This document provides objectives and content for a chemistry unit on ionic and molecular compounds. The objectives include describing how ions combine to form compounds, writing formulas, determining compound types, naming compounds, writing formulas for compounds containing polyatomic ions, determining ion charges, naming compounds from formulas, and testing ions in solutions. The content reviews ionic bonding, writing formulas, naming binary ionic compounds and those containing polyatomic ions, determining ion charges, acid and base naming, and molecular compound naming. It also outlines labs to identify common ions and practice these skills.
Chemical nomenclature is the system used to name chemical compounds. It allows chemists to communicate effectively. The name of a compound provides information about its structure. There are currently 114 known elements, some of which are gases while most are solids. In the early 1800s, Berzelius established the modern system of using the first letter of the element's name as its symbol. Chemical formulas represent the elements in a compound along with subscript numbers indicating mole ratios. Empirical formulas provide the simplest whole number ratio of atoms in a compound, while molecular formulas give the exact number of atoms in a molecule.
Chpt 7 part 1 - chemical nomenclature 042403phspsquires
The document provides an overview of chemical nomenclature and naming conventions for compounds. It discusses the need for a systematic naming system to 1) prevent confusion between compounds, 2) avoid complex formulas, and 3) group similar compounds into families. It then covers naming conventions for binary compounds containing two nonmetals, binary compounds containing a metal and nonmetal, and compounds named using the "ic/ous" method involving metal oxidation states. The goal is to establish a logical and consistent system for naming chemical compounds based on their formulas and elemental components.
This document provides rules for naming inorganic compounds, including binary molecular compounds, ionic compounds, oxyanions, and acids. It explains that Greek prefixes are used to indicate the number of elements in binary compounds, with the more electronegative element written last with an -ide ending. For ionic compounds, the cation name comes first followed by the anion name with -ide ending. Oxyanion names follow patterns with -ate, -ite, per-, and hypo- prefixes indicating oxygen content. Acid names are derived from the related anion name by changing endings to -ic or -ous according to specific rules outlined in the document.
To name ionic compounds, the name of the metal is written followed by the nonmetal with the suffix -ide. For transition metals, the oxidation state of the metal ion is indicated in Roman numerals in parentheses. To name compounds containing polyatomic ions, the name of the metal is written followed by the name of the polyatomic ion. For covalent compounds, the least electronegative element is named first along with a prefix to indicate the number of atoms, then the most electronegative element followed by a suffix of -ide and a prefix to indicate its number of atoms.
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.
1) The document discusses predicting ionic charges and writing formulas for ionic compounds.
2) It provides examples of determining the empirical and molecular formulas for different compounds.
3) The key steps shown are calculating formula mass, percentage composition, and determining empirical formulas based on the mass percentages of elements in a compound.
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.
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.
Chemical nomenclature is the system used to name chemical compounds. It allows chemists to communicate effectively. The name of a compound provides information about its structure. There are currently 114 known elements, some of which are gases while most are solids. In the early 1800s, Berzelius established the modern system of using the first letter of the element's name as its symbol. Chemical formulas represent the elements in a compound along with subscript numbers indicating mole ratios. Empirical formulas provide the simplest whole number ratio of atoms in a compound, while molecular formulas give the exact number of atoms in a molecule.
Chpt 7 part 1 - chemical nomenclature 042403phspsquires
The document provides an overview of chemical nomenclature and naming conventions for compounds. It discusses the need for a systematic naming system to 1) prevent confusion between compounds, 2) avoid complex formulas, and 3) group similar compounds into families. It then covers naming conventions for binary compounds containing two nonmetals, binary compounds containing a metal and nonmetal, and compounds named using the "ic/ous" method involving metal oxidation states. The goal is to establish a logical and consistent system for naming chemical compounds based on their formulas and elemental components.
This document provides rules for naming inorganic compounds, including binary molecular compounds, ionic compounds, oxyanions, and acids. It explains that Greek prefixes are used to indicate the number of elements in binary compounds, with the more electronegative element written last with an -ide ending. For ionic compounds, the cation name comes first followed by the anion name with -ide ending. Oxyanion names follow patterns with -ate, -ite, per-, and hypo- prefixes indicating oxygen content. Acid names are derived from the related anion name by changing endings to -ic or -ous according to specific rules outlined in the document.
To name ionic compounds, the name of the metal is written followed by the nonmetal with the suffix -ide. For transition metals, the oxidation state of the metal ion is indicated in Roman numerals in parentheses. To name compounds containing polyatomic ions, the name of the metal is written followed by the name of the polyatomic ion. For covalent compounds, the least electronegative element is named first along with a prefix to indicate the number of atoms, then the most electronegative element followed by a suffix of -ide and a prefix to indicate its number of atoms.
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.
1) The document discusses predicting ionic charges and writing formulas for ionic compounds.
2) It provides examples of determining the empirical and molecular formulas for different compounds.
3) The key steps shown are calculating formula mass, percentage composition, and determining empirical formulas based on the mass percentages of elements in a compound.
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.
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.
Chapter 7.1 : Chemical Names and FormulasChris Foltz
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.
The document discusses chemical nomenclature, which is the system used to name chemical compounds. It describes the rules for naming ionic compounds, molecular compounds, acids, and binary ionic and molecular compounds. Key aspects covered include naming cations and anions, identifying if a compound is ionic or molecular, and applying prefixes and suffixes in naming different compound types.
