This document contains science sheets for primary 4 students covering topics on measuring tools, states of matter, elements, physical and chemical changes, the solar system, rotation of the Earth and sun, phases of the moon, and tides. It includes lessons, activities, problems and explanations of key concepts. Measurements of length, mass and volume are defined using standard units like meters, grams and liters. The three states of matter and changes between them are also described.
(1) The document provides explanations for various scientific phenomena. It explains that different substances have different densities, which leads to differences in volume and mass. It also explains why some objects float and others sink based on their density relative to water.
(2) The document then defines various scientific terms related to physics and chemistry, including density, melting point, molecules, energy levels, and more.
(3) It provides examples of calculating density using mass and volume measurements. It also lists the electronic configurations of neon, magnesium, calcium and fluorine.
This document provides an overview of different types of materials including gases, condensed matter, metals, polymers, ceramics, composites, and electronics. It discusses the importance of materials science and engineering in areas like the economy, design, and new applications. The main classes of materials covered are metallic, polymeric, and ceramic materials. Composites combine two or more materials while maintaining a distinct boundary between them. Recent advances discussed include smart materials that react to stimuli and nanomaterials that have particle sizes smaller than 100 nm.
Chapter 1: Material Structure and Binary Alloy Systemsyar 2604
This is an introduction to material structure and periodic table system. This topic also describes microstructure of the metals and alloys solidification.
Chapter 2 section 3 notes 2011 (properties of matter)Mr. Motuk
Physical properties can be observed without changing a substance's composition, such as its boiling point, color, or density. A chemical change alters a substance's composition, forming new substances with different properties, like wood burning to ash. Matter exists in four states - solid, liquid, gas, and plasma - with the amount of energy determining the state. As energy increases, the density of matter decreases, changing from a solid to liquid to gas and finally to plasma.
The document contains a chemistry unit on the solid state with questions ranging from one to three marks. It includes questions about crystal lattices, crystal defects, stoichiometric and non-stoichiometric defects, crystal structures, and properties of solids such as ionic bonding and conductivity. Numerical problems calculate properties like density from information about the unit cell structure and composition.
The document discusses key concepts in material technology including:
1. It defines the basic structure of atoms and different types of materials including elements, mixtures, and compounds.
2. It describes atomic structure including atomic number, atomic mass, and atomic orbits. The periodic table is introduced as a way to classify and understand elements and their properties.
3. Different types of crystal structures are defined including body centered cubic, face centered cubic, and hexagonal close packed. Bonding types such as covalent, metallic, and ionic are also introduced.
4. Terminology used in phase diagrams is defined including phases, equilibrium, composition, liquidus, and solidus. Binary alloy systems containing two components are also
The document provides information on solidification processes and binary alloy systems. It discusses:
1) The three main steps in the solidification process: formation of stable nuclei, growth of nuclei into crystals, and formation of a grain structure.
2) The different types of solid solutions including substitutional and interstitial solid solutions. Substitutional solutions involve solute atoms replacing solvent atoms, while interstitial solutions involve solute atoms filling spaces between solvent atoms.
3) Phase diagrams and how they represent the relationship between temperature, composition, and phases in equilibrium for a binary alloy system. Key points include liquidus lines, triple points, and using phase diagrams to interpret cooling curves.
4) An
The document summarizes Week 2 of an MME 323 materials science course focusing on atomic structure and interatomic bonding. It outlines the lecture topics which include atomic number, mass, and configuration, quantum numbers, the periodic table, and primary bonding types like ionic, covalent, and metallic. The learning objectives are to define key atomic concepts and describe different bonding mechanisms. Ionic bonding occurs between metals and non-metals and involves electron transfer. Covalent bonding is between non-metals and the sharing of electrons. Metallic bonding is within metals and due to positively charged metal ions in a "sea" of delocalized electrons.
(1) The document provides explanations for various scientific phenomena. It explains that different substances have different densities, which leads to differences in volume and mass. It also explains why some objects float and others sink based on their density relative to water.
(2) The document then defines various scientific terms related to physics and chemistry, including density, melting point, molecules, energy levels, and more.
(3) It provides examples of calculating density using mass and volume measurements. It also lists the electronic configurations of neon, magnesium, calcium and fluorine.
This document provides an overview of different types of materials including gases, condensed matter, metals, polymers, ceramics, composites, and electronics. It discusses the importance of materials science and engineering in areas like the economy, design, and new applications. The main classes of materials covered are metallic, polymeric, and ceramic materials. Composites combine two or more materials while maintaining a distinct boundary between them. Recent advances discussed include smart materials that react to stimuli and nanomaterials that have particle sizes smaller than 100 nm.
Chapter 1: Material Structure and Binary Alloy Systemsyar 2604
This is an introduction to material structure and periodic table system. This topic also describes microstructure of the metals and alloys solidification.
Chapter 2 section 3 notes 2011 (properties of matter)Mr. Motuk
Physical properties can be observed without changing a substance's composition, such as its boiling point, color, or density. A chemical change alters a substance's composition, forming new substances with different properties, like wood burning to ash. Matter exists in four states - solid, liquid, gas, and plasma - with the amount of energy determining the state. As energy increases, the density of matter decreases, changing from a solid to liquid to gas and finally to plasma.
The document contains a chemistry unit on the solid state with questions ranging from one to three marks. It includes questions about crystal lattices, crystal defects, stoichiometric and non-stoichiometric defects, crystal structures, and properties of solids such as ionic bonding and conductivity. Numerical problems calculate properties like density from information about the unit cell structure and composition.
The document discusses key concepts in material technology including:
1. It defines the basic structure of atoms and different types of materials including elements, mixtures, and compounds.
2. It describes atomic structure including atomic number, atomic mass, and atomic orbits. The periodic table is introduced as a way to classify and understand elements and their properties.
3. Different types of crystal structures are defined including body centered cubic, face centered cubic, and hexagonal close packed. Bonding types such as covalent, metallic, and ionic are also introduced.
4. Terminology used in phase diagrams is defined including phases, equilibrium, composition, liquidus, and solidus. Binary alloy systems containing two components are also
The document provides information on solidification processes and binary alloy systems. It discusses:
1) The three main steps in the solidification process: formation of stable nuclei, growth of nuclei into crystals, and formation of a grain structure.
