Periodic table-shells-valence
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Each row of the periodic table is called a period. Elements in the same period have the same number of electron shells. Each column is called a group. Elements in the same group have the same number of valence electrons, except for helium which has two electrons. Valence electrons are the outermost electrons of an atom and are involved in bonding. Reactive elements bond easily to gain or lose valence electrons to achieve a full outer electron shell of eight electrons.
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Early chemists believed matter was made of four elements - air, earth, fire and water. Later, it was discovered that all matter is composed of atoms, which contain protons, neutrons and electrons. Atoms of the same element have the same number of protons but can differ in neutrons, forming isotopes. Chemical bonds form when atoms gain, lose or share electrons to achieve stable electron configurations, resulting in ionic bonds between oppositely charged ions, or covalent bonds where atoms share electrons. Chemical reactions occur when bonds are formed or broken.
Covalent Bonds
The document summarizes key concepts about covalent bonds, including how they form through the sharing of valence electrons between atoms to achieve stability. It discusses ionic vs. covalent bonds, how covalent bonds are represented using Lewis dot structures, and how the octet rule determines bonding patterns for atoms in different groups on the periodic table. Examples of writing Lewis dot structures for several diatomic and polyatomic molecules are provided.
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.
Interactive textbook ch. 13 chemical bonding
Ionic bonds form when valence electrons are transferred from metal atoms to nonmetal atoms, resulting in positively charged metal ions and negatively charged nonmetal ions that are attracted to each other. Metal atoms easily lose electrons to achieve stable full outer energy levels, while nonmetal atoms gain electrons for the same reason. The ions associate in repeating three-dimensional crystal lattices to form solid ionic compounds that are brittle with high melting points and often dissolve in water.
Atoms
1) Atoms are the smallest units that make up matter and consist of protons, neutrons and electrons. Electrons orbit the nucleus in shells.
2) There are two main types of bonds between atoms - ionic bonds which involve transfer of electrons between metals and non-metals, and covalent bonds which involve sharing of electrons between non-metals.
3) Isotopes are atoms of the same element that have different numbers of neutrons, giving them different masses but the same chemical properties. Radioactive isotopes are unstable and decay over time.
Chemical Bonding Template for free use.pptx
This is a chemical bonding template, so you can download and use it for free.
Chemistry - Midterm Study Guide 2011
The document provides information about an upcoming Chemistry Midterm Exam, including:
- The exam is divided into 3 sections testing multiple choice, short answer, and mixed question types.
- Students should bring a calculator, pen, and pencil, as reference tables will be provided.
- The exam covers 12 topics such as matter and change, atomic structure, bonding, and chemical reactions.
- The purpose of the review packet is to highlight key ideas from the course that will be on the exam, and should be used along with other study materials to thoroughly prepare for the test. Active study is required to do well.
Learn Basics of chemistry myassignmenthelp.net
Early chemists believed that all matter was composed of combinations of four elements - air, earth, fire and water. Later, it was discovered that all matter is composed of atoms, which are mostly empty space. Atoms contain electrons, protons and neutrons. Electrons orbit the nucleus in distinct energy levels. The number of protons determines the element. Chemical bonds form when atoms gain, lose or share electrons to achieve a full outer energy level. There are three main types of bonds - ionic, covalent and metallic. Chemical reactions occur when bonds are formed or broken.
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.
Lewis structuresvsepr theory cheat sheet
1. The document provides an overview of key concepts for Lewis structures and VSEPR theory, including how to draw Lewis structures for covalent compounds and ions.
2. It explains valence shell electron pair repulsion theory (VSEPR) which is used to predict the 3D shape of molecules based on electron pairs around a central atom.
3. A table is included that lists common molecular geometries determined by VSEPR theory based on the number of electron regions around the central atom.
Chemistry - Midterm Study Guide 2011
The document provides information about the Chemistry Midterm Exam, including its three sections and topics covered. It notes the exam allows one class period and a scientific calculator. The exam covers 12 topics such as matter and change, the periodic table, and chemical reactions. The purpose of the review packet is to help students prepare for the exam using key ideas from the core curriculum along with their own notes, review sheets, and reference tables. Active preparation is necessary as there are no shortcuts to passing.
Elements and Chemical Bonds
Atoms bond together by sharing or transferring valence electrons. Valence electrons are found in the outermost energy level of an atom and participate in chemical bonding. The number of valence electrons an atom has determines how many bonds it can form. Atoms are most stable when they have eight valence electrons, as this full outer energy level is very unlikely to react. Atoms with fewer than eight valence electrons seek to gain or share electrons through bonding in order to achieve a stable electron configuration.
G9 chemistry vocabulary
A nearly-comprehensive list of vocabulary terms needed for introductory chemistry in grade 9 science, including a variety of source websites for reference.
Ionic Trends
The document discusses ionic trends in atomic radius, ionization energy, and electronegativity across the periodic table. It explains that atomic radius generally decreases from left to right as more protons are added to the nucleus, attracting the electrons closer. Ionization energy decreases from right to left as the right side has more full valence shells, making them less likely to lose electrons. Electronegativity increases from left to right and decreases down groups as the distance from the valence electrons to the nucleus changes.
Periodic trends
The document discusses periodic trends in elemental properties, including atomic radius, ionization energy, electron affinity, electronegativity, and reactivity. It explains that Dmitri Mendeleev was the first to organize elements into a periodic table based on their properties and predicted undiscovered elements. The trends are due to changes in atomic structure and the effective nuclear charge as protons and electrons are added. Atomic radius generally decreases left to right and increases top to bottom. Ionization energy and electronegativity increase as you move up and to the left on the periodic table.
Basic electronics
This document provides information about atomic structure and bonding. It discusses:
- The basic components of atoms (protons, neutrons, electrons) and their properties.
- Electron orbitals and energy levels within atoms. Electrons occupy discrete shells and energy levels.
- Covalent bonding between atoms, where valence electrons are shared. This forms crystalline structures.
- Semiconductors like silicon and germanium have incomplete valence shells, so their atoms form covalent bonds to share electrons until each has a full outer shell. This tightly binds electrons.
- Doping semiconductors with impurities introduces extra electrons or holes, increasing conductivity and making the material n-type or p-
Human Physiology Chemistry
Human physiology involves the study of molecules, cells, tissues, organs and organ systems that make up the human body. At the most basic level, atoms combine through chemical bonds like ionic and covalent bonds to form molecules, which then organize into cells. Cells further organize into tissues and organs to carry out specific functions and form organ systems that allow the human body to function as a whole.
CHEMICAL BONDING2012 PART1.pptx
Chemical bonds form as atoms attempt to achieve stable electronic configurations like noble gases. There are three main types of bonds: ionic bonds form when atoms transfer electrons to become ions that are attracted via opposite charges. Covalent bonds form when atoms share electrons to achieve full outer shells. Coordinate bonds occur when a central atom shares an electron pair with two other atoms.
Ss Chapter 3
This document summarizes key concepts about atomic structure and the periodic table. It explains that atoms are made up of protons, neutrons, and electrons, with protons and neutrons located in the nucleus and electrons in shells surrounding the nucleus. The periodic table arranges elements based on their atomic number and properties. Elements can be classified as metals, nonmetals, metalloids, or noble gases. Atoms can undergo radioactive decay, emitting alpha, beta, or gamma particles as they change to different elements. Nuclear fission and fusion can also occur.
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