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Matter is anything that occupies space and has mass. It is classified into pure substances and mixtures. Pure substances have a fixed composition and cannot be further purified, while mixtures are combinations of two or more pure substances that can be separated.
Pure substances have a fixed composition and cannot be further purified. They are further classified into elements and compounds. Elements cannot be subdivided by chemical or physical means, while compounds are made up of two or more elements united in fixed ratios by mass.
Elements are the simplest form of matter that cannot be broken down into simpler substances, while compounds are substances formed when two or more elements chemically combine in fixed ratios.
Mixtures are classified into homogeneous and heterogeneous mixtures. Homogeneous mixtures have a uniform composition, while heterogeneous mixtures have a non-uniform composition.
Blood is an example of a heterogeneous mixture when viewed microscopically, as it contains various components that are not uniformly distributed.
Important elements in the human body include Sodium (Na) for regulating electrical balance, Potassium (K) for nerve conduction, Calcium (Ca) for strengthening bones and teeth, Phosphorus (P) for energy storage in DNA and RNA, Iodine (I) for thyroid hormone production, and Iron (Fe) for oxygen transport in hemoglobin.
Elements are classified into metals, nonmetals, and metalloids. Metals are good conductors of heat and electricity, nonmetals are poor conductors, and metalloids possess properties of both.
Metals, found on the left portion of the periodic table, are typically solid at room temperature (except for mercury), are good conductors of heat and electricity, and have high melting and boiling points.
Nonmetals, located on the right portion of the periodic table, are poor conductors of heat and electricity, can exist in various states at room temperature (solid, liquid, or gas), and include elements like sulfur and carbon.
Metalloids possess properties of both metals and nonmetals and are found along the zigzag line on the periodic table. Examples include Boron, Silicon, and Arsenic.
A compound is a substance made up of two or more elements united in fixed ratios by mass. For example, water is a compound formed from two hydrogen atoms and one oxygen atom.
Atoms can be illustrated using molecular formulas, structural formulas, ball-and-stick models, and space-filling models, each providing different levels of detail about the arrangement of atoms.
The nucleus of an atom is a dense core that contains protons and neutrons, which are surrounded by electrons that occupy various energy levels.
Electrons are arranged in energy levels, starting from the lowest energy orbital. Each orbital can hold a maximum of two electrons with opposite spins, and when orbitals are equal in energy, one electron is added to each before any orbital is completely filled.
The periodic table organizes elements based on their atomic number, electron configuration, and recurring chemical properties, allowing for the prediction of element behavior and the relationships between different elements.
Understanding the classification of matter is crucial for identifying substances, predicting their behavior in chemical reactions, and applying this knowledge in practical applications such as medicine, engineering, and environmental science.
Trace elements, though required in small amounts, are essential for various biological functions, including enzyme activity, hormone production, and maintaining overall health.
Chemical bonds form when atoms share or transfer electrons, resulting in the formation of molecules or compounds. The type of bond (ionic, covalent, or metallic) depends on the elements involved and their electronegativity.
Ionic bonds form through the transfer of electrons from one atom to another, resulting in charged ions, while covalent bonds form when two atoms share electrons to achieve stability.
Electronegativity is a measure of an atom's ability to attract electrons in a bond. It influences whether a bond will be ionic or covalent, as differences in electronegativity between atoms determine the nature of the bond formed.
The octet rule states that atoms tend to bond in such a way that they have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases.