Naming Compounds Writing Formulas Chapter 5 Systematic Naming
![Naming Compounds Writing Formulas Chapter 5 Naming Compounds Writing Formulas Chapter 5](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-1.jpg)
![Systematic Naming There are too many compounds to remember the names of them all. Systematic Naming There are too many compounds to remember the names of them all.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-2.jpg)
![Periodic Table More than a list of elements. l Put in columns because of Periodic Table More than a list of elements. l Put in columns because of](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-3.jpg)
![1 A Representative elements The group A 2 A elements l The tall columns 1 A Representative elements The group A 2 A elements l The tall columns](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-4.jpg)
![Metals Metals](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-5.jpg)
![Transition metals l The Group B elements Transition metals l The Group B elements](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-6.jpg)
![Dull l Brittle l Nonconductorsinsulators l Non-metals Dull l Brittle l Nonconductorsinsulators l Non-metals](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-7.jpg)
![Metalloids or Semimetals Properties of both l Semiconductors l Metalloids or Semimetals Properties of both l Semiconductors l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-8.jpg)
![Atoms and ions Atoms are electrically neutral. l Same number of protons and electrons. Atoms and ions Atoms are electrically neutral. l Same number of protons and electrons.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-9.jpg)
![Anion A negative ion. l Has gained electrons. l Non metals can gain electrons. Anion A negative ion. l Has gained electrons. l Non metals can gain electrons.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-10.jpg)
![Cations Positive ions. l Formed by losing electrons. l More protons than electrons. l Cations Positive ions. l Formed by losing electrons. l More protons than electrons. l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-11.jpg)
![Two Types of Compounds 1 Molecular compounds Made of molecules. l Made by joining Two Types of Compounds 1 Molecular compounds Made of molecules. l Made by joining](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-12.jpg)
![Two Types of Compounds 2 Ionic Compounds Made of cations and anions. l Metals Two Types of Compounds 2 Ionic Compounds Made of cations and anions. l Metals](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-13.jpg)
![Two Types of Compounds Smallest piece Types of elements State Melting Point Ionic Molecular Two Types of Compounds Smallest piece Types of elements State Melting Point Ionic Molecular](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-14.jpg)
![Chemical Formulas Shows the kind and number of atoms in the smallest piece of Chemical Formulas Shows the kind and number of atoms in the smallest piece of](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-15.jpg)
![Formula Unit l The smallest whole number ratio of atoms in an ionic compound. Formula Unit l The smallest whole number ratio of atoms in an ionic compound.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-16.jpg)
![Charges on ions l For most of Group A elements, location on the Periodic Charges on ions l For most of Group A elements, location on the Periodic](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-17.jpg)
![Charge in groups 1 A, 2 A and 3 A is the group number Charge in groups 1 A, 2 A and 3 A is the group number](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-18.jpg)
![Can also use electron dots l If it has a few it loses them Can also use electron dots l If it has a few it loses them](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-19.jpg)
![What about the others? l We have to figure those out some other way. What about the others? l We have to figure those out some other way.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-20.jpg)
![Naming ions l Cation- if the charge is always the same (Group A) just Naming ions l Cation- if the charge is always the same (Group A) just](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-21.jpg)
![Naming ions l. A few, like silver, zinc and cadmium only form one kind Naming ions l. A few, like silver, zinc and cadmium only form one kind](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-22.jpg)
![l. Na 1+ 2+ l. Ca 3+ l. Al l. Fe 3+ l. Fe l. Na 1+ 2+ l. Ca 3+ l. Al l. Fe 3+ l. Fe](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-23.jpg)
![Write Formulas for these l. Potassium ion l. Magnesium l. Copper(II) ion K 1+ Write Formulas for these l. Potassium ion l. Magnesium l. Copper(II) ion K 1+](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-24.jpg)
![Naming Anions l Anions are always the same. l Change the element ending to Naming Anions l Anions are always the same. l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-25.jpg)
![Naming Anions l Anions are always the same. l Change the element ending to Naming Anions l Anions are always the same. l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-26.jpg)
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-27.jpg)
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-28.jpg)
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-29.jpg)
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-30.jpg)
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-31.jpg)