The document provides information on naming and writing formulas for different types of compounds including:
1) Binary ionic compounds, ionic compounds with multivalent metals, ionic compounds with polyatomic ions, acids, hydrated salts, acid salts, and double salts.
2) Molecular compounds consisting of non-metals are also covered, with prefixes converted to subscripts in formulas.
3) Key concepts include identifying cation/anion charges, recognizing polyatomic ions, and applying naming conventions based on compound type.
Chemistry - Chp 9 - Chemical Names and Formulas - PowerPointMr. Walajtys
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.
Chemistry - Chp 9 - Chemical Names and Formulas - NotesMr. Walajtys
1) This document provides information on naming and writing formulas for ionic and molecular compounds. It discusses monatomic and polyatomic ions, and how to determine the charges on cations and anions.
2) Rules are provided for writing formulas and naming ionic compounds, including those containing transition metals. Prefixes are introduced for naming molecular compounds based on the number of atoms present.
3) Examples are worked through for writing formulas from names and names from formulas for different types of compounds. Practice problems are also included for students to try.
This document provides an overview of the general rules for naming compounds in chemistry. It discusses four main rules:
1) For compounds with metals in groups 1, 2, or 13, simply name the elements.
2) For compounds with metals in groups 3-12 or 14-16, include the metal's charge as a Roman numeral in parentheses.
3) For compounds of nonmetals, use prefixes to indicate the number of atoms and designate one element as the cation.
4) For acids containing hydrogen, add prefixes like "hydro" and suffixes like "ic" or "ous" to indicate the anion. Exceptions are made for polyatomic ions which keep their own names.
The document discusses naming molecular compounds and writing their formulas. It explains that molecular compounds contain only non-metals or metalloids and their naming follows certain prefixes to indicate the number of each atom. The prefixes are mono, di, tri, tetra etc. It provides examples of naming compounds from their formulas like NO2 as nitrogen dioxide and writing formulas from names like carbon tetrachloride as CCl4.
This document provides instructions on writing chemical formulas. It explains that chemical symbols represent elements and come from the element name. Subscript numbers indicate the number of atoms in a compound. Ionic formulas are written with the metal first followed by the nonmetal and hyphenated name. Covalent prefixes like mono, di and tri are used to denote the number of atoms bonded to the central element. Roman numerals specify the metal's oxidation state in some compounds. The document uses examples to demonstrate how to apply these rules to write correct chemical formulas.
This document provides an overview of inorganic chemical nomenclature. It discusses the naming of elements, ions, binary compounds including hydrides, oxides, peroxides, halides, hydroxides, oxoacids and oxosalts. Different naming systems are covered, including compositional, stoichiometric, oxidation number, traditional and IUPAC nomenclature. Key concepts covered include oxidation numbers, types of ions, writing formulas for binary compounds, and distinguishing features of different compound classes.
This document discusses writing formulas for ionic compounds and naming ionic compounds and oxyanions. It provides rules for determining the formula unit of ionic compounds based on the ratio of ions present. Cation symbols are always written first, followed by anion symbols. Subscripts indicate the number of each ion. Polyatomic ions act as individual units in formulas. Oxyanions contain nonmetals bonded to oxygen. Five rules are provided for naming ionic compounds based on cation and anion names and oxidation states.
The document discusses the nomenclature of inorganic compounds according to IUPAC rules. It covers naming conventions for binary ionic compounds such as metal oxides, salts, metal hydrides, non-metal halides, and binary acids. It also discusses determining oxidation states and writing chemical formulas. Key points include naming metal oxides as "stock name of metal cation" + "oxide", salts as "stock name of metal cation" + "root name of non-metal anion" + "-ide", and distinguishing between ionic and molecular compounds in nomenclature.
The document discusses naming conventions and rules for molecular and ionic compounds. It describes how to determine the formula mass from atomic masses and how to write formulas based on the order of elements. It provides rules for naming binary ionic compounds, acids, and compounds containing polyatomic ions based on their formulas.
This document provides an overview of chemical nomenclature and naming conventions for different types of chemical compounds. It discusses naming rules for ionic compounds, molecular compounds, acids, and bases. For ionic compounds, it describes how to name binary ionic compounds and polyatomic compounds based on the cation and anion present. It also addresses naming metal ions with different oxidation states. For molecular compounds, it outlines using prefixes to indicate the number of each type of atom. The document concludes with sections on naming simple acids based on replacing the nonmetal element ending with "-ic acid" and an overview of oxoacids and bases.
This document provides an overview of key concepts in atomic structure and chemical bonding:
- It describes early theories of atoms proposed by thinkers like Democritus, Dalton, and Thomson. Experiments by Thomson, Millikan, and Rutherford provided evidence for the atom's internal structure.
- The document defines subatomic particles like protons, neutrons, and electrons. It introduces concepts like isotopes, ions, ionic and covalent bonding.
- Naming conventions for ions, ionic compounds, acids, and hydrates are outlined. Rules for writing chemical formulas are also summarized.
- Key models and experiments that advanced understanding of atomic structure are highlighted, including Dalton's atomic theory and the discoveries of the
The document discusses 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.
The document provides instructions for naming ionic and binary covalent compounds. Ionic compounds are formed from metals and nonmetals, with the metal ions taking positive charges and the nonmetal ions taking negative charges. Binary covalent compounds are formed from two nonmetals sharing electrons in ratios indicated by prefixes like di-, tri-, and tetra-. The naming process for ionic compounds involves writing the name of the metal ion followed by the name of the nonmetal ion. For binary covalent compounds, the process involves writing the names of the two nonmetals, changing the second to end in "-ide", and adding prefixes to indicate ratios.
