“periodic table”的概念、定义、翻译、参考文献-科学参考

periodic table

Physics

A table of elements arranged in order of increasing proton number to show the similarities of chemical elements with related electronic configurations. (The original form was proposed by the Russian Dmitri Mendeleev in 1869 using relative atomic masses.) The elements fall into vertical columns, known as groups. Going down a group, the atoms of the elements all have the same outer shell structure, but an increasing number of inner shells. All the elements in the middle of the table are classified as transition elements and the nontransition elements are regarded as main-group elements. Horizontal rows in the table are periods. The first three are called short periods; the next four (which include transition elements) are long periods. Within a period, the atoms of all the elements have the same number of shells, but with a steadily increasing number of electrons in the outer shell. The periodic table can also be divided into four blocks depending on the type of shell being filled: the s-block, the p-block, the d-block, and the f-block. There are certain general features of chemical behaviour shown in the periodic table. In moving down a group, there is an increase in metallic character because of the increased size of the atom. In going across a period, there is a change from metallic (electropositive) behaviour to nonmetallic (electronegative) because of the increasing number of electrons in the outer shell. Consequently, metallic elements tend to be those on the left and towards the bottom of the table; nonmetallic elements are towards the top and the right. See Appendix 5

The existence of the periodic table is due to the shell structure of atoms—which, in turn, is due to the Pauli exclusion principle.

https://www.webelements.com/ The WebElements table, produced by Mark Winter at the University of Sheffield

http://www.meta-synthesis.com/webbook/35_pt/pt_database.php Over fifty different forms of the periodic table in the Chemogenesis web book by Mark R. Leach

Chemistry

A table of elements (see Appendix 5) arranged in order of increasing proton number to show the similarities of chemical elements with related electronic configurations. (The original form was proposed by Dimitri Mendeleev in 1869 using relative atomic masses.) In the modern short form, the lanthanoids and actinoids are not shown. The elements fall into vertical columns, known as groups. Going down a group, the atoms of the elements all have the same outer shell structure, but an increasing number of inner shells. Traditionally, the alkali metals were shown on the left of the table and the groups were numbered IA to VIIA, IB to VIIB, and 0 (for the noble gases). All the elements in the middle of the table are classified as transition elements and the nontransition elements are regarded as main-group elements. Because of confusion in the past regarding the numbering of groups and the designations of subgroups, modern practice is to number the groups across the table from 1 to 18. Horizontal rows in the table are periods. The first three are called short periods; the next four (which include transition elements) are long periods. Within a period, the atoms of all the elements have the same number of shells, but with a steadily increasing number of electrons in the outer shell. The periodic table can also be divided into four blocks depending on the type of shell being filled: the s-block, the p-block, the d-block, and the f-block.
There are certain general features of chemical behaviour shown in the periodic table. In moving down a group, there is an increase in metallic character because of the increased size of the atom. In going across a period, there is a change from metallic (electropositive) behaviour to nonmetallic (electronegative) because of the increasing number of electrons in the outer shell. Consequently, metallic elements tend to be those on the left and towards the bottom of the table; nonmetallic elements are towards the top and the right.
There is also a significant difference between the elements of the second short period (lithium to fluorine) and the other elements in their respective groups. This is because the atoms in the second period are smaller and their valence electrons are shielded by a small 1s² inner shell. Atoms in the other periods have inner s- and p-electrons shielding the outer electrons from the nucleus. Moreover, those in the second period only have s- and p-orbitals available for bonding. Heavier atoms can also promote electrons to vacant d-orbitals in their outer shell and use these for bonding. See also diagonal relationship; inert-pair effect.
https://www.webelements.com/ The WebElements table produced by Mark Winter at the University of Sheffield
https://www.meta-synthesis.com/webbook/35_pt/pt_database.php Over 30 different forms of the periodic table in the Chemogenesis web book by Mark R. Leach

Chemical Engineering

The tabular arrangement of all the chemical elements in order of their atomic numbers. The table consists of vertical columns containing groups of elements with similar properties, demonstrating the periodic law. The elements in each group have the same number of electrons in their outer orbitals and therefore share the same valency, thereby accounting for their similar chemical properties. The horizontal rows are periods. The table was originally devised and published by Russian chemist Dmitri Ivanovich Mendeleev (1834–1907) in 1869 and was based on relative atomic masses. See Appendix 7.

Electronics and Electrical Engineering

The classification of chemical elements, first introduced by Mendeléev, that demonstrates a periodicity of chemical properties when the elements are arranged in order of their atomic numbers. One form of periodic table is given in Table 11, in the back matter. Elements of similar chemical properties occur in the same vertical group in the periodic table. The periodic table was used to predict the existence of undetected elements.

