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Arsenic should have 5 electron dots in its Lewis structure, one for each valence electron.
In a Lewis dot diagram, phosphorus has five valence electrons, which are represented as dots around the element symbol (P). Therefore, five dots are drawn for phosphorus to illustrate its valence electrons. These dots can be arranged in pairs and single electrons to show potential bonding configurations.
In a Lewis dot structure for an oxygen atom, there should be six dots. Lone pairs of electrons are represented by dots around the symbol for the atom. Oxygen has six valence electrons, so it will have a total of six dots in its Lewis dot structure.
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Arsenic should have 5 electron dots in its Lewis structure, one for each valence electron.
For fluorine: 8 dots.
A Lewis dot structure for potassium (K) would have one dot, representing its single valence electron.
Iodine has 7 dots around it in its Lewis dot structure as it has 7 valence electrons.
The amount of dots in total in the Lewis Dot Diagram of AsF4+ (Arsenic tetrafloride) is twenty six. Each "F" (fluorine atom) has six dots in total, two on three "sides". The As (arsenic atom) in the middle of the structure has two dots adjacent to it. Each dot resembles the amount of electrons available in the very outer shell of the atoms structure, known as valance electrons.
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An atom of potassium should have one dot in its Lewis-dot structure. This dot represents the single valence electron in the outer shell of the potassium atom.