logging in or signing up Inorganic Compounds janina Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 2558 Category: Science & Tech.. License: All Rights Reserved Like it (1) Dislike it (0) Added: August 05, 2008 This Presentation is Public Favorites: 1 Presentation Description Year III First Quarter Comments Posting comment... By: lokeswar (42 month(s) ago) it is good . Also add the naming of Hydrates Saving..... Post Reply Close Saving..... Edit Comment Close Premium member Presentation Transcript NOMENCLATURE : NOMENCLATURE Nomen – name Calare – to call CHEMICAL NOMENCLATURE is the naming of substances. INORGANIC COMPOUNDS : INORGANIC COMPOUNDS Compounds composed of elements other than carbon. Associated with the nonliving portion of the world NOMENCLATURE OF INORGANIC COMPOUNDS : NOMENCLATURE OF INORGANIC COMPOUNDS Ionic Compounds Molecular Compounds Acids NAMING IONIC COMPOUNDS : NAMING IONIC COMPOUNDS CATIONS ( POSITIVE IONS) A. Cations formed from metal atoms have the same name as the metal. Na+ sodium ion Zn2+ zinc ion Al3+ aluminum ion Slide 5: B. If a metal can form cations of different charges, the positive charge is given by a Roman numeral in parenthesis following the name of the metal. Fe2+ iron (II) ion Cu+ copper (I) ion Fe3+ iron (III) ion Cu2+ copper (II) ion Slide 6: Ions with different charges exhibit different properties, such as color. Most of the metals that have variable charges are transition metals. Slide 7: Apply –ous or –ic The endings represent the lower and higher charged ions, respectively. Fe2+ ferrous ion Cu+ cuprous ion Fe3+ ferric ion Cu2+ cupric ion IONIC CHARGES OF REPRESENTATIVE ELEMENTS : IONIC CHARGES OF REPRESENTATIVE ELEMENTS FORMULAS AND NAMES OF COMMON METAL IONS WITH MORE THAN ONE IONIC CHARGE : FORMULAS AND NAMES OF COMMON METAL IONS WITH MORE THAN ONE IONIC CHARGE Slide 10: C. Cations formed from nonmetals have names that end in –ium NH4+ ammonium ion H3O+ hydronium ion Slide 11: REFER TO PAGE 58 OF YOUR BOOKS FOR THE LIST OF THE COMMON CATIONS EXERCISES: : EXERCISES: Name each of the following: Sn2+ Sn4+ K+ Ba2+ Co2+ Co3+ Slide 13: Sn2+ Tin (II) ion Sn4+ Tin (IV) ion K+ Potassium ion Ba2+ Barium ion Co2+ Cobalt (II) ion Co3+ Cobalt (III) ion Slide 14: 2. ANIONS (NEGATIVE IONS) A. Monoatomic (one-atom) anions have names formed by replacing the ending of the name of the element with –ide H- O2- N3- Hydride ion Oxide ion Nitride ion Slide 15: B. Polyatomic (many-atoms) anions containing oxygen have names ending in –ate or –ite These are called oxyanions -ate is used for the most common oxyanion of an element -ite is used for an oxyanion that has the same charge but one less O atoms NO3- nitrate ion SO42- sulfate ion NO2- nitrite ion SO32- sulfite ion Slide 16: Prefixes are used when the series of oxyanions of an element extends to four members, as with halogens The prefix per- indicates one or more O atom than the oxyanion ending in –ate The prefix hypo- indicates one less O atom than the oxyanion ending in –ite Slide 17: ClO4- perchlorate ion (one more O atom than chlorate) ClO3- chlorate ion ClO2- chlorite ion (one less O atom than chlorate) ClO- hypochlorite ion (one less O atom than chlorite) Slide 18: C. Anions derived by adding H+ to an oxyanion are named by adding as a prefix the word hydrogen or dihydrogen CO32- carbonate ion HCO3- hydrogen carbonate ion PO43- phosphate ion H2PO4- dihydrogen phosphate ion Slide 19: REFER TO PAGE 59 OF YOUR BOOK FOR THE LIST OF COMMON ANIONS COMMON POLYATOMIC IONS : COMMON POLYATOMIC IONS Slide 21: 3. IONIC COMPOUNDS Names of ionic compounds consist of the cation name followed by the anion name CaCl2 calcium chloride Al(NO3)3 aluminum nitrate Cu(ClO4)2 copper (II)perchlorate cupric perchlorate EXERCISES: : EXERCISES: What is the charge of the ion typically formed by each element? Sulfur Lead, 4 electrons lost Strontium Argon Bromine Copper, 1 electron lost Slide 23: Sulfur 2- Lead, 4 electrons lost 4+ Strontium 2+ Argon no ion formed Bromine 1- Copper, 1 electron