chapter 7dmbillings.weebly.com/uploads/2/6/1/3/26139392/chapter_7.pdf · 2018-09-10 · chapter 7...
TRANSCRIPT
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Chapter 7
Atomic Theory – Inside the Invisible
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7.1 Development of A Modern Atomic Theory
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Dalton’s Theory
○ Dalton envisioned the atom as the smallest piece of any element, as a smooth, solid sphere, without an electrical charge
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Thompson’s Model of the Atom
○ A new model was needed as Michael Faraday discovered atoms contained electric charges
○ Thompson proposed that an atom was mostly positively charged matter, with small negatively charged electrons scattered throughout.
○ Sometimes referred to as the raisin bun model.
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Rutherford’s Gold Foil Experiment
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Rutherford’s Model
○ Most of the mass of the atom and all the positive charge is concentrated in the centre.
○ The nucleus contains protons and neutrons.
○ Electrons are orbiting the nucleus.
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Assignment
○ P. 208 #4-5, 7-10, 12
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7.2 Bohr Model of the Atom
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Bohr Model of the Atom
○ Electrons are restricted to specific “allowed” orbits, or shells around the nucleus.
○ The amount of energy an electron has is related to how far it is from the nucleus.
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○ The periodic law states that the properties of elements are a periodic or regularly repeating function of their atomic number
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○ The atomic number is the number of protons in the nucleus of an atom
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○ The mass number is the total number of protons and neutrons in the nucleus of an atom
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17 protons, 17 electrons, 18 neutrons
Standard Atomic Notation
35Cl17
SymbolMass number
Atomic number
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○ In an atom, the number of electrons equals the number of protons
○ In an ion, the number of electrons does not equal the number of protons. Electrons have been added or removed.
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Assignment
○ Subatomic Particles Worksheet
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7.2 Structure of an Atom
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Subatomic Particles
Particle Charge Mass Location
Proton 1+ 1 Nucleus
Neutron 0 1 Nucleus
Electron 1- 1/1800 Outside nucleus
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○ Ions are charged atoms ○ A positive ion has had electrons
removed. There are more protons than electrons
○ A negative ion has had electrons added. There are more electrons than protons.
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35Cl-17
o Protons
o Neutrons
o Electrons
17
18
18
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24Mg2+
o Protons
o Neutrons
o Electrons
12
12
10
12
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Assignment
○ P. 212 #2, 5, 6-7, 10-11
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7.3 Modern Periodic Table
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○ The atomic mass is the average of all the naturally occurring isotopes
○ Isotopes are atoms with the same atomic number, but different mass number (protons are the same but neutrons are different).
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Assignment
○ P. 217 #1-18
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7.4 Bohr Models
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Drawing Bohr Diagrams
○ Each atom can have 2 electrons in the inner most shell, 8 in the second and 8 in the third
○ Shells are filled in the order of inner to outer
○ Electrons in the outer shell are involved in chemical reactions
○ Electrons in full shells do not take part in chemical reactions
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Assignment
○ Bohr Diagrams Worksheet
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7.4 Formation of Ions
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○ Li+ ion is held to F- ion by electrical forces
○ A molecular compound has two or more atoms joined together. Electrons are shared.
○ Ionic compounds are not made of molecules. Ions are attracted to one another due to their charges. Electrons have been transferred.
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Assignment
○ P. 223 #1, 5, 11-13
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Review Assignment
○ P. 230 #1-5, 7-8, 12, 13 ○ Atoms and Their Electrons Video