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Chemical Bonding

Chemical Bonding. Chapter 17. Chapter 17. Metals vs. Nonmetals (and what comes in between) We will be taking notes, so get out your notebooks and something to write with. Learning Objective Students will understand the difference between Metals, Nonmetals and Metalloids. Observations.

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Chemical Bonding

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  1. Chemical Bonding Chapter 17

  2. Chapter 17 Metals vs. Nonmetals (and what comes in between) We will be taking notes, so get out your notebooks and something to write with. Learning Objective Students will understand the difference between Metals, Nonmetals and Metalloids.

  3. Observations • Your lab group will be getting sealed test tubes with pure* elements in them. • You till copy the table that’s on the next slide • Then, fill in the information with what what you see in the test tube *Kind of…

  4. Chapter 17 Metals vs. Nonmetals (and what comes in between), ions, and molecules. We will be taking notes, so get out your notebooks and something to write with. Learning Targets Students will understand the difference between Metals, Nonmetals and Metalloids. Students will be able to apply what they know about ions to what they have learned abut metals and how they form metal ions.

  5. The Big Fat Black (or grey) Line • Why is there a dark line on the periodic table? • It marks a distinction between two kinds of elements: Metals and nonmetals.

  6. Periodic Trends • Group 1 Metals • These metals are soft and can be cut easily. • As you move down Group 1, the elements become more reactive with water.

  7. Metals • What is a metal? • Everything to the left of the big fat line. • Characteristics include: • Shiny, slivery • Malleable (bendable) • Conducts heat and electricity well. • Examples: • Tin, Zinc, Lead, & Magnesium

  8. Nonmetals • Everything to the right of the big fat line is. • Characteristics include: • Dull, multicolored • Brittle (breakable) • Conducts heat and electricity badly. • Examples: • Sulfur, Carbon, Iodine, & Nitrogen. • What is a nonmetal?

  9. Metalloids • Because nothing in science is allowed to be simple. • Most elements touching the big fat line is categorized as a metalloid. • Characteristics can include any for metals or nonmetals • Examples: • Boron, Silicon, Germanium, & Arsenic • What is a metalloid? • Silicon • Brittle like nonmetal • Conducts electricity well like metal

  10. Ions • What is an ion? • An atom that has either gained or lost one or more electrons • Positive ion – cation • Negative ion – anion • Electrons have a charge of -1 (be careful when you add or subtract)

  11. Ions • How do we determine charge? • Determine the number of electrons that should exist in the neutral atom (atomic number) • Determine how many electrons are present • Subtract and assign the charge, this is called the oxidation state NOTE: An element may have more than one oxidation state

  12. Sodium Ion • How many protons and electrons does sodium have? • What is the best way to make sodium stable? • 11 protons • 11 electrons • Lose 1 electron • Na1+

  13. Chlorine Ion • How many protons and electrons does chlorine have? • What is the best way to make chlorine stable? • 17 protons • 17 electrons • Gain 1 electron • Cl1-

  14. Most Common Oxidation States

  15. Ions • Determine how many electrons there are in the following ions: • Mg2+ • Fe3+ • C4- • I7- • Ar0 • lost 2 & has 10 electrons • lost 3 & has 23 electrons • gained 4 & has10 electrons • gained 7 & has 60 electrons • gained/lost none & has 18 electrons

  16. What does this have to do with ions? • Answer the below question on a loose piece of paper and turn it in to the box. It is NOT GRADED. It is only for my understanding of how well the lesson went. • Potassium reacts with water to make it more stable. What is happening to potassium during this reaction?

  17. Chapter 17 Molecules and Chemical Formulas We will be taking notes, so get out your notebooks and something to write with.

  18. Molecules • What is the difference between monatomic, diatomic and polyatomic? • Monatomic – only one atom • Metals and noble gases are monatomic atoms • Diatomic – contains two atoms • Ex. H2 or CO • Polyatomic - contains more than two atoms • Ex. H2O and O3

  19. Molecules • What are molecules? • Any diatomic or polyatomic combination of atoms • A molecule can be an element or a compound • Cl2 vs. O3 vs. H2O Element Element Compound

  20. Molecules and Ions • What is the connection between molecules and ions? • An ion is a charged atom • A polyatomic ion is a charged diatomic or polyatomic molecule • OH1- (hydroxide) • CN1- (cyanide) • CO32- (carbonate) • NH41+ (ammonium)

  21. Chemical Formulas • What is a chemical formula? • Shows us what elements there are in the molecule • How many atoms of each element are present

  22. Chemical Formulas • What is the formula for three caffeine molecules? • 3C8H10N4O2 • Subscript indicates how many of each element are in the molecule • 8 carbons • 10 hydrogens • 4 nitrogens • 2 oxygens • Coefficient shows how many molecules

  23. Chemical Formulas • How do sodium and chlorine combine? • Oppositely charged ions attract each other • Na1+ and Cl1- chemically combine to create the compound NaCl, which is table salt

  24. Chemical Formulas • How do we make a chemical formula neutral? • The total charge of the ions in the molecule equals zero • Must have positive and negative ions to do this • If the charges don’t cancel out use subscripts to balance them

  25. Chemical Formulas • How do you determine a chemical formula? • Use the “swap and drop” method • Ex. Iron (III) Sulfide NOTE! If the positive and negative charge are the same, the subscripts NEED to be set to 1

  26. Chemical Formulas • What is the formula for magnesium bromide? • Mg2+ and Br1- • “swap and drop” • Mg1Br2, but we do not write the 1 • MgBr2

