Chemical bonding 2 no bonds
•Download as PPTX, PDF•
1 like•782 views
Bonds form between elements when their molecules rearrange to become stable compounds. This requires energy and allows the outer electron levels of one element to reach eight electrons. There are three main types of bonds: ionic bonds between metals and nonmetals where electrons are transferred, covalent bonds between nonmetals where electrons are shared, and metallic bonds between metals. To identify bonds, locate the elements on the periodic table to determine if they are metals or nonmetals and then apply the appropriate bonding model.
Report
Share
Report
Share
Recommended
Atomic theory
This document provides an overview of the development of atomic theory from ancient Greek philosophers to modern atomic structure. It describes key contributors such as Democritus, Dalton, Thomson, Rutherford, Bohr, and Schrodinger who proposed models of the atom based on experiments and evidence available at the time. Their work established that atoms are the smallest particles of matter, have a small, dense nucleus surrounded by electrons, and can combine to form all chemical elements.
Atomic theory
Atomic theory has evolved over time as scientists have discovered more about the internal structure of atoms. Atoms are now understood to be the smallest particle of an element that retains the properties of that element. Atoms contain a nucleus of protons and neutrons surrounded by electrons. The number of protons determines the element, and atoms of the same element have the same number of protons but may vary in the number of neutrons forming different isotopes. Forces such as electromagnetic force hold the structure of the atom together.
Atomic theory
This document provides an overview of the development of atomic theory over time. It describes early Greek philosophers like Democritus who proposed the idea of atoms as indivisible particles. Later scientists like Dalton, Thomson, Rutherford, Bohr, Schrodinger and Heisenberg contributed improved atomic models including the plum pudding model, solar system model, and electron cloud model. The document outlines that atoms are composed of protons, neutrons, and electrons and that elements are defined by their atomic number of protons. Isotopes and forces within atoms are also summarized.
Periodic table
The periodic table organizes elements according to increasing atomic number and properties that repeat periodically. Elements are grouped based on their proton number and electron configuration which determine their bonding properties and how they form compounds. The location of an element on the periodic table can be used to predict its physical and chemical behavior.
Physical science 4.2 : The Atom
1) An atom is the smallest particle of an element and is approximately 0.00000003 cm in diameter.
2) Atoms are made up of a nucleus containing protons and neutrons, surrounded by electrons.
3) The number of protons determines the element, while the number of neutrons distinguishes between isotopes of that element.
Grade 9-U1-L10-History of atomic theory
This document provides a timeline of the development of atomic models from ancient Greek philosophers to present day. It describes early theories from Democritus and Aristotle that matter is made of indivisible particles. John Dalton later proposed atoms as indestructible, indivisible spheres that combine in simple ratios. J.J. Thomson's discovery of electrons led to the "plum pudding" model. Ernest Rutherford's gold foil experiment showed atoms are mostly empty space with a small, dense positively charged nucleus. Niels Bohr incorporated electrons orbiting the nucleus. James Chadwick's discovery of neutrons completed atomic structure.
Elements and Atoms
- Matter is made of atoms, which are the building blocks of all matter. Atoms contain protons, neutrons, and electrons. Protons and neutrons are located in the center nucleus, and electrons orbit the nucleus.
- Elements are the basic substances that atoms are made of. All elements are made up of the same parts - protons, neutrons, and electrons. The periodic table lists all known elements. It provides information like each element's symbol, atomic number, and atomic mass.
- There are two common models for representing atoms - the Bohr model, which shows all subatomic particles, and the Lewis dot structure, which shows only the outermost shell of electrons. These models can be used to
Atomic theory
This document outlines the development of atomic theory from ancient Greek philosophers to modern physics. It describes key contributors such as Democritus, Dalton, Thomson, Rutherford, Bohr, and Schrodinger who proposed models of the atom based on experiments. The modern atomic theory is that atoms contain a nucleus of protons and neutrons surrounded by electrons in electron clouds, and that elements are defined by their atomic number while isotopes differ in neutron number. The four fundamental forces that act on atoms are also summarized.
Recommended
Atomic theory
This document provides an overview of the development of atomic theory from ancient Greek philosophers to modern atomic structure. It describes key contributors such as Democritus, Dalton, Thomson, Rutherford, Bohr, and Schrodinger who proposed models of the atom based on experiments and evidence available at the time. Their work established that atoms are the smallest particles of matter, have a small, dense nucleus surrounded by electrons, and can combine to form all chemical elements.
Atomic theory
Atomic theory has evolved over time as scientists have discovered more about the internal structure of atoms. Atoms are now understood to be the smallest particle of an element that retains the properties of that element. Atoms contain a nucleus of protons and neutrons surrounded by electrons. The number of protons determines the element, and atoms of the same element have the same number of protons but may vary in the number of neutrons forming different isotopes. Forces such as electromagnetic force hold the structure of the atom together.
Atomic theory
This document provides an overview of the development of atomic theory over time. It describes early Greek philosophers like Democritus who proposed the idea of atoms as indivisible particles. Later scientists like Dalton, Thomson, Rutherford, Bohr, Schrodinger and Heisenberg contributed improved atomic models including the plum pudding model, solar system model, and electron cloud model. The document outlines that atoms are composed of protons, neutrons, and electrons and that elements are defined by their atomic number of protons. Isotopes and forces within atoms are also summarized.
Periodic table
The periodic table organizes elements according to increasing atomic number and properties that repeat periodically. Elements are grouped based on their proton number and electron configuration which determine their bonding properties and how they form compounds. The location of an element on the periodic table can be used to predict its physical and chemical behavior.
Physical science 4.2 : The Atom
1) An atom is the smallest particle of an element and is approximately 0.00000003 cm in diameter.
2) Atoms are made up of a nucleus containing protons and neutrons, surrounded by electrons.
3) The number of protons determines the element, while the number of neutrons distinguishes between isotopes of that element.
