in periodic trends and lattice structure, why does O, C, Na,S, fe, & diamond have low or high boiling points.?
953247
the previous answer is deficient on the following points...\nelemental C has the atoms held together by covalent bonding\nNa, being a metal, has metallic bonding, not ionic. Ionic bonds occure BETWEEN a metal and a non metal such as Na with Cl.\nMetallic character decreases as you cross the periodic table, and increases as you go down the periodic table, so Na is more metallic than Fe\nnon metallic character does the opposite..\nSo from the list above, metallic character would be Na > Fe >C  > S > O\nNa is a metallic lattice while O2 exists as discrete molecules\nHope that helps
7062
it's outer electrons are in the d orbitals.  the s and p orbital elements (the first 2 columns and the last 6) are the more reactive ones that really want to form octets. none of those d-block transition metals are all that reactive, especially the ones in the middle there where gold is.
1018878
Lithium boils at 1342 C.\nhttp://www.lenntech.com/Periodic-chart-elements/Li-en.htm
858037
carbon. because it can bond with more elements than any other, including itself.\n\nhence life is made out of it.\n\nit is extremely hard (diamond) and can be extremely soft (graphite). \n\nit doesnt have a melting point.
778725
Consider one cube of the lattice.  there will be one atom on each corner.\n\nWith BCC there will be one atom in the centre of the cube.\nWith FCC there is one atom in the centre of each face of the cube - a dice with one spot on each face.\nIt's a very long time since I did this, but I think steel is BCC at normal temperatures and chnges to FCC on heating.
19979
Well the lattices in the ionic compounds are formed by two spiecies. The cations and the anions. These being oppositely charged attract each other with a great magnitude of force. \n\nNa+  Cl-  Na+\nCl-  Na+  Cl-\nNa+  Cl-  Na+\n\n    but in metals the Metals are all arranged in a lattice. In this lattice the metal kernels(inner electrons not includeing valence electrons and the nucleus) that are positively charged are all arranged in space. The electrons move freely in the lattice spaces. These hold up the metal kernels together. They move around in a manner such that the totla charge distribution on each kernel remains the same. Thus you see there is a difference in the lattices of metals and ionic solids. Hence we  get the maleability of the Metals
975847
Crystal structure depends primarily on the size of the ions. The Cs+ ion has one closed electron shell more than the Ag+ ion. Therefore more Cl- ions can be packed around a Cs+ ion than around a Ag+ ion.\nCompare these two structure to see what I mean:\n http://cst-www.nrl.navy.mil/lattice/struk/b1.html          AgCl\n http://cst-www.nrl.navy.mil/lattice/struk/b2.html         CsCl
1037023
Water, when heated from a solid to liquid state, but ultimately in a gaseous state it again expands.  It still obeys all the laws of chemistry, but the bonds just arrange themselves in a more space efficient manner in liquid than in solid form.\n\nAnd moses with a P, no metals exist with the properties you say.  It is physically impossible, sorry man, but I'm a biochem major and it's my job to know what stuff does under different stresses, and nothing does what you claim.  However, if you do have a material that does this, get in touch with me, we'll talk to the patent office, and we'll license it out to companies for billions of dollars.
907805
Elements in the same column (group) will have similar chemical properties since chemical properties are derived from the interaction of valance electrons. All groups have the same number of valance electrons:)
149062
The question is not clear.  Are you asking what a crystal is?  Are you asking what the different crystal structures are?  Are you asking for the characteristics of crystals in general?
