Physical Science Chapter 4 Atomic Structure 4 1
![Physical Science Chapter 4 Atomic Structure Physical Science Chapter 4 Atomic Structure](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-1.jpg)
![4. 1 Studying Atoms � Democritus and Aristotle ◦ Democritus thought all matter consisted 4. 1 Studying Atoms � Democritus and Aristotle ◦ Democritus thought all matter consisted](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-2.jpg)
![Dalton’s Atomic Theory � Developed a theory to explain why the elements in a Dalton’s Atomic Theory � Developed a theory to explain why the elements in a](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-3.jpg)
![Thomson’s Model � Used a cathode ray tube to show evidence for subatomic, charged Thomson’s Model � Used a cathode ray tube to show evidence for subatomic, charged](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-4.jpg)
![Thomson continued � Plum pudding model (chocolate chip ice cream. � Negatively charged particles Thomson continued � Plum pudding model (chocolate chip ice cream. � Negatively charged particles](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-5.jpg)
![Rutherford’s Atomic Theory � The Gold Foil Experiment – Evidence for a nucleus. Rutherford’s Atomic Theory � The Gold Foil Experiment – Evidence for a nucleus.](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-6.jpg)
![Chapter 4 Lesson 2 “Structure of the Atom” Chapter 4 Lesson 2 “Structure of the Atom”](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-7.jpg)
![I. Subatomic Particles A. An atom 1. smallest part of matter 2. Ripping paper I. Subatomic Particles A. An atom 1. smallest part of matter 2. Ripping paper](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-8.jpg)
![b. Neutrons (N) – non-charged particle found in the nucleus. -has a mass of b. Neutrons (N) – non-charged particle found in the nucleus. -has a mass of](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-9.jpg)
![Neutrons Protons Electrons Neutrons Protons Electrons](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-10.jpg)
![Particles in an Atom Review Particle Mass Charge Location of particle Proton 1 1+ Particles in an Atom Review Particle Mass Charge Location of particle Proton 1 1+](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-11.jpg)
![II. Atomic Number A. Def – the # of protons in an atom’s nucleus. II. Atomic Number A. Def – the # of protons in an atom’s nucleus.](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-12.jpg)
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![III. Mass Number A. Def – The sum of protons and neutrons in the III. Mass Number A. Def – The sum of protons and neutrons in the](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-14.jpg)
![3. Mass # = Protons + Neutrons 4. How many Neutrons on average are 3. Mass # = Protons + Neutrons 4. How many Neutrons on average are](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-15.jpg)
![IV. Isotope A. Def – An atom that has a different number of neutrons. IV. Isotope A. Def – An atom that has a different number of neutrons.](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-16.jpg)
![4. How many neutrons do the following isotopes have? Oxygen-14 6 Titanium-50 28 Magnesium-22 4. How many neutrons do the following isotopes have? Oxygen-14 6 Titanium-50 28 Magnesium-22](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-17.jpg)
![III. Average Atomic Mass A. Def – average mass of all isotopes of one III. Average Atomic Mass A. Def – average mass of all isotopes of one](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-18.jpg)
![Chapter 4 Lesson 3 “Modern Atomic Theory” Chemistry Timeline…pg. 114 -115 Chapter 4 Lesson 3 “Modern Atomic Theory” Chemistry Timeline…pg. 114 -115](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-19.jpg)
![I. Bohr’s Model / Energy Levels A. Def – a specific area where an I. Bohr’s Model / Energy Levels A. Def – a specific area where an](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-20.jpg)
![Electrons in Energy Levels Energy Level Maximum # of Electrons 1 2 2 8 Electrons in Energy Levels Energy Level Maximum # of Electrons 1 2 2 8](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-21.jpg)
![In Class Assignment 1. Draw a picture of the following atoms with the correct In Class Assignment 1. Draw a picture of the following atoms with the correct](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-22.jpg)
![](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-23.jpg)
- Slides: 23
![Physical Science Chapter 4 Atomic Structure Physical Science Chapter 4 Atomic Structure](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-1.jpg)
Physical Science Chapter 4 Atomic Structure
![4 1 Studying Atoms Democritus and Aristotle Democritus thought all matter consisted 4. 1 Studying Atoms � Democritus and Aristotle ◦ Democritus thought all matter consisted](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-2.jpg)
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.
![Daltons Atomic Theory Developed a theory to explain why the elements in a Dalton’s Atomic Theory � Developed a theory to explain why the elements in a](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-3.jpg)
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.
![Thomsons Model Used a cathode ray tube to show evidence for subatomic charged Thomson’s Model � Used a cathode ray tube to show evidence for subatomic, charged](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-4.jpg)
Thomson’s Model � Used a cathode ray tube to show evidence for subatomic, charged particles.
