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Monday, May 20 th

Monday, May 20 th. Entry Task Create a 10 question test for chapter 5. You can have any type of questions. Make sure to cover what you feel are the most important things from chapter 5. Schedule: Chapter 5 Test. Homework: Read/RSG 6.1. Objective:

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Monday, May 20 th

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  1. Monday, May 20th Entry Task Create a 10 question test for chapter 5. You can have any type of questions. Make sure to cover what you feel are the most important things from chapter 5. Schedule: • Chapter 5 Test Homework: • Read/RSG 6.1 • Objective: • I can be assessed on important information about atoms, elements, and the periodic table.

  2. Tuesday, May 21st Entry Task Match the following definitions with the correct terms Definitions: • A negatively charged particle that moves around an atom’s nucleus • An atom that has lost an electron • An atom that has gained an electron Terms Electron, negative ion, positive ion Homework: • Page 173 #1-6 Schedule: • 6.1 Notes and Ratios Please have on desk: • 6.1 RSG • Objective: • I can explain how compounds are made from combinations of atoms • I can explain how chemical formulas represent compounds

  3. Properties of Compounds • Remember how we discussed that each element had its own specific property and that was how it was organized into the periodic table • Well when you put these elements together they form compounds • These compounds however have different properties than the elements that make them up • The elements are held together by bonds. The bonds (number and strength) help determine the properties • The specific elements that make up the compound and the amount of them also help determine properties

  4. Atoms combine in predictable numbers • Any specific compound always contains atoms of elements in a specific ratio • Ammonia • Hydrogen and nitrogen • 3 hydrogen 1 nitrogen • 3:1 • Hydrazoic acid • Hydrogen and nitrogen • 1 hydrogen 3 nitrogen • 1:3

  5. Chemical Formulas • Uses chemical symbols to repersent the atoms and their ratios in a chemical compound • Carbon dioxide • CO2 • One carbon two oxygen • Subscriptsubscript identifies how many of those atoms there are in the compound (two or more) • C6H12O6 -Glucose

  6. Chemical Formulas • Carbon Monoxide • Chemical Formula: • CO • Atoms: • C (carbon) O (oxygen) • Atomic Ratio: • 1:1 • What is the ratio of carbon to oxygen

  7. Chemical Formulas • Methane • Chemical Formula: • CH4 • Atoms: • C (carbon) H (hydrogen) • Atomic Ratio: • 1:4 • What is the ratio of hydrogen to carbon?

  8. Chemical Formulas • Sulfuric acid • Chemical Formula: • H2SO4 • Atoms: • H (hydrogen) S (sulfur) O (oxygen) • Atomic Ratio: • 2:1:4 • What is the ratio of hydrogen to sulfur? • What is the ratio of sulfur to oxygen?

  9. Wednesday, May 22nd Entry Task Write down the following and…. Finish the statement • Elements combine to form _______________________ • Electrons are located in a cloud around the ______________________ • Atoms can lose or gains electrons to form _______________________ Schedule: • 6.2 Questions Homework: • Page 182 #1-6 • Anything you didn’t finish yesterday Objective: I can understand how electrons are involved in chemical bonding • Please have on desk: • Questions from yesterday • 6.2 RSG

  10. Thursday, May 23rd Entry Task Share your 6.1 and 6.2 question answers with your partner. Fix any incorrect answers. Schedule: • Ionic Bonds Notes Homework: • Anything not done in class Objective: I can understand how electrons are involved in chemical bonding • Please have on desk: • 6.2 RSG • 6.1 and 6.2 questions

  11. Bonding of elements • Always involves electrons • Bonds make compounds more than just mixtures of atoms • Structure of an atom • Atoms have a nucleus • Protons and neutrons • Positive charge • Atoms also have an electron cloud around the nucleus • Electrons • Negative charge • How the electron clouds interact determines the kind of chemical bond that is formed.

  12. Transferring electrons • Ion is formed when an atom gains or loses electrons • Lose electrons + ion • Gain electrons – ion • Metals form positive ions (give up e- ) • Gases form negative ions (gain e- ) • RULE OF 8!!!

  13. Rule of 8 • Elements like to have 8 electrons orbiting in the outside electron shell • Group numbers can tell you how many electrons are in the outer shell • Group 1- has 1 • Group 2- has 2 • Group 13- has 3 • Group 14- has 4 • Group 15-has 5 • Group 16- has 6 • group 17- has 7 • group 18- has 8 • If a group has less than 4 they give up their electrons- making them + ions • If a group has more than 4 they take electrons- making them – ions • If they have 4 they can do either • What they do with their electrons determines what other elements they bond with • Oxygen has 6 electrons and Hydrogen has 1 electron • H2 o is two hydrogen (2 electrons) and one oxygen (6 electrons) 2 electrons+6 electrons is 8! IT’S A HAPPY MOLECULE!

  14. Ionic Bonds • Sodium atom • Na • Group 1 • Gives up one e- • Positive ion • Chlorine atom • Cl • Group 17 • Gains one e- • Negative ion Sodium gives up its electron to give to chlorine. Sodium is now positive and chlorine is now negative. Opposites attract! Sodium and Chlorine now bond together. Form NaCl Sodium Chloride SALT!

  15. Ionic Compound Names • Named after the elements that make up the compound • Positive ion name is the same as the same of the atom • The negative ion name is formed by adding -ide to the end. • Positive ion is always named first • NAME BaI2

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