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is all about between atoms. Metals lose electrons to become positively charged , while nonmetals gain electrons to form negatively charged . This process creates strong electrostatic attractions between the ions.

The charges of common ions are predictable based on their position in the periodic table. Ionic compounds maintain by balancing the positive and negative charges. This balance determines the ratio of cations to anions in the compound's formula.

Ionic Bonding

Formation of cations and anions

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  • Cations form when neutral atoms lose electrons resulting in a positive charge
    • Metals, typically on the left side of the periodic table (, alkaline earth metals), readily form cations by losing valence electrons
    • Examples: [Na](https://www.fiveableKeyTerm:Na)[Na](https://www.fiveableKeyTerm:Na) atom loses one electron to form Na+Na^+ cation, [Mg](https://www.fiveableKeyTerm:Mg)[Mg](https://www.fiveableKeyTerm:Mg) atom loses two electrons to form Mg2+Mg^{2+} cation
  • Anions form when neutral atoms gain electrons resulting in a negative charge
    • Nonmetals, typically on the right side of the periodic table (, ), readily form anions by gaining electrons to complete their valence shell
    • Examples: [Cl](https://www.fiveableKeyTerm:Cl)[Cl](https://www.fiveableKeyTerm:Cl) atom gains one electron to form Cl−Cl^- anion, [O](https://www.fiveableKeyTerm:O)[O](https://www.fiveableKeyTerm:O) atom gains two electrons to form O2−O^{2-} anion
  • The process of electron transfer between atoms leads to the formation of ions, following the

Charges of common ions

  • Group 1 elements (alkali metals) form ions with a 1+ charge due to loss of one valence electron
    • Examples: Li+Li^+ (lithium ion), Na+Na^+ (sodium ion), K+K^+ (potassium ion)
  • Group 2 elements (alkaline earth metals) form ions with a 2+ charge due to loss of two valence electrons
    • Examples: Mg2+Mg^{2+} (magnesium ion), Ca2+Ca^{2+} (calcium ion), Ba2+Ba^{2+} (barium ion)
  • Group 16 elements (chalcogens) form ions with a 2- charge due to gain of two electrons to complete octet
    • Examples: O2−O^{2-} (oxide ion), S2−S^{2-} (sulfide ion), Se2−Se^{2-} (selenide ion)
  • Group 17 elements () form ions with a 1- charge due to gain of one electron to complete octet
    • Examples: F−F^- (fluoride ion), Cl−Cl^- (chloride ion), Br−Br^- (bromide ion)
  • Transition metals can form ions with variable charges depending on the number of electrons lost
    • Examples: Fe2+Fe^{2+} (iron(II) ion), Fe3+Fe^{3+} (iron(III) ion), Cu+Cu^+ (copper(I) ion), Cu2+Cu^{2+} (copper(II) ion)

Electrical neutrality in ionic compounds

  • Ionic compounds are electrically neutral overall due to balanced positive and negative charges
    • The total positive charge from cations equals the total negative charge from anions in the compound
    • Example: [NaCl](https://www.fiveableKeyTerm:NaCl)[NaCl](https://www.fiveableKeyTerm:NaCl) () has equal numbers of Na+Na^+ and Cl−Cl^- ions, resulting in overall neutrality
  • The formula of an ionic compound reflects the ratio of cations to anions needed for neutrality
    • The charges of the ions determine the ratio in which they combine to form a neutral compound
    • Examples:
      1. NaClNaCl has a 1:1 ratio of Na+Na^+ to Cl−Cl^- since both ions have a charge magnitude of 1
      2. MgCl2MgCl_2 has a 1:2 ratio of Mg2+Mg^{2+} to Cl−Cl^- to balance the 2+ charge of Mg2+Mg^{2+} with two Cl−Cl^- ions
  • The charges of the ions in an ionic compound always add up to zero, ensuring electrical neutrality
    • Examples:
      1. In NaClNaCl, the charges of the ions sum to zero: (+1)+(−1)=0(+1) + (-1) = 0
      2. In MgCl2MgCl_2, the charges of the ions sum to zero: (+2)+2(−1)=0(+2) + 2(-1) = 0

Ionic bonding and structure

  • Ionic bonds form through between oppositely charged ions
  • In solid form, ionic compounds arrange into a three-dimensional structure called an
  • The ionic lattice maximizes the attractive forces between oppositely charged ions while minimizing repulsive forces between like-charged ions

Key Terms to Review (39)

