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By Mrs. Billings.  What is a bond?  4 Types of bonds  Naming type I, II, & III.

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Presentation on theme: "By Mrs. Billings.  What is a bond?  4 Types of bonds  Naming type I, II, & III."— Presentation transcript:

1 By Mrs. Billings

2  What is a bond?  4 Types of bonds  Naming type I, II, & III

3  A bond is an electrostatic force that holds atoms together.  Atoms will bond using their electrons.

4  Ionic bonding ◦ Electrons are transferred from one atom to the other. (give/take) ◦ Happens between metals & nonmetals (cations & anions). ◦ The atom that loses the electron becomes positive (cation) and the atom that gains the electron becomes negative (anion)...ions, get it, ionic bond. ◦ Why does this happen? The electrogegativity difference between the atoms is > 1.7 so one atom is able to rip the electron away. ◦ Form a crystal lattice structure.

5  Covalent Bonding ◦ Electrons are shared between atoms. ◦ Happens between nonmetals only. ◦ There are 2 types of covalent bonding based on the amount of sharing of electrons.  Polar covalent is uneven sharing, thus creating a pole.  Bond electronegativity difference <1.7  Structure asymmetrical.  Nonpolar covalent is even sharing, thus no pole.  Bond electronegativity difference <0.4  Structure symmetrical.

6  Metallic bonding ◦ Delocalized electrons float around the electron sea. ◦ Happens between metals only. ◦ Characteristics:  Malleable  Ductile  Luster  Conductor

7  A for ionic, B for covalent, and C for metallic ◦ Li 2 S ◦ AuAg ◦ PbNO 3 ◦ NO ◦ C 6 H 12 O 6 ◦ SnN

8  A for ionic, B for polar covalent, C for nonpolar covalent ◦K2O◦K2O ◦ NS 3 ◦N2◦N2 ◦ AuI ◦ NaF ◦ C 6 H 12

9  Type I ◦ Use for ionic bonds when the cation has only one charge (groups1A-3A). ◦ The first element keeps its name and the second element changes the end of its name to –ide (unless it already has a fancy name). ◦ Criss-cross charges if uneven.  Ex. NaBr is sodium bromide  Ex. CaCl 2 is calcium chloride  Ex. Be(ClO 3 ) 2 is beryllium chlorate

10  Type II ◦ Use for ionic bonds when the cation has more than one charge (transition metals). ◦ The first element keeps its name and the second element changes the end of its name to –ide (unless it already has a fancy name). ◦ Use a roman numeral to show the charge of the first ion. ◦ Criss-cross charges if uneven.  Ex. AuI is gold (I) iodide  Ex. Mn 2 O 3 is manganese (III) oxide  Ex. W 3 (PO 4 ) 2 is tungsten (II) phosphate

11  Type III ◦ Use for covalent bonds. ◦ Use prefixes to denote the number of atoms and change the ending of the second element to -ide.  Ex. S 2 O 3 is disulfur trioxide  Ex.N 3 P 4 is trinitrogen tetraphosphide  Ex. BrH 5 is bromine pentahydride

12

13  Li 2 S  AuI 3  PbNO 3  C 5 H 10  NO  SnN

14  Barium fluoride  Zinc (II) nitride  Carbon heptaiodide  Ammonium sulfate  Aluminum hypochlorite  Pentaphosporus nonanitride  Tungsten (IV) permanganate

15  whiteboards

16  What part of the atom is involved in a chemical bond? ◦ electrons

17  What type of bond is SrS? ◦ ionic

18  Name Ni 2 S 3. ◦ Nickel (III) sulfide

19  What happens to the electrons in a metallic bond? ◦ Delocalized electrons float in electron sea.

20  What structure does an ionic bond make? ◦ Crystal lattice

21  What type of bond is H 2 O? (Be specific!!) ◦ Polar covalent

22 Write the formula for Cobalt (III) oxide. Co 2 O 3

23  What happens to the electrons in a nonpolar covalent bond? ◦ Shared equally

24  Write the name for C 4 H 10. ◦ Tetracarbon decahydride

25  What happens to the electrons in an ionic bond? ◦ Transferred ◦ Give/take

26  What are 2 characteristics of metals? ◦ Malleable ◦ Ductile ◦ Luster ◦ Conductor ◦ Solid


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