Atomic structure
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The document discusses the atomic structure including protons, neutrons, and electrons. Protons and neutrons are found in the nucleus which contains over 99% of the atom's mass. Protons are positively charged while neutrons are neutral. Electrons are negatively charged and orbit the nucleus, balancing out the positive charge of the protons to give atoms a net neutral charge.
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Atomic structure
The document discusses the structure of atoms. It describes the historical understanding of atoms from Dalton's theory that atoms cannot be created or destroyed to Rutherford's discovery of the nucleus and Bohr's model of the atom. The key parts of an atom are protons, neutrons, and electrons. Protons are positively charged and located in the nucleus, electrons are negatively charged and orbit the nucleus, and neutrons have no charge and are also located in the nucleus. The number of protons defines the element. The total number of protons and neutrons is the nucleon number. Examples are provided to demonstrate how to calculate nucleon number from proton and neutron numbers.
Atomic Structure
1. Elements are the basic building blocks of all matter and are made up of atoms, which are the smallest particles of an element that retain its chemical properties.
2. Atoms consist of a tiny, dense nucleus surrounded by electrons. The nucleus contains protons and neutrons, while electrons orbit the nucleus. The number of protons determines the element.
3. Modern atomic theory developed through the works of scientists like Dalton, Thomson, Rutherford, and Bohr, who discovered the subatomic particles and proposed models of atomic structure.
Isotopes
Isotopes are atoms of the same element that have different numbers of neutrons. They have the same number of protons and electrons, so they have the same chemical properties. Some isotopes are stable while others are unstable and radioactive. Both stable and radioactive isotopes occur naturally, but radioisotopes are also produced artificially. Radioisotopes have important applications in medicine, industry, research and other areas due to their radioactive properties.
Parts on an atom
The document summarizes the key parts of an atom. An atom contains a dense nucleus at its center made of protons and neutrons. Electrons orbit the nucleus in an electron cloud with a negative charge. Everything is made of atoms, as atoms are the basic units that make up all matter. The nucleus is surrounded by electrons in energy levels, with the first level holding two electrons and the second holding eight according to the basic pattern of 2,8,8.
Structure of an Atom
- Dalton's model proposed that all matter is made of tiny particles called atoms, all atoms of the same element are alike but different from other elements, and compounds form from atoms combining in fixed proportions. Thomson's model pictured the atom as a positively charged sphere with electrons embedded within it. Rutherford's model showed that the atom's positive charge and most of its mass are concentrated in a tiny, dense nucleus at the center with electrons orbiting outside. The parts of an atom include the nucleus containing protons and neutrons at its center, surrounded by electrons. Protons have a positive charge while neutrons have no charge. Electrons have a negative charge and much less mass than protons or neutrons.
Atoms, molecules, elements, compounds, mixtures and solutions
The document defines key chemistry terms including atoms, molecules, elements, compounds, mixtures and solutions. Atoms are the smallest unit of matter that cannot be divided further. Molecules are formed when two or more atoms combine chemically. Matter is made up of elements, compounds, mixtures and solutions. Elements are made of the same type of atom, compounds contain two or more types of atoms bonded together with a specific chemical formula. Mixtures contain substances that are not chemically combined, while solutions occur when a substance dissolves evenly in another.
ION AND ITS TYPES
This document defines ions and describes the different types of ions. It states that ions are formed by the addition or removal of electrons from atoms. Positive ions, or cations, are formed when electrons are removed making the atom positively charged. Negative ions, or anions, are formed when electrons are added making the atom negatively charged. Cation formation is an endothermic oxidation reaction while anion formation is an exothermic reduction reaction. The document also explains that cations are smaller than the parent atom, while anions are larger, due to changes in nuclear charge upon electron addition or removal.
Isotopes & Atomic Mass
Magnesium has three naturally occurring isotopes: magnesium-24, magnesium-25, and magnesium-26. They have the same number of protons and electrons but different numbers of neutrons, giving them different atomic masses. Magnesium-24 makes up 79% of magnesium and has the greatest influence in calculating magnesium's average atomic mass of 24.3 amu.
