chapter 18 properties of atoms and the periodic table
TRANSCRIPT
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Chapter 18
Properties of Atoms and the Periodic Table
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Scientific Shorthand
Scientists use abbreviations to write the name of elements.
Abbreviations are easier to write than the whole element.
For example:Carbon is written asAluminum is written asSilver is written as
C
AlAg
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Scientific Shorthand
The first letter in the symbol is ALWAYS written with a capital letter.
If there is a second letter, it is ALWAYS written as a lowercase letter.
Some element symbols are based on their English names, while others are based on their Latin names.Silver is Ag from its Latin name Argentum.
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Atoms
Elements are made of atomsAtoms are the smallest piece of matter
that still retains the properties of the element.
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Subatomic ParticlesEach atom is
made up of smaller particles.
In the center of the atom is the nucleus.
The nucleus is made of protons and neutrons.
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Subatomic ParticlesEach atom is
made up of smaller particles.
Electrons orbit around the nucleus
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Subatomic Particles
Properties of ProtonsElectrical charge of +1Mass =1 amu.
Properties of NeutronsElectrical charge of 0.Mass =1 amu.
Properties of Electrons Electrical charge of -1Mass is approximately 1/1800 of a proton.
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Quarks
Protons, neutrons and electrons are all made up of even smaller particles called quarks.
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Quarks
To study quarks, scientists smash atoms together to break the protons apart.
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Quarks
Based on the data collected, they can reconstruct the structure of the atom.
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The Atomic Model - History
Democritus (400 B.C.)First proposed that
atoms made up all substances.
AristotleBelieved that matter is
uniform throughout.This idea lasted for
about 2,000 years.
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The Atomic Model - History
Dalton’s ModelEach atom was a solid sphere.Allowed scientists to explain how chemical
reactions occurred.Thomson, Rutherford, and Bohr
Each scientist’s experiments helped to identity different parts of the atom and the structure of the atom.
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Atomic Model
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Electron Cloud Model
The most current model of the atom.
The electron cloud is 100,000 times larger than the diameter of the nucleus, but each electron is smaller than the proton.
Electrons are so small, and moving so fast, that they are difficult to find.
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Protons in the nucleus bothrepel and attract each other.The repulsions are due toelectromagnetic force andthe attractions are due to thestrong nuclear force. Thestrong nuclear force onlyacts over very shortdistances, about the size ofan atomic nucleus. Neutronsand protons also attract eachother because of the strongnuclear force.
What holds the Nucleus Together?
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Atomic Masses
Most of the mass of an atom is within the nucleus.Protons and neutrons each weigh about
1.6726 x 10-24 kg.That’s 0.000 000 000 000 000 000 000 001 672 6 kg!Electrons are 1/1800 of the mass of a proton
or neutron.
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Atomic Masses
To measure atomic mass, we use the “atomic mass unit” or amu.Mass of 1 proton = 1 amuMass of 1 neutron = 1 amu
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Atomic Number
The number of protons in an atom identify the element.
Each element has a different number of protons.Atoms with 8 protons are always oxygen.Atoms with 6 protons are always carbon.Atoms with 16 protons are always sulfur.
The number of protons in an atom is called the atomic number.
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Atomic Number Practice
Use your periodic table to find the atomic number of the following elements:Aluminum (Al)Titanium (Ti)Tin (Sn)Osmium (Os)Erbium (Er)
How many protons does each atom have?The number of protons are equal to the
atomic number.
Al = 13Ti = 22Sn = 50Os = 76
Er = 68
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Mass Number
The mass number of an atom is the sum of the number of protons and neutrons in the nucleus.
Element Protons Neutrons Mass Number
Boron 5 6
Carbon 6 6
Oxygen 8 8
Sodium 11 12
Copper 29 34
6+6
8+8
5+6
11+12
29+34
11
12
16
23
63
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Using the Atomic Number & Mass Number
If you know the atomic number and mass number, you can determine the number of neutrons.
Mass Number
- Atomic Number
Number of Neutrons
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Practice
Determine the number of protons and neutrons in the following atoms:Lithium – Atomic Number = 3
Mass Number = 7Argon – Atomic Number = 18
Mass Number = 39Strontium – Atomic Number = 38
Mass Number = 88
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Answers
Determine the number of protons and neutrons in the following atoms:Lithium – Protons = 3
Neutrons = 7 – 3 = 4Argon – Protons = 18
Neutrons = 39 – 18 = 21Strontium – Protons = 38
Neutrons = 88 – 38 = 50
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Isotopes
Atoms of one type of element must have the same number of protons.
However, they can have different numbers of neutrons.
Atoms with the same number of protons and different numbers of neutrons are called isotopes.
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Isotopes
ExamplesCarbon-12 has a mass of 12 amu.
