Lesson: Wednesday 9/2
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The document discusses the composition of atoms. It states that atoms are made up of three subatomic particles: protons, neutrons, and electrons. It provides details on the properties of each particle, including their charge (protons are positive, electrons are negative, neutrons have no charge) and mass (protons and neutrons have a mass of approximately 1 atomic mass unit, electrons have virtually no mass).
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Atoms intro (2)
Atoms are extremely small, around three one-hundred-millionths of a centimeter. Atoms are made up of a nucleus containing protons and neutrons, and electrons that orbit the nucleus. The nucleus contains positively charged protons and neutral neutrons, while negatively charged electrons surround it. Elements are defined by the number of protons, which determines the element's identity, while isotopes of an element can vary in their number of neutrons. Ions are formed when atoms gain or lose electrons.
Electricity 1
Electrical charges are caused by positive and negative charges from protons and electrons. All objects begin neutral but can become positively or negatively charged by gaining or losing electrons. There are two forces between charged objects - attraction between opposite charges and repulsion between like charges. Charges can be induced through friction, conduction, or induction without direct contact. The triboelectric series ranks materials based on their ability to gain or lose electrons through friction charging.
Notes lab 04b the atom structure
Elements are made of atoms, which are the basic building blocks of matter. Atoms consist of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons surround the nucleus in electron clouds. Protons are positively charged, electrons are negatively charged, and neutrons have no charge. The number of protons determines the element and its atomic number. The total number of protons and neutrons determines the atom's mass number. Elements are organized on the periodic table based on their atomic structure.
subatomic particles
Protons, neutrons, and electrons are the three main subatomic particles. Protons have a positive charge, neutrons have no charge, and electrons have a negative charge. Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. The atomic number identifies the number of protons in an atom's nucleus, while atomic mass refers to the total number of protons and neutrons.
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,chemsitry ,igcse ,0620 ,lesson ,atoms ,subatomic particles ,protons ,neutrons ,electrons ,atomic mass ,atomic number ,neutral ,charge ,postitive ,negatie
IGCSE 0620 Lesson 1 Slide 1
,chemsitry ,igcse ,0620 ,lesson ,atoms ,subatomic particles ,protons ,neutrons ,electrons ,atomic mass ,atomic number ,neutral ,charge ,postitive ,negatie
Subatomic Particles and Isotopes
This document discusses subatomic particles, isotopes, and ions. It defines atoms as the smallest unit of matter that retains chemical properties. Atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit the nucleus. The number of protons determines the element, while the number of neutrons defines the isotope. Ions are formed when atoms gain or lose electrons, becoming positively or negatively charged. Practice problems are provided to calculate subatomic particle numbers for elements, isotopes, and ions.
Atoms
Matter is composed of basic building blocks called atoms. Atoms were originally thought to be indivisible spheres, but are now understood to have internal structure. Atoms contain a tiny, dense nucleus of protons and neutrons surrounded by electrons. The number of protons determines the element, while neutrons and electrons can vary between atoms of the same element. Most atoms are electrically neutral, but can become ions by gaining or losing electrons.
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Atoms intro (2)
Atoms are extremely small, around three one-hundred-millionths of a centimeter. Atoms are made up of a nucleus containing protons and neutrons, and electrons that orbit the nucleus. The nucleus contains positively charged protons and neutral neutrons, while negatively charged electrons surround it. Elements are defined by the number of protons, which determines the element's identity, while isotopes of an element can vary in their number of neutrons. Ions are formed when atoms gain or lose electrons.
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Electrical charges are caused by positive and negative charges from protons and electrons. All objects begin neutral but can become positively or negatively charged by gaining or losing electrons. There are two forces between charged objects - attraction between opposite charges and repulsion between like charges. Charges can be induced through friction, conduction, or induction without direct contact. The triboelectric series ranks materials based on their ability to gain or lose electrons through friction charging.
Notes lab 04b the atom structure
Elements are made of atoms, which are the basic building blocks of matter. Atoms consist of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons surround the nucleus in electron clouds. Protons are positively charged, electrons are negatively charged, and neutrons have no charge. The number of protons determines the element and its atomic number. The total number of protons and neutrons determines the atom's mass number. Elements are organized on the periodic table based on their atomic structure.
subatomic particles
Protons, neutrons, and electrons are the three main subatomic particles. Protons have a positive charge, neutrons have no charge, and electrons have a negative charge. Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. The atomic number identifies the number of protons in an atom's nucleus, while atomic mass refers to the total number of protons and neutrons.