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Atomic structure
The document discusses the structure of atoms. It describes the historical understanding of atoms from Dalton's theory that atoms cannot be created or destroyed to Rutherford's discovery of the nucleus and Bohr's model of the atom. The key parts of an atom are protons, neutrons, and electrons. Protons are positively charged and located in the nucleus, electrons are negatively charged and orbit the nucleus, and neutrons have no charge and are also located in the nucleus. The number of protons defines the element. The total number of protons and neutrons is the nucleon number. Examples are provided to demonstrate how to calculate nucleon number from proton and neutron numbers.
Atomic Structure
1. Elements are the basic building blocks of all matter and are made up of atoms, which are the smallest particles of an element that retain its chemical properties.
2. Atoms consist of a tiny, dense nucleus surrounded by electrons. The nucleus contains protons and neutrons, while electrons orbit the nucleus. The number of protons determines the element.
3. Modern atomic theory developed through the works of scientists like Dalton, Thomson, Rutherford, and Bohr, who discovered the subatomic particles and proposed models of atomic structure.
Isotopes
Isotopes are atoms of the same element that have different numbers of neutrons. They have the same number of protons and electrons, so they have the same chemical properties. Some isotopes are stable while others are unstable and radioactive. Both stable and radioactive isotopes occur naturally, but radioisotopes are also produced artificially. Radioisotopes have important applications in medicine, industry, research and other areas due to their radioactive properties.
Parts on an atom
The document summarizes the key parts of an atom. An atom contains a dense nucleus at its center made of protons and neutrons. Electrons orbit the nucleus in an electron cloud with a negative charge. Everything is made of atoms, as atoms are the basic units that make up all matter. The nucleus is surrounded by electrons in energy levels, with the first level holding two electrons and the second holding eight according to the basic pattern of 2,8,8.
Structure of an Atom
- Dalton's model proposed that all matter is made of tiny particles called atoms, all atoms of the same element are alike but different from other elements, and compounds form from atoms combining in fixed proportions. Thomson's model pictured the atom as a positively charged sphere with electrons embedded within it. Rutherford's model showed that the atom's positive charge and most of its mass are concentrated in a tiny, dense nucleus at the center with electrons orbiting outside. The parts of an atom include the nucleus containing protons and neutrons at its center, surrounded by electrons. Protons have a positive charge while neutrons have no charge. Electrons have a negative charge and much less mass than protons or neutrons.
Atoms, molecules, elements, compounds, mixtures and solutions
The document defines key chemistry terms including atoms, molecules, elements, compounds, mixtures and solutions. Atoms are the smallest unit of matter that cannot be divided further. Molecules are formed when two or more atoms combine chemically. Matter is made up of elements, compounds, mixtures and solutions. Elements are made of the same type of atom, compounds contain two or more types of atoms bonded together with a specific chemical formula. Mixtures contain substances that are not chemically combined, while solutions occur when a substance dissolves evenly in another.
ION AND ITS TYPES
This document defines ions and describes the different types of ions. It states that ions are formed by the addition or removal of electrons from atoms. Positive ions, or cations, are formed when electrons are removed making the atom positively charged. Negative ions, or anions, are formed when electrons are added making the atom negatively charged. Cation formation is an endothermic oxidation reaction while anion formation is an exothermic reduction reaction. The document also explains that cations are smaller than the parent atom, while anions are larger, due to changes in nuclear charge upon electron addition or removal.
Isotopes & Atomic Mass
Magnesium has three naturally occurring isotopes: magnesium-24, magnesium-25, and magnesium-26. They have the same number of protons and electrons but different numbers of neutrons, giving them different atomic masses. Magnesium-24 makes up 79% of magnesium and has the greatest influence in calculating magnesium's average atomic mass of 24.3 amu.
Atomic Theory
Atomic theory describes matter as composed of atoms, the basic units that constitute chemical elements. Democritus first proposed the idea of indivisible atoms in ancient Greece. In the early 1900s, J.J. Thomson discovered the electron and proposed a "plum pudding" model of the atom. Ernest Rutherford discovered the nucleus through alpha particle scattering experiments, leading to the planetary model of electrons orbiting the nucleus. Niels Bohr later adjusted this model to account for electron stability.
Atomic number, Mass number, Relative atomic mass and Atomic mass unit
The document discusses atomic number, mass number, and relative atomic mass. It states that the atomic number of an element equals the number of protons in its nucleus. The mass number is the sum of protons and neutrons. An example problem finds an atom has 92 protons and 146 neutrons from a given mass number of 238 and atomic number of 92. Relative atomic mass is the average mass of an atom's isotope compared to carbon-12, measured in atomic mass units.