Grade 9-U1-L10-History of atomic theory
This document provides a timeline of the development of atomic models from ancient Greek philosophers to present day. It describes early theories from Democritus and Aristotle that matter is made of indivisible particles. John Dalton later proposed atoms as indestructible, indivisible spheres that combine in simple ratios. J.J. Thomson's discovery of electrons led to the "plum pudding" model. Ernest Rutherford's gold foil experiment showed atoms are mostly empty space with a small, dense positively charged nucleus. Niels Bohr incorporated electrons orbiting the nucleus. James Chadwick's discovery of neutrons completed atomic structure.
Elements and Atoms
- Matter is made of atoms, which are the building blocks of all matter. Atoms contain protons, neutrons, and electrons. Protons and neutrons are located in the center nucleus, and electrons orbit the nucleus.
- Elements are the basic substances that atoms are made of. All elements are made up of the same parts - protons, neutrons, and electrons. The periodic table lists all known elements. It provides information like each element's symbol, atomic number, and atomic mass.
- There are two common models for representing atoms - the Bohr model, which shows all subatomic particles, and the Lewis dot structure, which shows only the outermost shell of electrons. These models can be used to
Atomic theory
This document outlines the development of atomic theory from ancient Greek philosophers to modern physics. It describes key contributors such as Democritus, Dalton, Thomson, Rutherford, Bohr, and Schrodinger who proposed models of the atom based on experiments. The modern atomic theory is that atoms contain a nucleus of protons and neutrons surrounded by electrons in electron clouds, and that elements are defined by their atomic number while isotopes differ in neutron number. The four fundamental forces that act on atoms are also summarized.
Periodic table shortened (1)
The periodic table organizes the chemical elements by atomic number and shows that elements with similar atomic structures tend to have similar chemical properties; elements are classified as metals, metalloids and nonmetals according to their properties, and the table illustrates how elements gain or lose electrons to achieve stable electron configurations through periodic trends in atomic structure across periods and down groups. The periodic table provides a framework for understanding relationships between elements and predicting properties based on atomic structure.
Atoms, Molecules, And Matter
An atom is the smallest particle of an element that contains protons, neutrons, and electrons. Elements are substances made of a single type of atom that combine to form molecules, which are made of two or more atoms joined together. Molecules such as water, written as H2O with two hydrogen atoms and one oxygen atom, are the smallest particles that combine without chemical change to form all matter in the world.
Atoms
Matter is composed of basic building blocks called atoms. Atoms were originally thought to be indivisible spheres, but are now understood to have internal structure. Atoms contain a tiny, dense nucleus of protons and neutrons surrounded by electrons. The number of protons determines the element, while neutrons and electrons can vary between atoms of the same element. Most atoms are electrically neutral, but can become ions by gaining or losing electrons.
Atoms and molecules
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.
Atoms, Ions and Molecules
This document discusses atoms, ions, and molecules. It defines atoms as the smallest particle of an element that cannot be broken down further. Atoms are made up of protons, neutrons, and electrons. Ions are formed when atoms gain or lose electrons, giving them a positive or negative charge. The document also defines molecules as two or more atoms chemically bonded together, and can be made of the same or different elements. Chemical formulas indicate the types of elements and number of each atom in a substance.
structure of the atom
This document provides information about the structure of the atom. It discusses the three main subatomic particles - electrons, protons, and neutrons. It describes the discoveries of these particles by scientists like Thomson, Goldstein, and Chadwick. The document then explains four major atomic models - Thomson's model, Rutherford's model, Bohr's model, and the distribution of electrons in shells. It also discusses concepts like atomic number, mass number, isotopes, isobars, and valency.
Atoms and Molecules, Ions, Isobars, Isotops etc... Chemistry PPT
Atoms and molecules, atoms, molecules, ions, isobars, isotops, Ionic Bonding, Covalent Bonding, polarity, Molecules bond componds,
Chemistry PPT
Intro to atoms
This document provides information about atoms including:
- Atoms are the smallest particle into which an element can be divided and still be the same substance.
- Atoms are made up of protons, neutrons, and electrons, with protons and neutrons in the nucleus and electrons orbiting around it.
- The number of protons determines the identity of an element.
- Various exercises and questions are provided to help teach and test understanding of atomic structure and terminology.
Atoms
The document discusses the basic building blocks of matter at the atomic level. It explains that atoms are made up of protons, neutrons, and electrons. Protons are positively charged and found in the atom's nucleus along with neutrons, which have no charge. Electrons are negatively charged and orbit the nucleus. It provides examples of hydrogen, oxygen, and sodium atoms, showing their proton, neutron, and electron composition. The atomic number is the number of protons, while the mass number includes protons and neutrons. Atoms can gain or lose electrons to become ions that are electrically charged.
Atomic theory 2014
This document outlines the development of atomic theory from Democritus' idea of indivisible atoms to modern atomic structure. It describes key contributors such as Dalton who proposed atoms as fundamental units of matter, Thomson who discovered the electron, and Rutherford whose gold foil experiment showed atoms have a small, dense nucleus. Later scientists such as Bohr, de Broglie, Schrödinger, Chadwick, and Curie further refined atomic models through discoveries like isotopes, wave-particle duality, and subatomic particles like neutrons. Their work disproved early ideas of atoms as indivisible and showed matter is made of even smaller constituents that can change form through radioactivity.
Atoms & molecule & its structure
This document provides information about the structure and composition of atoms. It discusses the discovery of subatomic particles like electrons, protons and neutrons through the models of Thomson and Rutherford. It explains that atoms are very small, around 10-10 meters, and describes the shells and number of electrons in the K, L, M and N shells. Tables listing common elements and their symbols are included. The document also defines molecules as groups of atoms bonded together, and provides examples of monoatomic and diatomic molecules like hydrogen, oxygen and ozone. It introduces the concept of ions as charged particles in compounds.