Alkali Metals: Alkali metals are a group of highly reactive chemical elements in the periodic table, characterized by their soft, silvery-white appearance and their tendency to readily lose their outermost electron to form positive ions. These elements are essential for various chemical processes and have numerous applications in industry and technology.
Anions: Anions are negatively charged ions that form when an atom or molecule gains one or more electrons. They are an essential component in the formation of ionic and molecular compounds, playing a crucial role in various chemical processes and phenomena.
Ba2+: Ba2+ is a barium ion that has lost two electrons, resulting in a +2 charge. This positively charged ion is formed when barium, an alkaline earth metal, reacts with other elements and compounds. Understanding Ba2+ is essential in studying ionic bonding, as it highlights the behavior of metals in forming ionic compounds and their interactions with nonmetals.
Br-: Br- is the chemical symbol for the bromide ion, which is a negatively charged ion of the element bromine. Bromide ions are important in various chemical and biological processes, particularly in the context of ionic bonding.
Ca2+: Ca2+ is the calcium ion, a positively charged ion with a charge of +2. It is an essential mineral that plays crucial roles in various biological processes, including ionic bonding and precipitation and dissolution reactions.
Cations: Cations are positively charged ions that form when an atom loses one or more of its valence electrons. They are a fundamental concept in understanding ionic and molecular compounds, ionic bonding, electrolysis, and periodicity.
Chalcogens: Chalcogens are a group of chemical elements in the periodic table, including oxygen (O), sulfur (S), selenium (Se), tellurium (Te), polonium (Po), and livermorium (Lv). These elements are known for their ability to form covalent bonds and participate in various chemical reactions, particularly in the context of ionic bonding.
Cl: Cl is the chemical symbol for the element chlorine, which is a highly reactive halogen gas that is essential for many chemical processes and biological functions in living organisms.
Cl-: Cl- is the chemical symbol for the chloride ion, which is a negatively charged ion consisting of a chlorine atom that has gained an extra electron. This ion is an important component in various chemical processes and contexts, including writing and balancing chemical equations, ionic bonding, electrolytes, and precipitation and dissolution.
Cu+: Cu+ is the chemical symbol and ionic form of the copper element, representing a copper atom that has lost one electron, resulting in a positively charged ion with a +1 charge. This ionic state of copper is important in the context of ionic bonding.
Cu2+: Cu2+ is the divalent cation of copper, which is a transition metal element. It is a common ion that plays a crucial role in various chemical and biological processes due to its unique electronic configuration and ability to participate in redox reactions.
Electrical Neutrality: Electrical neutrality is a fundamental concept in chemistry that describes the overall balance of positive and negative charges within a system or a particle. It is a crucial principle in understanding ionic bonding and the formation of ionic compounds.
Electron Transfer: Electron transfer is the fundamental process in which electrons move from one atom or molecule to another, resulting in the formation of ionic bonds or redox reactions. This term is central to understanding both ionic bonding and redox chemistry.
Electrostatic Attraction: Electrostatic attraction is the force of attraction between oppositely charged particles or objects. It is a fundamental concept in the study of ionic bonding, where the attractive force between positively and negatively charged ions holds the ionic compound together.
F-: F- is the chemical symbol for the fluoride ion, which is a negatively charged ion of the element fluorine. The fluoride ion is an important ion in the context of ionic bonding, as it can form ionic bonds with various cations to create ionic compounds.
Fe2+: Fe2+ is an iron ion that carries a +2 charge, indicating it has lost two electrons. This cation plays a crucial role in ionic bonding, where it often pairs with anions to form stable ionic compounds. The formation of Fe2+ occurs when iron loses two of its valence electrons, resulting in a stable electron configuration that allows for various chemical interactions and compounds.
Fe3+: Fe3+ is the chemical symbol for the ferric ion, which is the trivalent oxidation state of the iron (Fe) atom. This positively charged ion is an important species in various chemical and biological processes, particularly in the context of ionic bonding.
Halogens: Halogens are a group of elements in Group 17 of the periodic table known for their high reactivity and tendency to form salts with metals. They include fluorine, chlorine, bromine, iodine, and astatine.
Halogens: Halogens are a group of five highly reactive nonmetallic elements in the periodic table, including fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). These elements are known for their strong tendency to form ionic bonds and their widespread use in various applications.
Inert pair effect: The inert pair effect is the tendency of the outermost s-electrons to remain non-bonding or inert in heavier elements of groups 13 through 17. This results in the element exhibiting lower oxidation states than expected.
