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Atomic Structure
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Atomic Structure
• As we said……• Atoms are made up of Protons (P+),
Neutrons(N0) and Electrons (E-)
Charge(e) Relative Mass LocationProtons 1 1 In NucleusNeutrons 0 1 In NucleusElectrons -1 0.0005 Outside Nucleus
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History of the atom
• The Rutherford Experiment.
Alpha Particles
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The Elements
• Another Definition:
• Element– A substance made of atoms which all contain
the same number of protons (P+).
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It’s all about electrons
• The number of electrons in an atom is the same as the number of protons.
• Electrons are arranged in orbits around the nucleus.
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It’s all about electrons
• Electron Configuration– The arrangement of electrons in an atom
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It’s all about electrons
• Each orbit can only hold a certain number of electrons.– The first orbit can hold only 2 electrons.
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It’s all about electrons
• Each orbit can only hold a certain number of electrons.– The second orbit can hold 8 electrons.
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It’s all about electrons
• Each orbit can only hold a certain number of electrons.– The third orbit can hold 18 electrons.
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It’s all about electrons
• I am not going to keep drawing dots!
1 2
2 8
3 18
4 32
5 50
6 72
Shell Electrons
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The Periodic Table
You should have one like this………
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The Periodic Table
• On the periodic table, elements are arranged in groups and periods– Groups are arranged vertically– Periods are horizontal.
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The Periodic TableLet’s look at group 1
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The Periodic Table
• In group 1, all the elements have just one electron in their outer orbit. Even Hydrogen although for this discussion I have removed it.– Elements with similar arrangements of
electrons in their outer orbit behave in a similar way
– Hydrogen is sort of its own group
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The Periodic Table
• Since all the elements in group 1 have only one electron in their outer orbit they all have similar properties. They are all reactive metals.
• They are often called Alkali Metals
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The Periodic Table
Now let’s look at group 7 or 17
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The Periodic Table
• In group 7 (17), all the elements have seven electrons in their outer orbit.
• Group 7 (17) elements all behave in very similar ways.
• They are called the halogens
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The Periodic Table
OK, now group 0 ( or 18)
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The Periodic Table
• In the last group, the elements all have 8 electrons in the outer orbits. These elements are very unreactive.
• Also called Noble Gases
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The Periodic Table
• Start by drawing this……
Fe26
55.85Iron
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The Periodic Table
• Element Name and Symbol– In this case. Fe is the symbol for the element
Iron
Fe26
55.85Iron
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The Periodic Table
• Atomic Number– The number of protons an atom contains.
Fe26
55.85Iron
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The Periodic Table
• Mass Number– The total number of protons and neutrons
Fe26
55.85Iron
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Ionic Bonding
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Ionic Bonding
• As we have said, electron and their orbits are very important to the behavior of an atom.
• For example………
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Ionic Bonding
• Sodium2 Electrons in
Orbit
8 Electrons in Orbit
1 Stupid and Annoying
Electron in Orbit
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Ionic Bonding
That one Stupid and annoying Electron in its outer orbit makes sodium unstable and reactive.
1 Stupid and Annoying
Electron in Orbit
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Ionic Bonding
Sodium (Na) really wants to shed the electron so that it has a full outer orbit. When Na does shed the electron, Na has one more proton than electrons so it has a net positive charge…
escaping electron
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Ionic Bonding
When Na looses its outer electron it becomes and ion.
Ion – An atom with an overall electrical charge
10 electrons +
11 protons =
Positive Ion
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Ionic Bonding
In this case, we have more protons than electrons so the net charge is positive, so it is called…..
Cation – An ion with a positive charge 10 electrons +
11 protons =
Positive Ion
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Ionic Bonding
• Now let’s look at the other form of ion. For example…..