  27. Chemical Formulas • What happens when we have a polyatomic ion? • What is the formula for potassium cyanide (CN1-)? • Treat the polyatomic as one piece with one charge • K1+ and CN1- • “swap and drop” • KCN

  28. Chapter 17 Chemical Formulas We will be taking notes, so get out your notebooks and something to write with.

  29. Chemical Formulas Practice • What are the formulas of the following chemicals: • Lithium and Bromide • Aluminum and Chloride • Beryllium and Oxide • Sodium and Hydroxide • Calcium and Nitrate • Yttrium and Orthosilicate • LiBr • AlCl3 • BeO • NaOH • Ca(NO3)2 • Y4(SiO4)3 Same charges, so subscripts changed to 1 Need parentheses to show that it is one piece

  30. Chemical Formulas Undone • How do you determine the oxidation states from the formula? • Al2O3 • FrF • FeCl3 • KOH • Ca(MnO4)2 • WBr6 • Reverse the “swap and drop” method • Remember: The cation always comes before the anion! • Al 3+ and O2- • Fr1+ and F1- • Fe3+ and Cl1- • K1+ and OH1- • Ca2+ and MnO41- • W6+and Br1- One piece with one charge!

  31. Ion Puzzle Cards • Please combine the following ion puzzle pieces and write the chemical formula in your notes: • Barium and Chloride • Potassium and Bromide • Cesium and Fluoride • Silver and Chloride • Scandium and Nitride • Barium and Hydroxide

  32. Ion Puzzle Cards Continued • Aluminum and Hydroxide • Zinc and Chloride • Barium and Sulfide • Potassium and Cyanide • Ammoniumand Chloride • Lead andChloride • Zincand Carbonate • Sodium andOxide • Lead and Sulfide (Careful with this one!)

  33. Ion Puzzle Cards Continued • Iron (II) and Chlorate • Iron (II) and Sulfide • Mercury (I) and Chromate • Osmium and Chloride • Ammoniumand Phosphate • Potassium andPermanganate • Scandiumand Sulfide • Thallium (I) andBenzoate • Barium and Cyanide • Francium and Nitrate • Gold andPeroxide

  34. Chapter 17 Naming Compounds

  35. Naming Compounds • What scientific word do we use for naming? • What is the difference between organic and inorganic compounds? • Nomenclature • Organic compounds contain primarily carbon and hydrogen and inorganic compounds don’t

  36. Naming Compounds • What two main categories can we divide inorganic compounds into? • Covalent compounds are made up of only non-metals or metalloids • Metalloids are B, Si, Ge, As, Sb, Te and Po • Ionic compounds are made up of metals and non-metals

  37. Naming Ionic Compounds • How do you name an ionic compound? • Step 1: Write the name of the cation first • Step 2: Write the name of the anion but change the suffix (ending) to –ide • NaCl • Ex. Sodium Chloride • NOTE: If there is a polyatomic ion, its name does not change

  38. Naming Ionic Compounds • How do you name an ionic compound that has more than one oxidation state? • Using roman numerals to represent the oxidation state • Ex. Iron • Iron(II) or Fe(II) • Iron(III) or Fe (III) • Ex. Fe2O3 • Iron (III) Oxide

  39. Naming Ionic CompoundsPractice • Please name the following ionic compounds: • AlCl3 • NaOH • HgO • MoI6 • Y2Te3 • NbF5 • IrI • Cr2O3 • HgCl • Pb(NO3)4 • Aluminum Chloride • Sodium Hydroxide • Mercury (II) Oxide • Molybdenum Iodide • Yttrium Telluride • Niobium (V) fluoride • Iridium Iodide • Chromium (III) oxide • Mercury (I) chloride • Lead (IV) nitrate

  40. Naming Covalent compounds • How do you name covalent compounds? • Step 1: Write the name of the first part without any suffix • If there is more than one, add the appropriate prefix • Step 2: Write the name of the second part change the suffix (ending) to –ideand add the appropriate prefix • CO2 • Ex. Carbon Dioxide

  41. Naming Covalent CompoundsPractice • Please name the following covalent compounds: • SO2 • BF3 • SiO4 • C2S4 • NF3 • PoBr2 • SeI4 • NO2 • CO • Sulfur dioxide • Boron trifluoride • Silicon tetroxide • Dicarbontetrasulfide • Nitrogen trifluoride • Polonium dibromide • Selenium tetraiodide • Nitrogen dioxide • Carbon monoxide

  42. Chapter 17 Metallic Bonding Learning Targets: Students will understand the configuration of metal ions and electrons in metallic bonds Students will understand how alloys work, and why they are used by society.

  43. Chemical Bonds • What is a chemical bond? • A force that holds two or more elements together • Three types: • Metallic • Ionic • Covalent

  44. Metallic Bonds • What do metals do with their valence electrons? • Lose/donate them and become cations (positively charged) to become stable

  45. Metallic Bonds • How do the metal ions arrange themselves? • Arranged in perfect rows and columns • In a crystal structure, called a lattice

  46. Metallic Bonds • Where are the electrons that were lost/donated? • Moving through the lattice around the metal ions • “Sea of Electrons” • These electrons hold the ions together in a metallic bond

  47. Metallic Bonds • What are metallic bonds responsible for? • Metals can: • Conduct electricity and heat because electrons are easily moved • Be easily bent and shaped because of the lattice structure • Malleable – bendable • Ductile – drawn into a wire

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