Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity...
-
Upload
camilla-hart -
Category
Documents
-
view
237 -
download
0
Transcript of Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity...
![Page 1: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/1.jpg)
Periodicity
![Page 2: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/2.jpg)
Periodicity
• Atomic radius• Ionic radius• Ionization energy• Electron affinity• Electronegativity• Metallic character
![Page 3: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/3.jpg)
Atomic radius• (Size) One half the distance between the nuclei of
identical atoms that are bonded together.Period• Decreases across a period• Atoms shrink across a period because added protons
in the nucleus pull the added electrons more tightlyGroup• Increases down a group• Atoms get bigger as you go down the group/ family
because orbitals are added to make room for more electrons
![Page 4: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/4.jpg)
Atomic radius
![Page 5: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/5.jpg)
Ionic Radius
• The trend is the same as atomic radius– size increases down a group and decreases across a period
![Page 6: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/6.jpg)
Ionization Energy• Amount of energy required to remove an electron
from an atom.Period• Increases across a period • The outer-most electron becomes more difficult to remove
across a period since added protons exert a stronger attraction.
Group• Decreases down a group• The outer-most electron is easier to remove as you move
down a column since each time you are one energy level farther from the nucleus
![Page 7: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/7.jpg)
Ionization energy
![Page 8: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/8.jpg)
Electron Affinity• The amount of energy released when an
atom takes on an electron.
Period• Increases across a period
Group• Increases down a group
![Page 9: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/9.jpg)
Electron affinity
![Page 10: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/10.jpg)
Electronegativity• The tendency of a bonded atom to attract the electrons in
that bond.• Period• Increases across a period• The pull of the increased protons in the nucleus is enough to
attract electrons that come close to the outer limits of the atom from other sources.
• Group• Decreases down a group• Electrons are more difficult to hold onto as you move down
a column.
![Page 11: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/11.jpg)
Electronegativity
![Page 12: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/12.jpg)
Metallic characterPeriod•Decreases across a period •Metallic properties are most pronounced at the left side of the table where shielding is at a maximum.
Group•Increases down a group•Properties will also increase as you move down a family since shielding improves.
![Page 13: Periodicity. Atomic radius Ionic radius Ionization energy Electron affinity Electronegativity Metallic character.](https://reader035.fdocuments.us/reader035/viewer/2022081503/5697bfc51a28abf838ca66b4/html5/thumbnails/13.jpg)
Metallic character
• Fr (Francium) is the most reactive metal.• F (Fluorine) is the most reactive non-metal.• The noble gases are very un-reactive.