Naming chemical compounds
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This document discusses chemical naming conventions. It explains that chemicals can have common names as well as systematic IUPAC names, and provides examples of chemicals referred to primarily by their common names. It also outlines rules for naming ionic compounds, including writing the metal cation and nonmetal anion, indicating transition metal ion charges with Roman numerals, and using Greek prefixes and suffixes like "-ate" or "-ite" to indicate atom counts and oxygen compounds.
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Naming compounds chemistry
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.
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 Compound
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.
10 naming and formula writing 2012
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.
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.
GC-S010-Nomenclature
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.
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.
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Naming compounds chemistry
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.
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 Compound
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.
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The document provides information on naming and writing formulas for different types of compounds including:
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3) Key concepts include identifying cation/anion charges, recognizing polyatomic ions, and applying naming conventions based on compound type.
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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.
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CH1000 Fundamentals of ChemistryModule 2 – Chapter 6
CH1000
Fundament
als of
Chemistry
Module 2 – Chapter 6
Common and Systematic Names
• Chemical nomenclature is the systematic naming of chemical compounds
• Common names are historical names of compounds which are not based
on systematic rules
• Common names are often used because systematic names are too long
and technical for everyday use
• Chemists prefer systematic names that precisely identify the chemical
composition of compounds.
• Example CaO
• Common name: lime
• Systematic name: calcium oxide
Naming
Flowchart
We will focus on nomenclature of inorganic compounds
Elements and Ions
• The formula for most elements is the symbol of the element off of
the periodic table.
• Diatomic molecules are an exception:
• Two other elements also exist in polyatomic arrangements:
Naming Anions
•Remember from Chapter 5
that any neutral atom that
gains an electron is called
an anion
•When naming anions,
change the element ending
to -ide
Symbols
of the
Elements
•Each element has an
abbreviation called a symbol.
•The first letter of a symbol
must always be capitalized.
•If a second letter is needed, it
should be lowercase.
Predicting Ion
Charge from
Periodic Table
•Metals form cations
•The positive charge is equal
to the group number
Predicting Ion
Charge from
Periodic Table
•Nonmetals form anions
•The negative charge is equal
to 8 – the group number
Writing Formulas from Names of Ionic Compounds
•Ionic compounds contain both a cation and
an anion.
•Ionic compounds must have a net charge of
0
•The sum of charges of the cations and
anions in an ionic compound equal 0
•Rules for writing formulas for ionic
compounds:
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nonmetal ion formula
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of each ion to provide an overall
charge equal to zero
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metal and nonmetal, using subscripts
determined from Step 2 for each ion
Naming Ionic
Binary
Compounds
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a metal which forms only one
cation
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written/named first followed
by the anion
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compounds:
• Name the cation
• Write the anion root and
add the –ide suffix
Naming
Compounds
Containing
Metals with
Multiple
Charges
•Rules for Naming Compounds Involving Metals that Could Form
Multiple Charges
• Write the cation name.
• Write the cation charge in Roman numerals in parentheses.
• Write the root of the anion and use the –ide suffix.
•Exception: for metals that only form two cations, a Latin root with
either an –ous or –ic suffix can also be used.
Formula Name Classical Name Formula Name Classical Name
Cu+ Copper(I) cuprous Sn2+ Tin(II) stannous
Cu2+ Copper(II) cupric Sn4+ Tin(IV) stannic
Fe2+ Iron(II) ferrous Pb2+ Lead(II) plumbous
Fe3+ Iron(III) ferric Pb4+ Lead(IV) plumbic
Naming Molecular
Compounds
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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.pptx
An ionic compound is named by writing the cation name first, followed by the anion name. The cation keeps the elemental name and the anion name replaces the ending with "ide". Hydrates are named by adding the prefix indicating the number of water molecules (such as mono, hexa) followed by the suffix "-hydrate" to the name of the ionic compound. Molecular compounds are named by placing the more electropositive element first followed by the more electronegative element with an "-ide" ending. Prefixes indicate the number of each element present.
Chemical Reaction Analysis
This document discusses chemical concepts related to combustion analysis, oxidation states, assigning oxidation states, naming inorganic compounds, binary compounds, polyatomic ions, and oxoacids. It provides examples and rules for determining oxidation states, naming inorganic compounds based on their formulas, and identifying common polyatomic ions and their names. Key points include that combustion analysis can be used to analyze chemical substances, oxidation states are related to electrons gained or lost by atoms, and there are systematic rules for naming inorganic compounds and identifying polyatomic ions based on their structures and formulas.
