CAS CH 101 Lecture Notes - Lecture 7: Effective Nuclear Charge, Atom, Valence Electron

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4 Dec 2017

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The potential energy of the attraction between the nucleus and the electrons (effective nuclear charge, We can use zeff to predict properties, if we determine it"s pattern on the periodic table. Increasing number of filled energy levels between the nucleus and valence electrons. Strengthens from left to right across a period. Electrons are being added to the same principle energy level. Electrons are more strongly attracted to the nucleus. The quantity of energy required to remove an electron from the gaseous atom or ion. First ionization energy: decreases moving down a group increases from left to right across a period; First ionization energy (i first electron: is that required to remove the. Second ionization energy (i: - the second electron. Increasing energy required to remove successive etc. etc. electrons zeff. The effective nuclear charge increases as you remove electrons (proton : electron ratio)

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: __________

Explain clearly, all of the number.

CAS CH 101 Lecture Notes - Lecture 7: Effective Nuclear Charge, Atom, Valence Electron

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