Lec01 Matters At Atomic Level
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The document discusses atomic structure and bonding. It describes the basic components of an atom, including protons, neutrons, and electrons. It also discusses different types of atomic bonding structures: covalent, ionic, metallic, and Van der Waals. Additionally, it examines atomic arrangements in different states of matter, such as gases, crystals, liquids, and amorphous solids. Gases have no order, crystals have long and short range order, while liquids and amorphous solids have partial, unstable short range order but no long range order.
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Lec01 Matters At Atomic Level
The document discusses atomic structure and bonding, as well as the arrangement of atoms in different materials. It describes the basic components of an atom, including protons, neutrons, and electrons. It also explains different types of atomic bonding: covalent (e.g. in chlorine molecules), ionic (e.g. in lithium fluoride), and metallic. Additionally, it discusses Van der Waals bonding and the atomic arrangements in gases (chaotic with no order), crystals (highly ordered), liquids and amorphous solids (partially and unstably ordered), through 2D illustrations.
CLASS 9 CHEMISTRY CHAPTER 3 ATOMS AND MOLECULES PART 2 WRITING CHEMICAL FORMULAE
This document discusses writing chemical formulas from elements and their valences. It provides rules for writing formulas such as writing the metal before the non-metal and using subscripts for their valences. A valency table lists common elements and ions with their valences. Examples show applying the rules to write formulas for compounds such as sodium chloride and aluminum oxide. Practice problems at the end ask the reader to write formulas for compounds and name compounds given their formulas.
Atomic structure.KM
The Presentation Includes:
1. Introduction to Atom
2. Atomic Number & Atomic Mass Calculations
3. Understanding Isotopes
4. Deducing Mass Spectra
5. Relative Atomic Mass Calculations
Ionic bonds (site)
Ionic bonds form between oppositely charged ions, such as metals and non-metals. Metals easily lose electrons to become cations, while non-metals gain electrons to become anions. The attractive electrostatic forces between cations and anions give ionic compounds high melting points and crystalline structures. The total charge of an ionic compound is always zero.
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This document provides an overview of bonding concepts including molecular and ionic bonding. It discusses how elements form compounds through attraction and sharing or transferring of electrons to form stable electron configurations. Molecular compounds consist of nonmetals bonding through covalent bonds, with examples like H2O and C6H12O6. Properties of covalent bonds are described. Ionic bonding occurs between metals and nonmetals through transfer of electrons to form cations and anions. Formula writing and naming conventions are outlined for both ionic and molecular compounds.
SOLID STATE -XII BY SULEKHA RANI R , PGT CHEMISTRY
Here are the definitions and differences you asked for:
Short range order - Atoms are arranged in a disordered manner within a small region but this arrangement does not extend over long distances.
Anisotropic - A material whose physical properties vary with the direction of measurement.
Unit cell - The smallest repeating unit that constructs the entire crystal by translation.
Voids - Empty spaces between closely packed spheres in crystal structures. There are two types - octahedral and tetrahedral voids.
Impurity defect - Occurs when an atom of one element replaces an atom of the host element in its normal lattice position.
Monoclinic - Unit cell with two axes at 90 degrees and one axis not at 90 degrees
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This document discusses the structure and properties of ionic compounds. It begins by explaining that ionic compounds are formed through the electrostatic attraction between oppositely charged ions. The ions form a crystalline lattice structure held together by strong ionic bonds. This lattice structure results in ionic compounds having high melting points, hardness, and brittleness. The document then discusses how ionic bonding occurs through the transfer of electrons between metals and nonmetals. It provides examples of writing chemical formulas and naming ionic compounds based on their ion charges.
CH.6 - Bonding (2022).ppt
The document provides information on writing chemical formulas and naming compounds. It begins by defining oxidation numbers and discussing how they are used to write formulas for binary ionic compounds and polyatomic ionic compounds. Cationic elements are written first, followed by anionic elements or polyatomic ions in parentheses. Naming conventions are also outlined, with binary ionic compounds taking the cation name followed by "-ide" and polyatomic compounds taking the cation name followed by the name of the polyatomic ion. Lewis structures, molecular shapes, and intermolecular forces are also summarized.
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Lec01 Matters At Atomic Level
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This document discusses writing chemical formulas from elements and their valences. It provides rules for writing formulas such as writing the metal before the non-metal and using subscripts for their valences. A valency table lists common elements and ions with their valences. Examples show applying the rules to write formulas for compounds such as sodium chloride and aluminum oxide. Practice problems at the end ask the reader to write formulas for compounds and name compounds given their formulas.
