What is beryllium's normal phase and what element family does it belong to?
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It is a solid metal of the alkaline earth family.
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...
38819
Transition metal.\n\nName: Copper \nSymbol: Cu \nAtomic Number: 29 \nAtomic Mass: 63.546 amu \nMelting Point: 1083.0 °C (1356.15 K, 1981.4 °F) \nBoiling Point: 2567.0 °C (2840.15 K, 4652.6 °F) \nNumber of Protons/Electrons: 29 \nNumber of Neutrons: 35 \nClassification: Transition Metal \nCrystal Structure: Cubic \nDensity @ 293 K: 8.96 g/cm3 \nColor: red/orange
421190
Element #18 (Argon) is a member of the noble gases (Family 8).  All elements in this family contain a full outer orbit of electrons making them stable and unreactive.  The elements surrounding it (ie 15-17) are all trying to obtain a full outer orbit to be like the noble gases by sharing and borrowing electrons from surrounding elements.
714217
The metal which is the furtherest to the right-hand top corner of the periodic table will be the most electronegative. Those who said fluorine didn't read the question properly because you are asked for a metal and fluorine, although the most electronegative 'element', is not a metal. In answering this question, I'm going to assume that the metalloids aren't included and not a subset of the cagetory of metals. The most electronegative metal would be aluminium (13). Have a look at the periodic table, it's the element which is closest to the top-right hand side but is still classified as a metal.
784694
All s, d, and f elements are metals.\n\nBlock p includes metals, non-metals, and some metaloids in between.  Metals include Aluminum and down in that group.  Tin and down in that group. and Polonium in its group.  So the lower left corner of the p block are metals and the upper right corner are non-metals.  Boron, Silicon, Germanium, Antimony, and Tellurium, tend to be considered metaloids.  (Depends on who you read.)
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Follows the periodic table trend in halogen elements. Lower atomic weight - gas fluorine, chlorine - liquid bromine - solid iodine - higher atomic weight. Thats just the way it is babe!
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You left out the "f" orbitals.\n\nFollow the increasing atomic numbers as you move across the periodic table, and you'll see that you have to go through the lanthanides before you go to the "d" block.\n\nmercury is  [Xe] 6s2 4f14 5d10
861365
I think that the proper name is Beryllium.\n\nThe usual name is Beryl = Be3Al2Si6O18 (!!!) It's an oxide (of Si, Al and Be - only 5%).\n\nOriginated from Mainly granitic pegmatites. \n\nFrom the ancient Greek, beryllos, signifying a "precious blue-green color of sea water" stone, but through later usage, applied only to beryl. \n\nOthers names:\n   Aquamarine - blue  \n   Emerald - green  \n   Goshenite - colorless  \n   Heliodor - yellow  \n   Morganite - pink
852308
Because they have a low atomic number Li (Z=3) Be (Z=4). Theoretically, they should give one electron in the case of Li and 2 electrons in the case of Be giving rise to ions Li+ and Be ++. But since their small sises the electron are attached to the nucleus and difficult to remove. So , the lithium ha so their properties than the other alkali metals
930659
Just in general\n\nAlkali Earth Metals- Pretty reactive they are found in many compounds\n\nBoron group- Low reactivity\n\nCarbon group- More reactive then boron group but still pretty low\n\nNitrogen group- More reactive then Carbon group\n\nOxygen group- Very reactive oxygen has an unually high affinty for electrons relative to where it is on the periodic table\n\nHalogen group- Even more reactive than oxygen th&#92;ey have very hi\naffinity for electrons\n\nNoble gases- Basically inert, they have a full outer orbital of electrons and will only react in rare cases such as with flourine
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try here:http://rds.yahoo.com/_ylt=A0oGkjr5altFbCIATYFXNyoA;_ylu=X3oDMTE2aWNrczNxBGNvbG8DdwRsA1dTMQRwb3MDOARzZWMDc3IEdnRpZANERlg1XzMw/SIG=12odtnv12/EXP=1163705465/**http%3a//www.theodoregray.com/PeriodicTable/Elements/013/index.s7.html
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The nonmetals are halogens, noble gases and the following elements in order of atomic number (nonmetals as chemical series):\n\nhydrogen (H) \ncarbon (C) \nnitrogen (N) \noxygen (O) \nphosphorus (P) \nsulfur (S) \nselenium (Se) \n\nhere's an example:\n\nhttp://en.wikipedia.org/wiki/Periodic_table_%28metals_and_non-metals%29
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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.
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Column 1 on the left is alkali metals (not counting hydrogen).\n\nColumn 2 is alkaline earth metals.\n\nColumns 3-12 are transition metals\n\nColumn 13 is the Boron Group\n\nColumn 14 is the Carbon Group\n\nColumn 15 is the pnicogens\n\nColumn 16 is the chalcogens\n\nColumn 17 is the halogens\n\nColumn 18 is the noble gases\n\nThe ones down on the bottom are the rare earth metals... top row is the lanthanide series, bottom row the actinide series
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a) Ru - ruthenium\nb) S - sulfur\nc) Ir - iridium; with an incomplete d-subshell, it must be a transition metal\nd) Sb - antimony
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how far it is from the edge of the periodic table. i.e., Francium has a charge of -1 because to get it to the noble gases it has to gain an electron. on the other hand, lithium would need to lose an electron to make it happy, giving it a charge of +1. Same concept for all elements.exclude scandium's period thru zinc's, as they are very different. Carbon's group is able to go either way, as it is equidistant from the noble gases. email me if you have any more questions.