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KCL: Ionic Bonds

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KCL is an ionic bond. This is because potassium (K) has a charge of +1 and chorine having a charge of
-1. K gives one electron to chlorine, this makes it so both of them have a full valence shell. GeCl4 is a covalent bond, due to it being hard to separate its 4 valence electrons so Germanium shares its 4 valance electrons to Chlorine therefore making 5 full outer valence shells. BrCl is a covalent bond.
Chlorine has a high electronegativity then bromine, and is a dipole-dipole which indicates to why it has a low melting point. Lastly CrCl3 is an ionic bond.
Elements have melting points and how metallic an element is determines the melting point. When the element is metallic the melting point is very high and when it becomes more gaseous the …show more content…

KCl and CrCl3 has a high melting point because the bond is strong and requires a lot of energy to break. Covalent bonds such as GeCl4 and BrCl have very low melting points due to the opposite reasons, it has a very weak structure and requires less energy to break the bond. This is represented on the table with KCl having a melting point of 770*C then CrCl3 with
1150*C Then GeCl4 with -50*C and BrCl with -66*C respectively.
Ionization energy (IE) increases from the bottom left side to the top right side of the periodic table, due to the stability of the elements and how far away the electrons are from the nucleus which determines how easily it can be transferred or taken away. Potassium has a low IE because its final shell has 1 valence electron, meaning it requires very little energy to remove that electron.
Chromium, Germanium and Bromine all have increases of ionization energy respectively making it harder and requiring more energy to remove an electron from the outer shell. Therefore also making the atom stability

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