Ionic bonds typically form between a metal and a non-metal.
What is a cation?
A cation is a positively charged ion formed when a metal atom loses electrons.
What is an anion?
An anion is a negatively charged ion formed when a non-metal atom gains electrons.
What type of attraction holds ions together in an ionic bond?
Electrostatic attraction holds ions together in an ionic bond.
What is the stable electron configuration achieved by ions?
Ions achieve a stable electron configuration, often a full outer shell (duplet or octet).
Give two examples of ionic compounds.
Sodium chloride (NaCl) and magnesium oxide (MgO) are two examples of ionic compounds.
In the formation of NaCl, which atom loses an electron?
In the formation of NaCl, the sodium atom (Na) loses an electron.
In the formation of NaCl, which atom gains an electron?
In the formation of NaCl, the chlorine atom (Cl) gains an electron.
What is the charge on a sodium ion (Na⁺)?
The charge on a sodium ion is +1.
What is the charge on a chloride ion (Cl⁻)?
The charge on a chloride ion is -1.
Do ionic compounds conduct electricity in a solid state?
No, ionic compounds do not conduct electricity in a solid state.
Do ionic compounds conduct electricity when molten?
Yes, ionic compounds conduct electricity when molten.
What is the typical solubility of ionic compounds in water?
Ionic compounds are typically soluble in water.
What is the typical solubility of ionic compounds in organic solvents?
Ionic compounds are typically not soluble in organic solvents.
Are ions free to move within the crystal structure of a solid ionic compound?
No, ions are not free to move within the crystal structure of a solid ionic compound; they are in fixed positions.
What term is used to describe the arrangement of ions in an ionic compound?
The arrangement of ions in an ionic compound is described as a giant lattice structure.
What is the electron configuration of a magnesium atom?
The electron configuration of a magnesium atom is 2.8.2.
What is the electron configuration of a magnesium ion (Mg²⁺)?
The electron configuration of a magnesium ion (Mg²⁺) is 2.8.
What is the electron configuration of an oxygen atom?
The electron configuration of an oxygen atom is 2.6.
What is the electron configuration of an oxide ion (O²⁻)?
The electron configuration of an oxide ion (O²⁻) is 2.8.
Explanation Questions
Explain why noble gases are generally unreactive?
Noble gases are generally unreactive because they have a full outer shell of electrons (either 2 for Helium or 8 for all the others). This stable electron configuration means they do not need to gain, lose, or share electrons to achieve stability.
Describe the process of how an ionic bond forms between a metal and a non-metal.
An ionic bond forms when a metal atom transfers one or more of its valence electrons to a non-metal atom. The metal atom becomes a positively charged ion (cation) and the non-metal becomes a negatively charged ion (anion). These oppositely charged ions are then held together by strong electrostatic attraction, forming the ionic bond.
Explain why metals tend to form cations and non-metals tend to form anions.
Metals have a small number of electrons in their outer shell and it is easier for them to lose these electrons to achieve a full outer shell. By losing electrons they become positively charged (cations). Non-metals have almost full outer shells and it is easier to gain electrons to complete their outer shell, becoming negatively charged (anions).
How does the transfer of electrons lead to the formation of charged ions?
The transfer of electrons results in an imbalance of protons and electrons in the atoms. When an atom loses electrons, it has more protons than electrons and becomes a positively charged ion (cation). When an atom gains electrons, it has more electrons than protons, becoming a negatively charged ion (anion).
Why are electrostatic forces in ionic bonds considered strong?
Electrostatic forces in ionic bonds are strong because they arise from the attraction between oppositely charged ions. The larger the charges on the ions and the closer they are to each other, the stronger the electrostatic attraction.
Explain why ionic compounds have high melting and boiling points.
Ionic compounds have high melting and boiling points because of the strong electrostatic forces that hold the ions together in a lattice structure. A large amount of energy is required to overcome these strong forces and separate the ions, resulting in high melting and boiling temperatures.
Explain why ionic compounds are able to conduct electricity when molten or in aqueous solution.
Ionic compounds can conduct electricity when molten or in aqueous solution because the ions are free to move. In the solid state, ions are fixed in a lattice and cannot move freely. When molten or dissolved in water, ions are mobile and are able to carry an electrical charge.
Describe the structure of an ionic compound, such as sodium chloride, in its solid state.
In the solid state, an ionic compound like sodium chloride has a giant lattice structure. The positive sodium ions (Na⁺) and negative chloride ions (Cl⁻) are arranged in a regular, repeating three-dimensional pattern, with each ion surrounded by ions of the opposite charge.
Using sodium chloride (NaCl) as an example, explain how the transfer of electrons results in the formation of the compound.
In the formation of NaCl, a sodium atom (2.8.1) transfers its single valence electron to a chlorine atom (2.8.7). This results in a sodium ion (Na⁺) with an electron configuration of 2.8 and a chloride ion (Cl⁻) with an electron configuration of 2.8.8. The oppositely charged ions are then attracted to each other by electrostatic forces, forming the ionic compound sodium chloride.
How does the arrangement of electrons in the ions achieve stability?
The arrangement of electrons in ions achieves stability by forming full outer electron shells. When metals lose electrons, they attain the electron configuration of the preceding noble gas. When non-metals gain electrons, they attain the electron configuration of the next noble gas. These full outer shells make ions stable.