Naming ionic compounds cations anions
•Download as PPTX, PDF•
6 likes•7,705 views
This document discusses naming ionic compounds by first naming the cation and anion components. It provides rules for naming main group and transition metal cations, such as naming sodium as the "sodium cation" and copper as the "copper (II) cation". It also provides rules for naming anions by taking the root of the element name and adding "-ide", such as naming chloride and bromide anions. Examples and practice problems are given to demonstrate applying these rules to name common cations and anions.
Report
Share
Report
Share
Recommended
Ionic compounds naming
1. Ionic compounds are formed from the combination of cations and anions. Cations are positively charged ions, usually metals, while anions are negatively charged, usually nonmetals.
2. To name ionic compounds, the cation is written first followed by the anion with the "-ide" ending. Transition metals may have multiple oxidation states requiring a Roman numeral to be included.
3. To determine the oxidation state of a transition metal, the charges of the cation and anion must balance out to zero. This can involve using subscripts or recognizing the set charge of common polyatomic ions.
Atoms, Molecules, and Ions
This document outlines the key concepts and objectives for a unit on atoms, molecules, and ions. It will cover early atomic theories like Dalton's atomic theory, discoveries leading to the nuclear model of the atom including cathode rays and Rutherford's gold foil experiment. Students will learn about atomic structure including atomic and mass numbers. The periodic table is introduced along with chemical bonds like ionic and covalent bonds. The document also outlines naming ionic and molecular compounds as well as writing chemical formulas.
Writing and Naming formula
This document discusses writing and naming chemical formulas and ions. It begins by explaining that cations are positively charged ions that migrate to the cathode, while anions are negatively charged ions that migrate to the anode. Examples of common cations and anions are provided. The document then discusses rules for writing formulas for ionic compounds without transition metals, ionic compounds with transition metals, and covalent compounds. It also covers naming conventions for polyatomic ions and provides examples of writing formulas from names and names from formulas.
Ionic Bonding
This document discusses ionic and metallic bonding. It explains that ions are formed when atoms gain or lose electrons to achieve stable noble gas electron configurations. Metals form cations by losing electrons while nonmetals form anions by gaining electrons. Ionic compounds contain cations and anions in ratios represented by chemical formulas. Metallic bonding occurs via delocalized valence electrons that are shared between metal atoms.
Atoms molecules and ions
objective
theory of atom
dalton`theory
Thomson, s model of atom
atomic number and mass number
isotopes, molecules formula, empirical formula
ions, formula of ionic compound, polyatomic ions, chemical nomenclature
Lewis dot structures
Lewis dot structures are a way to represent covalent bonding between atoms using dots to represent valence electrons. Atoms form bonds by sharing electrons in order to achieve stable electron configurations like the octet rule. Multiple bonds can form when more than one pair of electrons is shared between two atoms. Sometimes bonds form with both electrons coming from the same atom. Drawing accurate Lewis structures involves counting valence electrons and placing them between atoms to represent shared pairs and complete octets following the rules of covalent bonding. Resonance structures can occur when more than one valid Lewis structure exists for the same molecule.
Naming & Writing Ionic Formulas PowerPoint
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.
Atomic Mass Presentation
This document discusses atomic structure and masses of atoms. It explains that the mass number of an atom equals the number of protons plus neutrons. Isotopes are atoms of the same element that have different mass numbers. The relative atomic mass of an atom is calculated relative to 1/12 the mass of a carbon-12 atom. To calculate the average atomic mass of an element, the percentage and atomic mass of each isotope is determined and a weighted average is calculated.
Recommended
Ionic compounds naming
1. Ionic compounds are formed from the combination of cations and anions. Cations are positively charged ions, usually metals, while anions are negatively charged, usually nonmetals.
2. To name ionic compounds, the cation is written first followed by the anion with the "-ide" ending. Transition metals may have multiple oxidation states requiring a Roman numeral to be included.
3. To determine the oxidation state of a transition metal, the charges of the cation and anion must balance out to zero. This can involve using subscripts or recognizing the set charge of common polyatomic ions.
Atoms, Molecules, and Ions
This document outlines the key concepts and objectives for a unit on atoms, molecules, and ions. It will cover early atomic theories like Dalton's atomic theory, discoveries leading to the nuclear model of the atom including cathode rays and Rutherford's gold foil experiment. Students will learn about atomic structure including atomic and mass numbers. The periodic table is introduced along with chemical bonds like ionic and covalent bonds. The document also outlines naming ionic and molecular compounds as well as writing chemical formulas.
Writing and Naming formula
This document discusses writing and naming chemical formulas and ions. It begins by explaining that cations are positively charged ions that migrate to the cathode, while anions are negatively charged ions that migrate to the anode. Examples of common cations and anions are provided. The document then discusses rules for writing formulas for ionic compounds without transition metals, ionic compounds with transition metals, and covalent compounds. It also covers naming conventions for polyatomic ions and provides examples of writing formulas from names and names from formulas.
Ionic Bonding
This document discusses ionic and metallic bonding. It explains that ions are formed when atoms gain or lose electrons to achieve stable noble gas electron configurations. Metals form cations by losing electrons while nonmetals form anions by gaining electrons. Ionic compounds contain cations and anions in ratios represented by chemical formulas. Metallic bonding occurs via delocalized valence electrons that are shared between metal atoms.
Atoms molecules and ions
objective
theory of atom
dalton`theory
Thomson, s model of atom
atomic number and mass number
isotopes, molecules formula, empirical formula
ions, formula of ionic compound, polyatomic ions, chemical nomenclature
Lewis dot structures
Lewis dot structures are a way to represent covalent bonding between atoms using dots to represent valence electrons. Atoms form bonds by sharing electrons in order to achieve stable electron configurations like the octet rule. Multiple bonds can form when more than one pair of electrons is shared between two atoms. Sometimes bonds form with both electrons coming from the same atom. Drawing accurate Lewis structures involves counting valence electrons and placing them between atoms to represent shared pairs and complete octets following the rules of covalent bonding. Resonance structures can occur when more than one valid Lewis structure exists for the same molecule.
Naming & Writing Ionic Formulas PowerPoint
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.
Atomic Mass Presentation
This document discusses atomic structure and masses of atoms. It explains that the mass number of an atom equals the number of protons plus neutrons. Isotopes are atoms of the same element that have different mass numbers. The relative atomic mass of an atom is calculated relative to 1/12 the mass of a carbon-12 atom. To calculate the average atomic mass of an element, the percentage and atomic mass of each isotope is determined and a weighted average is calculated.
Formula writing
The document discusses the rules and steps for writing chemical formulas:
1) Formulas use symbols and subscripts to show which elements are present and how many atoms of each.
2) Rules include balancing charges by "criss-crossing" valence numbers, omitting subscripts of 1, and using parentheses for polyatomic ions.
3) The steps are to determine symbols and valences, write the positive element first, and balance charges to obtain the correct subscripts.
Stoichiometry
Stoichiometry allows us to use balanced chemical equations to determine the amounts of reactants and products involved in chemical reactions. It treats the chemical equation like a recipe, using mole ratios derived from the coefficients to solve mole-mole, mole-mass, and mass-mass problems. For example, if 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water, how many moles of oxygen are needed to produce 4 moles of water? By using the 1:1 mole ratio of oxygen to water given in the balanced equation, we can determine that 4 moles of oxygen are needed.
