Chemical Bonding | Ionic and Covalent | Grade 9 Science Quarter 2 Week 2

Recent questions

• What is chemical bonding?

  Chemical bonding refers to the lasting attraction between atoms, ions, or molecules that results in the formation of chemical compounds. This fundamental concept in chemistry explains how different elements interact to create various substances. There are primarily two types of chemical bonds: ionic and covalent. Ionic bonding occurs when electrons are completely transferred from one atom (usually a metal) to another (usually a non-metal), leading to the formation of charged ions. In contrast, covalent bonding involves the sharing of electron pairs between non-metal atoms, allowing them to achieve stability. Understanding chemical bonding is crucial for grasping how compounds are formed and how they behave in different environments.

• What are ionic compounds?

  Ionic compounds are chemical compounds formed through ionic bonding, which involves the complete transfer of electrons from metals to non-metals. This process results in the creation of positively charged ions (cations) and negatively charged ions (anions). A classic example of an ionic compound is sodium chloride, commonly known as table salt, which is formed when sodium (a metal) loses an electron and chlorine (a non-metal) gains that electron. Ionic compounds typically exhibit distinct properties: they exist only in solid form, possess high melting and boiling points, and are soluble in water but generally insoluble in organic solvents. These characteristics make ionic compounds essential in various applications, including in biological systems and industrial processes.

• How do covalent bonds work?

  Covalent bonds are formed when two non-metal atoms share electron pairs, allowing them to achieve a more stable electronic configuration. This type of bonding is crucial for the formation of many essential compounds, such as water (H2O), where oxygen shares electrons with two hydrogen atoms. Covalent bonds can be classified into two categories: non-polar and polar. Non-polar covalent bonds occur when electrons are shared equally between atoms, as seen in diatomic molecules like hydrogen (H2). In contrast, polar covalent bonds involve unequal sharing of electrons, leading to partial charges on the atoms, as exemplified by the bond between hydrogen and fluorine. The nature of covalent bonds significantly influences the physical and chemical properties of the resulting compounds.

• What are the properties of ionic compounds?

  Ionic compounds possess several distinctive properties that set them apart from other types of compounds. They exist only in solid form at room temperature and are characterized by high melting and boiling points due to the strong electrostatic forces of attraction between the oppositely charged ions. Additionally, ionic compounds are soluble in water, which allows them to dissociate into their constituent ions, making them conductive in aqueous solutions. However, they are generally insoluble in organic solvents. These properties are a direct result of the ionic bonding that holds the compound together, making ionic compounds vital in various applications, including in the production of salts and electrolytes.

• What are covalent compounds?

  Covalent compounds are substances formed through covalent bonding, where non-metal atoms share electron pairs to achieve stability. Unlike ionic compounds, covalent compounds can exist in various states: solids, liquids, or gases, depending on the specific compound and its molecular structure. They typically have lower melting and boiling points compared to ionic compounds, reflecting the weaker forces holding the molecules together. Covalent compounds are generally insoluble in water but can be soluble in organic solvents, which is a key factor in their behavior in different environments. The conductivity of covalent compounds is very low, as they do not dissociate into ions in solution. Understanding the properties of covalent compounds is essential for exploring their applications in chemistry and industry.