r the periodic table. d’mitri mendeleev 1860’s first to publish placed similar elements in same...
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R The Periodic Table
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D’Mitri Mendeleev
• 1860’s• First to publish• Placed similar elements in same
vertical column• Left open spaces for elements he
predicted would someday be discovered
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Describing the Periodic Table
• The periodic table is a chemistry reference
• It arranges all the known elements in an informative grid
• Elements are arranged left to right and top to bottom in order of increasing atomic number
• This order usually coincides with increasing atomic mass
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Describing the Periodic Table
• The Table's pattern and arrangement shows the arrangement of electrons in the atom.
• Elements have different atomic numbers - the number of protons or electrons increases up the table as electrons fill the shells.
• Elements have different atomic masses - the number of protons plus neutrons increases up the table.
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Families on the Periodic Table
• Elements on the periodic table can be grouped into families bases on their chemical properties.
• Each family has a specific name to differentiate it from the other families in the periodic table.
• Elements in each family react differently with other elements.
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Columns
• The vertical (up and down) columns of the periodic table (there are 18) are called groups or families.
• Elements in the same group or family have similar characteristics or properties.
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Rows
• The horizontal rows of the periodic table are called periods.
• Elements in a period are not alike in properties.
• The first element in a period is usually an active solid, and the last element in a period is always an inactive gas.
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Rows• Atomic size (number of protons)
increases from left to right across a period.
• Atomic mass (number of protons & Neutrons) increases from left to right across a period.
• The period number of an element signifies the highest energy level an electron in that element occupies.
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Rows
• Electrons are added one at a time moving from left to right across a period.
• The electrons on the outermost shell have increasingly strong nuclear attraction, so the electrons become closer to the nucleus.
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Describing the Periodic Table
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Interpreting the Periodic Table
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Interpreting the Periodic Table
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Interpreting the Periodic Table
• The number of protons in an atom tells what element it is.
• The number of protons in an atom is referred to as the atomic number of that element.
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Interpreting the Periodic Table
Atomic Symbol:• The atomic symbol is one or two
letters chosen to represent an element ("H" for "hydrogen," etc.).
• These symbols are used every where in the world
• Usually, a symbol is the abbreviation of the element or the abbreviated Latin name of the element.
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Interpreting the Periodic Table
Atomic Mass:• The atomic mass is the average
mass of an element in atomic mass units ("amu").
• Though individual atoms always have a whole number of amu’s, the atomic mass on the periodic table is shown as a decimal number because it is an average of all the isotopes of an element.
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Interpreting the Periodic Table
Mass Number:• The sum of the protons and neutrons
that make up that nucleus.• The mass number is different for
each isotope of an element.
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Groups and PeriodsAlkali Metals• Very reactive metals that do not occur freely in nature
• Malleable, ductile, good conductors of heat and electricity, solids at room temperature
• Have low densities and low melting points
• Softer than most other metals
• Can explode if they are exposed to water
• Used to produce chemicals, metals, soap, glass, ceramics, and petroleum products
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Groups and Periods
Alkaline Earth Metals• Metals• Very Reactive (give up 2 electrons during
reactions)• Never found free in nature
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Groups and PeriodsTransition Metals• ductile and malleable,
and conduct electricity and heat
• iron, cobalt, and nickel, are the only elements known to produce a magnetic field
• Used in jewelry, industry (copper, steel, iron), technology, light bulbs, and in the food we eat
• Less reactive than most metals
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Groups and Periods
Other Metals
• are ductile and malleable
• are solid, have a relatively high density, and are opaque
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Groups and Periods
Metalloids•Have properties of both metals and non-metals
•Appearance will vary
•Some of the metalloids, such as silicon and germanium, are semi-conductors. This means that they can carry an electrical charge under special conditions. This property makes metalloids useful in computers and calculators. • Conduct better than nonmetals but not as well as metals
•NOTE: any element above 92 is too unstable to occur in nature and must be done in a lab, scientist were able to predict existence of elements (neon and germanium before they were even discovered
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Groups and Periods
Nonmetals Metals
•not able to conduct electricity or heat very well
•exist in two of the three states of matter at room temperature: gases (such as oxygen) and solids (such as carbon).
•very brittle, and cannot be rolled into wires or pounded into sheets
•have no metallic luster, and do not reflect light.
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Groups and PeriodsHalogens• halogen" means "salt-former" and compounds
containing halogens are called "salts"
• Very reactive nonmetals that form salts when combined with many metals• Very reactive; often bond with elements from group one.
• Used to kill harmful micro-organisms in hospitals, to purify drinking water, and prevent growth of algae in swimming pools.
•exists in all three states
• Solid- Iodine, Astatine • Liquid- Bromine • Gas- Fluorine,
Chlorine
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Groups and Periods
Noble Gases• Exist as gases, non-metals• 8 electrons on outer shell=
full• Not reactive with other
elements.
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Groups and Periods
Rare Earth Metals• The Rare Earth Metals are typically silver, silvery-
white, or gray metals.• Good conductors of electricity• 2 Subgroups
– Lanthanide Series: many forms, some with magnetic properties
– Actinide Series• All are radioactive