2) The different types of solid solutions including substitutional and interstitial solid solutions. Substitutional solutions involve solute atoms replacing solvent atoms, while interstitial solutions involve solute atoms filling spaces between solvent atoms.
3) Phase diagrams and how they represent the relationship between temperature, composition, and phases in equilibrium for a binary alloy system. Key points include liquidus lines, triple points, and using phase diagrams to interpret cooling curves.
4) An
The document summarizes Week 2 of an MME 323 materials science course focusing on atomic structure and interatomic bonding. It outlines the lecture topics which include atomic number, mass, and configuration, quantum numbers, the periodic table, and primary bonding types like ionic, covalent, and metallic. The learning objectives are to define key atomic concepts and describe different bonding mechanisms. Ionic bonding occurs between metals and non-metals and involves electron transfer. Covalent bonding is between non-metals and the sharing of electrons. Metallic bonding is within metals and due to positively charged metal ions in a "sea" of delocalized electrons.
1) The document describes the structure of materials at different length scales from atomic to macroscopic levels. It discusses how atomic structure influences properties and technological applications of materials.
2) Key concepts covered include the structure of the atom, electronic configuration, periodic table, different types of atomic bonding, and how bonding influences properties like conductivity and strength.
3) Examples calculate the number of atoms in materials and compare properties like electronegativity between elements. Diagrams illustrate different types of bonding and how structure determines properties.
Chapter 1 material structure and binary alloy systemsakura rena
This document discusses the structure of materials and binary alloy systems. It begins by defining key terms like atom, element, mixture, compound, atomic number, atomic mass, and atomic orbits. It then explains the periodic table, including its characteristics, groups, periods, and function. The document also covers crystal structures, bonding types, solidification of metals and alloys, solid solutions, and equilibrium phase diagrams.
Solids are characterized by their definite shape and also their considerable mechanical strength and rigidity. The particles that compose a solid material(with few exceptions), whether ionic, molecular, covalent or metallic, are held in place by strong attractive forces between them.
This document discusses diffusion in solids. It defines diffusion as the tendency of molecules, atoms, or ions to distribute evenly in space due to random kinetic motion. Diffusion occurs due to concentration gradients and stops when concentrations equalize. In solids, diffusion results from thermally-activated random atomic motion. There are two mechanisms - interstitial, where small atoms fit between others, and vacancy, where atoms jump into vacant sites. Examples given are carbon diffusion in steel via the interstitial mechanism, salt dissolving in water as a solid-liquid diffusion example, and dust particles suspended in air as a solid-gas diffusion example.
The document summarizes key concepts about materials including:
1) At the atomic level, materials are composed of elements with distinct atomic structures, which bond together in crystalline or noncrystalline forms. Common bonding types include ionic, covalent, and metallic.
2) Crystalline materials have long-range ordered atomic structures with repeating unit cells, while noncrystalline materials lack long-range order.
3) Metals typically have body-centered cubic, face-centered cubic, or hexagonal crystalline structures and metallic bonding, making them strong yet ductile. Ceramics and polymers have other bonding types and properties.
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1) The document discusses atomic structure and bonding, covering the history of atomic theory from Dalton to Chadwick. It describes the structure of atoms including protons, neutrons and electrons.
2) Atomic number and mass are defined, and electron configuration is explained using quantum numbers. Different types of chemical bonds are covered - ionic formed by electron transfer, covalent by electron sharing, and metallic by delocalized electrons.
3) Secondary bonds such as hydrogen and van der Waals bonds are also summarized. The periodic table is shown organizing elements by electron configuration. Different classes of elements - metals, nonmetals and metalloids - are defined by their bonding properties.
SOLID STATE -XII BY SULEKHA RANI R , PGT CHEMISTRYSulekha Nisanth
Here are the definitions and differences you asked for:
Short range order - Atoms are arranged in a disordered manner within a small region but this arrangement does not extend over long distances.
Anisotropic - A material whose physical properties vary with the direction of measurement.
Unit cell - The smallest repeating unit that constructs the entire crystal by translation.
Voids - Empty spaces between closely packed spheres in crystal structures. There are two types - octahedral and tetrahedral voids.
Impurity defect - Occurs when an atom of one element replaces an atom of the host element in its normal lattice position.
Monoclinic - Unit cell with two axes at 90 degrees and one axis not at 90 degrees
This document summarizes different types of solids. Crystalline solids have long-range order between particles which gives them distinct properties like sharp melting points and anisotropy. Amorphous solids only have short-range order, making them similar to supercooled liquids with no distinct melting point. Crystalline solids can be classified as molecular, ionic, metallic or covalent based on the interactions between particles. Each type of solid has distinct physical properties depending on these interactions.
This document provides revision notes on chemical bonding for a science class. It explains that atoms form ionic bonds through the transfer of electrons from metals to non-metals, creating cations and anions, while covalent bonds form through the sharing of electrons between nonmetal atoms. It lists common cations and anions and provides examples of ionic and covalent compounds. There are also practice questions for students to test their understanding of chemical bonding concepts.
Solid-state chemistry, also sometimes referred as materials chemistry, is the study of the synthesis, structure, and properties of solid phase materials, particularly, but not necessarily exclusively of, non-molecular solids. It therefore has a strong overlap with solid-state physics, mineralogy, crystallography, ceramics, metallurgy, thermodynamics, materials science and electronics with a focus on the synthesis of novel materials and their characterisation. Solids can be classified as crystalline or amorphous on basis of the nature of order present in the arrangement of their constituent particles,
This document discusses different states of matter and properties of liquids and solids. It defines key terms like phases, intermolecular forces, and boiling point. It describes different types of solids like ionic, molecular, metallic and network solids. It also discusses properties of liquids like surface tension, capillary action, and viscosity.
I hope You all like it. I hope It is very beneficial for you all. I really thought that you all get enough knowledge from this presentation. This presentation is about materials and their classifications. After you read this presentation you knowledge is not as before.
