trends in pt

• Atomic radius is the size of atoms, not including transition metals.
• As you go down a group in the periodic table, the atoms get bigger due to more shells.
• The melting point of a group decreases as you go down the group because the atoms are bigger, reducing the electrostatic attraction between the nuclei and the free electrons.
• The distance between electrons and the nucleus is smallest when the electrons are between the nucleus and the electrons.
• Group two metals have a higher melting point than group one because there are more free electrons and more delocalized electrons.
• If the difference in electronegativity is greater than two, one of the atoms will get all of the electrons all the time, resulting in an ionic bond.
• Electronegativity does not apply to inert gases such as the noble gases because they do not form bonds.
• Going left to right across a period in the periodic table, the atoms get smaller due to more protons.
• Electronegativity is how attractive an atom is in a compound, with two electrons.
• Fluorine is the most attractive atom in a compound due to its high electronegativity.
• The pattern of electronegativity follows the same trend as atomic radius, with the smallest atom being the most attractive.