Fluorine Lewis symbol

We can extend the Lewis symbols introduced in Section 2.2 to describe covalent bonding by using a line (—) to represent a shared pair of electrons. For example, the hydrogen molecule formed when two H- atoms share an electron pair (H=H) is represented by the symbol H—H. A fluorine atom has seven valence electrons and needs one more to complete its octet. It can achieve an octet by accepting a share in an electron supplied by another atom, such as another fluorine atom ... 

Bond structure can also be represented by lines. Each electron pair is shown by a line. In other words two electrons are shown by a line So the line representation of the fluorine molecule is IF—FI. The line between the two fluorine atoms represents the bond. Sometimes both the Lewis symbol and line representation can be used in the same molecule. For example, the F2 molecule can also be represented as F— F ... 

Using Lewis symbols, write a balanced chemical equation showing the formation of lithium fluoride, LiF, from isolated lithium and fluorine atoms. 

Magnesium reacts with fluorine to form magnesium fluoride. Write an equation to describe the bonding using Lewis symbols. 

Given the Lewis symbols for nitrogen and fluorine in Table 8.1, predict the formula of the stable binary compound (a compound composed of two elements) formed when nitrogen reacts with fluorine and draw its Lewis structure. 

Analyze The Lewis symbols for nitrogen and fluorine reveal that nitrogen has five valence elections and fluorine has seven. 

The Lewis symbols for the atoms are F and Mg- (see Table 9.1). The magnesium atom loses two electrons to assume a noble-gas configuration. But because a fluorine atom can accept only one electron to fill its valence shell, two fluorine atoms must take part in the electron transfer. We can represent this electron transfer as follows ... 

Draw the Lewis dot symbol for each of the following atoms, (a) boron, (b) fluorine, (c) selenium, (d) indium... 

Covalent bonding between many-electron atoms involves only the valence electrons. Consider the fluorine molecule, F2. The electron configuration of F is ls 2s 2p. The li electrons are low in energy and stay near the nucleus most of the time. For this reason, they do not participate in bond formation. Thus, each F atom has seven valence electrons (the 2s and 2p electrons), and there is only one unpaired electron on F. Using Lewis dot symbols, the formation of the F2 molecule can be represented as follows ... 

Use Lewis electron-dot symbols to represent the transfer of electrons from magnesium to fluorine atoms to form ions with noble-gas configurations. 

When used to show the bonding arrangement between atoms in a molecule, electron-dot symbols are commonly called Lewis diagrams, Lewis formulas, or Lewis structures. Notice that the unshared electron pairs of fluorine are shown for two of the Lewis diagrams for F2 and HF, but they are omitted in the F—F and H— F diagrams. Technically, they should always be shown, but they are frequently omitted when not absolutely needed. Unshared electron pairs are often called lone pairs. 

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