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Chemical Bonds Study Guide Define the following: 1. Chemical formula - the way of expressing information about the proportions of atoms that constitute a particular chemical compound, using element symbols and numbers. 2. Molecule- electrically neutral group of two or more atoms held together by chemical bonds 3. Valence electrons- electrons located in the outermost electron level of an atom 4. Octet rule- chemical rule of thumb that states that atoms want to have 8 valence electrons 5. ionic bonds- a type of chemical bond that involves a metal and a nonmetal; formed due to the attraction of opposite charges on the cation and anion; formed when metals donate electrons to nonmetals 6. ion- formed when an atom gains or loses an electron. 7. Cation- a positively charged ion formed when metals donate electrons 8. Anion- a negatively charged ion, formed when nonmetals accept electrons 9. oxidation number- the charge on an ion 10. metallic bonds- describes how metal atoms are held together in a solid 11. alloy- a combination of 2 or more elements, at least one is a metal 12. covalent bonds- bonds formed when nonmetals share electrons 13. polar bonds- covalent bonds that have a positive end and a negative end 14. dipoles- polar bonds 15. electronegativity- the ability of an atom to attract electrons Use the following chemical formulas to determine the number of atoms/element. 1. H2O H: 2 O: 1 2. MgCl2 Mg: 1 Cl:2 3. C6H12O6 C:6 H:12 O: 6 4. Na2SO4 Na:2 S:1 O:4 Ionic Bonds 1. Ionic bonds form between metals and nonmetals 2. Metals typically donate electrons, while nonmetals accept electrons. 3. Name the following ionic bonds. A. NaCl- sodium chloride B. CaBr2- calcium bromide C. BeO – beryllium oxide D. Li2S- lithium sulfide 4. Complete the following table: Use Lewis structures for your illustrations. Be sure to diagram movement of electrons. Include oxidation numbers. Compounds Symbols with Oxidation Number Formula Na,Cl Na+1 NaCl K, S K+1 S-2 K2S Ca, F Ca+2 F-1 CaF2 Mg, S Mg+2 S-2 MgS Al, O Al+3 O-2 Al2O3 Cl-1 Illustration Metallic Bonds 1. Metals are like cations floating in a sea of electrons, because the valence electrons of one atom are shared with all surrounding atoms. 2. List and describe three properties of metals. Shiny Conduct electricity- electrons are free to move around Ductile- can be drawn into thin wires Malleable- can be hammered into shapes 3. Define and give 2 examples of metal alloys. Alloys- combination of 2 or more elements, at least one is a metal Examples- steel, sterling silver, 14K gold Covalent Bonds 1. Covalent Bonds form between a nonmetal and a nonmetal 2. Covalent bonds form when 2 atoms share electrons. 3. Illustrate the following compounds using Lewis structures. Be sure to draw circles around shared electrons. A. CH4 D. CO2 B. CHCl3 D. N2 4. Complete the following table. Include + and - on polar bonds. Bonded Atoms Bond Type Li2S Electronegat ivity Difference 1.5 NH3 0.9 Polar covalent Ionic (metal and nonmetal) Which is more negative S N Illustration CS2 0 Nonpolar covalent Equal H2 0 Nonpolar covalent equal KBr 2.0 Ionic Br N2 0 Nonpolar covalent Equal CCl4 0.5 Polar covalent Cl 5. Name the following covalent bonds. A. H2O- dihydrogen monoxide B. NO2- nitrogen dioxide C. CCl4- carbon tetrachloride D. NH3- nitrogen trihydride 6. Complete the following table comparing ionic and covalent bonds. Ionic Bonds Metal and nonmetal Donate and Accept Electrons High melting and boiling points Soluble in water (polar substances) Conduct electricity when dissolved or melted Solid crystalline structure Covalent Bonds Nonmetal and nonmetal Share electrons Low melting and boiling points Non-soluble in water (polar substances) Does not conduct electricity Solid, liquid, or gas