Chapter 2 the structure of the atom
The document discusses the structure of atoms and isotopes. It begins by defining matter and the particle theory of matter. It then explains that atoms are made up of protons, neutrons and electrons. The atomic structure of various elements is discussed through their electron configurations. Isotopes are then introduced as atoms of the same element that have the same number of protons but different numbers of neutrons. Examples of isotopes including hydrogen and oxygen isotopes are provided.
Electron,nutron,proton
The document defines and describes several elementary particles and properties of atoms:
- Electrons are negatively charged subatomic particles that have no known components. They have a mass about 1/1836 that of a proton.
- Protons are positively charged subatomic particles found in the nucleus of an atom. The number of protons determines the element and its atomic number.
- Neutrons have no charge and have a mass slightly larger than protons. Along with protons, they make up the nucleus of atoms.
- The atomic number is the number of protons in an atom's nucleus and identifies the element. For neutral atoms, it equals the number of electrons.
Struture of an atom
This document provides an outline for a presentation on the history and structure of atoms. It begins with the early ideas of Democritus and Thomson, then describes the atomic models of Rutherford, Bohr, and others. The structure of the atom is explained, including the nucleus, protons, neutrons, and electrons. Isotopes and isobars are also introduced. The presentation would provide details on the key scientists and experiments that led to the current understanding of atoms as tiny particles consisting of a nucleus surrounded by electrons.
Atomic structure.ppt 1
Atoms are composed of a nucleus containing protons and neutrons surrounded by an electron cloud. The nucleus contains positively charged protons and neutral neutrons. Negatively charged electrons reside outside the nucleus in the electron cloud. The number of protons defines the identity of an element and is equal to its atomic number. The total number of protons and neutrons is the mass number. The number of electrons equals the number of protons to maintain electroneutrality. Models such as the Bohr model depict electron arrangement in shells surrounding the nucleus.
Chemistry - Chp 4 - Atomic Structure - PowerPoint
The document discusses the history and development of atomic theory and the periodic table. It describes early atomic models proposed by Democritus and Dalton. Rutherford's gold foil experiment provided evidence that atoms have a small, dense nucleus containing protons and neutrons. Elements are distinguished by their atomic number and isotopes differ in their number of neutrons. The periodic table organizes elements according to recurring trends in their physical and chemical properties, allowing relationships between elements to be identified.
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The document discusses the basics of atomic structure including what atoms are made of, their subatomic particles, and how electrons are arranged in atoms. Atoms are the building blocks of elements and consist of protons, neutrons, and electrons. The number of protons defines the element and electrons are arranged in shells around the nucleus according to certain rules.
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The document discusses electron configurations, which describe how electrons are distributed in atomic orbitals. It explains the Aufbau principle, which states that electrons fill lower energy orbitals first. The Pauli exclusion principle is described, stating that no more than two electrons can occupy any single orbital. Hund's rule is also covered, regarding the filling of degenerate orbitals. Examples are provided to illustrate these principles.
Atoms And Subatomic Particles
An atom is incredibly small, with its diameter needing to be increased 200 million times to equal the diameter of a penny. Atoms are made up of subatomic particles, including protons and neutrons in the central nucleus and electrons orbiting the nucleus. Most of an atom's mass comes from its nucleus. The number of protons determines the element and is called the atomic number. Isotopes are atoms of the same element that differ in their number of neutrons.
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The document provides information about ionic and covalent (molecular) bonding:
- Ionic bonds occur between metals and non-metals and involve the transfer of electrons. Covalent bonds occur between two non-metals and involve the sharing of electrons.
- Ionic compounds have high melting and boiling points and conduct electricity when melted or dissolved. Molecular compounds have lower melting and boiling points and do not conduct electricity.
- Ionic compounds exist as crystal lattices of ions, while molecular compounds exist as distinct molecules made of two or more nonmetal atoms bonded together.
