Select all the atoms that have at least one lone (unshared) pair of electrons. • Gray = C; white H; red= 0; blue = N; dark green= Cl; brown Br; light green F; purple = 1; yellow S; orange – P • Double click to select atoms. You can zoom in and out using the mouse scroll wheel (or pinch to zoom on touch screens). Convert the model below to a skeletal drawing. wireframe H H H HH H H + labels H H None Select all the atoms that have at least one lone (unshared) pair of electrons. • Gray = C; white H; red= 0; blue = N; dark green= Cl; brown Br; light green F; purple = 1; yellow=S; orange – P Double click to select atoms. You can zoom in and out using the mouse scroll wheel (or pinch to zoom on touch screens). Convert the model below to a skeletal drawing. wireframe H H H C H H + labels H
The Correct Answer and Explanation is :
In the provided molecular model, the atoms with at least one lone (unshared) pair of electrons are:
- Oxygen (O): Oxygen typically has two lone pairs of electrons in its valence shell.
- Nitrogen (N): Nitrogen usually has one lone pair of electrons in its valence shell.
- Chlorine (Cl): Chlorine generally has three lone pairs of electrons in its valence shell.
- Bromine (Br): Bromine also typically has three lone pairs of electrons in its valence shell.
- Fluorine (F): Fluorine has three lone pairs of electrons in its valence shell.
- Sulfur (S): Sulfur can have two lone pairs of electrons in its valence shell.
- Phosphorus (P): Phosphorus can have one lone pair of electrons in its valence shell.
These lone pairs are non-bonding electron pairs localized on the respective atoms and are not involved in bonding with other atoms.
In contrast, carbon (C) and hydrogen (H) atoms do not have lone pairs of electrons. Carbon typically forms four bonds to achieve a stable electron configuration, and hydrogen forms one bond. Both elements have their valence electrons involved in bonding rather than existing as lone pairs.
Understanding the presence of lone pairs is crucial for predicting the geometry and reactivity of molecules. Lone pairs occupy space around an atom and can influence the shape of the molecule by repelling bonding pairs of electrons, leading to deviations from ideal bond angles. For example, in water (H₂O), the oxygen atom has two lone pairs, which repel the bonding pairs, resulting in a bent molecular geometry. Similarly, in ammonia (NH₃), the nitrogen atom has one lone pair, leading to a trigonal pyramidal shape.
For a more detailed explanation on determining the number of lone pairs, you might find the following video helpful:
videoHow To Calculate The Number of Lone Pairs Using a Formulaturn0search5