How Many Neutrons Does the Element Iodine Have?

Iodine is a chemical element with the symbol I and atomic number 53. The name is from Greek ἰός (ios), meaning violet or purple, due to the color of iodine vapor. Iodine has 49 electrons, most of which reside in the innermost orbital, the 4d shell. This makes iodine very chemically similar to tellurium and thallium. Iodine's half-filled inner orbital gives iodine some properties more like halogens, which are in the same column in the periodic table, and diatomic iodine (I2), more than other elements in the same row.

Iodine is the heaviest element in the halogen group. Iodine vapor has a lilac color. In a flame test, iodine produces a greenish-brown color. In solution, iodine is moderately colored, ranging from yellow to dark brown, depending on the amount of iodine present.

Iodine has 29 isotopes, with mass numbers 114–142. The most common ones are 127I (half-life of 15.7 million years) and 131I (half-life of 8 days).

Iodine has 17 protons and 36 neutrons.

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The element iodine has a total of 53 electrons, with 37 of them being in the first shell, 8 in the second, 18 in the third, and so on. In terms of neutrons, iodine has a total of 74, with 20 in the first shell, 28 in the second, and 26 in the third. Therefore, the most common isotope of iodine has 53 electrons and 74 neutrons.

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The element iodine has 35 electrons and its least common isotope has 53 neutrons.

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Iodine is a chemical element with symbol I and atomic number 53. The heaviest of the stable halogens, it exists as a lustrous, purple-black metallic solid at standard conditions, but readily sublimes to form a violet gas. The element was discovered by the French chemist Bernard Courtois in 1811. It was named by Joseph Louis Gay-Lussac after the Greek ἰώδες (iodés), meaning violet or purple.

Most iodine is used for its radioisotopes and iodine-releasing compounds. These radioisotopes include some used in medical diagnosis and therapy, such as iodine-123 and iodine-131, and some used in nuclear power production, such as iodine-129. Iodine is also used in many industrial and agricultural chemicals, especially in dyes.

The abundance of iodine in the Earth's crust is about 50 parts per million, making it the 37th most abundant element. Seawater has approximately 60 parts per billion of iodine, making it the 60th most abundant element in seawater. The main commercial use of iodine is in the production of acetic acid and derivatives, which contain about 0.1% of iodine.

The element iodine has 27 isotopes, with mass numbers from 114 to 140. All of these are radioactive, with half-lives ranging from seconds to hours, except for iodine-127, which is stable. The isotopes with mass numbers 121 and 136 decay by electron capture to isotopes of tellurium. Mass number 125 is a synthetic radioisotope with a half-life of about 10 minutes, produced by fusion of two atoms of iodine-124.

The most stable isotope of iodine is iodine-127, with a half-life of 15.7 million years. This is also the longest-lived isotope of iodine, and the only one with a half-life over a day. Iodine-129 has a half-life of only 1.6 hours, making it the shortest-lived naturally-occurring isotope of iodine.

Iodine has 27 isotopes, with mass numbers from 114 to 140. All of these are radioactive, with half-lives ranging from seconds to hours, except for iodine-127, which is stable. The isotopes with mass numbers 121 and 136 decay by electron capture to isotopes of tellurium. Mass

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Iodine is a chemical element with the symbol I and atomic number 53. The heaviest of the stable halogens, it exists as a lustrous, purple-black metallic solid at standard conditions that sublimes readily to form a violet gas. The element was discovered by French chemist Bernard Courtois in 1811. It was named after the Greek goddess of the rainbow, Io, by the French Academy of Sciences.

Iodine has several radioactive isotopes, the most stable of which are 127I with a half-life of 1.57×10^7 years, 129I with a half-life of 1.57×10^7 years, and 131I with a half-life of 8.02 days. Several other iodine isotopes have been synthesized, including 100-117. The most common isotopes of iodine are 127I (27.73%), 128I (4.29%), 129I (36.04%), and 130I (31.93%).

The least stable isotope of iodine is 100I, with a half-life of only 53 seconds. This makes it the shortest-lived known isotope of any element.

The number of neutrons in an element's least stable isotope can give us clues about that element's behavior. For example, the element with the most stable isotope is lead, whose isotopes all have 82 or 84 neutrons. This stability is due to the "magic number" of 82 protons in the nucleus, which provides a strong repulsive force that overcomes the attractive forces between nucleons.

Iodine's stability, on the other hand, comes from a different source. Iodine's least stable isotope is actually relatively stable compared to other elements' least stable isotopes. This is due to the fact that iodine has a very strong nuclear force holding its nucleus together. This strong force is due to the fact that iodine has a higher than average number of neutrons in its nucleus.

