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CH. 5 Activity Lists

CH. 5 Activity Lists. Equipment box Print out of electron shells Chips representing electrons Compound and molecule sets (balls and springs) Aluminum foil, metal wire (properties) Handouts: Counting atoms in compounds and identifying as a compound or molecule

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CH. 5 Activity Lists

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  1. CH. 5 Activity Lists Equipment box • Print out of electron shells • Chips representing electrons • Compound and molecule sets (balls and springs) • Aluminum foil, metal wire (properties) Handouts: • Counting atoms in compounds and identifying as a compound or molecule • Venn diagram of molecule and compound • Venn diagram of bonds • Counting valence electrons and predict type of bond

  2. Chapter 5 Menu Lesson 1:How do Atoms Form Compounds? Lesson 2:How do Solids Form? Standards: Structure of Matter BIG IDEA: Atoms of two or more elements can combine to make compounds that are different from the elements the made them. Click on a hyperlink to view the corresponding lesson.

  3. 5.1 How Atoms Form CompoundsImportant Vocabulary 1) Compound 5) ionic bond 2) chemical formula 6) valence 3) Molecule 7) covalent bond 4) chemical bond REVIEW VOCAB • Atom • Nucleus

  4. 5.1 How Atoms Form Compounds What is a compound? • A compound is a pure substance that contains two or more elements. • Compounds are combinations of elements with properties that are different from the elements that formed them.

  5. 5.1 How Atoms Form Compounds How are compounds written? • A chemical formula contains the elements’ symbol and how many atoms of each element (subscript). • Example: H2O subscript

  6. 5.1 How Atoms Form Compounds Compounds (cont.) • A water molecule, or H2O, is two hydrogen atoms bonded to one oxygen atom. • The subscript number shows how many atoms the element are in the compound. • A molecule is a neutral particle that forms as a result of electron sharing. • Activity #1: Building simple compounds How can a molecule model be built?

  7. What is the difference between a compound and a molecule? Molecules have more than one atom. Compounds always have more than one element (and more than one atom) Ex. H2O: compound and molecule O2: molecule NaCl: compound and molecule Compounds are always molecules, but molecules are not always compounds. (Venn diagram)

  8. 5.1 How Atoms Form Compounds Describing Compounds (cont.) • The chemical formula for sucrose, C12H22O11, includes all the atoms in one molecule.

  9. 5.1 How Atoms Form Compounds Compounds and Their Elements • Compounds have different properties than the elements that make them up. • Sodium chloride (NaCl) is table salt. • Sodium (Na) is a soft metal. • Chlorine (Cl) is a greenish-yellow gas. • Handout #1

  10. 5.1 How Atoms Form Compounds What holds compounds together? • A chemical bond is a force that holds atoms together in a compound. • A chemical bond is made when electrons are transferred.

  11. 5.1 How Atoms Form Compounds Why do atoms make chemical bonds? Atoms make chemical bonds so that they can have full shells of electrons. So when atoms do not have a full shell, they can give electrons, get electrons, or share electrons.

  12. What are the types Chemical Bonds? • When an atom gives away electrons or gets electrons an IONIC BOND forms. • When an atom shares electrons, a COVALENT BOND forms.

  13. How can you tell what kind of bonds an atom will form? • You must draw the atom and count the number of electrons in the last shell (these electrons are called valence electrons) • If an atom has: • 1,2, or 3 electrons it will give them away (ionic) • 4 electrons it will share (covalent) • 5,6, or 7 it will get electrons (ionic) Activity and Handout #2: Counting valence electrons and predicting type of bond

  14. 5.1 How Atoms Form Compounds Which elements bond together? • Just count valence electrons • How many electrons does it need to give away or take away to have a full shell 3) Find an atom that needs to take that amount or needs to give that amount away .

  15. Why do atoms form chemical bonds? SO THAT THEY HAVE FULL ELECTRON SHELLS

  16. 5.1 How Atoms Form Compounds Examples of Ionic bonds: (cont.) • A lithium atom gives up an electron to a fluorine atom. • The result is the compound lithium fluoride (positively charged lithium ion and a negatively charged fluoride ion).

  17. 5.1 How Atoms Form Compounds Ionic Bonds—Transferring Electrons (cont.)

  18. 5.1 How Atoms Form Compounds Examples of Ionic Bond Compounds • Elements in Group 1 can transfer 1 electron • Non-metals in Group 17 can gain an electron • When an ion from Group 1 and an ion from Group 17 combine, they form an ionic bond and make NaCl • Now Na and Cl have FULL SHELLS OF ELECTRONS Atoms in Group 2 have two valence electrons (give away) and Group 16 need two electrons (take), so these two groups make compounds together.

  19. 5.1 How Atoms Form Compounds Other Ionic Compounds (cont.) • Magnesium can transfer one electron to each of 2 Fluorine atoms to form magnesium fluoride (MgF2).

  20. 5.1 How Atoms Form Compounds Properties of Ionic Compounds • Usually solids at room temperature • Brittle and break apart easily • Have high melting and boiling points • Many dissolve in water

  21. 5.1 How Atoms Form Compounds What is a Covalent Bonds? • Some elements need to gain or lose too many electrons. • A covalent bond is a chemical bond formed when atoms share electrons.