Slide1
,chemsitry ,igcse ,0620 ,lesson ,atoms ,subatomic particles ,protons ,neutrons ,electrons ,atomic mass ,atomic number ,neutral ,charge ,postitive ,negatie
IGCSE 0620 Lesson 1 Slide 1
,chemsitry ,igcse ,0620 ,lesson ,atoms ,subatomic particles ,protons ,neutrons ,electrons ,atomic mass ,atomic number ,neutral ,charge ,postitive ,negatie
Subatomic Particles and Isotopes
This document discusses subatomic particles, isotopes, and ions. It defines atoms as the smallest unit of matter that retains chemical properties. Atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit the nucleus. The number of protons determines the element, while the number of neutrons defines the isotope. Ions are formed when atoms gain or lose electrons, becoming positively or negatively charged. Practice problems are provided to calculate subatomic particle numbers for elements, isotopes, and ions.
Atoms
Matter is composed of basic building blocks called atoms. Atoms were originally thought to be indivisible spheres, but are now understood to have internal structure. Atoms contain a tiny, dense nucleus of protons and neutrons surrounded by electrons. The number of protons determines the element, while neutrons and electrons can vary between atoms of the same element. Most atoms are electrically neutral, but can become ions by gaining or losing electrons.
atoms
This document provides an overview of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons. Protons have a positive charge, electrons have a negative charge, and neutrons have no charge. The number of protons determines the element, and the number of neutrons contributes to the mass number. The document also discusses the periodic table and how it can be used to find information about elements such as the number of protons, neutrons, and electrons. It includes some example calculations and provides additional online resources for learning more about atomic structure.
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2) Atomic mass is the total number of protons and neutrons, while the atomic number indicates just the number of protons. Neutrons can be calculated by subtracting the atomic number from atomic mass.
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Atomic structure part 1 fundamental particles
Atoms are composed of protons, neutrons, and electrons. Protons and neutrons have mass while electrons have negligible mass. The number of protons is the atomic number and the total number of protons and neutrons is the mass number. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different mass numbers but the same atomic number and chemical properties. Examples provided are the isotopes of carbon, chlorine, and their atomic and mass numbers.
Mod+13,+Atomic+Structure+Part+B
Each element is unique due to its atomic structure. Atoms consist of protons and neutrons located in the nucleus, and electrons outside the nucleus. The number of protons determines the element, while the total of protons and neutrons is the mass number. Isotopes are atoms of the same element with different numbers of neutrons.
Atom notesshort
The document discusses the structure of atoms. It explains that atoms are made up of a nucleus containing protons and neutrons, surrounded by electrons. The number of protons determines the element's identity and the number of neutrons is used to calculate atomic mass. Electrons occupy different energy levels surrounding the nucleus. Valence electrons, in the outermost shell, determine an element's chemical properties and reactivity.
Atomicsstructure
- Atoms are the building blocks of matter and are made up of protons, neutrons, and electrons. The nucleus contains protons and neutrons and accounts for nearly all an atom's mass, while electrons orbit the nucleus.
- The number of protons determines the element and cannot be changed. Neutrons can vary between atoms of the same element, creating isotopes of that element.
- An atom's mass number is the total number of protons and neutrons, while its atomic mass refers to the average mass of all isotopes of that element as found in nature.
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The document provides information about the structure of atoms including:
1) Atoms have a nucleus containing protons and neutrons at the center, surrounded by an electron cloud containing electrons.
2) There are three main subatomic particles - protons with a positive charge, neutrons with no charge, and electrons with a negative charge.
3) Atoms can have different numbers of neutrons forming isotopes of the same element.
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An atom consists of a dense nucleus containing protons and neutrons surrounded by a cloud of electrons. The nucleus contains protons which have a positive charge and neutrons which have a neutral charge. Electrons orbit the nucleus and have a negative charge. The atomic number represents the number of protons in an atom's nucleus, while the mass number is the total number of protons and neutrons.
Lesson 2
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G Tthe Atom
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This 4 step process for writing Lewis dot structures involves: 1) arranging atoms with the central atom having lower electronegativity, 2) adding up valence electrons and accounting for any charges, 3) drawing single bonds between atoms and removing 2 electrons for each, and 4) distributing any remaining electrons in pairs to satisfy the octet rule and complete the structure.
Ch 9-section-1
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Atom notes
- Atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit in energy levels around the nucleus.
