Phosphorus and sulfur are two non-metallic elements found on the right-hand side of the Periodic Table. For each element, describe the observations you would see when it burns in air, and write a balanced equation for the reaction. phosphorus: observation; equation. sulfur: observation; equation.
White phosphorus, $\text{P}_4$, is made industrially by heating calcium phosphate(V) rock together with silica, $\text{SiO}_2$, and coke in an electric furnace at $1400\,^{\circ}\text{C}$. Calcium silicate, $\text{CaSiO}_3$, and carbon monoxide are two of the other products. Balance the equation below, which shows the overall reaction. $\_\_\ \text{Ca}_3(\text{PO}_4)_2 + \_\_\ \text{SiO}_2 + \_\_\ \text{C} \rightarrow \_\_\ \text{P}_4 + \_\_\ \text{CaSiO}_3 + \_\_\ \text{CO}$
When white phosphorus is heated to $400\,^{\circ}\text{C}$ without air, it is converted into the red form of the element. The table below gives some properties of the two forms, which are called allotropes. Suggest the type of structure and bonding in each allotrope.
In both allotropes, phosphorus has valency 3. Suggest by means of diagrams how the phosphorus atoms may be joined together in each allotrope.