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Periodic Trends Project
5
Periodic Trends
By: Amauri Barrinuevo
Introduction
Introduction
History And Background
History And Background Of The Periodic Table
Mendeleev
Mendeleev's Role in Creating the Periodic Table Of The Elements
The Russian chemist Dmitri Mendeleev was the first scientist to make a periodic table similar to the one used today. Mendeleev arranged the elements by atomic mass, corresponding to relative molar mass. ... The elements, if arranged according to their atomic mass, exhibit an apparent periodicity of properties.
Organization
Organization Of The Periodic Table
What groups (columns) have in common
What groups (columns) have in common
What the group numbers mean
The periodic table has a special name for its vertical columns. Each column is called a group. The elements in each group have the same number of electrons in the outer orbital. Those outer electrons are also called valence electrons.
What the group numbers mean
What periods (rows) have in common
Like PERIODic table.). All of the elements in a period have the same number of atomic orbitals. For example, every element in the top row (the first period) has one orbital for its electrons. All of the elements in the second row (the second period) have two orbitals for their electrons.
What periods (rows) have in common
Atomic Radii
Atomic Radii
Atomic radius decreases from left to right within a period. This is caused by the increase in the number of protons and electrons across a period. One proton has a greater effect than one electron; thus, electrons are pulled towards the nucleus, resulting in a smaller radius.
Size Of Ions
Size Of Ions
Neutral atoms tend to increase in size down a group and decrease across a period. When a neutral atom gains or loses an electron, creating an anion or cation, the atom's radius increases or decreases, respectively.
Electronegativity And Ionization Energy
Electronegativity And Ionization Energy
Electronegativity
Electronegativity
As you move down a group on the periodic table, the electronegativity of an element decreases because the increased number of energy levels puts the outer electrons very far away from the pull of the nucleus. Electronegativity increases as you move from left to right across a period on the periodic table.
Ionization Energy
Ionization Energy
Ionization energy increases from left to right on the periodic table. Another factor that affects ionization energy is electron shielding. Electron shielding describes the ability of an atom's inner electrons to shield its positively-charged nucleus from its valence electrons.
Conclusion
Conclusion
Conclusion
Conclusion
In conclusion, I have come to notice a pattern within most of the properties shared in each group and each period. The pattern that I observed seems to be that each characteristic, from atomic radii to ionization energy increases from left to right and increases from bottom to top, and decreases from right to left and decreases from top to bottom
Works Cited
Works Cited
Mainly I used two websites, but I also used Wikipedia. https://www.wikipedia.org/
Website #1
Website #1
http://www.chem4kids.com/
Website #2
Website #2
https://chem.libretexts.org/