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Atoms to Minerals

Atoms to Minerals. Section 3.1: Atomic Structure of Matter. What is matter?. Section 3.1: Atomic Structure of Matter. Matter is anything that has mass and volume. Section 3.1: Atomic Structure of Matter. We can classify matter by using the Periodic Table

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Atoms to Minerals

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  1. Atoms to Minerals

  2. Section 3.1: Atomic Structure of Matter What is matter?

  3. Section 3.1: Atomic Structure of Matter Matter is anything that has mass and volume

  4. Section 3.1: Atomic Structure of Matter We can classify matter by using the Periodic Table 3 Large Groups of elements on the periodic table

  5. Section 3.1: Atomic Structure of Matter 1. Metal: shiny, ductile, conducts electricity 2. Non-metal: dull, does not conduct electricity 3. Metalloid: Shares properties of both metal and non-metal Elements are classified according to their place on the Periodic Table.

  6. 6 C Carbon 12.011 Periodic Table

  7. 6 C Carbon 12.011 Periodic Table Atomic number

  8. 6 C Carbon 12.011 Periodic Table Atomic number Element Symbol

  9. 6 C Carbon 12.011 Periodic Table Atomic number Element Symbol Element Name

  10. 6 C Carbon 12.011 Periodic Table Atomic number Element Symbol Element Name Atomic mass

  11. Section 3.1: Atomic Structure of Matter Structure of the Atom Nucleus: This contains positively charged protons and neutrally charged neutrons. Electrons: These surround the nucleus in an electron cloud and are negatively charged.

  12. Section 3.1: Atomic Structure of Matter Structure of the Atom The atomic number, or identity of the atom, is determined by the number of PROTONS!

  13. The Nature of Matter I. Atom: _____________________________________ A. Subatomic Particles Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  14. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  15. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  16. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  17. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  18. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  19. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  20. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  21. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of ________ and _____. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  22. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of ______and _______. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  23. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of protons and electrons. Atoms that lose electrons have a ________________ charge. Atoms that gain electrons have a ________________ charge.

  24. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of protons and electrons. Atoms that lose electrons have a positive charge. Atoms that gain electrons have a ________________ charge.

  25. The Nature of Matter I. Atom: smallest unit of matter A. Subatomic Particles Most atoms are neutral because they have equal numbers of protons and electrons. Atoms that lose electrons have a positive charge. Atoms that gain electrons have a negative charge.

  26. The Nature of Matter I. Element: ______________________________________ A. atomic number: _____________________________ B. mass number: _____________________________ C. isotope: __________________________________ ______________________________________________ D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________ ___________________________________________

  27. The Nature of Matter I. Element: substance made of one type of atom A. atomic number: _____________________________ B. mass number: _____________________________ C. isotope: __________________________________ ______________________________________________ D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________ ___________________________________________

  28. The Nature of Matter I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: _____________________________ C. isotope: __________________________________ ______________________________________________ D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________ ___________________________________________

  29. The Nature of Matter I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: sum of protons + neutrons in an atom C. isotope: __________________________________ ______________________________________________ D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________ ___________________________________________

  30. The Nature of Matter I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: sum of protons + neutrons in an atom C. isotope: atoms of the same element with different numbers of neutrons D. radioactive isotope: ________________________ ___________________________________________ 1. uses: _________________________________ ___________________________________________

  31. The Nature of Matter I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: sum of protons + neutrons in an atom C. isotope: atoms of the same element with different numbers of neutrons D. radioactive isotope: isotope with an unstable nucleus that breaks down over time (emits radiation) 1. uses: _________________________________ ___________________________________________

  32. The Nature of Matter I. Element: substance made of one type of atom A. atomic number: #protons – defines an element B. mass number: sum of protons + neutrons in an atom C. isotope: atoms of the same element with different numbers of neutrons D. radioactive isotope: isotope with an unstable nucleus that breaks down over time (emits radiation) 1. uses: dating fossils, diagnosing and treating diseases, killing bacteria in food/ on surgical equipment

  33. Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 7 neutrons 6 electrons 6 protons 8 neutrons The Nature of Matter

  34. Section 3.1: Atomic Structure of Matter Structure of the Atom Isotopes are atoms with usually more neutrons than protons. The mass number equals the sum of protons plus neutrons.

  35. Section 3.2: Composition of Minerals Structure of the Atom A compound is a substance with two or more elements. Example is table salt or Sodium Chloride (NaCl)

  36. The Nature of Matter • III. Compound: _________________________________ • ______________________________________________ • IV. Chemical Bonds • valence electrons: _________________________ • ion: ______________________________ • B. ionic bond:___________________________________ • ____________________ • C. covalent bond: _______________________________ • ___________ • molecule: ___________________________________

  37. The Nature of Matter • III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions • IV. Chemical Bonds • valence electrons: _________________________ • ion: ______________________________ • B. ionic bond:___________________________________ • ____________________ • C. covalent bond: _______________________________ • ___________ • molecule: ___________________________________

  38. The Nature of Matter • III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions • IV. Chemical Bonds • valence electrons: outermost electrons in an atom • ion: ______________________________ • B. ionic bond:___________________________________ • ____________________ • C. covalent bond: _______________________________ • ___________ • molecule: ___________________________________

  39. The Nature of Matter • III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions • IV. Chemical Bonds • valence electrons: outermost electrons in an atom • ion: atom that has gained or lost electrons • B. ionic bond:___________________________________ • ____________________ • C. covalent bond: _______________________________ • ___________ • molecule: ___________________________________

  40. The Nature of Matter • III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions • IV. Chemical Bonds • valence electrons: outermost electrons in an atom • ion: atom that has gained or lost electrons • B. ionic bond: bond formed by the transfer of electrons from one atom to another • C. covalent bond: _______________________________ • ___________ • molecule: ___________________________________

  41. The Nature of Matter • III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions • IV. Chemical Bonds • valence electrons: outermost electrons in an atom • ion: atom that has gained or lost electrons • B. ionic bond: bond formed by the transfer of electrons from one atom to another • C. covalent bond: bond formed when atoms share electrons • molecule: ___________________________________

  42. The Nature of Matter • III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions • IV. Chemical Bonds • valence electrons: outermost electrons in an atom • ion: atom that has gained or lost electrons • B. ionic bond: bond formed by the transfer of electrons from one atom to another • C. covalent bond: bond formed when atoms share electrons • molecule: group of atoms covalently bonded together

  43. Sodium atom (Na) Chlorine atom (Cl) Transfer of electron Protons +11 Electrons -11 Charge 0 Protons +17 Electrons -17 Charge 0 The Nature of Matter

  44. Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na+) Chloride ion (Cl-) Transfer of electron Protons +11 Electrons -11 Charge 0 Protons +17 Electrons -17 Charge 0 Protons +11 Electrons -10 Charge +1 Protons +17 Electrons -18 Charge -1 The Nature of Matter

  45. Section 3.2: Composition of Minerals Bonding of Atoms Ions are formed when the number of electrons is either more or less than the number of protons.

  46. Section 3.2: Composition of Minerals Bonding of Atoms A covalent bond is when two atoms share electrons. A molecule is formed by covalent bonding of two or more atoms.

  47. Section 3.2: Composition of Minerals Bonding of Atoms An ionic bond is when atoms are held together by electrical attraction.

  48. Section 3.2: Composition of Minerals What is a mineral?

  49. Section 3.2: Composition of Minerals It occurs naturally. It is solid. It has a chemical composition. It’s atoms are arranged in an orderly pattern (crystal structure). It is inorganic (not alive).

  50. Section 3.2: Composition of Minerals How do minerals form?

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