Which noble gas has the same electron configuration as the anion in the compound aluminum bromide?
813548
The answer is a) Krypton.\n\nThe bromide anion exists as Br-.\nWith the single negative charge, you know that it has an extra electron, therefore it's electron config is like the noble gas nearest to it on the periodic table: krypton.
3803
Neon won't form any stable compounds because it is too small to accommodate 8 fluorine ligands and, unlike the heavier noble gases, cannot use empty d-orbitals to rearrange the electron configuration.\n\nHeavier noble gases can form fluorine compounds which can be kept stable under certain conditions.
148525
Do you mean what where are the d sublevels? If you do they are the transition metals.  But i do not think that is your question. Do you mean the fourth row? That would be the latest last noble gas configuration then s2 of next level up then d2 of same level of last noble gas. I hope it helped. Maybe you should clarify your question.
337603
Here is the answer.. Just remember periodi table...\nElements on left most side are electro positive and elements on right most are electro negative. (The last row is nobel gases..so leave it)\nNow Cl- belongs to right most side... its more electro-ve\nRb, Ca are on left side.... they are electro positive(They will give  electron with out much force)\nSi, S are in middle-- their properties are in between...\n\nThats it!
1047499
If it existed, it would be boron pentafluoride, but as far as I know, this is not a stable molecule.\n\nAre you sure you don't mean BrF5 (bromine pentafluoride), which does exist as a stable molecule?
559636
Aargon, Helium. Noble gases are all monoatomic. Gases of Group 8 in the periodic table that is. But as you go down the group, radioactive properties start to develop, like for Radon.
734854
I'm going to cheat a little bit in both cases by just referring back to the nearest noble gas.  That itself may be acceptable for your purposes (it's how most chemists list them because things past that point are usually of no interest)... if you need, I'll pass on the underlying noble gas configuations too.\n\n13:  [Ne] 3s2 3p1\n33:  [Ar] 4s2 3d10 4p3\n\nBasically, the electrons usually fill up the shells just as you see the elements arranged on the periodic table.  Group 1 and 2 (the two columns on the left) are the s shell, and the number of the s shell is indicated by the row number.  Group 13 through 18 (the six columns on the right) are the p shell; its number is also the same as the row number.  The middle stretch are d orbitals, and they're so expensive energetically that the ones on each row are orbitals from one shell down.  That chart is handy for all kinds of things!\n\nHope that helps!
146528
27=13 protons + 14 neutrons.  For aluminium always have 13 protons (the atomic numbers), otherwise will be another element.  Number of electrons, it is not anion just the alumnium in the metallic state will be the same as atomic number, in this case 13.
458583
aluminum has 3 valence electrons
887306
Name one of the "Noble gases"?
948794
protons is the atomic number\nvalence electrons corresponds to this:\nGroup 1 (I) (alkali metals) :1\nGroup 2 (II) (alkaline earth metals) :2\nGroups 3-12 (transition metals) :1 or 2\nGroup 13 (III) (boron group) :3\nGroup 14 (IV) (carbon group) :4\nGroup 15 (V) (nitrogen group) :5\nGroup 17 (VII) (halogens) :7\nGroup 18 (VIII or 0) (noble gases) :8\n\n\nEvery element in the top row (the first period) has one orbital for its electrons. All of the elements in the second row (the second period) have two orbitals for their electrons. It goes down the periodic table like that. At this time, the maximum number of electron orbitals or electron shells for any element is seven.
921116
I'm not directly giving you the answers, you have to know how to do this stuff, but I'll give you the process to get to each.\n\n9: Americium and Curium (wikipedia!)\n\n10: Potassium ion wants to be like the noble gas closest to it (the one right before it), so it loses 1e- to get there and be K+.  If that's not a choice, then look for another ion, positive or negative, that adds up to the electronic configuration of the aforementioned noble gas. (1s2 2s2 2p6 3s2 3p6), 18 total e-'s...\n\n11: Mg is in column 2, things in the same period tend to be chemically similar.  Find the other one in the choices that's in that column\n\n12: U235 and U238 are isotopes, same atomic number, different weight.  If you change the number of protons, you change the atomic number, so that wouldn't be U anymore.  Changing electrons can make ions, but not change weight.  So different number of neutrons for the same element makes an isotope.\n\n13: Same explanation as above, it'll also be Hydrogen's atomic number because it's an isotope.\n\n14: shell 2 contains the 2s and 2p subshells.  2s can hold 2 because it's an s orbital.  2p can hold 2 per p orbital, and a p subshell has 3 p orbitals, so 6.  Total would then be...\n\n15: If an atom loses electrons, it's LOSING -1 per electron lost, so it's becoming more positive.\n\n16: Which element in that list only has 1s shell? Which one has a  stable ion as just a proton or with a configuration like Helium (1s2)?\n\n17: Inert elements are on the far right of the periodic table.  They are inert because they have 8 valence (outer shell) electrons (or 2 in Helium's case) so they can't take anymore and are stable.  Look at your periodic table or count up electrons for each of those atomic numbers.  Only one of them will have 8 in the outer shell...
905246
Yes.  You just begin to take electrons away from the outermost, least stable orbitals.  In this case the first two electrons will come from the 4s2 shell, and then the one from the 3d.  This will leave you with just [Ar], which is a noble gas, and if you remember back to the beginning of chemistry, elements become ionic (gain or lose electrons) because they all wish to achieve this noble gas configuration.
983415
D) reducing agent\n\nBr2 is neutral,whereas Br- is negatively charged (There has been an addition on of electron).Electron gain is reduction.So Br2 has been reduced.\nHence Sodium bisulfite is a reducing agent.
174730
You must be asking about the families on the periodic table.  The group that gains one electron is the Halides, or group 7A.  These contain Fluorine, Chlorine, Bromine... The group that gains two electrons is the Oxygen group, or group 6A.  The group that steals one electron would be the same as gain one electron.  But the group that loses one electron is the Alkali metals, group 1A.  And the Group that loses two electrons is the Alkaline Earth Metals, group 2A.  Finally, the group that never reacts is the nobel (or inert) gases, group 8A.
762215
Noble Gases:  He, Ar, Ne, Xe\nHalogens:  F2, Cl2, Br2, I2, At2\nOthers:  N2, O2
269322
1. All the members of the noble gases have a full shell of valence electrons, so they don't easily bond with other atoms.\n\n2. Because of the full shell, the noble gases have very weak intermolecular forces (IMF's), so they all have very low melting and boiling points. Helium actually doesn't become a liquid at normal atmospheric pressure until you get down to 4.22 K (-452 degrees Fahrenheit).\n\n3. They don't. Well, not usually. The larger noble gases (Krypton and Xenon) will bond with others, but only when using an expanded octet, in the d orbital. This makes compounds such as xenon tetrafluoride, XeF4. However, Helium and Neon will not react with anything, as their ionization energy is extremely high and their electron affinity is very low.\n\nNOTE: The answers above me are WRONG. Noble gases definitely do not form diatomic compounds. They are confusing the noble gases with the halogens, the elements that are in the second to the right column on the periodic table. It took all the way until 1962 for a chemist to synthesize a true noble gas compound, Xe[PtF6]- (xenon hexafluoroplatinate).\n\nEDIT: Tarangoyal, I'm reporting you for plagiarism. That answer is virtually identical to the first answer. There's no way that's a coincidence. You even made the same mistakes.