Chemical Bonds

Atoms bond to become stable. When atoms bond, they share, gain, or lose electrons in order to achieve a full outermost energy level, also known as a valence shell. This allows the atom to have a more stable electron configuration, similar to that of a noble gas. By achieving stability, atoms minimize their energy and increase their overall stability, which is why they bond with other atoms.

Ionic bonds transfer electrons between atoms. In an ionic bond, one atom donates electrons to another atom, resulting in the formation of positively and negatively charged ions. This transfer occurs between a metal and a non-metal, where the metal atom loses electrons to become a positively charged ion, and the non-metal atom gains those electrons to become a negatively charged ion. The attraction between these opposite charges holds the ions together, forming an ionic bond.

The Octet Rule states that atoms lose, gain, or share electrons in order to obtain 8 valence electrons. This is because having a full outer electron shell, which consists of 8 electrons, makes an atom more stable. By gaining, losing, or sharing electrons, atoms can achieve this stable electron configuration and become more chemically stable.

A covalent bond is formed when one or more electrons are shared between atoms. In this type of bond, the atoms involved share their outer electrons to achieve a more stable electron configuration. This sharing of electrons allows both atoms to fill their outermost energy levels and form a strong bond. Covalent bonds are typically formed between nonmetal atoms and can be either single, double, or triple bonds depending on the number of shared electrons.

Metallic bonds are formed between metal atoms, where the valence electrons are delocalized and free to move throughout the metal lattice. This sharing of electrons creates a strong bond, but it is weaker than covalent and ionic bonds. In covalent bonds, atoms share electrons, forming a strong bond, while in ionic bonds, atoms transfer electrons, creating a strong electrostatic attraction between oppositely charged ions. Therefore, the statement that metallic bonds are weaker than covalent and ionic bonds is true.

The dots on the Lewis Dot Structure represent the valence electrons. Valence electrons are the outermost electrons in an atom and they are involved in chemical bonding. The Lewis Dot Structure is a way to represent the valence electrons of an atom using dots around the symbol. Each dot represents one valence electron, and this structure helps to determine the type of bond and the overall structure of a molecule.

Two hydrogen atoms form a covalent bond. In a covalent bond, the atoms share electrons to achieve a stable electron configuration. In the case of hydrogen, each atom has one electron, and they share these electrons to fill their outermost energy level. This sharing of electrons creates a strong bond between the two hydrogen atoms, resulting in the formation of a stable molecule of hydrogen gas. Therefore, the correct answer is covalent.

A single covalent bond involves the sharing of two electrons between two atoms. This bond is formed when two atoms come together and each contributes one electron to the shared pair. Therefore, the correct answer is 2.

NaCl is a formula unit, so 13 NaCl would mean you have 13 formula units

There are 2 hydrogen atoms in 1 molecule of H2O. You have 12 of them, so multiply 2 x 12 = 24

Ionic bonds hold cation and anions. KCl is the only compound with a cation and anion

only nonmetals are considered molecules. Na is a metal

Covalent bonds hold nonmetals together. NO2 is the only compound that have all nonmetals.

From the Homework video