What is the advantages of using noble gases in our daily live?
477468
They are inert and so don't react with other elements/compounds.  Often used in situations where oxidation would occur if oxygen was present.\n\nExample:  Xenon is car head lights.  Get very hot and the filaments would oxidise (burn up) if oxygen was present.
917329
Realllllll Simply:\n\nCovalent molecules (atoms that make up the molecule) each contribute enough electrons (which are shared) to each other so that each atom thinks is has the nearest Noble Gas configuration. \n\nIonic molecules (the atoms that make up the molecule) transfer the electrons. One atom gains them and one atom loses them. Thus the atoms become ions (as in ionic bond), so they have charges.\n\nGet an "A".
706309
You want an atom that is easy to take one electron from, but hard to take a second.\n\nRemoving an electron from Sr or Mg would give them a configuration isoelectronic with the alkali metals.\nWhich don't hold onto their electrons very well,  and would have low ionisation energies.\nSo it's not a) or b).\n\n\nRemoving an electron from Na or K would give them a configuration isoelectronic with the noble gases.\nWhich would require a lot of energy to get the second electron from.\n\nHmm sodium or potassium ...\n \nSodium is a smaller atom than potassium, so it holds its valence electron tighter, and more energy is required to remove it.\nBut once it is isoelectronic with neon, it will have a much higher ionisation energy because it will be so much smaller.\n\nPotassium's first ionisation energy is lower than sodium's, but the second ionisation value (when it is isoelectronic with argon)\nwill be lower than the sodium ion's, when it is isoelectronic with neon.\n\nI'm going with sodium.
758277
the amount of electrons in an atom.\n\nif you're going to use noble gas configuration, you would use the noble gas and then continue the configurations.\n\nex. i want the configuration of... flourine (F)\nfor noble gas configuration i would say: (He) 2s 2 2p 6\n\nthe parenthasese is actually a bracket, and the numbers that are spaced should be in the upper righthand corner of the letter before it.
1000320
Helium, CO2, Hydrogen and various others.
697444
Advantages\n\nCan use when there is a scarce of electricity\nJobs for lot of people\nCan use in major research activities\n\n\nDisadvantages\n\nVery Dangerous if leaked\nCan cause thousands of human loss if handled incorrectly\nMay bore new types of diseases if leaked\nNeighbourhood people are always at risk\nNeed a large area to construct\nLot of people need to be on site for maintenance\nThreats from other countries if used inappropriately\n\nBYE
548851
Some pros to this energy source are: 1) Vast new source of energy 2) Fuels (mostly hydrogen) are plentiful 3) Inherently safe since a malfunction results in a rapid shutdown 4) No atmospheric pollution leading to acid rain or "greenhouse" effect 5) Radioactivity of the reactor structure, caused by neutrons, decays rapidly and can be minimized by careful selection of low-activation materials. There is basically only one con to these energy sources though. Scientists have not figured out a way to make it efficiently. At this point they have sustained a reaction at the break-even point, which essentially means they used as much energy as they created to make the reaction take place.
959515
advantages:\nYou can get a general idea of the shape of the molecule\nit gives a 3d representation of the molecule\n\ndisadvantages:\nif the molecule has double/triple bonds it doesnot give an accurate representation of sigma and pi bonds
138726
Mg more reactive than Al cuz it has lesser valence electrons to release,making it easier to achieve stable noble gas configuration
335683
Noble gases (or inert gases) are in group 8 of the periodic table, at least when I was at school, I think it is now known as Group 18 though.\n\nThere are 6 and they are:\nHelium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe) and Radon (Rn)\n\nThey all have an oxidation number of O, meaning that they have no empty shells in their outer energy level suitable to accept electrons, and therefore form bonds, with other elemnets.\n\nXenon is an exception though as XeF2, XeF4 and XeF6 are all known.  I don't think there are any compounds of the other noble gases.\n\nHope this helps.
321288
Alkaline earths are in the second column on the periodic table (Be, Mg, Ca, etc.)  They have two electrons in their outer (valence) shell, which they readily give away to form ions with a 2+ charge.  They are not as reactive as the alkali metals (in column 1), but are more reactive than most other elements.  (Reactive refers to how readily they will form compounds with other elements.)\n\nThe noble gases are He, Ne, Ar, Kr, Xe, and Rn.  They are stable because they have full valence shells.  For example, He has 2 electrons, so the first shell is filled, as it can only hold 2. He has 10 electrons, so with 2 in the first shell and 8 in the second, the valence shell is again full, since the second shell can hold up to 8 electrons.  And so on.  The third shell can also hold 8, so Argon's 18 electrons fill its three shells completely.  The fourth shell can hold up to 18 electrons, which is why Krypton has a full four shells with 36 electrons (2+8+8+18).