Atoms, Element, Molecule and Compound
This document defines and provides examples of atoms, elements, molecules, and compounds. It states that atoms are the basic unit of a chemical element and are made up of protons, neutrons, and electrons. An element is made of only one type of atom, while a molecule forms when two or more atoms bond together, whether of the same or different elements. A compound contains at least two different elements bonded together. It provides examples like water (H2O) as both a molecule and compound since it contains hydrogen and oxygen atoms bonded together.
Elements, Compounds, And Mixtures
An element is a pure substance that cannot be separated into simpler substances. Elements have unique characteristic properties like melting point and reactivity that can be used to identify them. Elements are grouped into metals, nonmetals, and metalloids based on shared properties. Compounds are formed when two or more elements chemically combine to form a new substance with different properties. Mixtures are combinations of substances that do not chemically combine and can be separated physically.
Elements
Elements are pure substances that cannot be broken down further through chemical or physical means. There are currently 118 known elements, with new ones occasionally being discovered through artificial nuclear reactions. Elements are identified by their atomic number, which represents the number of protons in the nucleus. Elements are the basic building blocks of all matter and are used to create thousands of materials, though some like plutonium are also used in nuclear weapons due to their radioactive properties.
2. atomic structure
Atoms are composed of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons surround the nucleus in orbitals. Over time, scientists such as Dalton, Thomson, Rutherford, and Bohr contributed to the developing atomic model. Bohr refined Rutherford's model by proposing that electrons exist in specific energy levels or orbits around the nucleus. Elements have unique atomic structures that are indicated by their atomic number and mass number.
Structure of atom ppt
Atoms are the basic building blocks of all matter. John Dalton proposed that atoms are indivisible and identical for each element. Rutherford discovered that atoms have a small, dense nucleus at the center surrounded by electrons. Niels Bohr modeled atoms with electrons orbiting the nucleus in fixed energy levels or shells. The nucleus contains protons and neutrons, while electrons orbit outside. The number of protons determines the element, and protons and neutrons together equal the mass number.
Chemistry: Electron orbitals and sub levels
Electrons occupy specific energy levels labeled n=1, 2, 3 etc, with increasing energy as n increases. Within each level are sublevels that further organize the electrons. The s sublevel has the lowest energy, followed by p, d and f sublevels. Orbitals represent the spaces electrons occupy, with different shapes for s, p, d and f orbitals. Orbital diagrams visually depict the arrangement of electrons in orbitals and energy levels.
Ion formation
1) Chemical bonding involves the transfer or sharing of valence electrons between atoms. Valence electrons are in the outermost energy level and determine an element's chemical properties.
2) Atoms bond in order to achieve a noble gas electron configuration of 8 valence electrons, following the octet rule. Metals lose electrons to form cations, while nonmetals gain electrons to form anions.
3) Cations are positively charged ions formed when metals lose electrons. Group 1 cations have a +1 charge and Group 2 cations have a +2 charge. Transition metal cations can have varying charges. Anions are negatively charged ions formed when nonmetals gain electrons, taking on charges of -1.
Structure of atom
This document provides an overview of the structure of an atom according to different atomic models over time. It begins with Dalton's atomic theory from 1807 that atoms are fundamental units of matter. Later models include Thomson's "plum pudding" model from 1897, Rutherford's discovery of the nucleus from experiments in 1908, and Bohr's model from 1913 which proposed electrons orbit in distinct energy levels. The document then discusses the subatomic particles of protons, neutrons, and electrons and their roles. It concludes with definitions of related atomic concepts such as atomic number, mass number, isotopes, and isobars.
Atomic structure ppt
The document outlines the history of the atomic model from ancient Greek philosophers to modern atomic theory. It describes early atomic theories from Democritus and Dalton who proposed atoms as indivisible and spherical particles. It then discusses the discoveries of J.J. Thompson, Rutherford, and Bohr that led to developments in atomic structure. Key developments included the discovery of the electron by Thompson, Rutherford's nuclear model from alpha scattering experiments, and Bohr's refinement incorporating electron orbits around the nucleus. The document concludes with explanations of atomic structure including electronic configurations and dot and cross diagrams.
Atom e
This document provides information about the structure of atoms including:
- The basic subatomic particles that make up atoms are protons, neutrons, and electrons.
- Atoms can gain or lose electrons to become ions with a positive or negative charge.
- Isotopes are atoms with the same number of protons but different numbers of neutrons.
