hjælp angiv rumlige opbygning af O atomet i molekylet?

The shape of hydrogen peroxide is bent with <109.5 bonding angles on both central atoms because of the number of electron groups on the oxygens which is 4 (2 bonds and 2 lone pairs)). The  ideal molecular shape but not the actual molecular shape.

Let's determine the molecular shape step-by-step:

1) the formula and the valence electrons of Hydrogen peroxide is H2O2.

Based on that, we count the number of valence electrons as 14 (2 from the hydrogens, 12 from the oxygens)

2)  the Lewis structur

First we make single bonds to connect the atoms. We know that hydrogen cannot be the central atoms, so we use oxygen as the central atoms.

H-O-O-H

Then we put lone pairs around the oxygens to complete the octet shells for the oxygens. The number of valence electrons and bonding electrons should equal 14.

3) Predict the ideal arrangement for central atoms.

Both oxygens have four electron groups, so its ideal electron arrangement would be AX4 and tetrahedral. However there are two lone pairs around each oxygen, and lone pairs will distort the bonding angles so we need to take that into account.

4) Predict the VSEPR shape.

Because of the lone pairs, the predicted electron arrangement is AX2E2 and the actual molecular shape is bent with < 109.5 bonding angle because of the lone pairs.