- The number of protons determines the element and is equal to its atomic number. The total number of protons and neutrons determines the atomic mass of an element.
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The document contains information from a chemistry class, including:
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- A snowman challenge activity had students work in groups to balance sample chemical equations.
- An exit slip posed sample chemistry problems related to balancing equations and stoichiometry.
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This document summarizes atomic structure and particles. It discusses protons, neutrons, and electrons, and how they make up the nucleus and electron cloud of an atom. Protons determine the element, while neutrons and atomic mass take both protons and neutrons into account. The nucleus is held together by the strong nuclear force between nucleons, while electrons orbit outside the nucleus and usually equal the number of protons. Isotopes of an element have different numbers of neutrons.
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Protons have a positive charge and are found in the nucleus. Neutrons have no charge and are also found in the nucleus. Electrons have a negative charge and are found outside the nucleus.
The number of protons determines the element. The number of neutrons can vary between isotopes of the same element. Isotopes are identified using hyphen or nuclear notation. To find the number of neutrons in an isotope, subtract the atomic number from the atomic mass.
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This document provides a review of key concepts in atomic structure:
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2) Atomic mass is the total number of protons and neutrons, while the atomic number indicates just the number of protons. Neutrons can be calculated by subtracting the atomic number from atomic mass.
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Atoms are composed of protons, neutrons, and electrons. Protons and neutrons have mass while electrons have negligible mass. The number of protons is the atomic number and the total number of protons and neutrons is the mass number. Isotopes are atoms of the same element that have different numbers of neutrons, giving them different mass numbers but the same atomic number and chemical properties. Examples provided are the isotopes of carbon, chlorine, and their atomic and mass numbers.
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Each element is unique due to its atomic structure. Atoms consist of protons and neutrons located in the nucleus, and electrons outside the nucleus. The number of protons determines the element, while the total of protons and neutrons is the mass number. Isotopes are atoms of the same element with different numbers of neutrons.
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The document discusses the structure of atoms. It explains that atoms are made up of a nucleus containing protons and neutrons, surrounded by electrons. The number of protons determines the element's identity and the number of neutrons is used to calculate atomic mass. Electrons occupy different energy levels surrounding the nucleus. Valence electrons, in the outermost shell, determine an element's chemical properties and reactivity.
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- The number of protons determines the element and cannot be changed. Neutrons can vary between atoms of the same element, creating isotopes of that element.
- An atom's mass number is the total number of protons and neutrons, while its atomic mass refers to the average mass of all isotopes of that element as found in nature.
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The document provides information about the structure of atoms including:
1) Atoms have a nucleus containing protons and neutrons at the center, surrounded by an electron cloud containing electrons.
2) There are three main subatomic particles - protons with a positive charge, neutrons with no charge, and electrons with a negative charge.
3) Atoms can have different numbers of neutrons forming isotopes of the same element.
Parts on an atom
An atom consists of a dense nucleus containing protons and neutrons surrounded by a cloud of electrons. The nucleus contains protons which have a positive charge and neutrons which have a neutral charge. Electrons orbit the nucleus and have a negative charge. The atomic number represents the number of protons in an atom's nucleus, while the mass number is the total number of protons and neutrons.
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The document discusses atomic number, mass number, and isotopes. It defines atomic number as the number of protons in an atom's nucleus, which determines an element's chemical properties. Mass number is the sum of protons and neutrons. Isotopes are atoms with the same number of protons but different neutrons. Isotopes are identified by their mass number written as chemical symbol followed by mass number. The document also discusses molecular formula, empirical formula, and structural formula as examples of chemical formulas that show the number and arrangement of atoms in a compound. It defines molecular, empirical, and structural formulas and provides an example of a structural formula. Finally, it describes ball-and-stick and space-filling molecular models used to
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G Tthe Atom
Matter is made up of tiny particles called atoms. Atoms are too small to see, so scientists use models to explain their structure. Early models proposed atoms as indivisible spheres, while modern models show atoms with a tiny nucleus surrounded by electrons. The nucleus contains protons and neutrons, while electrons orbit around the outside. Atoms can form ions by gaining or losing electrons, changing their electrical charge but not their identity. Atoms of the same element can also vary in neutron number, forming isotopes of that element.
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The document discusses atomic structure and ions. It defines isotopes as atoms of the same element with different numbers of neutrons. The outermost electrons of an atom are involved in chemical reactions. The periodic table arranges elements by their number of outermost electrons. Noble gases have full outermost shells with 2 or 8 electrons. Atoms form ions by gaining or losing electrons to achieve stable configurations. Positively charged ions are formed when electrons are lost, and negatively charged ions are formed when electrons are gained.
