![Objective 1:Relate the electron configuration of an atom to its chemical reactivity.Chemical ReactivityDepends on achievement of octet rules2p6 electron configuration - eight valence electrons[O] s2p4 Needs 2 electrons[Ne] s2p6 Needs 0 electrons – stableMost Reactive:Alkali Metals [Na] s1 Needs to lose 1 electronHalogen [Cl] s2p5 Needs 1 electron](https://image.slidesharecdn.com/chapter5-1applied-100331135621-phpapp02/85/Applied-Chapter-5-1-Simple-Ions-2-320.jpg)
![Objective 2Determine an atom’s number of valence electrons, and use the octet rule to predict what stable ions the atom is likely to form.Valence ElectronsUse periodic table – electron configurationEx: [Mg] s22 valence electrons [P] s2p35 valence electronIon – atoms that has gained or lost one or more electrons and has a positive or negative charge](https://image.slidesharecdn.com/chapter5-1applied-100331135621-phpapp02/85/Applied-Chapter-5-1-Simple-Ions-3-320.jpg)
![Forming a Cation – positive charge[K] s1 will lose 1 electron Creating +1 ionSo K+ is formed. Called a potassium ionSTABLEForming an Anion – Negative charge[S] s2p4 will gain 2 electrons Creating -2 ionSo S-2 is formed. Called a sulfur ionSTABLEBoth Now have s2p6 configuration](https://image.slidesharecdn.com/chapter5-1applied-100331135621-phpapp02/85/Applied-Chapter-5-1-Simple-Ions-4-320.jpg)
Applied Chapter 5.1 : Simple Ions
- 1. Chapter 5.1Ions and Ionic Compounds
- 2. Objective 1:Relate the electron configuration of an atom to its chemical reactivity.Chemical ReactivityDepends on achievement of octet rules2p6 electron configuration - eight valence electrons[O] s2p4 Needs 2 electrons[Ne] s2p6 Needs 0 electrons – stableMost Reactive:Alkali Metals [Na] s1 Needs to lose 1 electronHalogen [Cl] s2p5 Needs 1 electron
- 3. Objective 2Determine an atom’s number of valence electrons, and use the octet rule to predict what stable ions the atom is likely to form.Valence ElectronsUse periodic table – electron configurationEx: [Mg] s22 valence electrons [P] s2p35 valence electronIon – atoms that has gained or lost one or more electrons and has a positive or negative charge
- 4. Forming a Cation – positive charge[K] s1 will lose 1 electron Creating +1 ionSo K+ is formed. Called a potassium ionSTABLEForming an Anion – Negative charge[S] s2p4 will gain 2 electrons Creating -2 ionSo S-2 is formed. Called a sulfur ionSTABLEBoth Now have s2p6 configuration
- 5. Periodic table – predict ions+1-1-3+2+3D- block-2Charges VaryDon’t form ions
- 6. Objective 3Explain why the properties of ions differ from those of parent atoms.Ions formed have completely different properties than parent atoms.Sodium atom Chlorine atom sodium chloride Na Cl Na+ Cl-Loses one electronProperties:Very reactivemetalgains one electronProperties:Very reactivenonmetalGas at room tempAfter ions are formedProperties:StableGood on French fries
- 7. What they look like!