Physical Science 115 1 AtomsThe Building Block of Matter The atom is the fundamental building block of matter 2 History of Atomic Structure Democritus ancient Greek philosopherfirst proposed idea of atoms ID: 422132
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Slide1
Introduction to the Atom and the Periodic Table
Physical Science 115
1Slide2
Atoms—The Building Block of Matter
The atom is the fundamental
building block of matter.
2Slide3
History of Atomic Structure
Democritus (ancient Greek philosopher)-first proposed idea of atoms
3Slide4
The Periodic Table
4Slide5
Atoms are small.
There are as many atoms of air in your lungs at any moment as there are breaths of air in the Earth’s atmosphere.
There are more atoms in a thimble full of water than there are thimbles of water in the ocean.
There are more atoms in a single apple than there are apples that can fit inside the earth.
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Atoms are too small to see
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Subatomic Particles
The proton is about 2000 times more massive than an electron.
The neutron is about 2000 times more massive than an electron.
Nucleons are protons and neutrons.
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Examples of Conceptual Modes
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Rutherford’s Model
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Bohr’s Model
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Evolution of the Atomic Model
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The Nucleus & The Electron Cloud
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Probability Cloud
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Electron Cloud Model
James Chadwick(1932) Discovered the Neutron
The nucleus is kept together by the strong force. (A force that overcomes the electric force.)
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The Periodic Table
Lists all known elements
Atomic Symbol
Atomic Number
Atomic Masses
Much more:
Structure of the elements and how they behave.
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Atomic Radius
The atomic radius
r
is usually determined from the distances between atoms in covalent bonds.
How big is an atom?
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Periodicity 1
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Atomic Size
Atomic size is a periodic (repeating) property.
Size decreases
→
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Ionization Energy vs. Atomic Number
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Electronegativity
The ability to attract more electrons than it has.
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The Periodic Table
These two subsets have properties unlike the transition metals.
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Groups and Periods
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Traditional Names of Families
Alkali Metals
Alkaline-Earth Metals
Transition Metals
No
Common
Names
Halogens
Nobel Gases
Inner Transition Metals
28Slide29
Predicting Ion Charges
Count the valence electrons, add or subtract electrons (whichever is the smaller number) to achieve a full valence level.
1+
2+
3-
2-
1-
n/a
Note that metals tend to lose electrons (become positive)
While
nonmentals
gain electrons (become negative)!
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In terms of protons and electrons, what does it mean for an atom to be electrically neutral?
Atomic Number
The number of protons each atom of an element contains.
34Slide35
Mass Number
Total number of protons and neutrons
35Slide36
Isotopes
Isotope
Atoms of the same element that contain different numbers of neutrons
36Slide37
Isotopic Notation
Mass Number
Atomic Number
Charge
37Slide38
Other Notations
Calcium-40
There are two different notations that mean the same thing.
What is the atomic number?
What is the mass number?
38Slide39
Problem Solving
If you are given the isotopic notation and you need to find the number of protons, neutrons or electrons, do the following:
To find the number of
protons:
To find the number of
neutrons:
To find the number of
electrons:
39Slide40
Examples: For each of the following. What is the atomic number, mass number, number of protons, number of neutrons, and number of electrons?
1) 2) 3)
Examples
40Slide41
Atomic Mass
The average atomic mass of its various isotopes
41Slide42
The Study of Spectra.
Every atom can only emit or absorb certain energies or wavelengths.
42Slide43
Color Separation
43Slide44
Some Emission Spectra
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Example
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Three Possible Energy Transitions
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The Electromagnetic Spectrumm
Color, or frequency, is related to energy.
48Slide49
The Shell Model
49Slide50
Draw a Bohr diagram for Carbon-14
6 p
8 n
50Slide51
Draw a Bohr diagram for Oxygen-15
8 p
7 n
51Slide52
The periodic table and the shell model.
Elements in the same period have electrons in the same shells.
Elements in the same period differ from one another by the number of electrons in the outermost shell.
52Slide53
Each box represents an orbital.
Each electron is represented by an arrow.
Orbitals of similar energy are partitioned together and referred to as a “shell” of orbitals.