Lewis Dot Structures
This 4 step process for writing Lewis dot structures involves: 1) arranging atoms with the central atom having lower electronegativity, 2) adding up valence electrons and accounting for any charges, 3) drawing single bonds between atoms and removing 2 electrons for each, and 4) distributing any remaining electrons in pairs to satisfy the octet rule and complete the structure.
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This document discusses different types of chemical bonds including ionic bonds, covalent bonds, and the factors that determine bond strength. It defines ionic bonds as electrostatic attractions between oppositely charged ions, and covalent bonds as the sharing of valence electrons between nonmetals. Bond length and bond energy are inversely related, with shorter, stronger bonds forming from increased orbital overlap and multiple bonds. Lewis structures are used to represent electron arrangements in molecules using dots or lines to indicate bonding and non-bonding electron pairs.
Atom notes
- Atoms are made up of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus, while electrons orbit in energy levels around the nucleus.
- The number of protons determines the element and is equal to its atomic number. The total number of protons and neutrons determines the atomic mass of an element.
- Electrons occupy different energy levels based on their distance from the nucleus, with the first level holding up to 2 electrons and subsequent levels holding more. Valence electrons in the outermost level determine an element's reactivity.
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The document contains information from a chemistry class, including:
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- An upcoming unit exam on Thursday will cover balancing equations, the mole concept, and conversions between grams, moles, atoms, and grams.
- A snowman challenge activity had students work in groups to balance sample chemical equations.
- An exit slip posed sample chemistry problems related to balancing equations and stoichiometry.
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The document provides a lesson plan and materials for a chemistry class reviewing solutions, acids, and bases. It includes:
1) A jeopardy game for students to review concepts with questions about solutions, acids, bases, and dissolving processes.
2) Announcements that the unit 6 exam will be the next day without notes and that the goal is to review.
3) Sample jeopardy questions about solutions, concentrations, acids, bases, and chemical reactions.
4) Properties of acids and the definition of a Bronsted-Lowry base.
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The document outlines a jigsaw activity where students are split into three groups to become experts on one of three types of chemical bonds - ionic, covalent, or metallic. The groups then present their findings to each other. Examples of each bond type are provided, including that ions are exchanged in ionic bonds between metals and nonmetals, electrons are shared in covalent bonds between nonmetals, and electrons are shared freely in metallic bonds between metals.
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This document discusses three types of nuclear reactions: radioactive decay, fission, and fusion. Radioactive decay occurs when an unstable isotope emits particles and becomes more stable. Fission involves a heavy nucleus splitting into lighter nuclei. Fusion is when two nuclei merge to form a heavier nucleus. Nuclear reactions are over 1 million times more powerful than chemical reactions because a small amount of mass can be converted to a large amount of energy according to Einstein's equation E=mc2.
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The document outlines a chemistry class schedule for the week, focusing on topics related to the periodic table including atomic radius, electronegativity, atomic structure, and a midterm exam on Friday. It provides examples of classifying elements as metals, nonmetals, semimetals and assigning them to groups based on their properties. Students are instructed to ask questions if they don't understand and complete homework on classifying elements and properties.
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The document provides guidance and questions for students on a chemistry quiz and homework assignment covering topics like the differences between mass and charge, identifying subatomic particles, and drawing an atom model. Key points covered include that mass is a measure of how much "stuff" an object has while charge can be positive, negative, or neutral; identifying protons, neutrons, and electrons; and that neutrons are subatomic particles with no charge while the nucleus is the center region of an atom. Students are asked to complete practice questions drawing an atom and labeling its parts.
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12 16 Mole Review Part Ii
I apologize, upon reviewing the document again I do not see enough context to summarize it in 3 sentences or less. The document provides some details about an upcoming exam and homework assignments but does not have an overall topic or theme that can be succinctly summarized. Please provide more context if you would like me to attempt a summary.
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The document contains notes from a chemistry class that include:
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2. An example reaction of N2 + H2 → NH3 is used to demonstrate the balancing process. After changing the coefficient of H2 to 3, the equation is balanced with N2 + 3H2 → NH3.
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10/14 Review: How is the periodic table organized?
10/26 What are the 3 types of chemical bonds? - Part II
10/26 What are the 3 types of chemical bonds? - Part II
10/5 What are the three types of radioactive decay?
