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The group 7 halogens require to gain or share the least electrons to form an ion or molecule in which the halogen atom has a very stable noble gas electron arrangement. This requires the least energy, so the group 7 halogens tend to be the most reactive non-metals on the right-hand side of the periodic table.

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Electron-pair geometry maximizes the distance between every pair of electrons around a central atom. For example, if there are three pairs of electrons, increasing the angle between two electron pairs in a trigonal planar arrangement would push one of the pairs closer to the third pair, which would increase the potential energy of the third pair.

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Silicon has 14 electrons and so has an electron arrangement of 2, 8, 4. Making A Diagram: Once we know the numbers of electrons in each layer, all we need do is draw them onto a basic picture of an atom like that at the start of the page. I will use Silicon as the example in the following steps.

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Determine the electron group arrangement around the central atom that minimizes repulsions. Assign an AXmEn designation; then identify the LP-LP, LP-BP, or BP-BP interactions and predict deviations from ideal bond angles. Describe the molecular geometry.

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An ion is an atom or group of atoms which carries a charge. To form a negative ion, an atom would have to gain an extra electron (or more than one electron). For example, chlorine has an atomic number of 17, and the neutral atom must have 17 electrons.

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By examining an element's position on the periodic table, one can infer the electron configuration. Elements that lie in the same column on the periodic table (called a "group") have identical valance electron configurations and consequently behave in a similar fashion chemically. For instance, all the group 18 elements are inert gases. Step 2. Assign one of the five electron-group arrangements by counting all electron groups (bonding plus nonbonding) around the central atom. Step 3. Predict the ideal bond angle from the electron-group arrangement and the effect of any deviation caused by lone pairs or double bonds. Step 4.

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