Naming Ionic and Covalent Compounds
1. The document provides an overview of writing formulas and naming ionic and covalent compounds. It reviews the periodic table and properties of metals, nonmetals and metalloids.
2. Key concepts covered include ion formation, the octet rule, polyatomic ions, oxidation numbers, naming conventions for ionic compounds containing metals or transition metals, and prefixes used in naming covalent compounds.
3. The document distinguishes between ionic and covalent bonding, lattice structures, and molecular structures of compounds.
Naming compounds
The document provides an overview of naming chemical compounds. It discusses the rules for naming binary ionic compounds that contain metals and nonmetals (types I and II), binary covalent compounds between two nonmetals (type III), compounds containing polyatomic ions, and acids. Examples of applying the naming conventions are provided throughout. The overall strategies are to consider whether the compounds are ionic or covalent, identify cations and anions or elemental names, and apply prefixes or suffixes accordingly when arriving at the systematic name.
Naming compounds given their formula
The document describes three methods for naming compounds based on their chemical formulas:
1) Ionic compounds are named by identifying the metal and nonmetal elements and using the metal name followed by the nonmetal name with "-ide". Transition metals use Roman numerals to indicate charge.
2) Polyatomic compounds name the polyatomic ion group and add the cation element name. Changes in oxygen content alter the ending.
3) Covalent compounds use Latin prefixes to indicate the number of atoms of each element and combine the element names.
Polyatomic Ions
Polyatomic ions are groups of atoms that are covalently bonded together and carry an overall electric charge. They behave as a single unit of charge when balancing equations for ionic compounds. Common examples include the nitrate ion (NO3-), which has one more electron than protons overall. Polyatomic ions are different from monatomic ions which involve a single atom with an electric charge due to having more or fewer electrons than protons.
writing chemical formulas
The document discusses chemical formulas and how they are used to express information about the proportions of atoms in compounds. It covers:
- Chemical formulas for covalent molecular compounds, covalent networks, and ionic compounds show the number or ratio of elements present
- Formulas are written using element symbols and subscripts to indicate atom counts
- Valence and Roman numerals are used to indicate an element's bonding tendency which helps write formulas
- Prefixes like mono-, di-, tri- are also used to show atom ratios
- Polyatomic ions, ions formed of multiple elements, are also represented in formulas
- Ionic formulas show the charges of ions present in ionic substances
Naming and writing compounds
This document provides instructions for writing formulas and naming different types of compounds. It explains that to write formulas, you must identify the elements and ions using the periodic table and write the cation first followed by the anion, balancing charges using the crisscross method. The three main types of compounds are ionic without transition metals, ionic with transition metals specified by Roman numerals, and covalent using prefixes and suffixes. Polyatomic ions also have set names and follow normal compound naming rules.
Valence and lewis dot structure
Here are the Lewis electron dot diagrams for the requested elements and ions:
1.
Br
Ga
2.
Mg2+
S2-
What is an ion? - Chemistry presentation
An ion is an atom or molecule that has gained or lost electrons, giving it a positive or negative charge. Atoms can become ions through ionization, where metals typically lose electrons to form cations and nonmetals gain electrons to form anions. Ionic compounds are formed when oppositely charged ions bond via ionic bonds, while covalent bonds involve the sharing of electron pairs between nonmetal atoms.
Ion formation
Atoms form ions by gaining or losing electrons to achieve a full outer shell like noble gases. Sodium loses 1 electron to form Na+ with 10 electrons and a positive charge as a cation. Fluorine gains 1 electron to form F- with 10 electrons and a negative charge as an anion. An element's group number helps determine its ionic charge when forming cations or anions to achieve a full outer shell.
Lewis Dot Structure
The document discusses Lewis dot structures, which use dots to represent valence electrons around an atomic symbol. It explains that ions have Lewis dot diagrams with fewer (for cations) or more (for anions) dots than the corresponding atom due to gaining or losing electrons. The document provides examples of Lewis dot diagrams for various ions, such as Ca2+ and O2-. It also includes practice problems asking students to draw Lewis dot diagrams for additional ions.
Law of conservation of mass 1
In the late 18th century, French chemist Antoine Lavoisier recognized the importance of accurate measurements in chemistry. He extensively studied combustion and discovered it involved reaction with oxygen. He also established the law of conservation of mass, which states that mass is neither created nor destroyed in chemical reactions, though atoms may be rearranged. A chemical equation balances the reactants and products to show equal numbers of each type of atom.
Balancing chemical equation
This document discusses balancing chemical equations. It explains that a chemical equation describes a chemical reaction by showing the reactants and products. It also notes that balancing a chemical equation establishes the quantitative relationship between reactants and products by using coefficients. There are three main steps to balancing an equation: 1) writing the unbalanced equation, 2) balancing the equation by applying the law of conservation of mass so each element has the same number of atoms on both sides, and 3) indicating the states of matter of the reactants and products using abbreviations like (g) or (s). An example problem of balancing the equation for the reaction of tin oxide with hydrogen gas to form tin and water vapor is provided.
Atoms And Subatomic Particles
An atom is incredibly small, with its diameter needing to be increased 200 million times to equal the diameter of a penny. Atoms are made up of subatomic particles, including protons and neutrons in the central nucleus and electrons orbiting the nucleus. Most of an atom's mass comes from its nucleus. The number of protons determines the element and is called the atomic number. Isotopes are atoms of the same element that differ in their number of neutrons.
Chemical Bonding
The atoms of molecules are linked together through a reaction known as chemical bonding. A chemical bond is a force that holds atoms together.
Properties of Compounds - Ionic, Covalent and Metallic
Ionic compounds are crystalline solids that have high melting points and dissolve in water. They have high melting points because opposite charges attract in strong ionic bonds, requiring a lot of energy to separate ions. They dissolve in water because water molecules are polar and attract ions, breaking up the crystal lattice. Ionic compounds conduct electricity when molten or dissolved as ions are then free to move but not as solids where ions are tightly bound. Metallic bonding involves metal atoms giving electrons to a "sea of electrons" allowing conductivity and properties like malleability. The key differences between compounds are that ionic compounds conduct when dissolved, metals conduct when solid, and covalent compounds do not conduct or dissolve.
Oxyanion nomenclature
This document discusses the nomenclature (naming) of oxyanions. Oxyanions are polyatomic ions containing oxygen and another nonmetal element. They are named by taking the root of the non-oxygen element and adding "-ate" or "-ite" suffixes, with "-ate" indicating more oxygen atoms. Pairs of oxyanions often exist for a given element, and the number of oxygen atoms distinguishes the names.
Chemical bonding
This document discusses different types of chemical bonds:
1) Metallic bonds form when valence electrons are delocalized and shared between all metal atoms in a lattice, holding the positive ions together.
2) Ionic bonds form when a metal transfers electrons to a nonmetal, creating oppositely charged ions that are attracted to each other.
3) Covalent bonds form when two nonmetals share valence electrons in a molecule through electron pairs. Lewis structures are used to represent electron sharing in covalent bonds.
History of the atom
The document provides a history of discoveries related to the atom from ancient Greek philosophers to modern quantum mechanics. It describes key contributors such as Democritus proposing atoms, Dalton establishing atomic theory, Rutherford discovering the nucleus, Bohr introducing quantum mechanics, and Heisenberg establishing the uncertainty principle. The development of atomic models progressed from simple spheres to planetary structures to quantum mechanical probability distributions.
