electron configurations of the elements oor Indonesies
electron configurations of the elements
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The form of the periodic table is closely related to the electron configuration of the atoms of the elements.
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It has been suggested that this layout originated in the 1940s, with the appearance of periodic tables relying on the electron configurations of the elements and the notion of the differentiating electron.
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The number of electrons donated or accepted in a redox reaction can be predicted from the electron configuration of the reactant element.
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And how those electrons are configured, and how the electrons of other elements are configured, or maybe other atoms of that same element.
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Columns (groups) are determined by the electron configuration of the atom; elements with the same number of electrons in a particular subshell fall into the same columns (e.g. oxygen and selenium are in the same column because they both have four electrons in the outermost p-subshell).
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Knowledge of the electron configuration of different atoms is useful in understanding the structure of the periodic table of elements.
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According to the principle, unpenttrium should have an electronic configuration of 8s25g186f147d1 and filling the 5g-subshell should be stopped at element 138.
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The element is calculated have electronic configuration of 8s28p1/21, which is not associated with transition metals, without having a partially filled d-subshell.
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It is a shiny gray solid which bears a close physical resemblance to the other five elements in the second column (group 2, or alkaline earth metals) of the periodic table: all group 2 elements have the same electron configuration in the outer electron shell and a similar crystal structure.
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For example, all the elements of group 2 have an electron configuration of ns2 (where is an inert gas configuration), and have notable similarities in their chemical properties.
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While such a placement is common for hydrogen, it is rarely used for helium outside of the context of electron configurations: When the noble gases (then called "inert gases") were first discovered around 1900, they were known as "group 0", reflecting no chemical reactivity of these elements known at that point, and helium was placed on the top of that group, as it did share the extreme chemical inertness seen throughout the group.
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Modern quantum mechanical theories of atomic structure explain group trends by proposing that elements within the same group generally have the same electron configurations in their valence shell.
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The octet rule is a chemical rule of thumb that reflects observation that atoms of main-group elements tend to bond in such a way that each atom has eight electrons in its valence shell, giving it the same electron configuration as a noble gas.
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This group lies in the s-block of the periodic table of elements as all alkali metals have their outermost electron in an s-orbital: this shared electron configuration results in their having very similar characteristic properties.
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Although main group elements of the second period and beyond usually react by gaining, losing, or sharing electrons until they have achieved a valence shell electron configuration with a full octet of (8) electrons, hydrogen (H) can only form bonds which share just two electrons.
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However, some elements like hydrogen and lithium need only two electrons in their outermost shell to attain this stable configuration; these atoms are said to follow the duet rule, and in this way they are reaching the electron configuration of the noble gas helium, which has two electrons in its outer shell.
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16 sinne gevind in 9 ms. Hulle kom uit baie bronne en word nie nagegaan nie.