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Chapter 6: Inorganic and Organic Compounds 6.5 Chem 1110 Figures: Basic Chemistry 3 rd Ed., Timberlake and Timberlake.

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Presentation on theme: "Chapter 6: Inorganic and Organic Compounds 6.5 Chem 1110 Figures: Basic Chemistry 3 rd Ed., Timberlake and Timberlake."— Presentation transcript:

1 Chapter 6: Inorganic and Organic Compounds 6.5 Chem 1110 Figures: Basic Chemistry 3 rd Ed., Timberlake and Timberlake

2 Ionic vs. Covalent Bonding Ionic Bonding Covalent Bonding Metal - nonmetal (NaCl) Electron transfer and electrostatic interactions Formula Unit (from larger arrays) Solids Dissolve in water and conduct electricity Two nonmetals (O 2, H 2 O) Electron sharing in bonds Discrete molecules All physical states (solid, liquid and gas) If they dissolve in water, they do not conduct electricity

3 The Covalent Bond Covalent Bonding: a chemical bond that results from two nuclei attracting the same shared electron pair

4 Forming a H 2 Molecule A covalent bond forms as two H atoms move close together to share electrons

5 Diatomic Elements Several elements share electrons to form diatomic, covalent molecules:

6 Octet Rule Covalent compounds also obey the Octet Rule: Each atom in the bond is seeking a noble gas configuration Electrons are shared to achieve the octet For Example: Br → needs 1 electron to achieve an octet

7 Lewis Dot Structures We can use Lewis Dot structures to help us form Covalent Bonds: H with Cl H with O P with Br

8 Electron-Dot Formulas Electron-dot formulas: the order of bonded atoms in a covalent compound the bonding pairs of electrons between atoms the unshared (lone) valence electrons a central atom with an octet

9 Covalent Compounds

10 Bonding and Lone Pair Electrons Bonding pair of electrons are shared to create the covalent bond Non-bonding pair or lone pair make up the octet

11 Bonding and Lone Pair Electrons Bonding pair of electrons are shared to create the covalent bond Non-bonding pair or lone pair make up the octet Cl 2 HBr H 2 S

12 Naming Covalent Compounds 1)Most metallic atom comes first then the more negative + “-ide” For Example: NO NO 2 N 2 O 2)Name includes the total number of each atom: Table 6.10 (p. 178)

13 Naming Covalent Compounds For Example: SiBr 4 P 4 O 10

14 Naming Covalent Compounds Many covalent compounds have common names that you are most likely familiar with: NH 3 H 2 O H 2 S CH 4

15 Formulas and Names of Some Covalent Compounds

16 Select the correct name for each compound: A.SiCl 4 1) silicon chloride 2) tetrasilicon chloride 3) silicon tetrachloride B. P 2 O 5 1) phosphorus oxide 2) phosphorus pentoxide 3) diphosphorus pentoxide C.Cl 2 O 7 1) dichlorine heptoxide 2) dichlorine oxide 3) chlorine heptoxide Learning Check

17 Write the name of each covalent compound: CO_____________________ CO 2 _____________________ PCl 3 _____________________ CCl 4 _____________________ N 2 O_____________________ Learning Check


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