1 / 25

Chapter 12 Elements and Their Properties

Chapter 12 Elements and Their Properties. Objectives. 12.1 Describe the properties of a typical metal 12.1 Identify the alkali and alkaline earth metals 12.1 Differentiate between three groups of transition elements. Minor Objectives.

pembroke
Download Presentation

Chapter 12 Elements and Their Properties

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Chapter 12 Elements and Their Properties

  2. Objectives • 12.1Describe the properties of a typical metal • 12.1 Identify the alkali and alkaline earth metals • 12.1 Differentiate between three groups of transition elements

  3. Minor Objectives • 12.2Distinguish among elements classified as lanthanides, actinides, and transuranium elements • 12.2 Determine the uses of transuranium elements • 12.2 Compare the pros and cons of making new elements

  4. Objectives • 12.3Recognize hydrogen as a nonmetal • 12.3 Compare and contrast properties of halogens • 12.3 Describe properties and uses of noble gases

  5. Objectives • 12.4Distinguish among metals, nonmetals, and metalloids • 12.4 Describe the nature of allotropes • 12.4 Recognize the significance of differences in crystal structure in carbon

  6. Metallic Bonding Name 4 Characteristics of a Metallic Bond. What is a Metallic Bond? - A metallic bond occurs in metals. A metal consists of positive ions surrounded by a “sea” of mobile electrons. • Good conductors of heat and electricity • Great strength • Malleable and Ductile • Luster This shows what a metallic bond might look like.

  7. Definition of Words • Malleable: Bendable, can be hammered to be thinner or rolled up in sheets • Ductile: Stretchable, can be pulled apart like laffy taffy • Luster: Reflects light, looks shiny

  8. Alkali Metals • First column (one word) • Highly Reactive, not found in nature by themselves • React with Water • Lose 1 Electron

  9. Alkaline Earth Metals • Second Column (Two words) • Some are found in nature by themselves (Top of column) such as Magnesium • Not as reactive as the Alkali Metals • Lose Two electrons • Calcium: Bones • Magnesium: Muscles (as well as bones)

  10. Transition Metals • Less reactive than other metals to left. • General Rule for metals is closer to bottom left, more reactive • Important sections include Iron Triad, Coinage Metals

  11. Iron Triad • Iron, Cobalt, Nickel • Only common metals known to create a magnetic field • Iron second most abundant element among metals in crust • Aluminum is first

  12. Coinage Metals • Copper, Silver, Gold • Very unreactive, which leads to be being able to be used as money • These also are the best conductors out of all the metals • Silver > Copper > Gold • Silver plays role also in photography

  13. Other notables • Zinc and Cadmium: Used to coat other metals for protection from rust (They do rust, but maintain good strength) • Mercury: Liquid metal at room temperature, poisonous

  14. Metals in the Crust • Oxygen 47% • Silicon 28% • Aluminum 8% • Iron 5% • Calcium 3.6% • Sodium 2.8% • Potassium 2.6% • Magnesium 2.1%

  15. 12 -2 Transuranium Elements • Uranium is largest atom that exists naturally (92 Protons) • Elements beyond Uranium are synthetic (made in laboratory) • Smash elements together at super speeds to collide and hopefully fuse • Is it worth it? They hope so, you may disagree.

  16. 12-3 Non-Metals • Properties of Non-Metals • Dull, Brittle, Powdery • Non-Metals alone tend to be gases at room temperature • Tightly Held Electrons • Can form ionic or covalent bonds

  17. Hydrogen • Most abundant element in universe (75 – 90%) depending on what you read • Number continues to drop… via fusion • A non-metal which tends to be fairly reactive (flammable, central to the role of acid/base) • Diatomic • Di means 2 atoms. Hydrogen Gas means 2 Hydrogens bound • Dr. HOFBrINCl (all of the diatomic)

  18. Halogens • “Salt Makers” • Have 7 valence electrons, exist diatomically • Very reactive (Flourine most) • Uses include: Etching glass, cleaning pools, keeping water safe, dyes (including lipstick), and warfare

  19. Noble Gases • Name comes from nobles not hanging out with the common folk. • Full outer shell. Inert (Unreactive) • Used in locations of high heat, light bulbs, blimps, storage of reactive elements

  20. Boron’s Column • Many are semiconductors (used by computers) • Aluminum is used all over the place (most abundant metal in crust) • Boron used in eyewash (boric acid) and water softeners

  21. Carbon Group • Carbon: Basis of organic life (the definition of organic – does it have carbon?) • Allotropes – Same element, different molecular structures • Carbon has many – graphite, diamond, fullerenes, coal • Silicon – Sand component • Lead – poisonous, used in ancient rome/paints

  22. Nitrogen’s Group • Nitrogen makes up 80% of atmosphere • Nitrogen – needed by plants (not in gas form, nitrates) as fertilizer • Phosphorus – Matches (as well as fertilizer) • Allotropes – Red and White matches

  23. Oxygen’s Group • Similar properties to halogens • Oxygen 20% of atmosphere • Allotropes – oxygen and ozone • Sulfur – Used in paints (pigments) and battery acid (Sulfuric acid)

More Related