Straight forward naming of inorganic compounds adopting a pattern acceptable by WAEC and IGCSE. Naming of ions, binary compounds, oxo-acids, acids, complex salts, radicals are well simplified for easy understanding.
The document provides examples of naming and writing formulas for various chemical compounds. It gives the names for 20 chemical formulas, such as sodium bromide for NaBr. It then gives the formulas for 20 chemical names, such as silicon dioxide for SiO2. Finally, it provides 20 more examples of naming or writing formulas for ionic and covalent compounds and identifies whether they are ionic or covalent.
This document provides notes on chemical nomenclature and bonding. It discusses the naming of ionic and molecular compounds using common names and IUPAC rules. Key topics covered include naming binary ionic compounds, transition metal ions, polyatomic ions, acids, and writing formulas from names and vice versa. The document emphasizes memorizing common monatomic ions and using subscripts, prefixes and Roman numerals correctly in naming various chemical species.
The document discusses naming binary ionic compounds, binary covalent compounds, and ternary compounds. It provides examples of naming compounds containing metals and nonmetals such as NaCl, ZnI2, Al2O3. It also discusses naming transition metal compounds and compounds with variable metal ions using Roman numerals. The document provides examples and practice problems for naming various compound types.
The document provides information on naming and writing formulas for ionic compounds and compounds containing polyatomic ions. It defines characteristics of ionic compounds and explains that ionic compounds are named by writing the name of the metal followed by the nonmetal with the "-ide" ending. It also discusses transition metals which can have multiple oxidation states indicated by Roman numerals. Polyatomic ions are ions made of more than one atom and examples are provided along with how to write formulas for compounds containing polyatomic ions.
This document provides the names and formulas of various ionic compounds. It lists the names of 40 ionic compounds along with their corresponding chemical formulas. The names provide the cation and anion present in each compound as well as the ionic charges. The formulas identify the elements and their ratios that make up each ionic compound.
The document provides information on naming and writing formulas for various types of chemical compounds including:
1. Ionic compounds formed from cations and anions are named by writing the metal first followed by the nonmetal with the appropriate ending (e.g. NaCl is sodium chloride).
2. Molecular compounds formed from nonmetals use prefixes to indicate the number of atoms and the second element takes the "-ide" ending (e.g. CO2 is carbon dioxide).
3. Acids are named by identifying if they contain one or two elements and whether they contain oxygen, and using appropriate endings like "-ic", "-ous", or specifying the anion (e.g. HCl is hydrochlor
1. The document discusses naming ionic and covalent compounds according to IUPAC rules. It provides examples of determining formulas from names and vice versa.
2. Rules are given for naming acids, including binary acids like HCl and oxyacids containing polyatomic ions like H2SO4. Examples of naming acids based on their formulas are provided.
3. Hydrates are discussed, which contain water molecules as part of their chemical structure. Their names indicate the number of water molecules using Greek prefixes.
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.
The document provides examples of naming and writing formulas for various chemical compounds. It gives the names for 20 chemical formulas, such as sodium bromide for NaBr. It then gives the formulas for 20 chemical names, such as silicon dioxide for SiO2. Finally, it provides 20 more examples of naming or writing formulas for ionic and covalent compounds and identifies whether they are ionic or covalent.
This document provides notes on chemical nomenclature and bonding. It discusses the naming of ionic and molecular compounds using common names and IUPAC rules. Key topics covered include naming binary ionic compounds, transition metal ions, polyatomic ions, acids, and writing formulas from names and vice versa. The document emphasizes memorizing common monatomic ions and using subscripts, prefixes and Roman numerals correctly in naming various chemical species.
The document discusses naming binary ionic compounds, binary covalent compounds, and ternary compounds. It provides examples of naming compounds containing metals and nonmetals such as NaCl, ZnI2, Al2O3. It also discusses naming transition metal compounds and compounds with variable metal ions using Roman numerals. The document provides examples and practice problems for naming various compound types.
