This document provides information about atoms and molecules:
1) It summarizes Dalton's atomic theory, including that atoms are indivisible and combine in small whole number ratios to form compounds.
2) It describes what atoms and molecules are, noting atoms are the smallest particle of an element and molecules are groups of atoms held together.
3) Key concepts like atomic mass, molecular mass, ions, and the mole concept are explained. The mole represents 6.022 x 1023 particles and relates mass, moles, and molar mass.
This document provides information about atoms, molecules, ions and chemical formulas. It discusses key concepts such as:
- Dalton's atomic theory which states that matter is made of tiny indivisible particles called atoms that combine in small whole number ratios.
- Atoms have symbols to represent them and an atomic mass that is measured relative to carbon-12. Molecules are groups of atoms that are chemically bonded.
- Chemical formulas show the types and numbers of atoms or ions that make up a compound. Formulas are written with the cation written first followed by the anion.
1. The document discusses atoms, molecules, ions and chemical formulas. It explains concepts like atomic mass, molecular mass, valency and the mole concept.
2. Key points include Dalton's atomic theory, that atoms combine in small whole number ratios to form compounds, and that the mass of elements and compounds can be expressed in atomic mass units or grams.
3. Molecular mass is calculated by adding the atomic masses of each element in a molecule. A mole represents 6.022 x 1023 particles and can be used to relate mass, number of particles, and molar mass.
The document discusses atoms, molecules, and moles. It explains Dalton's atomic theory that matter is made of tiny indivisible particles called atoms that combine in small whole number ratios to form compounds. It defines atoms, molecules, and ions. It describes how atomic and molecular masses are measured. It introduces the mole concept which relates the number of particles, mass of a substance, and Avogadro's number.
This document provides a summary of key concepts about atoms and molecules:
1) It defines atoms as the smallest particle of an element that retains chemical properties, and molecules as a group of atoms held together.
2) It explains Dalton's atomic theory, including that atoms combine in small whole number ratios to form compounds.
3) It discusses the symbols and masses of atoms, atomicity and valency, writing chemical formulas, and calculating molecular mass.
4) It introduces the mole concept relating the number of particles, mass, and molar mass.
AkWrite about different classes of people on the clothes Aman Pathak:
Conclusion on Trace the train in clothes worn at work,leisure, sports in the early 19th century qnd today in the world and india
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in india with title
Conclusion of
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in indiaAs mentioned earlier, "Chirag" is a two-word short story by Phanishwar Nath Renu. The story goes as follows:
A lamp was burning in a room. A gust of wind blew through the window and extinguished the flame. The end.
The story may seem simple and straightforward, but it has a deeper meaning. The lamp represents life, and the wind represents death. The sudden extinguishing of the lamp symbolizes how life can be snuffed out in an instant. It also emphasizes the fragility of life and how we should cherish every moment we have.
Overall, "Chirag" is a poignant and thought-provoking story that leaves a lasting impact on the reader.Write about different classes of people on the clothes they were when they wear youngAman Pathak:
Conclusion on Trace the train in clothes worn at work,leisure, sports in the early 19th century qnd today in the world and india
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in india with title
Conclusion of
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in indiaBuried Treasure
X: -104 Z: 1,176they were when they wear youngAs mentioned earlier, "Chirag" is a two-word short story by Phanishwar Nath Renu. The story goes as follows:
A lamp was burning in a room. A gust of wind blew through the window and extinguished the flame. The end.
The story may seem simple and straightforward, but it has a deeper meaning. The lamp represents life, and the wind represents death. The sudden extinguishing of the lamp symbolizes how life can be snuffed out in an instant. It also emphasizes the fragility of life and how we should cherish every moment we have.
Overall, "Chirag" is a poignant and thought-provoking story that leaves a lasting impact on the reader.Aman Pathak:
Conclusion on Trace the train in clothes worn at work,leisure, sports in the early 19th century qnd today in the world and india
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in india with title
Conclusion of
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in indiaWrite about different classes of people on the clothes they were when they wear y
This document provides a summary of key concepts about atoms and molecules:
1) It describes Dalton's atomic theory which states that all matter is made of tiny indivisible particles called atoms that combine in small whole number ratios to form compounds.
2) It defines an atom as the smallest particle of an element that retains chemical properties, and a molecule as the smallest particle of an element or compound that exists independently.
3) It explains how atoms of different elements have different masses and properties, and how they combine to form molecules according to their valencies based on their atomic symbols and masses.
This document provides information about several chemistry concepts including:
1. It discusses the laws of conservation of mass and constant proportions, and provides examples of experiments demonstrating these laws.
2. It defines key terms like atoms, elements, molecules, ions, and provides examples of common elements and their symbols.
3. It explains concepts like atomic mass, molecular mass, moles, and the relationship between mass, moles, molar mass and Avogadro's number. Formulas for calculating these values are provided.
