The atom number counts _______ of atoms and ions of an element.?
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The "atomic" number refers to the place in the periodic table which corresponds directly (is equal to) the number of protons. The mass number is a weighted average involving commonly found isotopes.
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Um, there's over a hundred elements.  I'm not going to name them all for you.  Look at a periodic table.  I'm sure there's one in your chemistry book.
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Ions are basically charged atoms. The formula of an ion can be found out if you have the valency of the atom. You can figure out the valency of any atom by finding the group at which the atom is located in the periodic table. For example, Sodium (Na) is located in group 1A of the periodic table. Hence the valency is +1. The formula of the sodium ion would be Na+1.\n\nHope that helps!
27684
Protons, neutrons, and electrons.
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Atoms have mass which can sometimes have volume and there are about 6.022x10^23 particles in a mole of an element. A mole of an element is the atomic mass in grams. Now, you can use all this and do some further research on the Internet and in books to write a nonfiction book on atoms and how the periodic table of the elements is set up.
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it describes the # of protons & electrons in that element.
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1.ATOMIC NUMBER\n2.ELECTRON\n3.SHELL\n4.ORBIT
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Atomic Number 3\nhttp://www.jergym.hiedu.cz/~canovm/vyhledav/varianty/litva.gif
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well.. the atomic number for the nucleus is the number of protons inside of it.
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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....)
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actually, it's arranged by the number of protons in the nucleus of an atom of each element, though the list in this song: http://www.privatehand.com/flash/elements.html\nis not.
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All of the answers are in the periodic table. The atomic number is the number above the symbol. The number of protons is the atomic number. The number of electrons is the number of protons (if there's no charge). To find the number of valence electrons, look at the number of the column it's in (as in, Fluorine is in column #7, so it has 7 valence electrons).\n\nAs for the type of ion formed, everything to the left of the "staircase" (diving non-metals from metals) makes cations. Everything to the right makes anions.
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Determining the number of valance electrons\nValance electrons \n \nHelium atom model\nThis helium (He) model displays two valence electrons\nlocated in its outermost energy level.\nHelium is a member of the noble gases and contains\ntwo protons, neutrons, and electrons. \nTo determine the quantity of valance electrons an element has, one must look at the family (vertical column) in which the element is categorized. With the exception of groups 3–12 (transition metals), the number within the unit's place identifies how many valance electrons are contained within the elements listed under that particular column.\n\nGroup Quantity of valance electrons \nGroup one (1) (alkali metals) One \nGroup two (2) (alkaline earth metals) Two \nThe (transition metals) (3-12) One to two \nGroup three (13) (boron group) Three \nGroup four (14) (carbon group) Four \nGroup five (15) (nitrogen group) Five \nGroup six (16) (oxygen group) Six \nGroup seven (17) (halogens) Seven \nGroup eight / zero (18) (noble gases) *Eight \n\nThe asterisk (*) is used to indicate that all of the noble gases contain eight valance electrons with the exception of helium (He), which only contains two.\n\n\nValance electrons in chemical reactions\nThe chemical behavior of atoms is largely due to interactions between electrons. Electrons of an atom remain within certain, predictable electron configurations. Electrons fall into shells based on their relative energy level which is usually visualized as their mean distance from the nucleus. The valance electrons have the greatest influence on chemical behavior. Core electrons (those not in the outer shell) play a role, but it is usually in terms of a secondary effect due to screening of the positive charge in the atomic nucleus.\n\n \nThe atomic orbital wavefunctions of hydrogen. The principal quantum number is at the right of each row and the azimuthal quantum number is denoted by letter at top of each column.Each shell, numbered from the one closest to the nucleus (lowest in energy), can hold up to a specific number of electrons due to its differing sublevel and orbital capacity:\n\nShell number Electron capacity Sublevels  Orbitals \nOne 2 S  1 \nTwo 8 S, P  4 \nThree 18 S, P, D  9 \nFour 32 S, P, D, F  16 \n\nTo determine the electron capacity of a shell, the formula 2n² is used, where n is the shell number or principal quantum number. Electrons fill orbitals and shells from the inside out, beginning with shell one. Whichever occupied shell is currently most outward is the valence shell, even if it only has one electron.\n\nThe reason why shells fill up in order is that the energy levels of electrons in the innermost shells are significantly lower than the energy levels of electrons in outer shells. So if the inner shells were not completely full, the electron in an outer shell would quickly "fall" into the inner shell (with the emission of a photon that would carry away the difference in the energy).\n\nThe number of electrons in an atom's outermost valence shell governs its bonding behavior. Therefore, elements with the same number of valence electrons are grouped together in the periodic table of the elements. As a general rule, the fewer electrons in an atom's valence shell, the more reactive it is. Group 1 metals are therefore very reactive, with caesium, rubidium, and francium being the most reactive of all metals.\n\nEvery atom is much more stable, or less reactive, with a full valence shell. This can be achieved one of two ways: an atom can either share electrons with neighboring atoms, a covalent bond, or it can remove electrons from other atoms, an ionic bond. Another form of ionic bonding involves an atom giving some of its electrons to another atom; this also works because it can end up with a full valence by giving up its entire outer shell. By moving electrons, the two atoms become linked. This is known as chemical bonding and serves to build atoms into molecules or ionic compound
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The atomic number tells you how many protons there are in the nucleus, and that's what identifies the element.  Subtract that number from the atomic weight and you get the number of neutrons.  Uranium has 92 protons and 143 neutrons (U235) or 146 neutrons (U238).  The different weights are called isotopes.  In an electrically neutral atom the number of electrons is the same as the number of protons.  Strip a few electrons away you get an ion (an ionized atom).  It's the structure of the electrons that strongly influences the chemical properties of the element.
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Atomic number\nThis was an idea by Mossely
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The atomic number of Aluminum is 13 (look at a periodic table). This means 13 protons and 13 electrons (since these are oppositely charged they have to balance each other.) To find the number of neutrons you subtract the number of protons from the atomic mass (the atomic mass is 27). So 27-13= 14 neutrons
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density,volume,weight,number of electron and proton.