The document provides information on naming and writing formulas for ionic compounds and compounds containing polyatomic ions. It defines characteristics of ionic compounds and explains that ionic compounds are named by writing the name of the metal followed by the nonmetal with the "-ide" ending. It also discusses transition metals which can have multiple oxidation states indicated by Roman numerals. Polyatomic ions are ions made of more than one atom and examples are provided along with how to write formulas for compounds containing polyatomic ions.
This document provides the names and formulas of various ionic compounds. It lists the names of 40 ionic compounds along with their corresponding chemical formulas. The names provide the cation and anion present in each compound as well as the ionic charges. The formulas identify the elements and their ratios that make up each ionic compound.
The document provides information on naming and writing formulas for various types of chemical compounds including:
1. Ionic compounds formed from cations and anions are named by writing the metal first followed by the nonmetal with the appropriate ending (e.g. NaCl is sodium chloride).
2. Molecular compounds formed from nonmetals use prefixes to indicate the number of atoms and the second element takes the "-ide" ending (e.g. CO2 is carbon dioxide).
3. Acids are named by identifying if they contain one or two elements and whether they contain oxygen, and using appropriate endings like "-ic", "-ous", or specifying the anion (e.g. HCl is hydrochlor
1. The document discusses naming ionic and covalent compounds according to IUPAC rules. It provides examples of determining formulas from names and vice versa.
2. Rules are given for naming acids, including binary acids like HCl and oxyacids containing polyatomic ions like H2SO4. Examples of naming acids based on their formulas are provided.
3. Hydrates are discussed, which contain water molecules as part of their chemical structure. Their names indicate the number of water molecules using Greek prefixes.
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.
The document discusses chemical nomenclature and naming conventions for ionic compounds, covalent compounds, and acids. It provides examples of common polyatomic ions and monatomic ions. Guidelines are given for determining formulas based on ion charges and for writing names based on element symbols and ion charges. Roman numerals are used to indicate variable metal ion charges. Prefixes indicate the number of atoms in covalent compound names. Suffixes like -ide, -ate, and -ite are used to derive acid names from anions.
The document defines oxidation number and provides rules for determining oxidation numbers of elements in compounds and polyatomic ions. The rules state that the oxidation number of atoms is 0, ions take the charge, and the sum of oxidation numbers in compounds and polyatomic ions equals the overall charge. Examples are provided to demonstrate applying the rules to calculate the oxidation number of underlined elements in various compounds and polyatomic ions.
The document provides instructions for naming binary ionic compounds and writing their chemical formulas. It discusses naming compounds based on the ions present and balancing charges by adding subscripts. Examples of named compounds and their formulas are given to illustrate the process. Key information includes naming cations and anions, determining charges, and balancing formulas so the total charge is zero.
This document provides information on naming and writing formulas for various types of compounds including:
- Ionic compounds formed from cations and anions
- Molecular compounds formed from nonmetals
- Acids
It discusses common names versus IUPAC names, determining charges on ions, writing formulas to balance charges, and using prefixes to indicate the number of atoms in molecular compounds. Examples are provided to illustrate each type of nomenclature.
This document provides information on naming ionic and molecular compounds. It discusses how to name ionic compounds containing two elements by identifying the cation and anion. It also discusses how to name compounds containing transition metals with variable charge by including the ionic charge in Roman numerals. The document shows examples of writing formulas from compound names and vice versa. It introduces molecular compound naming using prefixes to indicate the number of atoms of each element. Finally, it discusses naming polyatomic ions based on their chemical formulas.
This document provides information on naming ionic and molecular compounds. It includes photos of periodic tables and note cards on elements, polyatomic ions, and acids. There are also tables with examples of binary compounds labeled with their molecular or ionic nature and name. Additional tables provide practice naming polyatomic ions, acids, and compounds containing these species. The document concludes with questions asking to describe the effect of adding H+ to phosphate and the fixed charge of aluminum, as well as the difference between molecular and ionic compounds.
