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Ions and Ionic Bonding

Ions and Ionic Bonding. What is an Ion?. ION : Is an atom that has a different number of protons and electrons. Due to this they have a +’ ve or –’ ve charge. Elements form ions to fill their valence electron shell . Metals form +’ ve charged ions.

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Ions and Ionic Bonding

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  1. Ions and Ionic Bonding

  2. What is an Ion? • ION: Is an atom that has a different number of protons and electrons. Due to this they have a +’ve or –’ve charge. • Elements form ions to fill their valence electron shell. • Metals form +’ve charged ions. • Non-metals form –’ve charged ions. • The groupnumber on the P.T. tells us the number of valence electrons.

  3. How Atoms Behave • Atoms are trying to make a full valence shell of electrons. • This can happen in two ways: • 1. They gain electrons to completely fill the partly full valence shell. OR • 2. They lose electrons which empties the outer shell so the one inside of it is full. • You must decide; will it do #1 or #2 but atoms always take the easiest way (less work).

  4. Let’s Look at an Example • Would oxygen gain or lose electrons to fill it’s outer shell? Why? e- e- • It would gain to form a negative ion with a charge of -2 (8P+ and 10e- = -2)

  5. How Do You Write an Ion? (Ion notation) • It contains the chemical symbol and the ions’ charge above it. • This shows that the oxygen atom has gained two electrons and is an ion. O2- e- e-

  6. A Positive Example! • In this case sodium (Na) a metal, donates gets rid of an electron in order to have a full valence shell. • We would write this as Na+

  7. Ionic Bonding  What is it? • An ionic bond occurs when a metal donates electrons to a non-metal so that each atom has a full valence shell. • In this case sodium has lost an electron to a chlorine atom.

  8. Getting Formulas of Ionic Compounds (The X-Over Rule) • Let’s look at Magnesium (Mg) bonding with Chlorine (Cl) • You must first determine the charge on each atom. (Will it gain or lose e-?) • Mg  Group #2, would it gain 6 e- or lose 2 e-? • It would lose 2 e- creating Mg2+ • Cl  Group #7, would it gain 1 e- or lose 7 e- • It would gain 1 e-  Cl-

  9. The X-Over Rule Mg2+ Cl- • We rewrite the chemical symbols, cross the charges over to determine the number of atoms of each element in the compound. MgCl2

  10. Naming Ionic Compounds • Here’s how: • The metal’s name stays the same as it appears on the P.T. • The non-metal’s ending changes to “ide” • E.G. for MgCl2 • It would be called Magnesium Chloride • What would LiF be called? • Lithium Fluoride

  11. Ionic Bonding with Polyatomic Molecules

  12. What’s a Polyatomic Ion? • A polyatomic ion is a molecule or group of atoms that have an overall charge. • They are located on the back of your P.T. • E.G.

  13. Getting the Formulas of Polyatomics • We again use the X-Over rule. • When writing the formula put the polyatomic ion in a bracket. • E.G. Magnesium is bonding with chlorate. Mg2+ (ClO3)- Mg(ClO3)2

  14. Naming Compounds With Polyatomic Ions • The name of the metaland polyatomic ionstays the same. • E.G. When magnesium bonds with chlorate Mg(ClO3)2 what will it be called? • A: Magnesium Chlorate

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