CHEM 1210 Chapter Notes - Chapter 7: Electron Affinity, Nonmetal

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aquamarineguinea-pig798

19 Aug 2016

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Ohio State University

Department

Chemistry

Course

CHEM 1210

Professor

Kroner Steven

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CHEM 1210 Full Course Notes

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Elements in same column contain same amount of electrons in valance orbitals. Mendeleev noticed pattern in groups of elements, arranged them in the periodic table. Effective nuclear charge (zeff): a net attraction that is the result of the nuclear attraction decreased by the electron-electron repulsions. Effective nuclear charge increases from left to right and less so from top to bottom. Bonding atomic radius: equal to half the bond distance (the distance between the nuclei of two atoms) Radius increases from right to left and from top to bottom. Isoelectric series: group of ions all containing the same number of electrons. Ionization energy: the minimum energy required to remove an electron from the ground state of the isolated gaseous atom or ion. Ionization energies are successively higher as electrons are removed. There is a sharp increase in ionization energy when an inner shell electron is removed.

Related Questions

\Within a family, elements with higher atomic numbers pull less strongly on electrons in a bond, because the valance electrons are in higher principal energy levels.

True False

Within a period, elements with lower atomic numbers have atoms of smaller radius because the atoms have higher effective nuclear charge.
Within a family, elements with lower atomic numbers require more energy to remove an electron from the atom, because the atoms have higher effective nuclear charge.
Within a family, elements with higher atomic numbers have lower electronegativity because the atoms have lower effective nuclear charge.
Within a period, elements with lower atomic numbers require more energy to remove an electron from the atom, because the atoms have lower effective nuclear charge.
Within a family, elements with higher atomic numbers have lower ionization energy because the valance electrons are in higher principal energy levels.

True or False.

(a) Effective nuclear charge (Zeff) is the positive charge experienced by the electron from the nucleus and it increases from left to right across the period. Answer: __________

(b) Effective nuclear charge slightly decreases going down a group. Answer: __________

(d) Atomic radius tends to decrease from top to bottom of a group because of the increase in the principle quantum number. Answer: __________

(e) Anions are larger than their parent atoms because electrons are added to the valence shell reducing the electron-electron repulsions. Answer: __________

(f) Al3+ is larger than Na+ because Na+ has two extra electrons. Answer: __________

(g) The ionization energy of Na2+ is significantly higher than Na+ because it takes more energy to remove the inner-shell electron. Answer: __________

(h) Bromine, calcium and sodium are metallic elements because they are on the left side of the periodic table. Answer: __________

(i) Calcium, antimony, and silicon are metalloids that their properties fall between those of metals and those of nonmetals. Answer: __________

(j) Lattice energy is the energy required to completely separate one mole of solid ionic compound into its gaseous ions and it is always a negative number. Answer: __________

Which of the following statements about effective nuclear charge for the outermost valence electron of an atom is incorrect? (i) The effective nuclear charge can be thought of as the true nuclear charge minus a screening constant due to the other electrons in the atom. (ii) Effective nuclear charge increases going left to right across a row of the periodic table. (iii) Valence electrons screen the nuclear charge more effectively than do core electrons. (iv) The effective nuclear charge shows a sudden decrease when we go from the end of one row to the beginning of the next row of the periodic table. (v) The change in effective nuclear charge going down a column of the periodic table is generally less than that going across a row of the periodic table.

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CHEM 1210 Chapter Notes - Chapter 7: Electron Affinity, Nonmetal

CHEM 1210 Full Course Notes

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