Transcript Atomic Structure and the Periodic Table

Atomic Structure and the Periodic
Table
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All Matter is Made of Atoms
 Hydrogen is the most
common atom of our
universe
 Types of atoms in Earth’s
Crust
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Iron 5%, Aluminum 8%,
Silicon 28%, Oxygen 47%,
Other 12%
 Types of atoms in Humans
Nitrogen 3%, Hydrogen 10%,
Oxygen 61%, Other 26 %
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Names and Symbols of Elements
 Each element has its own symbol
 Some elements use the first letter of the name:
hydrogen (H), Sulfur (S),Carbon (C)
 Other elements use the first letter of the name
plus another letter: aluminum (Al), Platinum (Pt),
Zinc (Zn)
 The first letter is always capitalized and the
following letters are lower case.
Early Greek Philosophers
determined that atoms are the
building blocks of matter.
John Dalton (1766–1844)
John Dalton’s theory of the
atom started out as a solid
sphere with no charges
Proposed the atomic theory
by investigating atomic
weights of atoms
J.J. Thomson determines that an atom
is made up of negative electrons
embedded in a sea of positive charges .
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Ernest Rutherford did some
experiments with thin metal foils and
found that the positive charge is
located within a central nucleus
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Neils Bohr worked under Rutherford but
found problems with his theory. He
ultimately determined that Electrons are in
circular orbits with increasing energy
levels.
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The modern atomic model shows that
electrons occupy regions of space
whose shape is described by complex
mathematical equations. (James
Chadwick)
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History of Atomic Theory
 John Dalton’s theory of the atom started out as a solid
sphere with no charges.
 Then J.J. Thomson figured out there were positive and
negative charges in an atom.
 Rutherford determined that the positive charges
(protons) were located in the center of the atom and the
negative charges (electrons) were scattered around the
nucleus
 Bohr’s theory said that the protons are in the middle and
the electrons travel in specific energy levels and orbits
around the nucleus
 Modern model- protons and neutrons in nucleus,
electrons on energy levels
Review
 An atom is made up of protons (+),
neutrons (no charge), and electrons(-).
 The protons and neutrons are found in
the nucleus
 There has to be an equal number of
protons and electrons because atoms
have no net charge!
 Atomic mass is the number of protons
and neutrons
 Atomic number is the number of
protons (which is the same as the
number of electrons)
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Vocabulary
Atom: the smallest particle of an element that has the
chemical properties of the element
Nucleus: found in the center of the atom and contains the
protons and neutrons
Proton: a positively charged particle found in the nucleus
of an atom
Neutrons: an uncharged particle found in the nucleus of an
atom
Electron: negatively charged particles that move around
outside the nucleus of the atom
Isotopes: atoms of the same element that have a different
number of neutrons. Chlorine atoms have 17 protons, but some
atoms of chlorine have 18 or 20 neutrons these atoms are the
isotopes of chlorine
Atoms form Ions
 Ions: formed when an
atom loses or gains one
or more electrons(- or +
charge)
 Cation: formed when an
atom loses an electron
(+ charge)
 Anion: formed when an
atom gains an electron
(-charge)
Elements are organized by similarity
 Modern Periodic
Table organized by
the atomic # of the
elements
 Dmitri Mendeleev
began organizing
elements by their
physical and chemical
properties (1860’s)
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Periodic Table of the Elements
 Mendeleev
produced the first
periodic table
 Called the periodic
table because a
periodic, or
repeating pattern of
properties of the
elements
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Periodic Table
 Period: each row of the
periodic table is called a
period. If you read from
left to right one proton
and one electron are
added from one element
to the next
 Group/Family: Each
column of the table is
called a group or family.
Elements in a group
share similar properties.
Groups/Families are read
from top to bottom
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Atomic Size on the Periodic Table
Left to right atomic size decreases
Top to bottom atomic size increases
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More Properties of Periodic Table
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Periodic Table has distinct regions
Reactive: indicates how likely an element
is to undergo a chemical change
Most elements are somewhat reactive and
combine with other materials
The most reactive are in groups (up/down)
1 and 17
The least reactive are in group (up/down)
18
Elements combine by the outside
electrons
 All of the electrons in the combining elements do not interact with
each other to form compounds….
 Valence Electrons: Only the electrons in the element’s outside
energy level interact with each other.
 The most stable configuration has 8 electrons in the outer
energy level.
 Elements in group 1 have 1 electron in outside energy level and
elements in group 17 have 7 electrons in outside energy level so
they react with each other easily to form compounds and fulfill the 8
electron stable configuration.
 Most elements are
metals
 Metals are
elements that
conduct electricity
and heat, have
shiny appearance,
and can be
shaped by
pounding
(malleability),
bending, or being
drawn into a thin
wire (ductility)
Metals
Metal types
 Reactive metals: Group (up/down) 1 most reactive
 Transition Metals: Group 3-12 (up/down) generally
less reactive than most metals
Rare Earth Elements
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 Top row of the two rows of metals that are outside of the main
periodic table
 Also known as Lanthanides because they follow the element
lanthanum (La) on the table
 Scientists once thought these metals were available only in tiny
amounts on the Earth
Actinide
• bottom row of the two
rows of metals that are
outside of the main
periodic table
• The Actinide series is
all radioactive and
some are not found in
nature.
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Nonmetals
 Nonmetals: the elements on the right side of the
periodic table
 Many are gases at room temperature, dull
surfaces on the solid nonmetals, cannot be
shaped by ductility or malleability
Halogens
 Elements in group 17
 7 valence electrons
 Greek “forming salts
 Very reactive non-metals
that easily form compounds
with metals. These
compounds are known as
salts.
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Noble Gases
 Group 18 on the
periodic table
 8 valence electrons
 Noble or inert
because they almost
never react with other
elements
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Metalloids
 Have properties of both metals and nonmetals
 Located on either side of the zigzag line
separating metals and nonmetals
 Most common is Silicon
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Radioactivity
 Radioactivity: the process by
which the nucleus of an atom
releases energy and particles
 Marie Curie was the first person to
isolate two radioactive elements
(polonium and radium)
 An isotope is radioactive if the
nucleus has too many or too few
neutrons
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 Radioactive atoms
produce energy and
particles from their nuclei
Radioactive Decay
 The identity of these
atoms changes because
the # of protons changes.
(radioactive decay)
 Occurs at a steady rate
characteristic to each
isotope
 The amount of time for
one-half of the atoms to
decay is called the halflife of the isotope
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Radioactive Decay
 Parent decays into daughter isotope.
 Combination of both is 100%
 Parent starts at 100% and decays to 50%
 100% 1 half-life to 50% (daughter 50%)
 50% 2 half-lives to 25% (daughter 75%)
 25% 3 half-lives to 12.5% (daughter 87.5%)
 12.5% 4 half-lives to 6.25% (daughter 93.75%)