how does the atomic number affect the energy needed to remove the easiest electron.?
832209
As you go down any column in the periodic table it requires less energy to remove the first electron.  As you go across the rows it requires more energy to remove each electron.
838528
No elements are there.\n(If it would have been there, one would have to discover another quantum number in order to distinguish between them).\n& like the previous answerer said it would have been violated the Pauli's exclusion principle.\nThe quantum numbers are there to distinguish between different electrons.
272390
1 electron as its already 1s1 n its needs 1 more to to get to 1s2 which is normal valency of s orbital
748503
s p d f blocks tell which set of orbitals are the last to fill for those elements.\n\n+ or - depending on whether it will lose or gain an e-\n\ncations are smaller than atoms b/c they lose e-\nanions are larger than atoms b/c they gain e-\n\neach successive ionization energy gets higher becasue the #protons is more and more unbalanced by # e-\n\nhalogens have 7 valence e- and noble gases have 8.  by gaining one e- the halogens now have the e- configuration of a noble gas and are more stable.  gain 1 e- = 1- charge
888504
The atomic number equals the number of protons.  Electrons should equal the number of protons, but may not if it's an ion.  Neutrons vary as to the specific isotope of the atom.\n\nExample:\nHydrogen, atomic number = 1.  Therefore, 1 proton, 1 electron.\nIt has three isotopes:\nH-1 (1 proton, 1 electron, no neutrons)\nH-2 (1 proton, 1 electron, 1 neutron)\nH-3 (1 proton, 1 electron, 2 neutrons).\n\nYou might check the section you are asking this in, though.  This is the Religion section.
906940
Energy level is much more significant to atomic size.
872530
Magnesium has 2 valence electrons. Hence, the first and second ionization energies are not as much as third ionization energy. Its already difficult to remove its third electron because it would come from an orbital that follows the octet rule (meaning already stable). To visualize:\n\n1st ionization: Mg + energy ---> Mg+  + e-\n2nd ionization: Mg+  + energy ---> Mg2+  + e-\nnote that Mg2+ is the stable form of magnesium ion, it occurs naturally.\n3rd ionization: Mg2+  + energy ---> Mg3+  + e-\nnote that Mg3+ does not occur naturally
881836
I don't think you can choose one or the other.  Small atoms do have less of a shielding effect, but the other factor to consider is the number of protons in the nucleus.  As atoms increase in atomic number, the number of protons increases but so does the number of electrons around the nucleus, which results in the shielding effect.  Generally, as you move up and to the right of the periodic table, atoms tend to have a higher electronegativity (a measure of their ability to attract electrons).
365377
atomic number represents the number of protons or electrons in an atom
891179
The greater the atomic number, the greater the number of protons in the nucleus, which USUALLY means a higher number of neutrons and electrons. The greater number of particles (protons, neutrons, and electrons) the greater the atomic radius. \n\nNote: There are different answers to this question depending upon what level of chemistry you are taking. But if you're taking a basic chemistry, it's the right answer.
82058
A normal Hydrogen atom has one proton and one electron.  If you strip away the electron, you are left with the Hydrogen +1 ion, which is the same thing as a proton.\n\nThere are two other Hydrogen isotopes (much MUCH less common than Hydrogen-1), there are Hydrogen-2 (1 proton, 1 neutron, 1 electron), and Hydrogen-3 (1 proton, 2 neutron, 1 electron).\nIf you were to strip away their electrons, they would still be the a Hydrogen +1 ion, but would be heavier since they have an extra 1 or two neutrons.
33642
Use the periodic table to find the atomic mass of the element and subtract from this the atomic number.  \n\nThe atomic mass is equal to sum of proton and neutrons, and the atomic number is the number of protons an atom has.  Electrons have such a small mass that they don't really have any noticable effect on the atomic mass.\n\nEx: Oxygen (atomic mass - 16, atomic number - 8)\n\n16 - 8 = 8, therefore the number of protons is equal to 8
714831
the atomic number is 5 b/c atomic number equals the number of elctrons and protons. You have 5 electrons so it should be 5.
