Bohr Diagrams
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A step by step program for creating Bohr Diagrams and Electron dot structures. Usefule for Index Cards and Flash cards for chemistry and physical science students Grades 9-12 or freshman college
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- Lewis structures show valence electron bonding using dots. Molecular shape is predicted by VSEPR to minimize electron pair repulsions based on the steric number.
- Resonance structures average to best depict molecules like HNO3 that resonate between structures. Formal charges help identify the most stable Lewis structure.
Bohr Rutherford Atomic Model
The document describes the Bohr-Rutherford atomic model. It states that the atom consists of a small, dense nucleus containing protons and neutrons, surrounded by electrons in shells. The atomic number equals the number of protons, and a neutral atom has the same number of protons and electrons. Electrons are located in shells outside the nucleus, with the first shell holding 2 electrons and subsequent shells able to hold more. Diagrams illustrate atoms showing their arrangement of subatomic particles. Examples are provided of looking up atomic properties and drawing Bohr-Rutherford diagrams for different elements.
3a d,3h atomic structure info + qs
The document provides information about atomic structure including:
- Atoms consist of a nucleus surrounded by electrons, with protons and neutrons in the nucleus.
- Electrons are arranged in shells, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each.
- The number of protons equals the atomic number and number of electrons. Neutrons plus protons equals the mass number.
- Students are assigned tasks to learn about electron configurations, atomic shorthand, and properties of elements based on their position in the periodic table.
Periodic table and elements along with a
All notes on the atomic structure and the periodic table. Very easy to understand and fill with simple explanations
Atomic structure
This document defines key concepts in chemistry including matter, atoms, molecules, subatomic particles, atomic number, mass number, moles, and the periodic table. It explains that atoms are made up of protons, neutrons, and electrons. The atomic number is the number of protons, and the mass number includes both protons and neutrons. It also defines what a mole is and how it relates to atomic mass. The periodic table is arranged based on atomic number and electronic configuration.
Valence Electrons
Valence electrons are the outermost shell electrons of an atom that are involved in bonding. Elements in the same group on the periodic table have the same number of valence electrons because they exhibit similar chemical properties based on their valence electron configuration. Atoms seek to attain a full outer shell of 8 electrons to achieve stability through gaining, losing or sharing valence electrons in chemical bonds.
Atomic models are useful because they allow us to picture what is in.docx
Atomic models are useful because they allow us to picture what is inside of an atom, something we will never be able to actually see. We're going to talk about two models, the Bohr model and the Quantum model. While we know that the Quantum model is the correct way to represent atoms, the Bohr model is still useful for a very basic understanding. Think of it as a stick figure sketch of an atom. The parts are all there, its just not quite filled in all of the way.
Bohr Model
The Bohr model of the atom was developed in 1914 by Niels Bohr. In this model, electrons move around the nucleus in fixed, concentric circles. Picture the planets orbiting the Sun. These circles are called energy levels and electrons must have a specific amount of energy to be in each level. The energy levels closest to the nucleus require the least amount of energy. In order for an electron to move further from the nucleus (or move up an energy level) they must gain energy. If they lose energy they fall down to an energy level closer to the nucleus.
Drawing the Bohr model for an atom gives you valuable information about the atom's valence electrons. The
valence electrons
--
those in the outermost energy leve
l--are the ones that determine the chemical properties of an atom. In order to draw a Bohr model you must first use the periodic table to tell you the number of protons, neutrons, and electrons in an atom. For Bohr models we usually draw what the "average" atom for that element looks like and just round the average atomic mass to a whole number and use that for the mass number.
Steps for Drawing a Bohr Model:
1. Count the number of protons, electrons, and neutrons for that atom.
2. Draw the nucleus. Indicate the correct number of protons and neutrons in the nucleus.
3. Draw energy levels around the nucleus, starting with the energy level closest to the nucleus. Fill up each energy level before moving on to the next.
Each energy level in a Bohr model can only hold a specific number of electrons, as shown in the table below.
Energy Level
Max # of electrons
1
2
2
8
3
18
4
32
For example, here is a Bohr model for the average oxygen atom:
Here is one for phosphorus:
You try drawing one for Magnesium (Mg) and for Boron (B). Count the number of electrons on the outermost energy level to find the number of valence electrons. Check your answers by looking at the handout.
Quantum Model
In 1925 the Quantum model of the atom was developed after it was determined that electrons can behave like a wave and a particle at the same time. In addition, you can't know the precise location of an electron. Instead of traveling in orderly circles around the nucleus, we describe the electrons as existing in a three-dimensional
electron cloud
--a shape surrounding the nucleus. You will learn more about the Quantum model in chemistry.
These are some of the orbital shapes possible in the first two energy levels of an atom.
Draw a Bohr model for elements wi.
chemical bonding
Atoms form bonds to attain a lower potential energy state. They do this through ionic bonds, where oppositely charged ions attract, or covalent bonds, where atoms share valence electrons. Whether a bond is ionic or covalent depends on the electronegativity difference between the atoms. Ionic bonds form between metals and nonmetals, while covalent bonds form between two nonmetals. Lewis structures use dots to represent valence electrons and show how atoms share electrons to achieve stable configurations like noble gases. Valence shell electron pair repulsion theory explains molecular shapes based on electron pair positioning.
SLM- Molecular structure Class- 8
This document discusses the molecular structure of atoms. It begins by explaining that all substances are composed of elements, which are the basic substances, and that elements are made up of very small particles called atoms. It then describes the basic structure of an atom, including that atoms have a small, positively charged nucleus surrounded by negatively charged electrons. The number of protons determines the element and equals the number of electrons. Atoms can gain, lose, or share electrons to attain stable electron configurations, forming ions or molecules.
Bohr diagrams
This document discusses the key parts of an atom including atomic number, mass, protons, neutrons, and electrons. It explains that the atomic number tells us the number of protons and it shows how to calculate neutrons by subtracting the atomic number from the atomic mass. The number of electrons is the same as the number of protons to maintain neutral charge. It demonstrates this process for carbon and neon atoms and teaches how to draw Bohr diagrams showing the nucleus and electron shells.
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Atomic models are useful because they allow us to picture what is in.docx
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Electronconfig
Rutherford discovered that the atom has a small, dense nucleus at its center, changing the old atomic model. Niels Bohr is most responsible for the current atomic model, which uses quantum mechanics to describe electrons orbiting the nucleus in shells and subshells based on their energy levels. Electrons fill these orbitals according to specific rules.
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