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Ion formation

1) Chemical bonding involves the transfer or sharing of valence electrons between atoms. Valence electrons are in the outermost energy level and determine an element's chemical properties. 2) Atoms bond in order to achieve a noble gas electron configuration of 8 valence electrons, following the octet rule. Metals lose electrons to form cations, while nonmetals gain electrons to form anions. 3) Cations are positively charged ions formed when metals lose electrons. Group 1 cations have a +1 charge and Group 2 cations have a +2 charge. Transition metal cations can have varying charges. Anions are negatively charged ions formed when nonmetals gain electrons, taking on charges of -1.

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Chemical BondingIons
Valence ElectronsElectrons in the highest occupied energy level of an element’s atomsNumber of valence electrons determines the chemical properties of the elementNumber of valence electronsRepresentative elementsLast number in the group numberHelium has 2 valence electrons because it only has 1 energy level (other noble gases have 8)Electron dot diagramsDiagrams that show valence electrons as dots (see Table 7.1, page 188)
Octet RuleIn forming compounds, atoms tend to achieve the electron configuration of a noble gas.Octet – a set of 8 valence electronsAtoms of metals tend to lose all of their valence electrons leaving a complete octet in the next-lower energy level.Atoms of nonmetals tend to gain electrons or share electrons with another nonmetal to achieve an octet.
Formation of CationsCations are formed when metal atoms lose electrons.Cation – positive ion whose charge is equal to the number of electrons lostName of the cation is the same as the element’s nameSodium atoms(Na) become sodium ions(Na+) when they lose their 1 valence electron.
Cations of Group 1 elements always have a 1+ charge.
Cations of Group 2 elements always have a 2+ charge.
Cations of transition metals (groups 3 – 12) vary in charge.
Cations with charges of 3 or higher are uncommon.
aluminum cations always have a charge of 3+. Pseudo-noble gas configurationFormed by some transition metalsCharacterized by filled s, p, and d sublevels in the highest occupied energy levelExampleWhen Ag loses the 5s1 electron, its next lower energy level is 4s24p64d10