Isotopes

In an analogy, think of a baby's building blocks. Stock the blocks one on top of another. Eventually the tower of blocks becomes unstable and fall over. Radio-activity can be thought of in the same way. Protons( & Neutrons) stacked 'one on top of another'' become unstable when there are too many of them, hence the atom disintegrates(falls over). This is radio activity a larger atom breaking down into smaller atoms with the release of energy and particles.

Bromine is the only nonmetallic liquid element. It is a heavy, mobile, reddish-brown liquid, volatilizing readily at room temperature to a red vapor with a strong disagreeable odor, resembling chlorine, and having a very irritating effect on the eyes and throat; it is readily soluble in water or carbon disulfide, forming a red solution, is less active than chlorine but more so than iodine.

It unites readily with many elements and has a bleaching action; when spilled on the skin it produces painful sores. It presents a serious health hazard, and maximum safety precautions should be taken when handling it.

Much of the bromine output in the U.S. was used in the production of ethylene dibromide, a lead scavenger used in making gasoline anti-knock compounds. Lead in gasoline, however, has been drastically reduced due to environmental considerations. This will greatly affect future production of bromine.

Bromine is used in making fumigants, flameproofing agents, water purification compounds, dyes, medicines, sanitizers, inorganic bromides for photography,etc.

Organic bromides are also important.

Bromine is prepared by a method which comprises contacting hydrogen peroxide with an aqueous solution containing bromide ion and rapidly removing the bromine as it is formed. This method is particularly suitable for obtaining bromine from seawater, using the conventional intermediate, bromosulfuric solution.

Hydrogen-2 is commonly referred to as deuterium, in addition to that it is known as Deuterium-1

Number of neutrons = Mass number - atomic number = 23 - 9 = 14

Differences between uranium isotopes: natural isotopes (U-234, U-235, U-238) and the artificial isotopes; differences in atomic mass; differences in the number of neutrons; differences of the half life; differences in the emitted radiations (type, energy, percentage); differences in the decay chain; differences in the technological importance; etc.

elements are isotopes, when different atoms of the same element have different number of neutrons

An example with a zinc isotope: 81Zn (mass number as superscript before the chemical symbol)

If it was fully radio-active at the beginning, after 5 hrs it is 50%, at 10 hrs it is 25%, at 15 hrs it is 12.5%, and at 20 hrs it is only 6.25% as radioactive as it was at the beginning.

The half-life of carbon is roughly 6000 years. That means that every 6000 years, the amount of Carbon halves. Therefore, in a million years, the amount of carbon-14 would be so low that it would be extremely difficult to determine the exact age of the shell. So radioactive elements of longer half-lives, such as Uranium-238(half-life of 4.9 billion years) are used to date older objects.

in russia

According to an Answers.com search for "Gustav Kirchhoff", the spectroscope was invented in Germany.

Sodium-23 and Sodium-22 are two isotopes of sodium. Na-23 is the only stable isotope of Sodium. Na-22 is one of the two isomers (the other of which is Na-24).

Chlorine has isotopes with mass numbers ranging from 32 to 40. There are two principal stable isotopes, 35Cl (75.77%) and 37Cl (24.23%), giving chlorine atoms in bulk an apparent atomic weight of 35.5 g/mol.

Different isotopes of the same element are usually considered not to be chemically different. The atoms of different isotopes of the same element differ only in mass, not in their electronic structure, and it's the electronic structure of an atom that determines its chemical properties.

A partial exception: hydrogen and its isotopes deuterium and tritium. Because the isotopes of hydrogen weigh twice and three times as much respectively, but have the same electronic structure, while they take part in the same chemical reactions, the reaction rates differ.

The stable carbon isotopes are carbon-12 & carbon-13. There are several other unstable isotopes.

Half-life (in units of time).
Half-Life is the rate of radioactive decay, measured in time. The half life gives the time it take for half of the radioactive atoms in a system to decay. Fore example, if you have 10 grams of carbon-14, it will take 5730 years for half of it to decay, giving you 5 grams. In another 5730 years, you'll have 2.5 grams left, etc...
Isotopes decay at an exponential rate. A half-life is the time that half of the population of an isotope will decay. The measure is a statistical probability and is more accurate when a large population is observed. The term half-life is applied to describe a property of a given isotope (i.e. the half-life of Carbon 14 is 5730).
half life

Isotopes have the same number of protons, but a different number of neutrons (they are the same element however).

Isotones have different numbers of protons, but the same number of neutrons, and are thus different elements.

It emits an electron and an antineutrino and increases by one in atomic number while ending up with one fewer neutrons, or it emits a positron and a neutrino and decreases by one in atomic number while ending up with one more neutron. In both cases the total number of protons and neutrons remains unchanged, and the number of orbital electrons will eventually change to match the new atomic number.

Yes Neon has isotopes from 16-34.

an isotope is a different form of that element. They just have different mass numbers/ atomic mass. Therefore having the same characteristics of the atom except for an increased/decreased number of neutrons. Isotopes have the same atomic number as each other.

There are about 33 isotopes of arsenic. Only one of them is stable, and that's 75 As 33. All the other isotopes are synthetic.

An atom of Sodium weighs the same as 23 protons.

subtract the number of protons from the number of electrons.

The above answer does not answer the question!!

Radioactive substances in the environment can harm cells, damage DNA, and cause cancer. If we take gamma rays, they kill living cells upon contact as they have high penetration power. But this doesn't mean that they are totally dangerous and can't be used by living things. We have to see the level of radioactive isotopes used in order to say they are dangerous to others. Low levels of radioactive isotopes is used in a sample and it becomes a tracer by which to detect molecular changes. Melvin Calvin and his coworkers used Carbon 14 to detect all the various reactions that occur during the process of photosynthesis. Radioactive isotopes are being used largely in the medical field. The high level of radioactive isotopes (radiation) has been used to sterilize medicine and dental products for many years. Now, it can be used to sterilize the US mail and other packages to free them of possible pathogens such as anthrax spores. In addition to this, cancer treatment through radioisotopes to destroy only cancer cells, with little risk to the rest of the body is another important use of radioactive isotopes.