However, when you put the diagrams side by side, then the fluorine molecule should be smaller than the chlorine molecule. Well, when you draw them separately, the dot- and- cross diagrams of the two look similar.
Since we are showing only the outermost electrons, you may be wondering if the dot- and- cross diagram of both fluorine and chlorine are the same. This means that one fluorine atom will share 1 electron with another fluorine atom and both will achieve stable octet configuration. Let chlorine, fluorine has 7 valence electrons (as it is in Group VII), it needs just 1 more electron to achieve stable octet configuration. It will achieve stable octet configuration in fluorine molecule. Dot- and- cross diagram of covalent molecule (fluorine) F 2įluorine is in the second period of the periodic table, and is the first element in Group VII. This means that one chlorine atom will share 1 electron with another chlorine atom and both will achieve stable octet configuration. Since chlorine has 7 valence electrons (as it is in Group VII), it needs just 1 more electron to achieve stable octet configuration. Hence, we’ll look at having 8 valence electrons for chlorine. Unlike hydrogen, it will tend to achieve stable octet configuration. Dot- and- cross diagram of covalent molecule (chlorine) Cl 2Ĭhlorine is in the third period of the periodic table. In the molecule of hydrogen, each hydrogen atom donates one electron to the covalent bonding, and both hydrogen atoms will have the stable duplet configuration. Instead of achieving stable octet configuration, hydrogen achieves stable duplet configuration. This means that it can only hold a maximum of 2 electrons. Hydrogen is in the first period of the periodic table. Drawing dot- and- cross diagrams of Diatomic moleculesĭrawing dot- and- cross diagrams of Polyatomic moleculesĭiatomic Molecules Dot- and- cross diagram of covalent molecule (hydrogen) H 2 In all the examples below, only the outermost electrons are shown.Ĭlick on the link below to go directly to the molecule.
Polyatomic molecules – such molecules are formed from more than 2 atoms.Diatomic molecules – such molecules are formed from 2 atoms covalently bonded to each other.I have divided the examples into two groups:
#Simple diagrams of atoms how to
Let’s look at how to illustrate the covalent bonds using dot- and- cross diagrams. As covalent bonds are formed by sharing of electrons between atoms, we draw overlapping circles to show the overlapping of the electron shells, and draw in pairs of dots and crosses to show the sharing of electrons. In these diagrams, we use circles to represent the electron shells. A method to represent the covalent bonds in a diagram is by drawing dot- and- cross diagrams. Now that we know that non- metals and non- metals form covalent bonds, let’s look at how are these covalent bonds represented. Drawing covalent bonding in molecules using dot- and- cross diagrams In short, non- metals and non- metals form covalent bonds with one another as it’s easier for them to achieve stable electronic configuration this way. That’s why, non- metals and non- metals form covalent compounds.
If you have 2 atoms that want to gain electrons in order to achieve the stable octet configuration, then it will be easier for the atoms to share and achieve 8 than to lose or gain electrons. In these groups, it is easier to gain stable electronic configuration by sharing electrons, or gaining electrons, rather than losing them. Think of it as when you have non-metals and non-metals, which are usually in Groups IV – VII. In O Level Chemistry, students learn that generally, non- metals and non- metals share pair(s) of electrons to form covalent bond(s). Why do non- metals form covalent compounds In this post, let’s talk about drawing dot- and- cross diagrams of covalent molecules.Ī covalent bond is a chemical bond formed by sharing of electron pairs between atoms.
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