History, Theory, Structure. How can we describe something we can’t even see? Compare to Black...
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![Page 1: History, Theory, Structure. How can we describe something we can’t even see? Compare to Black Box Experiment Can’t see internal structure](https://reader036.fdocuments.net/reader036/viewer/2022081603/56649f1b5503460f94c31165/html5/thumbnails/1.jpg)
electron
neutron
proton
AtomsHistory, Theory,
Structure
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What’s In the Box?
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How can we describe something we can’t even see?
Compare to Black Box Experiment Can’t see internal structure Discovery by experimenting with how
matter behaves Constantly changing and/or refining
definition
How Do We Know Atomic Structure?
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Our current understanding of atomic structure is based on:
What is Inside an Atom?
NucleusContains Protons (+) and Neutrons (N)
+N+
Electron Shells (Not exact locations) e-
Drawn as an outer “wall” only for reference; Energy
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Historical Perspective
“Ancient” “Modern”
Aristotle: matter may be continuously divided without changing its intrinsic properties
Democritus:matter is composed of tiny, indivisible particles; atoms may not be divided
Dalton: Atoms may not be further divided.
Thomson: pudding theory; electrons
Rutherford: gold foil Bohr: quantum theory Schrodinger:
charge-cloud
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1808 English Two very important tenets
◦ Law of Conservation of Mass◦ Law of Definite Proportions
Dalton
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All matter is made up of atoms. All atoms of an element are identical in size,
mass, and chemical properties. Atoms of an element are different from atoms
of all other elements. Atoms may neither be divided nor destroyed. Atoms may be combined, separated, and
rearranged to form new compounds. Atoms of different elements combine in
whole-number ratios to form compounds.
Dalton’s Main Points
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Thompson
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1911 Rutherford’s Gold Foil Experiment Actually conducted by Rutherford’s
assistant Hugely advanced for time period
The Nucleus
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Bohr’s model related structure and position of electrons to energy levels
Ground state Excited state Line-emission spectrum Continuous spectrum Only worked consistently for hydrogen
Bohr and Quantum Theory
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Based on Bohr’s ideas with one main difference Electrons are not traveling in fixed positions Use of orbitals rather than orbits Areas where electrons are most likely to be
found For example, an electron will never be expected to be found in the atom’s nucleus
Charge-Cloud
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Protons have a positive charge.◦ Mass of 1 unit◦ Located in nucleus◦ Identity of an atom
Neutrons have no charge◦ Mass of 1 unit◦ Located in nucleus◦ Help to stabilize nucleus
What’s Inside an Atom?
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Located outside of the nucleus◦ Negative charge◦ Mass is insignificant to mass of whole atom◦ Responsible for chemical reactivity of an atom
Though mass is tiny, equal but opposite charge◦ Can change position◦ Relate to energy of an atom
Electrons
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Protons Neutrons
Positive charge
Located in nucleus
Determine properties of an atom
Unique to each element
No charge (neutral)
Located in nucleus
Thought to provide stability to nucleus
Numbers may vary (isotopes)
•Negative charge•Located in energy levels around nucleus•Responsible for chemical reactivity of an atom
Electrons
Sub-Atomic Particles
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All mass measurements are comparisons based on standards
All atoms based on mass of carbon-12 atom Weighted average of all known isotopes
based on measured frequency Combination of protons and neutrons
Atomic Mass
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12.011
C6
Quantifying Atoms
Atomic Mass• represents
combined masses of protons and neutrons
Atomic Number• Represents
number of protons; in a neutral atom represents number of electrons
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While all atoms of an element have the same number of protons, numbers of neutrons may differ
These atoms still retain the basic properties of the element
Small differences in behavior Atoms of the same element with differing
numbers of neutrons Indicated by symbol with number to
indicate number of neutrons or mass
Isotopes
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Mendeleev (1834-1907); Russian; 1880’s◦ listed approximately 73 known elements in
columns in order of increasing atomic mass◦ left blank spaces for unknown elements
Moseley (1887-1915); British; worked w/ Rutherford; 1913◦ determined atomic number of atoms of known
elements◦ arranged elements by atomic number
The Periodic Table of the Elements: History
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Periods◦ Horizontal
◦ 7
◦ Periodic Law
◦ Properties change as you go from left to right on the Periodic Table. Atomic mass increases Atomic number increases
Modern Periodic Table
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Group or Family
Vertical
Similar physical and chemical properties
Significance of Group Number◦ For main group elements represents number of
valence electrons
Modern PT, cont.
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Approximately 80% of known elements
Alkali: Group I◦ Highly reactive
Alkaline Earth: Group 2◦ Highly reactive
Transition, inner transition
Properties◦ malleable, ductile, lustrous◦ solids at room temp except Hg◦ good conductors of heat and electricity
Metals
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Not lustrous
Poor conductors of electricity and heat
Halogens◦ Group 7
Noble gases◦ Group 8
Right side of Periodic Table
Nonmetals
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Zig zag line
Properties of both metals and nonmetals
Used in computer chips and solar cells; semiconductors
Metalliods
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Periodic Table of the Elements
Source: Jefferson Labs
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Historical perspective◦ Models of atoms based on behavior rather than a
visual analysis All atoms of an element have same basic
properties◦ Isotopes
Atoms of same element with differing # of neutrons Identity of an atom based on protons Chemical reactivity of an atom based on
electrons Periodic Table of the Elements
◦ Organization and Patterns
Summary