Unit 10 real gases vdw fl14 final
A conceptual explanation of the Kinetic Molecular Theory of Gases (KTG) with examples. General Chemistry
Naming ionic compounds examples
This document provides examples for naming ionic compounds according to IOPAC rules. It gives the steps for naming compounds as: 1) write the cation, 2) name the anion as an element or polyatomic ion, 3) include the cation charge in Roman numerals if it is a transition metal. Mini quizzes are worked through, such as naming calcium chloride, sodium oxide, copper (II) oxide, and copper (I) oxide. The charge of the cation is determined by considering charges that balance the anion.
More Related Content
What's hot
Formula writing
The document discusses the rules and steps for writing chemical formulas:
1) Formulas use symbols and subscripts to show which elements are present and how many atoms of each.
2) Rules include balancing charges by "criss-crossing" valence numbers, omitting subscripts of 1, and using parentheses for polyatomic ions.
3) The steps are to determine symbols and valences, write the positive element first, and balance charges to obtain the correct subscripts.
Stoichiometry
Stoichiometry allows us to use balanced chemical equations to determine the amounts of reactants and products involved in chemical reactions. It treats the chemical equation like a recipe, using mole ratios derived from the coefficients to solve mole-mole, mole-mass, and mass-mass problems. For example, if 2 moles of hydrogen gas react with 1 mole of oxygen gas to produce 2 moles of water, how many moles of oxygen are needed to produce 4 moles of water? By using the 1:1 mole ratio of oxygen to water given in the balanced equation, we can determine that 4 moles of oxygen are needed.
Naming Ionic and Covalent Compounds
1. The document provides an overview of writing formulas and naming ionic and covalent compounds. It reviews the periodic table and properties of metals, nonmetals and metalloids.
2. Key concepts covered include ion formation, the octet rule, polyatomic ions, oxidation numbers, naming conventions for ionic compounds containing metals or transition metals, and prefixes used in naming covalent compounds.
3. The document distinguishes between ionic and covalent bonding, lattice structures, and molecular structures of compounds.
Naming compounds
The document provides an overview of naming chemical compounds. It discusses the rules for naming binary ionic compounds that contain metals and nonmetals (types I and II), binary covalent compounds between two nonmetals (type III), compounds containing polyatomic ions, and acids. Examples of applying the naming conventions are provided throughout. The overall strategies are to consider whether the compounds are ionic or covalent, identify cations and anions or elemental names, and apply prefixes or suffixes accordingly when arriving at the systematic name.
Naming compounds given their formula
The document describes three methods for naming compounds based on their chemical formulas:
1) Ionic compounds are named by identifying the metal and nonmetal elements and using the metal name followed by the nonmetal name with "-ide". Transition metals use Roman numerals to indicate charge.
2) Polyatomic compounds name the polyatomic ion group and add the cation element name. Changes in oxygen content alter the ending.
3) Covalent compounds use Latin prefixes to indicate the number of atoms of each element and combine the element names.
Polyatomic Ions
Polyatomic ions are groups of atoms that are covalently bonded together and carry an overall electric charge. They behave as a single unit of charge when balancing equations for ionic compounds. Common examples include the nitrate ion (NO3-), which has one more electron than protons overall. Polyatomic ions are different from monatomic ions which involve a single atom with an electric charge due to having more or fewer electrons than protons.
writing chemical formulas
The document discusses chemical formulas and how they are used to express information about the proportions of atoms in compounds. It covers:
- Chemical formulas for covalent molecular compounds, covalent networks, and ionic compounds show the number or ratio of elements present
- Formulas are written using element symbols and subscripts to indicate atom counts
- Valence and Roman numerals are used to indicate an element's bonding tendency which helps write formulas
- Prefixes like mono-, di-, tri- are also used to show atom ratios
- Polyatomic ions, ions formed of multiple elements, are also represented in formulas
- Ionic formulas show the charges of ions present in ionic substances
Naming and writing compounds
This document provides instructions for writing formulas and naming different types of compounds. It explains that to write formulas, you must identify the elements and ions using the periodic table and write the cation first followed by the anion, balancing charges using the crisscross method. The three main types of compounds are ionic without transition metals, ionic with transition metals specified by Roman numerals, and covalent using prefixes and suffixes. Polyatomic ions also have set names and follow normal compound naming rules.
Valence and lewis dot structure
Here are the Lewis electron dot diagrams for the requested elements and ions:
1.
Br
Ga
2.
Mg2+
S2-
What is an ion? - Chemistry presentation
An ion is an atom or molecule that has gained or lost electrons, giving it a positive or negative charge. Atoms can become ions through ionization, where metals typically lose electrons to form cations and nonmetals gain electrons to form anions. Ionic compounds are formed when oppositely charged ions bond via ionic bonds, while covalent bonds involve the sharing of electron pairs between nonmetal atoms.
Ion formation
Atoms form ions by gaining or losing electrons to achieve a full outer shell like noble gases. Sodium loses 1 electron to form Na+ with 10 electrons and a positive charge as a cation. Fluorine gains 1 electron to form F- with 10 electrons and a negative charge as an anion. An element's group number helps determine its ionic charge when forming cations or anions to achieve a full outer shell.
Lewis Dot Structure
The document discusses Lewis dot structures, which use dots to represent valence electrons around an atomic symbol. It explains that ions have Lewis dot diagrams with fewer (for cations) or more (for anions) dots than the corresponding atom due to gaining or losing electrons. The document provides examples of Lewis dot diagrams for various ions, such as Ca2+ and O2-. It also includes practice problems asking students to draw Lewis dot diagrams for additional ions.
Law of conservation of mass 1
In the late 18th century, French chemist Antoine Lavoisier recognized the importance of accurate measurements in chemistry. He extensively studied combustion and discovered it involved reaction with oxygen. He also established the law of conservation of mass, which states that mass is neither created nor destroyed in chemical reactions, though atoms may be rearranged. A chemical equation balances the reactants and products to show equal numbers of each type of atom.
Balancing chemical equation
This document discusses balancing chemical equations. It explains that a chemical equation describes a chemical reaction by showing the reactants and products. It also notes that balancing a chemical equation establishes the quantitative relationship between reactants and products by using coefficients. There are three main steps to balancing an equation: 1) writing the unbalanced equation, 2) balancing the equation by applying the law of conservation of mass so each element has the same number of atoms on both sides, and 3) indicating the states of matter of the reactants and products using abbreviations like (g) or (s). An example problem of balancing the equation for the reaction of tin oxide with hydrogen gas to form tin and water vapor is provided.
Atoms And Subatomic Particles
An atom is incredibly small, with its diameter needing to be increased 200 million times to equal the diameter of a penny. Atoms are made up of subatomic particles, including protons and neutrons in the central nucleus and electrons orbiting the nucleus. Most of an atom's mass comes from its nucleus. The number of protons determines the element and is called the atomic number. Isotopes are atoms of the same element that differ in their number of neutrons.
Chemical Bonding
The atoms of molecules are linked together through a reaction known as chemical bonding. A chemical bond is a force that holds atoms together.
Properties of Compounds - Ionic, Covalent and Metallic
Ionic compounds are crystalline solids that have high melting points and dissolve in water. They have high melting points because opposite charges attract in strong ionic bonds, requiring a lot of energy to separate ions. They dissolve in water because water molecules are polar and attract ions, breaking up the crystal lattice. Ionic compounds conduct electricity when molten or dissolved as ions are then free to move but not as solids where ions are tightly bound. Metallic bonding involves metal atoms giving electrons to a "sea of electrons" allowing conductivity and properties like malleability. The key differences between compounds are that ionic compounds conduct when dissolved, metals conduct when solid, and covalent compounds do not conduct or dissolve.