CHEMICAL BONDING (naming of compound).pptx
This document provides information about compounds and their formation. The key points are:
1. Compounds are combinations of two or more elements that form a chemical bond and have a distinct identity from their component elements. A chemical bond occurs when electrons are gained, lost, or shared between atoms.
2. Binary ionic compounds contain two elements, with one being a metal and the other a non-metal. Their formulas are written by crossing the ions' charges. Examples of writing formulas from names and determining ionic charges are provided.
3. Ternary compounds contain at least three elements, including a polyatomic ion. Their names are similar to binary ionic compounds, with the polyatomic ion name in
Ch. 9.1 acids salts and oxidation numbers
This document discusses acids and salts. It begins by naming common acid compounds: sodium fluoride (NaF), calcium chloride (CaCl2), silicon dioxide (SiO2), and dinitrogen pentoxide (N2O5). It then defines acids as molecular compounds, distinguishing between binary acids containing hydrogen and a halogen, and oxyacids containing hydrogen, oxygen, and a third element. Salts are formed from cations and anions, such as sodium chloride (NaCl) from hydrochloric acid (HCl) and calcium sulfate (CaSO4) from sulfuric acid (H2SO4). The document also covers oxidation numbers, which help track electron distribution and are assigned according to rules such as
Naming chemical compounds
Names and formulas of inorganic compounds, organic compounds, cyclic compounds. Binary compounds of two nonmetals. Functional groups.
Chemical nomenclature and reactions
This document provides information about chemical nomenclature and reactions. It discusses writing chemical formulas, empirical formulas, chemical naming conventions, chemical equations, balancing equations, and types of chemical reactions. Specifically, it covers how to write formulas using oxidation numbers and valence, how to determine empirical and molecular formulas from composition data, rules for naming ionic and molecular compounds, the components and symbols used in chemical equations, and methods for balancing equations. It also defines four main types of chemical reactions: combination, decomposition, single displacement, and double displacement.
Lecture 9.3 through 9.5- Naming molecules & acids
The document discusses naming binary molecular compounds and acids and bases. It provides guidelines for naming compounds based on their formulas or vice versa. The key points are:
- Binary molecular compounds are named with prefixes to indicate the number of atoms and the suffix "-ide" for the second element.
- Acids are named after their anions and have formulas starting with hydrogen and ending with the anion formula. Their names indicate the anion stem.
- Bases are named by the cation name followed by the hydroxide anion name and have the hydroxide formula.
- The laws of definite and multiple proportions describe the consistent element ratios in compounds.
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.
Chemical nomenclature 1
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.
ICSE Class IX Chemistry The Language of Chemistry- TopperLearning
The document discusses the language of chemistry, including chemical symbols, elements, ions, valency, molecular formulas, and chemical equations. It provides details on:
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2. The development of the modern periodic table and symbols assigned by IUPAC.
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Chem m12 chemical nomenclature
This document provides information about a module on chemical nomenclature. It begins with an introduction that names are used to identify and distinguish between people and compounds. It then outlines the lessons contained in the module, which are on chemical symbols, formulas, empirical formulas, molecular formulas, and nomenclature. The document concludes by explaining how students should approach learning from the module, including taking pre- and post-tests.
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Naming chemical compounds
- 3. • a lot of chemicals have common names as well as the proper IUPAC name • common name = “nickname” • proper name = systematic name developed by methods of the International Union of Pure and Applied Chemistry”
- 4. • Though chemicals have both a common and proper name, some chemicals are called exclusively by their common name • H2O – water not dihydrogen monoxide • NH3 – ammonia not hydrogen trihidride
- 5. • Write the name of the metal (cation) • write the name of the nonmetal with the ending changed to –ide (anion) • examples ??
- 6. 1. BeF 2. Li2O 3. B2O3 4. Mg3N2
- 7. • Transition metals - Have multiple ion charges - A roman numeral indicates the charge of ion - Examples : Fe, Cu - Nonmetals do not have multiple charges so no roman numerals
- 8. 1. CuCl 2. Mn2S3 3. SnO2 4. Cu3N2 5. Fe2S3 6. KCN 7. NH4Cl
- 9. • Ions containing oxygen always end in “-ate” or “-ite” • Greek prefixes are used to show the number of atoms of each element in a compound. - mono, di, tri