This document discusses the nomenclature and formation of inorganic compounds. It focuses on binary compounds such as oxides, hydrates, hydroxides, acids and salts formed from metals and nonmetals. Specifically, it describes the naming and formation of haloid salts through the reaction of metals with nonmetallic halogens such as fluorine, chlorine and bromine. Examples of naming haloid salts using IUPAC nomenclature rules and balancing chemical equations for their formation are provided.
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.
This document provides information about atomic structure:
1. It explains that atoms are made up of even smaller particles called subatomic particles, including protons, neutrons, and electrons.
2. Protons and neutrons are located at the center of the atom in a dense core called the nucleus. Electrons orbit around the outside of the atom.
3. Atoms have an overall neutral charge because they contain an equal number of positively charged protons and negatively charged electrons. Neutrons have no charge.
This document provides information about naming ionic and molecular compounds. It discusses atomic number, mass number, and isotopes. It explains that ions are formed when atoms gain or lose electrons to become positively or negatively charged. The document outlines rules for writing chemical formulas, including ionic formulas which involve balancing charges between cations and anions. It also discusses naming conventions for ionic compounds based on metal cations and nonmetal anions. The document concludes by stating that molecular compounds consist of nonmetals and do not involve ion formation.
Chemistry is involved with various and diverse interactions of matter either around us or simply inside the laboratory. These are described using the language of chemistry which consists of symbols, formulas and equations.
Chapter 7.1 : Chemical Names and FormulasChris Foltz
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.
The document discusses chemical nomenclature, which is the system used to name chemical compounds. It describes the rules for naming ionic compounds, molecular compounds, acids, and binary ionic and molecular compounds. Key aspects covered include naming cations and anions, identifying if a compound is ionic or molecular, and applying prefixes and suffixes in naming different compound types.
The document provides information on naming and writing formulas for different types of compounds including:
1) Binary ionic compounds, ionic compounds with multivalent metals, ionic compounds with polyatomic ions, acids, hydrated salts, acid salts, and double salts.
2) Molecular compounds consisting of non-metals are also covered, with prefixes converted to subscripts in formulas.
3) Key concepts include identifying cation/anion charges, recognizing polyatomic ions, and applying naming conventions based on compound type.
Chemistry - Chp 9 - Chemical Names and Formulas - PowerPointMr. Walajtys
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.
Chemistry - Chp 9 - Chemical Names and Formulas - NotesMr. Walajtys
1) This document provides information on naming and writing formulas for ionic and molecular compounds. It discusses monatomic and polyatomic ions, and how to determine the charges on cations and anions.
2) Rules are provided for writing formulas and naming ionic compounds, including those containing transition metals. Prefixes are introduced for naming molecular compounds based on the number of atoms present.
3) Examples are worked through for writing formulas from names and names from formulas for different types of compounds. Practice problems are also included for students to try.
This document provides an overview of the general rules for naming compounds in chemistry. It discusses four main rules:
1) For compounds with metals in groups 1, 2, or 13, simply name the elements.
2) For compounds with metals in groups 3-12 or 14-16, include the metal's charge as a Roman numeral in parentheses.
3) For compounds of nonmetals, use prefixes to indicate the number of atoms and designate one element as the cation.
4) For acids containing hydrogen, add prefixes like "hydro" and suffixes like "ic" or "ous" to indicate the anion. Exceptions are made for polyatomic ions which keep their own names.
The document discusses naming molecular compounds and writing their formulas. It explains that molecular compounds contain only non-metals or metalloids and their naming follows certain prefixes to indicate the number of each atom. The prefixes are mono, di, tri, tetra etc. It provides examples of naming compounds from their formulas like NO2 as nitrogen dioxide and writing formulas from names like carbon tetrachloride as CCl4.
This document provides instructions on writing chemical formulas. It explains that chemical symbols represent elements and come from the element name. Subscript numbers indicate the number of atoms in a compound. Ionic formulas are written with the metal first followed by the nonmetal and hyphenated name. Covalent prefixes like mono, di and tri are used to denote the number of atoms bonded to the central element. Roman numerals specify the metal's oxidation state in some compounds. The document uses examples to demonstrate how to apply these rules to write correct chemical formulas.
This document provides an overview of inorganic chemical nomenclature. It discusses the naming of elements, ions, binary compounds including hydrides, oxides, peroxides, halides, hydroxides, oxoacids and oxosalts. Different naming systems are covered, including compositional, stoichiometric, oxidation number, traditional and IUPAC nomenclature. Key concepts covered include oxidation numbers, types of ions, writing formulas for binary compounds, and distinguishing features of different compound classes.
This document discusses writing formulas for ionic compounds and naming ionic compounds and oxyanions. It provides rules for determining the formula unit of ionic compounds based on the ratio of ions present. Cation symbols are always written first, followed by anion symbols. Subscripts indicate the number of each ion. Polyatomic ions act as individual units in formulas. Oxyanions contain nonmetals bonded to oxygen. Five rules are provided for naming ionic compounds based on cation and anion names and oxidation states.
