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Why thermal stability of alkali metal hydride decreases down the group?
As the size of alkali metals increases down the group the M-H bond becomes weaker hence its stability decreases from LiH to CsH
Why thermal stability decreases down the group?
Thermal stability decreases down the group due to the increase in atomic size and metallic character. Larger atoms have weaker metallic bonds, leading to decreased thermal stability as we move down the group. Additionally, the presence of higher energy levels and more electron shielding diminishes the attraction between the nucleus and outer electrons, making the elements less stable at higher temperatures.
What is the trend in ionic character of the group 2 compounds going down the group?
The ionic character increases for group 2 compounds as we go down the group. The metallic character also increases.
What is the periodic trend for electrongativity?
Electronegativity generally increases from left to right across a period and decreases from top to bottom within a group on the periodic table. This trend is due to the increasing nuclear charge across a period and the increasing distance between the nucleus and valence electrons down a group.
How does the atomic radius change from top to bottom in a group 1 and 2 in the periodic table?
Going down and to the left on the periodic table, atomic radius increases. Therefore, the smallest atomic radius is that of Helium (He), and the largest is that of Francium (Fr). Coincidentally, these are also the most and least reactive elements.
Why thermal stability of alkali metal hydride decreases down the group?
As the size of alkali metals increases down the group the M-H bond becomes weaker hence its stability decreases from LiH to CsH
What is the trend of thermal stability in periodic table?
The trend of thermal stability in the periodic table generally increases as you move down a group. This is because lower elements have more electron shells which shield the outer electrons from the nucleus, making it harder to break bonds. Additionally, elements with larger atomic radius tend to be more thermally stable.
Why thermal stability decreases down the group?
Thermal stability decreases down the group due to the increase in atomic size and metallic character. Larger atoms have weaker metallic bonds, leading to decreased thermal stability as we move down the group. Additionally, the presence of higher energy levels and more electron shielding diminishes the attraction between the nucleus and outer electrons, making the elements less stable at higher temperatures.
What is the trend in ionic character of the group 2 compounds going down the group?
The ionic character increases for group 2 compounds as we go down the group. The metallic character also increases.
What do you predict the trend in atomic mass will be going down a group?
The atomic mass increases down a group.
What general trend in electronegativity do you note going down a group across a period?
going down a group, electronegativity decreases going across a period, electronegativity increases
How do elements change going down the periodic table?
Down a group, the atomic number generally increases, size increases, ionization energy decreases, reactivity increases.
What property increases going down a group in periodic table?
Atomic size increases going down a group in the periodic table. This is because additional energy levels are being filled with electrons, leading to an increase in distance between the nucleus and the outermost electron shell.
Why metlic character increases from top to bottom in a group of metals?
Down a group, the number of shells increases, also the atomic size. Thus , the metallic character increase does increase as going DOWN a group. It is easy to remove an electron froman atom of bigger...
Thermal stability of group 2 carbonates?
Carbonates are decomposed by heating in oxides and carbon dioxide; the temperatures of decomposition are: - Beryllium carbonate: decomposed at room temperature. - Magnesium carbonate: 400 0C - Calcium carbonate: 900 0C - Strontium carbonate: 1 280 0C - Barium carbonate: 1 360 0C - Radium carbonate: I have not yet found data.
What is the periodic trend for elctronegativity?
Electronegativity generally increases across a period from left to right due to an increase in effective nuclear charge, making it harder for atoms to release electrons. It tends to decrease down a group as the atomic size increases, leading to weaker attraction for valence electrons.
What is the periodic trend for electrongativity?
Electronegativity generally increases from left to right across a period and decreases from top to bottom within a group on the periodic table. This trend is due to the increasing nuclear charge across a period and the increasing distance between the nucleus and valence electrons down a group.