Ionic Bonding: Ionic bonding is a type of chemical bond that results from the transfer of electrons between atoms, typically a metal and a nonmetal. This transfer creates positively and negatively charged ions that are attracted to each other, forming a stable ionic compound.
Ionic Lattice: An ionic lattice is a three-dimensional arrangement of positively and negatively charged ions held together by strong electrostatic forces. It is a fundamental concept in understanding the structure and properties of ionic compounds.
K+: K+ is the chemical symbol for the potassium ion, a positively charged particle that plays a crucial role in ionic bonding and various physiological processes within the body.
Li+: Li+ is the chemical symbol for the lithium ion, which is the positively charged form of the lithium atom. Lithium ions play a crucial role in the context of ionic bonding, a fundamental concept in chemistry.
Mg: Mg, or magnesium, is a chemical element that is essential for various biological processes in the human body. It is a key component in ionic bonding, a type of chemical bond formed through the transfer of electrons between atoms.
Mg2+: Mg2+ is the divalent cation of the element magnesium, which has an atomic number of 12 and an atomic mass of 24.305 g/mol. As a positively charged ion, Mg2+ is an important participant in various chemical processes, particularly in the context of ionic bonding.
MgCl2: Magnesium chloride (MgCl2) is an ionic compound composed of magnesium ions (Mg^2+) and chloride ions (Cl^-), forming a crystalline solid at room temperature. This compound exemplifies the principles of ionic bonding, where electrons are transferred from one atom to another, resulting in the formation of charged ions that attract each other due to electrostatic forces.
Na: Na is the chemical symbol for the element sodium, which is a soft, silvery-white alkali metal that is highly reactive and essential for various physiological processes in the human body.
Na+: Na+ is the chemical symbol for the sodium ion, a positively charged particle that plays a crucial role in various chemical processes and biological functions. This term is particularly important in the context of writing and balancing chemical equations, ionic bonding, and the behavior of electrolytes.
NaCl: NaCl, commonly known as sodium chloride, is a chemical compound that consists of one sodium atom (Na) and one chlorine atom (Cl) bonded together. It is an ionic compound that is essential for various biological and industrial processes, and it is the primary component of table salt.
O: O, or oxygen, is a chemical element that is essential for life and plays a crucial role in various chemical processes, including the formula mass and mole concept, the determination of empirical and molecular formulas, and ionic bonding. As one of the most abundant elements on Earth, O is a highly reactive nonmetal that forms compounds with most other elements.
O2-: O2- is the superoxide ion, a negatively charged oxygen species that forms during the process of ionic bonding. It is an important intermediate in various biological and chemical processes, playing a crucial role in redox reactions and energy production.
Octet rule: The octet rule states that atoms tend to form bonds in such a way that they achieve eight electrons in their valence shell, gaining a stable electron configuration similar to noble gases. This rule is fundamental for understanding molecular structures and chemical bonding.
Octet Rule: The octet rule is a fundamental concept in chemistry that states that atoms tend to form stable configurations by attaining a full outer electron shell, typically containing eight electrons. This principle helps explain the formation of ionic and covalent bonds, as well as the stability of various chemical compounds.
Oxyanions: Oxyanions are polyatomic ions that contain one or more oxygen atoms bonded to another element, typically a non-metal. They often carry a negative charge due to the presence of extra electrons.
S2-: S2- is the chemical notation for the sulfide ion, which consists of one sulfur atom with a -2 charge. This ion is formed when sulfur gains two electrons, resulting in its ability to participate in ionic bonding with various cations, leading to the formation of ionic compounds. The presence of S2- influences both the properties of these compounds and the equilibria that can exist in chemical reactions involving sulfides.
Se2-: Se2- is the diatomic selenide ion, which consists of two selenium atoms bonded together and carrying a 2- charge. This ion is an important species in the context of ionic bonding, as it can form ionic compounds with various cations.
Sodium Chloride: Sodium chloride, commonly known as table salt, is a chemical compound composed of one sodium (Na) atom and one chlorine (Cl) atom. It is an ionic compound that is essential for various physiological processes in living organisms and has numerous industrial and household applications.
Δoct: Δoct, also known as crystal field splitting energy, represents the energy difference between the higher-energy and lower-energy sets of d-orbitals in an octahedral coordination complex. It plays a crucial role in determining the electronic structure and properties of transition metal complexes.
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7.2 Covalent Bonding