- Electrons occupy different energy levels in an atom according to specific rules. Atoms seek to fill their outer electron shells in order to achieve a stable noble gas configuration.
Elements 10
This document is a 10 element challenge that lists the symbols of 10 chemical elements and asks the reader to provide the name for each one. The elements are hydrogen, boron, phosphorus, potassium, magnesium, manganese, chlorine, nitrogen, iodine, and gold.
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Atomic theory describes matter as composed of atoms, the basic units that constitute chemical elements. Democritus first proposed the idea of indivisible atoms in ancient Greece. In the early 1900s, J.J. Thomson discovered the electron and proposed a "plum pudding" model of the atom. Ernest Rutherford discovered the nucleus through alpha particle scattering experiments, leading to the planetary model of electrons orbiting the nucleus. Niels Bohr later adjusted this model to account for electron stability.
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The document discusses atomic number, mass number, and relative atomic mass. It states that the atomic number of an element equals the number of protons in its nucleus. The mass number is the sum of protons and neutrons. An example problem finds an atom has 92 protons and 146 neutrons from a given mass number of 238 and atomic number of 92. Relative atomic mass is the average mass of an atom's isotope compared to carbon-12, measured in atomic mass units.
Chapter 2 the structure of the atom
The document discusses the structure of atoms and isotopes. It begins by defining matter and the particle theory of matter. It then explains that atoms are made up of protons, neutrons and electrons. The atomic structure of various elements is discussed through their electron configurations. Isotopes are then introduced as atoms of the same element that have the same number of protons but different numbers of neutrons. Examples of isotopes including hydrogen and oxygen isotopes are provided.
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The document defines and describes several elementary particles and properties of atoms:
- Electrons are negatively charged subatomic particles that have no known components. They have a mass about 1/1836 that of a proton.
- Protons are positively charged subatomic particles found in the nucleus of an atom. The number of protons determines the element and its atomic number.
- Neutrons have no charge and have a mass slightly larger than protons. Along with protons, they make up the nucleus of atoms.
- The atomic number is the number of protons in an atom's nucleus and identifies the element. For neutral atoms, it equals the number of electrons.
Struture of an atom
This document provides an outline for a presentation on the history and structure of atoms. It begins with the early ideas of Democritus and Thomson, then describes the atomic models of Rutherford, Bohr, and others. The structure of the atom is explained, including the nucleus, protons, neutrons, and electrons. Isotopes and isobars are also introduced. The presentation would provide details on the key scientists and experiments that led to the current understanding of atoms as tiny particles consisting of a nucleus surrounded by electrons.
Atomic structure.ppt 1
Atoms are composed of a nucleus containing protons and neutrons surrounded by an electron cloud. The nucleus contains positively charged protons and neutral neutrons. Negatively charged electrons reside outside the nucleus in the electron cloud. The number of protons defines the identity of an element and is equal to its atomic number. The total number of protons and neutrons is the mass number. The number of electrons equals the number of protons to maintain electroneutrality. Models such as the Bohr model depict electron arrangement in shells surrounding the nucleus.
Chemistry - Chp 4 - Atomic Structure - PowerPoint
The document discusses the history and development of atomic theory and the periodic table. It describes early atomic models proposed by Democritus and Dalton. Rutherford's gold foil experiment provided evidence that atoms have a small, dense nucleus containing protons and neutrons. Elements are distinguished by their atomic number and isotopes differ in their number of neutrons. The periodic table organizes elements according to recurring trends in their physical and chemical properties, allowing relationships between elements to be identified.
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The document discusses the basics of atomic structure including what atoms are made of, their subatomic particles, and how electrons are arranged in atoms. Atoms are the building blocks of elements and consist of protons, neutrons, and electrons. The number of protons defines the element and electrons are arranged in shells around the nucleus according to certain rules.
Electronic configuration final
The document discusses electron configurations, which describe how electrons are distributed in atomic orbitals. It explains the Aufbau principle, which states that electrons fill lower energy orbitals first. The Pauli exclusion principle is described, stating that no more than two electrons can occupy any single orbital. Hund's rule is also covered, regarding the filling of degenerate orbitals. Examples are provided to illustrate these principles.