The document summarizes key concepts about atoms and molecules:
1) It describes Dalton's atomic theory which states that all matter is composed of tiny indivisible particles called atoms that combine in simple whole number ratios to form compounds.
2) It defines key terms like atoms, molecules, ions, and molar mass. Atoms are the smallest particles that make up elements while molecules are groups of atoms that combine to form compounds.
3) It explains concepts like atomic structure, mass, and symbols. The mass of atoms is measured relative to carbon-12 and atoms are represented by elemental symbols.
4) Molecular mass is the sum of atomic masses of all atoms in a molecule. Compounds are
This document provides information about atoms, molecules, ions and chemical formulas. It discusses key concepts such as:
- Dalton's atomic theory which states that matter is made of tiny indivisible particles called atoms that combine in small whole number ratios.
- Atoms have symbols to represent them and an atomic mass that is measured relative to carbon-12. Molecules are groups of atoms that are chemically bonded.
- Chemical formulas show the types and numbers of atoms or ions that make up a compound. Formulas are written with the cation written first followed by the anion.
1. The document discusses atoms, molecules, ions and chemical formulas. It explains concepts like atomic mass, molecular mass, valency and the mole concept.
2. Key points include Dalton's atomic theory, that atoms combine in small whole number ratios to form compounds, and that the mass of elements and compounds can be expressed in atomic mass units or grams.
3. Molecular mass is calculated by adding the atomic masses of each element in a molecule. A mole represents 6.022 x 1023 particles and can be used to relate mass, number of particles, and molar mass.
The document discusses atoms, molecules, and moles. It explains Dalton's atomic theory that matter is made of tiny indivisible particles called atoms that combine in small whole number ratios to form compounds. It defines atoms, molecules, and ions. It describes how atomic and molecular masses are measured. It introduces the mole concept which relates the number of particles, mass of a substance, and Avogadro's number.
This document provides a summary of key concepts about atoms and molecules:
1) It defines atoms as the smallest particle of an element that retains chemical properties, and molecules as a group of atoms held together.
2) It explains Dalton's atomic theory, including that atoms combine in small whole number ratios to form compounds.
3) It discusses the symbols and masses of atoms, atomicity and valency, writing chemical formulas, and calculating molecular mass.
4) It introduces the mole concept relating the number of particles, mass, and molar mass.
AkWrite about different classes of people on the clothes Aman Pathak:
Conclusion on Trace the train in clothes worn at work,leisure, sports in the early 19th century qnd today in the world and india
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in india with title
Conclusion of
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in indiaAs mentioned earlier, "Chirag" is a two-word short story by Phanishwar Nath Renu. The story goes as follows:
A lamp was burning in a room. A gust of wind blew through the window and extinguished the flame. The end.
The story may seem simple and straightforward, but it has a deeper meaning. The lamp represents life, and the wind represents death. The sudden extinguishing of the lamp symbolizes how life can be snuffed out in an instant. It also emphasizes the fragility of life and how we should cherish every moment we have.
Overall, "Chirag" is a poignant and thought-provoking story that leaves a lasting impact on the reader.Write about different classes of people on the clothes they were when they wear youngAman Pathak:
Conclusion on Trace the train in clothes worn at work,leisure, sports in the early 19th century qnd today in the world and india
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in india with title
Conclusion of
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in indiaBuried Treasure
X: -104 Z: 1,176they were when they wear youngAs mentioned earlier, "Chirag" is a two-word short story by Phanishwar Nath Renu. The story goes as follows:
A lamp was burning in a room. A gust of wind blew through the window and extinguished the flame. The end.
The story may seem simple and straightforward, but it has a deeper meaning. The lamp represents life, and the wind represents death. The sudden extinguishing of the lamp symbolizes how life can be snuffed out in an instant. It also emphasizes the fragility of life and how we should cherish every moment we have.
Overall, "Chirag" is a poignant and thought-provoking story that leaves a lasting impact on the reader.Aman Pathak:
Conclusion on Trace the train in clothes worn at work,leisure, sports in the early 19th century qnd today in the world and india
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in india with title
Conclusion of
Trace the impact of colonization on the handloom workers and industry and compare it with changes in handloom and khadi industry since independence in indiaWrite about different classes of people on the clothes they were when they wear y
This document provides a summary of key concepts about atoms and molecules:
1) It describes Dalton's atomic theory which states that all matter is made of tiny indivisible particles called atoms that combine in small whole number ratios to form compounds.
2) It defines an atom as the smallest particle of an element that retains chemical properties, and a molecule as the smallest particle of an element or compound that exists independently.
3) It explains how atoms of different elements have different masses and properties, and how they combine to form molecules according to their valencies based on their atomic symbols and masses.
This document provides information about several chemistry concepts including:
1. It discusses the laws of conservation of mass and constant proportions, and provides examples of experiments demonstrating these laws.
2. It defines key terms like atoms, elements, molecules, ions, and provides examples of common elements and their symbols.
