september 15. dmitri mendeleev, a russian chemist, noticed that when the elements were arranged by...
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PERIODIC TABLE TRENDS
September 15
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Mendeleev & Moseley
Dmitri Mendeleev , a Russian chemist, noticed that when the elements were arranged by atomic mass, there was a periodic pattern in properties He left blank spaces open for new elements
to be discovered He was one of the first to arrange the
elements in an organized table
His arrangement had its faults though…
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When new elements were discovered, it became apparent that they didn’t fit into Mendeleev’s table properly When arranged by mass, the properties
did not correspond
Moseley (1913) – Arranged periodic table by atomic number Elements close to one another have
similar properties
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Periodic Law
Periodic Law: there is a periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number
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How to read those numbers…Atomic Mass: Approx. the mass of the
protons in the element 1 atomic mass unit (amu)= mass of 1 Carbon
12 atom
Atomic Number: # of protons in the nucleus The atomic number increases by 1 as you go
across a row Also the number of electrons in the element if
it is neutral
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What is in an element/atom? Protons: Positive Charge (+) Neutrons: No Charge Electrons: Negative Charge (-)
Protons +Neutrons make up a nucleus Electrons circle around the nucleus in orbitals
In general, #protons=#electrons (neutral) Also #neutrons= atomic mass-atomic number
If they differ in neutrons, it is called an isotope▪ C12, C13, C14
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So…
If elements are ordered in the periodic table by atomic number, then they are also ordered according to the number of electrons they have.
The lineup starts with hydrogen, which has one electron.
Helium comes next in the first horizontal row because helium has two electrons. Lithium has three.
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Valence Electrons
In an atom there are multiple orbitals (think planets)
Valence electrons: electrons in the outer most orbital…these determine the chemical properties of the element
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Back to the periodic table
Period: Horizontal Row (think sentence) Numbered from top to bottom
Group/Family: Column/Vertical Numbered from left to right
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Proximity Matters
Elements in the same group have characteristics similar to each other, yet different from the other elements in the periodic table. Similarities occur because elements in the
same group have the same number of valence electrons
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Names & Organization
Periodic table is divided into 4 main groups Representative or main-group elements Transition metals Lanthanide series Actinide series
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Groups 1A – Alkali metals Very reactive Explosive reactions with water One valence electron All metals
Groups 2A – Alkaline Earth Metals Quite reactive Two valence electrons All metals
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Groups 3A – Boron Family Varies from semi-metallic to non-metallic
in properties Three valence electrons
Group 4A – Carbon Family Varies from non metallic to metallic in
properties Four valence electrons
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Group 5A – Nitrogen Family Varies from non-metallic to metallic
properties Five valence electrons
Groups 6A – Oxygen Family Mostly non-metallic Six valence electrons
Group 7A – Halogens All are non-metallic and make colorful
gases Seven valence electrons
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Group 8A – Noble gases All non metals and highly unreactive Eight valence electrons
Transition metals All have metallic properties Valence number varies
Lanthanoids & Actinoids Radioactive, many are non-natural or man-
made Valence number varies
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Metallic Character
Metallic Character Element on the left side of the periodic
table are metals, while those on the right side are non metals.
Elements that touch the dividing line between metals and nonmetals are called metalloids
Metallic character increases as you move down a column and across a row to the left
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Reactivity
Reactivity Reactivity for metallic element increases
as you move down a column and across a row to the left ▪ The most reactive metal is Francium (bottom,
left corner) Reactivity for nonmetal increases as you
move up a column and across a row to the right▪ The most reactive nonmetal is Fluorine (top,
right corner)
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Ionization Energy
Ionization Energy1. The energy needed to remove the
outermost electron from an element (increases dramatically with successive removals)
2. Ionization energy depends on the number of valence electrons and the size of the atom▪ Elements with nearly full valence shells will have
higher ionization energy than those with nearly empty valence shells
▪ Larger elements will have a lower ionization energy than smaller elements
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Ionization energy increases as you move up a column and across a row to the right.
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Electronegativity
Electronegativity (similar trend to ionization) Ability of an element to attract shared
electrons to itself Depends on the number of valence
electrons and the size of the element Increases as you move up a column and
across a row to the right
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Atomic Radius
Atomic Radius Close approximation of the relative size of an
atom Determined by finding the distance from the
center of an atom nucleus to it’s outermost electron
Increases as you move down a column▪ Each step down in a column increases the number of
orbitals (electron shells) Increases as you move across a row to the left▪ Decreasing the number of protons in the nucleus
causes the electrons to be held more loosely
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How size changes…
Ionic Size Size of an atom when electrons are
added or removed Electrons removed atom become smaller Electrons added atoms become larger
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Your Project
http://www.azuregrackle.com/periodictable/table/
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Due Tues Nov. 23
Creativity(Does your artwork relate to the
element?)
25
Element Symbol(More Creative the Better)
5
1 Page Paper properly typed or written (grammar) about your
element (include facts!!!)
20
Does your paper relate your artwork to the element?
10
Your Special Element RubricTotal Points: 60
Total = 60 points