History of Atomic Structure
Democritus first proposed the idea of atoms in 400 BC, stating that all matter is composed of tiny indivisible particles called atoms that differ in size and shape. John Dalton later elaborated on this theory in the 1800s, postulating that atoms of different elements have unique properties and can combine to form compounds. J.J. Thomson's discovery of the electron in the late 1800s led to the plum pudding model of the atom. However, Ernest Rutherford's gold foil experiment in the early 1900s revealed that atoms are mostly empty space with a tiny, dense nucleus at the center, containing positive charge. Niels Bohr then incorporated Rutherford's findings into his 1913 model of the atom, proposing that electrons
atoms
This document provides an overview of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons. Protons have a positive charge, electrons have a negative charge, and neutrons have no charge. The number of protons determines the element, and the number of neutrons contributes to the mass number. The document also discusses the periodic table and how it can be used to find information about elements such as the number of protons, neutrons, and electrons. It includes some example calculations and provides additional online resources for learning more about atomic structure.
Science 8.1.1
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.
History of atomic theory
Early philosophers proposed that all matter was made of tiny indivisible particles called atoms. John Dalton later proposed the first atomic theory with evidence, stating that atoms are uniform spheres that make up elements. J.J. Thomson's experiments discovered the electron, showing atoms contain negatively charged particles. Rutherford's experiments demonstrated that atoms have small, dense positively charged nuclei surrounded by empty space occupied by electrons. This led to the modern understanding of atomic structure with protons, neutrons, and electrons.
Structure of Atom
This lesson plan outlines a science class on the atomic structure. It includes general and specific objectives of the lesson, a knowledge pre-test, and an outline of the presentation. The presentation will discuss early atomic models proposed by Thomson and Rutherford, and the drawbacks of Rutherford's model. It will then explain Niels Bohr's model of the atom, including his postulates that electrons orbit in discrete energy levels and absorb or emit energy in quantized amounts when changing orbits. Students will learn about the distribution of electrons in shells and orbits in atoms.
Atomic structure demo 02
The document discusses the structure of atoms. It introduces subatomic particles like protons, neutrons, and electrons. It explains that atoms are composed of these particles, with protons and neutrons located in the nucleus at the center, and electrons surrounding the nucleus. The number of protons determines the element, while the total of protons and neutrons is the mass number. The document provides examples of atomic numbers and mass numbers for different elements.
3. the material world, atoms
All matter is made up of atoms, which are composed of subatomic particles including electrons, protons, and neutrons. Atoms are mostly empty space with a dense nucleus at the center containing protons and neutrons. Electrons orbit the nucleus in shells or orbitals. Atoms can form ions by gaining or losing electrons, becoming positively or negatively charged. Multiple atoms can bond together to form molecules or crystalline solids, and compounds are made of different types of atoms chemically bonded together.
Atoms, elements and compounds academy
Atoms are the basic unit of matter and are composed of protons, neutrons, and electrons. Elements are pure substances made of one type of atom, while isotopes are different forms of the same element that vary in the number of neutrons. Compounds are formed when two or more elements chemically combine in fixed proportions and have different properties than their constituent elements.
Atoms
What is matter made of?
What are the building blocks of our universe?
Read this presentation to learn more.
Ps1 chapter 1
This chapter discusses physical science and the scientific method. Physical science involves the study of matter and energy, including chemistry which examines all forms of matter and physics which analyzes how energy affects matter. The scientific method involves asking a question, forming a hypothesis, testing the hypothesis through experimentation, analyzing results, drawing a conclusion, and communicating findings. Key terms defined include the independent and dependent variables, control groups, and different types of models used to represent scientific concepts. Laws summarize experimental evidence while theories provide explanations for observed phenomena.
Heat
The document discusses key concepts relating to temperature and heat transfer. It defines temperature as a measure of the average kinetic energy of particles in an object. As temperature increases, particles move faster, spreading out through thermal expansion. Different temperature scales are presented, with Fahrenheit and Celsius defined by their freezing and boiling points and Kelvin having absolute zero as its lowest value. Heat transfers between objects with different temperatures in order to equalize thermal energy, which is the kinetic energy of particles. Materials are classified as conductors or insulators based on their ability to transfer thermal energy through conduction, convection, or radiation.
More Related Content
What's hot
Periodic table shortened (1)
The periodic table organizes the chemical elements by atomic number and shows that elements with similar atomic structures tend to have similar chemical properties; elements are classified as metals, metalloids and nonmetals according to their properties, and the table illustrates how elements gain or lose electrons to achieve stable electron configurations through periodic trends in atomic structure across periods and down groups. The periodic table provides a framework for understanding relationships between elements and predicting properties based on atomic structure.
Atoms, Molecules, And Matter
An atom is the smallest particle of an element that contains protons, neutrons, and electrons. Elements are substances made of a single type of atom that combine to form molecules, which are made of two or more atoms joined together. Molecules such as water, written as H2O with two hydrogen atoms and one oxygen atom, are the smallest particles that combine without chemical change to form all matter in the world.
Atoms
Matter is composed of basic building blocks called atoms. Atoms were originally thought to be indivisible spheres, but are now understood to have internal structure. Atoms contain a tiny, dense nucleus of protons and neutrons surrounded by electrons. The number of protons determines the element, while neutrons and electrons can vary between atoms of the same element. Most atoms are electrically neutral, but can become ions by gaining or losing electrons.
Atoms and molecules
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.
Atoms, Ions and Molecules
This document discusses atoms, ions, and molecules. It defines atoms as the smallest particle of an element that cannot be broken down further. Atoms are made up of protons, neutrons, and electrons. Ions are formed when atoms gain or lose electrons, giving them a positive or negative charge. The document also defines molecules as two or more atoms chemically bonded together, and can be made of the same or different elements. Chemical formulas indicate the types of elements and number of each atom in a substance.
structure of the atom
This document provides information about the structure of the atom. It discusses the three main subatomic particles - electrons, protons, and neutrons. It describes the discoveries of these particles by scientists like Thomson, Goldstein, and Chadwick. The document then explains four major atomic models - Thomson's model, Rutherford's model, Bohr's model, and the distribution of electrons in shells. It also discusses concepts like atomic number, mass number, isotopes, isobars, and valency.