Oxyanion nomenclature
This document discusses the nomenclature (naming) of oxyanions. Oxyanions are polyatomic ions containing oxygen and another nonmetal element. They are named by taking the root of the non-oxygen element and adding "-ate" or "-ite" suffixes, with "-ate" indicating more oxygen atoms. Pairs of oxyanions often exist for a given element, and the number of oxygen atoms distinguishes the names.
Chemical bonding
This document discusses different types of chemical bonds:
1) Metallic bonds form when valence electrons are delocalized and shared between all metal atoms in a lattice, holding the positive ions together.
2) Ionic bonds form when a metal transfers electrons to a nonmetal, creating oppositely charged ions that are attracted to each other.
3) Covalent bonds form when two nonmetals share valence electrons in a molecule through electron pairs. Lewis structures are used to represent electron sharing in covalent bonds.
History of the atom
The document provides a history of discoveries related to the atom from ancient Greek philosophers to modern quantum mechanics. It describes key contributors such as Democritus proposing atoms, Dalton establishing atomic theory, Rutherford discovering the nucleus, Bohr introducing quantum mechanics, and Heisenberg establishing the uncertainty principle. The development of atomic models progressed from simple spheres to planetary structures to quantum mechanical probability distributions.
What's hot (20)
Properties of Compounds - Ionic, Covalent and Metallic
Properties of Compounds - Ionic, Covalent and Metallic
Viewers also liked
Unit 10 real gases vdw fl14 final
A conceptual explanation of the Kinetic Molecular Theory of Gases (KTG) with examples. General Chemistry
Naming ionic compounds examples
This document provides examples for naming ionic compounds according to IOPAC rules. It gives the steps for naming compounds as: 1) write the cation, 2) name the anion as an element or polyatomic ion, 3) include the cation charge in Roman numerals if it is a transition metal. Mini quizzes are worked through, such as naming calcium chloride, sodium oxide, copper (II) oxide, and copper (I) oxide. The charge of the cation is determined by considering charges that balance the anion.
Matter and Measurement
Here are the answers to the significant figure questions to the correct number of significant figures:
1. 2.5
2. 40.6
3. 1400
Unit 10 daltons law fl14 final
Mostly conceptual explanation of Dalton's Law of Partial Pressures plus a few examples. General Chemistry
Naming ionic compounds writing emp formulas
This document discusses how to write empirical formulas for ionic compounds. It explains that ionic compounds are electrically neutral, meaning the positive charge of cations must cancel out the negative charge of anions. It provides an example of determining the charges on potassium (K+) and bromine (Br-) ions and writing the formula for the ionic compound potassium bromide (KBr). The document also gives a mini quiz example of determining the charges on lithium (Li+) and fluorine (F-) ions and writing the formula for the ionic compound lithium fluoride (LiF).
Density final version
The document defines density and describes how to calculate it using the equation density = mass/volume. Density is a measure of how concentrated a substance is and has units of mass/volume (e.g. g/mL). Examples show how to use the density equation to calculate density, mass, or volume by rearranging the terms. Practice problems demonstrate calculating density, mass, and volume for different substances using the given values and density equation.
Bonding: General Concepts
This document outlines the key concepts from Chapter 8 on bonding and chemical bonds. It begins with an introduction to the chapter and objectives. It then covers types of chemical bonds such as ionic and covalent bonds. It discusses electronegativity and how it relates to bond polarity. Additional sections cover ion sizes and configurations, lattice energies of ionic compounds, partial ionic character of covalent bonds, molecular geometry models, bond energies, Lewis structures for writing electron configurations of molecules, and more. The overall document provides an overview of general concepts in bonding and serves as a table of contents and outline for the chapter.
Unit 10 intro&early gaslaws final
Solving Boyle's and Charles' Law problems, with a short discussion of selected pressure units and Avogadro's Law. General Chemistry.
Matter and elements final
This document provides an introduction to chemistry, including definitions and classifications of matter. It discusses that matter can be classified as either pure substances or mixtures. Pure substances are either elements or compounds, while mixtures contain two or more substances mixed together. The document also describes the three phases of matter - solids, liquids, and gases - and provides examples of different types of mixtures and how they are classified.
Unit 10 kinetic theory fl14 final
A conceptual description of the van der Waals equation for real gases. Discussion of van der Waals constants a and b, plus conceptual example. Does not assume that intermolcular forces have been learned previously. General Chemistry
Dimensional analysis final
This document discusses dimensional analysis and conversion factors. It explains that equivalent units can be related by an equal sign and used to convert between units. Conversion factors set up the relationship between units and allow one to cancel units to isolate the desired unit. Examples show how to set up conversion factors and use them to change between eggs and dozen, pounds and kilograms, and other unit conversions.
Thermochemistry
This document provides an overview of Chapter 6: Thermochemistry from a textbook. It includes the following:
- Section 6.1 covers the nature of energy, including defining energy, work, potential energy, kinetic energy, endothermic and exothermic processes. It discusses the first law of thermodynamics and enthalpy.
- Section 6.2 discusses enthalpy changes, calorimetry (measuring heat), and using calorimetry to solve problems involving heat and temperature changes.
- The document provides learning objectives, tables of contents, definitions, concepts, examples, and practice problems to help students understand thermochemistry concepts.
Acid nomenclature
This document discusses the nomenclature (naming) of acids. It provides three rules for naming acids based on whether they contain oxygen or not. For acids containing oxyanions, the ending is changed from "-ate" to "-ic" or from "-ite" to "-ous" before adding "acid". For acids containing monatomic or polyatomic anions without oxygen, the ending is changed from "-ide" to "-ic" and "hydro-" is prefixed before adding "acid". Examples of applying each rule are given.
Formulas and Equations
This document provides an outline and objectives for a unit on formulas and equations. The unit covers calculating atomic mass, the mole concept including molar mass and conversions between moles and mass, determining empirical and molecular formulas through combustion analysis, and stoichiometry including writing and balancing chemical equations, limiting reactants, theoretical and percent yields. Example problems are provided to illustrate key concepts like calculating atomic mass, determining moles of atoms from mass, finding empirical and molecular formulas, and stoichiometry calculations.
Unit 10 ideal gaslaw final
The document discusses the ideal gas law, which relates the pressure, volume, temperature, and number of moles of a gas. It describes how the ideal gas law was developed by combining Boyle's law, Charles' law, and Avogadro's law. The ideal gas law equation is PV=nRT, where P is pressure, V is volume, n is moles of gas, R is the gas constant, and T is temperature in Kelvin. An example problem demonstrates how to use the ideal gas law to calculate the moles of gas produced in a chemical reaction.
Naming ionic compounds intro
This document discusses the formation of ionic bonds between ions. Ionic bonds are electrostatic attractions between oppositely charged ions. Cations are positively charged ions formed when metals lose electrons. Anions are negatively charged ions formed when nonmetals gain electrons. Ionic bonds generally form between metallic cations and nonmetallic anions. The document provides examples of common cations and anions and identifies metals, nonmetals, and metalloids on the periodic table.
Gases
This document provides an overview of key concepts related to gases, including:
- The properties of ideal gases and units of pressure like pascals and atmospheres.