CBSE Class 12 Chemistry Chapter 1 (The Solid State) | Homi InstituteHomi Institute
The document discusses various types of bonding and intermolecular forces found in solid state materials, including covalent bonding, metallic bonding, ionic bonding, hydrogen bonding, and van der Waals forces. It also describes different types of crystal defects such as point defects, line defects, stoichiometric defects, impurity defects, and non-stoichiometric defects. Finally, it covers topics like semiconductors, ferromagnetism, and the magnetic properties associated with orbiting and spinning electrons.
Ionic solids are composed of positively charged cations and negatively charged anions arranged in a 3D array. The electrostatic attractions between opposite charges hold the ions in fixed positions, making ionic solids hard and brittle. The melting point of ionic solids is generally over 150 degrees C because strong electrostatic forces must be overcome for melting to occur. The radius ratio rule can be used to predict the coordination number of ions based on the ratio of cation to anion radii, with different ratios corresponding to different coordination geometries like tetrahedral or octahedral. While useful, the radius ratio rule has limitations as it treats ions as hard spheres and does not account for variations in effective ionic radii.
this is based on jee, nee, aipmt, maharahstra board, icse and cbse board. if you want this ppt to download please donate me Rs200/- for my each hard dedicated ppt. put on my paytm acount- 8879919898.
you can also go to my site-
www.akchem.blogspot.com
contact - aktr000@gmail.com
The document discusses the characteristics of solids. It describes how solids have fixed positions and rigid structures, unlike liquids and gases which can flow freely. Solids are classified as either crystalline or amorphous based on the ordering of particles. Crystalline solids have long-range orderly patterns that repeat, while amorphous solids only have short-range order and irregular particle shapes. Properties like melting point and ability to flow differ between the two types of solids based on their particle arrangements.
A solid is a state of matter characterized by particles arranged in a stable, close-packed structure that gives solids a definite shape and volume. Solids can be crystalline or amorphous. Crystalline solids have particles arranged in a regular, repeating pattern throughout the crystal lattice. Amorphous solids lack long-range order and have particles arranged irregularly over short distances. The crystal lattice is made up of repeating units called unit cells, which define the symmetry and geometry of the crystal structure. Unit cells come in seven main types depending on their parameters. Crystalline solids are further classified based on the type of bonds between particles as ionic, covalent, metallic, or molecular solids.
The document summarizes the history and development of atomic theory through three major discoveries:
1) J.J. Thompson's "plum pudding" model of 1897 which proposed that electrons are distributed throughout the atom balancing out a positively charged medium.
2) Ernest Rutherford's gold foil experiment of 1909-1911 which showed that the mass of an atom is concentrated in a tiny, dense nucleus through alpha particle deflection.
3) The Rutherford model established atoms having a tiny, dense nucleus surrounded by orbiting electrons, accounting for most physical and chemical atomic properties.
The document discusses the states of matter and the kinetic molecular theory. It introduces the three common states of matter - solid, liquid, and gas - and explains their properties based on how the particles that make up matter move and interact. It describes how changes between states occur when particles gain or lose enough energy to change their motion. The kinetic molecular theory proposes that all matter is made of particles in constant motion, and explains a variety of physical phenomena based on the motion and interaction of these particles.
This document provides an introduction to chemistry, including:
1. Definitions of key terms like elements, compounds, physical and chemical properties and changes.
2. An overview of the major branches of chemistry like organic, inorganic, physical and analytical chemistry.
3. Descriptions of the periodic table, including groups like alkali metals and halogens, and periodic trends.
This document provides an introduction to chemistry. It defines chemistry as the study of matter and its properties. Matter is anything that has mass and takes up space. There are several branches of chemistry including organic, inorganic, physical, analytical, biochemistry, and theoretical chemistry. The document discusses the development of the periodic table by Mendeleev and its key elements like periods and groups. It also defines core concepts in chemistry including atoms, elements, compounds, physical and chemical properties and changes. Key topics covered are the three states of matter, phase changes, and the conservation of mass in chemical reactions.
1) The document describes the structure of materials at different length scales from atomic to macroscopic levels. It discusses how atomic structure influences properties and technological applications of materials.
2) Key concepts covered include the structure of the atom, electronic configuration, periodic table, different types of atomic bonding, and how bonding influences properties like conductivity and strength.
3) Examples calculate the number of atoms in materials and compare properties like electronegativity between elements. Diagrams illustrate different types of bonding and how structure determines properties.
Chapter 1 material structure and binary alloy systemsakura rena
This document discusses the structure of materials and binary alloy systems. It begins by defining key terms like atom, element, mixture, compound, atomic number, atomic mass, and atomic orbits. It then explains the periodic table, including its characteristics, groups, periods, and function. The document also covers crystal structures, bonding types, solidification of metals and alloys, solid solutions, and equilibrium phase diagrams.
Solids are characterized by their definite shape and also their considerable mechanical strength and rigidity. The particles that compose a solid material(with few exceptions), whether ionic, molecular, covalent or metallic, are held in place by strong attractive forces between them.
This document discusses diffusion in solids. It defines diffusion as the tendency of molecules, atoms, or ions to distribute evenly in space due to random kinetic motion. Diffusion occurs due to concentration gradients and stops when concentrations equalize. In solids, diffusion results from thermally-activated random atomic motion. There are two mechanisms - interstitial, where small atoms fit between others, and vacancy, where atoms jump into vacant sites. Examples given are carbon diffusion in steel via the interstitial mechanism, salt dissolving in water as a solid-liquid diffusion example, and dust particles suspended in air as a solid-gas diffusion example.
The document summarizes key concepts about materials including:
1) At the atomic level, materials are composed of elements with distinct atomic structures, which bond together in crystalline or noncrystalline forms. Common bonding types include ionic, covalent, and metallic.
2) Crystalline materials have long-range ordered atomic structures with repeating unit cells, while noncrystalline materials lack long-range order.
3) Metals typically have body-centered cubic, face-centered cubic, or hexagonal crystalline structures and metallic bonding, making them strong yet ductile. Ceramics and polymers have other bonding types and properties.
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Our Vision & Mission - Simplifying Students Life
Our Belief - “The great breakthrough in your life comes when you realize it, that you can learn anything you need to learn; to accomplish any goal that you have set for yourself. This means there are no limits on what you can be, have or do.”
