Ions And Ionic Bonding

Halogens such as oxygen and fluorine exist as diatomic molecules, meaning they naturally occur as pairs of atoms bonded together. This is because they have a high electronegativity, which allows them to form strong covalent bonds with each other. Therefore, the statement that halogens hang around in pairs is true.

This is an example of a covalent bond because in a covalent bond, atoms share electrons to achieve a full valence shell.

The correct answer is an arrangement of cations and anions attracted to each other. A lattice refers to a regular, repeating pattern of positive and negative ions in a crystal structure. In a lattice, cations (positively charged ions) and anions (negatively charged ions) are arranged in a way that their opposite charges attract each other, creating a stable and organized structure. This arrangement is commonly found in ionic compounds, where the strong electrostatic forces between the ions hold them together in a lattice formation.

During bonding, atoms try to gain a full valence shell. This is because a full valence shell is the most stable configuration for an atom. By gaining or losing electrons, atoms can achieve a full valence shell and become more stable. This stability is achieved by following the octet rule, where atoms strive to have 8 electrons in their outermost shell, except for hydrogen and helium which strive to have 2 electrons. By gaining a full valence shell, atoms can achieve a lower energy state and increase their stability.

When magnesium gives away 2 electrons, it loses those negatively charged particles, resulting in a positively charged ion. This type of ion is called a cation. The charge on the cation is determined by the number of electrons lost, which in this case is 2, so the charge is +2.

Atoms can bond in three ways: ionic bond, covalent bond, and metallic bond. In an ionic bond, atoms transfer electrons to achieve a stable electron configuration. This results in the formation of positively and negatively charged ions that are attracted to each other. In a covalent bond, atoms share electrons to fill their outermost electron shells. This sharing of electrons creates a strong bond between the atoms. In a metallic bond, electrons are delocalized and free to move within a lattice of positively charged metal ions. This results in a strong bond between the metal atoms.

This is an ionic bond because it involves the transfer of electrons from a metal to a non-metal. The metal, which wants to give electrons, becomes a positive cation, while the non-metal, which wants to take electrons, becomes a negative anion. The opposite charges of the cation and anion attract each other, forming an ionic bond.

The Al ion has a 3+ charge because it is a metal and tends to lose electrons to form positive ions. The O2- ion has a 2- charge because oxygen tends to gain two electrons to achieve a stable octet configuration. When we combine these ions, we need two Al3+ ions to balance the charge of three O2- ions, resulting in the formula Al2O3.

The given equation, 4Al + 3O_2 --> 2(Al_2 O_3), is the balanced form of the chemical equation Al + O_2 --> Al_2 O_3. In order for a chemical equation to be balanced, the number of atoms of each element on both sides of the equation must be equal. The balanced equation shows that there are 4 atoms of aluminum (Al) and 6 atoms of oxygen (O) on both sides of the equation, satisfying the law of conservation of mass.

The given answer, Li (NO_3), represents a lithium ion (Li+) combined with a nitrate ion (NO3-). This compound is formed when a lithium atom loses one electron to become a positively charged ion (Li+), and a nitrate ion (NO3-) donates its negative charge to combine with the lithium ion. The resulting compound is Li (NO3), where the lithium ion and nitrate ion are held together by ionic bonds.