The document discusses matter and chemical change. It defines matter as anything that has mass and takes up space. Matter exists in different states - solid, liquid, and gas - which are determined by the motion and spacing of particles. Changes between states of matter involve adding or removing heat. Chemical and physical properties are also discussed, where chemical changes alter the chemical composition and physical changes do not. The document provides examples of physical and chemical properties and changes. Classifying matter as elements, compounds, or mixtures is also covered.
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 introduction to chemistry, including:
1. Definitions of key terms like matter, elements, compounds, properties and changes in matter.
2. The major branches of chemistry like organic, inorganic, physical and analytical chemistry.
3. An overview of the periodic table, including periodic trends and classifications of elements as metals, nonmetals, metalloids and noble gases.
This document provides an overview of chemistry concepts including:
- Atoms are made of protons, neutrons, and electrons. Protons and neutrons are in the nucleus while electrons orbit around it.
- Elements are substances made of only one type of atom. Compounds are formed when elements combine via ionic or covalent bonds.
- Dmitri Mendeleev is credited with creating the first recognizable periodic table in 1869, which organized elements by atomic mass and predicted new elements.
- Chemical reactions involve changes in atoms or molecules and can be identified by physical changes like temperature, color, or bubbling. Reaction rates depend on factors like temperature, particle size, and stirring.
Matter and energy are the fundamental building blocks of chemistry. The periodic table organizes elements based on atomic structure and properties to help understand relationships between different types of matter. Physical changes alter a substance's state without changing its chemical makeup, while chemical changes form new substances through atomic rearrangements. Scientific models are used to represent unobservable phenomena and further our understanding of how matter behaves.
The document outlines the evolution of atomic structure models from early ideas to modern understanding. It discusses early thinkers like Democritus who proposed atoms as fundamental units of matter. John Dalton later proposed his atomic theory which stated that atoms are indivisible and cannot be created or destroyed. J.J. Thomson's discovery of the electron through deflection experiments in a cathode ray tube provided evidence that atoms contain smaller subatomic particles, contradicting Dalton's ideas. This led to proposals of early atomic structure models like the plum pudding model.
This document provides an overview of the periodic table of elements and key information about each group. It discusses the physical and chemical properties of elements in groups 1-18, including alkali metals, alkaline earth metals, transition metals, and noble gases. Diagrams showing atomic structure (Bohr models and Lewis dot structures) are provided for many elements, along with examples of common compounds and reactions. The periodic trends of atomic radius, ionization energy, and reactivity across periods and down groups are also covered.
This document provides an overview of several key concepts in chemistry including:
- The structure of atoms and how they interact through ionic bonds by transferring electrons or covalent bonds by sharing electrons.
- How the periodic table organizes elements based on their atomic structure and valence electrons.
- The formation of ions when atoms gain or lose electrons to achieve full energy levels. Ionic bonds are formed when oppositely charged ions attract.
- Covalent bonds form when atoms share valence electrons to achieve full energy levels.
- Polar molecules that have unequal sharing of electrons can form hydrogen bonds through weak electrostatic attractions between partially positive and negative regions.
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 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 introduction to chemistry, including:
1. Definitions of key terms like matter, elements, compounds, properties and changes in matter.
2. The major branches of chemistry like organic, inorganic, physical and analytical chemistry.
3. An overview of the periodic table, including periodic trends and classifications of elements as metals, nonmetals, metalloids and noble gases.
This document provides an overview of chemistry concepts including:
- Atoms are made of protons, neutrons, and electrons. Protons and neutrons are in the nucleus while electrons orbit around it.
- Elements are substances made of only one type of atom. Compounds are formed when elements combine via ionic or covalent bonds.
- Dmitri Mendeleev is credited with creating the first recognizable periodic table in 1869, which organized elements by atomic mass and predicted new elements.
- Chemical reactions involve changes in atoms or molecules and can be identified by physical changes like temperature, color, or bubbling. Reaction rates depend on factors like temperature, particle size, and stirring.
Matter and energy are the fundamental building blocks of chemistry. The periodic table organizes elements based on atomic structure and properties to help understand relationships between different types of matter. Physical changes alter a substance's state without changing its chemical makeup, while chemical changes form new substances through atomic rearrangements. Scientific models are used to represent unobservable phenomena and further our understanding of how matter behaves.
The document outlines the evolution of atomic structure models from early ideas to modern understanding. It discusses early thinkers like Democritus who proposed atoms as fundamental units of matter. John Dalton later proposed his atomic theory which stated that atoms are indivisible and cannot be created or destroyed. J.J. Thomson's discovery of the electron through deflection experiments in a cathode ray tube provided evidence that atoms contain smaller subatomic particles, contradicting Dalton's ideas. This led to proposals of early atomic structure models like the plum pudding model.
This document provides an overview of the periodic table of elements and key information about each group. It discusses the physical and chemical properties of elements in groups 1-18, including alkali metals, alkaline earth metals, transition metals, and noble gases. Diagrams showing atomic structure (Bohr models and Lewis dot structures) are provided for many elements, along with examples of common compounds and reactions. The periodic trends of atomic radius, ionization energy, and reactivity across periods and down groups are also covered.
This document provides an overview of several key concepts in chemistry including:
- The structure of atoms and how they interact through ionic bonds by transferring electrons or covalent bonds by sharing electrons.
- How the periodic table organizes elements based on their atomic structure and valence electrons.
- The formation of ions when atoms gain or lose electrons to achieve full energy levels. Ionic bonds are formed when oppositely charged ions attract.
- Covalent bonds form when atoms share valence electrons to achieve full energy levels.
- Polar molecules that have unequal sharing of electrons can form hydrogen bonds through weak electrostatic attractions between partially positive and negative regions.
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 provides an overview of key chemistry concepts including the states of matter, atoms, bonding, and molecular structures.