- Gas laws including Boyle's, Charles', Gay-Lussac's, Avogadro's, and the ideal gas law.
- Conditions of STP and using gas laws to perform stoichiometric calculations.
- The kinetic molecular theory which explains gas properties in terms of particle motion.
- How real gases differ from ideal gases due to intermolecular forces.
Standard Enthalpy Formation
This document discusses standard enthalpies of formation (ΔHf°) and how to calculate the standard enthalpy of reaction (ΔH°) using ΔHf° values. Standard enthalpies of formation are defined as the enthalpy change for the formation of one mole of a compound from its constituent elements in their standard states. ΔHf° values are tabulated at 298 K and 1 atm and can be looked up in tables. The standard enthalpy of reaction can be calculated using the equation ΔH° = ΣΔHf°(products) - ΣΔHf°(reactants). An example reaction of N2O4(g) → 2NO2(g
Atomic Structure and Periodicity
This document outlines objectives and content for a chapter on atomic structure and periodicity. It covers electromagnetic radiation, the quantum mechanical model of the atom, atomic orbitals and quantum numbers, electron configuration and trends in the periodic table. Key topics include the dual particle-wave nature of light and electrons, quantization of energy levels, the Bohr model of the hydrogen atom, shapes of atomic orbitals, and building up the periodic table using the Aufbau principle.
Kinetic and Potential Energy
The document discusses the First Law of Thermodynamics regarding energy conservation. It defines kinetic energy as the energy of motion and potential energy as stored energy due to position. Examples are given of objects possessing kinetic or potential energy. The law states that energy cannot be created or destroyed, only converted between forms. An example of a ball rolling down a ramp demonstrates the conversion between potential and kinetic energy, with total energy remaining constant.
Viewers also liked (20)
Similar to Naming ionic compounds cations anions
Ionic Naming
The document provides information on naming ionic compounds, cations, anions, and polyatomic ions. It discusses how to name monatomic and transition metal cations by adding "-ion" or the charge in Roman numerals after the element name. Anions are named by adding "-ide" after the element root. Ionic compounds are formed by writing the cation first followed by the anion. Polyatomic ions are also included.
11 stem odl (1)
The document discusses naming conventions and formulas for common chemical substances, providing examples of naming monoatomic and polyatomic ions as well as binary ionic compounds and acids, and explaining the importance of chemical formulas in representing elements in compounds and understanding chemical reactions.
Applied Chapter 5.3 : Names and Formulas of Compounds
This document discusses naming and writing formulas for ionic compounds and compounds containing polyatomic ions. It explains that ionic compounds are made up of positive and negative ions in the simplest ratio to achieve neutral charge. Formulas show the types and numbers of ions present. Names specify the cation first followed by the anion. Polyatomic ions are named and treated as a single unit. Examples are provided to illustrate naming and writing formulas for various ionic compounds and those containing common polyatomic ions.
GENCHEM1-nomenclature.pptx
Nomenclature is the process of naming chemical compounds with systematic names so they can be easily identified. This document discusses the naming of ionic compounds, including binary ionic compounds composed of a metal and nonmetal, and ternary ionic compounds containing a polyatomic ion. It explains that the cation is always named first and the anion name ends in "-ide" for binary ionic compounds. For transition metals, Roman numerals indicate the ion charge. Ternary compounds contain two ions, with at least one being a polyatomic ion, and both ions are simply named in order.
PP_15a_chp_2_8_naming_ionic_compounds.ppt
The document discusses naming simple ionic compounds. It provides rules for naming type I and type II binary ionic compounds. For type I compounds, the cation is named first followed by the anion with the "-ide" suffix. For type II compounds containing metals with multiple charges, the roman numeral for the metal's charge is included in parentheses. The document also discusses naming compounds containing polyatomic ions by following similar rules.
SCIENCE 9 MODULE
This document discusses the rules for naming ionic compounds, covalent compounds, and compounds containing transition metals. It provides examples of naming compounds from their formulas, such as sodium hydroxide (NaOH), lithium sulfide (Li2S), and iron(III) chloride (FeCl3). It also gives examples of writing formulas from compound names, like beryllium chloride (BeCl2), copper(I) oxide (Cu2O), and diphosphorus pentoxide (P2O5).
Formula-Writing-and-Naming-Compounds.pdf
This document provides information on naming ions and compounds. It discusses rules for naming positive and negative ions, as well as binary ionic compounds, binary molecular compounds, exceptions, binary acids, ternary compounds, and ternary acids. Examples are given for each type of compound. The objectives are for learners to be able to name compounds from formulas and write formulas from names. Review questions and an assignment are included at the end.
Chemistry - Chp 9 - Chemical Names and Formulas - PowerPoint
This document covers naming and writing formulas for ions, ionic compounds, molecular compounds, acids, and bases. It provides objectives and definitions for each section, examples of naming and writing formulas, and explanations of naming conventions and rules including prefixes, charges, and endings for different types of compounds.
Chapter 7.1 : Chemical Names and Formulas
Chemical formulas indicate the relative number and type of atoms in a chemical compound or molecule. A chemical formula for an ionic compound represents one formula unit and uses the simplest whole number ratio of ions present. Binary ionic compounds are composed of two elements and the total positive charges must equal the total negative charges. Molecular compounds use a prefix system to indicate the number of atoms of the less electronegative element present. Polyatomic ions are named as units within chemical formulas.
NWTC General Chemistry Ch 06
This chapter discusses the nomenclature of inorganic compounds. It covers common and systematic naming of compounds, writing formulas from names of ionic compounds, and naming binary ionic compounds. The key points are:
- Common names are arbitrary while systematic names precisely identify chemical composition.
- Ions are named by changing the element name or using stock/classic prefixes depending on the charge. Formulas are written by balancing charges between cations and anions.
- Binary ionic compounds are named by identifying the cation and anion, including charge information for transition metals.
Ionic nomenclature
This document provides information on naming ionic compounds. It discusses that ionic compounds are made of positive and negative ions. It explains how to name binary ionic compounds containing two elements and ternary compounds containing three elements, with two elements in a polyatomic ion. It provides examples of naming binary ionic compounds like NaCl and ternary compounds like Mg(OH)2. It also discusses writing formulas from compound names.
Chapter 9
This document provides information on naming and writing formulas for different types of chemical compounds including:
1. Ionic compounds consisting of monatomic and polyatomic ions are named by writing the cation first followed by the anion. Transition metal ions have stock and classical naming systems.
2. Molecular compounds consisting of two nonmetals are named using prefixes to indicate the number of atoms of each element followed by the "-ide" suffix.
3. Acids are named based on the anion present, using prefixes like "hydro-", "-ous", or "-ic" depending on the anion suffix. Their formulas are written with hydrogen and the anion.
4. Bases are named by writing the cation
Naming_compounds.ppt
This document provides information on naming and writing formulas for different types of chemical compounds. It discusses binary ionic compounds composed of a metal and nonmetal, where the metal takes a Roman numeral charge and the nonmetal suffix is changed to "-ide". Ternary ionic compounds containing a polyatomic ion are also described. Polyatomic ions are groups of atoms that behave as a unit with a charge. The document outlines steps for writing formulas and uses examples like calcium phosphate and aluminum nitrate to illustrate the process. Finally, it defines binary molecular compounds as those containing two nonmetals covalently bonded, requiring the use of numerical prefixes in the naming.