The document discusses the nomenclature of inorganic compounds according to IUPAC rules. It covers naming conventions for binary ionic compounds such as metal oxides, salts, metal hydrides, non-metal halides, and binary acids. It also discusses determining oxidation states and writing chemical formulas. Key points include naming metal oxides as "stock name of metal cation" + "oxide", salts as "stock name of metal cation" + "root name of non-metal anion" + "-ide", and distinguishing between ionic and molecular compounds in nomenclature.
The document discusses naming conventions and rules for molecular and ionic compounds. It describes how to determine the formula mass from atomic masses and how to write formulas based on the order of elements. It provides rules for naming binary ionic compounds, acids, and compounds containing polyatomic ions based on their formulas.
This document provides an overview of chemical nomenclature and naming conventions for different types of chemical compounds. It discusses naming rules for ionic compounds, molecular compounds, acids, and bases. For ionic compounds, it describes how to name binary ionic compounds and polyatomic compounds based on the cation and anion present. It also addresses naming metal ions with different oxidation states. For molecular compounds, it outlines using prefixes to indicate the number of each type of atom. The document concludes with sections on naming simple acids based on replacing the nonmetal element ending with "-ic acid" and an overview of oxoacids and bases.
This document provides an overview of key concepts in atomic structure and chemical bonding:
- It describes early theories of atoms proposed by thinkers like Democritus, Dalton, and Thomson. Experiments by Thomson, Millikan, and Rutherford provided evidence for the atom's internal structure.
- The document defines subatomic particles like protons, neutrons, and electrons. It introduces concepts like isotopes, ions, ionic and covalent bonding.
- Naming conventions for ions, ionic compounds, acids, and hydrates are outlined. Rules for writing chemical formulas are also summarized.
- Key models and experiments that advanced understanding of atomic structure are highlighted, including Dalton's atomic theory and the discoveries of the
The document discusses 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.
The document provides instructions for naming ionic and binary covalent compounds. Ionic compounds are formed from metals and nonmetals, with the metal ions taking positive charges and the nonmetal ions taking negative charges. Binary covalent compounds are formed from two nonmetals sharing electrons in ratios indicated by prefixes like di-, tri-, and tetra-. The naming process for ionic compounds involves writing the name of the metal ion followed by the name of the nonmetal ion. For binary covalent compounds, the process involves writing the names of the two nonmetals, changing the second to end in "-ide", and adding prefixes to indicate ratios.
This document discusses the nomenclature and formation of inorganic compounds. It focuses on binary compounds such as oxides, hydrates, hydroxides, acids and salts formed from metals and nonmetals. Specifically, it describes the naming and formation of haloid salts through the reaction of metals with nonmetallic halogens such as fluorine, chlorine and bromine. Examples of naming haloid salts using IUPAC nomenclature rules and balancing chemical equations for their formation are provided.
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.
This document provides information about atomic structure:
1. It explains that atoms are made up of even smaller particles called subatomic particles, including protons, neutrons, and electrons.
2. Protons and neutrons are located at the center of the atom in a dense core called the nucleus. Electrons orbit around the outside of the atom.
3. Atoms have an overall neutral charge because they contain an equal number of positively charged protons and negatively charged electrons. Neutrons have no charge.
This document provides information about naming ionic and molecular compounds. It discusses atomic number, mass number, and isotopes. It explains that ions are formed when atoms gain or lose electrons to become positively or negatively charged. The document outlines rules for writing chemical formulas, including ionic formulas which involve balancing charges between cations and anions. It also discusses naming conventions for ionic compounds based on metal cations and nonmetal anions. The document concludes by stating that molecular compounds consist of nonmetals and do not involve ion formation.
Chemistry is involved with various and diverse interactions of matter either around us or simply inside the laboratory. These are described using the language of chemistry which consists of symbols, formulas and equations.
This PowerPoint document provides an overview of chemical reactions for a Year 10 science class. It discusses the structure of atoms, chemical bonds, ions, and writing chemical formulas. The summary is:
1) It introduces chemical reactions and the structure of atoms made up of protons, neutrons, and electrons.
2) Students learn about ions, chemical bonds, and writing formulas for ionic and covalent compounds by balancing charges between reactants.
3) The document provides examples of naming compounds and common polyatomic ions, explaining how to write formulas that include multiple ions.
This document provides an overview of basic chemistry concepts related to naming and writing formulas for ionic compounds. It discusses:
1) How to name ionic compounds by writing the cation first followed by the anion with "-ide" ending, except for polyatomic ions.
2) How to write formulas for ionic compounds by ensuring charges are balanced between cations and anions using subscripts.
3) Special rules for writing formulas involving polyatomic ions and d-block metal cations, which can have multiple oxidation states requiring specifying the oxidation number.
4) How to calculate formula masses of compounds by multiplying the number of atoms of each element by the atomic mass and summing the products.
The document discusses the concepts of constant composition of pure substances and the molecular basis for this observation. It specifically addresses:
- Pure substances have a constant ratio of elements regardless of sample size due to their molecular makeup.
- Compounds are made of molecules with specific numbers and types of atoms, so every sample contains identical molecules.
- The document provides examples of using formulas to represent compounds and determining the number of atoms present. It also discusses classifying different types of elements and compounds.
The document provides information on naming and writing formulas for various types of chemical compounds including:
- Monoatomic ions and how they are named based on their group number and charge.
- Transition metal ions and how their charge is indicated using Roman numerals.
- Polyatomic ions which contain more than one atom and have different naming conventions based on their ending.
