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Exam 8: Electron Configuration and Chemical Periodicity

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Question 41

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Metallic behavior is generally associated with

A) elements with very negative electron affinities.
B) elements with low ionization energies.
C) elements with small atomic radii.
D) elements with unpaired electrons.
E) elements with partially filled p orbitals.

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Question 42

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Which one of the following statements about orbital energies is incorrect?

A) In the hydrogen atom, the energy of an orbital depends only on the value of the quantum number n.
B) In many-electron atoms the energy of an orbital depends on both n and l.
C) Inner electrons shield outer electrons more effectively than do electrons in the same orbital.
D) The splitting of sublevels in many-electron atoms is explained in terms of the penetration effect.
E) The energy of a given orbital increases as the nuclear charge Z increases.

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Question 43

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"Electrons added to atomic orbitals of the same energy will remain unpaired with parallel spins until the subshell is more than half-filled" is a statement of

Select the correct set of quantum numbers (n, l, m_l, m_s) for the first electron removed in the formation of a cation for strontium, Sr.

Consider the element with the electron configuration: [Rn]7s25f7. How would you classify this element?

Moseley's measurements of nuclear charges of the elements provided the basis for arranging the elements of the periodic table in order of increasing atomic number.

Which of the following ions will be most likely to form when selenium ionizes?

How many valence electrons are there in an atom with the electron configuration [noble gas]ns²(n -1) d¹⁰np³?

Which of the following elements has the smallest atomic radius?

Which one of the following statements about atomic structure and quantum numbers is incorrect?

In forming ions of the first series of transition metals, the 4s electrons are lost before the 3d electrons.

Select the diamagnetic ion.

Which of the following elements has the smallest first ionization energy?

The maximum number of electrons in an atom with the same value of n is 2n².

Select the element with the most negative electron affinity (i.e., accepts an electron most readily) .

Select the element with the greatest metallic character.

Elements in which the outermost electron has the same principal quantum number n, show similar chemical properties.