If I take the weight of a proton plus that of the electron would it equal the weight of one hydrogen atom?
365764
Your second statement is correct, i.e proton mass+electron mass = constant mass and energy.\nok, This is with reference with another question you asked about mass defect(and chose my answer as the best, thanks). The sum of individual masses is greater than the actual mass of the atom. I am sure of this because this is what explains the stability of an atom(less energy, more stable).\nI'll give you an example which I took from my chem book\n\nMe = 0.0005486 amu(atomic mass unit)\nMp = 1.007277 amu\nMn = 1.008665 amu\nMe,Mp,Mn are masses of electron, proton and neutron respectively and 1 amu = 1.6605 x 10^-27 Kg\n\nOne He atom contains two electrons, two protons and two neutrons.\nSumming up the values of the constituents you get 4.032981amu as the expected mass of the atom.\nHowever the actual mass of the atom is 4.002603amu\nDifference = 0.030378 amu\n\nThe formula to find the binding evergy(energy required to bring the constituents together) is: mass defect x 931.48MeV\n\nHere that would be 0.030378 x 931.48 = 28.296 MeV\ni.e that is the equivalent of the mass defect in energy.\nThe '931.48' part is calculated using Einstein's formula E=mc^2.
850332
Light does not consist of proton, it consists of photons which are quantum of electromagnetic radiation, photons have their own antiparticle. Antiparticle is a particle that has the same mass of another particle but its other properties are opposite which result in cancelling the opposite properties. The net result is the production of radiant energy which is light (not according to me, but according to quantum theory). So no question of mass.\n\nAnd light has very high but not infinity velocity, then how would the mass (do not say weight, both are different) be infinite (even if we consider what you say to be true)\n\nProtons are not insignificant, they make up about half the mass of an atom (under normal conditions)
575905
It is  1.008 g/mol. for hydrogen atoms\n\nOne hydrogen atom weights on the average 1.67323 * 10^-24 grams.\n\nHydrogen gas contains 2 atoms so it weights 3.4646 *10^-24 grams.\n\nAverage mass is average abundunce of all the isotopes of hydrogen
287143
From Rule 1 and 2 we are ready to obtain an expression for one of the atomic properties, in this case is the velocity of the electron. Multiply both sides of Eq.(1) by r/mv, we obtain\n\nv= Z e2/4p eo mvr\n\nbut mvr in the denominator of this equation can be replaced nh/2 pi. we immediately have an explicit expression for the allowed values of velocity of the electron,\n\nv = Z e2/2peoh n ...(3)\n\nEq. (3) tells us that the velocity of the electron is directly proportional to the nuclear charge Z (in case of hydrogen Z=1) and inversely proportional to the principle quantum number n.\n\nvn = 2.188 x 106 m/s x (Z/n)\n\nFor H, n = 1.\n\n2,188,000 m/s = 4,894,000 miles per hour\n= 0.729 %c, c = speed of light in vacuum, 3 x 10^8 m/s
47846
Look up the atomic mass (sometimes called atomic weight) on the periodic table, and subtract the atomic number from it.  The atomic mass is (practically) equal to the total number of protons and neutrons, and the atomic number is equal to the number of protons.  When you subtract atomic number from atomic mass your subtracting the number of protons from the total number of protons and neutrons, which leaves you with just neutrons.
844991
Potassium is number 19. That means it has 19 protons. If it is an atom and not an ion, it has the same nimber of electrons as protons. Since protons are positive + and electrons are negative - , they have to balance. You find the neutrons by subtracting the atomic number from the atomic mass, since both the protons and neutrons weigh 1 and make up the mass. The electrons in the energy levels can move to another atom in compound formation.(ions)
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.
781216
there is only one atom in the valence shell of Hydrogen but it shares an electron with Oxygen in the covalent bond giving it two. But if the Hydrogen is just by itself then it only have one electron in its valence shell and i said above
40150
The atomic # of the element is the # of protons and (some times electrons) in the element
393625
mass # =#protons + # neutrons\nand # protons = # electrons in an electronically neutral atom.\nso you can therefore find the # nuetrons\n#neutrons=mass#-# protons
68763
One proton, it is hydrogen.  The extra mass comes from a neutron.  This isotope is called deuterium.
60596
Gaining an electron...
716161
Well if it's stable, there will be the same amount of protons as electrons. If it has a charge add or subtract. \n(If you have a plus charge, that means there's 1 more proton than electron... if you have a -2 there are two more electrons than protons etc.)
805822
Technically yes, because electrons do have mass, but it is negligible.  An electron has a mass of 9 x 10^-31 kg.  Still, if you had an infinitely sensitive measuring device, a negatively charged object would be heavier than an identical object with no charge.
792926
You got it right when saying the more N+P it has, the heavier it will be. But you forget one thing:\n\nPeriodic table is sorted by the number of protons, not their atomic weight. Atomic weight noted there is calculated on the base of the proportion of naturally occuring isotopes. I guess you know what an isotope is. They are nuclei having same amount of protons but differ in neutrons. \n\n99.6% argon are 40Ar18 whilst 93% Potassium are 39K19\nBoth has the same number of nucleon = 58. Small differences may apply because of the contribution of other isotopes.
705478
An ion differs from the original element in terms of the number of electrons.\n\nThe mass of an electron is about 1/1836 of a proton or a neutron.\n\nTherefore there would be a tiny difference in atomic mass, however in most cases it's fairly negligable.
936423
Standard hydrogen has one proton and one electron. Standard helium has two protons, two electrons and two neutrons (so it's about four times as massive as hydrogen). Also, hydrogen has one positive chemical link, while helium has no chemical links (it's a noble gas, and therefore very inert).