Atoms and Molecules, Ions, Isobars, Isotops etc... Chemistry PPT
Atoms and molecules, atoms, molecules, ions, isobars, isotops, Ionic Bonding, Covalent Bonding, polarity, Molecules bond componds,
Chemistry PPT
Intro to atoms
This document provides information about atoms including:
- Atoms are the smallest particle into which an element can be divided and still be the same substance.
- Atoms are made up of protons, neutrons, and electrons, with protons and neutrons in the nucleus and electrons orbiting around it.
- The number of protons determines the identity of an element.
- Various exercises and questions are provided to help teach and test understanding of atomic structure and terminology.
Atoms
The document discusses the basic building blocks of matter at the atomic level. It explains that atoms are made up of protons, neutrons, and electrons. Protons are positively charged and found in the atom's nucleus along with neutrons, which have no charge. Electrons are negatively charged and orbit the nucleus. It provides examples of hydrogen, oxygen, and sodium atoms, showing their proton, neutron, and electron composition. The atomic number is the number of protons, while the mass number includes protons and neutrons. Atoms can gain or lose electrons to become ions that are electrically charged.
Atomic theory 2014
This document outlines the development of atomic theory from Democritus' idea of indivisible atoms to modern atomic structure. It describes key contributors such as Dalton who proposed atoms as fundamental units of matter, Thomson who discovered the electron, and Rutherford whose gold foil experiment showed atoms have a small, dense nucleus. Later scientists such as Bohr, de Broglie, Schrödinger, Chadwick, and Curie further refined atomic models through discoveries like isotopes, wave-particle duality, and subatomic particles like neutrons. Their work disproved early ideas of atoms as indivisible and showed matter is made of even smaller constituents that can change form through radioactivity.
Atoms & molecule & its structure
This document provides information about the structure and composition of atoms. It discusses the discovery of subatomic particles like electrons, protons and neutrons through the models of Thomson and Rutherford. It explains that atoms are very small, around 10-10 meters, and describes the shells and number of electrons in the K, L, M and N shells. Tables listing common elements and their symbols are included. The document also defines molecules as groups of atoms bonded together, and provides examples of monoatomic and diatomic molecules like hydrogen, oxygen and ozone. It introduces the concept of ions as charged particles in compounds.
History of Atomic Structure
Democritus first proposed the idea of atoms in 400 BC, stating that all matter is composed of tiny indivisible particles called atoms that differ in size and shape. John Dalton later elaborated on this theory in the 1800s, postulating that atoms of different elements have unique properties and can combine to form compounds. J.J. Thomson's discovery of the electron in the late 1800s led to the plum pudding model of the atom. However, Ernest Rutherford's gold foil experiment in the early 1900s revealed that atoms are mostly empty space with a tiny, dense nucleus at the center, containing positive charge. Niels Bohr then incorporated Rutherford's findings into his 1913 model of the atom, proposing that electrons
atoms
This document provides an overview of atoms and their subatomic particles. It explains that atoms are made up of protons, neutrons, and electrons. Protons have a positive charge, electrons have a negative charge, and neutrons have no charge. The number of protons determines the element, and the number of neutrons contributes to the mass number. The document also discusses the periodic table and how it can be used to find information about elements such as the number of protons, neutrons, and electrons. It includes some example calculations and provides additional online resources for learning more about atomic structure.
Science 8.1.1
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.
History of atomic theory
Early philosophers proposed that all matter was made of tiny indivisible particles called atoms. John Dalton later proposed the first atomic theory with evidence, stating that atoms are uniform spheres that make up elements. J.J. Thomson's experiments discovered the electron, showing atoms contain negatively charged particles. Rutherford's experiments demonstrated that atoms have small, dense positively charged nuclei surrounded by empty space occupied by electrons. This led to the modern understanding of atomic structure with protons, neutrons, and electrons.
Structure of Atom
This lesson plan outlines a science class on the atomic structure. It includes general and specific objectives of the lesson, a knowledge pre-test, and an outline of the presentation. The presentation will discuss early atomic models proposed by Thomson and Rutherford, and the drawbacks of Rutherford's model. It will then explain Niels Bohr's model of the atom, including his postulates that electrons orbit in discrete energy levels and absorb or emit energy in quantized amounts when changing orbits. Students will learn about the distribution of electrons in shells and orbits in atoms.
Atomic structure demo 02
The document discusses the structure of atoms. It introduces subatomic particles like protons, neutrons, and electrons. It explains that atoms are composed of these particles, with protons and neutrons located in the nucleus at the center, and electrons surrounding the nucleus. The number of protons determines the element, while the total of protons and neutrons is the mass number. The document provides examples of atomic numbers and mass numbers for different elements.
3. the material world, atoms
All matter is made up of atoms, which are composed of subatomic particles including electrons, protons, and neutrons. Atoms are mostly empty space with a dense nucleus at the center containing protons and neutrons. Electrons orbit the nucleus in shells or orbitals. Atoms can form ions by gaining or losing electrons, becoming positively or negatively charged. Multiple atoms can bond together to form molecules or crystalline solids, and compounds are made of different types of atoms chemically bonded together.
Atoms, elements and compounds academy
Atoms are the basic unit of matter and are composed of protons, neutrons, and electrons. Elements are pure substances made of one type of atom, while isotopes are different forms of the same element that vary in the number of neutrons. Compounds are formed when two or more elements chemically combine in fixed proportions and have different properties than their constituent elements.
Atoms
What is matter made of?
What are the building blocks of our universe?
Read this presentation to learn more.