It begins by explaining the particle nature of matter and defining solids, liquids, and gases. Atoms are introduced as the smallest particles that make up elements, which can combine to form compounds. Bonding types - ionic, covalent, and metallic - are then described along with their characteristic properties. Molecular structures like diamond, graphite, and silica are used as examples of giant covalent networks.
The document concludes by recapping the main differences between ionic, covalent and metallic bonding in terms of structure and properties. Key areas of chemistry are covered concisely with definitions and
Scientists have developed many models to explain the structure of matter over time. Early Greek philosophers proposed that all matter was made of different combinations of four elements. Democritus was the first to propose that all matter was made of tiny indivisible particles called atoms. Later scientists like Dalton, Thompson, and Rutherford contributed to the modern atomic model through discoveries like electrons and the nucleus. The states of matter - solid, liquid, gas - can be explained by the kinetic molecular theory, which describes how the motion and energy of atoms changes between states. Physical properties can be observed directly while chemical properties describe how matter interacts or changes during chemical reactions.
The document discusses various topics relating to chemistry including chemical reactions, the periodic table, chemical bonding, and reaction rates. It provides definitions and explanations of key terms and concepts. Examples are given to illustrate different types of chemical reactions like synthesis, decomposition, combustion, and displacement reactions. Factors that affect reaction rates like concentration, temperature, surface area, and catalysts are also summarized.
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 provides an overview of physical science concepts related to matter. It defines matter as anything that has mass and takes up space. All matter is made up of atoms, which are the smallest units comprising over 100 different elements. The document discusses the structure of atoms including protons, neutrons, and electrons. It also defines key terms like elements, compounds, mixtures, solutions, and homogeneous and heterogeneous mixtures. Students are provided guidance on setting up their lab notebooks and navigating the class wiki page to access course resources and assignments.
The document provides an overview of the periodic table and classification of elements and matter. It discusses how elements are classified based on their properties, including metals and nonmetals. Key periodic patterns are described, such as how the chemical behavior of elements is determined by their electron configuration. The periodic law is explained, as well as the development of the modern periodic table with periods and families.
Water is a polar solvent that is able to dissolve many other polar substances through hydrogen bonding. Solutions are homogeneous mixtures of two or more substances, with water being the most common solvent. The concentration of a solution depends on the amount of solute dissolved and can be measured in various ways. Acids and bases are defined by whether they donate or accept protons in water, with pH used to measure their strength on a logarithmic scale. Salts are formed through neutralization of acids and bases. Buffers resist changes in pH through reactions between their components.
- The document discusses atomic structure and the development of atomic models.
- Early experiments showed atoms were divisible, with Thomson discovering electrons and Rutherford discovering protons.
- Rutherford's gold foil experiment disproved Thomson's "plum pudding" atomic model and led Rutherford to propose a nuclear model with electrons in empty space around a tiny, dense nucleus.
This document discusses the structure and composition of matter. It explains that all matter is made up of elements, which are composed of atoms. Atoms contain protons, neutrons, and electrons. Elements can bond together through ionic bonds, covalent bonds, or hydrogen bonds to form molecules or compounds. Some important compounds are electrolytes, acids, bases, and salts. Chemical reactions cause bonds to form or break as atoms rearrange. The human body relies on many chemical processes and requires maintaining a narrow pH range in the blood for survival.
The document discusses the structure of atoms. It describes John Dalton's model of indivisible atoms and J.J. Thomson's model with a positive sphere and negative electrons. Ernest Rutherford proposed a model with protons and neutrons in the nucleus and electrons orbiting it. Neils Bohr proposed electron shells, and James Chadwick discovered neutrons in the nucleus. Atoms have protons, neutrons, and electrons. The number of protons determines the element. Isotopes have the same number of protons but different neutrons. Electron configuration involves filling shells with a maximum of 2, 8, 8 electrons.
Chemistry 9th class Chapter 1 Basic Definitions CompleteGhanwaSamad
This document provides definitions and explanations of fundamental chemistry concepts. It defines matter as anything that has mass and occupies space, and classifies matter as either a substance or mixture. A substance is a pure form of matter with fixed composition and properties, while a mixture contains two or more substances mixed together without a fixed ratio. Elements are substances made of only one type of atom that cannot be broken down further, while compounds are formed by chemical combination of two or more elements in a fixed ratio to form a new substance with different properties. Mixtures can be separated into their original substances using physical methods, while compounds require chemical processes to decompose.
This document provides an overview of key concepts in biology and physical science, including:
- Chemistry is the study of matter, physics is the study of energy and its effects on matter. Matter is anything that has mass and takes up space.
- Atoms are the basic building blocks of matter. Atoms can combine to form molecules and compounds with unique properties.
- The periodic table organizes the known elements based on their atomic structure. Elements combine via ionic or covalent bonds to reach stable electron configurations.
- Matter exists in solid, liquid, gas or plasma states, depending on temperature and pressure. Physical and chemical properties can be observed and measured without changing the identity of the substance.
For more such informative content, go to https://scifitechify.blogspot.com/. This video will introduce you to the world of ATOMS & MOLECULES. HOPE YOU ENJOY IT. NEXT POST ON: WHY DO WE WEIGH LESS ON THE MOON ?
This chapter introduces key concepts in chemistry including distinguishing science from technology, defining important terms like hypothesis and theory, and classifying types of matter. It outlines learning objectives related to the states and properties of matter, physical and chemical changes, and using units and calculations. Students will learn to differentiate elements, compounds, mixtures and various research types as well as manipulate matter concepts like density, heat, temperature and phases. Critical thinking skills will also be developed.
This document provides information about classifying matter and its composition. It defines pure substances as elements or compounds made of uniform particles and mixtures as substances with two or more types of particles. Pure substances undergo physical or chemical changes, which respectively involve changes in properties or the formation of new substances. The document also discusses atoms as the basic building blocks of matter, containing subatomic particles like protons, neutrons, and electrons. It introduces the periodic table as organizing the elements by their chemical properties and number of protons.