3. It explains concepts like atomic mass, molecular mass, moles, and the relationship between mass, moles, molar mass and Avogadro's number. Formulas for calculating these values are provided.
The document summarizes key concepts about atoms and molecules:
1) It describes Dalton's atomic theory which states that all matter is composed of tiny indivisible particles called atoms that combine in simple whole number ratios to form compounds.
2) It defines key terms like atoms, molecules, ions, and molar mass. Atoms are the smallest particles that make up elements while molecules are groups of atoms that combine to form compounds.
3) It explains concepts like atomic structure, mass, and symbols. The mass of atoms is measured relative to carbon-12 and atoms are represented by elemental symbols.
4) Molecular mass is the sum of atomic masses of all atoms in a molecule. Compounds are
The document discusses several laws of chemical changes and principles of naming chemical compounds. It describes the law of conservation of mass, law of definite proportions, and law of multiple proportions. It also discusses Dalton's atomic theory and how it can explain these laws. The document provides rules for naming binary, ternary, molecular, and acidic compounds based on their composition and oxidation states. Examples of naming ionic compounds, acids, and writing chemical formulas from compound names are also presented.
This document contains information about chemical laws, atoms, molecules, ions, and formulas. It begins with acknowledging its sources and stating its educational purpose. It then defines the laws of conservation of mass and constant proportions established by scientists. Later sections explain atoms and their properties according to Dalton's atomic theory. It also describes molecules as groups of bonded atoms and provides examples. Ions are defined as charged particles in compounds of metals and nonmetals. The document concludes with multiple choice questions.
This presentation is designed for the students of grades 11 and 12. You can know about the importance and scope of chemistry. Atomic mass, the process of naming compounds, acids, the chemical name of substances, and so on.
The document discusses several key chemistry concepts:
1. Atomic symbols represent chemical elements and isotopes have the same number of protons but different neutrons.
2. Chemical formulas describe elements and compounds. The periodic table arranges elements by atomic number and identifies groups like metals and nonmetals.
3. A mole is defined as 6.02x10^23 particles and is used to relate amounts of substances to mass and numbers of atoms/molecules. Avogadro's number provides this link between microscopic and macroscopic scales.
A PERFECT POWERPOINT PRESENTATION FOR CHAPTER ATOMS AND MOLECULES FOR CLASS 9. IT COVERS ALL THE MAJOR CONCEPTS AND TOPICS OF THE CHAPTER. HOPE YOU LIKE IT.
This document provides an overview of atomic theory, molecules, ions, and chemical nomenclature. It discusses Dalton's atomic theory, laws of multiple proportions and conservation of mass. Models of the atom including Thomson's plum pudding model, Rutherford's nuclear model, and isotopes are summarized. The periodic table is introduced along with molecular and ionic compounds, formulas, and nomenclature rules for acids, bases, and hydrates. Key topics are covered in under 3 sentences.
This document provides an overview of several key chemistry concepts across multiple chapters:
Chapter 1 introduces fundamental concepts like the three states of matter, elements and compounds, and physical and chemical properties.
Chapter 2 discusses atomic structure, including Dalton's atomic theory, early experiments that led to modern atomic models, and the organization of the periodic table. It also introduces molecules, ions, and chemical bonding.
Chapter 3 covers stoichiometry, including atomic masses, the mole concept, and percent composition of compounds.
The document defines important terms and provides examples to illustrate concepts like the periodic table, naming simple ionic and covalent compounds, and acid naming conventions. Diagrams and figures are included to summarize key ideas.
2011 topic 01 lecture 1 - the mole and avogadro's constantDavid Young
This document provides an overview of quantitative chemistry concepts including:
- The mole is a unit used to quantify amounts of substances and represents 6.02x1023 particles.
- Pure substances can exist as individual atoms, molecules, ions or molecular units.
- Chemical formulas represent the types and ratios of elements in compounds.
- Molar mass allows conversion between mass of a sample and number of moles.
- Stoichiometry problems use molar mass and the mole concept to interconvert between moles, atoms, molecules and mass.
This document provides an overview of early atomic theory and the development of modern atomic structure and chemical bonding models. It discusses the Greek concept of atoms, early atomic theories of Democritus and Dalton, experiments by Thomson, Rutherford and others that led to discovery of the electron and nuclear atom, and development of the periodic table. Key concepts introduced include atoms, molecules, ions, isomers, naming binary compounds and acids.
This document discusses chemical formulas and nomenclature. It explains that chemical formulas indicate the relative number and ratio of atoms in a compound. It also describes systems for naming ionic compounds, acids, salts, and covalent network compounds. Oxidation numbers are introduced as a method for determining formulas based on the electronegativity of elements. Molar mass and formula mass are defined as ways to determine the mass of compounds from their chemical formulas.
