Deduce the reason why silicon dioxide has high melting point, taking into consideration what you know about it's structure and type of bonding.

Silicon dioxide, SiO2 , and silicon(IV) chloride, SiCl4 , are both covalently bonded compounds.The table shows the melting and boiling points of these two compounds, and the physical state of silicon dioxide at room temperature. Compound Melting point in °C Boiling point in °C Physical state at room temperature SiO2 1710 2230solid SiCl4 −6958(i) Complete the table by giving the physical state of silicon(IV) chloride at room temperature. (1)(ii) Explain, in terms of structure and bonding, why silicon dioxide has a much higher melting point than silicon(IV) chloride.(6)

Explain why ionic substances have high melting points.

Potassium iodide is an ionic compound.What is the reason for potassium iodide's high melting point?They are solids at room temperature.The large number of strong electrostatic attractive forces.Strong covalent bonds in all directions in the lattice.Weak forces between the molecules.

At what temperature does silicon melt?98°C883°C1414°C3185°C3265°C

The melting point of copper is 1085°C.Order the following statements to explain why the melting point of copper is so high. 1st point2nd point3rd pointPossible AnswersThere are weak forces of attraction in all direction in the structure.A lot of energy is needed to overcome these forces of attraction between metal atom and the delocalised electron.There are strong forces of attraction in all direction in the structure.A lot of energy is needed to overcome these forces of attraction between metal ion and the delocalised electron.This causes the melting point to be very high.I DON'T KNOWRESETSUBMIT ANSWER