This document provides an overview of key concepts in chemistry. It discusses the study of matter and its composition, properties, and interactions. Matter can exist in various phases and be classified as elements, compounds, or mixtures. Properties include physical characteristics that do not change composition and chemical properties that involve compositional changes. Measurements in chemistry require units and have uncertainty. The document outlines common units in the International System of units and concepts like accuracy and precision in reported values.
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.
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.
Scientists have developed many models to explain the structure of matter over time. Early Greek philosophers proposed that all matter was made of different combinations of four elements. Democritus was the first to propose that all matter was made of tiny indivisible particles called atoms. Later scientists like Dalton, Thompson, and Rutherford contributed to the modern atomic model through discoveries like electrons and the nucleus. The states of matter - solid, liquid, gas - can be explained by the kinetic molecular theory involving the motion and arrangement of atoms. Physical properties describe observable characteristics while chemical properties involve interactions and reactions between substances. Changes in a substance's properties indicate either a physical change that does not alter identity, or a chemical change forming a new substance.
Physical, chemical changes & states of matter.pptJenny Dixon
Physical changes alter the shape or form of a substance but not its chemical composition. Chemical changes alter the molecular structure of a substance and create new substances. States of matter include solids, liquids, gases, and plasmas, which substances can transition between when temperature or other conditions change. A Bose-Einstein condensate is a state of matter that occurs when atoms are cooled to near absolute zero and behave as a single superatom.
This chapter discusses the fundamental concepts of chemistry including the structure of atoms, phases of matter, physical and chemical properties and changes, elements and compounds. It explains that chemistry is the study of matter and its transformations, and covers topics such as the submicroscopic nature of atoms and molecules, the three phases of matter, and how to distinguish physical and chemical changes. It also provides guidelines for naming common chemical compounds using prefixes and suffixes based on the elements present.
This document provides an overview of key chemistry concepts including the states of matter, atoms, bonding, and molecular structures.
It begins by explaining the particle nature of matter and defining solids, liquids, and gases. Atoms are introduced as the smallest particles that make up elements, which can combine to form compounds. Bonding types - ionic, covalent, and metallic - are then described along with their characteristic properties. Molecular structures like diamond, graphite, and silica are used as examples of giant covalent networks.
The document concludes by recapping the main differences between ionic, covalent and metallic bonding in terms of structure and properties. Key areas of chemistry are covered concisely with definitions and
Scientists have developed many models to explain the structure of matter over time. Early Greek philosophers proposed that all matter was made of different combinations of four elements. Democritus was the first to propose that all matter was made of tiny indivisible particles called atoms. Later scientists like Dalton, Thompson, and Rutherford contributed to the modern atomic model through discoveries like electrons and the nucleus. The states of matter - solid, liquid, gas - can be explained by the kinetic molecular theory, which describes how the motion and energy of atoms changes between states. Physical properties can be observed directly while chemical properties describe how matter interacts or changes during chemical reactions.
The document discusses various topics relating to chemistry including chemical reactions, the periodic table, chemical bonding, and reaction rates. It provides definitions and explanations of key terms and concepts. Examples are given to illustrate different types of chemical reactions like synthesis, decomposition, combustion, and displacement reactions. Factors that affect reaction rates like concentration, temperature, surface area, and catalysts are also summarized.
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 provides an overview of physical science concepts related to matter. It defines matter as anything that has mass and takes up space. All matter is made up of atoms, which are the smallest units comprising over 100 different elements. The document discusses the structure of atoms including protons, neutrons, and electrons. It also defines key terms like elements, compounds, mixtures, solutions, and homogeneous and heterogeneous mixtures. Students are provided guidance on setting up their lab notebooks and navigating the class wiki page to access course resources and assignments.
The document provides an overview of the periodic table and classification of elements and matter. It discusses how elements are classified based on their properties, including metals and nonmetals. Key periodic patterns are described, such as how the chemical behavior of elements is determined by their electron configuration. The periodic law is explained, as well as the development of the modern periodic table with periods and families.
Water is a polar solvent that is able to dissolve many other polar substances through hydrogen bonding. Solutions are homogeneous mixtures of two or more substances, with water being the most common solvent. The concentration of a solution depends on the amount of solute dissolved and can be measured in various ways. Acids and bases are defined by whether they donate or accept protons in water, with pH used to measure their strength on a logarithmic scale. Salts are formed through neutralization of acids and bases. Buffers resist changes in pH through reactions between their components.
- The document discusses atomic structure and the development of atomic models.
- Early experiments showed atoms were divisible, with Thomson discovering electrons and Rutherford discovering protons.
- Rutherford's gold foil experiment disproved Thomson's "plum pudding" atomic model and led Rutherford to propose a nuclear model with electrons in empty space around a tiny, dense nucleus.
This document discusses the structure and composition of matter. It explains that all matter is made up of elements, which are composed of atoms. Atoms contain protons, neutrons, and electrons. Elements can bond together through ionic bonds, covalent bonds, or hydrogen bonds to form molecules or compounds. Some important compounds are electrolytes, acids, bases, and salts. Chemical reactions cause bonds to form or break as atoms rearrange. The human body relies on many chemical processes and requires maintaining a narrow pH range in the blood for survival.
The document discusses the structure of atoms. It describes John Dalton's model of indivisible atoms and J.J. Thomson's model with a positive sphere and negative electrons. Ernest Rutherford proposed a model with protons and neutrons in the nucleus and electrons orbiting it. Neils Bohr proposed electron shells, and James Chadwick discovered neutrons in the nucleus. Atoms have protons, neutrons, and electrons. The number of protons determines the element. Isotopes have the same number of protons but different neutrons. Electron configuration involves filling shells with a maximum of 2, 8, 8 electrons.
