properties of metals

[captain_kirk]

okay, so we have to investigate the properties of metal for our next sac.
we have been given the rubric and are being graded on the prac report relating to the experiment.
we are finding out the melting point, electrical conductivity, density, magnetism etc.
the rubric says, to get top marks, we need to make multiple links between what has been investigated about metals and other aspects of chemistry and many links have been made between the properties of metals and their uses in society.
does anyone know what it means by this?
i get the second part kinda, in terms of linking the metals to society, but what is meant by linking the properties of the metals to other aspects of chemistry?

[the.watchman]

Maybe they mean that you need to be able to explain, chemically, why the metal would have those properties?
I'm not too sure though

[Edmund]

You need to understand the different structures metal could have. E.g. Metal lattice or whether the structure has delocalised electrons, if it does, what would this say about electrical conductivity? Also, what bonds are there and how will this affect the melting point?

[the.watchman]

You need to understand the different structures metal could have. E.g. Metal lattice or whether the structure has delocalised electrons, if it does, what would this say about electrical conductivity? Also, what bonds are there and how will this affect the melting point?

Yep, that's what I meant

[kyzoo]

0.o is metal bonding even a significant part of the 3/4 course?

[superflya]

0.o is metal bonding even a significant part of the 3/4 course?

no, id say captain kirks doing 1&2.

[captain_kirk]

so basically, if it is a good electrical conductor, i would say if one of there was a poor electrical conductor, that this was due to the fact that ionic compounds are very poor conductors in the solid state as in the solid lattic there are no free moving charge particles, and ifi were to melt this ionic compound the charged particles would no longer be held in fixed positions, meaning that this would allow them to be able to conduct electricity.
and if it were a good electrical conductor i would say that this is due to the fact that they have metal lattices, meaning that the delocalised electrons are free to move throughout the lattice and can easily transprt charge.

so does this also mean i would say, because we have to note the appearance, if the metal appeared lustrous, i would sauy that it is due to the fact that light is reflecting off of the delocalised electrons?
is that the direction i meed to go, the same with melting point and boiling point and density?
and question how does the structure impact magnetism?

[Edmund]

You are on the right track here. You could start by listing out the different structures:

- Metallic
- Ionic
- Molecular
- Covalent Network E.g. Silicon dioxide
- Covalent Lattice E.g. Graphite

You can then go on to describe their structures, you would be able to find lots of stuff in your book.

By understanding the structure, you should then explain properties such as solubility, electrical conductivity and melting point

Here's an example for Metallic structure:

Structure: Metal lattice

Solubility:
In metallic substances, there is a strong bond between them, known as the metallic bond. There are delocalised electrons which hold the cations together. Unlike the hydrogen bonds in some molecular solids, they cannot be broken. Since they cannot be broken, they therefore cannot be dissolved.

Conductivity:
In solid metallic substances, electricity could be conducted. In solid metallic substances, there are delocalised electrons which hold the cations together. These free moving delocalised electrons are able to conduct a current therefore metallic solids are good conductors of electricity.

Melting Point:
High. Its structure is made up of cations and delocalised electrons. There is a metallic bond between the particles. Melting point is usually high in metallic lattices due to the large amount of thermal energy which is needed to overcome the strong forces that operate throughout the structure.

This is just an example, you would look up the rest of the structures and deduce the rest of the information

[captain_kirk]

so would this be correct for ionic compounds:
solubility:?

electrical conductivity:Due to the fact that there are no free moving charged particles in the solid lattic, ionic compounds are very poor conductors in the solid state. On the other hand, when melted, the charge particles are no longer held in fixed positions and are therefore able to conduct electricity. When an ionic compound is dissolved in water the are also able to conduct electricity as the ions dissociate.

melting point:very high.  due to the strong attraction between the oppositely chraged ions (strong electrostatic bond between particles) it requires a large amount of energy to break bonds apart. This means that if we heat up the compound to add energy it would take a huge amount of energy to break it apart.
boiling point [see melting point]

and do all metals have a metal lattice structure?
and does this structure influence magnatism?

[Edmund]

electrical conductivity:Due to the fact that there are no free moving charged particles in the solid lattic, ionic compounds are very poor conductors in the solid state. On the other hand, when melted, the charge particles are no longer held in fixed positions and are therefore able to conduct electricity. When an ionic compound is dissolved in water the are also able to conduct electricity as the ions dissociate.

That's correct. In ionic compounds, think of it as being made up of ions - positive and negative ions (E.g. NaCl). These ions are held together by ionic bonds. Ions are fixed, and no delocalised electrons. But as you said, it's  different in aqueous since there are no longer in fixed positions. The ionic bonds have been broken by water.

melting point:very high.  due to the strong attraction between the oppositely chraged ions (strong electrostatic bond between particles) it requires a large amount of energy to break bonds apart. This means that if we heat up the compound to add energy it would take a huge amount of energy to break it apart.

Also correct, similar to metallic lattice, but ionic has higher melting point.

About the lattice, a lattice means some sort of ordered structure, which is different for all metals.

About magnetism, the metal having different charges would influence magnetism. (E.g. NaCl) - not entirely sure.

[captain_kirk]

is an ionic structure only present in compounds?
and for pure elements
Copper, Iron, Lead, Zinc, Sodium, Nickel, Lithium, Calcium, Aluminium, Magnesium
do they all have similar structures? a metallic lattice? or do they vary from element to element? does it also have to do with the valence electrons i.e sodium is more reactive than zinc etc.

[Edmund]

is an ionic structure only present in compounds?
and for pure elements
Copper, Iron, Lead, Zinc, Sodium, Nickel, Lithium, Calcium, Aluminium, Magnesium
do they all have similar structures? a metallic lattice? or do they vary from element to element? does it also have to do with the valence electrons i.e sodium is more reactive than zinc etc.

Ionic compounds = Ionic structure = NaCl etc, basically metal and non-metal

Copper, Iron, Lead, Zinc, Sodium, Nickel, Lithium, Calcium, Aluminium, Magnesium are all metallic structures with metallic lattice (these are just the metals on your periodic table)

does it also have to do with the valence electrons i.e sodium is more reactive than zinc etc.

Nah

[captain_kirk]

okay, thanks heaps, cause we are only using pure metals for this experiment, so i should only have to explain the relationship between the metallic lattice and the effect on their properties   

[captain_kirk]

one more thing, it says the properties of the metals and their links to society... does that mean i have to talk about how their high melting points etc. aid their uses? etc

[Edmund]

one more thing, it says the properties of the metals and their links to society... does that mean i have to talk about how their high melting points etc. aid their uses? etc

Well yeah, wouldn't be too hard to come up with a few