The document provides information about atoms, molecules, and ions. It discusses:
- Atomic number and mass number
- Isotopes and examples of isotopes of hydrogen
- Molecular and empirical formulas
- Ionic compounds and how their formulas are determined
- Naming common compounds and ions
- Acids, bases, and naming acid anions and hydrate compounds
This document provides names and formulas for various chemical compounds and classifies them into categories such as ionic, molecular, acid, base, hydrate, or organic. It lists the names and formulas for 34 compounds total and identifies the category each belongs to. Example compounds named and classified include sodium sulfate as an ionic compound, sulfuric acid as an acid, hexane as an organic alkane, and calcium carbonate as an ionic compound.
1) The document discusses naming compounds, cations, and anions by providing examples of common elements and polyatomic ions along with rules for naming ionic and covalent compounds.
2) Key elements discussed include hydrogen, lithium, carbon, oxygen, sodium, magnesium, chlorine, and copper as well as common polyatomic ions like hydroxide, sulfate, and phosphate.
3) The naming rules indicate that ionic compounds are named by combining the cation and anion names, and covalent compounds are named by identifying functional groups or indicating multiple bonds between elements.
This document provides information on chemical formulas, ionic compounds, and molecular compounds. It discusses how to write formulas and name compounds based on their ionic or molecular structure. Key points include:
- Chemical formulas indicate the types and numbers of atoms in a compound.
- Ionic compounds are held together by ionic bonds between oppositely charged ions. Their formulas are based on the charges of the ions.
- Molecular compounds consist of non-metals bonded covalently. The ratio of elements is not determined by ionic charges.
- Naming involves identifying the cation/anion or elements and indicating stoichiometry. Oxidation numbers represent electron distribution among bonded atoms.
This document provides an overview of naming compounds, cations, anions and polyatomic ions. It lists common elements and their symbols. It outlines four main rules for naming compounds based on whether they contain two identical elements, a halogen/oxygen/sulfur, hydrogen and oxygen, or oxygen. Examples are given to illustrate each rule. Finally, it distinguishes between ionic and covalent formulae for various compounds like NaCl, CaCl2, H2O and others.
1. The document provides information about bonding, naming compounds and ions, properties of metals and alloys.
2. It asks questions about ionic and covalent bonding, properties of metals and alloys, and differentiating between hard and soft steel.
3. The responses define ions, polyatomic ions, and explain why atoms bond and the sea of electrons model of metallic bonding.
This document provides information on naming and writing formulas for various types of chemical compounds including:
1) Binary ionic compounds consisting of a metal and non-metal are named by writing the metal followed by the non-metal with "ide" ending. The chemical formula is written with the symbols.
2) Ionic compounds with multivalent metals or polyatomic ions are named using prefixes like "ous" and "ic". Formulas include charges in parentheses.
3) Molecular compounds of non-metals are named by writing the non-metals with the second element having an "ide" ending. Prefixes are converted to subscripts in formulas.
This document provides information about ions and salts, including:
- Cations are atoms that lose electrons to form positively charged ions, while anions are atoms that gain electrons to form negatively charged ions. Common examples like NaCl are described.
- Transition metal ions and polyatomic ions that can combine to form various salts are listed, along with methods for naming monoatomic and polyatomic salts.
- Properties of salts like high melting points and conductivity are discussed briefly.
- The basics of Lewis dot structures and molecular geometry are introduced for covalent bonding in organic compounds. Electronegativity and molecular polarity are also covered.
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.
The document provides information on naming and identifying different types of chemical compounds including:
- Ionic compounds can be identified by their metal and nonmetal components and named using stock nomenclature.
- Molecular compounds contain two nonmetals and include acids, hydrocarbons, and binary compounds.
- Practice problems are provided to test the ability to identify, name, and write formulas for various ionic and molecular compounds.
The document provides information on naming binary ionic compounds and writing their chemical formulas. It also discusses naming and writing formulas for ternary ionic compounds and molecular compounds. Key points include using cation and anion names and charges to determine formulas for ionic compounds, and using prefixes to indicate the number of atoms in molecular compounds when writing their names.