What's hot (20)
Atoms and Molecules, Ions, Isobars, Isotops etc... Chemistry PPT
Atoms and Molecules, Ions, Isobars, Isotops etc... Chemistry PPT
Viewers also liked
Ps1 chapter 1
This chapter discusses physical science and the scientific method. Physical science involves the study of matter and energy, including chemistry which examines all forms of matter and physics which analyzes how energy affects matter. The scientific method involves asking a question, forming a hypothesis, testing the hypothesis through experimentation, analyzing results, drawing a conclusion, and communicating findings. Key terms defined include the independent and dependent variables, control groups, and different types of models used to represent scientific concepts. Laws summarize experimental evidence while theories provide explanations for observed phenomena.
Heat
The document discusses key concepts relating to temperature and heat transfer. It defines temperature as a measure of the average kinetic energy of particles in an object. As temperature increases, particles move faster, spreading out through thermal expansion. Different temperature scales are presented, with Fahrenheit and Celsius defined by their freezing and boiling points and Kelvin having absolute zero as its lowest value. Heat transfers between objects with different temperatures in order to equalize thermal energy, which is the kinetic energy of particles. Materials are classified as conductors or insulators based on their ability to transfer thermal energy through conduction, convection, or radiation.
Equipment 2016
The document lists various pieces of scientific equipment commonly found in a laboratory including beakers, erlenmeyer flasks, stir rods, graduated cylinders, microscopes, bunsen burners, weigh papers, rulers, test tubes, funnels, pipettes, filter paper, scales, scissors, probes, forceps, dissecting trays, pins, and scalpels.
Periodic table shortened
The periodic table organizes elements according to their atomic structure. Dmitri Mendeleev organized the first periodic table by atomic mass, which allowed him to predict undiscovered elements. Henry Moseley later determined that atomic number provided an even more logical ordering. Most elements are metals and are found on the left side of the periodic table, while nonmetals are on the right. Elements in the same column have similar properties due to their valence electron configuration. The periodic table provides a wealth of information about each element and illustrates patterns in their chemical and physical properties.
Acids and bases
Acids contain hydrogen and produce hydronium ions in water. They have a sour taste, are corrosive, and react with metals. Common acids include hydrochloric acid and sulfuric acid. Acids are used to make paper, paint, detergents, and fertilizer. Bases contain hydroxide ions and have a bitter taste and slippery feel. They are also corrosive and conduct electricity. Common bases are used to make soap, cleaners, and antacids. Strong acids and bases fully dissociate in water, producing more hydrogen or hydroxide ions, while weak acids and bases only partially dissociate. A neutralization reaction between an acid and base produces a salt and water
Chap 2 sec 1
Matter occupies space and has mass. Volume is the amount of space an object occupies. Mass is the amount of matter in an object and remains constant anywhere, while weight depends on gravitational force and location. Mass is measured in grams using a balance, while weight is measured in Newtons using a spring scale. Mass is a measure of an object's inertia, or resistance to changes in motion. The more mass an object has, the harder it is to start or stop its motion according to Newton's First Law of Motion.
Chap 2 chem & phy properties
This document discusses the differences between physical and chemical properties of matter. Physical properties can be observed or measured without changing the identity of the substance, such as boiling point, density, state, and color. Physical changes alter the substance's form but not its composition, like melting, freezing, or bending. Chemical properties describe a substance's ability to undergo chemical reactions, for example flammability or reactivity. Chemical changes result in one or more new substances forming through chemical reactions. The identity of the original substance is changed in a chemical change.
Tools and measurement
This document discusses tools and units for measuring various physical properties including volume, mass, length, force, temperature, time, area, and volume. It lists common tools used to measure each property and their standard metric units. The document also introduces the International System of Units (SI) as the global standard for measurement and explains that density is calculated by dividing an object's mass by its volume rather than being directly measured.
States of matter
This document discusses the different states of matter and the changes between states. It explains that solids have a definite shape and volume due to the tight packing and vibration of particles. Liquids can change shape but not volume as their particles can slide past one another. Gases expand to fill their containers as their particles are far apart and move independently. Changes between solid, liquid and gas require the addition or removal of energy. The document provides examples of different states and phase changes.
Mixtures, solutions, elements, compounds
This document defines and provides examples of mixtures, solutions, suspensions, colloids, and gas mixtures. It explains that mixtures can be physically separated into their original substances, while solutions appear homogeneous. Suspensions can settle out but colloids cannot. It also defines elements as pure substances that cannot be broken down further, and compounds as pure substances formed by a chemical combination of elements in fixed ratios that have unique properties.
Chemical reactions
This document discusses key concepts in chemistry including types of chemical reactions such as single displacement, synthesis, decomposition, and double displacement reactions. It also covers important laws like the law of conservation of energy and mass. Exothermic and endothermic reactions are defined as well as activation energy, catalysts, and inhibitors. The key components of a balanced chemical equation like reactants and products are outlined. Finally, the six steps for balancing chemical equations are provided.
Energy 2 without alternatives
Energy can exist in various forms and can be transferred from one form to another but not created or destroyed. There are nine main types of energy: kinetic, potential, mechanical, thermal, chemical, electrical, sound, light, and nuclear. Energy transfers allow important functions like photosynthesis, cellular respiration, and power generation. Chemical energy is a common form of stored potential energy that can be released to do work.
Electricity
Electricity is the movement of electric charge. Electric charge can be positive or negative, and like charges repel while opposite charges attract. The amount of charge and distance between charges determine the electric force. An electric field exists around charged objects, and objects become charged through friction, conduction, or induction. Electricity can be used to power circuits consisting of a source, wires, and a load to convert the energy into other forms. Circuit failures are prevented by fuses and circuit breakers.
Speed, time, distance
This document defines key concepts related to motion, including speed, velocity, acceleration, force, friction, gravity, and mass. It explains that speed is distance divided by time, velocity includes both speed and direction, and acceleration is the rate of change of velocity. Forces can be added or subtracted depending on their direction. Net force determines if motion occurs, with balanced forces resulting in no motion. Gravity is the force of attraction between objects due to their mass, and increases with mass but decreases with distance. Weight is the measure of gravitational force on an object and depends on its location and mass.
