CHEM 1031 Lecture 28: 11/9/2016 Ionization Energy: Electron Affinity: Metallic Character

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8 Mar 2017

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6. 5 period variants in element properties: changes across the period table ex. Elements at the lower part of the table are more metallic: variation in covalent radius, covalent radius: half the distance between two of the same atoms in a covalent bond. In hydrogen (one electron), the nuclear charge and the effective nuclear charge are equal. So zeff will increase: with the increased pull, electrons pull closer to the nucleus, reducing the overall radius. Anions are larger than neutral atoms because they gain electrons and the the zeff decreases. Isoelectric: describing atoms and ions that have the same electronic configuration: nuclear charge determines size, a greater nuclear charge will pull the electrons in, resulting in a, variation in ionization energies smaller radius. Ionization energy: the energy needed to remove the least bound electron from a gaseous atom that is in the ground state.

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Select the false statement below.

Generally speaking, as you go down a group in the periodic table, there is successively greater shielding of the outer-shell electrons by the inner-shell electrons.

Generally speaking, as you go across a period in the periodic table, the effective nuclear charge (Zeff) increases because each successive element contains more protons in the nucleus than the previous element and the outer electrons are all in the same shell as you go across a period.

Generally speaking, the lighter halogens can be predicted to exhibit greater shielding of the outer-shell electrons by the inner-shell electrons than heavier halogens.

Generally speaking, non-metallic elements have greater effective nuclear charge (Zeff) than metallic elements in the same period.

Classify each statement about effective nuclear charge, Zeff, as true or false.

In a Be atom, a 1s electron has a greater Z_eff than a 2s electron.

Across a period, as Z_eff increases, atomic size decreases.

Electrons in a p orbital are more effective than those in other orbitals at shielding other electrons from the nuclear charge.

A 1s electron is a Be atom has a smaller Z_eff than a 1s electron in a Li atom.

Effective nuclear charge decreases from left to right across a period on the periodic table.

Effective nuclear charge is dependent on the number of electrons present in an atom.

Select the false statement below.

A. Generally speaking, as you go down a group in the periodictable, there is successively less shielding of the outer-shellelectrons by the inner-shell electrons.
B. Generally speaking, the heavier alkaline earth metals can bepredicted to exhibit greater shielding of the outer-shell electronsby the inner-shell electrons than lighter alkaline earthmetals.
C. Generally speaking, non-metallic elements have greater effectivenuclear charge (Zeff) than metallic elements in the sameperiod.
D. Generally speaking, as you go across a period in the periodictable, the effective nuclear charge (Zeff) increases because eachsuccessive element contains more protons in the nucleus than theprevious element and the outer electrons are all in the same shellas you go across a period.

CHEM 1031 Lecture 28: 11/9/2016 Ionization Energy: Electron Affinity: Metallic Character

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