This document discusses chemical formulas and nomenclature. It explains that chemical formulas indicate the relative number and ratio of atoms in a compound. It also describes systems for naming ionic compounds, acids, salts, and covalent network compounds. Oxidation numbers are introduced as a method for determining formulas based on electronegativity differences between elements. Molar mass and formula mass are defined as ways to determine the mass of compounds from their chemical formulas.
This document provides information on chemical formulas and nomenclature. It discusses how subscripts indicate the number of atoms in formulas. Binary ionic compounds are formed from two elements and have charges that are balanced through subscripts. Polyatomic ions contain more than one atom and oxyanions contain oxygen. Molecular compounds are named using prefixes to indicate the number of atoms. Percent composition gives the percentage by mass of each element in a compound. Empirical formulas show the simplest whole number ratio of atoms in a compound, while molecular formulas give the actual number of atoms, which is a whole number multiple of the empirical formula.
1. Atoms are the smallest particles that make up elements, consisting of a nucleus surrounded by electrons. John Dalton established the first atomic theory in 1808.
2. In the early 20th century, experiments by Thomson, Rutherford, and Chadwick led to discoveries about the internal structure of atoms, including the identification of protons, electrons, and neutrons within the nucleus.
3. Isotopes are atoms of the same element that differ in their number of neutrons. Molecules, ions, and compounds are formed through combinations and interactions between atoms.
This document provides information about chemical nomenclature and reactions. It discusses writing chemical formulas, empirical formulas, chemical naming conventions, chemical equations, balancing equations, and types of chemical reactions. Specifically, it covers how to write formulas using oxidation numbers and valence, how to determine empirical and molecular formulas from composition data, rules for naming ionic and molecular compounds, the components and symbols used in chemical equations, and methods for balancing equations. It also defines four main types of chemical reactions: combination, decomposition, single displacement, and double displacement.
This document provides an overview of basic chemistry concepts including:
- Dalton's atomic theory and modern atomic theory which established atoms as the fundamental units of matter and that they can exist as isotopes.
- Berzelius hypothesis and Avogadro's law which established that equal volumes of gases under similar conditions contain equal numbers of molecules.
- Definitions of atoms, molecules, atomic mass, molecular mass, gram atomic mass, gram molecular mass, formula mass, and gram formula mass.
- Introduction of the mole concept based on Avogadro's number, which established a mole as a specific number of particles (atoms or molecules).
This document provides an overview of atomic structure and chemical bonding. It begins with a brief history of atomic theory from Dalton to Rutherford, including Thomson's discovery of the electron. Key topics covered include atomic number, mass number, isotopes, ions, molecules, chemical formulas and nomenclature. The periodic table is introduced as a way to organize elements based on atomic structure. Chemical formulas are used to represent ionic compounds, molecular compounds and acids/bases. Hydrates are also defined as compounds that contain bonded water molecules.
This document provides an overview of key concepts in atomic structure and chemical bonding:
- It describes early theories of atoms proposed by thinkers like Democritus, Dalton, and Thomson. Experiments by Thomson, Millikan, and Rutherford provided evidence for the atom's internal structure.
- The document defines subatomic particles like protons, neutrons, and electrons. It introduces concepts like isotopes, ions, ionic and covalent bonding.
- Naming conventions for ions, ionic compounds, acids, and hydrates are outlined. Rules for writing chemical formulas are also summarized.
- Key models and experiments that advanced understanding of atomic structure are highlighted, including Dalton's atomic theory and the discoveries of the
The document discusses naming and classification of ions according to IUPAC rules. It defines ions as atoms or groups of atoms with a charge. Cations are positively charged and named by the element followed by "ion". Anions are negatively charged and named by dropping the end of the element name and adding "-ide". Metals that form multiple ions are named with the charge state in Roman numerals. The document also discusses monoatomic and polyatomic ions and common metal ion charges.
This document discusses the history and development of atomic theory. It describes how ancient Indian and Greek philosophers first proposed that matter is divisible into smaller particles. Democritus named these indivisible particles "atoms." Later, scientists like John Dalton and Antoine Lavoisier established laws of chemistry, including the law of conservation of mass and the law of constant proportions, which supported the atomic theory. Dalton further proposed that elements are made of atoms that combine in whole number ratios. The document defines key concepts like molecules, ions, chemical formulas, and moles. It provides examples of atomic structure and molecular formulas of common compounds.
This document discusses the classification of matter into elements, compounds, and mixtures. It defines each term and provides examples. Elements are pure substances made of only one type of atom that cannot be broken down further. Compounds are pure substances composed of two or more elements chemically bonded together in fixed ratios to form new substances with different properties from the original elements. Mixtures are physical combinations of elements or compounds that are not chemically bonded and can be separated by physical means such as filtration or evaporation.
Andreas Schleicher presents PISA 2022 Volume III - Creative Thinking - 18 Jun...EduSkills OECD
Andreas Schleicher, Director of Education and Skills at the OECD presents at the launch of PISA 2022 Volume III - Creative Minds, Creative Schools on 18 June 2024.