- Binary ionic compounds and how to write their formulas by balancing the charges of the ions using subscripts.
- Molecular and acidic compounds and how the prefixes and suffixes in their names relate to the number of atoms in their formulas.
The document also discusses the laws of definite and multiple proportions and provides examples of writing word equations for
This document discusses the nomenclature (naming systems) for inorganic compounds, which differ depending on whether the compound is ionic or molecular. For ionic compounds, the cation is named first followed by the anion. Binary ionic compounds consisting of a metal and nonmetal are generally named by removing the ending from the nonmetal and adding -ide. For transition metals that form multiple ions, the modern system uses Roman numerals in parentheses after the metal to indicate charge. Molecular compounds are named by identifying the number of atoms of each element present using prefixes, and adding -ide to the second element. Several elements exist as diatomic molecules like H2, N2, O2, F2, Cl2, Br
This document discusses chemical formulas and compounds. It covers:
- The importance of chemical formulas in showing elemental composition compared to common names.
- How to write formulas for binary compounds and name them.
- Charges of transition metals and how they are represented in names using Roman numerals.
- Writing formulas for compounds containing polyatomic ions by treating them as whole units.
- Naming molecular compounds using prefixes to indicate number of atoms.
- Common acids and how to name salts containing acid anions.
- Oxidation numbers and how to determine them based on element properties and charge balance.
The document contains a word scramble activity using element symbols. It provides the scrambled element combinations and clues to figure out 4 words. The answers are:
1. RETINA (Sodium + Titanium + Rhenium)
2. PERSON (Sulfur + Nitrogen + Phosphorous + Oxygen + Erbium)
3. CABIN (Calcium + Indium + Boron)
4. POKER (Erbium + Polonium + Potassium)
The document contains a word scramble activity using element symbols. It provides the scrambled element combinations and clues to figure out 4 words. The answers are:
1. RETINA (Sodium + Titanium + Rhenium)
2. PERSON (Sulfur + Nitrogen + Phosphorous + Oxygen + Erbium)
3. CABIN (Calcium + Indium + Boron)
4. POKER (Erbium + Polonium + Potassium)
This document provides instructions on writing chemical formulas. It explains that chemical symbols represent elements and come from element names. Subscript numbers indicate the number of atoms in a compound. Ionic formulas are written with the metal first followed by the nonmetal and hyphenated name. Covalent prefixes like mono, di and tri are used to denote the number of non-metal atoms bonded to the central atom. Roman numerals specify the metal's oxidation state in some compounds. The document uses examples to demonstrate how to apply these rules to write formulas for ionic and covalent compounds.
This document provides information about groups, periods, and electrons on the periodic table. It discusses how elements in the same group have the same number of valence electrons and will therefore react similarly. It gives examples of sodium and potassium both having one valence electron. It also discusses how atoms gain or lose electrons to form ions, and how the periodic table is organized by increasing atomic number.
1. The document discusses naming ionic and covalent compounds. It provides steps for naming ionic compounds, which involve writing the name of the metal ion and nonmetal ion. Covalent compounds are named by writing the names of the nonmetals and adding prefixes to indicate ratios.
2. Binary covalent compounds are between two nonmetals and are named using prefixes like mono, di, and tri to show ratios of elements. Polyatomic ions are also named and used in ionic compounds.
3. Determining if a compound is ionic or covalent depends on whether it contains a metal and nonmetal (ionic) or only nonmetals (covalent).
This document provides instructions for naming ionic and binary covalent compounds. It explains that ionic compounds are formed from metals and nonmetals, while covalent compounds contain only nonmetals. The naming process for ionic compounds involves writing the name of the metal ion followed by the nonmetal ion changed to -ide. For covalent compounds, prefixes are used to indicate the number of each nonmetal present. Practice problems are provided to name compounds and write formulas.
This document provides instructions for naming ionic and binary covalent compounds. It explains that ionic compounds are formed from metals and nonmetals, while covalent compounds contain only nonmetals. The naming process for ionic compounds involves writing the name of the metal ion followed by the nonmetal ion changed to -ide. For covalent compounds, prefixes are used to indicate the number of each nonmetal present.
This document provides information about naming and writing formulas for ionic and molecular compounds. It defines ions and discusses how to predict ionic charges based on location on the periodic table. Rules are explained for naming monoatomic and polyatomic ions as well as cations with multiple possible charges. The document outlines the process for writing formulas for ionic compounds using criss-cross method and provides examples. It also introduces prefixes used for naming molecular compounds and indicates formulas can be determined directly from these prefixes.
This document provides information about naming and writing formulas for different types of chemical compounds including:
1) Ions and how to predict their charges based on location on the periodic table. Common monatomic and polyatomic ions are identified.
2) Ionic compounds - rules for writing formulas based on cation and anion identities and balancing charges. Rules for naming ionic compounds are also outlined.
3) Molecular compounds - uses prefixes to indicate number of each atom in the compound name which then directly provides the formula.