Chemistry 9th class Chapter 1 Basic Definitions CompleteGhanwaSamad
This document provides definitions and explanations of fundamental chemistry concepts. It defines matter as anything that has mass and occupies space, and classifies matter as either a substance or mixture. A substance is a pure form of matter with fixed composition and properties, while a mixture contains two or more substances mixed together without a fixed ratio. Elements are substances made of only one type of atom that cannot be broken down further, while compounds are formed by chemical combination of two or more elements in a fixed ratio to form a new substance with different properties. Mixtures can be separated into their original substances using physical methods, while compounds require chemical processes to decompose.
This document provides an overview of key concepts in biology and physical science, including:
- Chemistry is the study of matter, physics is the study of energy and its effects on matter. Matter is anything that has mass and takes up space.
- Atoms are the basic building blocks of matter. Atoms can combine to form molecules and compounds with unique properties.
- The periodic table organizes the known elements based on their atomic structure. Elements combine via ionic or covalent bonds to reach stable electron configurations.
- Matter exists in solid, liquid, gas or plasma states, depending on temperature and pressure. Physical and chemical properties can be observed and measured without changing the identity of the substance.
For more such informative content, go to https://scifitechify.blogspot.com/. This video will introduce you to the world of ATOMS & MOLECULES. HOPE YOU ENJOY IT. NEXT POST ON: WHY DO WE WEIGH LESS ON THE MOON ?
This chapter introduces key concepts in chemistry including distinguishing science from technology, defining important terms like hypothesis and theory, and classifying types of matter. It outlines learning objectives related to the states and properties of matter, physical and chemical changes, and using units and calculations. Students will learn to differentiate elements, compounds, mixtures and various research types as well as manipulate matter concepts like density, heat, temperature and phases. Critical thinking skills will also be developed.
This document provides information about classifying matter and its composition. It defines pure substances as elements or compounds made of uniform particles and mixtures as substances with two or more types of particles. Pure substances undergo physical or chemical changes, which respectively involve changes in properties or the formation of new substances. The document also discusses atoms as the basic building blocks of matter, containing subatomic particles like protons, neutrons, and electrons. It introduces the periodic table as organizing the elements by their chemical properties and number of protons.
This document provides an overview of key concepts in chemistry. It discusses the study of matter and its composition, properties, and interactions. Matter can exist in various phases and be classified as elements, compounds, or mixtures. Properties include physical characteristics that do not change composition and chemical properties that involve compositional changes. Measurements in chemistry require units and have uncertainty. The document outlines common units in the International System of units and concepts like accuracy and precision in reported values.
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.
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.
Scientists have developed many models to explain the structure of matter over time. Early Greek philosophers proposed that all matter was made of different combinations of four elements. Democritus was the first to propose that all matter was made of tiny indivisible particles called atoms. Later scientists like Dalton, Thompson, and Rutherford contributed to the modern atomic model through discoveries like electrons and the nucleus. The states of matter - solid, liquid, gas - can be explained by the kinetic molecular theory involving the motion and arrangement of atoms. Physical properties describe observable characteristics while chemical properties involve interactions and reactions between substances. Changes in a substance's properties indicate either a physical change that does not alter identity, or a chemical change forming a new substance.
Physical, chemical changes & states of matter.pptJenny Dixon
Physical changes alter the shape or form of a substance but not its chemical composition. Chemical changes alter the molecular structure of a substance and create new substances. States of matter include solids, liquids, gases, and plasmas, which substances can transition between when temperature or other conditions change. A Bose-Einstein condensate is a state of matter that occurs when atoms are cooled to near absolute zero and behave as a single superatom.
This chapter discusses the fundamental concepts of chemistry including the structure of atoms, phases of matter, physical and chemical properties and changes, elements and compounds. It explains that chemistry is the study of matter and its transformations, and covers topics such as the submicroscopic nature of atoms and molecules, the three phases of matter, and how to distinguish physical and chemical changes. It also provides guidelines for naming common chemical compounds using prefixes and suffixes based on the elements present.
This chapter discusses the fundamental concepts of chemistry including the structure of atoms, phases of matter, physical and chemical properties and changes, elements and compounds. It explains that chemistry is the study of matter and its transformations, and covers topics such as the submicroscopic nature of atoms and molecules, the three phases of matter, and how to distinguish physical and chemical changes. It also provides guidelines for naming common chemical compounds using prefixes and suffixes based on the elements present.
This chapter discusses the fundamental concepts of chemistry including the structure of atoms, phases of matter, physical and chemical properties and changes, elements and compounds. It explains that chemistry is the study of matter and its transformations, and covers topics such as the submicroscopic nature of atoms and molecules, the three phases of matter, and how to distinguish physical and chemical changes. The chapter also provides guidelines for naming compounds using prefixes and common names.
This document provides information on the structure and composition of matter. It discusses the basic units that make up all matter including atoms, elements, molecules, compounds, and mixtures. Atoms are made up of protons, neutrons, and electrons. Elements are composed of only one type of atom, while compounds contain at least two elements chemically bonded together. Chemical and physical properties depend on how atoms are arranged and bonded. The document also covers states of matter, chemical reactions, energy, and the role of catalysts like enzymes in biological reactions.
The document summarizes several atomic models proposed by scientists like Dalton, Rutherford, Bohr, Thompson, and Schrodinger. It also discusses physical properties and changes like density, melting/boiling points, and state changes. Chemical properties and changes involving combustion, corrosion, and neutralization are covered. Key physical processes like distillation, evaporation, filtration are explained. Electrolysis and uses are summarized as a chemical process, along with combustion and corrosion.
The document discusses the key concepts of elements, compounds, atoms, molecules, and ions. It defines elements as basic forms of matter that cannot be broken down further, while compounds are formed by chemical bonds between different elements. Atoms are the basic building blocks that make up elements and can combine to form molecules or ions. Molecules may contain atoms of the same or different elements, while ions are charged particles that form when atoms gain or lose electrons.
