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Physical Science Chapter 4

Physical Science Chapter 4. Atomic Structure. 4.1 Studying Atoms. Democritus and Aristotle Democritus thought all matter consisted of extremely tiny particles that could not be divided. (Cut aluminum foil in half)

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Physical Science Chapter 4

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  1. Physical Science Chapter 4 Atomic Structure

  2. 4.1 Studying Atoms • Democritus and Aristotle • Democritus thought all matter consisted of extremely tiny particles that could not be divided. (Cut aluminum foil in half) • Also thought matter in liquids was round and smooth; in solids rough and prickly • Aristotle thought there was no limit to the number of times matter could be divided.

  3. Dalton’s Atomic Theory • Developed a theory to explain why the elements in a compound always behave in the same way. • Main Points • 1) All elements are composed of atoms. • 2) All atoms of the same element have the same mass, and atoms of different elements have different masses. • 3) Compounds contain atoms of more than one element. • 4) In a compound, atoms of different elements always combine in the same way.

  4. Thomson’s Model • Used a cathode ray tube to show evidence for subatomic, charged particles.

  5. Thomson continued • Plum pudding model (chocolate chip ice cream. • Negatively charged particles evenly spaced throughout a solid mass of positive charge.

  6. Rutherford’s Atomic Theory • The Gold Foil Experiment – Evidence for a nucleus.

  7. Chapter 4Lesson 2 “Structure of the Atom”

  8. I. Subatomic Particles A. An atom 1. smallest part of matter 2. Ripping paper example B. Areas of an atom 1. Nucleus – center of an atom -holds protons and neutrons a. Protons (P) – positively charged particle found in the nucleus. -has a mass of 1 -has a charge of 1+

  9. b. Neutrons (N) – non-charged particle found in the nucleus. -has a mass of 1 -has no charge “0” 2. Electron Cloud – area around the nucleus which contains electrons a. Electrons (e) – negatively charged particle found outside of the nucleus -has a mass of 0 -has a charge of 1- -moves around the outside of the nucleus

  10. Protons Electrons Neutrons

  11. Particles in an Atom Review Proton 1 1+ nucleus Neutron 1 0 nucleus Electron 1- 0 Electron cloud

  12. II. Atomic Number A. Def – the # of protons in an atom’s nucleus. 1. Every carbon atom has 6 protons… 2. Every neon atom has 10 protons… B. On P.T. – located right above the chemical symbol *Protons dictate the type of element we have* *Electrons always equal the # of protons*

  13. III. Mass Number A. Def – The sum of protons and neutrons in the nucleus of an atom. 1. On P.T. – bottom number -round up/down 2. Ex: What is the mass number of the following elements? Carbon Oxygen Iron Calcium Sodium Zinc 12 16 40 56 65 23

  14. 3. Mass # = Protons + Neutrons 4. How many Neutrons on average are found in the following elements? Boron Fluorine Silicon Copper Silver Gold 6 10 35 14 118 61

  15. IV. Isotope A. Def – An atom that has a different number of neutrons. 1. Does not affect the element 2. Only changes the weight of the element 3. Ex: Boron-10 and Boron-11 This means the mass # 5 protons 5 protons p p p p p p p p p p n n n n n n n n n n n Boron-10 Boron-11 5 neutrons 6 neutrons

  16. 4. How many neutrons do the following isotopes have? Oxygen-14 Titanium-50 Magnesium-22 Potassium-43 Aluminum-23 Iodine-130 6 28 10 24 10 77

  17. III. Average Atomic Mass A. Def – average mass of all isotopes of one element combined. 1. Found on P.T. underneath chemical symbol. 2. Ex: Carbon = 12.011 “Carbon has 3 known isotopes. Carbon-12, 13, and 14. Carbon-12 makes up 99% of all carbon on earth. Carbon-13 and 14 make up 1%.”

  18. Chapter 4Lesson 3 “Modern Atomic Theory” Chemistry Timeline…pg. 114-115

  19. I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. e- e- e- e- e- e- e- e- e- 18 electrons e- e- 2 electrons e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- 32 electrons e- e- 8 electrons e- e- e- e- e- e- e- e- e- e- nucleus e- e- e- e- e-

  20. Electrons in Energy Levels 1 2 8 2 3 18 4 32

  21. In Class Assignment 1. Draw a picture of the following atoms with the correct number of e’s, p’s, and n’s… a. Na d. He b. Al e. C c. K f. S 2. Assign: Read pg. 118 and 119 3. What is the difference between a ground state and an excited state?

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