Work, power and machines with pitucres
The document defines work as energy transferred by a force causing movement, with the formula W=Fxd. Power is the rate of work over time, with the formula P=W/t. Machines make work easier by changing the amount or direction of force, classified as simple machines like levers, pulleys, wheels and axles, inclined planes, wedges, screws, or compound machines combining simple machines. Mechanical advantage is the number of times a machine multiplies force, while efficiency is the ratio of work output to input accounting for energy lost to friction.
Force, mass, acceleration
This document discusses key concepts relating to gravity, motion, and Newton's laws of motion:
- Galileo determined that the rate at which objects fall is not dependent on their mass, and acceleration depends on force and mass.
- All objects accelerate towards Earth at 9.8 m/s^2 due to gravity. Newton's second law relates force, mass, and acceleration.
- Newton's three laws of motion are: 1) an object remains in motion unless acted on by an external force, 2) acceleration depends on net force and mass, and 3) for every action there is an equal and opposite reaction.
Waves and light without star stuff
This document discusses different types of waves including mechanical waves that require a medium and electromagnetic waves that can travel through empty space. It describes properties of waves like amplitude, wavelength, frequency, and speed. Key behaviors of waves are also outlined such as reflection, refraction, diffraction, interference, and absorption. The document provides details about electromagnetic waves, sound waves, and how lenses and mirrors interact with light waves.
Heat
This document discusses key concepts relating to temperature and heat transfer. It defines temperature as a measure of the average kinetic energy of particles in an object. As temperature increases, particles move faster, spreading out through thermal expansion. Different temperature scales are presented, with Fahrenheit and Celsius defined by their freezing and boiling points of water, and Kelvin having the lowest possible temperature of absolute zero. Heat is defined as the transfer of thermal energy between objects with different temperatures, while thermal energy is the kinetic energy within an object. Materials are classified as conductors or insulators based on their ability to transfer heat. The three main methods of heat transfer are conduction (direct contact), convection (movement of molecules in gases and liquids), and radiation (
Atomic theory
This document outlines the development of atomic theory from ancient Greek philosophers to modern physics. It describes key contributors such as Democritus, Dalton, Thomson, Rutherford, Bohr, and Schrodinger who proposed models of the atom based on experiments. The modern atomic theory is that atoms are composed of a nucleus of protons and neutrons surrounded by electrons in electron clouds, and that elements are distinguished by their atomic number. Isotopes are variants of the same element that differ in neutron number. Forces like electromagnetic, strong, and weak govern atomic structure.
Speed, time, distance
This document defines key concepts related to motion, including speed, velocity, acceleration, force, friction, gravity, and mass. It explains that speed is distance divided by time, velocity includes both speed and direction, and acceleration is the rate of change of velocity. Forces such as gravity and friction can cause or oppose motion depending on whether they are balanced or unbalanced. The law of universal gravitation describes how gravitational force is related to mass and distance. Formulas for calculating speed, distance, and time are also provided.
Viewers also liked (20)
More from tracyconover
Endocrine and reproduction modified
The endocrine system produces hormones that control body functions and are released by glands. The major glands include the pituitary, thyroid, parathyroid, adrenals, pancreas, ovaries, and testes. Hormones travel through the bloodstream and bind to receptors on cells to regulate processes like metabolism, immune function, reproduction, and stress response. Endocrine disorders occur when hormone levels are too high or too low, leading to conditions such as diabetes, thyroid disorders, and reproductive issues.
Circulatory and lymphatic, respiratory
The circulatory, lymphatic, and respiratory systems work together to transport nutrients, gases, and waste throughout the body. The cardiovascular system uses the heart, blood vessels and blood to carry oxygen and nutrients to cells and remove waste. Blood contains plasma, red blood cells, white blood cells and platelets. The lymphatic system returns fluids leaked from tissues to the bloodstream and fights pathogens using lymph nodes and vessels. The respiratory system takes in oxygen through the nose, pharynx, larynx, trachea, bronchi and lungs where gas exchange occurs in alveoli, then expels carbon dioxide.
Digestion and urinary
The tentative schedule outlines that the class will cover the digestive/circulatory systems from 3-12 to 3-16, the circulatory/respiratory and lymphatic systems from 3-19 to 3-23, and the reproductive/endocrine systems from 3-26 to 4-10. A pig dissection will take place around 4-11 and last until 4-27.
The digestive system breaks down food into nutrients that can be absorbed and used by the body. It consists of the mouth, esophagus, stomach, small intestine, large intestine, and anus. Both mechanical and chemical digestion occur through the actions of teeth/muscles and enzymes. The liver, gallbladder, and pancre
Skeletal, skin, muscle. nervous ppt
The document describes several key body systems including the skeletal, muscular, integumentary, and nervous systems. It explains that cells combine to form tissues, tissues combine to form organs, and organs work together in organ systems to carry out important body functions. The skeletal system provides structure and support, while storing minerals. The muscular system allows for movement via muscles connecting to bones. The integumentary system acts as a protective barrier for the body with the skin, hair, and nails. Lastly, the nervous system collects and processes information as the command center of the body using electrical signals transmitted through the brain and nerves.
Invertebrates
This document summarizes key characteristics of invertebrate animals. It describes their structures and functions including systems for digestion, respiration, circulation, excretion, response, movement, and reproduction. Specific phyla are examined in more detail, including worms, mollusks, arthropods, and echinoderms. Evolutionary trends are discussed such as the development of specialized cells/tissues, body symmetry, cephalization, segmentation, and a coelom.
Invertebrates modified 1 10-18
This document discusses the structure and function of various invertebrate phyla including annelids, mollusks, and insects. It outlines key characteristics like segmented bodies in annelids, soft bodies with shells in mollusks, and three-part bodies in insects. The document also covers evolutionary trends in early invertebrates from soft bodied to forms with shells and skeletons. Additionally, it describes trends in digestion, respiration, circulation, excretion, response, movement, reproduction, and skeletal systems across invertebrate groups.