This document provides an overview of atomic theory and the laws of chemical combination. It discusses the early Greek philosophers' debates on the nature of matter and whether it is continuous or made of discrete particles. John Dalton developed the modern atomic theory in the early 19th century, which included five main points. The document outlines the contributions of scientists like Thomson, Rutherford, and Bohr to models of atomic structure. It describes the three states of matter and defines the fundamental laws of conservation of mass, definite proportions, and multiple proportions discovered by scientists like Lavoisier, Proust, and Dalton. Examples are provided to illustrate applications of these laws.
The document discusses the history of atomic theory from ancient Greek philosophers to modern scientists. It explains that Democritus first proposed the idea of atoms as indivisible pieces of matter. John Dalton further developed atomic theory in the 1700s, proposing that elements are made of unique atoms that combine in fixed ratios. J.J. Thomson, Ernest Rutherford, Niels Bohr, and James Chadwick contributed key discoveries about atomic structure through the early 1900s, such as identifying the electron and nucleus. The periodic table organizes elements based on their atomic structure and properties.
Chemistry
Chemistry is the branch of science that deals with the composition, structure and properties of matter.
Chemistry is also called the science of atoms and molecules.
Chemistry is the study of matter and the changes it undergoes.
Nursing
Nursing is a profession within the healthcare sector focused on the care of individuals, families and communities so they may attain, maintain or recover optimal health and quality of life.
Nurses may be differentiated from the other healthcare providers by their approach to patient care, training and scope of practice.
Chemistry in nursing is very important, as it sets the basis for understanding the medications that are being administered to certain patients
Nurses must understand how particular medicines will react in different patients. This helps to avoid wrong combinations of drugs that can lead to adverse effects.
Nursing programs feature different chemistry courses, including biochemistry, pharmacology, general level chemistry and organic chemistry. All of these courses play an important role in helping nurses understand different organic compounds, chemical equations, chemical reactions and chemical processes.
Therefore, chemistry knowledge allows nurses to understand the effects of different medicines when used alone or in combination with others.
The nurse must understand the present condition of the patient, importance and difference in sodium, potassium, chloride, bicarbonate, oxygen and many other elements and electrolytes in the body. This understanding will guide the nurse to identify if there is an electrolyte imbalance.
Thus, it is vital for nurses to have the skills to take care of their patients emotionally, but it is also important that the nurse have the necessary knowledge to interpret data regarding the patient condition to treat physically accurately and in a timely manner.
The term matter refers to anything that occupies space and has mass. All matter is made up of substances called elements, which have specific chemical and physical properties and cannot be broken down into other substances through ordinary chemical reactions.
There are two ways of classifying the matter:
(A) Physical Classification
Matter can exist in three physical states:
Solids
Liquids
Gases.
(B) Chemical classification
Based upon the composition, matter can be divided into two main types:
Pure Substances
Mixtures.
1. Solids
The solid state is one of the fundamental states of matter.
Solids differ from liquids and gases by the characteristic of rigidity.
The molecules of solids are tightly packed because of strong intermolecular forces; they only oscillate about their mean positions.
Whereas, liquids and gases possess the property of fluidity and can easily flow.
Solids can be defined as the state of matter which has definite shape and volume and has a rigid structure.
Solids possess the least compressibility and thermal expansion.Example: Iron (Fe)
2. Liquid
The molecules in a liquid are
This document provides an introduction to general chemistry concepts. It begins with defining chemistry and discussing its branches, including analytical chemistry, physical chemistry, organic chemistry, and inorganic chemistry. It then discusses the importance of chemistry for nurses, focusing on understanding drug composition and properties, diagnosis, disease mechanisms, and sterilization. The document also defines matter and the three states of matter - solid, liquid, and gas. It provides examples and descriptions of the properties and changes between each state. Finally, it classifies matter as either pure substances like elements and compounds, or impure substances like mixtures, and provides brief definitions of each.
chap 1 Chapter 1 chapter1 chapter1 chapter 1.pptxTaroTari
This document provides an overview of key concepts in medical physics related to electricity and magnetism. It discusses the structure of atoms including protons, neutrons, electrons and shells. It describes the four fundamental states of matter - solids, liquids, gases and plasma. It also covers types of elements like conductors and insulators. Additionally, it summarizes the three methods of heat transmission - conduction, convection and radiation. The document provides definitions and examples for many physics concepts applied in medical fields like ions, isotopes, isobars and the formation of ionic and covalent compounds.
1. The document outlines the history of atomic theory from Democritus to Bohr. It describes early atomic models proposed by Dalton, Thomson, and Rutherford and experiments that led to advances.
2. Rutherford's gold foil experiment showed that atoms have a small, dense nucleus containing most of their mass.
3. Bohr incorporated Rutherford's findings into his model where electrons orbit in fixed energy levels.
Similar to Unit b matter and chemical change notes (20)
The document provides instructions for a structural engineering challenge to build the tallest structure possible using 5 pieces of paper and masking tape within 10 minutes. It defines key structural concepts like strength, stability, and the three basic structural forms: solid/mass, frame, and shell structures. A sketch of the completed structure must be provided.
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hematic appreciation test is a psychological assessment tool used to measure an individual's appreciation and understanding of specific themes or topics. This test helps to evaluate an individual's ability to connect different ideas and concepts within a given theme, as well as their overall comprehension and interpretation skills. The results of the test can provide valuable insights into an individual's cognitive abilities, creativity, and critical thinking skills
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Abstract: Equivariant neural networks are neural networks that incorporate symmetries. The nonlinear activation functions in these networks result in interesting nonlinear equivariant maps between simple representations, and motivate the key player of this talk: piecewise linear representation theory.
