Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.
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Transcript of Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.
![Page 1: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/1.jpg)
Atoms, Ions and the Periodic Table
Chemistry 131Chapter 2
![Page 2: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/2.jpg)
Dalton’s Atomic Theory
Structure of the Atom
Atomic Mass
Periodic Table
Ions
![Page 3: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/3.jpg)
Dalton’s Atomic Theory
![Page 4: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/4.jpg)
Two Key Ideas led to Atomic Theory
![Page 5: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/5.jpg)
Law of Conservation of Mass
1787 - Lavoisier
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Law of Definite Proportions
1804 - Proust
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Dalton’s Atomic TheoryPublished in 1808 with Four Postulates
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All matter is composed of exceedingly small, invisible particles called Atoms.
![Page 9: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/9.jpg)
Atoms of an element have a given mass and properties, atoms of differing elements differ in mass and properties.
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Atoms are not created or destroyed in a chemical reaction.
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Atoms combine is simple, fixed, whole-number ratios to form compounds
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Structure of the Atom
![Page 13: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/13.jpg)
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Dalton perceived Atoms as the smallest unit of matter.
![Page 15: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/15.jpg)
Thomson’s discovery of the electron posited a different model.
Positive Charge
Negative ChargeElectron
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Rutherford’s Gold Foil experiments led to yet another revision
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The Nuclear Model of the Atom
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Even atoms have sub-structure.
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Hydrogen
![Page 20: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/20.jpg)
ProtonMass = 1.6726×10-24
g Charge = +1.6022×10-19 C
![Page 21: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/21.jpg)
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NeutronMass = 1.6749×10-24 gCharge = 0
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ElectronMass = 9.1094×10-28
gCharge = -1.6022×10-19 C
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Atomic Number = Number of protons
Mass Number= # Protons + # Neutrons
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Hydrogen
Also Hydrogen
Isotopes
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Ions
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Number of Electrons = Number of Protons, if the atom is neutral.
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Li +1Ions
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Atomic Mass
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1.6749×10-24 g isn’t a lot
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Atomic Mass Unit (amu)
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1 amu = 1/12 the mass of 1 Carbon-12 atom
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All atomic masses are therefore relative to Carbon-12
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The atomic masses on the periodic table are relative atomic masses
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Relative Atomic Mass=(Isotope 1 mass × Abundance 1) + (Isotope 2 mass × Abundance 2)+…
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Example (Silver)107Ag 106.9051 amu is 51.82%109Ag 108.9048 amu is 48.18%
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106.9051 amu × 0.5182 = 55.40 amu108.9048 amu × 0.4818 = 52.47 amu55.40 amu+52.47 amu =107.87 amu
![Page 41: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/41.jpg)
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Problem
Given the following information, calculate the relative atomic mass of Magnesium.
24Mg = 23.985 amu at 20.00%25Mg = 24.985 amu at 20.00%26Mg = 25.983 amu at 60.00%
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Problem
The copper mined on Earth consist of 63Cu (62.93 amu) and 65Cu (64.93 amu). Which isotope is more abundant? Why?
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Periodic Table
![Page 45: Atoms, Ions and the Periodic Table Chemistry 131 Chapter 2.](https://reader033.fdocuments.us/reader033/viewer/2022051214/56649d975503460f94a804b4/html5/thumbnails/45.jpg)
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Review Problems
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Review Problem 1How many carbon atoms are present in each sample?(a)120 amu(b)12,000 amu(c)7.22 × 1024 amu
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Review Problem 2
During a typical physical exam blood tests measure the cholesterol level. A high result is anything over 240.0 mg/dL. What is this in pounds/fluid ounce? If a typical human has 5.000 L of blood, how many pounds of cholesterol are present in the blood of a patient with a total cholesterol of 260.0 mg/dL?