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3. Understanding Isotopes
4. Deducing Mass Spectra
5. Relative Atomic Mass Calculations
Ionic bonds (site)
Ionic bonds form between oppositely charged ions, such as metals and non-metals. Metals easily lose electrons to become cations, while non-metals gain electrons to become anions. The attractive electrostatic forces between cations and anions give ionic compounds high melting points and crystalline structures. The total charge of an ionic compound is always zero.
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SOLID STATE -XII BY SULEKHA RANI R , PGT CHEMISTRY
Here are the definitions and differences you asked for:
Short range order - Atoms are arranged in a disordered manner within a small region but this arrangement does not extend over long distances.
Anisotropic - A material whose physical properties vary with the direction of measurement.
Unit cell - The smallest repeating unit that constructs the entire crystal by translation.
Voids - Empty spaces between closely packed spheres in crystal structures. There are two types - octahedral and tetrahedral voids.
Impurity defect - Occurs when an atom of one element replaces an atom of the host element in its normal lattice position.
Monoclinic - Unit cell with two axes at 90 degrees and one axis not at 90 degrees
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This document discusses the structure and properties of ionic compounds. It begins by explaining that ionic compounds are formed through the electrostatic attraction between oppositely charged ions. The ions form a crystalline lattice structure held together by strong ionic bonds. This lattice structure results in ionic compounds having high melting points, hardness, and brittleness. The document then discusses how ionic bonding occurs through the transfer of electrons between metals and nonmetals. It provides examples of writing chemical formulas and naming ionic compounds based on their ion charges.
CH.6 - Bonding (2022).ppt
The document provides information on writing chemical formulas and naming compounds. It begins by defining oxidation numbers and discussing how they are used to write formulas for binary ionic compounds and polyatomic ionic compounds. Cationic elements are written first, followed by anionic elements or polyatomic ions in parentheses. Naming conventions are also outlined, with binary ionic compounds taking the cation name followed by "-ide" and polyatomic compounds taking the cation name followed by the name of the polyatomic ion. Lewis structures, molecular shapes, and intermolecular forces are also summarized.
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An ionic compound is formed when an atom gains or loses electrons to achieve a stable electron configuration. Ions with opposite charges are attracted to each other, forming an ionic bond. Transition metals can form multiple stable ionic states due to their complex electron configurations. Polyatomic ions contain multiple atoms that travel together and are indicated using brackets. Covalent bonds form between non-metal atoms by sharing electrons rather than transferring them.
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Ionic compounds are made up of positive metal ions and negative non-metal ions arranged in a crystal lattice. In ionic compounds like sodium chloride, the oppositely charged ions are held together by strong electrostatic forces of attraction. Potassium oxide and lithium oxide are examples where the metal ions (potassium and lithium) outnumber the oxygen ions in a ratio of about 1:2, as represented by their chemical formulas K2O and Li2O.
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Lecture 5
I. Ionic bonds form when an atom with high electronegativity steals an electron from a atom with low electronegativity, giving them partial charges that attract via electromagnetic force.
II. Covalent bonds form when two atoms share electrons equally. Polar covalent bonds occur when sharing is unequal, giving partial charges.
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Ikatan kimIa Arum
1. The document discusses different types of chemical bonding including ionic bonding, covalent bonding, and metallic bonding.
2. Ionic bonding occurs when atoms transfer electrons to form oppositely charged ions that are then attracted via electrostatic forces, such as in sodium chloride (NaCl).
3. Covalent bonding involves the sharing of electron pairs between atoms to form molecular compounds, like in water (H2O) and methane (CH4).
02 Ch02chemistry2005 1
- Life requires around 25 essential chemical elements, with carbon, hydrogen, oxygen, and nitrogen making up 96% of living matter. Four additional elements - phosphorus, calcium, sulfur, and potassium - make up most of the remaining 4%.
- Atoms are made up of protons, neutrons, and electrons. The number of protons determines the element and its properties. Atoms can form bonds by gaining or losing electrons to form ions (ionic bonds) or by sharing electrons to form molecules (covalent bonds).
- Weak hydrogen bonds between polar molecules like water allow for their unique properties and are important in biological processes. The shape of molecules determines their function in chemical reactions in living things.