4) Acids - three main rules for identifying if the anion ends in -ide, -ate or -ite and how this determines the acid name and whether a prefix like "hydro
This document provides an overview of chemical reactions including:
1. Key vocabulary like reactants, products, and chemical equations.
2. How to write and balance chemical equations.
3. The five basic types of chemical reactions.
4. Factors that affect the rate of chemical reactions like temperature, concentration, and catalysts.
This document outlines the key concepts to be covered in a Year 11 100 Science course on aspects of acids and bases, including atomic structure, properties of acids and bases, rates of reaction and particle theory, uses of acids and bases, and restrictions on the acids and bases included in the course. Students will study electron configuration, ionic bonding, naming ionic compounds, properties of acids and bases such as releasing hydrogen ions in water and reacting to form salts, and the rates of reactions and particle theory explanations. Assessment will include selected aspects of acids and bases such as atomic structure, properties, uses, and rates of reaction.
Gender and Mental Health - Counselling and Family Therapy Applications and In...PsychoTech Services
A proprietary approach developed by bringing together the best of learning theories from Psychology, design principles from the world of visualization, and pedagogical methods from over a decade of training experience, that enables you to: Learn better, faster!
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
हिंदी वर्णमाला पीपीटी, hindi alphabet PPT presentation, hindi varnamala PPT, Hindi Varnamala pdf, हिंदी स्वर, हिंदी व्यंजन, sikhiye hindi varnmala, dr. mulla adam ali, hindi language and literature, hindi alphabet with drawing, hindi alphabet pdf, hindi varnamala for childrens, hindi language, hindi varnamala practice for kids, https://www.drmullaadamali.com
বাংলাদেশের অর্থনৈতিক সমীক্ষা ২০২৪ [Bangladesh Economic Review 2024 Bangla.pdf] কম্পিউটার , ট্যাব ও স্মার্ট ফোন ভার্সন সহ সম্পূর্ণ বাংলা ই-বুক বা pdf বই " সুচিপত্র ...বুকমার্ক মেনু 🔖 ও হাইপার লিংক মেনু 📝👆 যুক্ত ..
আমাদের সবার জন্য খুব খুব গুরুত্বপূর্ণ একটি বই ..বিসিএস, ব্যাংক, ইউনিভার্সিটি ভর্তি ও যে কোন প্রতিযোগিতা মূলক পরীক্ষার জন্য এর খুব ইম্পরট্যান্ট একটি বিষয় ...তাছাড়া বাংলাদেশের সাম্প্রতিক যে কোন ডাটা বা তথ্য এই বইতে পাবেন ...
তাই একজন নাগরিক হিসাবে এই তথ্য গুলো আপনার জানা প্রয়োজন ...।
বিসিএস ও ব্যাংক এর লিখিত পরীক্ষা ...+এছাড়া মাধ্যমিক ও উচ্চমাধ্যমিকের স্টুডেন্টদের জন্য অনেক কাজে আসবে ...
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
"Learn about all the ways Walmart supports nonprofit organizations.
You will hear from Liz Willett, the Head of Nonprofits, and hear about what Walmart is doing to help nonprofits, including Walmart Business and Spark Good. Walmart Business+ is a new offer for nonprofits that offers discounts and also streamlines nonprofits order and expense tracking, saving time and money.
The webinar may also give some examples on how nonprofits can best leverage Walmart Business+.
The event will cover the following::
Walmart Business + (https://business.walmart.com/plus) is a new shopping experience for nonprofits, schools, and local business customers that connects an exclusive online shopping experience to stores. Benefits include free delivery and shipping, a 'Spend Analytics” feature, special discounts, deals and tax-exempt shopping.
Special TechSoup offer for a free 180 days membership, and up to $150 in discounts on eligible orders.
Spark Good (walmart.com/sparkgood) is a charitable platform that enables nonprofits to receive donations directly from customers and associates.
Answers about how you can do more with Walmart!"
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
-------------------------------------------------------------------------------
Find out more about ISO training and certification services
Training: ISO/IEC 27001 Information Security Management System - EN | PECB
ISO/IEC 42001 Artificial Intelligence Management System - EN | PECB
General Data Protection Regulation (GDPR) - Training Courses - EN | PECB
Webinars: https://pecb.com/webinars
Article: https://pecb.com/article
-------------------------------------------------------------------------------
For more information about PECB:
Website: https://pecb.com/
LinkedIn: https://www.linkedin.com/company/pecb/
Facebook: https://www.facebook.com/PECBInternational/
Slideshare: http://www.slideshare.net/PECBCERTIFICATION
Communicating effectively and consistently with students can help them feel at ease during their learning experience and provide the instructor with a communication trail to track the course's progress. This workshop will take you through constructing an engaging course container to facilitate effective communication.
B. Ed Syllabus for babasaheb ambedkar education university.pdf
Unit 3 lecture s2015
1. Unit 3 Ch 4Objectives:
1. Describe how ions combine to form neutral ionic compounds. 3.5 B SC
12.2.1.a
2. Write formulas for binary compounds. 3.5 B
3. Determine the type of compound: Acid, Base, Salt, or Molecule. 4.1,
4.2, PT
4. Correctly name the 4 types of compounds: acid, base, salt, or
molecule. 4.1 and 4.2, PT
5. Write formulas for compounds containing polyatomic ions, determine
the type of compound, and then correctly naming it. 4.2 SC 12.2.1.a
6. Determine the unknown charge of an ion within a balanced
compound. 4.1 A SC 12.2.1.a & SC 12.2.1.g
7. Name compounds from their formulas. 4.2 C
8. Test for chemical properties of ions to identify them in solutions. Lab
SC 12.2.1.g & SC 12.1.1.a & SC 12.1.1.b & SC 12.1.1.d
3. Unit 2 Test Day lecture
Online test code: 2
Read Pages: pg93-102
When done, start on
Vocabulary, we’ll lecture and
work some new stuff soon
4. Information given in a
formula.