Lesson_3_Names_and_Formulas_for_Ionic_Compounds_SLIDES.pdf
1) This document discusses the names and formulas of ionic compounds. It defines key terms like monatomic ions, polyatomic ions, and oxyanions.
2) Ionic compounds are made up of positively charged cations and negatively charged anions. Monatomic ions contain a single atom while polyatomic ions contain multiple atoms.
3) The document provides rules for writing formulas and naming ionic compounds containing polyatomic ions. The cation is written first followed by the anion and charges are balanced to give the overall formula unit a net neutral charge.
Ionic Compounds
The document discusses ionic compounds and their properties. It defines ionic compounds as formed from positively and negatively charged ions. Sodium chloride is given as an example where sodium loses an electron to become Na+ and chlorine gains an electron to become Cl-. Ionic compounds form crystalline structures and dissolve into ions in water, allowing them to conduct electricity. Common polyatomic ions are also discussed.
Lecture 9.1 & 9.2- Naming Salts
The document discusses chemical names and formulas of ions. It explains that monatomic cations form when metals lose electrons and gain a positive charge equal to their group number. Monatomic anions form when non-metals gain electrons and have a negative charge equal to the group number minus 8. Polyatomic ions consist of multiple atoms and have an overall positive or negative charge. Transition metals can form multiple ions with different charges that must be specified. Ionic compounds are named by writing the cation first followed by the anion.
Chemical Names and Formulas
This document discusses classifying and naming ionic and covalent compounds, as well as writing their formulas. It provides rules for:
- Classifying compounds as ionic or covalent based on their formula
- Naming ionic compounds using stock systems and identifying polyatomic ions
- Naming covalent compounds using prefixes to indicate the number of atoms
- Writing formulas for ionic compounds by balancing charges and for covalent compounds using prefixes
It also discusses acids, bases, and how to name and write formulas for acids based on their anion name endings.
Ions And Naming
When atoms or molecules gain or lose electrons, they form ions. Positively charged ions are called cations, and negatively charged ions are called anions. Groups of atoms can also carry a charge and are called polyatomic ions. Ionic compounds are named by combining the name of the cation and anion. Binary molecular compounds are systematically named using Greek prefixes and suffixes that indicate the number of atoms in the compound.
7. chemical formulas and naming compnds [Autosaved].pptx
This document provides information on naming and writing formulas for different types of compounds. It discusses binary ionic compounds and how their names and formulas are determined based on the ions present. It also covers binary covalent compounds and how prefixes are used in their names to indicate the ratio of elements. Finally, it mentions polyatomic ions and how their names are used in ionic compound names and formulas.
Ionic Bonds - Chapter 7
Ionic bonding occurs when atoms transfer electrons to form ions with opposite charges that are attracted via electrostatic forces. Metals form cations by losing electrons to achieve stable electron configurations like noble gases, while nonmetals form anions by gaining electrons. This transfer of electrons allows the formation of ionic compounds with crystalline structures where ion attractions are maximized and repulsions minimized. Properties of ionic compounds include high melting points, solubility in water, defined crystal structures, and the ability to conduct electricity when molten. Metallic bonding also involves cations but is characterized by delocalized valence electrons that form a "sea" allowing metals to conduct electricity and be malleable and ductile.
Similar to Naming ionic compounds cations anions (20)
Applied Chapter 5.3 : Names and Formulas of Compounds
Applied Chapter 5.3 : Names and Formulas of Compounds
Chemistry - Chp 9 - Chemical Names and Formulas - PowerPoint
Chemistry - Chp 9 - Chemical Names and Formulas - PowerPoint
Lesson_3_Names_and_Formulas_for_Ionic_Compounds_SLIDES.pdf
Lesson_3_Names_and_Formulas_for_Ionic_Compounds_SLIDES.pdf
7. chemical formulas and naming compnds [Autosaved].pptx
7. chemical formulas and naming compnds [Autosaved].pptx
More from Lumen Learning
What is Life
This document provides an overview of life science concepts including:
- Biology is the study of life, which is defined by cells, DNA, and basic components.
- The properties of life include being organized, using energy, maintaining internal environments, reproducing, responding to the environment, growing and developing, and evolving.
- Organisms are organized in a hierarchy from atoms to biosphere. The tree of life shows relationships between domains of life - bacteria, archaea, and eukarya. The scientific method involves making observations, hypotheses, experiments, theories, and conclusions to build knowledge.
Collective Action
This document discusses collective action and the two main barriers to it - coordination and the prisoner's dilemma. It provides examples of focal points that helped large groups coordinate for collective action, such as Franklin's "Join or Die" cartoon and King's leadership in the civil rights movement. The prisoner's dilemma concept is explained using a hypothetical bank robbery scenario and in examples like free riders benefiting from public goods without paying for them. Tragedies of the commons are also summarized as situations where individual self-interest can undermine the common good.
Powerpoint kutsonova melody week 1
This document provides an overview of basic musical elements including melody, harmony, and scales. It defines melody as a sequence of pitches that form a single musical idea. Harmony is described as two or more notes played simultaneously, whether as intervals between two notes or chords with three or more notes. Scales are introduced as the basis for melody and harmony, with examples given of major, minor, pentatonic, chromatic, and other scale types. The document includes listening examples and activities to illustrate different melodic concepts like contour, motion, and range as well as consonant and dissonant harmonies.
Practice Problems - General Concepts Blank
This document provides practice problems for a general chemistry unit covering concepts such as physical and chemical changes, pure substances and mixtures, separation techniques, properties, and density. It includes questions asking students to define terms, analyze samples, identify properties, describe separation methods, design experiments, and perform calculations.
Problem Solution - Dimensional Analysis
This document provides conversion factors and example problems for dimensional analysis. It includes conversions between common units like inches and centimeters, as well as metric prefix conversions. Example problems show how to set up multiple-step conversions between unusual units like picometers to feet and gallons to cubic centimeters. Justifications are provided to check if answers seem reasonable based on relative unit sizes.
Practice Problems - Dimensional Analysis Blank
This document provides conversions between various units including miles to cm, pm to feet, gallons to cm3, Angstroms to miles, mg to μg, m2 to cm2, μm2 to cm2, mL to pages printed, minutes to sort sheets of paper, g⋅cm3/s2 to kg⋅m3/hour2, g/L to lb/ft3, and m/s to miles/day. It also provides examples of dimensional analysis problems involving multiple conversion steps and significant figures that students will need to solve for a chemistry class.
Problem Solutions - Conversions
This document provides conversion factors for various units including quarts, gallons, miles, feet, inches, pounds, kilograms, centimeters, meters, micrometers, nanometers, and Kelvin and Celsius temperatures. It also gives examples of converting between these units and checking answers in scientific notation. Conversions between metric units can be done using multiplication and division with the appropriate conversion factors.
Practice Problems - Conversions Blank
This document provides conversion factors and example problems for converting between different units of measurement for length, volume, and temperature. It includes conversions between gallons/quarts, miles/feet, meters/centimeters/nanometers/micrometers, degrees Celsius/Kelvin, and milliliters/cubic centimeters. Students are advised that metric conversions will not be provided on exams and are expected to know temperature conversions between degrees Celsius and Kelvin. Several multi-part problems walk through conversions between various units.
