how can you calculate the number of electrons?
108641
if you want to know the number of electrons for a sample, you need to calculate the molarity of the substance and then multiply by the number of electrons that that element has. \n\nFor example:  you have 18 grams of water.  I picked that amount since the molecular weight of water is 18grams/mol.  (the mol weight of oxygen is 16 and 1 for hydrogen H2O =18grams of water is one mol of water)  A mol of sample is 6.02214199 × 10^23.  Yes thats a big number but its just like saying I have a dozen of something, a mol is a quantity of something.  I could have a mol of cars which would be 6.02x10^23 cars.  The reason we use such a big number is that there are so many atoms in even a tiny sample.  \n\nAnyways, 18 grams of water is one mol of water which is 6.02x10^23 molecules of water.  Now we need to figure out how many electrons are in one molecule of water and multiply it by the number of water molecules.  Oxygen has 8 protons and thus 8 electrons, hydrogen has 1 electron each, so a water molecule has 10 electrons.  So 6.02x10^23 times 10 more would equal 6.02x10^24 electrons in 18 grams of water.  (lots)
194958
The atomic number of nickel is 28 which is the number of electrons.  It is also the number of protons in its nucleus\n\nhttp://periodic.lanl.gov/default.htm\n\nhttp://en.wikipedia.org/wiki/Atomic_number
737924
You can figure it out.\n\nIf a neutral atom of zinc has an atomic number of 30, and a mass number of 65, then it has 30 protons, 35 neutrons, and 30 electrons.\n\nProtons and neutrons are found in the nucleus.\nSo, draw a circle. Write "30p+" and "35 n" inside it.\nThis represents the nucleus.\n\nIn Bohr's model, electrons orbit the nucleus at specific energy levels. The first level holds up to 2 electrons.\nThe second holds up to 8.\nThe third holds up to 8.\nThe fourth holds up to 18.\nWe use dots to represent electrons.\n\nDraw a ring around the nucleus.\nAdd two dots to the ring, usually at noon and 6:00.\n\nDraw another ring around the first one.  Draw eight dots: two at noon, two at 3:00, two at 6:00, and two at 9:00.\n\nContinue adding rings and electrons.\nYou should end up with twelve dots in the outermost ring.\n\n(Which doesn't correspond with the  Lewis diagram for zinc, but that's  another story....)
968601
this is what you do to find how many neurons and element has k What you do is Like if you look at tthe periodic table like the element Uranium and subtract the atomic mass from the atomic # and thats how you find out how many nuerons there are in an element and to find the electrons what you do is if you see a # on the right side of the element if it has  a # by it with a +/ -you do the oppisite of the sign taht is by the # like in Uranium since the atomic # is 92 subtract the # that is right next to the Symbol if it is a + and if it is a - then you would add it
236619
There are several steps used to do Lewis Dot Structures.\n1) Determine the number of electrons required ( in this example there are 40 electrons required)\n2) Determine the number of valence elestrons ( there are 6 +6+6+6+6 = 30 ), however since you have a -2 formal charge there are 2 extra electrons, which means you have 32\n3) Determine the number of bonds (subract the number of valence electrons from the total required and then divide by 2) ie: 40 - 32 = 8/2 = 4 bonds\n4) write the atom symbols on this page ( in this example you're going to write Se in the center with one Oxygen on every side)\n5) connect with the number of bonds that were calculated\n6) fill in electrons until all the atoms have conformed to the octet rule except for hydrogen\n7) then count the number of electrons shown to check your work\nAnswer: 1 bond connects each Oxygen to the one Selenium and each Oxygen is going to have six dots on the outside and Selenium is going to have four dots.
254116
"mathematician" is correct.\n\nAny atom of a given element will have the same number of protons in its nucleus.  If the atom is neutral (i.e. has no charge), then it will have the same number of electrons as protons.\nHowever, the number of neutrons in the nucleus can vary slightly from atom to atom for a given element.  Atoms of the same element but with different numbers of neutrons in their nucleus are called isotopes.  With a greater/less number of neutrons, the over all atomic weight of the atom will varry.  By taking into account the naturally occuring percentages of each of these isotopes of a given element, we can obtain the average atomic mass of all the atoms of that element.\n\nCommon isotopes you might hear would be, "Carbon-12" or "Carbon-14", these are two different isotopes of the element Carbon.  The -# after the element name indicates the total atomic mass of the atom.  Since we know that Carbon always has 6 protons, we can easily determine the number of neutrons if we know the atomic mass.
246055
51 electrons.\n\nbtw-the atomic number of an element (antimoney is 51) corresponds to the number of electrons in a neutral atom.\n\ni.e.=hydrogen is 1, and has 1 electron in a neutral state.
