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Ionic and Covalent Bonds Chemistry Ms. Piela

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Presentation on theme: "Ionic and Covalent Bonds Chemistry Ms. Piela"— Presentation transcript:

1 Ionic and Covalent Bonds Chemistry Ms. Piela
The Chemical Bond Ionic and Covalent Bonds Chemistry Ms. Piela

2 Ionic Compounds Overview
Bonds formed between a metal and a nonmetal Metals form positive ions called cations Trick to remember: “ca+ion” Non-metals form negative ions called anions Ionic bonds are formed by a transfer of electrons

3 Properties of Ionic Compounds
Ionic compounds dissociate (or break apart) in liquids Example: Table salt in water Ionic compounds can conduct electricity If something conducts electricity, then ions/charges must be able to move Solid ionic compounds are rigid, not allowing charges to move Two conditions allow ionic compounds to conduct electricity: Molten (or liquid) Dissolved in solution Example: Li-ion batteries

4 Properties of Ionic Compounds
Ionic compounds tend to have high melting points This is due to the high strength of the ionic bonds Stronger bonds need more energy to break apart!

5 Formation of Ionic Compounds
Ionic bonds follow the Octet Rule Octet rule – Each element tends to form compounds based on the easiest way to gain 8 valence electrons Example: Na and Cl Sometimes combinations are not an easy one-to-one ratio! Example: Ca and Cl

6 Formation of Ionic Compounds
Examples Mg and O K and S Practice Ba and N Li and P

7 Formation of Ionic Compounds
Transition metal ionic compounds All form positive ions (cations), but can form multiple ions Example: FeCl2 and FeCl3

8 Covalent Compounds Overview
Covalent bonds are made between nonmetals only Does NOT depend on charges!! Covalent bonds will share electrons as both elements need to gain electrons to obtain full outer shell (8 valence electrons)

9 Properties of Covalent Compounds
Forms longer bonds because bonds are weaker than ionic bonds Energy is lowered when atoms form a covalent bond This is the main driving force behind their formation There is a balance between their attractive and repulsive forces

10 Two Types of Covalent Bonds
Polar covalent bonds are covalent bonds where electrons are shared unequally between the atoms Non-polar covalent bonds are covalent bonds where electrons are shared equally between the atoms

11 Polarity Polarity depends on differences in electronegativity
The greater the difference in electronegativity, the more polar the bond is Example: Cl2 and HF The more polar the bond, the stronger the bond Polar covalent bonds have stronger bonds than non-polar bonds Stronger bonds give higher boiling points (just like ionic compounds)

12 The Chemical Bond Overview
Nonpolar Covalent Polar Covalent Ionic In order of increasing bond strength: In order of increasing bond length: Ionic Polar Covalent Nonpolar Covalent

13 Naming Ionic Compounds
Simple Naming Rules Identify the compound as Ionic (Metal and a non-metal) Determine charges for each ion Overall charge of compound must be zero General formula for names: Cation + Anion Root-ide

14 Examples Calcium fluoride Calcium phosphide Magnesium nitride
Potassium oxide

15 Examples LiCl2 SrBr2 BaI2

16 Transition Metal Compounds
Since transition metals form multiple ions, roman numerals denote charge Roman numerals are not the number of molecules!

17 Examples iron (III) chloride copper (II) oxide iron (III) oxide
silver (I) sulfide

18 Polyatomic Ion Compounds
Some elements are considered as a charged group of two or more atoms. They are considered as a single ion called a polyatomic ion. You will not need to memorize these, only recognize it when you see them

19 Examples Aluminum chromate Potassium hydroxide Sodium thiosulfate
Calcium acetate

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