All carbon atoms must have 6 protons.Neutrons = 12 – 6 = 6.C-12 has 6 protons and 6 neutrons.
Carbon-14 has a mass of 14 amu.All carbon atoms must have 6 protons.Neutrons = 14 – 6 = 8.C-14 has 6 protons and 8 neutrons.
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Isotopes
ExamplesUranium-235 has a mass of 235 amu.
All uranium atoms must have 92 protons.Neutrons = 235 – 92 = 143.U-235 has 92 protons and 143 neutrons.
Uranium-238 has a mass of 238 amu.All uranium atoms must have 92 protons.Neutrons = 238 – 92 = 146.U-238 has 92 protons and 146 neutrons.
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Average Atomic Mass
Because atoms can have different numbers of neutrons, the mass numbers can be different.
To get an overall mass of one element, we take the weighted-average of all the isotopes and determine the average atomic mass for the element.
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Neutral Atoms
In the nucleus, which particles have charge?Protons
What charge do they have?Positive
What particle is opposite that charge?Electrons
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Neutral Atoms
To balance the charges in the atom, the number of protons must equal the number of electrons.Li has 3 protons, so the nucleus has a charge
of +3.To balance that charge, there must be 3
electrons that add up to -3.Overall, the charge is (+3) + (-3) = 0, so the
atom is neutral.
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Practice
Determine how many electrons the following atoms have:Magnesium, Protons = 12Beryllium, Protons = 4Nitrogen, Atomic Number = 7Bromine, Atomic Number = 35
12 Electrons
4 Electrons
7 Electrons
35 Electrons
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Practice
Element Symbol Atomic Number
Mass Number
Protons Neutrons Electrons
Iodine I 53 127
Mercury Hg 80 201
Neon 10 20
Mg 12 12 12
Rb 37 48
41 51
75 111
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Practice
Element Symbol Atomic Number
Mass Number
Protons Neutrons Electrons
Iodine I 53 127 53 74 53
Mercury Hg 80 201 80 121 80
Neon Ne 10 20 10 10 10Magnesium Mg 12 24 12 12 12Rubidium Rb 37 85 37 48 37
Niobium Nb 41 92 41 51 41
Rhenium Re 75 186 75 111 75
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Bohr Models of the Atoms
Each atom had orbitals or shells in which the electrons can fit.1st Shell: up to 2 electrons can fit2nd Shell: up to 8 electrons can fit3rd Shell: up to 18 electrons can fit4th Shell: up to 32 electrons can fit
Must start with the smallest/closest orbital or shell first.
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Drawing Bohr Models
HydrogenAN = 1AM = 1e- = 1
BoronAN = 5
AM = 11e- = 5
1 p+, 0 no
5 p+, 6 no
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Drawing Bohr Models
ChlorineAN = 17AM = 35e- = 17
17 p+, 18 no
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Electron Dot Diagrams
1. Write the symbol of the element
2. Determine the number of valence electrons (electrons in the outermost energy level)
3. Start placing valence electrons around the symbol
4. Pair electrons only after all four sides (top, bottom, left, right) have been used once
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Example: Hydrogen
H
Hydrogen has 1 valence electron
Chose one side, and place the electron
H H HOR OR OR
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Example: Chlorine
Cl
Chlorine has 7 valence electrons
Place one on each side first
Then begin to pair the remaining electrons
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Example: Nitrogen
N
Nitrogen has 5 valence electrons
Place one on each side first
Then begin to pair the remaining electrons
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Example: Beryllium
Be
Beryllium has 2 valence electrons
Place each electron on different sides
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Example: Helium
He
Helium has 2 valence electrons
Helium is an EXCEPTION
Pair the two electrons because the energy level can only 2 electrons
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Periodic Law
Scientists Julius Lothar Meyer and Dmitri Mendeleev individually produced classification schemes for elements in 1869.
Periodic Law: When elements are arranged in order of increasing atomic numbers, elements with similar chemical properties will occur at regular (periodic) intervals.
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Periodic Table
The rows on the periodic table are separated into periods.
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As chemists worked on determining which substances were elements, they noticed that some elements acted very much like other elements. For example, one atom of some metals always reacts with two atoms of oxygen. Chemists called these similar elements a group of elements.
Periodic Table
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Periodic Table
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Regions of the Periodic Table
Metals: Elements to the lower left side of the periodic table.
Nonmetals: Elements to the upper right of the periodic table.
Metalloids: Elements in between the metals and nonmetals.
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Metalloids
1
2
3 4 5 6 7 8 9 10 11 12
13 14 15 16 17
18
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Metals
1
2
3 4 5 6 7 8 9 10 11 12
13 14 15 16 17
18Hydrogen is an exception
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Nonmetals
Hydrogen is an exception 1
2
3 4 5 6 7 8 9 10 11 12
13 14 15 16 17
18