Elemental phosphorus exists in a few different allotropes, two of which are listed below.White phosphorus: a molecular substance with the formula P4.Black phosphorus: an extended network of phosphorus atoms connected by covalentbonds.Which of these two allotropes would you expect to have the higher melting point andwhy?White phosphorus, because the strongest interaction broken while melting is LDFs,which require more energy to overcome.White phosphorus, because the strongest interaction broken while melting iscovalent bonds, which require more energy to overcome.Black phosphorus, because the strongest interaction broken while melting is LDFs,which require more energy to overcome.Black phosphorus, because the strongest interaction broken while melting iscovalent bonds, which require more energy to overcome.O Not enough information is given in order to determine relative melting points.

To answer whether white or black phosphorus has a high melting point and explain the reason.

Elemental phosphorus exists in a few different allotropes, two of which are listed below. White phosphorus: a molecular substance with the formula P4. Black phosphorus: an extended network of phosphorus atoms connected by covalent bonds. Which of these two allotropes would you expect to have the higher melting point and why? White phosphorus, because the strongest interaction broken while melting is LDFs, which require more energy to overcome. O White phosphorus, because the strongest interaction broken while melting is covalent bonds, which require more energy to overcome. Black phosphorus, because the strongest interaction broken while melting is LDFs, which require more energy to overcome. Black phosphorus, because the strongest interaction broken while melting is covalent bonds, which require more energy to overcome. O Not enough information is given in order to determine relative melting points.

Elemental phosphorus exists in a few different allotropes, two of which are listed below. White phosphorus: a molecular substance with the formula P4. Black phosphorus: an extended network of phosphorus atoms connected by covalent bonds. Which of these two allotropes would you expect to have the higher melting point and why? White phosphorus, because the strongest interaction broken while melting is LDFs, which require more energy to overcome. O White phosphorus, because the strongest interaction broken while melting is covalent bonds, which require more energy to overcome. Black phosphorus, because the strongest interaction broken while melting is LDFs, which require more energy to overcome. Black phosphorus, because the strongest interaction broken while melting is covalent bonds, which require more energy to overcome. O Not enough information is given in order to determine relative melting points.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter8: Molecules And Materials

Section: Chapter Questions

Problem 8.92PAE

See similar textbooks

Similar questions

8.45 Describe how interactions between molecules affect the vapor pressure of a liquid.
Silicon carbide, SiC, is a very hard, high-melting solid. What kind of crystal forces account for these properties?
Classify each substance in the table as either a metallic, ionic, molecular, or covalent network solid: Substance Appearance Melting Point Electrical Conductivity Solubility in Water X lustrous, malleable 1500 C high insoluble Y Soft, yellow 113 C None Insoluble Z Hard, white 800 C Only if melted/dissolved soluble
8.41 What is the specific feature of N, O, and F that causes them to play a role in hydrogen bonding?
A common prank on college campuses is to switch the salt and sugar on dining hall tables, which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearance, these two substances differ greatly in their properties, since one is a molecular solid and the other is an ionic solid. How do the properties differ and why?
8.39 Under what circumstances are ion-dipole forces important?
8.81 Carbon tetrachloride (CCl4) is a liquid at room temperature and pressure, whereas ammonia (NH3) is a gas. How can these observations be rationalized in terms of intermolecular forces?