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Similar to ppt.ppt of class 9 science ncert cbse ch 2
The document discusses several laws of chemical changes and principles of naming chemical compounds. It describes the law of conservation of mass, law of definite proportions, and law of multiple proportions. It also discusses Dalton's atomic theory and how it can explain these laws. The document provides rules for naming binary, ternary, molecular, and acidic compounds based on their composition and oxidation states. Examples of naming ionic compounds, acids, and writing chemical formulas from compound names are also presented.
This document contains information about chemical laws, atoms, molecules, ions, and formulas. It begins with acknowledging its sources and stating its educational purpose. It then defines the laws of conservation of mass and constant proportions established by scientists. Later sections explain atoms and their properties according to Dalton's atomic theory. It also describes molecules as groups of bonded atoms and provides examples. Ions are defined as charged particles in compounds of metals and nonmetals. The document concludes with multiple choice questions.
This presentation is designed for the students of grades 11 and 12. You can know about the importance and scope of chemistry. Atomic mass, the process of naming compounds, acids, the chemical name of substances, and so on.
The document discusses several key chemistry concepts:
1. Atomic symbols represent chemical elements and isotopes have the same number of protons but different neutrons.
2. Chemical formulas describe elements and compounds. The periodic table arranges elements by atomic number and identifies groups like metals and nonmetals.
3. A mole is defined as 6.02x10^23 particles and is used to relate amounts of substances to mass and numbers of atoms/molecules. Avogadro's number provides this link between microscopic and macroscopic scales.
A PERFECT POWERPOINT PRESENTATION FOR CHAPTER ATOMS AND MOLECULES FOR CLASS 9. IT COVERS ALL THE MAJOR CONCEPTS AND TOPICS OF THE CHAPTER. HOPE YOU LIKE IT.
This document provides an overview of atomic theory, molecules, ions, and chemical nomenclature. It discusses Dalton's atomic theory, laws of multiple proportions and conservation of mass. Models of the atom including Thomson's plum pudding model, Rutherford's nuclear model, and isotopes are summarized. The periodic table is introduced along with molecular and ionic compounds, formulas, and nomenclature rules for acids, bases, and hydrates. Key topics are covered in under 3 sentences.
This document provides an overview of several key chemistry concepts across multiple chapters:
Chapter 1 introduces fundamental concepts like the three states of matter, elements and compounds, and physical and chemical properties.
Chapter 2 discusses atomic structure, including Dalton's atomic theory, early experiments that led to modern atomic models, and the organization of the periodic table. It also introduces molecules, ions, and chemical bonding.
Chapter 3 covers stoichiometry, including atomic masses, the mole concept, and percent composition of compounds.
The document defines important terms and provides examples to illustrate concepts like the periodic table, naming simple ionic and covalent compounds, and acid naming conventions. Diagrams and figures are included to summarize key ideas.
2011 topic 01 lecture 1 - the mole and avogadro's constantDavid Young
This document provides an overview of quantitative chemistry concepts including:
- The mole is a unit used to quantify amounts of substances and represents 6.02x1023 particles.
- Pure substances can exist as individual atoms, molecules, ions or molecular units.
- Chemical formulas represent the types and ratios of elements in compounds.
- Molar mass allows conversion between mass of a sample and number of moles.
- Stoichiometry problems use molar mass and the mole concept to interconvert between moles, atoms, molecules and mass.
This document provides an overview of early atomic theory and the development of modern atomic structure and chemical bonding models. It discusses the Greek concept of atoms, early atomic theories of Democritus and Dalton, experiments by Thomson, Rutherford and others that led to discovery of the electron and nuclear atom, and development of the periodic table. Key concepts introduced include atoms, molecules, ions, isomers, naming binary compounds and acids.
This document discusses chemical formulas and nomenclature. It explains that chemical formulas indicate the relative number and ratio of atoms in a compound. It also describes systems for naming ionic compounds, acids, salts, and covalent network compounds. Oxidation numbers are introduced as a method for determining formulas based on the electronegativity of elements. Molar mass and formula mass are defined as ways to determine the mass of compounds from their chemical formulas.
This document discusses chemical formulas and nomenclature. It explains that chemical formulas indicate the relative number and ratio of atoms in a compound. It also describes systems for naming ionic compounds, acids, salts, and covalent network compounds. Oxidation numbers are introduced as a method for determining formulas based on electronegativity differences between elements. Molar mass and formula mass are defined as ways to determine the mass of compounds from their chemical formulas.
This document provides information on chemical formulas and nomenclature. It discusses how subscripts indicate the number of atoms in formulas. Binary ionic compounds are formed from two elements and have charges that are balanced through subscripts. Polyatomic ions contain more than one atom and oxyanions contain oxygen. Molecular compounds are named using prefixes to indicate the number of atoms. Percent composition gives the percentage by mass of each element in a compound. Empirical formulas show the simplest whole number ratio of atoms in a compound, while molecular formulas give the actual number of atoms, which is a whole number multiple of the empirical formula.