Like Us - https://www.facebook.com/FellowBuddycom-446240585585480
1) The document discusses atomic structure and bonding, covering the history of atomic theory from Dalton to Chadwick. It describes the structure of atoms including protons, neutrons and electrons.
2) Atomic number and mass are defined, and electron configuration is explained using quantum numbers. Different types of chemical bonds are covered - ionic formed by electron transfer, covalent by electron sharing, and metallic by delocalized electrons.
3) Secondary bonds such as hydrogen and van der Waals bonds are also summarized. The periodic table is shown organizing elements by electron configuration. Different classes of elements - metals, nonmetals and metalloids - are defined by their bonding properties.
SOLID STATE -XII BY SULEKHA RANI R , PGT CHEMISTRYSulekha Nisanth
Here are the definitions and differences you asked for:
Short range order - Atoms are arranged in a disordered manner within a small region but this arrangement does not extend over long distances.
Anisotropic - A material whose physical properties vary with the direction of measurement.
Unit cell - The smallest repeating unit that constructs the entire crystal by translation.
Voids - Empty spaces between closely packed spheres in crystal structures. There are two types - octahedral and tetrahedral voids.
Impurity defect - Occurs when an atom of one element replaces an atom of the host element in its normal lattice position.
Monoclinic - Unit cell with two axes at 90 degrees and one axis not at 90 degrees
This document summarizes different types of solids. Crystalline solids have long-range order between particles which gives them distinct properties like sharp melting points and anisotropy. Amorphous solids only have short-range order, making them similar to supercooled liquids with no distinct melting point. Crystalline solids can be classified as molecular, ionic, metallic or covalent based on the interactions between particles. Each type of solid has distinct physical properties depending on these interactions.
This document provides revision notes on chemical bonding for a science class. It explains that atoms form ionic bonds through the transfer of electrons from metals to non-metals, creating cations and anions, while covalent bonds form through the sharing of electrons between nonmetal atoms. It lists common cations and anions and provides examples of ionic and covalent compounds. There are also practice questions for students to test their understanding of chemical bonding concepts.
Solid-state chemistry, also sometimes referred as materials chemistry, is the study of the synthesis, structure, and properties of solid phase materials, particularly, but not necessarily exclusively of, non-molecular solids. It therefore has a strong overlap with solid-state physics, mineralogy, crystallography, ceramics, metallurgy, thermodynamics, materials science and electronics with a focus on the synthesis of novel materials and their characterisation. Solids can be classified as crystalline or amorphous on basis of the nature of order present in the arrangement of their constituent particles,
This document discusses different states of matter and properties of liquids and solids. It defines key terms like phases, intermolecular forces, and boiling point. It describes different types of solids like ionic, molecular, metallic and network solids. It also discusses properties of liquids like surface tension, capillary action, and viscosity.
I hope You all like it. I hope It is very beneficial for you all. I really thought that you all get enough knowledge from this presentation. This presentation is about materials and their classifications. After you read this presentation you knowledge is not as before.
CBSE Class 12 Chemistry Chapter 1 (The Solid State) | Homi InstituteHomi Institute
The document discusses various types of bonding and intermolecular forces found in solid state materials, including covalent bonding, metallic bonding, ionic bonding, hydrogen bonding, and van der Waals forces. It also describes different types of crystal defects such as point defects, line defects, stoichiometric defects, impurity defects, and non-stoichiometric defects. Finally, it covers topics like semiconductors, ferromagnetism, and the magnetic properties associated with orbiting and spinning electrons.
Ionic solids are composed of positively charged cations and negatively charged anions arranged in a 3D array. The electrostatic attractions between opposite charges hold the ions in fixed positions, making ionic solids hard and brittle. The melting point of ionic solids is generally over 150 degrees C because strong electrostatic forces must be overcome for melting to occur. The radius ratio rule can be used to predict the coordination number of ions based on the ratio of cation to anion radii, with different ratios corresponding to different coordination geometries like tetrahedral or octahedral. While useful, the radius ratio rule has limitations as it treats ions as hard spheres and does not account for variations in effective ionic radii.
this is based on jee, nee, aipmt, maharahstra board, icse and cbse board. if you want this ppt to download please donate me Rs200/- for my each hard dedicated ppt. put on my paytm acount- 8879919898.
you can also go to my site-
www.akchem.blogspot.com
contact - aktr000@gmail.com
The document discusses the characteristics of solids. It describes how solids have fixed positions and rigid structures, unlike liquids and gases which can flow freely. Solids are classified as either crystalline or amorphous based on the ordering of particles. Crystalline solids have long-range orderly patterns that repeat, while amorphous solids only have short-range order and irregular particle shapes. Properties like melting point and ability to flow differ between the two types of solids based on their particle arrangements.
A solid is a state of matter characterized by particles arranged in a stable, close-packed structure that gives solids a definite shape and volume. Solids can be crystalline or amorphous. Crystalline solids have particles arranged in a regular, repeating pattern throughout the crystal lattice. Amorphous solids lack long-range order and have particles arranged irregularly over short distances. The crystal lattice is made up of repeating units called unit cells, which define the symmetry and geometry of the crystal structure. Unit cells come in seven main types depending on their parameters. Crystalline solids are further classified based on the type of bonds between particles as ionic, covalent, metallic, or molecular solids.
The document summarizes the history and development of atomic theory through three major discoveries:
1) J.J. Thompson's "plum pudding" model of 1897 which proposed that electrons are distributed throughout the atom balancing out a positively charged medium.
2) Ernest Rutherford's gold foil experiment of 1909-1911 which showed that the mass of an atom is concentrated in a tiny, dense nucleus through alpha particle deflection.
3) The Rutherford model established atoms having a tiny, dense nucleus surrounded by orbiting electrons, accounting for most physical and chemical atomic properties.
The document discusses the states of matter and the kinetic molecular theory. It introduces the three common states of matter - solid, liquid, and gas - and explains their properties based on how the particles that make up matter move and interact. It describes how changes between states occur when particles gain or lose enough energy to change their motion. The kinetic molecular theory proposes that all matter is made of particles in constant motion, and explains a variety of physical phenomena based on the motion and interaction of these particles.
