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Understanding Atomic Theory and the Composition of Matter

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tanya-jimenez
17 diapositives · 309 Views · Nov 20, 2014

The atomic theory posits that all matter is constituted of tiny particles known as atoms. Atoms are the smallest units of elements, maintaining the properties of those elements. Essential components of atoms include protons, neutrons, and electrons. The atomic number reflects the number of protons, while atomic mass helps to find neutron count. Elements are categorized into metals, non-metals, metalloids, halogens, and noble gases based on their properties and positions on the periodic table. Each group's electron configurations dictate their reactivity and stability.

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  1. ATOMIC THEORY of MATTER The Atomic Theory states that all matter is made up of tiny particles called Atoms.

  2. Definitions • Atoms- the smallest particle of an element with all of the properties of that element. • Element- a part of a substance not able to be separated into smaller substances by chemical means. • Nucleus- the center of an atom that accounts for most of the atom’s mass.

  3. Sub- Atomic Particles • Protons (+) – positively charged particles found in the nucleus of an atom. • Neutrons (o) – neutrally charged particles found in the nucleus of an atom. • Electrons (-) – negatively charged particles that revolve around the nucleus of an atom. Symbol for electrons (e-).

  4. Rules for AtomicConfigurations using the PERIODIC TABLE • The Atomic Number is equal to the number of Protons in the nucleus of an atom. • The number of Protons is equal to the number of Electrons. • To find the number of Neutrons, you must subtract the Atomic Number from the Atomic Mass.

  5. Rules (Continued) 4) The Period is equal to the number of Electron Shells for an atom. 5) The Group Number is equal to the number of electrons in the outer shell (Valence shell). 6) Use the correct number of Electrons pershell to do Atomic Configurations (see Max # e-/shell chart).

  6. Maximum Number of Electrons/Shell Chart Shell NumberMaximum Number of e- 1 2 2 8 3 8 or 18 4 8, 18 or 32 5 8 or 18 6 8 7 Whatever is needed!

  7. Match the Names of the Elements with the Elemental Symbols 1. H 2. Li 3. Be. 4. Na 5. Mg 6. K 7. Ca 8. Ti 9. Cr 10. Mn 11. Fe 12. Co 13. Ni 14. Cu 15. Zn 16. He 17. B 18. C 19. N 20. O 21. F 22. Ne 23. Al 24. Si 25. P 26. S 27. Cl 28. Ar 29. As 30. Rb 31. Zr 32. Ag 33. Sn 34. Br 35. Kr 36. Sb 37. I 38. Xe 39. Cs. 40. Ba 41. W 42. Pt 43. Au 44. Hg 45. Pb 46. Rn 47. Fr 48. Ra

  8. Elemental Classification • Elements are classified as Metals, Non-metals, Metalloids, Halogens or Noble Gases depending on where they are located on the Periodic Table.

  9. METALS • These make up the majority of the Periodic Table and are located on the LEFT side. Most are solids at room temperature. They are hard, have luster (shine), conduct heat and electricity. They usually will give up an e- because they only have a few in the outer shell.

  10. NON-METALS • These are found on the right side of the Periodic Table and are gases or dull, brittle solids at room temperature. Non-metals tend to gain electrons in order to fill their outermost shell.

  11. METALLOIDS • Elements that are found diagonally between the Metals and Non-metals are called METALLOIDS. They have the properties of metals and non-metals and are used in computer chip applications. Some act naturally as semi-conductor material to conduct electricity at high temperatures.

  12. HALOGENS • A series of non-metal elements in Group 17 which is the only group to contain elements in all three (3) familiar states of matter. The elements are Fluorine, Chlorine, Bromine, Iodine, and Astatine.

  13. NOBLE GASES • Rare gases to the far right on the Periodic Table that are non-reactive (INERT) with other elements. These elements are in Group VIII B or Group 18.

  14. Chemical Reactivity • This refers to the ability to lose or gain electrons. FAMILY REACTIVITY- when removing an electron this is IONIZATION, when gaining an electron this is electron affinity.

  15. Family Reactivity • Group IA (Alkali Metals)- only have to give up one electron to be stable, very reactive. +1 Charge. • Group IIA (Alkaline Earth Metals)- a little less reactive, but will give up 2 e- to have a +2 charge. • Group VIA- has to gain 2e- to become stable, so it has a -2 charge. • Group VIIB (Halogens)- will pick up 1e- to be stable so it will have a -1 charge. The most reactive non-metal elements.

  16. RULES of EIGHT (8) • It takes eight e- in the outer shell for an element to become STABLE. • IONS – when an element loses or gains an electron. • CATION – Positive Ions, positively charged element. • ANION – Negative Ion, negatively charged element.

  17. Periodic Table and the 4 Blocks GROUPS 1& 2 fill the S-block. GROUPS 13 – 18 fill the P-block. GROUPS 3 – 12 fill the D-block. F-block is at the bottom of the Periodic Table. Lanthanide #58-71 and Actinide (radioactive) # 90-103.