Lewis Dot Structures Tutorial

<p>$ns^2np^6$</p> Signup and view all the answers

<p>Due to electrostatic attraction</p> Signup and view all the answers

<p>Valence electrons = Number of electrons in the outermost shell of an atom Group valence = Number of dots in Lewis symbols or 8 minus the number of valence electrons Electronegative = Tendency to attract electrons in a chemical bond Electropositive = Tendency to donate electrons in a chemical bond</p> Signup and view all the answers

<p>Separation of halogens and alkali metals by noble gases = To stabilize negative and positive ions formed by electron transfer Stable noble gas electronic configurations = Outer shell configuration of eight electrons for stability Formation of negative ions from halogens = Associated with gain of an electron by halogen atoms Formation of positive ions from alkali metals = Associated with loss of an electron by alkali metal atoms</p> Signup and view all the answers

<p>Octet rule = Atoms tend to lose, gain, or share electrons to achieve a full outer shell of 8 electrons Duplet of electrons = Helium's stable configuration with 2 electrons in its outer shell Stabilization of ions by electrostatic attraction = Achieved by the opposite charges between positive and negative ions Lewis symbols = Representations of atoms showing their valence electrons as dots around the symbol</p> Signup and view all the answers

<p>Lewis dot structure = Helps in understanding how atoms form covalent bonds by sharing electrons Coordination compounds = Complexes where metal ions are surrounded by ligands through coordinate bonds Electrostatic attraction = Force that stabilizes ionic compounds through attraction between opposite charges Kössel's observations = Highlight the stability achieved when atoms attain noble gas electronic configurations</p> Signup and view all the answers