1. Atoms are the smallest particles that make up elements, consisting of a nucleus surrounded by electrons. John Dalton established the first atomic theory in 1808.
2. In the early 20th century, experiments by Thomson, Rutherford, and Chadwick led to discoveries about the internal structure of atoms, including the identification of protons, electrons, and neutrons within the nucleus.
3. Isotopes are atoms of the same element that differ in their number of neutrons. Molecules, ions, and compounds are formed through combinations and interactions between atoms.
This document provides information about chemical nomenclature and reactions. It discusses writing chemical formulas, empirical formulas, chemical naming conventions, chemical equations, balancing equations, and types of chemical reactions. Specifically, it covers how to write formulas using oxidation numbers and valence, how to determine empirical and molecular formulas from composition data, rules for naming ionic and molecular compounds, the components and symbols used in chemical equations, and methods for balancing equations. It also defines four main types of chemical reactions: combination, decomposition, single displacement, and double displacement.
This document provides an overview of basic chemistry concepts including:
- Dalton's atomic theory and modern atomic theory which established atoms as the fundamental units of matter and that they can exist as isotopes.
- Berzelius hypothesis and Avogadro's law which established that equal volumes of gases under similar conditions contain equal numbers of molecules.
- Definitions of atoms, molecules, atomic mass, molecular mass, gram atomic mass, gram molecular mass, formula mass, and gram formula mass.
- Introduction of the mole concept based on Avogadro's number, which established a mole as a specific number of particles (atoms or molecules).
This document provides an overview of atomic structure and chemical bonding. It begins with a brief history of atomic theory from Dalton to Rutherford, including Thomson's discovery of the electron. Key topics covered include atomic number, mass number, isotopes, ions, molecules, chemical formulas and nomenclature. The periodic table is introduced as a way to organize elements based on atomic structure. Chemical formulas are used to represent ionic compounds, molecular compounds and acids/bases. Hydrates are also defined as compounds that contain bonded water molecules.
This document provides an overview of key concepts in atomic structure and chemical bonding:
- It describes early theories of atoms proposed by thinkers like Democritus, Dalton, and Thomson. Experiments by Thomson, Millikan, and Rutherford provided evidence for the atom's internal structure.
- The document defines subatomic particles like protons, neutrons, and electrons. It introduces concepts like isotopes, ions, ionic and covalent bonding.
- Naming conventions for ions, ionic compounds, acids, and hydrates are outlined. Rules for writing chemical formulas are also summarized.
- Key models and experiments that advanced understanding of atomic structure are highlighted, including Dalton's atomic theory and the discoveries of the
The document discusses naming and classification of ions according to IUPAC rules. It defines ions as atoms or groups of atoms with a charge. Cations are positively charged and named by the element followed by "ion". Anions are negatively charged and named by dropping the end of the element name and adding "-ide". Metals that form multiple ions are named with the charge state in Roman numerals. The document also discusses monoatomic and polyatomic ions and common metal ion charges.
This document discusses the history and development of atomic theory. It describes how ancient Indian and Greek philosophers first proposed that matter is divisible into smaller particles. Democritus named these indivisible particles "atoms." Later, scientists like John Dalton and Antoine Lavoisier established laws of chemistry, including the law of conservation of mass and the law of constant proportions, which supported the atomic theory. Dalton further proposed that elements are made of atoms that combine in whole number ratios. The document defines key concepts like molecules, ions, chemical formulas, and moles. It provides examples of atomic structure and molecular formulas of common compounds.
This document discusses the classification of matter into elements, compounds, and mixtures. It defines each term and provides examples. Elements are pure substances made of only one type of atom that cannot be broken down further. Compounds are pure substances composed of two or more elements chemically bonded together in fixed ratios to form new substances with different properties from the original elements. Mixtures are physical combinations of elements or compounds that are not chemically bonded and can be separated by physical means such as filtration or evaporation.
Similar to ppt.ppt of class 9 science ncert cbse ch 2 (20)
Andreas Schleicher presents PISA 2022 Volume III - Creative Thinking - 18 Jun...EduSkills OECD
Andreas Schleicher, Director of Education and Skills at the OECD presents at the launch of PISA 2022 Volume III - Creative Minds, Creative Schools on 18 June 2024.
Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
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2. 1) Laws of chemical combination :-
i) Law of conservation of mass :- states that ‘Mass can neither be
created nor destroyed in a chemical reaction’.
This means that during a chemical reaction the sum of the masses of
the reactants and products remain unchanged.
