# group 1

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#1
why does the melting point of the group 1 metals decrease as you go down the group?

0
2 years ago
#2
As you move down the group the elements gain shells. This means the distance between the nucleus and the outer electrons (the ones moving to form ions) increases so the attraction between them decreases. Therefore, less energy is needed to break the attraction between them so the melting point decreases.
Hope this helps
0
2 years ago
#3
All elements in group 1 have the same number of valence electrons. However, down the group, the effective nuclear charge decreases.

Atomic radius increases down the group, due to the addition of shells and thus greater electron shielding = less electrostatic attraction between electrons and the nucleus. Atomic radius also increases as atomic number increases. Less energy is needed to remove an outer electron and thus make the group 1 element an ion.

For the highest element of group 1, lots of energy is needed to seperate the valence electron to make a +1 ion due to this greater electrostatic attraction between the electron and nucleus as a result of the smaller atomic radius and smaller nucleus.
0
2 years ago
#4
The exact wording of the answer will probably depend on the spec you're studying. I'd go with: the melting point of G1 metals is determined by the strength of the metallic bonds which (without going into band theory) is all to do with the attraction between the metal ions and the delocalised e- cloud. The radius (i.e. # of shells) of the ion most affects the strength of the attraction - the larger the radius, the weaker the attraction and hence the less energy needed to overcome the attraction.
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