The ability of an atom (or ion) to gain electrons. Why are ionization energies always increasing? For example, why is the second ionization energy higher than the first, and the third higher than the second? The same number of protons in the nucleus but less electrons hence the effective nuclear charge is higher for subsequent ionizations. One electron at a time! Is the first ionization energy of P or S higher? Why? Phosphorus is higher since it is 3p3 (half-filled shell) and removing an electron from sulfur, 3p4, is removing an electron that is paired and gives S+, a half-filled shell. There is a VERY big difference between S (g) → S2+ + 2e- and that is NOT the equation for the second ionization of sulfur. S (g) → S+ (g) + e- Write the equation for the second ionization of sulfur. P (g) → P+ (g) + e- Write the equation for the first ionization of sulfur, S. Write the equation for the first ionization of phosphorus, P. Polarity: nonpolar AX2E (steric number, geometry, bond angle(s), polarity) SN: 3īond angle: ni, and therefore this process is an absorption, hence energy must be gained in order to force the electron into a higher energy level, in this case, completely out of the atom. Polarity: nonpolar AX6 (steric number, geometry, bond angle(s), polarity) SN: 6 Polarity: nonpolar AX5 (steric number, geometry, bond angle(s), polarity) SN: 5 Polarity: nonpolar AX4 (steric number, geometry, bond angle(s), polarity) SN: 4 Polarity: nonpolar AX3 (Steric number, geometry, bond angle(s), polarity) SN: 3 valence shell expansion (elements with n greater or equal to 3 have empty d orbitals which means more than 8 electrons can fit around the central atom) AX2 (Steric number, geometry, bond angle(s), polarity) SN: 2 Which element has the smallest atomic radius?ĭ) Oxygen (O) D As zeff increases, atomic radius _ decreases as n increases, atomic radius _ increases ionization energy the minimum energy required to remove an electron from an atom Ionization energy _ going left to right, _ going down increases decreases can you remove electrons from noble gases no why are half filled shells more stable than unfilled shells they minimize electron electron repulsion why are noble gases the most stable? they have a full or closed shell and zeff is maximized electron affinity the ability of an atom or ion to gain electrons in general, electron affinity _ from left to right, then _ going down increases decreases zeff _ from left to right, and therefore the atomic radius _ increases, decreases n _ down the periodic table, therefore atomic radius _ increases, increases electronegativity the ability of an atom to attract an electron from another atom what is an electron donor an atom with a low electronegativity electronegativity _ from left to right, _ going down increases, decreases when it comes to atomic and ionic radii, anions are _ than cations bigger why does an anion have a bigger atomic radii than cations and neutral atoms? they have more electrons isoelectronic atoms or ions that have the same electron configuration why might one not follow the octet rule 1.
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