Chemistry: Valence Electrons and Bonding

Electrons in the outermost shell of an atom that are involved in chemical bonding, influencing how an atom interacts with other atoms.

Transition metals, unlike other elements, can use electrons from inner shells as valence electrons, contributing to their diverse properties.

Elements in Group 2 of the periodic table's 4th row have two valence electrons, impacting their bonding behavior.

The net electrical charge of an atom after it gains or loses electrons.

When an atom gains electrons, it becomes negatively charged, with the number of gained electrons determining the charge.

When an atom loses electrons, it becomes positively charged, with the number of lost electrons determining the charge.

A type of chemical bond formed between a metal (few valence electrons) and a nonmetal (many valence electrons) through the transfer of electrons. This results in the formation of oppositely charged ions that attract each other.

A type of chemical bond that occurs between closely packed, positively charged metal ions, where electrons are delocalized and can move freely. This makes metals good conductors of electricity and heat.

A type of chemical bond formed between atoms with similar numbers of valence electrons (typically between metals) where electrons are shared between the atoms. This leads to stable, neutral molecules.

In ionic bonds, electrons are completely transferred from one atom to another, forming oppositely charged ions that attract each other.

Electrons in metallic bonds are delocalized, meaning they can move freely throughout the metal lattice, making metals good conductors of electricity and heat.

In covalent bonds, electrons are shared between two atoms, resulting in a stable, neutral molecule. Each atom contributes to the shared electron pair.

Due to their strong, delocalized bonds, metals often have high melting points. This requires considerable energy to overcome the strong attractive forces between the metal ions and their shared electrons.

Ionic compounds readily dissolve in water, as water molecules can effectively surround and separate the ions, disrupting their electrostatic interactions and allowing them to move independently in solution.

Breaking covalent bonds, as seen in the explosive decomposition of dynamite, releases significant energy due to the strong attraction between the shared electrons in the bond.

Compounds have unique properties that differ from their constituent elements due to the chemical reactions that occur during their formation. This is because new bonds are formed, altering the properties of the individual atoms.

The three-dimensional arrangement of atoms in a molecule. Molecular shape influences the molecule's polarity, as symmetrical molecules tend to be nonpolar, while asymmetrical molecules are usually polar.

A special type of intermolecular interaction where a hydrogen atom bonded to a highly electronegative atom (like oxygen, nitrogen, or fluorine) is attracted to a lone pair of electrons on a nearby electronegative atom. These weak bonds play a crucial role in holding water molecules together, influencing its properties.

Different proportions of the same elements can result in different oxides with distinct properties. For example, carbon monoxide (CO) is toxic, while carbon dioxide (CO2) is essential for life.

The general formula for acids typically begins with H2 followed by an element or group that ends in 'ate' based on specific naming conventions. For example, sulfuric acid is H2SO4.