Chapter-1-2-Periodic-Table.pptxhshsjssks

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1. Introduction to the Periodic Table Atomic Number ● Symbol ● Atomic Weight Element ● Compound ● Mixture

2. I am Dmitri Mendeleev! I made the PERIODIC TABLE !

3. What is the PERIODIC TABLE? Shows all known elements in the universe. Organizes the elements by chemical properties.

4. Periodic Table Invented by Dmitri Mendeleev in the late 1800’s Many of the elements in the table were not discovered until long after the table was invented All elements are in their most basic form and cannot be simplified Table lists the atomic number and atomic mass The atomic number is the number of protons in the nucleus or the center of the atom The atomic mass is the sum of the masses of the protons and neutrons. Electrons weigh about 1/2000 as a proton. Carbon (C) has atomic number 6 because there are 6 protons in the nucleus.

5. Periodic Chart Organization Elements are divided into two groups- metals and nonmetals Of the 120 known elements (including synthesize), approximately 81 are metals. 92 occur naturally in the earth. Metals have the following characteristics to varying degrees High electrical conductivity and High thermal conductivity Luster- ability to reflext light. Ductility, maleability Loose electrons (low ionization energy) readily when they react with nonmetals Metallic character should decrease as we move across the Periodic Table and increase as we move down. Nonmetals tend to be insulators (solid, liquid, or gas) Gain electrons in chemical reactions Noble gases are inert Metalloids are semiconductors

6. How do you read the PERIODIC TABLE?

7. What is the ATOMIC NUMBER? The number of protons found in the nucleus of an atom Or The number of electrons surrounding the nucleus of an atom.

8. What is the SYMBOL? An abbreviation of the element name.

9. What is the ATOMIC WEIGHT? The number of protons and neutrons in the nucleus of an atom.

10. How do I find the number of protons, electrons, and neutrons in an element using the periodic table? # of PROTONS = ATOMIC NUMBER # of ELECTRONS = ATOMIC NUMBER # of NEUTRONS = ATOMIC _ ATOMIC WEIGHT NUMBER

11. Periodic Table IA IIA ….Groups… IIIA IVA VA VIA VIIA VIIIA Atm # Symbol Wgt Lanthanides Actinides 1 H 1.01 B Groups

12. Periodic Table Groups I: Group 1 is also called the alkali metal group. These are strong metals that are unusually soft and very reactive toward Oxygen forming Oxides and water forming hydroxides of the metal. II: Group 2 is called the alkaline earth metals. These metals are not as soft as Group 1 metals. They also react more mildly with Oxygen to produce oxides of the metals and only react with water at temperatures where the water is steam. Groups 3-12 are referred to as the transition metal groups. These metals are not as predictable

13. Periodic Table Groups 3B- are referred to as the transition metal groups. These metals are not as predictable because of the shielding effect of the inner electrons. As for the " shielding effect " this refers to the inner electrons found in the transition state elements and the inner transition (rare earth)elements. These electrons had a tendency to block the electrical effect of the positive nucleus upon the outer valence electrons of those atoms . This shielding effect helps to partially explain the erratic placement of the electrons in the d and f orbitals relative to the s and p orbitals. Groups 1A-2A and 3A-8A are referred to as the representative elements Group 7A is referred to as the halogen group Group 8A is referred to as the Noble gas group previously known as the inert gas group.

14. Periodic Table The metals which tend to have their atoms losing electrons during a chemical change are roughly found to the left Group 3 Non-metals which tend to have their atoms gaining electrons during chemical change are roughly found in Group 6A-7A with some elements in the lower parts of Groups 5A. Metalloids which tend to have their atoms sometimes losing and sometimes gaining electrons during chemical change are generally found in Groups 4A-6A The Noble gases really belong to their own category since their atoms tend neither to lose or gain electrons. There are only a handful of compounds involving the Noble Gases (mostly involving Xenon).

15. Periodic Table Properties As you proceed to the left in a period or as you proceed down within a group: The metallic strengths increase (non-metallic strengths decrease). The atomic radius of atoms (distance from the nucleus to the outermost occupied region) increases. Atomic radii are the distance between the outermost occupied probability region of an atom and its nucleus. The ionization potential (energy required to remove an electron from an atom) decreases. Ionization Potential is energy required to remove electron from atom. The electron affinity (energy released as electron is picked up by an atom) decreases . The electronegativity (the electron attracting ability of an atom) decreases .

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17. Elements, Compounds, and Mixtures

18. What is an ELEMENT? A substance composed of a single kind of atom. Cannot be broken down into another substance by chemical or physical means.

19. What is a COMPOUND? A substance in which two or more different elements are CHEMICALLY bonded together.

20. What is a MIXTURE? Two or more substances that are mixed together but are NOT chemically bonded.

21. Element, Compound or Mixture?

22. Element, Compound or Mixture?

23. Element, Compound or Mixture?

24. Element, Compound or Mixture?

25. Element, Compound or Mixture?

26. Element, Compound or Mixture?

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