This document discusses valency and variable valency in chemistry. It defines valency as the combining capacity of an element or radical to form molecules. Some elements like the inert gases have a valency of zero. It then lists the valencies of common elements like hydrogen, carbon, and oxygen. Variable valency is defined as elements that can exhibit more than one valency, such as iron which has valencies of 2 and 3. The document provides examples of how to denote lower and higher valencies using suffixes like -ous and -ic or roman numerals. It concludes by listing several elements that exhibit variable valency like copper, silver, and lead.
This document discusses valency and variable valency in chemistry. It defines valency as the combining capacity of an element or radical to form molecules. Some elements like the inert gases have a valency of zero. It then lists the valencies of common elements like hydrogen, carbon, oxygen and radicals like sodium, magnesium, hydroxide. Variable valency is defined as elements that can exhibit more than one valency, for example, iron can be Fe2+ or Fe3+ and copper can be Cu+ or Cu2+. The document explains that the suffixes -ous and -ic indicate lower and higher valencies and can also be written as roman numerals in brackets. It provides examples of variable valency for elements like
The document discusses chemical nomenclature and naming conventions for ionic compounds, covalent compounds, and acids. It provides examples of common polyatomic ions and monatomic ions. Guidelines are given for determining formulas based on ion charges and for writing names based on element symbols and ion charges. Roman numerals are used to indicate variable metal ion charges. Prefixes indicate the number of atoms in covalent compound names. Suffixes like -ide, -ate, and -ite are used to derive acid names from anions.
The document defines oxidation number and provides rules for determining oxidation numbers of elements in compounds and polyatomic ions. The rules state that the oxidation number of atoms is 0, ions take the charge, and the sum of oxidation numbers in compounds and polyatomic ions equals the overall charge. Examples are provided to demonstrate applying the rules to calculate the oxidation number of underlined elements in various compounds and polyatomic ions.
The document provides instructions for naming binary ionic compounds and writing their chemical formulas. It discusses naming compounds based on the ions present and balancing charges by adding subscripts. Examples of named compounds and their formulas are given to illustrate the process. Key information includes naming cations and anions, determining charges, and balancing formulas so the total charge is zero.
This document provides information on naming and writing formulas for various types of compounds including:
- Ionic compounds formed from cations and anions
- Molecular compounds formed from nonmetals
- Acids
It discusses common names versus IUPAC names, determining charges on ions, writing formulas to balance charges, and using prefixes to indicate the number of atoms in molecular compounds. Examples are provided to illustrate each type of nomenclature.
This document provides information on naming ionic and molecular compounds. It discusses how to name ionic compounds containing two elements by identifying the cation and anion. It also discusses how to name compounds containing transition metals with variable charge by including the ionic charge in Roman numerals. The document shows examples of writing formulas from compound names and vice versa. It introduces molecular compound naming using prefixes to indicate the number of atoms of each element. Finally, it discusses naming polyatomic ions based on their chemical formulas.
This document provides information on naming ionic and molecular compounds. It includes photos of periodic tables and note cards on elements, polyatomic ions, and acids. There are also tables with examples of binary compounds labeled with their molecular or ionic nature and name. Additional tables provide practice naming polyatomic ions, acids, and compounds containing these species. The document concludes with questions asking to describe the effect of adding H+ to phosphate and the fixed charge of aluminum, as well as the difference between molecular and ionic compounds.
The document provides information about atoms, molecules, and ions. It discusses:
- Atomic number and mass number
- Isotopes and examples of isotopes of hydrogen
- Molecular and empirical formulas
- Ionic compounds and how their formulas are determined
- Naming common compounds and ions
- Acids, bases, and naming acid anions and hydrate compounds
This document provides names and formulas for various chemical compounds and classifies them into categories such as ionic, molecular, acid, base, hydrate, or organic. It lists the names and formulas for 34 compounds total and identifies the category each belongs to. Example compounds named and classified include sodium sulfate as an ionic compound, sulfuric acid as an acid, hexane as an organic alkane, and calcium carbonate as an ionic compound.
