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What atomic property affects periodic periodic trends down a group in the periodic table?
Wiki User
∙ 13y ago
The phenomenon that comes into play as we go down toward the bottom of the Periodic Table through a group is electron screening. As we descend through a group, the atomic number of an atom increases, and so does the number of electrons shells. That means more electrons are between the nucleus (the positive charge) and the valence shell. You'll recall that the valence shell is the outer electron shell, and it is this shell and its population that largely determine the chemistry of an element. When atoms are larger with more electrons shells, the positive charge on the nucleus is "shielded" from the valence shell to a degree by the inner electron shells. That nucleus isn't "holding onto" the valence electrons as tightly. And in atoms that are electron "loaners" like those on the left side of the periodic table, the elements further down a group are "more willing" to loan out valence electrons. This means that they are more reactive. Electron screening serves to "interfere" with the grip the nucleus holds on the valence electrons for atoms farther down a group. On the right side of the periodic table, elements tend to be "borrowers" of electrons, and the translation of the effect of screening on the right is that the elements toward the bottom of a group are going to be less inclined to want to borrow an electron that elements higher up. Again, this is due to electron screening. If all of this is true, then the element of the bottom of Group 1, which is on the left of the table, will be the most reactive electron-loaning element. That's francium, and it is, indeed, the most reactive of the Group 1 elements. Conversely, on the right in the Group 17 elements (the halogens or halides), we'd expect the elements at the bottom to be less reactive than those at the top. And they are. The most reactive halogen is fluorine (at the top of the group), and it is the hungry wolf of the periodic table. Links are provided below.
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∙ 15y ago
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What periodic trends did did Mendeleev organize his periodic table by?
Atomic Mass Octaves and Triads
What 2 atomic properties will you examine for periodic trends?
- atomic number (number of protons)- electron configuration
Atomic mass trends in the periodic table?
Atomic Mass increases in size as the atomic number increases. For example, hydrogen weighs about 1.01 grams per mole and it has periodic #1. Helium is atomic #2 and it has an atomic mass of 4.00 g/mol. This trend continues all the way to the last known pure element.
What periodic trends did Mendeleev organize his periodic table by Atomic number Atomic mass Octaves Triads First ionization energy?
In 1869, Mendeleev organized his periodic table by increasing atomic mass (atomic weight), using what is called the "law of octaves," by which every 8th element in the sequence shared similar properties. This was first observed by John Newlands in his element table around 1863.
What is the noble gas configuration for element 117?
Based on the trends in the periodic table, the noble gas notation of the element with atomic number 117 will be[Rn]5f146d107s27p5
Which 3 atomic properties will you examine for periodic trends?
For periodic trends we will examine1- Electronic configuration 2- Ionization energy 3- Atomic radius
What periodic trends did did Mendeleev organize his periodic table by?
Atomic Mass Octaves and Triads
What periodic trends did Mendeleev organize his periodic table by?
atomic mass, triads, and octaves
What are the periodic trends in atomic size?
rsecdcvcdbhght cfcbyf rbn
What trends were seen in Mendeleev's periodic table?
he arranged his Periodic Table by each elements Atomic Mass
What 2 atomic properties will you examine for periodic trends?
- atomic number (number of protons)- electron configuration
What periodic trends are inversely proportional to effective nuclear charge?
atomic radius
What is the basis in which the present day periodic table is organized?
The Periodic Table is organized by atomic number, metals, nonmetals, metalloids, periods, groups, and stability.
How are the trends in the periodic table helpful in identifying an element?
The periodic trends that arise from the arrangement of the periodic table provide chemists with an invaluable tool to quickly predict an element's properties. These trends exist because of the similar atomic structure of the elements within their respective group families or period and the periodic nature of the elements.
What does it mean if a chemical or physical property is periodic?
The modern periodic table is based on the periodic law, which states that physical and chemical propertiesof the elements are a periodic function of their atomic numbers.Yes this answer is good!
What are 2 reasons for studying the periodic table?
Periodic table of elements provides us a lot of information about element's intrinsic properties. We can get the atomic weight of an element by looking at the periodic table. Trends about the electronegativity and atomic size can also be computed.
Why is the periodic table useful for studying the properties of different elements?
well, the periodic table is very useful because you have the atomic number, atomic mass, and even the trends across a period or down a group.
