give the electron distributions in Magnesium atoms and magnesium ions how do these electrons constitutions differ
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Secondary School Chemistry 5+3 pts
Show the electron distribution of a magnesium atom and a magnesium ion diagrammatically and also give their atomic number
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magnesium-24 atomic no
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Electron distribution of a magnesium atom and ion.
When the number of protons and electrons are not equal in an atom, it is called ion whereas if both are equal it is called an element.
The atomic number of elements represents the number of electrons and the number of protons present in it.
Accordingly, the atomic number of magnesium is 12. It means that it contains 12 electrons and 12 protons. Thus it is called a magnesium atom.
On the other hand, as the magnesium atoms due to valency 2, donates 2 electrons to bind with other atom and forms new product. Thus as magnesium donates 2 electrons, it becomes ion and has 10 electrons.
Thus the electronic distribution of magnesium in the form of atom and ion is as follows
Magnesium atom : 2,8,2
Magnesium ion: [2,8]^{2+}
The atomic number of both ion, as well as the atom, is 12.
The electron distribution of a magnesium atom and a magnesium ion diagrammatically is given in the attachment.
Answer:
Diagram of a helium atom, showing the electron probability density as shades of gray.
The atomic radius of a chemical element is a measure of the size of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding shells of electrons. Since the boundary is not a well-defined physical entity, there are various non-equivalent definitions of atomic radius. Three widely used definitions of atomic radius are: Van der Waals radius, ionic radius, and covalent radius.
Depending on the definition, the term may apply only to isolated atoms, or also to atoms in condensed matter, covalently bonding in molecules, or in ionized and excited states; and its value may be obtained through experimental measurements, or computed from theoretical models. The value of the radius may depend on the atom's state and context.[1]
Electrons do not have definite orbits, or sharply defined ranges. Rather, their positions must be described as probability distributions that taper off gradually as one moves away from the nucleus, without a sharp cutoff. Moreover, in condensed matter and molecules, the electron clouds of the atoms usually overlap to some extent, and some of the electrons may roam over a large region encompassing two or more atoms.
Under most definitions the radii of isolated neutral atoms range between 30 and 300 pm (trillionths of a meter), or between 0.3 and 3 ångströms. Therefore, the radius of an atom is more than 10,000 times the radius of its nucleus (1–10 fm),[2] and less than 1/1000 of the wavelength of visible light (400–700 nm).