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The Lewis structure of H 2 O indicates that there are four regions of high electron density around the oxygen atom: two lone pairs and two chemical bonds: We predict that these four regions are arranged in a tetrahedral fashion (Figure \(\PageIndex{6}\)), as indicated in Figure \(\PageIndex{9}\).
- Molecular Shape
A molecule with the formula AB 3, in which A and B represent...
- Problems
When two electrons are removed from the valence shell, the...
- Molecular Shape
We continue our discussion of structure and bonding by introducing the valence-shell electron-pair repulsion (VSEPR) model (pronounced “vesper”), which can be used to predict the shapes of many molecules and polyatomic ions.
VALENCE-SHELL ELECTRON-PAIR REPULSION (VSEPR) MODEL. Lewis structures show the two-dimensional distribution of atoms and electrons. The molecular geometry, or three-dimensional shape of a molecule or polyatomic ion, can be determined using valence-shell electron-pair repulsion (abbreviated VSEPR and pronounced “VES-per”) theory, in which ...
2 gru 2019 · 2.24 Shapes of Molecules. The shape of simple covalent molecules is determined by the number of bonding pairs of electrons and the number of lone pair of electrons. In determining shape the electron pairs repel away from each other, and will move as far away as possible. There are five basic shapes and then variations on each shape where lone ...
Oxygen, for example, has the electron configuration 1s22s22p4, whereas the oxygen anion has the electron configuration of the noble gas neon (Ne), 1s22s22p6. The two additional electrons required to fill the valence orbitals give the oxide ion the charge of 2– (O2–). Example 7.2.
Carbon (4 electrons in the valence shell) combines with four hydrogen atoms to form a stable covalent compound where it shares 8 electrons, while each hydrogen shares 2. Thus every atom in this stable molecule fulfills the octet rule. ELECTRON SHARING IN THE METHANE (CH4) MOLECULE.
To determine the hybridisation of an atom: Determine the number and type of atomic orbitals used by the atom; include all the electrons in the valence shell. For example, boron, with three valence electrons, uses one s and two p orbitals; nitrogen, with five valence electrons, uses one s and three p orbitals.