The Second Law of Thermodynamics: Entropy and Heat IV
The document discusses entropy and the Second Law of Thermodynamics. It explains that entropy increases with increasing temperature as heat is added to a system and the number of accessible energy states increases. It provides examples of how entropy increases for phase transitions like melting (fusion) and vaporization, as molecules gain more positional freedom and accessible states in the liquid and gas phases compared to the solid phase. The document predicts that the change in entropy (ΔS) is positive for vaporization, as the gas phase allows molecules even more possible positions than the liquid.
Chem 2 - Third Law of Thermodynamics and Standard Molar Entropy V
This document discusses the Third Law of Thermodynamics and how it relates to standard molar entropy (S°). The Third Law states that the entropy of a substance at 0 K is zero, meaning it is in a perfectly ordered state with one microstate. This allows the absolute entropies and standard molar entropies (S°) of substances to be calculated. S° values are provided in tables and can be used to calculate the entropy change (ΔS°) of chemical reactions based on the standard molar entropies of the reactants and products.
Chem 2 - Std Free Energy of Formation VII
This document discusses standard free energy of formation (ΔGf°) and how to calculate standard free energy change (ΔG°) for chemical reactions. ΔGf° is defined as the free energy change for the formation of one mole of a compound from its elements in their standard states. For elements in their standard states, ΔGf° is zero. ΔG° can be calculated using the standard free energies of formation of products and reactants. It can also be calculated using standard enthalpies of formation (ΔHf°) and standard molar entropies (S°) with the equation ΔG° = ΔH° - TΔS°.
Chem 2 - The Second Law of Thermodynamics: Spontaneous Reactions and Entropy S I
This document discusses the Second Law of Thermodynamics and entropy. It begins by defining spontaneous processes as those that occur automatically without energy input and tend to proceed in one direction. It then reviews that the First Law concerns energy transfer and conservation. While the First Law doesn't determine spontaneity, entropy does - the greater the number of possible molecular arrangements (microstates), the higher the entropy and more disorder. The Second Law states that the total entropy change for any spontaneous process in the universe must be positive.
Chem 2 - Gibbs Free Energy and Spontaneous Reactions VI
The document discusses how Gibbs free energy (ΔG) can be used to predict the spontaneity of chemical reactions. ΔG is calculated as ΔH - TΔS, where ΔH is the change in enthalpy and ΔS is the change in entropy. The sign of ΔG determines whether a reaction is spontaneous or not. If ΔG is negative, the reaction is spontaneous in the forward direction. If ΔG is positive, the reaction is nonspontaneous in the forward direction. Several examples are provided to illustrate how the signs of ΔH and ΔS impact the sign of ΔG and spontaneity.
Chem 2 - Free Energy and the Equilbrium Constant K VIII
This document discusses the relationship between the standard Gibbs free energy (ΔG°) and the equilibrium constant (K) for a chemical reaction. It states that ΔG° = -RTlnK, and that the value of K can be used to determine if ΔG° is positive or negative. It also distinguishes between ΔG°, the standard free energy which does not change, and ΔG, the actual free energy under non-standard conditions which does change over the course of a reaction.
Chem 2 - The Second Law of Thermodynamics: Entropy and Heat IV
The document discusses entropy and the Second Law of Thermodynamics. It explains that entropy increases with increasing temperature as heat is added to a system and the number of accessible energy states increases. It provides examples of how entropy increases for phase transitions like melting (fusion) and vaporization, as molecules gain more freedom of movement and positions when changing phases from solid to liquid to gas. The entropy change is positive for these spontaneous phase transitions as disorder and accessible states increase.
Chem 2 - The Second Law of Thermodynamics: Predicting Entropy Changes Qualita...
This document discusses the Second Law of Thermodynamics and predicting changes in entropy. It provides examples of how increasing volume leads to increased entropy due to more possible particle positions. Dissolving solids and diluting solutions are also described as increasing entropy. Finally, an example chemical reaction shows how converting gases to solids decreases entropy by removing thermal disorder of the gas phase.
Chem 2 - The Second Law of Termodynamics: Entropy Microstates and the Boltzma...
This document discusses entropy, microstates, and the Boltzmann equation as it relates to the Second Law of Thermodynamics. It provides examples to demonstrate how to calculate the number of microstates and changes in entropy. Specifically, it explains that entropy is related to the number of possible microscopic arrangements or "microstates" of a system. The Boltzmann equation relates the microscopic number of microstates to the macroscopic property of entropy. Examples are provided to show how to calculate the initial and final number of microstates for a system, and use the Boltzmann equation to determine the change in entropy.
Chem 2 - Acid-Base Equilibria VI: Weak Base Equilibria and Kb - Calculating p...
Chem 2 - Acid-Base Equilibria VI: Weak Base Equilibria and Kb - Calculating pH and pOH for a Weak Base Solution
Chem 2 - Acid-Base Equilibria V: Weak Acid Equilibria and Calculating the pH ...
This document discusses calculating the pH of weak acid solutions. It explains that weak acids only partially dissociate into hydronium ions and conjugate base ions according to an equilibrium reaction. The equilibrium constant Ka relates the concentrations of these species. An example problem calculates the pH of a 0.25 M nitric acid solution using its Ka value, finding the hydronium ion concentration to be 1.07 × 10-2 M and the pH to be 1.97. It also calculates the percent dissociation of the weak acid.
Chem 2 - Acid-Base Equilibria IV: Calculating the pH of Strong Acids versus W...
This document discusses the differences between strong acids and weak acids in aqueous solutions and calculating pH. It states that strong acids, like HCl, completely dissociate in water, resulting in hydronium ion concentrations equal to the original acid concentration. Therefore, the pH of a strong acid solution can be calculated directly from its concentration. Weak acids, like HF, exist in an equilibrium with their dissociated and undissociated forms. Their pH cannot be determined directly and requires calculating equilibrium concentrations. The document gives the example of calculating the pH of a 0.05 M HI solution as 1.30 since HI is a strong acid.
More from Lumen Learning (20)
The Second Law of Thermodynamics: Entropy and Heat IV
The Second Law of Thermodynamics: Entropy and Heat IV
Chem 2 - Third Law of Thermodynamics and Standard Molar Entropy V
Chem 2 - Third Law of Thermodynamics and Standard Molar Entropy V
Chem 2 - The Second Law of Thermodynamics: Spontaneous Reactions and Entropy S I
Chem 2 - The Second Law of Thermodynamics: Spontaneous Reactions and Entropy S I
Chem 2 - Gibbs Free Energy and Spontaneous Reactions VI
Chem 2 - Gibbs Free Energy and Spontaneous Reactions VI
Chem 2 - Free Energy and the Equilbrium Constant K VIII
Chem 2 - Free Energy and the Equilbrium Constant K VIII
Chem 2 - The Second Law of Thermodynamics: Entropy and Heat IV
Chem 2 - The Second Law of Thermodynamics: Entropy and Heat IV
Chem 2 - The Second Law of Thermodynamics: Predicting Entropy Changes Qualita...
Chem 2 - The Second Law of Thermodynamics: Predicting Entropy Changes Qualita...
Chem 2 - The Second Law of Termodynamics: Entropy Microstates and the Boltzma...
Chem 2 - The Second Law of Termodynamics: Entropy Microstates and the Boltzma...
Chem 2 - Acid-Base Equilibria VI: Weak Base Equilibria and Kb - Calculating p...
Chem 2 - Acid-Base Equilibria VI: Weak Base Equilibria and Kb - Calculating p...
Chem 2 - Acid-Base Equilibria V: Weak Acid Equilibria and Calculating the pH ...
