They would still be the same element, but we call them different "isotopes." Also, just to be thorough, two atoms can have the same number of protons and electrons and still be different in the number of neutrons. But if I remove two electrons from a calcium atom, I still have a calcium atom because the nucleus is the same. And since the periodic table lists atoms in their neutral state, this has the effect that the number of electrons happens to correlate with the number of protons and thus the charge of the nucleus. For atoms with neutral charge, this implies same number of protons and electrons. There are no electrons in the nucleus! As you move across the periodic table, the number of protons increases, increasing the charge of the nucleus by $+1$ for each proton added. Greater number of electrons doesn't increase the strength of the nucleus. Nuclear charge increases due to protons NOT electrons.As a result, the atomic radius decreases. The valence electrons are held closer towards the nucleus of the atom. This means that the nucleus attracts the electrons more strongly, pulling the atom's shell closer to the nucleus. The effect of increasing proton number is greater than that of the increasing electron number therefore, there is a greater nuclear attraction. However, at the same time, protons are being added to the nucleus, making it more positively charged. This is because, within a period or family of elements, all electrons are added to the same shell.
This is could be considered chemistry question and might receive a more interesting response on Chem.SE.
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