bonding?
The strong electrostatic attraction between positive and negative ions
Do Metals and non-metals have high melting points?
Yes because the strong electrostatic forces between positive and negstive ions need lots of energy to break a strong bond
Electrical conductivity in ionic solids?
None as no free ions
Electrical conductivity in molten or aqueous ionic liquids?
Yes, as ions are free to move through the structure
Drawing an ionic lattice mark scheme
3D cube with + and - in correct places
What happens across period 3?
- Increased nuclear charge
- Atomic radius decreases
- Stronger pull on outer shell electrons
- Same shielding
Why does Aluminium have a higher melting point than sodium
No. of outer shell electrons increases so more electrons can be delocalised leading to a greater attraction between positive ions and delocalised electrons
What is a lattice?
A regular repeating pattern
What is the difference between simple molecular and giant macromolecular?
Giant breaks actual covalent bonds, simple breaks weak intermolecular forces between molecules
