What is a consequence of electron-pair repulsion around an atom?

A. The atoms sharing the electron pairs will be lost as ions.

B. The atoms sharing the electron pairs will be pushed together.

c. The atoms sharing the electron pairs will spread out around the

central atom

D. The atoms sharing the electron pairs will form attractions with

other atoms.

Option C is correct.

The atoms sharing the electron pairs will spread out around the central atom.

Explanation:

In covalent bonding, the atoms involved form a bond by sharing a pair of electrons. These pairs of electrons are repulsive towards one another, when they occur together around a central atom.

Infact, the Valence shell electron pair repulsion (VSEPR) theory explains further that 'electron pairs around a central atom arrange themselves so that they can be as far apart as possible from each other'.

So, it becomes obvious that the atoms that share these electron pairs around a central atom are pushed to spread out as far as possible around that central atom.

Hope this Helps!!!

c. The atoms sharing the electron pairs will spread out around the

central atom

Explanation:

If an atom is bonded to two or more kinds of atoms for example many covalent molecule or ions, the shape of the system is determined by the geometry of the bonds around the central atom. The variations in the bond angle of such molecules and ions can be explained by the Valence shell electron pair repulsion theory.

The  Valence shell electron pair repulsion theory (VSEPR) model determines the total number of electron pairs surrounding the central atom of a species. The total number of electron pairs consists of lone pair and bond pairs. All the electron pairs will orient themselves in such a way as to minimize the electrostatic repulsion between them.

answer: a tank of height h is filled with water and sits on the ground. water squirts from a hole at a height y above the ground and has a range r. for two y values, 0 and h, r is zero. determine the value of y for which the range will be a maximum.

explanation: