the models you have built and sketched do not take into account the fact that bonding and bnonbonding pairsof electrons do not repel each other to exactly the samwe extent; repulsion by nonbonding pairs is pstronger than by bonding pairs. how will this affect the true geometric shape of the molecules you have drawn

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Explanation:

According to the valence shell electron pair repulsion theory, the number of electron pairs on the valence shell of the central atom in a molecule determines the shape of the molecule.

We know that electron pairs repel each other. The magnitude of electron repulsion causes the electron pairs to be positioned as far apart in space as possible.

Lone pairs cause greater repulsion than bond pairs. As a result, lone pairs tend to distort the molecule. This will decrease the expected bond angles and ultimately alter the molecular geometry of the molecule.

The repulsion between electrons greatly affected the true geometric shape of the molecules.

This is because of the same charge they repel each other and change the angle between molecules and change the geometric shape. The electron pairs on the valence shell of the central atom in a molecule determines the shape of the molecule. The magnitude of electron repulsion causes the electron pairs to be positioned as far apart in space as possible.  

Lone pairs produces greater repulsion than bond pairs. As a result, lone pairs distort the molecule which will decrease the expected bond angles and ultimately change the molecular geometry of the molecule so we can conclude that repulsion between electrons greatly affected the true geometric shape of the molecules.

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so what is the problem with your lab report and whats the subject of the lab report? i will you

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.