Using grammatically correct English sentences describe how the nature of the bonding in MgF2 (s) and Zn(s) differ. (Don't just name the different types of bonding-describe how they are different.

Which of the following are metallic? F2(g), Co(s), NaCl(s), H2O(s), C6H6(l) (benzene), Pb(s), Xe(g)

Could you not guess that F2 and Xe, since they are listed as gases, are not metallic? You know NaCl and H2O are not metals. The only solids are Co and Pb and those are the only possibilities out of those listed.

For the first one, MgF2 is a crystal made of ionic bonds. Zn solid metal are metallic bonds. Use those two types to describe how they are different. Someone here will be happy to critique your thoughts.

The nature of bonding in MgF2 (s) and Zn(s) is different.

MgF2 (s) is an ionic compound, which means it consists of a metal (Mg) and a nonmetal (F). The bonding in MgF2 involves the transfer of electrons from Mg to F, resulting in the formation of Mg2+ cations and F- anions. These ions are held together by electrostatic attractions, creating an ionic lattice.

On the other hand, Zn(s) is a metallic element. In metallic bonding, the atoms of a metal element share their valence electrons in a "sea" of delocalized electrons. This creates a network of positive metal ions surrounded by a cloud of mobile electrons. The positive ions are attracted to this electron cloud, which holds them together.

Regarding the second question, the metallic substances are Co(s), Pb(s), and Xe(g).

Co(s) refers to solid cobalt, which is a metallic element. It has metallic bonding between cobalt atoms, where valence electrons are shared among the metal atoms.

Pb(s) stands for solid lead, which is also a metallic element. Similar to cobalt, solid lead exhibits metallic bonding.

Xe(g) refers to gaseous xenon, which is a noble gas. Noble gases do not typically form compounds, and xenon exists as individual atoms in its gaseous state. Therefore, it does not exhibit metallic bonding.

The remaining substances in the list are not metallic:
- F2(g) is a diatomic molecule consisting of two fluorine atoms bonded by a covalent bond.
- NaCl(s) represents solid sodium chloride, which is an ionic compound.
- H2O(s) refers to solid water, also known as ice, and it forms a lattice structure through hydrogen bonding.
- C6H6(l) is liquid benzene, which is a molecular compound held together by covalent bonds.

The nature of the bonding in MgF2(s) and Zn(s) differs in terms of the type of bonding and the arrangement of atoms.

In MgF2(s), the bonding is ionic in nature. This means that there is a transfer of electrons from magnesium to fluorine atoms, resulting in the formation of positively charged magnesium ions (Mg2+) and negatively charged fluoride ions (F-). These ions are then held together by strong electrostatic forces of attraction.

On the other hand, the bonding in Zn(s) is metallic in nature. Metallic bonding occurs when there is a "sea" of delocalized electrons in a lattice of positive metal ions. In the case of zinc, the outermost electrons of each zinc atom are loosely held, allowing them to move freely throughout the metal lattice. This results in a collection of positively charged zinc ions surrounded by a cloud of delocalized electrons, creating a strong metallic bond.

Among the given substances, the metallic compounds are Co(s) (cobalt) and Pb(s) (lead). These substances exhibit metallic bonding due to the presence of freely moving electrons within their structures.

F2(g) (fluorine gas), NaCl(s) (sodium chloride), H2O(s) (water as ice), C6H6(l) (benzene), and Xe(g) (xenon gas) do not exhibit metallic bonding. They have different types of bonding, such as covalent and ionic bonds, depending on the specific compound.