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Ch.8 - Basic Concepts of Chemical Bonding
Chapter 8, Problem 4a

The orbital diagram that follows shows the valence electrons for a 2+ ion of an element. (a) What is the element?

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Identify the number of valence electrons in the 2+ ion from the orbital diagram.
Determine the number of electrons that were removed to form the 2+ ion.
Add the removed electrons back to the 2+ ion to find the total number of electrons in the neutral atom.
Use the total number of electrons to identify the element by its atomic number on the periodic table.
Verify the electron configuration of the neutral atom to ensure it matches the element identified.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how an element reacts chemically. They are involved in forming bonds with other atoms and are typically represented in an orbital diagram. For transition metals, the valence electrons can include those in both the outermost shell and the d subshell.
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Ion Formation

Ions are charged particles that form when atoms gain or lose electrons. A 2+ ion indicates that the element has lost two electrons, which affects its electron configuration and can help identify the element. Understanding how ions form is essential for predicting the behavior of elements in chemical reactions.
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Orbital Diagrams

Orbital diagrams visually represent the distribution of electrons in an atom's orbitals. Each box in the diagram corresponds to an orbital, and arrows indicate the presence of electrons. Analyzing these diagrams helps in understanding the electron configuration of ions and can be used to deduce the identity of the element based on its valence electron arrangement.
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Related Practice
Textbook Question

Illustrated are four ions — A, B, X, and Y— showing their relative ionic radii. The ions shown in red carry positive charges: a 2+ charge for A and a 1+ charge for B. Ions shown in blue carry negative charges: a 1- charge for X and a 2- charge for Y. (b) Among the combinations in part (a), which leads to the ionic compound having the largest lattice energy?

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Textbook Question

A portion of a two-dimensional 'slab' of NaCl(s) is shown here (see Figure 8.2) in which the ions are numbered. (a) Which colored balls must represent sodium ions?

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Textbook Question

A portion of a two-dimensional 'slab' of NaCl(s) is shown here (see Figure 8.2) in which the ions are numbered. (d) Consider ion 5. How many repulsive interactions are shown for it?

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Textbook Question

In the Lewis structure shown here, A, D, E, Q, X, and Z represent elements in the first two rows of the periodic table. Identify all six elements so that the formal charges of all atoms are zero.

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Open Question
Fill in the blank with the appropriate numbers for both electrons and bonds (considering that single bonds are counted as one, double bonds as two, and triple bonds as three). (a) Fluorine has _ valence electrons and makes _ bond(s) in compounds. (b) Oxygen has _ valence electrons and makes _ bond(s) in compounds. (c) Nitrogen has _ valence electrons and makes _ bond(s) in compounds. (d) Carbon has _ valence electrons and makes _ bond(s) in compounds.
Textbook Question

The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the molecule. The carbon—carbon bonds are labeled 1, 2, and 3. (a) How many hydrogen atoms are in the molecule?

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