Disclaimer: No one is perfect, so please mind that there might be mistakes and typos.
dtubbenhauer@gmail.com
Corrected slides: dtubbenhauer.com/talks.html
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Thematic analysis in qualitative research is a time-consuming and systematic task, typically done using teams. Team members must ground their activities on common understandings of the major concepts underlying the thematic analysis, and define criteria for its development. However, conceptual misunderstandings, equivocations, and lack of adherence to criteria are challenges to the quality and speed of this process. Given the distributed and uncertain nature of this process, we wondered if the tasks in thematic analysis could be supported by readily available artificial intelligence chatbots. Our early efforts point to potential benefits: not just saving time in the coding process but better adherence to criteria and grounding, by increasing triangulation between humans and artificial intelligence. This tutorial will provide a description and demonstration of the process we followed, as two academic researchers, to develop a custom ChatGPT to assist with qualitative coding in the thematic data analysis process of immersive learning accounts in a survey of the academic literature: QUAL-E Immersive Learning Thematic Analysis Helper. In the hands-on time, participants will try out QUAL-E and develop their ideas for their own qualitative coding ChatGPT. Participants that have the paid ChatGPT Plus subscription can create a draft of their assistants. The organizers will provide course materials and slide deck that participants will be able to utilize to continue development of their custom GPT. The paid subscription to ChatGPT Plus is not required to participate in this workshop, just for trying out personal GPTs during it.
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PPT on Direct Seeded Rice presented at the three-day 'Training and Validation Workshop on Modules of Climate Smart Agriculture (CSA) Technologies in South Asia' workshop on April 22, 2024.
2. What is matter?
• Matter: The stuff that makes up the universe that is
not energy
• Matter:
1. Has mass
2. Takes up space
3. The Particle Model of Matter
1. All matter is made of tiny particles
2. Particles are in constant motion
3. There are attractive & repulsive forces between particles
4. These are spaces between the particles
5. Difficult matter is made of different particles
7. Solid Liquid Gas
Motion of
Particles
Space between
particles
Behaviour in a
container
LOW LOW HIGH
Not affected
by the
container
Takes shape
of the
container
Fills the
container
8.
9. Changes Between States of Matter
Melting: Going from a solid to a liquid when heat is added
Boiling: Going from a liquid to a gas when heat is added
Condensation: Going from a gas to a liquid when heat is
removed
Freezing: Going from a liquid to a solid when heat is removed
Sublimation: Going from a solid to a gas when heat is added
Deposition: Going from a gas to a solid when heat is removed
12. Physical Properties
Physical Properties: a characteristic of matter that can be
observed and measured without changing the chemical
identity of the sample.
Note: It’s important to remember that when a substance
undergoes a physical change, such as melting, its
appearance or state may be altered, but its composition
stays the same.
13. Physical Properties:
• Melting Point
• Boiling Point
• Hardness
• Malleability
• Substance that can be rolled into a sheet
• Ductility
• Substance that can be stretched into a wire
• Crystal Shape
• Solubility
• Substance that can be dissolved into another
• Density
• Conductivity
• Ability to conduct electricity or heat
14.
15. Chemical Properties
Chemical Properties: a property or characteristic of a
substance that is observed during a reaction in which
the chemical composition or identity of the substance
is changed
Note: A chemical change always results in the
formation of a different substance or substances.
18. Classifying Matter
Pure Substance:
• is made of only one kind of matter
• has a unique set of properties that sets it apart from any other
kind of matter.
• (It is further classifies into an element or a compound)
Mixture:
• is a combination of pure substances not combined chemically
19. Pure Substances
Element (Example Na or Sodium/O or Oxygen):
• Matter than cannot be broken down into any simpler substance.
• The most purest matter because it contains only one kind of atom
• Represented by a symbol on the periodic table
Compounds (H20 or CO2) :
• A substance formed by 2 or more elements chemically fixed in
proportion (molecule).
20. Pure Substances
Compounds (H20 or CO2) :
• A substance formed by 2 or more elements chemically fixed in
proportion (molecule: atoms bonded together).
21. Mixtures
Mechanical Mixture (Heterogeneous):
• Some or all particles can be seen and be separated (Ex. Salad)
Solution (Homogeneous):
• Not separate visibly, as one is dissolved in another (Ex. coffee)
• A substance dissolved in water is called an aqueous solution
22. Mixtures
Suspension:
• Mixture where tiny particles of one substance are held within
another. Substances can be separated by centrifuging or
filtration. (Ex. Salad dressing)
Colloid:
• Cloudy mixture, where the
particles are suspended
and difficult to separate
(Ex. milk)
25. 1. How is an element different than a compound? Give an example of each.
2. What is the difference between a pure substance and a mixture?
3. How is a suspension different from a colloid?
4. Classify the following substances as an element, compound, or mixture:
a) Pop is composed of water, sugar, and carbon dioxide.
b) Graphite in a pencil is composed of carbon.
c) Carbon dioxide is composed of carbon and oxygen.
27. Physical Changes
Physical Change: When a substance undergoes a
physical change, its state may be altered, but its
chemical composition is the same
28.
29. Physical Changes
To identify a physical change:
• You can separate the end products (reactants) to
original substances. Ex. Salt water, sand & rocks
• You are able to re-freeze or melt the product again.
Ex. Ice cream
30. Chemical Changes
Chemical Change: When 2 or more substances react
and form 1 or more new substances (The new
substances formed are completely different from the
original reactants)
31.
32. Chemical Changes
Four actions that identify a chemical change:
1. Change in color
2. Change of odour (if present)…safety!!
3. Formation of a solid (precipitate) or a gas
4. Release or absorption of energy in the form of light & heat
35. 8000 BC
• Used stones & bone for tools
• Started to control Fire (cooking, baking)
36. 6000-1000 BC
• Found metals
• Gold became very valuable
• Chemists were only interested in materials of value
37. 4500 BC
• Copper was discovered and led to bronze
• Humans could now make hard strong tools (swords, spears &
other tools)
38. 1200 BC
• Hittites discovered how to extract iron from rocks
• This started the iron age (iron + copper = steel)
• Started to extract oils & juices from plants
39. 400 BC
• Greek philosopher (Democritus) used the word atomos to
describe the smallest particles that could not be broken down
any further
40. 350 BC
• Aristotle another more popular geek philosopher had the idea
that all matter came from Earth, Water, Fire and Air.