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An atom is incredibly small, with its diameter needing to be increased 200 million times to equal the diameter of a penny. Atoms are made up of subatomic particles, including protons and neutrons in the central nucleus and electrons orbiting the nucleus. Most of an atom's mass comes from its nucleus. The number of protons determines the element and is called the atomic number. Isotopes are atoms of the same element that differ in their number of neutrons.
Lecture 8.1- Ionic vs. Covalent
The document provides information about ionic and covalent (molecular) bonding:
- Ionic bonds occur between metals and non-metals and involve the transfer of electrons. Covalent bonds occur between two non-metals and involve the sharing of electrons.
- Ionic compounds have high melting and boiling points and conduct electricity when melted or dissolved. Molecular compounds have lower melting and boiling points and do not conduct electricity.
- Ionic compounds exist as crystal lattices of ions, while molecular compounds exist as distinct molecules made of two or more nonmetal atoms bonded together.
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This document defines and provides examples of atoms, elements, molecules, and compounds. It states that atoms are the basic unit of a chemical element and are made up of protons, neutrons, and electrons. An element is made of only one type of atom, while a molecule forms when two or more atoms bond together, whether of the same or different elements. A compound contains at least two different elements bonded together. It provides examples like water (H2O) as both a molecule and compound since it contains hydrogen and oxygen atoms bonded together.
Elements, Compounds, And Mixtures
An element is a pure substance that cannot be separated into simpler substances. Elements have unique characteristic properties like melting point and reactivity that can be used to identify them. Elements are grouped into metals, nonmetals, and metalloids based on shared properties. Compounds are formed when two or more elements chemically combine to form a new substance with different properties. Mixtures are combinations of substances that do not chemically combine and can be separated physically.
Elements
Elements are pure substances that cannot be broken down further through chemical or physical means. There are currently 118 known elements, with new ones occasionally being discovered through artificial nuclear reactions. Elements are identified by their atomic number, which represents the number of protons in the nucleus. Elements are the basic building blocks of all matter and are used to create thousands of materials, though some like plutonium are also used in nuclear weapons due to their radioactive properties.
2. atomic structure
Atoms are composed of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons surround the nucleus in orbitals. Over time, scientists such as Dalton, Thomson, Rutherford, and Bohr contributed to the developing atomic model. Bohr refined Rutherford's model by proposing that electrons exist in specific energy levels or orbits around the nucleus. Elements have unique atomic structures that are indicated by their atomic number and mass number.
Structure of atom ppt
Atoms are the basic building blocks of all matter. John Dalton proposed that atoms are indivisible and identical for each element. Rutherford discovered that atoms have a small, dense nucleus at the center surrounded by electrons. Niels Bohr modeled atoms with electrons orbiting the nucleus in fixed energy levels or shells. The nucleus contains protons and neutrons, while electrons orbit outside. The number of protons determines the element, and protons and neutrons together equal the mass number.
Chemistry: Electron orbitals and sub levels
Electrons occupy specific energy levels labeled n=1, 2, 3 etc, with increasing energy as n increases. Within each level are sublevels that further organize the electrons. The s sublevel has the lowest energy, followed by p, d and f sublevels. Orbitals represent the spaces electrons occupy, with different shapes for s, p, d and f orbitals. Orbital diagrams visually depict the arrangement of electrons in orbitals and energy levels.
Ion formation
1) Chemical bonding involves the transfer or sharing of valence electrons between atoms. Valence electrons are in the outermost energy level and determine an element's chemical properties.
2) Atoms bond in order to achieve a noble gas electron configuration of 8 valence electrons, following the octet rule. Metals lose electrons to form cations, while nonmetals gain electrons to form anions.
3) Cations are positively charged ions formed when metals lose electrons. Group 1 cations have a +1 charge and Group 2 cations have a +2 charge. Transition metal cations can have varying charges. Anions are negatively charged ions formed when nonmetals gain electrons, taking on charges of -1.
Structure of atom
This document provides an overview of the structure of an atom according to different atomic models over time. It begins with Dalton's atomic theory from 1807 that atoms are fundamental units of matter. Later models include Thomson's "plum pudding" model from 1897, Rutherford's discovery of the nucleus from experiments in 1908, and Bohr's model from 1913 which proposed electrons orbit in distinct energy levels. The document then discusses the subatomic particles of protons, neutrons, and electrons and their roles. It concludes with definitions of related atomic concepts such as atomic number, mass number, isotopes, and isobars.