Iodine's neutron number is important because it allows the element to have a large number of stable isotopes. This is due to the fact that the neutron number can be varied without changing the number of protons in the nucleus. This allows for a greater variety of stable isotopes, which is why iodine has more stable isotopes than any other element.

Iodine's neutron richness also allows for the element to be used

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Iodine is a chemical element with the symbol I and atomic number 53. The most common isotope of iodine is 127I, which has 54 neutrons. Iodine has a half-life of about 15.7 million years, which means that it is not radioactive and does not decay into other elements.

Iodine is a chemical element with the symbol I and atomic number 53. The heaviest of the stable halogens, it exists as a lustrous, purple-black metallic solid at standard conditions, but readily sublimes to a violet gas upon heating. The element was discovered by French chemist Bernard Courtois in 1811. He found iodine crystals in the ashes of seaweed from the coasts of Brittany.

Iodine has five isotopes with mass numbers of 127I (the most abundant), 126I, 124I, 125I, and 128I. All of these occur naturally except for 127I, which is radioactive with a half-life of about 15.7 million years. Naturally occurring iodine is found in the form of two isotopes, I-127, with a mass of 126.90447 u, and I-131, with a mass of 130.04), and their relative abundance is about 69.2% and 30.8%, respectively. The least abundant isotope of iodine is I-128, with a natural abundance of only about 0.001%.

The number of neutrons in an element's least abundant isotope can be determined by subtracting the element's atomic number from the mass number of the isotope. For iodine, the atomic number is 53 and the mass number of the least abundant isotope is 128, so the number of neutrons in I-128 is 128 - 53, or 75.

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Iodine is a chemical element with the symbol I and atomic number 53. The most common naturally occurring isotope of iodine is 132I, which has 74 neutrons. Iodine is found in small quantities in the Earth's crust, but it is mostly concentrated in the oceans, where it is a dissolved element in seawater.

Iodine is an essential trace element for many animals and plants, and is particularly important for the proper functioning of the thyroid gland. Iodine deficiency can lead to a number of health problems, including goiter, cretinism, and developmental problems in children.

Despite its importance, iodine is a relatively rare element. It is estimated that there is only about 25 grams of iodine in the Earth's crust, and about 0.45 grams in the oceans.

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Iodine is a chemical element with the symbol I and atomic number 53. The heaviest of the stable halogens, it exists as a lustrous, purple-black non-metallic solid at standard conditions that melts to form a deep violet liquid at 114 degrees Celsius, and boils to a violet gas at 184 degrees Celsius. Despite its relatively high atomic number, iodine is found in nature only as the iodide ion, I-, or, more rarely, in elemental form as atomic iodine, I, in areas where there is significance iodine geology.

Iodine has 43 isotopes with mass numbers 114 to 156, with iodine-153 (25%) being the most abundant. All but one of these are radioactive; they have half-lives ranging from 8.1 hours for iodine-133 to 154 years for iodine-129. The longer-lived, radioactive isotopes are used in medical imaging and as tracers in medical and industrial procedures. The only stable isotope is iodine-127 (100%), which is also the heaviest naturally occurring iodine.

Iodine dissolves readily in water to form hydroiodic acid (HI), giving a deep violet coloration that can be used for titration. It forms a charged complex, the polar bear, with water molecules at low concentrations. This interaction is responsible for the strong coloration of iodine solutions, and tends to cause yellowing of fabrics and paper in contact with those solutions.

Iodine is the least abundant of the stable halogens, found in the Earth's crust at an average concentration of 65 parts per million (ppm), compared to 82 ppm for chlorine and 78 ppm for bromine. This is significantly lower than the average concentration of any other element, except for potassium, sodium, and lithium. However, iodine is concentrated in seawater, with an average concentration of 0.5 ppm, compared to 0.045 ppm in fresh water. This is because iodine is highly soluble in water and is concentrated in seawater by evaporative processes.

Iodine occurs naturally in the form of two isotopes: iodine-127 (100%), and iodine-131 (99.99%). Iodine-131 is radioactive with a half-life of 8.02 days, decaying to xenon-131. It is used in medical imaging and in the treatment of Thyroid cancer. Iodine-127 is stable, with a half-life of over

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The element iodine has a total of 53 protons in its nucleus. However, the number of neutrons in the nucleus can vary. The most common man-made isotope of iodine is iodine-131, which has a total of 131 neutrons in its nucleus. Other common isotopes of iodine include iodine-129 (which has a total of 127 neutrons in its nucleus) and iodine-135 (which has a total of 135 neutrons in its nucleus).