Mitosis and meiosis
Cells divide through the process of cell division in order to replicate DNA and distribute it equally between daughter cells. Cell division involves mitosis, where the nucleus divides, and cytokinesis, where the cytoplasm divides. Mitosis consists of prophase, metaphase, anaphase, and telophase where chromosomes replicate and separate. Cytokinesis then divides the cell into two identical daughter cells each with a full set of chromosomes. Meiosis produces gametes through two rounds of division resulting in four haploid cells with half the number of chromosomes. This ensures genetic variation in sexual reproduction.
Mitosis and meiosis
Cells divide through the process of cell division in order to replicate DNA and distribute it equally between daughter cells. Cell division involves mitosis, where the nucleus divides, and cytokinesis, where the cytoplasm divides. Mitosis consists of prophase, metaphase, anaphase, and telophase where chromosomes replicate and separate. Cytokinesis then divides the cell into two identical daughter cells each with a full set of chromosomes. Meiosis produces gametes through two rounds of division resulting in four haploid cells with half the number of chromosomes. This ensures genetic variation in sexual reproduction.
Genetics
Gregor Mendel studied traits in pea plants such as color and height. He found that traits are controlled by alleles - dominant alleles will be expressed over recessive alleles in the first generation. Through subsequent generations and self-pollination, he discovered that recessive traits can be expressed according to his laws of inheritance and principles of dominance and segregation. Mendel's experiments laid the foundations for modern genetics.
DNA and RNA
This document discusses the history and key discoveries related to DNA and genetics. It covers:
- Griffith and Avery's early experiments showing DNA carries genetic information between generations
- Watson and Crick developing the double helix model of DNA structure
- DNA replication following Chargaff's rules of base pairing between A=T and G=C
- RNA and protein synthesis through transcription and translation of DNA into mRNA and proteins
- Types of mutations like point mutations, chromosomal mutations, and their harmful or beneficial effects
Cells
Cell theory states that all living things are composed of cells, cells are the basic units of structure and function, and new cells are produced from existing cells. There are two main types of cells - prokaryotic cells which lack a nucleus and eukaryotic cells which contain a nucleus. Organelles in cells such as the nucleus, mitochondria, chloroplasts, endoplasmic reticulum, golgi apparatus, lysosomes, and vacuoles each have specific functions that allow the cell to carry out its activities.
Cells
Cell theory states that all living things are composed of cells, cells are the basic units of structure and function, and new cells are produced from existing cells. There are two main types of cells - prokaryotic cells which lack a nucleus and eukaryotic cells which have a nucleus containing DNA. Organelles in cells such as the nucleus, mitochondria, chloroplasts, endoplasmic reticulum, golgi apparatus, lysosomes, and vacuoles each have specific functions that allow the cell to carry out its activities.
Characteristic of life
This document discusses the key characteristics of living things such as cells, DNA, metabolism, homeostasis, and response to stimuli. It also covers the four main types of organic compounds that make up living things: carbohydrates, lipids, nucleic acids, and proteins. Additionally, it provides information on chemistry of life, enzymes, viruses, bacteria, germ theory, and methods of disease transmission and prevention.
Chapter 9
Cellular respiration involves three main stages - glycolysis, the Krebs cycle, and the electron transport chain - to break down glucose and generate energy in the form of ATP. Glycolysis breaks down glucose and produces some ATP. The Krebs cycle further breaks down these products and generates more ATP and electron carriers. Finally, the electron transport chain uses these electron carriers to generate most of the cell's ATP through oxidative phosphorylation.
Chapter 8
Photosynthesis has two main stages: the light-dependent reaction uses light energy to produce ATP and NADPH, while the light-independent Calvin Cycle uses these products to incorporate CO2 into organic compounds like glucose. Key events in the history of photosynthesis research include the discoveries that plants require water, produce oxygen, and need light to carry out the process. The overall equation is: 6CO2 + 6H2O + light energy → C6H12O6 + 6O2.
Chapter 8
Photosynthesis has two main stages: the light-dependent reaction uses light energy to produce ATP and NADPH, while the light-independent Calvin Cycle uses these products to incorporate CO2 into organic compounds like glucose. Key events in photosynthesis history include discoveries that plants require water, produce oxygen, and need light to do so. The overall reaction is: 6CO2 + 6H2O + light energy → C6H12O6 + 6O2.
Evolution
- Charles Darwin proposed the theory of evolution through natural selection in 1859 after observing species variation on the Galapagos Islands. His theory built upon earlier ideas from scientists like Jean-Baptiste Lamarck and Thomas Malthus.
- Evolution occurs as inherited traits increase the chances of survival and reproduction in an organism's environment through natural selection and adaptation over many generations. The fossil record provides evidence of how species have changed over time.
- The earliest life on Earth was microbial and existed in the oceans around 3.8 billion years ago. Oxygen levels increased around 2.2 billion years ago allowing complex eukaryotic cells and later multi-cellular organisms to evolve. Major extinction events punctuated this pattern
Ecology
The document summarizes key concepts in ecology. It discusses the biosphere and how ecologists study relationships between individuals, populations, communities, ecosystems, and the entire biosphere. It then covers the basic methods used in ecological research - observing, experimenting, and modeling. It explains energy flow through ecosystems via photosynthesis and food chains. Matter is recycled through biogeochemical cycles like the water, carbon, and nitrogen cycles. The document also describes the abiotic and biotic factors that determine ecosystems and biomes, as well as population growth patterns.
Classifications
This document provides an overview of biological classification systems and kingdoms. It discusses how biologists classify organisms based on visible similarities and evolutionary relationships. Organisms are grouped in a hierarchical system with seven main levels from most specific (species) to most general (kingdom). There are currently six recognized kingdoms - Animalia, Plantae, Fungi, Protista, Archaea, and Bacteria. Molecular comparisons of DNA are also used to determine evolutionary relationships and estimate times of species divergence. The key kingdoms are described in terms of their basic characteristics.