This document provides an introduction to chemistry, including:
1. Definitions of key terms like elements, compounds, physical and chemical properties and changes.
2. An overview of the major branches of chemistry like organic, inorganic, physical and analytical chemistry.
3. Descriptions of the periodic table, including groups like alkali metals and halogens, and periodic trends.
This document provides an introduction to chemistry. It defines chemistry as the study of matter and its properties. Matter is anything that has mass and takes up space. There are several branches of chemistry including organic, inorganic, physical, analytical, biochemistry, and theoretical chemistry. The document discusses the development of the periodic table by Mendeleev and its key elements like periods and groups. It also defines core concepts in chemistry including atoms, elements, compounds, physical and chemical properties and changes. Key topics covered are the three states of matter, phase changes, and the conservation of mass in chemical reactions.
This document provides an overview of chemistry concepts including the definition of chemistry, major branches of chemistry, early theories of matter, and important figures in the development of modern chemistry such as Aristotle, Democritus, Boyle, Priestley, and Dalton. It also discusses the classification of matter as elements, compounds, and mixtures. Key chemistry concepts like physical and chemical properties, physical and chemical changes, energy, heat, and phase changes are introduced.
This document discusses matter and energy. It defines matter as anything that has mass and takes up space. It describes the general properties of matter, including mass and volume, as well as specific properties like color and hardness that are unique to different types of matter. It also discusses physical and chemical changes, where physical changes alter the size, shape or state of matter but do not create new substances, while chemical changes create new substances through chemical reactions. The document then covers different forms of energy including light, nuclear, chemical, thermal, electrical, and mechanical energy. It explains renewable energy sources like the sun, wind and flowing water, as well as non-renewable sources like fossil fuels and nuclear fuels.
This document discusses matter, materials, and recycling. It defines matter as everything around us, formed by atoms and molecules. It describes the three states of matter - solids have a fixed shape and volume, liquids take the shape of their container, and gases fill their container. Materials are made from matter and can be natural like wood, metal, and stone, or artificial like plastic and glass. The document outlines properties of materials like strength, flexibility, and weakness. It emphasizes the importance of recycling materials to preserve the environment and lists common recycling bins for different waste types.
The document provides information about the states of matter and changes between states. It discusses:
1) Matter is made of tiny particles that are in continuous motion and attract one another. The properties of solids, liquids, and gases depend on how tightly packed the particles are.
2) The three common states of matter are solids, liquids, and gases. Solids have a fixed shape and volume, liquids have a fixed volume but no shape, and gases have no fixed shape or volume. Changes between states, like melting, boiling, and sublimation occur when temperature or pressure changes the motion and spacing of particles.
3) Evaporation and boiling are examples of how interconversions between liquid and
This document discusses matter, materials, and recycling. It defines matter as anything formed from atoms and molecules, and describes the three states of matter - solid, liquid, and gas. Materials are defined as matter used to make objects, and are classified as natural or artificial. The properties of different materials like strength, flexibility, and weakness are also outlined. The document concludes by explaining the importance of recycling to preserve the environment and listing the different containers used to recycle materials like glass, paper, plastics, and organic wastes.
The document provides an overview of key concepts in chemistry including the structure of atoms, states of matter, properties of matter, and the periodic table. It defines atoms as the smallest particle of an element and notes they are composed of protons, neutrons, and electrons. The periodic table is introduced and elements are organized based on atomic number and recurring properties within periods and groups. Key terms like atomic number and mass number are defined. States of matter such as solids, liquids, and gases are contrasted based on properties like volume and shape. Physical and chemical properties and changes in matter are also distinguished.
This document provides an introduction to chemistry. It begins by defining chemistry as the study of matter and its properties. It then discusses the elements that make up the human body and where elements come from. There are several branches of chemistry including organic, inorganic, physical, analytical, biochemistry, and theoretical chemistry. It also defines key chemistry concepts like matter, elements, compounds, physical and chemical properties and changes. It introduces the three states of matter and phase changes. Finally, it provides an overview of the periodic table, including the development of the periodic table and periodic trends and characteristics of different groups of elements.
The document discusses various properties of matter and chemical changes. It provides information on:
1) Density being a ratio and not dependent on size. Ice having a lower density than water and therefore floating.
2) Buoyancy causing less dense substances to float in more dense liquids. Boats being made of lower density materials than water.
3) Viscosity being the resistance to flow, with cold syrup having a higher viscosity than warm syrup due to particle interactions.
The document provides a review of key concepts for an 8th grade physical science exam, including different types of measurements, scientific experimentation, phases and changes of matter, the structure and properties of atoms and elements, and the differences between physical and chemical changes and mixtures and pure substances. It defines length, volume, mass, weight, time, temperature, and density and their standard units. It also outlines the key characteristics of plasma, phases of matter, changes in state, and physical and chemical properties.
New chm-151-unit-1-20powerpoints-20sp13s-140227172225-phpapp01Cleophas Rwemera
This document outlines key concepts for a chemistry course, including:
- The goals of identifying elements, understanding measurement units, significant figures, and types of errors.
- Definitions of matter, properties, physical and chemical changes, and the three states of matter.
- The International System of Units (SI) including common units like meters, grams, kelvin, and moles.
- Concepts like energy, elements, and the periodic table, and examples of calculating density, conversions between units, and solving chemistry problems systematically.
This document provides an overview of chemistry, including its definition, major branches, early theories, and the rise of modern chemistry. It discusses key figures like Democritus, Aristotle, Boyle, Priestley, and Dalton and their contributions. It also defines matter, discusses chemical and physical properties, and distinguishes between physical and chemical changes. Finally, it covers topics like elements and their symbols, compounds and formulas, molecules, energy in matter including different forms of energy and laws of thermodynamics, and phase changes of matter.
This document discusses the classification and properties of matter. It describes how matter is made up of tiny particles that are in continuous motion. Matter exists in three states - solid, liquid and gas - which are distinguished by properties like shape, volume, particle movement and attraction. The document also explains how changing temperature or pressure can cause matter to convert between these different states through various phase changes like melting, boiling, sublimation and evaporation.
