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Atoms, Isotopes and Ions…Oh My!SOL Covered:
PS.3, PS.4a & bCH.2 a, b, c, g & i
Aron [email protected]
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Objectives
• Review the history of Atomic Theory
• Emphasize the importance of the Quantum Model
• Build atomic models with appropriate atomic mass and electron configuration
• Build models to represent ionic and covalent bonding
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A Brief History of the Atom
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What is Matter Made of? Aristotle vs. Democritus
(Around 2400 years ago)
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What is Matter Made of? Aristotle vs. Democritus
(Around 2400 years ago)
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John Dalton
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Dalton’s Theory Based on Experimentation!
• chemical elements are made of atoms. • the atoms of an element are identical in
their masses• atoms of different elements have different
masses • atoms only combine in small, whole
number ratios• atoms can be neither created nor
destroyed
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Dalton’s Atomic Model
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J.J. Thomson
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Ernest Rutherford
BOTTOM LINE- The nucleus is dense and positive and the atom is mostly empty space!
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Atoms are Mostly Empty Space
Imagine a raisin on home plate to represent the nucleus
The first electron would be represented by the outfield wall.
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Niels Bohr
• Rutherford quickly realized that his model would cause the electrons to be pulled into the nucleus and destroy the atom
• In 1913, Niels Bohr hypothesized that the electrons were in fixed energy levels at a set distance from the nucleus and that each energy level could hold a certain number of electrons.
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Bohr Model Continued
• Energy levels are sometimes called “shells”
• Each shell can hold a fixed number of electrons
• Electrons are particles but the position and velocity can not be determined at the same time– Heisenberg
Uncertainty Principal
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The Quantum ModelThe “Modern” Model
• In the early 1920’s, and Irwin Schrödinger theorized that the electrons behaved like particles and waves. His model kept electrons energy levels and the energy levels were broken into sub-levels.
• The energy levels aren’t traditional “orbital's” but areas where an electron has a high probability of being found.
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Quantum Orbital's Have Interesting Shapes
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The Quantum Model is also known as The Electron Cloud
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Even though the Quantum/Electron Cloud Model is the most accurate, the Bohr Model
is still used to help students understand atomic structure since it’s simplistic.
Correct- Quantum Model/Electron Cloud
Bohr’s model while not completely accurate, helps students understand energy levels and placement of electrons.
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So what’s the difference between protons, neutrons and electrons?
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Let’s Build Some Models!
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Hydrogen-1
Make an atom for…
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Hydrogen-2
Make an atom for…
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So what’s the difference between…
and
has 1 more neutron
and are _______ of HydrogenISOTOPES
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Helium-4
Make an atom for…
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![Page 27: Atoms, Isotopes and Ions… Oh My! SOL Covered: PS.3, PS.4a & b CH.2 a, b, c, g & i Aron Fristoe afristoe@msinnovation.info](https://reader035.vdocuments.site/reader035/viewer/2022081519/56649e405503460f94b31a3a/html5/thumbnails/27.jpg)
Make an atom for…
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Make an atom for…
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Make an atom for…
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Nitrogen-17
Make an atom for…
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Let’s Take a Break and Play a Game
• Slowly move around the designated area looking down
• When you bump into someone, share your number– The lower number will give 1 bean to the
higher number
• Continue until I call stop
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Now let’s make some Ions…
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Make an atom for…
2-
Atoms with a NEGATIVE net charge are called ANIONS
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2-
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Make an atom for…
1+
Atoms with a POSITVE net charge are called CATIONS
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Ionic BondingChemical Bonds Between Metals and Nonmetals
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Sodium and Chlorine
Na11 electrons
Cl17 electrons
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Sodium and Chlorine
Na1+
10 electrons
Cl1-
18 electrons
Electron from Na
8 electrons in each outer energy level
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Sodium chloride
NaCl
Opposites attract!
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Calcium and Chlorine
Ca ClCalcium has 2 electrons in it’s outer energy level
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Calcium and Chlorine
Ca2+ 2Cl1-
Calcium donates one electron to 2 Chlorine atoms
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Calcium chloride
CaCl2
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Covalent BondingChemical bonds between two or more nonmetals
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Hydrogen and Oxygen
2H O
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Water
H2O
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Water
Each Hydrogen atom has two electrons- the maximum number in the first (and only for Hydrogen) energy level
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Water
The Chlorine atom has 8 electrons in the second energy level which is the maximum number of electrons that the second energy level can hold.
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Ammonia (nitrogen trihydride)NH3
Nitrogen atom
3 Hydrogen atoms
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Ammonia (nitrogen trihydride)NH3
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Ammonia (nitrogen trihydride)NH3
Each Hydrogen has 2 electrons which is the maximum it can hold in it’s outer energy level.
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Ammonia (nitrogen trihydride)NH3
Nitrogen has 8 electrons in it’s outer energy level which is the maximum number of electrons the second energy level can hold.
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Methane (carbon tetrahydride)CH4 For chemistry, you can use this
to talk about sp hybridization (specifically sp3)