  22. 5.1 How Atoms Form Compounds Covalent Bonds—Sharing Electrons (cont.) • Carbon has 4 valence electrons. • It needs 4 more electrons to fill its energy shell, so it shares

  23. 5.1 How Atoms Form Compounds Single Covalent Bonds • Hydrogen has one unpaired electron. • Two hydrogen atoms share their single electrons to form a pair. • The shared pair of electrons is a single covalent bond, which holds the hydrogen molecule H2 together.

  24. 5.1 How Atoms Form Compounds Double and Triple Bonds • Some atoms may form stronger bonds by sharing more than one pair of electrons. • A double bond has two pairs of shared electrons and is stronger than a single bond. • A triple bond has three pairs of shared electrons and is stronger than a double bond.

  25. 5.1 How Atoms Form Compounds Properties of Covalent Compounds • Can be solids, liquids, or gases at room temperature • Usually have lower melting and boiling points than ionic compounds • Do not usually separate in water • Most do not conduct electricity • Activity and handout #3: Matching atoms to form compounds base on valence electrons (molecule sets) • Venn diagram of bonds

  26. 5.1 How Atoms Form Compounds Covalent Bonds—Sharing Electrons (cont.)

  27. 5.1 How Atoms Form Compounds Diagramming Electrons—Lewis Dot Diagrams • A Lewis dot diagram is a system to represent atoms and their electrons. • You must know the number of valence electrons an atom has. • Valence electrons are the electrons in the outermost energy level. • Handout practicing lewis dot diagrams • Activity with students having diagrams and students need to find their match.

  28. 5.1 How Atoms Form Compounds Diagramming Electrons—Lewis Dot Diagrams Diagramming Electrons—Lewis Dot Diagrams (cont.)

  29. 5.1 How Atoms Form Compounds What are Noble Gases? • Elements in Group 18 are the noble gases. • The noble gases are stable because their outer energy levels are filled. • Elements that are stable rarely react to form compounds.

  30. 5.1 How Atoms Form Compounds Lesson 1 Review • A • B • C • D Bromine is in Group 17. How many electrons does bromine need to gain or lose to obtain a noble gas structure? A gain one electron B gain two electrons C lose one electron D lose two electrons

  31. 5.1 How Atoms Form Compounds Lesson 1 Review • A • B • C • D Which element can form a negative ion? A carbon B magnesium C chlorine D lithium

  32. 5.2 How do Solids form? Important Vocabulary malleability Ductility Crystal Polymer monomer

  33. What are the types of solids? • Metals • Crystals 3) Polymers

  34. 5.2 Forming Solids What are Metals? • Metals are elements that are usually shiny, good conductors of electricity and heat, and solid at room temperature.

  35. 5.2 Forming Solids What are properties of metals? • Metals are good conductors because their electrons move freely. • Metals can be hammered into sheets or pulled into wires without breaking. • Malleability is the ability of a metal to be hammered or rolled into sheets • Ductility is the ability of a substance to be pulled into a wire.

  36. 5.2 Forming Solids How do atoms of a metal combine? • Metal atoms combine in a regular pattern in which some electrons are free to move about.

  37. 5.2 Forming Solids What are Crystals? • A crystal is a regular, repeating arrangement of atoms, ions, or molecules. • Crystals are formed from repeating patterns. • A unit cell is the smallest repeating pattern that shows how atoms, ions, or molecules are arranged in a crystal.

  38. 5.2 Forming Solids What is a polymer? • A polymer is a covalent compound made up of many repeating units linked together in a chain. • A monomer is a single molecule that forms a link in a polymer chain. • Many hundreds of monomers link together to form a solid polymer.

  39. 5.2 Forming Solids Example of polymer: Synthetic Polymers • Synthetic polymers, such as polyethylene, are polymers manufactured by humans.

  40. 5.2 Forming Solids Example of polymers: Natural Polymers • All living cells must contain three important kinds of natural organic polymers—proteins, carbohydrates, and nucleic acids. Labs: 1) Glurch vs. oobleck 2) Making crystals

  41. 5.2 Forming Solids Natural Polymers (cont.) • Amino acid monomers join together to form a protein. • Protein and carbohydrate polymers shown with their monomers.

  42. Chapter Assessment 1 • A • B • C • D How many dots are in a Lewis dot diagram for the Group 1 element lithium? A 1 B 2 C 3 D 4

  43. Chapter Assessment 3 • A • B • C • D Why are noble gases unlikely to form compounds with other elements? A They form ionic bonds. B They have 8 valence electrons. C They form covalent bonds. D Their outer energy levels are not filled with electrons.

  44. Chapter Assessment 4 • A • B • C • D Compounds sharing electrons are held together by ____. A ionic bonds B covalent bonds C metallic bonds D polymer chains

  45. SCI 3.b CA Standards Practice 1 • A • B • C • D Which elements are least likely to react with other elements? A metals B Group 17 elements C Group 16 elements D Noble gases

  46. CA Standards Practice 2 SCI 3.b • A • B • C • D In the ionic compound magnesium oxide (MgO), how many electrons did oxygen give magnesium? A 1 B 2 C 3 D none of the above

  47. CA Standards Practice 4 SCI 3.f • A • B • C • D Noble gases are in which group on the periodic table? A 1 B 2 C 17 D 18

  48. CA Standards Practice 5 SCI 7.c • A • B • C • D Which property of copper allows it to be pulled into wires? A ductility B malleability C conductivity D luster

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