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An ionic compound is formed when an atom gains or loses electrons to achieve a stable electron configuration. Ions with opposite charges are attracted to each other, forming an ionic bond. Transition metals can form multiple stable ionic states due to their complex electron configurations. Polyatomic ions contain multiple atoms that travel together and are indicated using brackets. Covalent bonds form between non-metal atoms by sharing electrons rather than transferring them.
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An ionic compound is formed when an atom gains or loses electrons to achieve a stable electron configuration. Ions are formed due to electrostatic attraction between oppositely charged ions. Transition metals can form multiple stable ionic states due to their complex electron configurations. Polyatomic ions contain multiple atoms that travel together and are indicated using brackets. Covalent bonds form between nonmetals by sharing electrons rather than transferring them. Latin prefixes indicate the number of atoms in covalent compounds.
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This document discusses radicals, ions, and how to write chemical formulas. Radicals are species with unpaired electrons that can exist independently, and there are two main types - acid and basic radicals. Ions are charged species formed when atoms gain or lose electrons to become cations (positively charged) or anions (negatively charged). To write a chemical formula, you need the symbols of the elements and their valencies (combining capacities), then cross-multiply the valencies to get the formula. Examples of common cation and anion symbols and their valencies are provided.
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Giant Ionic Structure
Ionic compounds are made up of positive metal ions and negative non-metal ions arranged in a crystal lattice. In ionic compounds like sodium chloride, the oppositely charged ions are held together by strong electrostatic forces of attraction. Potassium oxide and lithium oxide are examples where the metal ions (potassium and lithium) outnumber the oxygen ions in a ratio of about 1:2, as represented by their chemical formulas K2O and Li2O.
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Ionic bonding occurs when a metal atom transfers electrons to a non-metal atom to form ions. The ions have full outer electron shells, making them stable. The positively charged metal ions are attracted to the negatively charged non-metal ions, forming an ionic bond. To determine the formula of an ionic compound, you write the symbols of the elements, determine the charge of each ion, and balance the ions so the total charge is zero. This gives the ratio of ions used to write the chemical formula. For example, sodium oxide has a 2:1 ratio of sodium and oxide ions, so its formula is Na2O.
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The document provides information on naming ionic compounds and writing their formulas. It discusses the rules for writing formulas, such as ensuring the total positive and negative charges are equal. It describes the "swoosh and reduce" method for determining formulas, which involves writing the symbols and charges of the elements and crossing the charges to become subscripts on the other element. The document also covers naming cations and anions and how to combine them to name complete ionic compounds.
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Ionic compounds form when ions bond through electrostatic attraction. Metals form cations by losing electrons to achieve a full outer shell, while nonmetals form anions by gaining electrons. Cations and anions are attracted due to their opposite charges. Ionic compounds have high melting points, are crystalline solids, and dissolve in water due to the separation of ions. They do not conduct electricity as solids but do so as liquids or dissolved solutions.
Lecture 5
I. Ionic bonds form when an atom with high electronegativity steals an electron from a atom with low electronegativity, giving them partial charges that attract via electromagnetic force.
II. Covalent bonds form when two atoms share electrons equally. Polar covalent bonds occur when sharing is unequal, giving partial charges.
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This document discusses the steps and rules for writing chemical formulas. It begins by outlining the objectives of learning to write formulas and defining key terms like subscripts and coefficients. It then explains the four main steps to write formulas: 1) Determine element symbols 2) Predict oxidation states 3) Write symbols with charges 4) Balance charges. The rest of the document outlines four main rules for writing subscripts and parentheses correctly based on oxidation states and whether elements appear only once or multiple times in a compound.
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1. The document discusses atomic structure and bonding. It describes the structure of atoms in terms of electrons and the nucleus containing protons and neutrons. It also discusses the arrangement of electrons in shells and the significance of noble gas structures and valency electrons.
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This document discusses the structure of atoms and the types of chemical bonds. It begins by defining the atom and its components like protons, electrons, and electron shells. It then explains the three main types of chemical bonds: ionic bonds formed between ions through electron transfer, covalent bonds formed by electron sharing, and metallic bonds in metals involving delocalized electrons. Some key points about each bond type are described, including examples. The document also touches on atomic and molecular masses and formula weights.
