Chapter 8
Periodic Properties
By Boundless
![Thumbnail](../../../../../figures.boundless-cdn.com/9645/raw/periodic-table.jpg)
The periodic table is a methodical arrangement of the chemical elements, organized on the basis of their electron configurations.
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Elements of the same period have the same number of electron shells.
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The d-block elements are commonly known as transition metals or transition elements.
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The periodic table currently contains 7 periods, but theorists predict that two additional periods may exist.
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The position of elements on the periodic table is directly related to their electron configurations.
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The elements on the periodic table exhibit different levels of reactivity based on the number of electrons in their highest energy shells.
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An atom's electrons exist in discrete atomic orbitals, and the atom's electron configuration can be determined using a set of guidelines.
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The Aufbau principle determines an atom's electron configuration by adding electrons to atomic orbitals following a defined set of rules.
![Thumbnail](../../../../../figures.boundless-cdn.com/11026/raw/agram-carbon-hund-27s-rule.jpg)
Hund's Rule defines the behavior of unpaired valence shell electrons, providing insight into an atom's reactivity and stability.
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The shielding effect, approximated by the effective nuclear charge, is due to inner electrons shielding valence electrons from the nucleus.
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Diamagnetic atoms have only paired electrons, whereas paramagnetic atoms, which can be made magnetic, have at least one unpaired electron.
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The physical properties of elements vary across a period, mostly as a function of bonding.
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The physical properties (notably, melting and boiling points) of the elements in a given group vary as you move down the table.
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The electron configuration of a given element can be predicted based on its location in the periodic table.
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Atomic radii decrease from left to right across a period and increase from top to bottom along a group.
![Thumbnail](../../../../../figures.boundless-cdn.com/30037/square/atomic_&_ionic_radii.jpg.jpg)
Similarly charged ions tend to decrease in size across a period (row) and increase in size down a group (column).
![Thumbnail](../../../../../figures.boundless-cdn.com/10052/square/nizationenergyatomicweight.jpg)
The ionization energy tends to increase as one moves from left to right across a given period or up a group in the periodic table.
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The electron affinity of the elements generally increases across a period and sometimes decreases down a group in the periodic table.
![Thumbnail](../../../../../figures.boundless-cdn.com/10087/square/blocks.jpg)
In the periodic table, the elements are placed from left to right in each period in the sequence of their atomic numbers.
![Thumbnail](../../../../../figures.boundless-cdn.com/10089/square/halogens.jpg)
The halogens are a series of highly reactive, nonmetal elements from Group 17 of the periodic table.
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Noble gases are the six chemical elements of Group 18 of the periodic table, being monatomic and (with very limited exceptions) inert.
- The Nature of Light
- Bohr's Theory
- Quantum Mechanical Description of the Atomic Orbital
- Orbital Shapes