• Because Aristotle was more respected people accepted his
theory over Democritus' idea.
41. The Next 2000 Years
• Most work with matter was done by Alchemists, people who
were part chemist and part magician.
• Most of their job was working for the King to turn metals into
gold.
42. Late 1500
• People really started to investigate the world around them
• Started to form the scientific method.
43. 1660
• Robert Boyle experimented with the
behaviors of gases.
• He believed everything was made of tiny
particles of different size and shape.
• Boyle thought the purpose of chemistry
was to determine the types of particles in
each substance.
44. 1780
• Antoine Laurent Lavoisier "the father of
modern chemistry"
• Studied chemical interactions and
developed a system of naming them.
(everyone could use the same names)
45. 1808
• John Dalton suggested matter was made of
elements.
• Pure substances contained no other substances
(all one type of atom)
• Developed the billiard ball model (atoms are
solid spheres)
C
Cl
H
Fe
N
O
Na
46. 1897
• J. J. Thomson discovered electrons
• Developed a raisin bun model of matter.
• Negative electrons balance out positive sphere so atom has no
electrical charge.
47. 1904
• Hantaro Nagaoka modeled matter after the solar system
• Large positive center with negative electrons orbiting around
48. 1908
• Ernest Rutherford (working at McGill in
Montreal) found evidence of central
nucleus.
• In his experiment he shot positively
charge particles through thin foil and
found mostly empty space and
the nucleus was the core that would stop
the particles.
49. 1922
• Niels Bohr working with Rutherford found electrons orbit is
specific shells (circular orbits)
• Electrons jump between shells by gaining or losing energy
50. More 1922
• James Chadwick found protons & neutrons
(particles with no charge) inside the
nucleus of an atom.
51. Today
• People still use Bohr model of the atom
• Quantum mechanics found electrons exist
in a charged cloud around the nucleus.
53. Atom
• Proton: Part of an atom’s nucleus,
positive electric charge. Roughly
equal mass to neutrons.
• Neutron: Part of an atom’s nucleus,
no electric charge (Neutral).
Roughly equal mass to protons.
• Electron: Part of an atom, negative
electric charge
54. Size of an Atom
If an atomic nucleus was the size of a
pea, and that pea was inside a football
stadium... then a mosquito flying
around in the football stadium would
represent an electron and the football
stadium would represent the size of
the atom.
55. Early Organizing of the Elements
• Early chemists used symbols of the sun and planets to
represent seven metallic elements
• Early 1800’s more than 30 elements had been identified and as
chemistry developed even more were identified
• Chemists tried to group elements by properties but everyone
was using a different system and it was very confusing. They
needed a new system
57. Early Organizing of the Elements
• John Dalton developed a new set
of symbols in early 1800s
58. Early Organizing of the Elements
• Swedish chemist Jon Jacob Berzeliusin, 1814, suggested
using letters rather than pictures to represent the elements.
The first letter capitalized of an element would become the
symbol. A second smaller letter would be added for elements
that had the same first letter.
• H - Hydrogen, He - Helium
59. Early Organizing of the Elements
How did they put these elements into an order?
• Elements were organized in order of increasing
atomic mass. Atomic mass is the mass of one
atom of an element and is measured in an
atomic mass unit (amu). Scientists were able to
determine the average atomic mass unit of an
atom by comparing it to a carbon atom (12.0).
60. Early Organizing of the Elements
How did they put these elements into an order?
• 1864, English Chemist John Newlands recognized a pattern when
elements were listed by increasing atomic mass – they seemed to
repeat properties at regular intervals. He called this pattern “the law
of Octaves” as the pattern was similar to the octave scale on a piano.
Many scientists thought the idea was silly and refused to accept it.
61. Early Organizing of the Elements
Who found the pattern for the
elements?
• Dmitri Mendeleev collected
63 elements known to exist
in his time and used the
properties to organize them
into a pattern. He sorted
them using cards.
69. Groups/Families & Periods
Groups/Families: Vertical Columns – organized because of
their similar chemical behaviour, same number of electrons in
their outermost shell.
Periods: Horizontal Rows – same number of electron shells
71. Metals, Metalloids, Non-Metals
Metals: Shiny, Malleable, Ductile and conduct electricity
Non-Metals: Are dull, brittle and only carbon conducts
electricity
Metalloids: have properties of both metals and non-metals
76. Group 1 & 2 – Alkali/Alkaline-Earth Metals
Alkali Metals (Group 1): Most reactive metal (only need to lose
1 electron in their outer shell)
Alkaline-Earth Metals (Group 2): Also very reactive but not as
reactive as group 1 (Need to lose 2 electrons)
77. Color the 2nd Blank Periodic Table and
Label Categories
80. Group 17 & 18 – Halogens/Noble Gases
Halogens (Group 17): Most reactive, typically react with
metals (only need to gain 1 electron in their outer shell)
Noble Gases (Group 18): Odourless and colorless gasses,
essentially non reactive. (Complete outer shells)
97. Compounds
Compound: A chemical combination of two or more elements
in a specific ratio
Examples (Write One):
• Table Salt : NaCl (sodium chloride)
• Baking Soda : NaHCO3 (sodium bicarbonate)
• Water : H2O (dihydrogen oxide)
98. Compounds
Chemical Formula: Identifies the elements in the compound
and the number of each element.
Examples (Write One):
• Table Salt : NaCl (sodium chloride)
• Baking Soda : NaHCO3 (sodium bicarbonate)
• Water : H2O (dihydrogen oxide)
99. Compounds
Nomenclature: Naming system created by French chemist
Guyton de Morveau in 1787.
If you know the formula you can determine the name. If you
know the name you can determine the formula.