Chem 2 - Acid-Base Equilibria V: Weak Acid Equilibria and Calculating the pH ...
Chem 2 - Acid-Base Equilibria IV: Calculating the pH of Strong Acids versus W...
Chem 2 - Acid-Base Equilibria IV: Calculating the pH of Strong Acids versus W...
Recently uploaded
How to deliver Powerpoint Presentations.pptx
"How to make and deliver dynamic presentations by making it more interactive to captivate your audience attention"
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
Geography as discipline
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh - RAYH...
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh
Bossa N’ Roll Records by Ismael Vazquez.
Bossa N Roll Records presentation by Izzy Vazquez for Music Retail and Distribution class at Full Sail University
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
Physical pharmaceutics notes for B.pharm students
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
How to Predict Vendor Bill Product in Odoo 17
This slide will guide us through the process of predicting vendor bill products based on previous purchases from the vendor in Odoo 17.
Benner "Expanding Pathways to Publishing Careers"
This presentation was provided by Rebecca Benner, Ph.D., of the American Society of Anesthesiologists, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...Nguyen Thanh Tu Collection
https://app.box.com/s/qhtvq32h4ybf9t49ku85x0n3xl4jhr15Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
(𝐓𝐋𝐄 𝟏𝟎𝟎) (𝐋𝐞𝐬𝐬𝐨𝐧 𝟏)-𝐏𝐫𝐞𝐥𝐢𝐦𝐬
𝐃𝐢𝐬𝐜𝐮𝐬𝐬 𝐭𝐡𝐞 𝐄𝐏𝐏 𝐂𝐮𝐫𝐫𝐢𝐜𝐮𝐥𝐮𝐦 𝐢𝐧 𝐭𝐡𝐞 𝐏𝐡𝐢𝐥𝐢𝐩𝐩𝐢𝐧𝐞𝐬:
- Understand the goals and objectives of the Edukasyong Pantahanan at Pangkabuhayan (EPP) curriculum, recognizing its importance in fostering practical life skills and values among students. Students will also be able to identify the key components and subjects covered, such as agriculture, home economics, industrial arts, and information and communication technology.
𝐄𝐱𝐩𝐥𝐚𝐢𝐧 𝐭𝐡𝐞 𝐍𝐚𝐭𝐮𝐫𝐞 𝐚𝐧𝐝 𝐒𝐜𝐨𝐩𝐞 𝐨𝐟 𝐚𝐧 𝐄𝐧𝐭𝐫𝐞𝐩𝐫𝐞𝐧𝐞𝐮𝐫:
-Define entrepreneurship, distinguishing it from general business activities by emphasizing its focus on innovation, risk-taking, and value creation. Students will describe the characteristics and traits of successful entrepreneurs, including their roles and responsibilities, and discuss the broader economic and social impacts of entrepreneurial activities on both local and global scales.
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"National Information Standards Organization (NISO)
This presentation was provided by Racquel Jemison, Ph.D., Christina MacLaughlin, Ph.D., and Paulomi Majumder. Ph.D., all of the American Chemical Society, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.Wound healing PPT
This document provides an overview of wound healing, its functions, stages, mechanisms, factors affecting it, and complications.
A wound is a break in the integrity of the skin or tissues, which may be associated with disruption of the structure and function.
Healing is the body’s response to injury in an attempt to restore normal structure and functions.
Healing can occur in two ways: Regeneration and Repair
There are 4 phases of wound healing: hemostasis, inflammation, proliferation, and remodeling. This document also describes the mechanism of wound healing. Factors that affect healing include infection, uncontrolled diabetes, poor nutrition, age, anemia, the presence of foreign bodies, etc.
Complications of wound healing like infection, hyperpigmentation of scar, contractures, and keloid formation.
Recently uploaded (20)
REASIGNACION 2024 UGEL CHUPACA 2024 UGEL CHUPACA.pdf
REASIGNACION 2024 UGEL CHUPACA 2024 UGEL CHUPACA.pdf
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh - RAYH...
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh - RAYH...
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering.pptx
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) Curriculum
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
Naming ionic compounds cations anions
- 1. Naming Ionic Compounds Part 3: Naming Cations and Anions By Shawn P. Shields, Ph.D. This work is licensed by Shawn P. Shields-Maxwell under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License.
- 2. Learning to Name Ionic Compounds In part 2, we learned to write the empirical formula for ionic compounds. Our example: KBr In order to name this compound, we need to know how to name cations and anions separately.
- 3. Naming Cations Rule 1: Naming main group cations Cation names are the same as the element name. For instance, Na+ is a “sodium” cation Mg2+ is a “magnesium” cation
- 4. Naming Transition Metal Cations Rule 2: Naming transition metal cations: Transition metal cations are named just like the main group cations, except the charge on the ion is added in Roman numerals in parentheses after the cation (element) name. For instance, Cu+ is a “copper (I)” cation Cu2+ is a “copper (II)” cation Caution: Do NOT indicate charges in parentheses for main group cations, such as Na+, Mg2+, Al3+, etc. These elements only have one cation charge.
- 5. Mini Quiz: Naming Cations Name the following cations: Au+ Ca2+ Fe2+ Al3+ HINT: Remember to identify whether an element a main group metal or transition metal before naming the cation.
- 6. Mini Quiz Solution: Naming Cations Name the following cations: Au+ is a “gold (I)” cation
- 7. Mini Quiz Solution: Naming Cations Name the following cations: Au+ is a “gold (I)” cation Ca2+ is a “calcium” cation
- 8. Mini Quiz Solution: Naming Cations Name the following cations: Au+ is a “gold (I)” cation Ca2+ is a “calcium” cation Fe2+ is an “iron (II)” cation
- 9. Mini Quiz Solution: Naming Cations Name the following cations: Au+ is a “gold (I)” cation Ca2+ is a “calcium” cation Fe2+ is an “iron (II)” cation Al3+ is an “aluminium” cation NOTE: It is incorrect to name Al3+ as “aluminium (III)” and Ca2+ as “calcium (II)”
- 10. Naming Anions Rule 3: Naming anions Anion names are formed from the root of the element name with the suffix –ide added. For instance, Cl is formed from the element chlorine. Remove the –ine ending and add -ide a “chloride” anion
- 11. Naming Anions More examples: F is formed from the element Fluorine. Remove the –ine ending and add -ide a “Fluoride” anion O2 is formed from the element oxygen. Remove the –ygen ending and add -ide an “oxide” anion
- 12. Mini Quiz: Naming Anions Name the following anions: Br S2 Se2 I
- 13. Mini Quiz Solutions: Naming Anions Name the following anions: Br is formed from bromine. Brom- is the root name of the element. Remove the –ine and add –ide “Bromide” anion S2
- 14. Mini Quiz Solutions: Naming Anions Name the following anions: Br is formed from bromine. Brom- is the root name of the element. Remove the –ine and add –ide “Bromide” anion S2 is formed from sulfur. Sulf- is the root name of the element. Remove the –ur and add –ide “Sulfide” anion
- 15. Mini Quiz Solutions: Naming Anions Se2 is formed from selenium. Selen- is the root name of the element. Remove the –ium and add -ide “Selenide” anion
- 16. Mini Quiz Solutions: Naming Anions Se2 is formed from selenium. Selen- is the root name of the element. Remove the –ium and add -ide “Selenide” anion I is formed from iodine. Iod- is the root name of the element. Remove the –ine and add -ide “Iodide” anion