MgCl2
Subscript
How many of each
atom are present?
coefficient
3
Mg +2 Cl-1
Cl-1
Mg +2 Cl-1
Cl-1
Mg +2 Cl-1
Cl-1
5. Information given in a
formula.
Mg(NO3)2
Subscripts
How many of each
atom are present?
Mg +2 NO3
-1
NO3
-1
coefficient
4
Mg +2 NO3
-1
NO3
-1
Mg +2 NO3
-1
NO3
-1
Mg +2 NO3
-1
NO3
-1
6. Can you count Atoms &
ions
Na2O
Ca3PO4
Al2(SO3)4
(NH4)2Cr2O7
You try
Al(C2H302)3
Mo(ClO )
1. how many of each atom?
2.
how many of the various
polyatomic ions groups?
12. Polyatomic ion
a charged molecule (two
or more symbols that carry
a charge)
See the list on the back of the
PT. If you see more that 2
symbols in the formula look at
this list. Be careful though of the
acids.
14. Acid
start with H. Basically a
hydrogen acting as a
cation bonded to an
anion.
(a list is shown on the back
of the PT.) should be able
to name these right away.
15. Ionic (AKA Salts)
will be a cation with an
anion. Metal to nonmetal,
Metal to polyatomic ion, or
polyatomic ion to nonmetal, or
poly to poly
If it begins with a metal, it’s a
salt
If it begins with NH4, it’s a salt
17. Practice identifying (like a pre-test)
What are these? (IMAB or ion)
CaCl2 NO Li+
Li SO2 HCl NH4Cl
Al2(SO4)3 Ca3N2 LiOH
NaF H2SO4 S2O5 I I -1
CH4 I2 C3H8
20. Bonding
Why do elements bond?
Be able to do all objecives
Plan:
Binary I, II & poly
Acid & base* (*special ionic)
Molecule (binary II)
Common ions lab
21. THINKING
A metal bonded to a nonmetal form a
______ bond
Bonding involves only _____ electrons
All atoms want a ____ outer shell of e-s
An atom that has lost of gained e-s is
called ___
Non metal tend to ____ outer shell e-s
Metals tend to ____ outer shell e-s
31. Today in Chemistry -outline
As you come in: Read Lab, Discuss
pg 8-9 (walk by)
Charge on metal in B group salt
Lab
homework. Pg 3 & 12
32. Given a formula find the
roman number and name
How do we find the charge on a metal in a compound?
The simplest answer is to work backwards. We know that
Oxygen has a charge of –2, so how would a –2 and Fe,
come to become a 1 to 1 ratio?
FeO Fe (X)
+ O –2
If you said that Fe would have to have a +2 charge, then
you are correct. The charge on this metal, was +2.
therefore, the name would be Iron(II)Oxide.
33. Really I can teach you 3
ways
Backwards
Pictures
Math method
Let me show you each on the
board with the first couple on the
next slide
37. Charge of the ion or atom in a
compound or ion.
Cu3(PO4)2 (name this)
H2SO4 (charge of S)
C2H3O2
-1
(charge of C)
What is the correct name for
Sn3(PO4)2(whatisthechargeofPinthisbeast?)
41. Goal of the lab
To run standard tests with
common ions and
compare these results to
an unknown sample with
the intent to discover
what is in that unknown
42. Common ions Lab
Do each test one at a time
including the unknown.
# unknown, use little and store as
directed!
Wash everything (use special soap
that has NO ions. and rinse with
distilled H2O
46. sample data 1 I do
Item to
test Positive Negative Unknown A Unknown B
grape juice
bubbles in
Baking Soda
transparent or
clear in BS
clear in BS
yellow gas in
bs
phlegm
clears up and
becomes
transparent in
Acid
yellow gas
bubbles in
acid
bubbles in
acid
black solid in
acid
Slime
black ppt. in
CuCl2
clear in CuCl2
darb brown
ppt in CuCl2
light reg gas in
CuCl2
47. sample data 2 We do
Item to
test Positive Negative Unknown C Unknown D
grape juice
bubbles in
Baking Soda
transparent or
clear in BS
smoke comes
off in BS
clear in BS
phlegm
clears up and
becomes
transparent in
Acid
yellow gas
bubbles in
acid
yellow gas in
Acid
nothing
happened
Slime
black ppt. in
KCl
clear ripple
looking in KCl
Clear in KCl
Dark ppt. in
KCl
48. sample data 3 y’all do
Item to test Positive Negative
apple juice
bubbles in
Ca(OH)2
bubbles in
Ca(OH)2
Blah
clears up and
becomes
transparent in
Acid
yellow gas
bubbles in acid
blood black ppt. in FeO
brownish ppt. in
FeO
49. What questions do you
have?
Quiz
Get unknown (one per group)
Do Lab
Check homework sometime
today or tomorrow
51. After Ions Lab 1
So far: salt naming, acid
naming, ion lab 1,
DISCUSS PAGE 3 IN PACKET &
PG 12
Now: background on some of
these & molecule naming
Ion lab part 2
55. Sample Probs: Charge of the ion or
atom in a compound or ion.
Cu3(PO4)2 (name this)
H2SO4 (charge of S)
C2H3O2
-1
(charge of C)
What is the correct name for
Sn3(PO4)2(whatisthechargeofPinthisbeast?)