1) The document discusses naming compounds, cations, and anions by providing examples of common elements and polyatomic ions along with rules for naming ionic and covalent compounds.
2) Key elements discussed include hydrogen, lithium, carbon, oxygen, sodium, magnesium, chlorine, and copper as well as common polyatomic ions like hydroxide, sulfate, and phosphate.
3) The naming rules indicate that ionic compounds are named by combining the cation and anion names, and covalent compounds are named by identifying functional groups or indicating multiple bonds between elements.
This document provides information on chemical formulas, ionic compounds, and molecular compounds. It discusses how to write formulas and name compounds based on their ionic or molecular structure. Key points include:
- Chemical formulas indicate the types and numbers of atoms in a compound.
- Ionic compounds are held together by ionic bonds between oppositely charged ions. Their formulas are based on the charges of the ions.
- Molecular compounds consist of non-metals bonded covalently. The ratio of elements is not determined by ionic charges.
- Naming involves identifying the cation/anion or elements and indicating stoichiometry. Oxidation numbers represent electron distribution among bonded atoms.
This document provides an overview of naming compounds, cations, anions and polyatomic ions. It lists common elements and their symbols. It outlines four main rules for naming compounds based on whether they contain two identical elements, a halogen/oxygen/sulfur, hydrogen and oxygen, or oxygen. Examples are given to illustrate each rule. Finally, it distinguishes between ionic and covalent formulae for various compounds like NaCl, CaCl2, H2O and others.
1. The document provides information about bonding, naming compounds and ions, properties of metals and alloys.
2. It asks questions about ionic and covalent bonding, properties of metals and alloys, and differentiating between hard and soft steel.
3. The responses define ions, polyatomic ions, and explain why atoms bond and the sea of electrons model of metallic bonding.
This document provides information on naming and writing formulas for various types of chemical compounds including:
1) Binary ionic compounds consisting of a metal and non-metal are named by writing the metal followed by the non-metal with "ide" ending. The chemical formula is written with the symbols.
2) Ionic compounds with multivalent metals or polyatomic ions are named using prefixes like "ous" and "ic". Formulas include charges in parentheses.
3) Molecular compounds of non-metals are named by writing the non-metals with the second element having an "ide" ending. Prefixes are converted to subscripts in formulas.
This document provides information about ions and salts, including:
- Cations are atoms that lose electrons to form positively charged ions, while anions are atoms that gain electrons to form negatively charged ions. Common examples like NaCl are described.
- Transition metal ions and polyatomic ions that can combine to form various salts are listed, along with methods for naming monoatomic and polyatomic salts.
- Properties of salts like high melting points and conductivity are discussed briefly.
- The basics of Lewis dot structures and molecular geometry are introduced for covalent bonding in organic compounds. Electronegativity and molecular polarity are also covered.
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.
The document provides information on naming and identifying different types of chemical compounds including:
- Ionic compounds can be identified by their metal and nonmetal components and named using stock nomenclature.
- Molecular compounds contain two nonmetals and include acids, hydrocarbons, and binary compounds.
- Practice problems are provided to test the ability to identify, name, and write formulas for various ionic and molecular compounds.
The document provides information on naming binary ionic compounds and writing their chemical formulas. It also discusses naming and writing formulas for ternary ionic compounds and molecular compounds. Key points include using cation and anion names and charges to determine formulas for ionic compounds, and using prefixes to indicate the number of atoms in molecular compounds when writing their names.
This document discusses valency and variable valency in chemistry. It defines valency as the combining capacity of an element or radical to form molecules. Some elements like the inert gases have a valency of zero. It then lists the valencies of common elements like hydrogen, carbon, and oxygen. Variable valency is defined as elements that can exhibit more than one valency, such as iron which has valencies of 2 and 3. The document provides examples of how to denote lower and higher valencies using suffixes like -ous and -ic or roman numerals. It concludes by listing several elements that exhibit variable valency like copper, silver, and lead.
