An element X reacts with oxygen to form XO₂ and with chlorine to form XCl₄. XO₂ is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl₄ is a colorless liquid with a boiling point of 58 °C. (c) By using a sourcebook such as the CRC Handbook of Chemistry and Physics, try to determine the identity of element X.

Verified step by step guidance

1. Identify the possible oxidation states of element X based on the compounds XO2 and XCl4. In XO2, X is likely in the +4 oxidation state, and in XCl4, X is also likely in the +4 oxidation state.
2. Consider the physical properties of the compounds. XO2 is a white solid with a high melting point, suggesting it might be a metal or metalloid with strong ionic or covalent bonds. XCl4 is a colorless liquid with a relatively low boiling point, indicating it might be a molecular compound.
3. Consult the CRC Handbook of Chemistry and Physics to find elements that commonly form compounds with oxygen and chlorine in the +4 oxidation state. Look for elements that form stable oxides and chlorides with the given physical properties.
4. Cross-reference the melting and boiling points of XO2 and XCl4 with known compounds in the CRC Handbook. This can help narrow down the possible elements by matching the physical properties.
5. Consider elements that are known to form both XO2 and XCl4 with the described properties. Silicon (Si) is a strong candidate, as it forms SiO2 (a high melting point solid) and SiCl4 (a low boiling point liquid).