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The Lewis structure for SeO3-2 is shown below:
O
/ \
Se O
\ /
O
Using VSEPR theory, we can predict the geometry of the SeO3-2 ion to be trigonal planar.
To draw the Lewis structure for the SeO3-2 ion, we first need to determine the total number of valence electrons in the ion. The Se atom has 6 valence electrons and each O atom has 6 valence electrons, for a total of 24 valence electrons.
Next, we need to connect the atoms using single bonds. The Se atom forms three bonds with the O atoms, so we can place the O atoms at the corners of a triangle, with the Se atom at the center. This arrangement satisfies the octet rule for each atom, because each O atom has a full valence shell of eight electrons and the Se atom has an expanded valence shell of eight electrons as well.
Using VSEPR theory, we can predict the geometry of the SeO3-2 ion to be trigonal planar. In this geometry, the three O atoms are arranged in a plane around the central Se atom. The electronic structure of the ion can be described as follows: the central Se atom has a total of six valence electrons, and each of the three O atoms has a total of seven valence electrons. This results in a total of 25 valence electrons in the ion, giving it a -1 charge.
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