100. NaCl Salt
(sodium chloride)
1 atom Na
1 atom Cl
H2O Water
(dihydrogen oxide
)
2 atoms H
1 atom O
C6H12O6 Glucose 6 atoms C
12 atoms H
6 atoms O
H2SO4 Battery Acid
(sulfuric acid)
2 atoms H
1 atom S
4 atoms O
CH3COOH Vinegar
(acetic acid)
2 atoms C
4 atoms H
2 atoms O
101. Compounds
The Subscript (the small number behind some elements) tells you how
many of the element are in that compound.
After a chemical formula we can also have subscript letters in parentheses.
This lets us know the state of the compound.
(s) is a solid
(l) is a liquid
(g) is a gas
(aq) is an aqueous solution (a substance dissolved in water)
102.
103. Compounds
There are two different types of compounds depending on the types of
elements that make the compound.
They Are:
Ionic
Compounds
Molecular
Compounds
104. Ionic Compounds
Ionic Compounds: Contain at least one metal and one or more non-metal
Examples:
NaCl : Sodium chloride CuSO4 : Copper (II) Sulphate
105. Ionic Compounds
When a metal and non-metal combine they form IONIC bonds
In order to form a compound the metal loses electrons and becomes
positively charged.
The non-metal gains electrons and becomes negatively charged.
These charged elements are known as Ions.
107. Ionic Compounds
Magnesium chloride is an ionic compound.
Its chemical formula is MgCl2
That is 1 Mg and 2 Cl
Mg
-
-
-
-
- -
-
-
--
- -
The two outer electrons of the
metal are given to the chlorine
atoms, filling their
outer electron shell
108. Ionic Compounds
Properties of Ionic Compounds:
• High melting point
• Good conductivity
• Distinct crystal shape
• Solid at room temperature
Polyatomic ions - some atoms bond together and have an overall positive or
negative charge. these groups of atoms act as one.
110. Molecular Compounds
Molecular compounds form
COVALENT bonds
In order to form a compound
the non-metals must share
electrons in order to fill the
outer shell of each element.
111. Molecular Compounds
N
-
-
-
-
-
- -
Nitrogen trichloride is a
molecular compound. Its chemical
formula is NCl3
Each chlorine shares one electron
with the nitrogen. The
nitrogen shares 3 electrons, one
for each chlorine.
112. Molecular Compounds
Molecular Compounds:
• Solid, liquid or gas at room temperature
• Lower melting and boiling points because the covalent bond is weaker
than ionic bond
113. Practice
Identify the following chemicals as either ionic compounds or molecular
compounds
Sodium
Chloride
Ionic Magnesium
chloride
Ionic
H20 Molecular Tin(IV) oxide Ionic
SO2 Molecular Dinitrogen
pentaphosphide
Molecular
Nickel (II)
bromide
Ionic SiO2 Molecular
Carbon
monoxide
Molecular Mn2O7 Ionic
115. Naming Ionic Compounds
Step 1: Determine if the substance is a molecular or an ionic compound
Example: NaCl (Metal & Non-metal)
Step 2: Write the full name of the metal first
Na = Sodium
Step 3: Add the name of the non-metal second
Cl = chlorine
Step 4: Drop the ending of the non-metal, the “ine”, and change it to “ide”
chlorine chloride
NaCl = Sodium chloride
116. Naming Ionic Compounds
** Step 5. If the metal is not from group 1 or 2 (i.e.3-17) we may need to
determine and state the ionic charge of the metal.
For example SnO2.
There are 2 Oxygen atoms and 1 tin atom.
Each oxygen atom has a 2- charge (see common ion charges). That is 4-
charges in total.
There is only 1 tin atom and its charge must equal and
balance the negatives. The tin must have a 4+ charge, one of its common
ion charges (top right of the box).
117. Naming Ionic Compounds
For example SnO2.
Sn (charge +4) ----- O (charge -2)x2
Convert the ionic charge of the metal into a Roman
numerals number. (4 is IV)
Insert the Roman numeral between the metal and non
metal using brackets
Ex. Tin (IV) oxide
123. Naming Molecular Compounds
Step 1: Determine if the substance is a molecular or an ionic compound
Example: N2P5 (Non-metals)
Molecular compounds use Greek prefixes to tell us the number of each
atom. Copy the prefixes in your notes:
124. Naming Molecular Compounds
Example: N2P5 (Non-metals)
Step 2: Determine how many atoms of the first listed substance there are. (there
are 2 N’s)
Step 3: Attach the prefix for that number to the beginning of the elements name.
**If there is only one do not add a prefix to the first element.
Ex. 2=Di Dinitrogen
Step 4: Repeat step 2 and 3 for the second element.
** If there is only one atom use the prefix mono.
Ex. 5 = penta Dinitrogen pentaphosphorous
Step 5: Change the ending of the second element to and -ide ending.
Ex. Dinitrogen pentaphosphide
128. Creating Chemical Formulas
Example: Dicarbon tetrafluoride / Sodium Chloride
Step 1: Find the symbols for each
C F / Na Cl
Step 2: If the substance is molecular use the prefixes to tell you the
number of each atom.
Ex: C2F4
If the substance is ionic we must find the ion charges for each
atom.
Ex. Na +1 Cl -1
Step 3: Balance the charges so that there are the same number of
positives and negatives.
Ex. Only one of each is needed to balance Na and Cl
Sodium Chloride = NaCl
131. Naming with Polyatomic Ions
Sometimes when atoms group together, many atoms can work
as one.
Ex: SO4 -2
When this group of atoms act as a charged particle it is called
a polyatomic ion.
These polyatomic ions are only found in IONIC COMPOUNDS
132. Naming with Polyatomic Ions
Polyatomic ions have special rules for writing chemical formulas:
Step 1: Positive ions are written first negatives second (similar to
positive metals and negative non-metals)
Step 2: If more than one polyatomic ion is required to balance the
charges the entire ion is put in brackets.
Ex: Iron (III) Carbonate
Fe +3 CO3 -2 = Fe2(CO3)3
Note: the ending for polyatomic does not have an -ide ending. Each
are different