lost 1+ Slide 24: Name the following compounds: CuS K3N SnCl2 K2S CaI2 NaI Slide 25: CuS Copper (II) sulfide K3N Potassium Nitride SnCl2 Tin (II) chloride K2S Potassium sulfide CaI2 Calcium Iodide NaI Sodium Iodide Slide 26: Name the following: MgCl2 SnCl4 HgBr2 PbS2 FeO Write the formula for each of the following: Magnesium bromide Aluminum oxide Ferrous bromide Lead (II) sulfide Stannic oxide HOMEWORK: : HOMEWORK: Name the following: CoI2 Cs2O ZnS KCI BaO CuBr2 Slide 28: CoI2 Copper sulfide Cs2O Cesium Oxide ZnS Zinc sulfide KCI Potassium chloride BaO Barium Oxide CuBr2 Copper bromide Slide 29: NAMES OF FORMULAS OF ACIDS An acid is a substance whose molecules yield hydrogen ions (H+) when dissolved in water. Slide 30: Acid based on anions whose names end in –ide. Anions whose names end in –ide have he asociated acids that have the hydro- prefix and an –ic ending ANION CORRESPONDING ACIDS Cl- (chloride) HCl (hydrochloric acid) S2- (sulfide) H2S (hydrosulfuric acid) Slide 31: 2. Anions whose names end in –ate have associated acids with an –ic ending, whereas anions whose names end in –ite have acids with an -ous ending. Prefixes in the name of the anion are retained in the name of the acid. Slide 32: ANION CORRESPONDING ACID ClO4- perchlorate HClO4 – perchloric acid ClO3- chlorate HClO3 – chloric acid ClO2- chlorite HClO2 – chlorous acid ClO- hypochlorite HClO – hypochloric acid EXERCISES: : EXERCISES: Give the name or formula for the following: H2SO4 H2CO3 Nitric acid Phosphoric acid Slide 34: NAMES AND FORMULAS OF BINARY MOLECULAR COMPOUNDS Binary compounds (two-element) molecular compounds Similar to those used for naming ionic compounds Slide 35: The name of the element farthest to the left in the periodic table is usually written first. Exception: compounds that contain oxygen, oxygen always written last except when combined with chlorine Slide 36: 2. If both elements are in the same group in the periodic table, the lower one is named first. Slide 37: 3. The name of the second element is given an –ide ending. Slide 38: 4. Greek prefixes are used to indicate the number of atoms of each element. Mono- is never used with the first element. The prefix ends in a or o and the name of the second element begins with a vowel (example, oxide), the a or o is dropped. Slide 39: Cl2O dichlorine monoxide NF3 nitrogen trifluoride N204 dinitrogen tetroxide P4S10 tetraphosphorous decasulfide EXERCISES: : EXERCISES: Name these compounds: N2O PCl3 SF6 OF4 Cl2O8 SO3 Slide 41: N2O dinitrogen monoxide PCl3 phosphorus trichloride SF6 sulfur hexafluoride OF2 oxygen difluoride Cl2O8 dichlorine octoxide SO3 sulfur trioxide SOME SIMPLE ORGANIC COMPOUNDS : SOME SIMPLE ORGANIC COMPOUNDS Organic compounds are compounds that contain carbon and hydrogen, often in combination with oxygen, nitrogen, or other elements. Slide 43: ALKANES Compounds that contain only carbon and hydrogen are called hydrocarbons. In the most basic class of hydrocarbons, each carbon atom is boned to four other atoms. These are called alkanes. Slide 44: The 3 simplest alkanes are methane (CH4), ethane (C2H6), and propane (C3H8) Alkanes with 5 or more carbon atoms, the names are derived from prefixes: octane (C8H18) DERIVATIVES OF ALKANE : DERIVATIVES OF ALKANE Other classes of organic compounds are obtained when hydrogen atoms of alkanes are replaced with functional groups, which are specific groups of atoms. Slide 46: ALCOHOL Obtained by replacing an H atom of alkane with an –OH group The name of alcohols are derived from that of alkane by adding an –ol ending. Methanol, Ethanol, 1-Propanol EXERCISES: : EXERCISES: Consider the alkane called pentane. (a) Assuming that the carbon atoms are in a straight line, write a structural formula for pentane. (b) What is the molecular formula for pentane? You do not have the permission to view this presentation. In order to view it, please contact the author of the presentation.