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This document discusses the structure of atoms and the types of chemical bonds. It begins by defining the atom and its components like protons, electrons, and electron shells. It then explains the three main types of chemical bonds: ionic bonds formed between ions through electron transfer, covalent bonds formed by electron sharing, and metallic bonds in metals involving delocalized electrons. Some key points about each bond type are described, including examples. The document also touches on atomic and molecular masses and formula weights.
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This document discusses how to write chemical formulas. It explains that a chemical formula tells us the types and numbers of atoms in a compound. It then outlines five steps for writing chemical formulas: 1) Write the symbols of the ions side by side in order of positive then negative, 2) Write the valency of each ion, 3) Transfer the valencies to offset them, 4) Omit valencies that are the same, and include different valencies in the formula, 5) For radicals like sulfate and phosphate, the net charge indicates the radical's valency and it is written in parentheses.
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This document discusses ions and how they are formed. It explains that atoms become ions by gaining or losing electrons to obtain a full outer electron shell. Atoms that gain electrons become negatively charged ions and atoms that lose electrons become positively charged ions. The document also discusses different types of ions including monatomic ions, polyatomic ions, and how to name compound ions that contain multiple atoms like sulfate, nitrate, and hydroxide ions.
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This document is about atoms, elements, and chemical reactions. It contains three main sections: (1) what atoms and elements are, including their symbols and arrangement in the periodic table, (2) how elements can combine to form compounds with different properties, and (3) how chemical reactions allow atoms to join together to form new substances.
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Ikatan kimIa Arum
1. The document discusses different types of chemical bonding including ionic bonding, covalent bonding, and metallic bonding.
2. Ionic bonding occurs when atoms transfer electrons to form oppositely charged ions that are then attracted via electrostatic forces, such as in sodium chloride (NaCl).
3. Covalent bonding involves the sharing of electron pairs between atoms to form molecular compounds, like in water (H2O) and methane (CH4).
02 Ch02chemistry2005 1
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worksheet (LKS) ini berisi materi ikatan kimia secara lengkap. mulai dari ikatan ion hingga ikatan kovalen. monggo dimanfaatkan
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Atoms form ions by gaining or losing electrons to achieve a full outer electron shell like noble gases. Ions then bond to form ionic compounds between metals and nonmetals like NaCl. Covalent bonds form when atoms share electrons to achieve full outer shells, like in H2O. Polyatomic ions, which are ions of two or more bonded atoms, can also participate in ionic bonding, such as Ca(OH)2 which contains hydroxide ions bonding to calcium ions. The number of each type of atom in a compound is shown by subscripts based on the ions formed.
04 chemical bonds
This document discusses chemical bonding and intramolecular bonding. It begins by introducing ionic and covalent bonds as the two major types of intramolecular bonding that hold atoms together to form molecules. Ionic bonds form between ions through the transfer of electrons from metals to nonmetals. Covalent bonds form between nonmetals by the sharing of electrons. The document then goes into further detail about the formation of ions, ionic compounds through electron transfers, and the naming of ionic compounds according to IUPAC nomenclature rules.
chem_formulas.pdf
This document provides information on writing and naming ionic and covalent compounds. It discusses the key differences between ionic and covalent bonding, and how they relate to writing chemical formulas and naming compounds. The document outlines the steps for writing ionic formulas, including how to handle transition metals and polyatomic ions. It also reviews naming conventions and prefixes used for ionic versus covalent compounds. Examples are provided throughout to illustrate the concepts and procedures.
IB Chemistry on Resonance, Delocalization and Formal Charges
This document provides a tutorial on formal charges, resonance structures, and delocalization of electrons. It explains that formal charge is a tool used to determine which Lewis structure of a molecule or polyatomic ion is more accurate. The structure with the lowest overall formal charge is usually preferred. Resonance structures show delocalized bonding, with the actual structure being a combination or "resonance hybrid" of the contributing structures. Examples discussed include carbon dioxide, the carbonate ion, dinitrogen oxide, the nitrate ion, and the nitrite ion.
Chapter 1 material structure and binary alloy system
This document discusses the structure of materials and binary alloy systems. It begins by defining key terms like atom, element, mixture, compound, atomic number, atomic mass, and atomic orbits. It then explains the periodic table, including its characteristics, groups, periods, and function. The document also covers crystal structures, bonding types, solidification of metals and alloys, solid solutions, and equilibrium phase diagrams.
