Unit 7
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Chemistry is the science concerned with the composition, structure, and properties of matter, as well as the changes during chemical reactions. It includes disciplines like general chemistry, inorganic chemistry, organic chemistry, and biochemistry. A substance has a definite composition and set of properties, while an element consists of a single type of atom defined by its atomic number. Compounds contain different elements in specific ratios. Atoms are the basic units that make up elements and can combine through chemical bonds to form compounds.
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These notes are based on the Introduction to Biology 1: The Chemistry of Biology - Atoms, Molecules, and How They Support Life. I do apologize that some of it did not load correctly, but hopefully, your book will fill in those parts.
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This document discusses key chemistry concepts important for understanding biology. It explains that organisms are made of macromolecules, which are made of smaller molecules and atoms. Atoms are the smallest units and are made up of protons, neutrons and electrons. The number and arrangement of protons and neutrons determines an element's identity and properties. Elements can have different isotopes that vary in their number of neutrons. Atoms combine through ionic bonds, where they transfer electrons, or covalent bonds, where they share electrons to form molecules and compounds with unique properties.
Valence Shell of the Atom
There are several misconceptions about the valence shell of the atom. The key questions that arise in the minds of the learners are:
Is valence shell really the outermost shell?
2. Are there only seven shells in an atom?
3. When shells are supposed to be made up of subshells, why can we not represent the subshells in the valence shell structure of the atom?
4. When electrons are said to occur in orbitals, why can we not indicate the orbitals in the valence shell structure?
4. How can we represent the origins for valance band and conduction band in the atomic structure?
5. What are some good metaphors for the core of the atom and the rest of the atom?
Here is a lesson created by Chemistry teachers to address these misconceptions.
Applied Chemistry.pptx
The document provides an outline for an applied chemistry course. It covers topics such as physical chemistry, atomic structure and bonding, mechanical properties, thermo-chemistry, electrochemistry, industrial chemistry, and water treatment methods. It lists textbooks and defines applied chemistry as the scientific field for understanding basic chemical properties and producing new materials. Applied chemistry includes areas like physical chemistry, materials chemistry, chemical engineering, and environmental chemistry. Examples given are laundry detergents and oil refineries.
Grade 8 chemistry vocabulary list
I originally created this document for a grade 9 class, but now I use if more often with my grade 8 students.
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Class 9 Science Chapter 3 Atoms and Molecules notes pdf free pdf download
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- 3. Inorganic chemistry: the study of inorganic matter.
- 4. Organic chemistry: the study of organic (carbon based) matter.
- 5. Biochemistry: the study of substances found in biological organisms.
- 7. Element is a substance which is composed of a single type of atom. A chemical element is characterized by a particular number of protons in the nuclei of its atoms (the atomic number ). For example, all atoms with 6 protons in their nuclei are atoms of the chemical element carbon, and all atoms with 92 protons in their nuclei are atoms of the element uranium.
- 8. Compound is a substance with a particular ratio of atoms of particular chemical elements which determines its composition, and a particular organization which determines chemical properties. For example, water is a compound containing hydrogen and oxygen in the ratio of two to one.
- 9. Strictly speaking, a mixture of compounds, elements or compounds and elements is not a chemical substance, but it may be called a chemical or a mixture . Most of the substances we encounter in our daily life are some kind of mixture; for example: air, alloys, biomass, etc.
- 11. Element: a chemical element is a substance which is composed of a single type of atom. It is characterized by a particular number of protons in the nuclei of its atoms. This number is known as the atomic number of the element. For example, all atoms with 6 protons in their nuclei are atoms of the chemical element carbon, and all atoms with 92 protons in their nuclei are atoms of the element uranium.
- 12. Isotopes are atoms of one element (same number of protons in their nuclei) with a different number of number of neutrons.
- 13. Ion is a charged atom (or a molecule), that has lost or gained one or more electrons. Positively charged: cations (e.g. sodium cation Na+). Negatively charged: anions (e.g. chloride Cl−)
- 16. The octet rule is a simple chemical rule that states that atoms tend to combine in such a way that they each have eight electrons in their valence shells , giving them the same electronic configuration as a noble gas.
- 17. An ionic bond , the bonding electron is not shared at all, but transferred. In this type of bond, the outer atomic orbital of one atom has a vacancy which allows addition of one or more electrons. These newly added electrons potentially occupy a lower energy-state (effectively closer to more nuclear charge) than they experience in a different atom. Thus, one nucleus offers a more tightly bound position to an electron than does another nucleus, with the result that one atom may transfer an electron to the other. This transfer causes one atom to assume a net positive charge, and the other to assume a net negative charge. The bond then results from electrostatic attraction between atoms, and the atoms become positive or negatively charged ions.
- 19. Metallic bonding is the electromagnetic interaction between delocalized electrons, called conduction electrons and gathered in an "electron sea", and the metallic nuclei within metals. Understood as the sharing of "free" electrons among a lattice of positively charged ions (cations). Metallic bonding accounts for many physical properties of metals, such as strength, malleability, ductility, thermal and electrical conductivity, opacity, and luster.