Atomic structure ppt
The document outlines the history of the atomic model from ancient Greek philosophers to modern atomic theory. It describes early atomic theories from Democritus and Dalton who proposed atoms as indivisible and spherical particles. It then discusses the discoveries of J.J. Thompson, Rutherford, and Bohr that led to developments in atomic structure. Key developments included the discovery of the electron by Thompson, Rutherford's nuclear model from alpha scattering experiments, and Bohr's refinement incorporating electron orbits around the nucleus. The document concludes with explanations of atomic structure including electronic configurations and dot and cross diagrams.
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Atomic number, Mass number, Relative atomic mass and Atomic mass unit
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The Rutherford gold foil experiment discovered the atomic nucleus. In this experiment, Rutherford beamed particles at a gold foil and observed some particles bouncing back at large angles, indicating a small, dense nucleus at the center of the atom. Dalton's atomic theory proposed that atoms of different elements can combine in simple whole number ratios to form compounds. Isotopes are atoms that have the same number of protons but different numbers of neutrons, giving them the same atomic number but different atomic mass numbers. The periodic table arranges elements into groups based on repeating properties and allows easy comparison of elemental properties.
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Ps ch 3_presentation
This document provides an overview of atomic structure and the periodic table. It defines protons, neutrons, and electrons, and describes early atomic models including the Bohr model. It introduces electron orbitals and explains how they relate to an element's valence electrons and position on the periodic table. The document then explores periodic trends in atomic properties, including metals, nonmetals, and noble gases. It defines ions, isotopes, and molar mass, and discusses using moles as a unit for counting particles.
Applied Chapter 3.2 : Structure of Atoms
This document describes the subatomic particles that make up atoms - protons, neutrons, and electrons. It discusses their properties and discoveries. Atoms are identified by their atomic number, which is the number of protons, and also the number of electrons. Isotopes are atoms of the same element with different numbers of neutrons. The mass number is the total number of protons and neutrons. Examples are provided to demonstrate calculating the numbers of each type of particle in different isotopes.
Shells/ Valence Electrons
The document discusses the periodic table and properties of elements. It explains that each row of the periodic table is called a period, with elements in the same period having the same number of electron shells. It also explains that each column is called a group, with elements in the same group having the same number of valence electrons in their outer shell. The document provides examples of determining the number of shells and valence electrons for various elements based on their period and group.
Valence Electrons Worksheet
This document is a worksheet about valence electrons that contains questions asking students to:
1) Identify the number of electrons in various elements.
2) Draw Lewis structures and identify the number of outer shell electrons for different elements.
3) Identify the number of valence electrons elements have by filling in their electron configurations.
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.
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Gravity and inertia work together to keep planets in orbit around the Sun. Gravity provides an attractive force based on the masses of the planet and Sun that curves the planet's path. Inertia causes objects to travel in a straight line, but gravity pulls planets into an elliptical orbit rather than flying off into space in a straight line. Ancient models incorrectly thought Earth was the center, but it is now known that planets revolve around the Sun.
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The moon's surface has light and dark colored areas visible from telescopes. Large craters formed from impacts with space objects, and there are also large, flat dark areas called maria that appear smooth. The maria were formed when huge impacts caused lava to fill the impacted areas, and after cooling the lava gave the maria their dark, smooth appearance, though early observers mistakenly thought they were seas.
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Disclaimer: No one is perfect, so please mind that there might be mistakes and typos.
dtubbenhauer@gmail.com
Corrected slides: dtubbenhauer.com/talks.html
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Atomic structure
- 1. Atomic Structure • Arrangement and number of sub-atomic particles •Protons •Neutrons •Electrons
- 2. •Center or core of an atom •Contains 99.9% of the weight of an atom •Contains protons and neutrons
- 3. •Positively Charged Sub-atomic particles •Found in the nucleus •All protons are a like
- 4. •Neutrally charged (no charge) sub-atomic particle •Found in nucleus
- 5. •They are the negatively charged particles orbiting the nucleus. •It is much smaller than the protons and the neutrons .
- 6. What is the net charge of the atom ? • The atom is formed of positively charged proton in the nucleus and negatively charged electrons in the energy level ,but they are equal to each other in number ,making the net charge of the atom “neutral”. No of positive protons = No of negative electrons