The document discusses the importance of teaching students how to learn effectively and efficiently. It states that students should be taught strategies for organizing information, retaining knowledge, and applying concepts rather than just memorizing facts. These skills will help students become independent, self-motivated learners who are able to continually acquire new information throughout their lives.
This document provides an introduction to chemistry and matter. It discusses that chemistry is the study of matter and its properties. There are several branches of chemistry including organic, inorganic, physical, analytical, biochemistry, and theoretical chemistry. Matter can exist in solid, liquid, or gas states depending on the closeness and movement of its particles. A substance's properties, whether physical or chemical, can help identify it. Changes to matter can be physical, chemical, or nuclear, altering its identity or structure on different levels, while conserving total mass and energy.
This document provides an introduction to chemistry and matter. It discusses that chemistry is the study of matter and its properties. There are several branches of chemistry including organic, inorganic, physical, analytical, biochemistry, and theoretical chemistry. Matter can exist in solid, liquid, or gas states depending on the packing and movement of its particles. A substance's properties, whether physical or chemical, can help identify it. Changes to matter can be physical, chemical, or nuclear, altering its identity or structure on different levels. The total amount of matter and energy is conserved in any chemical reaction or change.
This document provides an introduction to chemistry, including:
1. Definitions of key terms like matter, elements, compounds, properties and changes in matter.
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The document summarizes key concepts about the nature of matter including:
- Matter is anything that has mass and takes up space. Physical properties like color, size and state can be observed without changing the substance.
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1. AlKa rma L a n g u a g e Sc h o o l
Ac a d emi c y e a r : 2 0 1 4 / 2 0 1 5
Pr imar y 4
Sc ience Sheet s
Fi r s t Term
· St udent Name: _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _
· Clas s : _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _
2. 1- Measuring Tools
2- States of Matter
3- Elements around us
4- Physical and Chemical Changes
4-
2
Unit one
Unit two
1-Stars and Planets
2- Motion of Sun and Earth
3- Motion of Moon
4- Atmosphere and weather
4. Lesson : Measuring tools
There are many different things around us like:
Bag Ball Glass Stone Apple
All of these objects differ in:
Shape, size and mass, but all of these objects are known as matter.
4
1
Matter: Everything that has mass and volume:
Study
well
Mass: The amount of matter in an object.
Volume: The space occupied by the matter.
5. ·When you buy cloth, the seller asks about the length.
·When you buy vegetables, fruits or meat he asks about
the mass.
· When you buy milk or oil, he asks you about the volume.
1)-The centimeter (cm)
LLeennggtthh
5
Measuring ruler
Measuring tape
Centimeter
Metre
kilometer
Examples
Measuring tools Measuring units
1 meter= 100centimeter
6. Used for measuring small lengths
(Such as the length of your pen or your book)
2)-The meter (m)
For measuring big lengths
(Such as the dimensions of your classroom)
3 )-The kilometer (Km )
For measuring very big lengths (such as the distance between Cairo and
Alexandria)
1 Kilometer (Km) = 1000 meters (m)
6
Sensitive balance for gold & chemicals
Common balance for fruits & vegetables
Gram
Kilogram
Ton
1kilogram=1000 gram
1Ton=1000 kilogram
7. Measuring tools Measuring units
MMaassss
1) - The gram (gm) :
For measuring small masses such as jewelry and
chemical substances.
2) - The kilogram (Kg):
For measuring large masses such as fruits &
vegetables.
3 ) - The ton: For very big objects
Measuring tools Measuring units
VVoolluummee
7
Graduated cylinder
(Liquids – irregular shaped solids)
Graduate ruler
(solid regular shape)
Liquid volumes:
milliliter
liter
Solid volumes:
cubic centimeter cm3
cubic meter m3
1Liter =1000 milliter= 1000 cm3
8. 1-Calculating the volume of a regular solid
object:
By using the ruler to measure its dimension
then calculate its volume
Volume = Length x Width x Height =--- cm3
Width
Height
Length
Find the volume of a brick, knowing that its length = 7cm, its width= 5cm
and its height = 1cm
Volume = length x width x height
= 7 x 5 x 1 = 35 cm3
Estimating volumes of irregular shaped solid and insoluble in water
Use a graduated cylinder contains a quantity of water
a- Record the level of water in cylinder v1
b- Put a piece of stone then record the level =v2
The volume of stone =v2-v1
8
PPrroobblleemm
Solution
9. Explanation
When a piece of stone is put in a jar containing 30cm3 of water, the water
level rises to 50 cm3 what is the volume of the stone?
Volume of stone = V2 – V1 = 50 – 30 = 20 cm3
How to read the volume of liquids?
Look horizontally at the lowest (bottom) point of the water level
Activity: Masses of equals volumes to different materials:
Put iron cube on a common balance and put a wooden cube on the other
Observation: the balance shows that the iron is heavier than wood cube
Conclusion: Equal volumes of different materials have different mass
9
PPrroobblleemm
Solution
Note
:
When an object is submerged in a measuring cylinder
contains water rises up with volume equals the volume of the object.
When the body is submerged completely in a cylinder full of a liquid,
the liquid is spilled out of the cylinder,
So.: the volume of the body= the volume of the spilled water.
10. Lesson 2 Matter states and changes
There are three states of matter:
1. Solid state: Examples: [wood – iron – gold – pen – disk – door – spoon ]
2. Liquid state: Examples: [water – milk – juices – tea – coffee]
3. Gaseous state: Examples: [oxygen – carbon dioxide – air – water vapour]
· Matter exists only in one state at room temperature .
10
11. 1. Properties of the three states of matter:
· Solid shape and volume:
Experiment Observation Conclusion
· Bring a stone and put
it in a jar then
transfer it in a dish.
The shape of solid does not
change.
The volume of stone does not
change
Solids have definite
shape and definite
volume.
· Liquid shape and volume:
Experiment Observation Conclusion
· Place 100cm3 of
water in each of the
following pots.
The water takes the shape of
its container.
The volume of water does not
change
Liquid has
definite volume
and indefinite
shape.