783373
This depends on how many electrons the element has to lose or gain to complete its outer layer. If the element is on the right side of the periodic table then it will gain electrons. The left side will lose electrons. How many electrons can be determined by how far away the element is from the nearest side of the periodic table.\n\nTHere is of course more technical depth to this however this thumb rule will do. For more info type ionisation into wikipedia. that should help...
813547
Carbon's atomic number is six.  The innermost shell contains two electrons.  The next shell needs eight to be complete, but carbon has only four left.  Therefore, it needs four additional electrons to complete the shell.
570306
1.ATOMIC NUMBER\n2.ELECTRON\n3.SHELL\n4.ORBIT
116277
the chemical formula is CaO. So total no. of electrons are \nequal to sum of electrons in Ca and O. \nElectrons in Ca = 20\nElectrons in O  = 8\nSo total electrons = 28\nsince no. of electrons is equal to that of protons,\nHence answer is = 28
1147679
Quantum numbers are used to describe every single electron in an atom or molecule. Each electron is assigned it's own set of four different quantum numbers. no electron in the same atom or molecule can have the same set of quantum numbers.\n\nIn atoms:\nn = the principle quantum number. It is an integer, starting with 1, then 2, then 3, and so forth. This tells the principle energy level that the electron occupies. On the periodic table, the row number tells the higest principle quantum number an electron in that elemet can have. For example, the lone electron in hydrogen is always in the n = 1 energy level. However, an element like iodine in the 5th row can have electrons all the way up to the n + 5 energy level.\n\nl is the angular momentum quantum number. It is an integer that ranges from 0 to n-1. This number determines the shape of the electrons orbital. 0 is a sphere. 1 is dumbell shapped. 2 is two dumbells. 3 is 6 dumbells. These orbital shapes are usually represented with letters: 0 = s, 1 = p, 2 = d, 3 = f, 4 = g, and so on. s,p,d,f are the most commonly seen. Since l can range from 0 to n-1, n determines which orbital shapes the electrons in a given atom can have. In the first row, only s is possible. The second row adds p orbitals, and the third row adds d orbitals. Even though no atoms in the third row have occupied d orbitals in the ground state, they are still avaliable for bonding or excited state electrons (which explains why sulfer can and often does form more than 4 bonds)\n\nm is the magnetic quantum number. It simple tells the orientation of the orbitals. It ranges from -l to l. s orbitals have l = 0, so there is only one orientation. p orbitals have l = 1, so there are three, corresponding to m = -1, m= 0, and m = 1. d orbitals have 5 orientations, and f orbitals have 7. The number of orientations is also equal to the number of each type of orbital an atom (1 s orbital, 3 p orbitals, 5 d orbitals, 7 f orbitals) per energy level.\n\nm sub s (written as an m with a subscript s) is thespin quantum number. Every orbital can hold two electrons, however due to Pauli's Exclusion Principle, they can't have the same set of quantum numbers. The spin quantum number is either +1/2 or - 1/2, and it determines the direction of the electron's "spin." This isn't spin in the normal sense, as electrons don't spin like tops.
829932
Take radium and subtract two from its atomic number. Then find the element with that result as its atomic number. I'm too lazy to see what that is right now.
292346
26 electrons. If it's an electrically neutral atom, then the number of protons must equal the number of electrons.
880214
53 protons, 53 electrons, and 72 neutrons.  53 protons are the defining characterstic of an iodine atom and it is the atomic number of iodine.  There are 53 electrons as this iodine is electrically neutral so the number of protons equals the number of electrons.  A neutron and proton both weigh one atomic mass unit.  So since the mass here is 125 subtract the number of protons from 125 to get the number of neutrons.
938184
Firstly. it's not squared (even it says 2 on the top). It says how many electrons u got on that 1S sub shell and on 2P sub shell. Carbon has 6 electrons and these electrons filled in to sub shells according to Pauli's exclusion principle. 2 electrons filled into 1S sub shell, another 2 electrons to 2S sub shell and rest 2 electrons filled into 2P sub shell. Remember that (S) sub shells hold on 2 electrons and P sub shells can hold 6 electrons. But in this case after 4 electrons are filled into S sub shells and the balance is 2 electrons. So it can be filled into P. If there are electrons more than 6, for ex 10.. 2 goes into 1S, another 2 goes into 2S and rest 6 electrons fill into 2P. This is how it happens
162059
Knowing the number of electrons present in the outer shell and  valence of each oxygen molecule.\n\nBesides there are techniques which actually helps us to visualize electrons like electron density map.\n\nHope this helps.