Inorganic Compounds janina Download Post to : URL : Related Presentations : Share Add to Flag Embed Email Send to Blogs and Networks Add to Channel Uploaded from authorPOINT lite Insert YouTube videos in PowerPont slides with aS Desktop Copy embed code: (To copy code, click on the text box) Embed: URL: Thumbnail: WordPress Embed Customize Embed The presentation is successfully added In Your Favorites. Views: 2558 Category: Science & Tech.. License: All Rights Reserved Like it (1) Dislike it (0) Added: August 05, 2008 This Presentation is Public Favorites: 1 Presentation Description Year III First Quarter Comments Posting comment... By: lokeswar (42 month(s) ago) it is good . Also add the naming of Hydrates Saving..... Post Reply Close Saving..... Edit Comment Close Premium member Presentation Transcript NOMENCLATURE : NOMENCLATURE Nomen – name Calare – to call CHEMICAL NOMENCLATURE is the naming of substances. INORGANIC COMPOUNDS : INORGANIC COMPOUNDS Compounds composed of elements other than carbon. Associated with the nonliving portion of the world NOMENCLATURE OF INORGANIC COMPOUNDS : NOMENCLATURE OF INORGANIC COMPOUNDS Ionic Compounds Molecular Compounds Acids NAMING IONIC COMPOUNDS : NAMING IONIC COMPOUNDS CATIONS ( POSITIVE IONS) A. Cations formed from metal atoms have the same name as the metal. Na+ sodium ion Zn2+ zinc ion Al3+ aluminum ion Slide 5: B. If a metal can form cations of different charges, the positive charge is given by a Roman numeral in parenthesis following the name of the metal. Fe2+ iron (II) ion Cu+ copper (I) ion Fe3+ iron (III) ion Cu2+ copper (II) ion Slide 6: Ions with different charges exhibit different properties, such as color. Most of the metals that have variable charges are transition metals. Slide 7: Apply –ous or –ic The endings represent the lower and higher charged ions, respectively. Fe2+ ferrous ion Cu+ cuprous ion Fe3+ ferric ion Cu2+ cupric ion IONIC CHARGES OF REPRESENTATIVE ELEMENTS : IONIC CHARGES OF REPRESENTATIVE ELEMENTS FORMULAS AND NAMES OF COMMON METAL IONS WITH MORE THAN ONE IONIC CHARGE : FORMULAS AND NAMES OF COMMON METAL IONS WITH MORE THAN ONE IONIC CHARGE Slide 10: C. Cations formed from nonmetals have names that end in –ium NH4+ ammonium ion H3O+ hydronium ion Slide 11: REFER TO PAGE 58 OF YOUR BOOKS FOR THE LIST OF THE COMMON CATIONS EXERCISES: : EXERCISES: Name each of the following: Sn2+ Sn4+ K+ Ba2+ Co2+ Co3+ Slide 13: Sn2+ Tin (II) ion Sn4+ Tin (IV) ion K+ Potassium ion Ba2+ Barium ion Co2+ Cobalt (II) ion Co3+ Cobalt (III) ion Slide 14: 2. ANIONS (NEGATIVE IONS) A. Monoatomic (one-atom) anions have names formed by replacing the ending of the name of the element with –ide H- O2- N3- Hydride ion Oxide ion Nitride ion Slide 15: B. Polyatomic (many-atoms) anions containing oxygen have names ending in –ate or –ite These are called oxyanions -ate is used for the most common oxyanion of an element -ite is used for an oxyanion that has the same charge but one less O atoms NO3- nitrate ion SO42- sulfate ion NO2- nitrite ion SO32- sulfite ion Slide 16: Prefixes are used when the series of oxyanions of an element extends to four members, as with halogens The prefix per- indicates one or more O atom than the oxyanion ending in –ate The prefix hypo- indicates one less O atom than the oxyanion ending in –ite Slide 17: ClO4- perchlorate ion (one more O atom than chlorate) ClO3- chlorate ion ClO2- chlorite ion (one less O atom than chlorate) ClO- hypochlorite ion (one less O atom than chlorite) Slide 18: C. Anions derived by adding H+ to an oxyanion are named by adding as a prefix the word hydrogen or dihydrogen CO32- carbonate ion HCO3- hydrogen carbonate ion PO43- phosphate ion H2PO4- dihydrogen phosphate ion Slide 19: REFER TO PAGE 59 OF YOUR BOOK FOR THE LIST OF COMMON ANIONS COMMON POLYATOMIC IONS : COMMON POLYATOMIC IONS Slide 21: 3. IONIC COMPOUNDS Names of ionic compounds consist of the cation name followed by the anion name CaCl2 calcium chloride Al(NO3)3 aluminum nitrate Cu(ClO4)2 copper (II)perchlorate cupric perchlorate EXERCISES: : EXERCISES: What is the charge of the ion