Taxonomy, Classifications
This document provides an overview of biological classification systems and kingdoms. It discusses:
1) Carolus Linnaeus' hierarchical classification system with 7 levels (species to kingdom); organisms were grouped based on visible similarities.
2) Evolutionary classification groups organisms based on evolutionary relationships and derived characters rather than just physical similarities.
3) Current systems recognize 6 kingdoms - Animalia, Plantae, Fungi, Protista, Archaea, and Bacteria. DNA comparisons help determine evolutionary relationships.
4) The kingdoms are described in brief, highlighting key distinguishing features of plants, animals, fungi, and protists.
More from tracyconover (20)
Recently uploaded
বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
আমাদের সবার জন্য খুব খুব গুরুত্বপূর্ণ একটি বই ..বিসিএস, ব্যাংক, ইউনিভার্সিটি ভর্তি ও যে কোন প্রতিযোগিতা মূলক পরীক্ষার জন্য এর খুব ইম্পরট্যান্ট একটি বিষয় ...তাছাড়া বাংলাদেশের সাম্প্রতিক যে কোন ডাটা বা তথ্য এই বইতে পাবেন ...
তাই একজন নাগরিক হিসাবে এই তথ্য গুলো আপনার জানা প্রয়োজন ...।
বিসিএস ও ব্যাংক এর লিখিত পরীক্ষা ...+এছাড়া মাধ্যমিক ও উচ্চমাধ্যমিকের স্টুডেন্টদের জন্য অনেক কাজে আসবে ...
CACJapan - GROUP Presentation 1- Wk 4.pdf
Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
Chapter 4 - Islamic Financial Institutions in Malaysia.pptx
Chapter 4 - Islamic Financial Institutions in Malaysia.pptxMohd Adib Abd Muin, Senior Lecturer at Universiti Utara Malaysia
This slide is special for master students (MIBS & MIFB) in UUM. Also useful for readers who are interested in the topic of contemporary Islamic banking.
The History of Stoke Newington Street Names
Presented at the Stoke Newington Literary Festival on 9th June 2024
www.StokeNewingtonHistory.com
Natural birth techniques - Mrs.Akanksha Trivedi Rama University
Natural birth techniques - Mrs.Akanksha Trivedi Rama UniversityAkanksha trivedi rama nursing college kanpur.
Natural birth techniques are various type such as/ water birth , alexender method, hypnosis, bradley method, lamaze method etcTop five deadliest dog breeds in America
Thinking of getting a dog? Be aware that breeds like Pit Bulls, Rottweilers, and German Shepherds can be loyal and dangerous. Proper training and socialization are crucial to preventing aggressive behaviors. Ensure safety by understanding their needs and always supervising interactions. Stay safe, and enjoy your furry friends!
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...National Information Standards Organization (NISO)
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.ANATOMY AND BIOMECHANICS OF HIP JOINT.pdf
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
South African Journal of Science: Writing with integrity workshop (2024)
South African Journal of Science: Writing with integrity workshop (2024)Academy of Science of South Africa
A workshop hosted by the South African Journal of Science aimed at postgraduate students and early career researchers with little or no experience in writing and publishing journal articles.MATATAG CURRICULUM: ASSESSING THE READINESS OF ELEM. PUBLIC SCHOOL TEACHERS I...
In this research, it concludes that while the readiness of teachers in Caloocan City to implement the MATATAG Curriculum is generally positive, targeted efforts in professional development, resource distribution, support networks, and comprehensive preparation can address the existing gaps and ensure successful curriculum implementation.
Thesis Statement for students diagnonsed withADHD.ppt
Presentation required for the master in Education.
Advantages and Disadvantages of CMS from an SEO Perspective
Advantages and Disadvantages of CMS from an SEO Perspective
Recently uploaded (20)
বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
বাংলাদেশ অর্থনৈতিক সমীক্ষা (Economic Review) ২০২৪ UJS App.pdf
Chapter 4 - Islamic Financial Institutions in Malaysia.pptx
Chapter 4 - Islamic Financial Institutions in Malaysia.pptx
Natural birth techniques - Mrs.Akanksha Trivedi Rama University
Natural birth techniques - Mrs.Akanksha Trivedi Rama University
Pride Month Slides 2024 David Douglas School District
Pride Month Slides 2024 David Douglas School District
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Pollock and Snow "DEIA in the Scholarly Landscape, Session One: Setting Expec...
Group Presentation 2 Economics.Ariana Buscigliopptx
Group Presentation 2 Economics.Ariana Buscigliopptx
South African Journal of Science: Writing with integrity workshop (2024)
South African Journal of Science: Writing with integrity workshop (2024)
Liberal Approach to the Study of Indian Politics.pdf
Liberal Approach to the Study of Indian Politics.pdf
MATATAG CURRICULUM: ASSESSING THE READINESS OF ELEM. PUBLIC SCHOOL TEACHERS I...
MATATAG CURRICULUM: ASSESSING THE READINESS OF ELEM. PUBLIC SCHOOL TEACHERS I...
Thesis Statement for students diagnonsed withADHD.ppt
Thesis Statement for students diagnonsed withADHD.ppt
Advantages and Disadvantages of CMS from an SEO Perspective
Advantages and Disadvantages of CMS from an SEO Perspective
Chemical bonding 2 no bonds
- 2. • Bonds are formed between elements that can rearrange their molecules to create stable compounds. • Bonds only form when energy is put in or taken away (endothermic or exothermic) • For bonds to form, the outer energy level must equal 8 (octet rule) for one of the elements. • Ionic bond – between metal and nonmetal – Electrons are transferred • Covalent bond – nonmetal and nonmetal – Electrons are shared • Metallic bond – metal and a metal
- 3. How to identify Bonds • Locate the elements on periodic table • Determine if the element is a metal, nonmetal • Identify the bonds • EXAMPLES: • Na (metal) + Cl (nonmetal) = ionic bond – electrons are transferred • C (nonmetal) + O (nonmetal) = covalent bond – Electrons are shared • Cu (metal) + Sn (metal) = metallic bond