introduction to the periodic table -...
TRANSCRIPT
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Introduction to the Periodic Table
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Atom Review
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Atom Review
▪ The atom consists of a nucleus surrounded by orbitals.
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Atom Review
▪ The nucleus contains positively charged protons and neutral (no charge) neutrons.
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Atom Review
▪ Negatively charged electrons circle the nucleus in the orbitals.
▪ There are 2 electrons in first orbital.
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Electron Orbitals
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Time Line
1750. Only 17 elements had been identified.
1789.Antoine Lavoisier grouped the known elements into metals, nonmetals, gases, and earths. The unknown elements caused problems.
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Time Line
1860s Dmitri Mendeleev organized the 63 known elements into a periodic table based on increasing mass with elements with similar properties in the same columns. He left spaces for the unknown elements.
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Mendeleev’s Periodic Table
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Time Line
1875. Gallium fit into the table as expected based on its melting point and density.
1879. Scandium fit as expected.
1886 Germanium fit as expected.
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Protons
▪ Protons where discovered in 1918 by Ernest Rutherford.
▪ Mendeleev had no knowledge of them.
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Protons
▪ All atoms of an element have the same number of protons.
▪ They do not all have the same atomic mass.
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Periodic Table
▪ Because of this, the modern table is arranged in order of increasing atomic number or number of protons.
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Periodic Table
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Isotopes
▪ The atoms of the same element with different masses are isotopes.
▪ They have different numbers of neutrons.▪ The atomic mass given on the table is an
average of all known masses for the element.
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Periodic Table
▪ Rows are called periods.▪ There are seven of these.▪ The number of orbitals increases from one
period to the next.
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Periodic Table
▪ Columns are called groups.▪ Groups have similar properties because they
have similar electron configurations.▪ The electron configurations determine their
chemical properties.▪ That pattern is called the periodic law.
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Periodic Table
17
ClChlorine
35.453
Aatomic # #
Element symbol
Element name
Atomic mass
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Math
▪ Atomic mass = protons + neutrons▪ Atomic number = protons▪ Protons = electrons (atoms are neutral/no
charge as listed on the periodic table)
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AMU
▪ Atomic mass unit▪ Because the mass of an atom in grams is very,
very small we measure the mass of individual atoms in amu.
▪ Each proton and neutron counts a 1 amu.▪ For example: carbon has 6 protons and 6
neutrons so its mass is 12 amu
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Elements(WRITE THE UNDERLINED NOTES!!!!)
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Periodic Table
▪ Elements 1-92 except 43 and 61 occur naturally on Earth.
▪ (The others can be made through process we will talk about in the future.)
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Elements
▪ Elements are grouped into 3 groups:▪ Metals▪ Nonmetals▪ Metalloids
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Metals
▪ Most of the elements are metals.▪ They are on the left side and middle of the
periodic table.
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Properties of Metals
▪ Except for mercury, they are all solid at room temperature.
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▪ They are good conductors of electric current and heat.
Properties of Metals
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Properties of Metals
▪ They are malleable (bendable).
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Properties of Metals
▪ They are ductile (can be drawn into thin wires).
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Properties of Metals
▪ They range from extremely reactive to difficult to make react.
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Transition Metals
▪ Groups 3-12
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Transition Metals
▪ They were among the 1st elements discovered.▪ They are able to form compounds with distinct
colors.▪ These groups have more in common than other
groups on the table.
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Transition Metals
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Nonmetals
▪ Located on the right side of the table except for hydrogen.
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Nonmetal Properties
▪ Poor conductors of heat and electricity
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Nonmetal Properties
▪ Low boiling point▪ All gases are nonmetals but not all nonmetals
are gases.
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Nonmetal Properties
▪ Brittle if solid at room temperature
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Nonmetal Properties
▪ Reactivity varies▪ Fluorine is the most reactive nonmetal.▪ Group 18 are the least reactive elements on the
table.
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Metalloids
▪ Separate metals and nonmetals on the table.▪ Conductivity varies▪ Changes in temperature cause some to change
from good insulators to good conductors.
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Trends
▪ As you move from left to right across the table, elements become less metallic and more nonmetallic in their properties.