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In terms of atomic radius, the sequence would be oxygen, carbon (both period 2), magnesium (period 3), rubidium (period 4), and cesium (period 5).
Note that order by periods is not absolute: in each period, the elements toward the far left side have the largest radii. For example, the radius for lithium in period 2 is larger than almost all of the elements in periods 3 and 4.
*Numerically, the elements O, C, Mg, Rb, and Cs have respective radii of about 60, 70, 150, 235, and 260 picometers.
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How is the periodic table arranged in terms of their ato mic structures?
The elements in the periodic table are arranged in order of increasing atomic numbers.
How can you compare and contrast the periodic table that Mendeleev developed to the periodic table that Mosley organized?
Mendeleev used atomic masses to classify the element, where as Moseley classified the element in terms of atomic number, he suggested that chemical and physical properties are the functions of the atomic number Elements in the periodic table is classified as Metals, Nonmetal and Metalloids. Normally Group 1 to 12 are metals... Sayed Abdul Aziem Sayed_abd2007@hotmail.com
Who is the inventor of the periodic table?
Dmitri Mendeleev is generally credited, as he was able to predict the properties of elements which had not yet been discovered based on 'gaps' in his table. He ordered the known elements in terms of their atomic mass in 1869; elements are listed in order of increasing atomic number in the modern version.
Why is the first ionization energy of aluminium is less than the first ionisation energy of silicon?
Al has atomic number 13, and silicon has atomic number 14. The extra electron that silicon has is in a 3p orbital. In simple terms the extra charge on the silicon nucleus contracts the electron shell, this increases the energy to remove an electron and also decreases the atomic radius. Al, first ionization energy 577.5 kJ/mol, atomic radius 125pm Si, first ionization energy 786.3 kJ/mol, atomic radius 110pm
Is The Ca plus 2 ion larger than the Ca atom?
Mg2+ is larger Now, as for the logic behind this problem...The first thing to do is recognize that Ca2+ (Calcium) has lost 2 of its electrons, therefore its valence electron structure is the same as Ar's (Argon). Ar is in the same row as Mg. The trend for atomic radii is increasing to the left and down. Atomic radius increases to the left because the atoms to the right have more particles in the nucleus than their counterparts to the left; thus, the electrons are drawn closer to the nucleus, and the atomic radius is diminished.
How is the periodic table arranged in terms of their ato mic structures?
The elements in the periodic table are arranged in order of increasing atomic numbers.
Rank these elements in terms of decreasing atomic radius?
Y (biggest) Fe Ga S F (smallest)
How did mendeleev arrange his version of the periodic table?
Mendeleev arranged his version of the Periodic Table in terms of ascending atomic weights and similar properties. Since it was first published in 1869, there have been updates and improvements.
What trends can be noticed in the periodic table in terms of atomic radii?
The general trend is a decrease in size as you move from left to right . This is apparent in periods 2 and 3 but in period 4 and above we have the transition metals and these have some exceptions. This is due to the fact that as we moves from left to right along a period while the nuclear charge increases we are also adding extra electrons but the effective charge is mainly affected by the inner core electrons that "shield" the outer electrons. The effective nuclear charge, the charge felt by the outer electrons, increases across a period thus causing a contraction in the shell.
How can you compare and contrast the periodic table that Mendeleev developed to the periodic table that Mosley organized?
Mendeleev used atomic masses to classify the element, where as Moseley classified the element in terms of atomic number, he suggested that chemical and physical properties are the functions of the atomic number Elements in the periodic table is classified as Metals, Nonmetal and Metalloids. Normally Group 1 to 12 are metals... Sayed Abdul Aziem Sayed_abd2007@hotmail.com
Who is the inventor of the periodic table?
Dmitri Mendeleev is generally credited, as he was able to predict the properties of elements which had not yet been discovered based on 'gaps' in his table. He ordered the known elements in terms of their atomic mass in 1869; elements are listed in order of increasing atomic number in the modern version.
How you calculate the relative atomic weight of uranium?
The atomic weight of an element is derived from the atomic masses of the isotopes of this element and from the percentage of these isotopes. The correct terms are: - atomic weight for elements - atomic mass for an isotope
Does the atomic radius increase as you go from left to right because principal energy levels are added?
It is not possible to give a sensible answer to this question because, in terms of the Periodic Table, the atomic radius DECREASES as you go from left to right! So the given reason would act in opposition to reality.
Is a sodium atom is larger than a silicon atom?
No. A cesium atom is larger both in terms of atomic mass and atomic radius.
Why is the first ionization energy of aluminium is less than the first ionisation energy of silicon?
Al has atomic number 13, and silicon has atomic number 14. The extra electron that silicon has is in a 3p orbital. In simple terms the extra charge on the silicon nucleus contracts the electron shell, this increases the energy to remove an electron and also decreases the atomic radius. Al, first ionization energy 577.5 kJ/mol, atomic radius 125pm Si, first ionization energy 786.3 kJ/mol, atomic radius 110pm
What is diameter in terms of radius?
diameter = 2 x radius
Is The Ca plus 2 ion larger than the Ca atom?
Mg2+ is larger Now, as for the logic behind this problem...The first thing to do is recognize that Ca2+ (Calcium) has lost 2 of its electrons, therefore its valence electron structure is the same as Ar's (Argon). Ar is in the same row as Mg. The trend for atomic radii is increasing to the left and down. Atomic radius increases to the left because the atoms to the right have more particles in the nucleus than their counterparts to the left; thus, the electrons are drawn closer to the nucleus, and the atomic radius is diminished.