![Thomson continued Plum pudding model chocolate chip ice cream Negatively charged particles Thomson continued � Plum pudding model (chocolate chip ice cream. � Negatively charged particles](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-5.jpg)
Thomson continued � Plum pudding model (chocolate chip ice cream. � Negatively charged particles evenly spaced throughout a solid mass of positive charge.
![Rutherfords Atomic Theory The Gold Foil Experiment Evidence for a nucleus Rutherford’s Atomic Theory � The Gold Foil Experiment – Evidence for a nucleus.](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-6.jpg)
Rutherford’s Atomic Theory � The Gold Foil Experiment – Evidence for a nucleus.
![Chapter 4 Lesson 2 Structure of the Atom Chapter 4 Lesson 2 “Structure of the Atom”](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-7.jpg)
Chapter 4 Lesson 2 “Structure of the Atom”
![I Subatomic Particles A An atom 1 smallest part of matter 2 Ripping paper I. Subatomic Particles A. An atom 1. smallest part of matter 2. Ripping paper](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-8.jpg)
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+
![b Neutrons N noncharged particle found in the nucleus has a mass of b. Neutrons (N) – non-charged particle found in the nucleus. -has a mass of](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-9.jpg)
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
![Neutrons Protons Electrons Neutrons Protons Electrons](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-10.jpg)
Neutrons Protons Electrons
![Particles in an Atom Review Particle Mass Charge Location of particle Proton 1 1 Particles in an Atom Review Particle Mass Charge Location of particle Proton 1 1+](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-11.jpg)
Particles in an Atom Review Particle Mass Charge Location of particle Proton 1 1+ nucleus Neutron 1 0 nucleus Electron 0 1 - Electron cloud
![II Atomic Number A Def the of protons in an atoms nucleus II. Atomic Number A. Def – the # of protons in an atom’s nucleus.](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-12.jpg)
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*
![](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-13.jpg)
![III Mass Number A Def The sum of protons and neutrons in the III. Mass Number A. Def – The sum of protons and neutrons in the](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-14.jpg)
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 12 Oxygen 16 Iron 56 Calcium 40 Sodium 23 Zinc 65
![3 Mass Protons Neutrons 4 How many Neutrons on average are 3. Mass # = Protons + Neutrons 4. How many Neutrons on average are](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-15.jpg)
3. Mass # = Protons + Neutrons 4. How many Neutrons on average are found in the following elements? Boron 6 Fluorine 10 Silicon 14 Copper 35 Silver 61 Gold 118
![IV Isotope A Def An atom that has a different number of neutrons IV. Isotope A. Def – An atom that has a different number of neutrons.](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-16.jpg)
IV. Isotope A. Def – An atom that has a different number of neutrons. 1. Does not affect the element This means 2. Only changes the weight of the element the mass # 3. Ex: Boron-10 and Boron-11 5 protons ppppp nnnnn 5 neutrons Boron-10 ppppp nnnnn n Boron-11 6 neutrons
![4 How many neutrons do the following isotopes have Oxygen14 6 Titanium50 28 Magnesium22 4. How many neutrons do the following isotopes have? Oxygen-14 6 Titanium-50 28 Magnesium-22](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-17.jpg)
4. How many neutrons do the following isotopes have? Oxygen-14 6 Titanium-50 28 Magnesium-22 10 Potassium-43 24 Aluminum-23 10 Iodine-130 77
![III Average Atomic Mass A Def average mass of all isotopes of one III. Average Atomic Mass A. Def – average mass of all isotopes of one](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-18.jpg)
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%. ”
![Chapter 4 Lesson 3 Modern Atomic Theory Chemistry Timelinepg 114 115 Chapter 4 Lesson 3 “Modern Atomic Theory” Chemistry Timeline…pg. 114 -115](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-19.jpg)
Chapter 4 Lesson 3 “Modern Atomic Theory” Chemistry Timeline…pg. 114 -115
![I Bohrs Model Energy Levels A Def a specific area where an I. Bohr’s Model / Energy Levels A. Def – a specific area where an](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-20.jpg)
I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. e- e- ee- e- 18 electrons eeeeee e- eee- eeee ee- eeee- e e 32 electrons e e 8 electrons eeeee- e- eeeenucleus ee- e 2 electrons
![Electrons in Energy Levels Energy Level Maximum of Electrons 1 2 2 8 Electrons in Energy Levels Energy Level Maximum # of Electrons 1 2 2 8](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-21.jpg)
Electrons in Energy Levels Energy Level Maximum # of Electrons 1 2 2 8 3 18 4 32
![In Class Assignment 1 Draw a picture of the following atoms with the correct In Class Assignment 1. Draw a picture of the following atoms with the correct](https://slidetodoc.com/presentation_image_h/0bdebdf36905281395060e6e2639598d/image-22.jpg)
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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