· Gases shape and volume:
Experiment Observation Conclusion
Blow a balloon and tie
The shape of balloon changes.
it with a thread then
The volume of balloon changes
press upon it by your
hand
Gases have
indefinite shape
and indefinite
volume.
Changes of Matter
11
Activities
Melting: Change of matter from solid into liquid by heating
12. Evaporation: Change of matter from liquid to gas by heating
Condensation: Change of matter from gas to liquid by cooling
Freezing: Change of matter from liquid to solid by cooling
SSttaatteess ooff mmaatttteerr
SSoolildid Liquid Liquid
12
GGaass
Freezing
Melting
Condensation
Evaporation
13. Its properties Its properties Its properties
Examples
Examples Examples
GaSolids Liquids s
Shape changes according to
the container (no definite
shape).
Shape changes
according to the
container (no definite
shape).
Definite
shape
Shape
Volume changes according to
the container (no definite
volume).
Definite Definite volume
volume
Volume
13
Definite shape
and definite
volume
Definite shape
and definite
volume
Definite volume and
indefinite shape. The
shape changes
according to the shape
of the container
Definite volume and
indefinite shape. The
shape changes
according to the shape
of the container
The volume and
shape change
according to the
shape of the
container
The volume and
shape change
according to the
shape of the
container
IIrroonn
AAirir
WWaatteerr
Lesson 3 Elements around us
EElelemmeennttss
Is the simplest
form of matter
that cannot be
decomposed into 2
substances or more
Is the simplest
form of matter
that cannot be
decomposed into 2
substances or more
14. Their properties Their properties
Examples Examples
· The Economic importance o f Elements (metals & non – metals
14
MMeettaalsls
NNoonn mmeettaalsls
1-Have luster (shiny) Have no luster (not shiny)
2-Good conductor of electricity Bad conductor except carbon
3-Good conductor of heat Bad conductor of heat
4-High melting point Low melting point
5-Malleable (can be bent) Not malleable (can’t be bent)
6-All are solid except mercury solid, liquid and gases
which is liquid
1-Have luster (shiny) Have no luster (not shiny)
2-Good conductor of electricity Bad conductor except carbon
3-Good conductor of heat Bad conductor of heat
4-High melting point Low melting point
5-Malleable (can be bent) Not malleable (can’t be bent)
6-All are solid except mercury solid, liquid and gases
which is liquid
Iron- copper- aluminum-gold-
silver and zinc
Solid as Carbon,sulphur and
phosphorus, liquid as bromine
Uses of metals and non metals
15. Metals Non - metals
15
1- Iron is used in bridges, car
frames, doors and lamp posts.
1-Carbon (graphite) as positive
poles in dry batteries. Why?
2- Aluminum is used in making
(manufacturing) cooking pots and
foil paper.
3- Gold & Silver are used in jewelers. 2-Diamond used in jewels.
4- Copper is used in making some
statues, metal coins & electric
wires.
16. 1- Electric wires are covered with a layer of plastic.
Because plastic is a bad conductor of electricity.
16
Give
reasons:
17. 2- Although metals are solids at room temperature, Mercury is
used in thermometers.
Because Mercury is the only liquid metal.
3- Although carbon is a non-metal, it is used to make the
positive poles of dry cells.
Because carbon is a good conductor of electricity.
Chemical change:
It is the change of the
structure of a substance
producing new substance with
new properties
Examples:
a- Burning of (candle- wood-sugar)
4- Car chassis (frames) & bridges are made of some metals.
Because metals can be hammered, bent and they are ductile.
Lesson Physical 4 and chemical change
Types of changes that occur to
Types of changes that occur to
matter
matter
17
Physical change
It is the change in the
appearance of matter
without a change in its
structure
Examples:
a- Dissolving of sugar & table
salt
b- Malleability, ductility and
bending of elements
C- Melting of wax & ice
d- Paper recycling.
Physical change
It is the change in the
appearance of matter
without a change in its
structure
Examples:
a- Dissolving of sugar & table
salt
b- Malleability, ductility and
bending of elements
C- Melting of wax & ice
d- Paper recycling.
Chemical change:
It is the change of the
structure of a substance
producing new substance with
new properties
Examples:
a- Burning of (candle- wood-sugar)
b- Iron rust
C-Fermentation of food
d- Production of yoghurt from
milk.
b- Iron rust
C-Fermentation of food
d- Production of yoghurt from
milk.
19. Lesson 1: Stars and planets
1-They are lighting bodies with different shapes in the space
2-They seems very small because they are very far from us
a- It is the center of solar system
b- It is a shining star
c- It radiates (emits) light and heat
d- It is the nearest star to us
-They are dark bodies revolve around the sun in fixed orbits
-There are 8 planets, these planets are arranged from the nearest to the
farthest from the sun as:
19
Sta
rs
SSoollaarr ssyysstteemm
Sun Planets Moons Celestial
bodies
Asteroids Comets Meteors Meteoroids
Sun
PPllaanneettss
20. Mercury- Venus- Earth- Mars- Jupiter- Saturn- Uranus and Neptune
The planets of the solar system:
Because of its small size whereas its size is less than one fifth of
the earth’s size.
a- Dark bodies, reflects the light of the sun so it seems shiny
b-Revolves around the planets
20
MMoooonnss
G.R/scientists do not classify Pluto as a planet
21. Activity
Use suitable colors :
The number of moons revolving around the planets:
Mercury Venus Earth Mars Jupiter Saturn Uranus Neptune
- - 1 2 62 60 27 13
Compare between Star, planet & moon
Star Planet Moon
1-It is a shiny body.
1-It is a dark body.
2-It emits heat and
2-It doesn't emit heat
light.
or light.
3-It rotates in the
3- It rotates in space
space.
around the sun.
(apparent rotation)
Ex: The Earth
Ex: The sun
1-It is a dark body.
2-It reflects sunlight
falling on it.
3- It rotates in space
around planets.