• Chlorine (Cl)
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Ionic Bonding
• Chlorine (Cl)2 Electrons in
Orbit
8 Electrons in Orbit
7 Stupid and Annoying Electrons
in Orbit
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Ionic Bonding
Chlorine (Cl) really wants to gain an electron so that it has a full outer orbit. When Cl does gain an electron, Cl has one fewer protons than electrons so it has a net negative charge…
joining electron
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Ionic Bonding
In this case, we have less protons than electrons so the net charge is negative, so it is called…..
Anion – An ion with a Negative charge 18 electrons +
17 protons =
Negative Ion
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Ionic Bonding
• When the electron jumps from the Na to the Cl, the atoms become Ions. One is cation the other a anion. These two charged atoms then stick together forming a compound.
• Compound – A substance which is made of two or more
kinds of atoms or ions that have joined together.
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Ionic Bonding
• In the case of our Na+ and Cl-, the attraction between positive and negative ions is very strong. It is called an Ionic Bond.
• Ionic Bond – A chemical link between two atoms caused by
the electrostatic force between oppositely-charged ions in an ionic compound.
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Ionic Bonding
• Electrostatic Force– The forces between particles that are caused by
their electric charges.• Na+ is a positive ion….cation
• Cl- is a negative ion…anion
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Ionic Bonding
• When Na+ and Cl- get close to each other they arrange themselves into a pattern called a lattice
• Lattice – Organized arrangement of ions
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Ionic Bonding
• Lattice
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Covalent Bonds
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Covalent Bonds
• We already talked about how compounds form when electrons jump from atom to atom creating positive and negative ions. But is there another way??
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Covalent Bonds
• Let’s look at the compound….BrCl
• Hmmm….how can this be???
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Covalent Bonds
• Both Cl and Br have seven outer electons….hmmm
• If both the Cl and the Br pick up one electron they will both become anions…..will that work?
• Can two ions of the same charge stick to each other?
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Covalent Bonds
• There is another way…….They can Share.
• Awww ain’t that special
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Covalent Bonds
• Let’s look at Hydrogen (H).
• Hydrogen (H) can not exist in nature as only H….it is too reactive. In its simplest state it is found as H2
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Covalent Bonds
• H2 does not lose electrons it shares electrons like this.
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Covalent Bonds
• H2 does not lose electrons it shares them like this.
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Covalent Bonds
• H2 does not lose electrons it shares them like this.
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Matter
• The Kinetic Theory– Atoms are always in motion.– The amount of motion dictates matters state
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The Three States of Matter
• Solid– Particles are fixed in position but still vibrate– A solid is poorly compressed and changes
volume only slightly.– Particles can not move past each other.
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The Three States of Matter
• Liquid– Particles will flow and take the shape of any
container.– A liquid is poorly compressed and changes
volume only slightly.– Particles are free to move around each other.
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The Three States of Matter
• Gas– Particles will flow and take the shape of any
container.– Volume of a gas is dependent of the size of the
contained and is easily compressed.– Particles are free to move around each other.
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The Kinetic Theory……more proof
• Diffusion– The movement of particles form high
concentration to low concentration.
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More Kinetic Theory
• Kinetic energy -the energy of motion
• Heating a solid causes its particles to vibrate faster, thus kinetic energy increases.
• As kinetic energy increases, particles break away from each other and move more freely. Eventually if the particles of a solid have enough kinetic energy, the solid melts.
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More Kinetic Theory
• If you continue to heat, kinetic energy increases even more and the particles move away from each other and the substance turns to gas.
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More Kinetic Theory
Solid Liquid Gas
Kinetic Energy
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Cheaters
• Sublimation – Changing directly from solid to gas.
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More Kinetic Theory
Solid
Liquid
Gas
The Temperature does not change during:
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Energy required to change phasefor water.
-75
-50
-25
0
25
50
75
100
125
150
175
0 oC
0 oC
100 oC
100 oC
These can go on forever
These can go on forever
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Energy required to change phasefor water.
-75
-50
-25
0
25
50
75
100
125
150
175
This requires 0.50 cal/g-degC
This requires 80.0 cal/g
This requires 1.00 cal/g-degC
This requires 540.0 cal/g
This requires 0.48 cal/g-degC