Bonding Notes
Ionic bonding occurs between metals and nonmetals due to their differences in electronegativity. Metals have relatively low ionization energies and lose electrons to form cations, while nonmetals have high electronegativity and gain electrons to form anions. Oppositely charged ions are then attracted through electrostatic forces to form an ionic compound.
Ch 8 ionic compounds
Ionic compounds form when a metal transfers electrons to a nonmetal, resulting in oppositely charged ions that are attracted in a crystal lattice structure. The ratio of cations to anions must result in an overall neutral charge. Ionic compounds are named by writing the cation first followed by the anion. Polyatomic ions are named based on the nonmetal and number of oxygen atoms. Metallic bonds form a "sea of electrons" that are delocalized and allow metal atoms to strongly attract each other.
1515753021_aqa-knowledge-mat-gcse-chemistry-p1.pptx
Rutherford's scattering experiment showed that the atom has a small, dense nucleus surrounded by electrons. Most alpha particles passed through the gold foil, but some were deflected or reflected, indicating a small, positively charged nucleus. The development of the atomic model over time led to the discovery of subatomic particles like protons, neutrons, and electrons. The periodic table arranges elements in order of atomic number and groups elements with similar properties together.
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Lec01 Matters At Atomic Level
- 1. Matters at atomic level Tran Anh Tuan Materials Engineer MES Team
- 2. Lecture map atomic arrangement in matters atomic bonding atomic structure covalent ionic metallic Van der Waals Gases Crystals Amorphous Liquids
- 4. Atom = proton + neutron + electron
- 7. Lecture map atomic arrangement in matters atomic bonding atomic structure covalent ionic metallic Van der Waals Gases Crystals Amorphous Liquids
- 10. Covalent bonding Cl Cl
- 11. Covalent bonding Chemically Unstable Cl Cl Individual Cl atoms with 7 outer electrons
- 12. Covalent bonding Chemically Unstable bonding Cl Cl Cl Cl Individual Cl atoms with 7 outer electrons
- 13. Covalent bonding Chemically Unstable Chemically Stable bonding Cl Cl Cl Cl Individual Cl atoms with 7 outer electrons One Cl2 molecular with 8 outer electrons
- 14. Ionic bonding Li F
- 15. Ionic bonding Li F Individual Li and F atoms with 1 and 7 outer electrons Chemically Unstable
- 16. Ionic bonding Li F Individual Li and F atoms with 1 and 7 outer electrons Chemically Unstable
- 17. Ionic bonding Li F bonding Li F Individual Li and F atoms with 1 and 7 outer electrons One LiF molecular with 8 outer electrons Chemically Unstable Chemically Stable
- 18. Metallic bonding metallic ion free electron Balanced Coulombic Stochastic Interaction. Metallic materials
- 19. Van der Waals bonding positively charged negatively charged Usually seen in polymeric materials + - + - + - + - Polarized molecular
- 20. Lecture map atomic arrangement in matters atomic bonding atomic structure covalent ionic metallic Van der Waals Gases Crystals Amorphous Liquids
- 22. Gaseous matters 2D illustration of atomic arrangement in gaseous matters
- 23. Gaseous matters absolutely chaotic 2D illustration of atomic arrangement in gaseous matters
- 24. Gaseous matters absolutely chaotic 2D illustration of atomic arrangement in gaseous matters no short-range order
- 25. Gaseous matters absolutely chaotic 2D illustration of atomic arrangement in gaseous matters no long-range order no short-range order
- 26. Solid crystals 2D illustration of atomic arrangement in solid crystals
- 27. Solid crystals absolutely ordered 2D illustration of atomic arrangement in solid crystals
- 28. Solid crystals absolutely ordered 2D illustration of atomic arrangement in solid crystals short-range order
- 29. Solid crystals absolutely ordered 2D illustration of atomic arrangement in solid crystals long-range order short-range order
- 30. Liquid and amorphous 2D illustration of atomic arrangement in liquids and amorphous
- 31. Liquid and amorphous Partly, unstably ordered 2D illustration of atomic arrangement in liquids and amorphous
- 32. Liquid and amorphous Partly, unstably ordered 2D illustration of atomic arrangement in liquids and amorphous short-range order
- 33. Liquid and amorphous Partly, unstably ordered near - ordered no long-range order 2D illustration of atomic arrangement in liquids and amorphous
- 34. End of Lecture 01 Next: Lecture 02: Crystal lattice