1 / 37

Chapter 10

Chapter 10. The Periodic Table. Section 1: Objectives. Describe how Mendeleev arranged elements in the first periodic table. Explain how elements are arranged in the modern periodic table.

miriam
Télécharger la présentation

Chapter 10

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 10 The Periodic Table

  2. Section 1: Objectives • Describe how Mendeleev arranged elements in the first periodic table. • Explain how elements are arranged in the modern periodic table. • Compare metals, non-metals, and metalloids based on their properties and on their location in the periodic table. • Describe the difference between a period and a group.

  3. How to Read the Periodic Table • Before we can sketch elements, we have to know how to read the periodic table. • Elements are divided into squares. • Each square tells you 5 things: • Element symbol • Atomic number • Element name • Atomic mass (mass number) • Physical state of element (M, NM, Mt)

  4. Discovering a Pattern • Before the 1860s, scientists had never arranged the elements. • In 1869, Russian chemist Dmitri Mendeleev arranged the elements inorder of increasing atomic mass. • These repeating patterns are periodic, meaning that they happen at regular intervals.

  5. Discovering a Pattern • His pattern had gaps in it though. • He predicted that elements that had not been discovered would fill these gaps. • By 1886, all the gaps had been filled and his predictions were right.

  6. Discovering a Pattern • A few elements did not fit the pattern. • In 1914, British scientists Henry Moseley found the number of protons in an atom. • When the elements were arranged by atomic number, they fit the pattern.

  7. Discovering a Pattern

  8. Discovering a Pattern • Elements are classified as metals, nonmetals, or metalloids. • Valence electrons (number of electrons in outer shell) helps determine an element’s properties. • The zigzag line on the periodic table helps you determine this.

  9. Discovering a Pattern • Metals are found to the left of the zigzag line. • Atoms of most metals have few electrons in their outer shell. • Most metals are: • Shiny • Malleable • Good conductors of heat/electricity

  10. Discovering a Pattern • Nonmetalsare found to the right of the zigzag line. • Almost all nonmetals have a complete set of electrons in their outer shell. • Nonmetals are: (the opposite of metals) • Not shiny • Not ductile • Not malleable • Poor conductors of heat/electricity

  11. Discovering a Pattern • Metalloids are elements that border the zigzag line. • Atoms of metalloids have about half the number of electrons in their outer shell. • Metalloids have some properties of metals and some of nonmetals. • Metalloids are also called semiconductors. (Si)

  12. Discovering a Pattern • Each square on the periodic table includes an element’s name, chemical symbol, atomic number, and mass number. • For most elements, the chemical symbol has one or 2 letters. • Why would some elements have 3 letters?

  13. Discovering a Pattern • Each horizontal row of elements is called a period. • The chemical and physical properties of elements in a row follow a repeating pattern. • Each vertical column of elements is called a group. • Elements in the same group often have similar chemical and physical properties.

  14. Discovering a Pattern • Elements in a group have the same number of valence electrons. • Atoms can give, take, or share electrons with other atoms. • An atom’s goal is to complete the outer energy level.

  15. Element Symbols (Ch. 10 Test) – Elements • 1) Carbon 8) Nitrogen 15) Bromine • 2) Iron 9) Lithium 16) Magnesium • 3) Oxygen 10) Beryllium 17) Manganese • 4) Potassium 11) Sodium • 5) Hydrogen 12) Calcium • 6) Helium 13) Neon • 7) Lead 14) Boron

  16. Section 1: Review Questions • 1)What is Mendeleev famous for? • 2) What did he predict about the periodic table? • 3) What did Moseley discover? • 4) What are valence electrons? • 5) List 2 properties of metals and nonmetals.

  17. Section 1: Review Questions • 6) What are metalloids also called? • 7)What does each square on the periodic table include? • 8) What does periodic mean? • 9) What determines the properties of an atom? • 10) Describe the goal for an atom.

  18. Section 2: Objectives • Explain why elements in a group often have similar properties. • Describe the properties of the elements in the groups of the periodic table.

