Bonding Flashcards
Why does (magnesium)metals have high boiling points?
S- Magnesium have a giant metallic lattice structure (with)
A- strong electrostatic forces of attraction (between)
B- positively charged Mg2+ cations and the negatively charged sea of delocalised mobile valence electrons
E- Hence a lot of energy is required to overcome the force.
Why can Magnesium(metals) conduct electricity?
Magnesium have a giant metallic lattice structure
their sea of mobile delocalised valence electrons act as mobile charged carriers to conduct electricity
Why is magnesium (metals) malleable and ductile
Magnesium have a giant metallic structure. The metal cations are of the same size and arranged in regular manner.
When a force is applied, the layers of cations can slide over each one another easily without breaking the non-directional metallic bonds
Why does NaCl (ionic substances) have high melting points?
S- NaCl have a giant ionic lattice structure (with)
A- strong electrostatic forces of attraction (between)
B- Na+ and Cl- ions
E. Therefore a lot of energy is required to overcome the force
Why NaCl (ionic substances) cannot conduct electricity in solid state?
The NA+ and Cl- are held in fixed positions by the strong electrostatic forces of attraction between the Na+ and Cl- ions in the giant ionic lattice structure.
Hence the ions cannot move freely to conduct electricity.
Why NaCl (ionic substances) conduct electricity in molten and aqueous state?
The strong electrostatic forces of attraction of the Na+ and Cl- ions are partially overcome. Hence the ions can move freely.
Why are NaCl (ionic substances) soluble in water?
There are effective interactions between the Na+ and Cl- ions and the water molecules
Why does CO2 (covalent molecules) have low melting points?
CO2 have a low melting and boiling point due to its simple covalent structure.
A small amount of force is required to overcome the weak intermolecular forces between the CO2 molecules
Why does covalent molecules not conduct electricity?
Covalent substance consists of uncharged molecules. Hence there is no mobile charged carriers to conduct electricity.
Why does diamond (giant covalent substances) have high melting points?
Diamond has a giant covalent structure and a lot of energy is required to overcome the strong covalent bonds between the carbon atom
Why does diamond not conduct electricity?
Diamond have a giant covalent structure and each carbon atom is bonded to 4 other carbon atoms and since all valence electrons are used in bonding, the are no mobile charged carriers.
Why does graphite conduct electricity?
Graphite can conduct electricity because each carbon atom is bonded to 3 other carbon atom,and uses 3 valence electrons in covalent bonding. hence the 4th valence electron is not used in bonding and is delocalised and can move freely along the layers to conduct electricity
Why is graphite soft and slippery?
Graphite is soft and slippery as a little amount of energy is required to overcome the weak intermolecular forces of attraction between the layers of carbon atoms enabling the layers to slide over each other easily
