metallic bonds are not fully broken until the metal has first melted and then boiled. the boiling points of sodium, magnesium and aluminium are 890 c 1110 c and 2470 c respectively what does this suggest about the srengths of the metallic bonds in these three elements? please help...................................
The boiling points of sodium, magnesium, and aluminium can provide insights into the strengths of their metallic bonds.
To understand this, we need to consider that metallic bonds are formed between metal atoms, where the valence electrons are shared among all the atoms in a lattice structure. These shared electrons create a sea of delocalized electrons, giving metals their unique properties like malleability, ductility, and electrical conductivity.
The strength of metallic bonds depends on several factors, including the number of valence electrons and the size of the metal atoms. Generally, metals with more valence electrons or smaller atomic radii tend to have stronger metallic bonds.
Now let's analyze the given data:
1. Sodium (Boiling point: 890°C): Sodium has only one valence electron, and its atomic radius is relatively large compared to the other two elements. These factors suggest that sodium has relatively weaker metallic bonds compared to magnesium and aluminium.
2. Magnesium (Boiling point: 1110°C): Magnesium has two valence electrons, one more than sodium. Additionally, magnesium has a smaller atomic radius than sodium. These factors imply that the metallic bonds in magnesium are stronger than in sodium but weaker than in aluminium.
3. Aluminium (Boiling point: 2470°C): Aluminium has three valence electrons, more than sodium and magnesium. Furthermore, aluminium has a smaller atomic radius than both sodium and magnesium. These factors indicate that the metallic bonds in aluminium are the strongest among the three elements mentioned.
Therefore, based on the boiling points, we can infer that the strength of metallic bonds increases in the order: sodium < magnesium < aluminium.
The boiling points of sodium, magnesium, and aluminum indicate the strengths of the metallic bonds in these elements.
Sodium has a relatively low boiling point of 890°C. This suggests that the metallic bonds in sodium are relatively weak. The lower boiling point indicates that the metallic bonds are easier to break, and therefore the metal has a lower melting and boiling point.
Magnesium has a higher boiling point of 1110°C compared to sodium. This suggests that the metallic bonds in magnesium are stronger than in sodium but still not as strong as in aluminum. The higher boiling point implies that more energy is required to break the metallic bonds and cause the metal to melt and boil.
Aluminum has the highest boiling point of the three elements, at 2470°C. This suggests that the metallic bonds in aluminum are the strongest among the three. The higher boiling point implies that a significant amount of energy is needed to overcome the attractive forces between aluminum ions and to break the metallic bonds, leading to melting and boiling.
In summary, the boiling points of sodium, magnesium, and aluminum suggest that the metallic bonds in these elements become progressively stronger from sodium to magnesium to aluminum.