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Chapter 2: Problem 32

Predict the charges for monoatomic ions of these elements. (a) Magnesium (b) Phosphorus (c) Iron (d) Selenium

Short Answer

Expert verified
Mg: +2, P: -3, Fe: +2/+3, Se: -2.

Step by step solution

01

Understanding Ion Formation

To predict the charges of monoatomic ions, start by considering the periodic groups of the elements. Elements form ions to achieve a stable electronic configuration similar to the nearest noble gas.
02

Magnesium Ionization

Magnesium is in Group 2 of the periodic table. Elements in Group 2 lose two electrons to achieve a noble gas configuration, forming ions with a charge of +2. So, magnesium forms an ion with a charge of +2, written as \( \text{Mg}^{2+} \).
03

Phosphorus Ionization

Phosphorus is in Group 15 of the periodic table. Elements in this group tend to gain three electrons to achieve the electron configuration of the nearest noble gas. Thus, phosphorus forms an ion with a charge of -3, written as \( \text{P}^{3-} \).
04

Iron Ionization

Iron can lose different numbers of electrons, commonly forming either a +2 or +3 charge. This is due to it being a transition metal with variable oxidation states, so iron can be \( \text{Fe}^{2+} \) or \( \text{Fe}^{3+} \).
05

Selenium Ionization

Selenium is in Group 16 of the periodic table. Elements in this group typically gain two electrons to complete their outer shell. Therefore, selenium forms an ion with a charge of -2, written as \( \text{Se}^{2-} \).

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Periodic Table Groups
The periodic table is a well-organized chart that categorizes elements into groups based on shared characteristics and behaviors. Each vertical column, known as a "group" or "family," contains elements with similar chemical properties.
  • Groups help predict how an element will react and the type of ions it will form.
  • Elements in the same group have the same number of valence electrons, which are the outermost electrons involved in chemical bonding.
  • For example, magnesium is in Group 2 and has 2 valence electrons. It tends to lose these electrons to form a +2 ion, achieving a stable electronic configuration like a noble gas.
Understanding the periodic table's groups is crucial for predicting how an element might form ions by losing or gaining electrons.
Noble Gas Configuration
A noble gas configuration refers to the electron arrangement of the elements in Group 18 of the periodic table, known as the noble gases. These gases are considered stable because they have a full valence shell, meaning they have achieved an optimal energy state.
  • Atoms tend to form ions that mimic the electron structure of the nearest noble gas through either gaining or losing electrons.
  • Magnesium, for example, loses two electrons to match the noble gas configuration of neon.
  • Phosphorus gains three electrons to resemble argon, leading to its typical formation of a -3 ion.
Adopting a noble gas configuration is a driving force behind ion formation and chemical bonding.
Transition Metals
Transition metals occupy the central block of the periodic table and include elements like iron, copper, and nickel. These metals are unique compared to other elements because they possess variable oxidation states. This means that they can form multiple ions with different charges.
  • Unlike main group elements, transition metals can lose different numbers of electrons from their d orbitals.
  • Iron, a classic example, can form \( \text{Fe}^{2+} \) and \( \text{Fe}^{3+} \).
  • This variability is due to the comparable energies of their s and d subshells, allowing flexibility in how they achieve stability.
Understanding the nature of transition metals is essential for comprehending their complex roles in both chemistry and materials science.
Oxidation States
Oxidation states are used to indicate the degree of oxidation of an atom in a chemical compound and show how many electrons an atom gains or loses during ion formation. These states can help predict the likely charges on ions.
  • For main group elements like magnesium and selenium, oxidation states are often consistent with their group number minus eight.
  • Transition metals, like iron, display multiple oxidation states, reflecting their ability to lose different numbers of electrons.
  • In compounds, the sum of oxidation states must equal the overall charge of the compound.
Mastering oxidation states is pivotal for understanding chemical reactions, predicting products, and balancing chemical equations.

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Most popular questions from this chapter

For each pair of elements, (i) through (vii), (a) Determine whether an ionic compound, a molecular compound, or no compound would form. (b) Write an appropriate formula for each compound you expect to form and name the compound. (i) \(\quad\) Chlorine and bromine (ii) \(\quad\) Lithium and tellurium (iii) Sodium and argon (iv) \(\quad\) Magnesium and fluorine (v) Nitrogen and bromine (vi) \(\quad\) Indium and sulfur (vii) Selenium and bromine

You have a pure sample of the antiseptic aminacrine, \(\mathrm{C}_{13} \mathrm{H}_{10} \mathrm{~N}_{2}\) (a) Calculate the mass in grams of 0.06500 mol aminacrine. (b) Calculate the number of aminacrine molecules in a \(0.2480-\mathrm{g}\) sample. (c) Calculate the number of nitrogen atoms in this \(0.2480-\mathrm{g}\) sample. (d) Calculate the mass of \(\mathrm{N}\) in 100 . \(\mathrm{g}\) aminacrine.

Write the molecular formula for each substance. (a) The hydrocarbon heptane, which has seven carbon atoms and 16 hydrogen atoms (b) Acrylonitrile (the basis of Orlon and Acrilan fibers), which has three carbon atoms, three hydrogen atoms, and one nitrogen atom

Correctly name each of these ionic compounds. (a) \(\mathrm{KH}_{2} \mathrm{PO}_{4}\) (b) \(\mathrm{CuSO}_{4}\) (c) \(\mathrm{CrCl}_{3}\) (d) \(\mathrm{Ca}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\) (e) \(\mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}\)

It's final exam time and a student drinks a 1.93 -oz bottle of 5-Hour Energy \(\mathbb{B}\) to stay awake. The drink contains, among other substances, \(212 \mathrm{mg}\) caffeine, \(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2}\) (a) Calculate the mass percent nitrogen in caffeine. (b) Calculate the number of caffeine molecules that the student ingested. (c) Calculate the number of carbon atoms in this mass of caffeine. (d) An 8-oz cup of regular coffee contains approximately \(100 \mathrm{mg}\) caffeine. Calculate how many times greater the caffeine concentration (mg/oz) is in the 5 -Hour Energy \(^{\oplus}\) drink than in the regular coffee.
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