51223
Benefits !! \nHope this help...
147599
it's vital in organisms. hydrogens make up the three most important types of molecules to human beings: carbohydrates, proteins, and fats.\n\nthey are trying to develop cars that run on hydrogen fuel.
796417
Noble gases are inactive\nhalogens are very active\nLast one, ionization energy decreases\nlanthanide and actinide are the bottom 2 periods
1111390
Is this a test question you have to answer?  Increased oxygen provides the "fuel" for your body to function effectively.  Exercise and increased respiration increase blood circulation, providing more nutrients to reach the cells and more waste to be filtered out.  From these basic processes, many other benefits follow.  I'd have to think harder to give you more details - what are you trying to acheive?
932777
ok. To tell which elements are more metallic then others, It depends on the left over valence electrons that are attracted to the positively charged cations in a metal. To tell which elements are more active then others it is towards the right of the periodic table. Noble gases are non-reactive. To tell which atoms are bigger then others remember going from top to bottom in a group, atomic size increases, going from left to right across a period, atomic size decreases.(there is a pattern to this). \nI think if there are more valence electrons, the stronger the metallic bond is.
585929
If it were not for concerns about the health effects of\nradiation, nuclear energy would have developed quite\ndifferently.\nRadiation is not new. Although it was discovered and\nnamed as recently as 1896, we and our ancestors have\nlived with it since the beginning of time. The earth is\nnaturally radioactive, so is the air we breathe, the\nfood we eat and the ground we stand on. It is only\nwhen we are subjected to relatively large doses of\nradiation that it becomes a danger to life or health.\nModern science has allowed us to develop safe ways\nof using radiation, and of exploiting its properties for\nthe benefit of mankind. Many valuable applications\nhave been developed:\n􀁺 nuclear medicine, especially the use of X-rays\n􀁺 use of radiation to develop drugs for people with\ndiabetes, arthritis or high blood pressure\ntreatment of car tyres with radioactive materials to\nmake them more durable and puncture-resistant\nradioactive sources in photocopiers to stop the\npaper sticking together.\nThese are just a few examples. We benefit from a\nlarge range of products and services made possible by\nradioactive materials, often without even realising it.\nEverything in the world, from the air we breathe to\nthe cars we drive, is made up of atoms\nSome atoms are ‘stable’ – an ordinary carbon atom,\nwith six protons and six neutrons, will stay that way\nuntil the end of the universe unless something\ndramatic happens to it, such as being absorbed by the\nsun. Others are unstable – for example, their nuclei\nmay be too big to hold together – so they shake off\nparticles and surplus energy from their nucleus until\nthey become stable. The process of shaking off these\nparticles and energy is called ‘radioactivity’, and the\nparticles and energy which are released are known as\n‘nuclear radiation’. The process is often called\n‘radioactive decay’, since over time the radioactive\nmaterial breaks up and changes into other more stable\natoms, sometimes through several radioactive\nintermediate stages. The process can take fractions of\na second or billions of years depending on the\nradioactive material involved, but in each case the\nradioactivity of the material falls steadily.\nThere are different types of radiation, and not all\ninvolve radioactive decay. The type of radiation we\nare looking at in this booklet is ‘ionising radiation’,\nand includes artificially made X-rays (which do not\narise from radioactive decay). When this type of\nradiation bumps into other matter, it produces\nelectrically charged particles, known as ‘ions’.\nIonisation causes chemical changes in materials, and\ncan affect our bodies as well as the things around us.\nIn high quantities, ionising radiation can damage\nliving tissue and even destroy human cells. This can\nbe beneficial in some circumstances – for example,\nradiotherapy is used in the treatment of cancer, the\nradiation being used to kill cancerous cells, leaving\nother cells nearby relatively unharmed. In this sense,\nradiation is rather like a surgeon’s scalpel. Usedcarefully it can provide many benefits and can enable\nus to live longer, healthier, more comfortable lives,\nalthough it can be dangerous if misused.\nWhen we refer elsewhere in this booklet to ‘radiation’\nwe mean ionising radiation. However, there are nonionising\nradiations, such as low energy\nelectromagnetic radiation (which includes light, infrared,\nradio waves and electrical and magnetic fields\nfrom power pylons), which are not normally\ndangerous.\nThere are several types of ionising radiation, of which\nthe most important are:\n􀁺 α (alpha): streams of atomic particles (helium\nnuclei) made up of two protons and two neutrons\nwith a positive charge (+2). By atomic standards\nthese are quite big chunks of matter, so they are\nvery easily stopped. They cannot pass through\npaper, for example, or through the dead outer layer\nof our skin. However, if materials emitting alpha