单词	periodic table
释义	periodic table Physics A table of elements arranged in order of increasing proton number to show the similarities of chemical elements with related electronic configurations. (The original form was proposed by the Russian Dmitri Mendeleev in 1869 using relative atomic masses.) The elements fall into vertical columns, known as groups. Going down a group, the atoms of the elements all have the same outer shell structure, but an increasing number of inner shells. All the elements in the middle of the table are classified as transition elements and the nontransition elements are regarded as main-group elements. Horizontal rows in the table are periods. The first three are called short periods; the next four (which include transition elements) are long periods. Within a period, the atoms of all the elements have the same number of shells, but with a steadily increasing number of electrons in the outer shell. The periodic table can also be divided into four blocks depending on the type of shell being filled: the s-block, the p-block, the d-block, and the f-block. There are certain general features of chemical behaviour shown in the periodic table. In moving down a group, there is an increase in metallic character because of the increased size of the atom. In going across a period, there is a change from metallic (electropositive) behaviour to nonmetallic (electronegative) because of the increasing number of electrons in the outer shell. Consequently, metallic elements tend to be those on the left and towards the bottom of the table; nonmetallic elements are towards the top and the right. See Appendix 5 The existence of the periodic table is due to the shell structure of atoms—which, in turn, is due to the Pauli exclusion principle. https://www.webelements.com/ The WebElements table, produced by Mark Winter at the University of Sheffield http://www.meta-synthesis.com/webbook/35_pt/pt_database.php Over fifty different forms of the periodic table in the Chemogenesis web book by Mark R. Leach Chemistry A table of elements (see Appendix 5) arranged in order of increasing proton number to show the similarities of chemical elements with related electronic configurations. (The original form was proposed by Dimitri Mendeleev in 1869 using relative atomic masses.) In the modern short form, the lanthanoids and actinoids are not shown. The elements fall into vertical columns, known as groups. Going down a group, the atoms of the elements all have the same outer shell structure, but an increasing number of inner shells. Traditionally, the alkali metals were shown on the left of the table and the groups were numbered IA to VIIA, IB to VIIB, and 0 (for the noble gases). All the elements in the middle of the table are classified as transition elements and the nontransition elements are regarded as main-group elements. Because of confusion in the past regarding the numbering of groups and the designations of subgroups, modern practice is to number the groups across the table from 1 to 18. Horizontal rows in the table are periods. The first three are called short periods; the next four (which include transition elements) are long periods. Within a period, the atoms of all the elements have the same number of shells, but with a steadily increasing number of electrons in the outer shell. The periodic table can also be divided into four blocks depending on the type of shell being filled: the s-block, the p-block, the d-block, and the f-block. There are certain general features of chemical behaviour shown in the periodic table. In moving down a group, there is an increase in metallic character because of the increased size of the atom. In going across a period, there is a change from metallic (electropositive) behaviour to nonmetallic (electronegative) because of the increasing number of electrons in the outer shell. Consequently, metallic elements tend to be those on the left and towards the bottom of the table; nonmetallic elements are towards the top and the right. There is also a significant difference between the elements of the second short period (lithium to fluorine) and the other elements in their respective groups. This is because the atoms in the second period are smaller and their valence electrons are shielded by a small 1s² inner shell. Atoms in the other periods have inner s- and p-electrons shielding the outer electrons from the nucleus. Moreover, those in the second period only have s- and p-orbitals available for bonding. Heavier atoms can also promote electrons to vacant d-orbitals in their outer shell and use these for bonding. See also diagonal relationship; inert-pair effect. https://www.webelements.com/ The WebElements table produced by Mark Winter at the University of Sheffield https://www.meta-synthesis.com/webbook/35_pt/pt_database.php Over 30 different forms of the periodic table in the Chemogenesis web book by Mark R. Leach Chemical Engineering The tabular arrangement of all the chemical elements in order of their atomic numbers. The table consists of vertical columns containing groups of elements with similar properties, demonstrating the periodic law. The elements in each group have the same number of electrons in their outer orbitals and therefore share the same valency, thereby accounting for their similar chemical properties. The horizontal rows are periods. The table was originally devised and published by Russian chemist Dmitri Ivanovich Mendeleev (1834–1907) in 1869 and was based on relative atomic masses. See Appendix 7. Electronics and Electrical Engineering The classification of chemical elements, first introduced by Mendeléev, that demonstrates a periodicity of chemical properties when the elements are arranged in order of their atomic numbers. One form of periodic table is given in Table 11, in the back matter. Elements of similar chemical properties occur in the same vertical group in the periodic table. The periodic table was used to predict the existence of undetected elements.
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