Activity :-
Take some sodium sulphate solution in a conical flask and some
barium chloride solution in an ignition tube. Hang the ignition tube in
the flask by a thread and pot a cork on the flask. Find the mass of the
flask on a balance. Then tilt the flask. A chemical reaction takes place
and sodium chloride and barium sulphate are formed. Then find the
mass of the flask again. It will be seen that the sum of the masses of the
reactants and products remain unchanged.
BaCl2
solution
BaSO4 white
3. ii) Law of constant proportions :- states that ‘ In a chemical
compound the elements are always present in a definite proportion by
mass’.
Eg :- Water ( H2O) always contains two elements hydrogen and oxygen
combined together in the same ratio of 2:16 or 1:8 by mass. If 9 g of
water is decomposed we get 1 g of hydrogen and 8 g of oxygen.
Ammonia (NH3) always contains two elements nitrogen and
hydrogen combined together in the same ratio of 14:3 by mass.
4.
5. 2) Dalton’s atomic theory :-
i) Matter is made up of tiny particles called atoms.
ii) Atoms are indivisible and cannot be created or destroyed
in a chemical reaction
iii) Atoms of a given element are similar in mass and
properties.
iv) Atoms of different elements have different masses and
properties.
v) Atoms combine in small whole number ratios to form
compounds.
vi) In a given compound the relative number and kind of
atoms are constant.
6. 3) Atom :-
An atom is the smallest particle of an element that may or
may not exist independently and retains all its chemical
properties.
Atoms are very small in size and smaller than anything
we can imagine or compare with.
Atomic radius is measured in nanometres (nm)
1 nanometer = 10 -9 m or 1 meter = 109 nm
Eg :- The atomic radius of an atom of hydrogen is 10-10 m.
The radius of a molecule of water is 10-9 m.
7. 4) Symbols of atoms of different elements :-
The symbols of elements are represented by letters.
The symbols of some elements are represented by one letter and the
symbols of some elements are represented by two letters.
If the symbol has only one letter it should be written as capital letter
and if the symbol has two letters then the first letter should be capital
letter and the second letter should be small letter.
Symbols of some common elements :-
Element Symbol Element Symbol Element Symbol
Aluminium Al Copper Cu Nitrogen N
Argon Ar Fluorine F Oxygen O
Barium Ba Gold Au Potassium K
Boron B Hydrogen H Silicon Si
Bromine Br Iodine I Silver Ag
Calcium Ca Iron Fe Sodium Na
Carbon C Lead Pb Sulphur S
Chlorine Cl Magnesium Mg Uranium U
Cobalt Co Neon Ne Zinc Zn
8. 5) Atomic mass :-
Since atoms are very small in size its mass is very small and
determining its mass is very difficult. So the mass of an atom is
compared with the mass of a standard atom.
The atom which is considered as a standard atom for comparing the
masses of other atoms is carbon – 12 atom whose atomic mass is
12 u (atomic mass unit).
One atomic mass unit (u) is the mass of 1/12th the mass of a carbon –
12 atom.
The atomic mass of an element is defined as the average mass of one
atom of the element compared with 1/12th the mass of a carbon – 12
atom.
Atomic masses of some elements :-
Element Atomic mass (u) Element Atomic mass (u)
Hydrogen 1 Magnesium 24
Carbon 12 Aluminium 27
Nitrogen 14 Sulphur 32
Oxygen 16 Chlorine 35.5
Sodium 23 Calcium 40
9. 6) Molecule :-
A molecule is the smallest particle of an element or
compound which exists independently and shows all the
properties of that substance.
A molecule is a group of two or more elements that are
held together by attractive forces.
Atoms of the same element or different elements can join
together to form molecules.
10. i) Molecule of elements :-
Molecule of an element contains atoms of the same element.
Molecules of some elements contain only one atom and molecules of
some elements contain two or more atoms.
Atomicity of an element :- is the number of atoms present in
one molecule of the element.
Atomicity of some elements :-
Type of element Name Atomicity
Non metal Argon Ar 1 – Monoatomic
Non metal Helium He 1 – Monoatomic
Non metal Oxygen O2 2 – Diatomic
Non metal Hydrogen H2 2 – Diatomic
Non metal Nitrogen N2 2 – Diatomic
Non metal Chlorine Cl2 2 – Diatomic
Npn metal Phosphorus P4 4 – Phosphorus
Non metal Sulphur S8 Poly atomic
Metal Sodium Na 1 – Monoatomic
Metal Iron Fe 1 – Monoatomic
Metal Aluminium Al 1 – Monoatomic
Metal Copper Cu 1 – Monoatomic
11. ii) Molecule of compounds :-
Molecule of a compound contains atoms of two or more different
types of elements.