932002
Okay this is kind of confusing but here goes...  Atoms have energy levels right?  There are sublevels to each major energy level, these are your s, p, d levels.  These sublevels can hold certain amounts of electrons.  S can hold 2.  P can hold 6.  D can hold 10.  These sublevels make up larger energy levels.  In the first major energy level there is only an S sublevel, so overall the first major energy level can oly hold 2 electrons.  In the second energy level there is an S sublevel and a P sublevel for a total of 8 electrons.  This keeps going on and on but I'll stop here    for now to keep it as simple as possible.  \n             Each element has a certain number of electrons.  The number of electrons is the same as its atomic number.  The atomic number is the number in the upper lefthand corner of the element's box on the periodic table.  The numbers go in order accross the table.  He has an atomic number of two.  This means it has two electrons.  You have to figure out which sublevels these electrons fill up.  Because there are only two electrons it can only fill up the first S sublevel.  So it is written    He 1s _2.  The 1 stands for the first major energy level.  The s is the sublevel and the 2 is the number of electrons in the sublevel when He is the element.  For He none of the other energy levels are used.\n             Ne has an atomic number of 10.  It has 10 electrons.  It fills up the first sublevel s and then moves to the second major energy level.  Here it fill up the s sublevel and the p sublevel (P can hold 6 electrons)  It can then be written  Ne 1s_2_2s_2_2p_6    Remember the number in front of the s of the p stands for the major energy level.  The letter( s or p) stands for the sublevel, and the number after the letter stand for the number of electrons in that sublevel for the given element.  Put a 0 in after the level not filled up.  \n         Hope this helps!  It's kind of hard to explain but I tried to make it clear.
905298
when electrons get energy or heat, they use that energy to move from their ground state to their excited state.  \n\nthey release the energy in the form of a color when they return to their ground state.\n\nthe amount of energy the electron absorbs (and then releases) determines the color.  purple has the most energy, and red has the least.\n\ni hope this was helpful!
547549
From elementary chemistry it is known that the atomic structure of any element is made up of a positively charged nucleus surrounded by electrons revolving around it. An element’s atomic number indicates the number of positively charged protons in the nucleus. The atomic weight of an atom indicates how many protons and neutrons in the nucleus. To determine the number of neutrons in an atom, the atomic number is simply subtracted from the atomic weight.\n\nAtoms like to have a balanced electrical charge. Therefore, they usually have negatively charged electrons surrounding the nucleus in numbers equal to the number of protons. It is also known that electrons are present with different energies and it is convenient to consider these electrons surrounding the nucleus in energy “shells.” For example, magnesium, with an atomic number of 12, has two electrons in the inner shell, eight in the second shell and two in the outer shell.\n\nAll chemical bonds involve electrons. Atoms will stay close together if they have a shared interest in one or more electrons. Atoms are at their most stable when they have no partially-filled electron shells. If an atom has only a few electrons in a shell, it will tend to lose them to empty the shell. These elements are metals. When metal atoms bond, a metallic bond occurs. When an atom has a nearly full electron shell, it will try to find electrons from another atom so that it can fill its outer shell. These elements are usually described as nonmetals. The bond between two nonmetal atoms is usually a covalent bond. Where metal and nonmetal atom come together an ionic bond occurs.\n\nhttp://www.tech.farmingdale.edu/depts/met/met205/atomicbonds.html\n\nhttp://web.jjay.cuny.edu/~acarpi/NSC/5-bonds.htm
791123
when electrons get energy or heat, they use that energy to move from their ground state to their excited state. \n\ntheir excited state is not very stable, so they move back down in energy to their ground state.\n\nthey release the energy in the form of a color when they return to their ground state.\n\nthe amount of energy the electron absorbs (and then releases) determines the color. purple has the most energy, and red has the least.\n\ni hope this was helpful!