10/5 What are the three types of radioactive decay?
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ATOM..ACT 1&2.pptx
1) Atoms contain positively charged protons and negatively charged electrons. Neutral atoms contain equal numbers of protons and electrons.
2) The proton and neutron have almost equal mass, with the proton being slightly heavier. It would take around 1836 electrons on one side of a seesaw to balance a single proton on the other side due to their relative masses.
3) Most of an atom's mass comes from its protons and neutrons in the nucleus. Protons and neutrons are similar in mass and collectively account for nearly all the atom's mass.
Notes lab 04 the atom structure
Each element is made of atoms with a unique atomic number, which are the basic building blocks of matter. Atoms consist of three subatomic particles - protons and neutrons found in the nucleus, and electrons located outside the nucleus. Protons are positively charged, neutrons have no charge, and electrons are negatively charged. The number of electrons in an element's outer shell allows for atomic bonding and determines the element's properties. Atoms of the same element can have different numbers of neutrons, called isotopes. Atoms can also become ions by gaining or losing electrons, acquiring a negative or positive charge respectively.
Presentation for Radioactivity
Atoms are made up of protons, neutrons, and electrons, with the number of protons defining the element. Different isotopes of an element have the same number of protons but different numbers of neutrons. Radioactive decay occurs spontaneously as nuclei emit alpha, beta, or gamma radiation to become more stable, conserving nuclear particles but decreasing mass.
atom.pptx
This document discusses the development of the atomic theory and model. It describes the key contributions of scientists like J.J. Thompson, Ernest Rutherford, Niels Bohr, Henry Moseley, and others. Thompson discovered the electron through cathode ray experiments. Rutherford concluded atoms have a small, dense nucleus through his gold foil experiment. Bohr proposed electrons orbit the nucleus in fixed energy levels. Moseley used X-ray spectroscopy to prove the atomic number is equal to the number of protons, allowing reorganization of the periodic table by atomic number. The modern nuclear model states the nucleus contains protons and neutrons and contains nearly all the atom's mass, with electrons orbiting around it.
ประจุไฟฟ้า Electric charges
This document discusses electric charge and where it comes from. It explains that there are two types of electric charge - positive and negative. Charge comes from protons, which have a positive charge, and electrons, which have a negative charge. For an atom to be neutral, it must have the same number of protons and electrons. The document also discusses electric forces between charged objects and how unlike charges attract and like charges repel. It provides an example of calculating the net charge of a system based on the number of protons or electrons.
GENCHEM1-atomic structure.pptx
This document defines atoms and their structure. Atoms are the building blocks of matter and composed of smaller subatomic particles, including protons, neutrons, and electrons. The nucleus is at the center of the atom and contains protons and neutrons. Electrons orbit the nucleus in one or more energy levels called the electron cloud. The number of protons determines the element, while the number of neutrons varies between isotopes of the same element.
Chapt-2-PPT-1-.pptx
This document provides an overview of atomic structure and bonding. It defines key terms like elements, atoms, subatomic particles, isotopes, ions and molecules. Atoms are made up of protons, neutrons and electrons. The number of protons defines the element and isotopes can have different numbers of neutrons. Electrons determine whether an atom is neutral or an ion. Atoms combine to form compounds and the smallest units of compounds are molecules. The mole is used to quantify very large numbers of small particles like atoms and molecules, with one mole equal to Avogadro's number of 6.022x1023 particles.
Atomic Theory
The document discusses atomic theory and the structure of atoms. It explains that all matter is made up of atoms, which are the smallest particles of elements that can exist. Atoms consist of a nucleus containing protons and neutrons, surrounded by electrons. The number of protons determines the element, while the number of neutrons can vary between isotopes of the same element. Chemical bonds form when atoms share or transfer electrons to fill their valence shells. This allows the formation of compounds with properties different from their constituent elements.
Inside the Atom~Notes
The document discusses the structure and composition of atoms. It can be summarized as follows:
1) Atoms have a small, dense nucleus containing protons and neutrons, surrounded by an electron cloud where electrons are found.
2) The number of protons determines the element, and protons plus neutrons equals the mass number. Electrons equal protons for neutral atoms.
3) Atoms can gain or lose electrons to become ions with a positive or negative charge.
4) Isotopes of the same element have different numbers of neutrons but the same number of protons.
Lesson: Friday 9/4
The document provides information about the structure of atoms including:
1) Atoms have two main parts - a nucleus at the center containing protons and neutrons, and electron rings on the outside containing electrons.