  19. Group 1: Alkali Metals • Contain 1 valence electron. • Share physical and chemical properties. • Most reactive metals. • Can easily give away one outer level electron. • Alkali metals are so reactive, in nature they are only found combined with other elements. • Examples: • (Li) • (K)

  20. Group 2: Alkaline-Earth Metals • Contain 2 valence electrons. • Less reactive than alkali metals. • It uses more energy for elements to give 2 outer shell electrons than to give one. • Examples: • (Be) • (Mg)

  21. Groups 3-12: Transition Metals • Either 1 or 2 valence electrons. • Do not give away electrons as easily as elements in Groups 1 and 2. • Less reactive than Groups 1 and 2. • Share all properties of metals, but other properties vary widely. • Some transition metals appear at the bottom of the periodic table: • Lanthanides • Actinides

  22. Electron Cloud Rules • For today, there are 2 rules to know before adding electrons to a sketch: • Electron number will equal proton number. • The first level can hold only 2 electrons.

  23. Identifying and Sketching Atoms • Directions: Draw each element square along with all information for that element. • Under the square write the number of protons, neutrons, and electrons.

  24. Identifying and Sketching Atoms • 1) Hydrogen (1 V.E.) • 2) Beryllium (2 V.E.) • 3) Boron (3 V.E.) • 4) Nitrogen (5 V.E.) • 5) Oxygen (6 V.E.) • 6) Fluorine ( 7 V.E.) • 7) Helium (2 V.E.)

  25. Writing Prompt: Listening to Directions • Listening to directions is an important part of completing any assignment/lab activity. Explain why listening to directions is essential in successfully completing an activity. Also in your response, describe some safety concerns when students do not follow directions. What should you do if you do not understand the directions for an activity? You may use examples in your response to help explain your viewpoint. Your response should be no less than one paragraph.

  26. Lanthanides • Shiny • Reactive • Metals • Some of these elements are used to make steel.

  27. Actinides • Radioactive (unstable) • The atoms of a radioactive element can change into atoms of another element. • Elements after Plutonium (94) on the periodic table are only man-made in laboratories.

  28. Group 13: Boron Group • Contain 3 valence electrons. • Solid at room temperature. • Reactive • Contains all metals and 1 metalloid (Boron) • Examples: • (Al) • (Ga)

  29. Group 14: Carbon Group • Contains 4 valence electrons. • Solid at room temperature. • The reactivity varies among the elements. • Contains one nonmetal, 2 metalloids, and 2 metals • Examples: • (C) • (Si)

  30. Group 15: Nitrogen Group • Contains 5 valence electrons. • Solid at room temperature (except for nitrogen). • The reactivity varies among elements. • Examples: • (N) • (P)

  31. Group 16: Oxygen Group • Contains 6 valence electrons. • All but oxygen are solid at room temperature. • Reactive. • Examples: • (O) • (S)

  32. Group 17: Halogens • Contains 7 valence electrons. • Poor conductors of electric current. • Causes violent reactions with alkali metals. • Very reactive. • Examples: • (Br) • (F)

  33. Group 18: Noble Gases • Contain 8 valence electrons. (except helium) • Colorless, odorless gases at room temperature. • Unreactive because their outer shell is full. (do not need to gain or lose electrons) • Examples: • (Ne) • (Ar) • (Rn)

  34. Hydrogen • Contains 1 valence electron. • Reactive. • Colorless, odorless gas at room temperature. • Low density. • Explosive reactions with oxygen. • The properties of hydrogen do not match the properties of any single group, so it is set apart from other elements on the periodic table.

  35. Chapter 10 Sec. 1-2 Recap 1) What are group 13 elements called? 2) How many valence electrons does the carbon group contain? 3) List 2 properties of lanthanides. 4) _____ found the # of protons in an atom. 5) ____ _____ are outer shell electrons 6) Name 2 of the most reactive groups.

  36. Chapter 10 Sec. 1-2 Recap 7) List 2 examples of elements in Group 16. 8) __________ is very reactive and has a very low density. 9) List 1 thing that all elements in the same group have in common. 10) Why is helium considered a Noble Gas (Group 18) when it only has 2 valence electrons?

  37. Chapter 10 Review Questions • List the Group #, V.E. #, Group Name, and Element Symbol: • Nitrogen • Phosphorous • Radon • Francium • Rhodium • Cobalt • Lead • Bismuth • Indium • Bromine

More Related