yo, what's up ( you don't have to answer that ) um I just need at least 2 of these answered if you want to do all 3 that's cool but you just need to do 2 of them.
1. compare the term " ground state " to the energy of an atom and its electron configuration.
2. describe how metallic bonding accounts for the conductive property of metals. discuss both electrical and heat conduction.
3. describe the relationship between intermolecular forces and physical property. What is the cause of the relationship?

Question

03-02-2021
Chemistry

contestada

yo, what's up ( you don't have to answer that ) um I just need at least 2 of these answered if you want to do all 3 that's cool but you just need to do 2 of them.
1. compare the term " ground state " to the energy of an atom and its electron configuration.
2. describe how metallic bonding accounts for the conductive property of metals. discuss both electrical and heat conduction.
3. describe the relationship between intermolecular forces and physical property. What is the cause of the relationship?

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Аноним Аноним · Answer 1 · 2021-02-03T21:16:01+01:00

Answer:

1. The ground state describes the lowest possible energy that an atom can have. An electron is normally in its ground state, the lowest energy state available.

2. In a metal, atoms readily lose electrons to form positive ions (cations). These ions are surrounded by delocalized electrons, which are responsible for conductivity. The solid produced is held together by electrostatic interactions between the ions and the electron cloud. These interactions are called metallic bonds. The metallic bonding model explains the physical properties of metals. Metals conduct electricity and heat very well because of their free-flowing electrons. As electrons enter one end of a piece of metal, an equal number of electrons flow outward from the other end.

3. Physical properties are affected by the strength of intermolecular forces. Melting, boiling, and freezing points increase as intermolecular forces increase. Vapor pressure decreases as intermolecular forces increase. The physical state and properties of a particular compound depend in large part on the type of chemical bonding it displays. This is because the energy required to disrupt the intermolecular forces between molecules is far less than the energy required to break the ionic bonds in a crystalline ionic compound.

Explanation:

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