2) The nucleus is made up of protons, which have a positive charge, and neutrons, which have no charge.
3) Electrons are negatively charged and located outside the nucleus in electron clouds or rings around it.
Atomic theory
This document discusses atomic theory and subatomic particles. It defines atoms as building blocks of elements made up of protons, neutrons and electrons. The key subatomic particles are electrons, protons and neutrons, which have specific masses and charges. Atoms are identified by their atomic number and mass number. Isotopes are atoms of the same element with different numbers of neutrons. The document also discusses radioactive decay and the three main types of radiation emitted: alpha, beta and gamma radiation. It describes their properties including mass, charge, penetrating power and ability to ionize. Decay laws regarding changes in nucleon number and proton number during alpha, beta and gamma decay are also summarized.
Atomictheory 120313010052-phpapp01
This document discusses atomic theory and subatomic particles. It defines atoms as the building blocks of elements, and notes that similar atoms in each element differ from atoms in other elements. It then describes the three main subatomic particles (protons, neutrons, electrons), their properties like mass and charge, and how they are arranged in the nucleus and surrounding area. The document also discusses atomic number, atomic symbols, isotopes, and provides examples of subatomic particle arrangement in different atoms.
Atomictheory 120313010052-phpapp01
This document discusses atomic theory and subatomic particles. It defines atoms as the building blocks of elements, and notes that similar atoms in each element differ from atoms of other elements. It then describes the three main subatomic particles (protons, neutrons, electrons), their relative masses and charges. The document also discusses the location of these particles within atoms, how atomic number relates to the number of protons, atomic symbols, and how the number of electrons equals the number of protons in a neutral atom. It provides examples of subatomic particle makeup in some atoms and defines isotopes.
Matter And Atoms
Matter is anything that takes up space and is composed of atoms. Atoms are made up of protons, neutrons, and electrons. Matter exists in five states: solid, liquid, gas, plasma, or Bose-Einstein condensate. Atoms are the basic building blocks of all things in the universe.
The Nuclear Atom
The discovery of the electron. Thomson measured the charge-to-mass ratio of the particles within cathode rays and it was -1.76 x 10^8 coulombs per gram. The mass of an electron
9.10 x 10^(-28) g.
The dense nucleus contains over 99.9% of the mass of the atom, but it occupies very little of its volume.
Animatter Explained
An anti-you would look exactly the same as you, but be composed of antimatter instead of matter. All the atoms that make up your body - in your skin, organs, blood, etc. - would have antimatter counterparts, like anti-carbon, anti-oxygen, etc. Your anti-you would have all the same physical characteristics as you, like appearance, size, etc., but if you touched, violent annihilation would occur as your matter and their antimatter atoms collided and were destroyed in flashes of energy. From a distance, an anti-you could be your perfect mirror image twin, but made of the "opposite stuff" from the Universe.
Ch 5 Notes
This document provides an overview of elements, atoms, ions, isotopes, and the periodic table. It defines elements as pure substances that cannot be broken down further. Atoms are the smallest particles that retain an element's chemical properties and consist of protons, neutrons, and electrons. Ions are atoms or groups of atoms with a positive or negative charge formed by gaining or losing electrons. Isotopes are atoms of the same element with different numbers of neutrons. The periodic table organizes the elements and provides their properties based on their atomic structure.
Subatomic particles.pptx
This document provides information about subatomic particles and atomic structure. It defines the three main subatomic particles - protons, neutrons, and electrons. It discusses early atomic models proposed by scientists like J.J. Thomson and Ernest Rutherford. Rutherford's gold foil experiment provided evidence that the mass of an atom is concentrated in a small, dense nucleus. The document also defines key terms like isotope, ion, and mass number. It provides an activity to introduce the concept of electric charge and notes that atoms contain positively and negatively charged subatomic particles.
Programed instructional material: Electricity
This is an initial attempt by my students of B.Ed. in creating Programmed Instructional material using the template I had provided them. Your observations and suggestions are welcome!
Atom
To determine the subatomic particles of an atom, one must:
1. Gather the atomic number and mass, with the number representing protons and electrons and mass representing total protons and neutrons.
2. Identify protons as equal to the atomic number.
3. Identify electrons as equal to protons to maintain neutral charge.
4. Calculate neutrons by subtracting the atomic number from the rounded atomic mass.
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Lesson: Wednesday 9/2
- 2. What is the atom made of? Mr. Heffner Chemistry 9/1/09