This document discusses valency and variable valency in chemistry. It defines valency as the combining capacity of an element or radical to form molecules. Some elements like the inert gases have a valency of zero. It then lists the valencies of common elements like hydrogen, carbon, oxygen and radicals like sodium, magnesium, hydroxide. Variable valency is defined as elements that can exhibit more than one valency, for example, iron can be Fe2+ or Fe3+ and copper can be Cu+ or Cu2+. The document explains that the suffixes -ous and -ic indicate lower and higher valencies and can also be written as roman numerals in brackets. It provides examples of variable valency for elements like
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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.
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Date: May 29, 2024
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𝐃𝐢𝐬𝐜𝐮𝐬𝐬 𝐭𝐡𝐞 𝐄𝐏𝐏 𝐂𝐮𝐫𝐫𝐢𝐜𝐮𝐥𝐮𝐦 𝐢𝐧 𝐭𝐡𝐞 𝐏𝐡𝐢𝐥𝐢𝐩𝐩𝐢𝐧𝐞𝐬:
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significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
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8. Class activity
Calculate the oxidation number of the underline
elements:
(1) MnO4
-
(2) K2Cr2O7
(3) KClO3
(4) Na
(5) N3-
(6) H2S
(7) NaNO2
(8) FeCl3
(9) N2O
11. IONS
Cations with Fixed
Valencies
Metals with
Variable Valencies
Anions
Ion Name
Na+ sodium ion
Ca2+ calcium ion
Al3+ aluminum
ion
Ion Name
H- Hydride ion
Cl- Chloride ion
Br- Bromide ion
I- Iodide ion
O2- Oxide ion
S2- Sulfide ion
N3- Nitride ion
P3- Phosphide
ion
C4- Carbide ion
12. POLYATOMIC IONS
Number of oxygen + Non-oxygen element + ate +(It’s valency) + ion
P R E F I X + N A M E + S U F F I X
Oxygen Number
Indicators
Exmples with
No Hydrogen
Examples with
Hydrogen
Number of
Oxygen
Prefix
1 monooxo
2 dioxo
3 trioxo
4 tetraoxo
5 heptaoxo
Ion Formula
trioxocarbonate (IV) ion CO3
2−
oxochlorate (I) ion
(hypochlorite ion)
ClO−
dioxochlorate(III)
ion(chlorite ion)
ClO2
−
trioxochlorate(V)
ion(chlorate ion)
ClO3
−
trioxonitrate (V) ion
(nitrate ion)
NO3
-
trioxosulphate (IV) ion
(sulphite ion)
SO3
2-
tetraoxosulphate (VI) ion
(sulphate ion)
SO4
2-
tetraoxomanganate (VII)
ion (permanganate ion)
MnO4
-
Ion Formula
hydrogen
trioxocarbonate
(IV) ion
(bicarbonate
ion)
HCO3
−
hydrogen
tetraoxosulphat
e (VI)
HSO4
-
13. COMPOUNDS
P R E F I X + N A M E + S U F F I X
Ionic Compounds Acids Acidic Salts
14. COVALENT COMPOUNDS, HYDRATED SALTS AND
COMPLEX SALTS
Covalent Compounds Hydrated Salts Complex Salts
Com-
pound
Name
HCl hydrogen chloride
H2S hydrogen sulfide
NF3 nitrogen fluoride
AlCl3 aluminium chloride
SnCl4 tin (IV) chloride
N2O5 dinitrogen (V)oxide*
N2O4 dinitrogen (IV) xide
N2O3 dinitrogen (III) oxide
Formula of
the
Compound
Name of the
compound
CuSO4.5H2O
Copper (II)
tetraoxosulphate
(VI) pentahydrate
FeSO4.7H2O
Iron (II)
tetraoxosulphate
(VI) heptahydrate
Formula Name
K3Fe(CN)6
Potassium hexa
cyano ferrate
(III) ion
Na2Sn(OH)4
Sodium tetra
hydroxo
stannate(II)
NaAlO2
Sodium
dioxoaluminate
(III)
Na2Fe(H2O)6
Sodium hexa
aquo iron(III)
K2Cu(NH3)4
Potassium tetra
ammine copper
(II) ion