5530
Arsenic is the metal, but at temperatures much lower than its melting point (not boiling point).  It sublimes at 614 degrees C and melts under pressure at 817 degrees C.\n\nAlthough Iodine has a metallic luster, it is not a metal.  It sublimes (evaporates) near its \nMelting Point of 114 degrees C.\n\nSee the reference below:
948227
a crystal structure is a unique arrangement of atoms in a crystal. A crystal structure is composed of a unit cell, a set of atoms arranged in a particular way; which is periodically repeated in three dimensions on a lattice. The spacing between unit cells in various directions is called its lattice parameters. The symmetry properties of the crystal are embodied in its space group. A crystal's structure and symmetry play a role in determining many of its properties, such as cleavage, electronic band structure, and optical properties.\n\n\nThe crystal structure of a material is often discussed in terms of its unit cell. The unit cell is a spatial arrangement of atoms which is tiled in three-dimensional space to describe the crystal. The unit cell is given by its lattice parameters, the length of the cell edges and the angles between them, while the positions of the atoms inside the unit cell are described by the set of atomic positions (xi,yi,zi) measured from a lattice point.\n\nFor each crystal structure there is a conventional unit cell, which is the smallest unit that has the full symmetry of the crystal (see below). However, the conventional unit cell is not always the smallest possible choice. A primitive unit cell of a particular crystal structure is the smallest possible unit cell one can construct such that, when tiled, it completely fills space. This primitive unit cell does not, however, display all the symmetries inherent in the crystal. A Wigner-Seitz cell is a particular kind of primitive cell which has the same symmetry as the lattice.\n\n\nfor further clarifications go to the site listed
103373
The atomic and molecular structure of each mineral determines the crystal shape. Each mineral is composed of a specific molecular compound, and those molecules arrange themselves in an ordered fashion based on their structure that will form a crystal.  \n\nThese regular and repeating groups of molecules and atoms form a unit that is known as a lattice. There are 14 lattice groups (Bravais lattices), which fall into six (some crystallographers use seven) different crystal systems. Each crystal system includes the different rotation and reflection symmetries around a fixed lattice point. \n\nTo make this all more confusing, and to the horror of most mineralogy students there are also 32 different crystal classes. Each crystal class is a different and unique set of symmetrical forms.\n\nTo see illustrations of Bravais Lattices go here:\nhttp://hyperphysics.phy-astr.gsu.edu/hbase/solids/bravais.html\n\nFor a more detailed explanation go here:\nhttp://dave.ucsc.edu/myrtreia/crystal.html#INTRO
30469
If you look at a periodic table you will see the number of protons in an element, these +ve particles are balanced by an equal number of -ve charged electrons.  The cloud theory of electrons is a bit confusing but if you consider the electrons to orbit the nucleus in set patterns/orbits it becomes a bit easier to explain (and the model works at a basic level).\n\nThe inner orbit of an atom can hold 2 electrons, if you look at hydrogen you will see that it has one electron, this means that it has a vacancy in that orbit - and it will want to fill this vacancy to become stable, this can be filled by sharing an electron with another atom perhaps another hydrogen atom to form 2H the normal format for gaseous hydrogen in the atmosphere.  \n\nOxygen has 16 electrons in 3 orbits - inner = 2 (full) layer 2 = 8 (full) layer 3 = 6 (2 vacancies).  It will want to fill these vacancies to become more stable.  Oxygen does this by combining with 2 hydrogen atoms each of which has a single atom to form H20.\n\nIf you look at the periodic table you will see that the materials in each vertical row have the most reactive material at the top going down to the least reactive at the bottom.  In general atoms with a single electron in its outermost orbit or an outermost orbit with a single vacancy (such as Hydrogen) will be more reactive than an atom with two electrons or two vacancies in its outermost orbit.  This can be proven by experiment and working out the number of electrons in the outer orbits.\n\nGenerally atoms combine together to form stable unreactive materials. Iron oxide (Fe02) is a stable natural form of Iron, we remove the oxygen to produce Iron products, but iron is fairly reactive in its Fe form and will naturally recombine with O2 to revert back to its stable form FeO2.
402942
An atom is stable when it has a full valence (outer) electron shell.  For the first row on the periodic table, the outer (and only) shell can hold up to 2 electrons.  For the next two rows, the atoms' outer shells can hold up to 8 electrons.  The next two can hold up to 18.\n\nAtoms like sodium, in column 1 of the periodic table, have one electron in its valence shell.  It is very reactive, since it wants to get rid of this extra electron so that its outer shell can be full.\n\nAtoms like chlorine, in the second last column, have one electron missing from their valence shells.  They are also very reactive, since they want to accept an electron to fill the outer shell.\n\nNoble gases are almost totally unreactive, since they have the unique property of having full outer shells without having to give away or accept any electrons.
121386
http://www.chemistrycoach.com/periodic_tables.htm#Periodic%20Table%20Songs\n I hope it helps you
467694
When atoms combine by covelant or ionic bonds, the resulting compound has properties that are different from those of the atoms.  For example, Sodium is a soft and very reactive metal, and Chlorine is a yellow-green poisonous gas, but when they combine ionically, the result is table salt: neither reactive nor poisonous.  This has to do with how the electrons are situated at the atomic level.  Often, bonding stabilizes the electrons and makes the resulting compound less reactive, which is why water will not react the way Hydrogen or Oxygen do.