typically formed by each element? Sulfur Lead, 4 electrons lost Strontium Argon Bromine Copper, 1 electron lost Slide 23: Sulfur 2- Lead, 4 electrons lost 4+ Strontium 2+ Argon no ion formed Bromine 1- Copper, 1 electron lost 1+ Slide 24: Name the following compounds: CuS K3N SnCl2 K2S CaI2 NaI Slide 25: CuS Copper (II) sulfide K3N Potassium Nitride SnCl2 Tin (II) chloride K2S Potassium sulfide CaI2 Calcium Iodide NaI Sodium Iodide Slide 26: Name the following: MgCl2 SnCl4 HgBr2 PbS2 FeO Write the formula for each of the following: Magnesium bromide Aluminum oxide Ferrous bromide Lead (II) sulfide Stannic oxide HOMEWORK: : HOMEWORK: Name the following: CoI2 Cs2O ZnS KCI BaO CuBr2 Slide 28: CoI2 Copper sulfide Cs2O Cesium Oxide ZnS Zinc sulfide KCI Potassium chloride BaO Barium Oxide CuBr2 Copper bromide Slide 29: NAMES OF FORMULAS OF ACIDS An acid is a substance whose molecules yield hydrogen ions (H+) when dissolved in water. Slide 30: Acid based on anions whose names end in –ide. Anions whose names end in –ide have he asociated acids that have the hydro- prefix and an –ic ending ANION CORRESPONDING ACIDS Cl- (chloride) HCl (hydrochloric acid) S2- (sulfide) H2S (hydrosulfuric acid) Slide 31: 2. Anions whose names end in –ate have associated acids with an –ic ending, whereas anions whose names end in –ite have acids with an -ous ending. Prefixes in the name of the anion are retained in the name of the acid. Slide 32: ANION CORRESPONDING ACID ClO4- perchlorate HClO4 – perchloric acid ClO3- chlorate HClO3 – chloric acid ClO2- chlorite HClO2 – chlorous acid ClO- hypochlorite HClO – hypochloric acid EXERCISES: : EXERCISES: Give the name or formula for the following: H2SO4 H2CO3 Nitric acid Phosphoric acid Slide 34: NAMES AND FORMULAS OF BINARY MOLECULAR COMPOUNDS Binary compounds (two-element) molecular compounds Similar to those used for naming ionic compounds Slide 35: The name of the element farthest to the left in the periodic table is usually written first. Exception: compounds that contain oxygen, oxygen always written last except when combined with chlorine Slide 36: 2. If both elements are in the same group in the periodic table, the lower one is named first. Slide 37: 3. The name of the second element is given an –ide ending. Slide 38: 4. Greek prefixes are used to indicate the number of atoms of each element. Mono- is never used with the first element. The prefix ends in a or o and the name of the second element begins with a vowel (example, oxide), the a or o is dropped. Slide 39: Cl2O dichlorine monoxide NF3 nitrogen trifluoride N204 dinitrogen tetroxide P4S10 tetraphosphorous decasulfide EXERCISES: : EXERCISES: Name these compounds: N2O PCl3 SF6 OF4 Cl2O8 SO3 Slide 41: N2O dinitrogen monoxide PCl3 phosphorus trichloride SF6 sulfur hexafluoride OF2 oxygen difluoride Cl2O8 dichlorine octoxide SO3 sulfur trioxide SOME SIMPLE ORGANIC COMPOUNDS : SOME SIMPLE ORGANIC COMPOUNDS Organic compounds are compounds that contain carbon and hydrogen, often in combination with oxygen, nitrogen, or other elements. Slide 43: ALKANES Compounds that contain only carbon and hydrogen are called hydrocarbons. In the most basic class of hydrocarbons, each carbon atom is boned to four other atoms. These are called alkanes. Slide 44: The 3 simplest alkanes are methane (CH4), ethane (C2H6), and propane (C3H8) Alkanes with 5 or more carbon atoms, the names are derived from prefixes: octane (C8H18) DERIVATIVES OF ALKANE : DERIVATIVES OF ALKANE Other classes of organic compounds are obtained when hydrogen atoms of alkanes are replaced with functional groups, which are specific groups of atoms. Slide 46: ALCOHOL Obtained by replacing an H atom of alkane with an –OH group The name of alcohols are derived from that of alkane by adding an –ol ending. Methanol, Ethanol, 1-Propanol EXERCISES: : EXERCISES: Consider the alkane called pentane. (a) Assuming that the carbon atoms are in a straight line, write a structural formula for pentane. (b) What is the molecular formula for pentane?