The contemporary periodic table has evolved since Mendeleev's initial table, but both are significant for the same reason: the periodic table groups elements according to comparable qualities, so you can identify an element's features merely by glancing at its location on the table.
Prior to the discovery of all naturally occurring elements, the periodic table was used to anticipate the chemical and physical attributes of elements in the chart's gaps.
Today, the table may be used to forecast the characteristics of elements yet to be found, despite the fact that these new elements are all highly radioactive and break down nearly rapidly into more known elements.
The chart is valuable for current students and scientists since it predicts the sorts of chemical reactions that an element is likely to undergo. Rather than memorizing facts and statistics for each element, a short glance at the table tells a lot about an element's reactivity, whether it is likely to conduct electricity, whether it is hard or soft, and many other properties.
Elements in the same column (groups) have comparable qualities. For example, the elements in the first column (alkali metals) are all metals that have a 1+ charge in reactions, react aggressively with water, and mix easily with nonmetals.
Elements in the same row (periods) have the maximum unexcited electron energy level.
Another advantageous characteristic of the table is that most tables include all of the information required to balance chemical processes at a glance. The table shows an element's atomic number and, in most cases, its atomic weight. The group of an element indicates the element's normal charge.
Periodicity or Trends
The periodic table is ordered based on changes in element properties:
Crossing the row from left to right
The Atomic Radius is shrinking.
The Energy of Ionization Increases
In general, electron affinity rises (except Noble Gases)
Electronegativity rises.
Moving from the top to the bottom of a column
The Atomic Radius Expands
Ionization Energy Diminishes
Moving down a group, electron affinity usually decreases.
Answers & Comments
Verified answer
IMPORTANCE OF PERIODIC TABLE OF ELEMENTS
Answer:
The contemporary periodic table has evolved since Mendeleev's initial table, but both are significant for the same reason: the periodic table groups elements according to comparable qualities, so you can identify an element's features merely by glancing at its location on the table.
Prior to the discovery of all naturally occurring elements, the periodic table was used to anticipate the chemical and physical attributes of elements in the chart's gaps.
Today, the table may be used to forecast the characteristics of elements yet to be found, despite the fact that these new elements are all highly radioactive and break down nearly rapidly into more known elements.
The chart is valuable for current students and scientists since it predicts the sorts of chemical reactions that an element is likely to undergo. Rather than memorizing facts and statistics for each element, a short glance at the table tells a lot about an element's reactivity, whether it is likely to conduct electricity, whether it is hard or soft, and many other properties.
Elements in the same column (groups) have comparable qualities. For example, the elements in the first column (alkali metals) are all metals that have a 1+ charge in reactions, react aggressively with water, and mix easily with nonmetals.
Elements in the same row (periods) have the maximum unexcited electron energy level.
Another advantageous characteristic of the table is that most tables include all of the information required to balance chemical processes at a glance. The table shows an element's atomic number and, in most cases, its atomic weight. The group of an element indicates the element's normal charge.
Periodicity or Trends
The periodic table is ordered based on changes in element properties:
Crossing the row from left to right
The Atomic Radius is shrinking.
The Energy of Ionization Increases
In general, electron affinity rises (except Noble Gases)
Electronegativity rises.
Moving from the top to the bottom of a column
The Atomic Radius Expands
Ionization Energy Diminishes
Moving down a group, electron affinity usually decreases.
Electronegativity is decreasing.
PERIODIC TABLE
classification of parts of period table
brainly.ph/question/15385962
#LETSSTUDY