Ex: The Moon
Lesson The rotation of the sun and earth
21
2
22. Celestial bodies: The stars, planets and moons are travelling in a
continuous rotation
The sun is a star but it seems larger than the other because it is the
nearest one to us
G.R
G.R
The apparent rotation of the sun
-The sun seems moving from the east to west because the earth rotates
around its axis and not due to the rotation of the sun
-Movement of the shadow of a fixed objectis as a result to the apparent
rotation of the sun
-The sun takes different apparent orbits from east to west
-A summer day is longer than the winter day because the apparent orbit
of the sun in summer is longer than the apparent orbit in winter
- In spring and autumn, the number of hours of the day is nearly equal to
the number of hours of the night.
22
1- The rotation of the sun
2- Rotation of the earth
a- Revolution of the
earth around the sun
b- Rotation of the
earth around its axis
Sequence of seasons Sequence of day and night
23. -The earth rotates around its axis once every 24 hours causing day
and night
-The hours of day is not equal to the hours of night because the
axis of the earth is inclined
-The earth revolves around the sun once every 365 and quarters a
day causing the sequence of the seasons
How to determine the length of day and night?
1- Read of sunset= Time of sunset [12: 00] t 12 hours [12: 00]
2- The length of day = Read of sunset [hour: min] – Read of sunrise
1- Read of sunset= Time of sunset [12: 00] t 12 hours [12: 00]
2- The length of day = Read of sunset [hour: min] – Read of sunrise
[hour : min]
[hour : min]
3- The length of night = 24 hours [24: 00] – length of day [hour: min]
3- The length of night = 24 hours [24: 00] – length of day [hour: min]
Lesson Motion of the moon
23
3
Rotation of the moon
24. Around its axis Around the earth
a-The moon rotates around its axis and around the earth
b-The moon rotates around the earth once every 28 days as the result of
its rotation around the earth the size of the area reflecting the sun light
on the moon changes and that’s why we see it shining
Phases of the moon
It begins in the form of a crescent then half of the moon becomes shining
and then it becomes full moon then changes into a crescent
New moon First Crescent first quadrature (half moon) first gibbous
2nd days 7th days 11thdays
At the beginning of the lunar month
Second crescent second quadrature (half moon) second gibbous
full moon
At the end of lunar month
Attraction among celestial bodies
24
Phases of the moon
2 days
4 days 3 days
21th days 17th days
14th days
25. -There are attraction forces among the celestial bodies
-There is an attraction force between the earth and the sun and between
the earth and the moon
Phenomena resulted from the attraction of both the sun and the moon
to the earth
Why the tide and ebb happens?
It is due to the attraction between the earth and the moon and the
attraction happens between
The earth and the sun as well but the moon is considered the main reason
for tide and ebb because it is nearer to the earth than the sun
Water falling effect
Activity
-put a plastic fan under a water tap and let the water fall
25
Tide
Is the rising of water level to
extend that water covers the
seashores the maximum of the
rising is when the moon is full
Ebb
It is when the water
returns back to its
normal level after the
tide
26. Observation: The rushing of the tap water rotates the fan this is the
idea of the turbines
-The turbines are rotated by the falling of water or by air pushing to
produce electricity
The benefits of tide and ebb:
1-Generating electricity: the flowing of water during the tide and its
retraction during the ebb makes the turbines rotate and produce
electricity
2-Cleaning the coast: water carries the wastes from the coast to the sea
3-Ships and boats: access to the shallow water paths
Lesson The atmosphere and the weather
4
Atmosphere components
26
1- Oxygen gas:
It represents about 1/5of air volume.
The main source of oxygen on Earth is the
photosynthesis process in green plants.
2- Carbon dioxide:
Lime water is used to test carbon dioxide.
27. Gas Oxygen Nitrogen Carbon dioxide other gases Water
27
vapour
Ratios 21% 78% 0.03% 0.79% changing
Im
por
tan
ce
of
3- Nitrogen gas:
It is the most abundant gas in the air as it represents
4/5 of the volume of the atmosphere.
4- Water vapour:
The humidity of air depends on the amount of water
vapour that presents in air so the humidity increases in
coastal regions.
28. Oxygen Carbon dioxide Nitrogen
28
1- Necessary for
respiration of living
organisms.
1- Green plants use it to
make photosynthesis
process.
1- Decrease the effect
of oxygen in combustion.
2- Helps in burning of
fuel.
2- Use to make soda
water.
2- Used in making
ammonia and nitrogenous
fertilizers
3- Divers use oxygen
cylinder to help them
breath under water
3- Helps in fire
extinguisher (put off)
because it doesn’t burn.
4- It is used with
acetylene in cutting and
welding metals.
WWeeaatthheerr
Is the expected conditions of the
atmosphere in an area during a short
period of time not exceeding one week
Clouds & rains
29. The
weather
factors
29
Temperature
Atmospheric pressure
Winds
Temperature
1
Maximum temperature
The expected
temperature during the
day time
Minimum temperature
The expected
temperature during the
night time
Measured by
Mercury thermometer or
digital thermometer
Atmospheric pressure
2
Measured by
Barometer
Activity
30. The cup of water and atmospheric pressure
-Fill a cup with water completely then cover it with white paper, then turn
the cup upside down
Observation: Water does not fall from the cup
Conclusion: the atmospheric pressure equals to water pressure in the cup
- There are places with high atmospheric pressure and others with
low atmospheric pressure
Formation of clouds
4 Clouds and rains
30
Wind
3
Is the movement of air from high
pressure areas toward lower pressure
areas
*The speed of wind causes the rising of
waves of the sea
Measured by
Anemometer measures wind speed
Vane determines the direction of the wind
a
Formation of clouds
The sun rays
The sun rays
evaporate the water
changing it into
water vapour then it
rises in the sky ,
cooled and condensed
evaporate the water
changing it into
water vapour then it
rises in the sky ,
cooled and condensed
forming clouds
forming clouds
Falling of rains
Winds move the
Falling of rains
Winds move the
clouds then it
changes into drops
of water air cannot
carry it so it falls
clouds then it
changes into drops
of water air cannot
carry it so it falls
as rains
as rains
31. The importance of weather prediction
People follow the weather forecast in T.V in order to face some
conditions as:
1-If predicting a lower temperature people should wear heavy
clothes
2-Predicting strong wind below, sea wavesrises up, fishing boats are
advised not to sail
3-Predicting a foggy morning car drivers should slow down ,to avoid
accidents
31