Yes. Non metals have larger electron affinity than metals as non metals accept electrons more easily than metals.
Protons have a larger mass, but it is unclear which (if either) have a larger radius. The electron does not seem to have ANY measurable radius.
It would be easier to remove an electron from Na compared to O. Sodium (Na) has a smaller effective nuclear charge and a larger atomic radius compared to oxygen (O), making its valence electron easier to remove. Oxygen has a higher electronegativity and a stronger pull on its electrons, making it harder to remove an electron from O.
The electron cloud around the nucleus of an atom includes probable locations rather than precise orbitals.Atoms with larger atomic numbers have a larger electron cloud, or system of orbitals.
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No. The electron and proton have the same amount of charge. Its just that the electron's charge is negative and the proton's charge is positive.
Nonmetals tend to gain electrons to become negatively charged ions, increasing in size due to the addition of the electron(s). This is because the added electron(s) repel the existing electrons, causing the electron cloud to expand and the ion to be larger than the neutral atom.
Down the group electron affinity decreases Across a period electron affinity increases. However, it should be noted that chlorine is having higher electron affinity than flourine due to the small size of fluorine atom)
in the case of non-metals, the anions are formed by the addition of electrons. So the ionic radius is larger than that of the atomic radius
Ionization energy is the energy needed to remove an electron. Elements other than transition metals gain or lose electrons from the s and p orbitals in order gain the more stable electron configuration of a Noble gas. Metals lose electrons to become isoelectronic (that is have the same electron configuration) to a noble gas (previous to them in the periodic table), while nonmetals tend to gain electrons in order to become isoelectronic to a Noble gas (next highest on the periodic table). Since ionization energy is the energy needed to REMOVE an electron, it is low for metals which form positive ions by losing electrons to become more stable, but very high for nonmetals that tend to gain, NOT LOSE, electrons. Most transition metals tend to lose electrons as well (other than Rhenium). Transition metals lose electrons from the d orbital, but still form positive ions, so their ionization energy is also usually lower than nonmetals.
No, I would expect a chlorine ion to be slightly larger than a magnesium ion. Chlorine gains an electron to form a chloride ion, which increases its electron cloud size, while magnesium loses electrons to form a magnesium ion, making it slightly smaller due to the loss of electron shielding.
The atomic radius of argon is larger than the other elements in the 3rd period because argon is a noble gas with a full outer shell of electrons, leading to increased electron-electron repulsion that causes the electron cloud to expand. In contrast, the other elements in the 3rd period are metals or nonmetals that typically lose or gain electrons to achieve a stable electron configuration, resulting in smaller atomic radii.
Atoms with larger atomic numbers have a larger electron cloud, or system of orbitals
The fluoride ion is larger than the fluoride atom because it has gained an extra electron, resulting in an increase in electron-electron repulsions, which causes the electron cloud to expand. This increase in electron-electron repulsions leads to a larger ionic radius compared to the atomic radius of the fluoride atom.
Yes it is.
Nitrogen is larger than carbon. Nitrogen has one more electron and proton than carbon, resulting in a larger size due to increased electron-electron repulsion.
Non-metal ions typically form negative ions (ie: Cl-) Therefore they now have an extra electron which is protected from the positive pull of the nucleus by the other electrons and therefore the electron shell has now expanded, making nonmetal ions larger than nonmetal atoms
Nonmetals have larger ionic sizes compared to metals. This is because nonmetals tend to gain electrons to form negatively charged ions (anions), leading to the increase in the overall size of the ion. Metals, on the other hand, tend to lose electrons to form positively charged ions (cations), resulting in smaller ionic sizes.