Molecules of some compounds :-
Compound Combining elements Number of atoms of each
elements
Water – H2O Hydrogen, Oxygen 2 - Hydrogen, 1 - Oxygen
Ammonia – NH3 Nitrogen, Hydrogen 1 - Nitrogen, 3 - Hydrogen
Carbon dioxide
CO2
Carbon, Oxygen I - Carbon, 2 - Oxygen
Hydrochloric acid
HCl
Hydrogen, Chlorine 1 - Hydrogen, 1 - Chlorine
Nitric acid
HNO3
Hydrogen, Nitrogen, Oxygen 1 - Hydrogen, 1 - Nitrogen,
3 - Oxygen
Sulphuric acid
H2SO4
Hydrogen, Sulphur, Oxygen 2 - Hydrogen, 1 - Sulphur,
4 - Oxygen
12. 7) Ions :-
Compounds containing metal and non metal elements contain
charged particles called ions.
An ion is a charged particle having positive or negative charge. A
positively charged ion is called ‘cation’ and a negatively charged ion is
called ‘anion’.
Valency :- is the combining capacity of an element.
Some common ions and their valencies :-
Valency Name of ion Symbol Name of ion Symbol Name of ion Symbol
1 Sodium Na+ Hydrogen H + Ammonium NH 4
-
1 Potassium K+ Hydride H - Hydroxide OH -
1 Silver Ag+ Chloride Cl - Nitrate NO3
-
1 Copper (I) Cu+ Bromide Br - Hydrogen carbonate HCO3
-
2 Magnesium Mg 2+ Iodide I -
2 Calcium Ca 2+ Oxide O 2- Carbonate CO3
2-
2 Zinc Zn 2+ Sulphite SO3
2-
2 Iron (II) Fe 2+ Sulphate SO4
2-
2 Copper (II) Cu 2+
3 Aluminium Al 3+ Nitride N 3- Phosphate PO4
3-
3 Iron (iii) Fe 3+
13. 8) Writing chemical formulae :-
i) Write the symbols / formula of the elements or ions so that the
symbol of the metal or positive ion is on the left and symbol / formula
of the non metal or negative ion is on the right.
ii) Write the valencies of the elements or ions below the elements or
ions.
iii) Cross over the valencies of the combining ions.
iv) Polyatomic ions should be enclosed in bracket before writing the
formula.
Examples :-
i) Formula of hydrogen chloride ii) Formula of hydrogen sulphide
Symbol H Cl Symbol H S
Valency 1 1 Valency 1 2
Formula HCl Formula H2S
iii) Formula of Magnesium chloride iv) Formula of Carbon tetrachloride
Symbol Mg Cl Symbol C Cl
Valency 2 1 Valency 4 1
Formula MgCl2 Formula CCl4
14. v) Formula of Calcium oxide vi) Formula of Aluminium oxide
Symbol Ca O Symbol Al O
Valency 2 2 Valency 3 2
Formula Ca2O2 = CaO Formula Al2O3
vii) Formula of Sodium nitrate viii) Formula of Calcium hydroxide
Symbol/ Na NO3 Symbol/ Ca OH
Formula Formula
Valency 1 1 Valency 2 1
Formula NaNO3 Ca(OH)2
ix) Formula of Sodium carbonate x) Formula of Ammonium sulphate
Symbol/ Na CO3 Symbol/ NH4 SO4
Formula Formula
Valency 1 2 Valency 1 2
Formula Na2CO3 (NH4)2SO4
15. 9) Molecular mass / Formula unit mass:-
The molecular mass of a substance is the sum of the
atomic masses of all the atoms in a molecule of the
substance.
Molecular mass is expressed in atomic mass units (u).
Eg:- Molecular mass of water – H2O
Atomic mass of H = I u
Atomic mass of O = 16 u
Molecular mass of H2O = 1x2+10 = 2+16 = 18 u
Molecular mass of Nitric acid – HNO3
Atomic mass of H = 1 u
Atomic mass of N = 14 u
Atomic mass of O = 16 u
Molecular mass of HNO3 = 1+14+16x3 = 1+14+48 = 63 u
16. 10) Mole concept :-
A mole of a substance is that amount of the substance which contains the
same number of particles (atoms, molecules or ions) that are present in 12g of
Carbon – 12.
The number of particles (atoms) present in 12g of Carbon – 12 is
6.022 x 1023 . This number is called Avagadro Number or Avagadro Constant.
A mole represents two things :-
i) It represents a definite number of particles (atoms, molecules or ions) equal to
6.022 x 1023 .
ii) It represents a definite mass of a substance equal to the gram atomic mass of
an element or the gram molecular mass of a compound.
Gram atomic mass of an element :- is its atomic mass expressed in grams.
Eg :- Gram atomic mass of Oxygen = O2 = 16 x 2 = 32g.
Gram molecular mass of a compound :- is its molecular mass expressed in
grams.
Eg :- Gram molecular mass of water = H2O = 1 x 2 + 16 = 2 + 16 = 18g.
Relationship between number of moles (n), mass (m), molar mass (M), Number
of atoms or molecules (N), and Avagadro number (NO).
m N m
n = ---- , n = ---- , m = n x N , M = ---
M NO n