59. Ionic
Sometimes called salts
Many times they are white powders, colored powders or
crystals
Ions are charged particles and stick together to make
neutral compounds. (conduct in solution or molten)
Picture on pg. 81. NaCl Show how Na & Cl stack
together in to a cube. NaCl is called a formula unit.
That is the lowest whole number ratio of ions in the compound
60. Ionic (cont.)
Look at charges or oxidation number on the
periodic table.
Metals are + (cations), nonmetals are - (anions)
What is listed on our P.T. is just the most common
charge.
FYI: When they dissolve, the dissociate in to ions
floating around. (ask for a drawing)
62. Ionic compounds & Bonding (formula units)
What does the charge have to
add up to in a compound
(balanced formula)
Metal to nonmetal
Be able to name these and write formulas given a name.
Be able to find and use roman numbers when appropriate.
63. How do we find the roman
number?
3 methods
Backward, picture, or math.
64. Polyatomic ions
Metal w/ Polyatomic ion
Polyatomic to polyatomic
Poly to nonmetal.
Discuss the charges. SO4
–2
(note: the charge on
the whole SO4 is –2
We treat these just like a single unit!
These are
still ionic!
65. Acid
See PT & my packet
What do acid formulas begin with? begin with H
It is a self contained molecule.
HCl
HC2H3O2 acetic acid
H3PO4
H2SO4
I would suggest they memorize the ic acids and
the ate salts they make up.
Many of the polyatomic
ions come from these.
66. Base
Bases are a cation with a hydroxide (which
is a polyatomic ion) These are special salts
Some examples
Sodium hydroxide
Barium hydroxide
Aluminum Hydroxide
NOTE These are ionic and will form
crystals like them.
Name to formula: parenthesis are needed.
67. Molecule
Non metal & non metal
Examples CO2 CH4 N2O5
what is the formula forcarbon tetrachloride
How do these differ from ionic? (they share
electrons)
Diagram (sharing) (PUT ON BOARD)
They don’t have a charge & they become “happy” by
sharing and are a self-contained unit. (we don’t reduce
the formula like we do for Formula units)
No crystal lattice structure like ionic
H O N Cl Br I F (describe how these happen)
DIATOMICS: SEE YOUR P.T. These are the
elements that are not found alone.
70. Naming flowchart
Do you see more than
2 elemental symbols?
Does it begin with H? It’s binary. Does it
start with a metal?
It’s an Acid. Use
the back of
your PT to
name it
It’s a salt. Does
it contain a
metals from a B
group?
Find the charge on
the metal by using
math, working
backward or
drawing a picture.
Use this charge as
a roman number in
the name. Then
follow this by the
anion’s name.
Name the
cation
followed
by the
anion using
the back
of your PT
for the
polynomial
It’s a salt. Does it
contain metals
from the B group?
It’s a molecule. Use
prefixes to name the
number of each
element. There is NO
WORK involved and
no swapping of
charges. Just write
them down.
Name the
cation
followed by
the anion and
it should end
in IDE
Find the charge on
the metal by using
math, working
backward or
drawing a picture.
Use this charge as a
roman number in
the name. Follow
this with the name
of the anion (it
ends in IdE
71. Practice naming & identifying
What are these? (IMAB or ion) Don’t just name
them
Ca(OH)2 NO Li+
SO2 HCl NH4Cl
Al2(SO4)3 (NH4) 3PO4 LiOH
H2SO4 H3PO4
S2O5 K9P NH4IO3
CH4 C3H8 CuC2H3O2
76. AFTER LAB AND REVIEW
THUS FAR
Options:
HUGE QUIZ (additional work for those who struggle)
POSSIBLE Book probs: pg 118-120 6, 8,
13, 19 NOT B, 21, 25, 26, 29 A E H I J K L,
32 Not C
REVIEW FOR TEST
77. What you should be able to
do.
Name to formula, formula to name
What will an atom look like (formula)
Diatomics?
HONClBrIF’s
What will an ion look like? (symbol/formula/name)
What will a salt look like? (symbol/formula/name)
What will a molecule look like?
(symbol/formula/name)
What will an acid look like?
(symbol/formula/name)
78. What you should be able to
do.
How are salts named
How are acids named
How are simple molecules named
How do you find the name of a
polyatomic ion
Which compounds include organic
substances
Carbon is contained in organic substances. FYI
Cations, anions, # p, n, e etc.
Editor's Notes
A couple questionsbefore we start
Roll the dice and move ahead that many spaces. Decide what card to draw. If you land on an anion, draw a cation card and vice versa. EVERYONE DOES THIS next part. Write down the place landed and the card drawn. Determine the charges for each and combine them to make the correct formula. Write the correct formula and name on your worksheet. You will have to write small so you can put all the information in the space provided.
If all the players at your game agree that the roller got the question correct, then the roller can stay on that spot. If not, then they must move back two places. The next player then rolls. Players do not go twice in a row.
Remember each player must write down everything. You should not share answers with each other unless the roller does not get it correct!
If you land on a transition metal (B groups) the roller can select the oxidation number they wish to use for the cation.
After a set time, we will change boards and go with the names board. The rules are the same.
Let’s Work through a couple of these. Pg 10 of packet
What types of things do we test for in the real world?
Obs. Data what might be in each unknown?
What do you see, what is in each unknown? Why?
What do you see? What might be wrong with this data ?