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-32.jpg)
![Name these l. Cl 1 l. N 3 l. Br 1 l. O 2 Name these l. Cl 1 l. N 3 l. Br 1 l. O 2](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-33.jpg)
![Write these l. Sulfide ion S 2 l. Iodide ion I 1 l. Phosphide Write these l. Sulfide ion S 2 l. Iodide ion I 1 l. Phosphide](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-34.jpg)
![Polyatomic ions l Groups of atoms that stay together and have a charge. l Polyatomic ions l Groups of atoms that stay together and have a charge. l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-35.jpg)
![1 - ions C 2 H 3 O 21 l Nitrate NO 31 l 1 - ions C 2 H 3 O 21 l Nitrate NO 31 l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-36.jpg)
![1 - ions Cl. O 41 l Chlorate Cl. O 31 l Chlorite Cl. 1 - ions Cl. O 41 l Chlorate Cl. O 31 l Chlorite Cl.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-37.jpg)
![2 - ions l Sulfate 2 - SO 4 2 l Sulfite SO 3 2 - ions l Sulfate 2 - SO 4 2 l Sulfite SO 3](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-38.jpg)
![3 - ions l Phosphate 3 - PO 4 3 l Phosphite PO 3 3 - ions l Phosphate 3 - PO 4 3 l Phosphite PO 3](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-39.jpg)
![Adding Hydrogen to Polyatomics l Hydrogen ions are 1+ l Attach to other polyatomic Adding Hydrogen to Polyatomics l Hydrogen ions are 1+ l Attach to other polyatomic](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-40.jpg)
![Ions in Ionic Compounds Ions in Ionic Compounds](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-41.jpg)
![Naming Binary Ionic Compounds Binary Compounds - 2 elements. l Ionic - a cation Naming Binary Ionic Compounds Binary Compounds - 2 elements. l Ionic - a cation](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-42.jpg)
![Naming Binary Ionic Compounds The problem comes with the transition metals. l Cation name Naming Binary Ionic Compounds The problem comes with the transition metals. l Cation name](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-43.jpg)
![Naming Binary Ionic Compounds Write the name of Cu. O l Need the charge Naming Binary Ionic Compounds Write the name of Cu. O l Need the charge](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-44.jpg)
![Naming Binary Ionic Compounds Write the name of Cu 2 S. l Since S Naming Binary Ionic Compounds Write the name of Cu 2 S. l Since S](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-45.jpg)
![Naming Binary Ionic Compounds Write the names of the following l KCl l Na Naming Binary Ionic Compounds Write the names of the following l KCl l Na](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-46.jpg)
![Ternary Ionic Compounds Will have polyatomic ions l At least three elements (3 capital Ternary Ionic Compounds Will have polyatomic ions l At least three elements (3 capital](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-47.jpg)
![Ternary Ionic Compounds l (NH 4)2 O l Fe(OH)3 l Li. CN l (NH Ternary Ionic Compounds l (NH 4)2 O l Fe(OH)3 l Li. CN l (NH](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-48.jpg)
![Writing Formulas The charges have to add up to zero. l Get charges on Writing Formulas The charges have to add up to zero. l Get charges on](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-49.jpg)
![Writing Formulas Write the formula for calcium chloride. l Calcium is Ca 2+ l Writing Formulas Write the formula for calcium chloride. l Calcium is Ca 2+ l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-50.jpg)
![Crisscross l Switch the numerical value of the charges 3 32 2+ Ba N Crisscross l Switch the numerical value of the charges 3 32 2+ Ba N](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-51.jpg)
![Write the formulas for these Lithium sulfide l tin (II) oxide l tin (IV) Write the formulas for these Lithium sulfide l tin (II) oxide l tin (IV)](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-52.jpg)
![Write the formulas for these Ammonium chloride l barium nitrate l Write the formulas for these Ammonium chloride l barium nitrate l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-53.jpg)
![Polyatomic? Roman Numeral? Yes No Charge from name Charge from table Yes No Formula Polyatomic? Roman Numeral? Yes No Charge from name Charge from table Yes No Formula](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-54.jpg)
![Yes Group 1 A, 2 A or 3 A? Poly atomic? Yes No Yes Yes Group 1 A, 2 A or 3 A? Poly atomic? Yes No Yes](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-55.jpg)
![Things to look for If cations have (), the number is their charge. Not Things to look for If cations have (), the number is their charge. Not](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-56.jpg)
![Molecular Compounds Writing names and Formulas Molecular Compounds Writing names and Formulas](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-57.jpg)
![Molecular compounds made of just nonmetals l smallest piece is a molecule l can’t Molecular compounds made of just nonmetals l smallest piece is a molecule l can’t](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-58.jpg)
![Easier l Ionic compounds use charges to determine how many of each. – Have Easier l Ionic compounds use charges to determine how many of each. – Have](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-59.jpg)
![Prefixes 1 monol 2 dil 3 tril 4 tetral 5 pental 6 hexal 7 Prefixes 1 monol 2 dil 3 tril 4 tetral 5 pental 6 hexal 7](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-60.jpg)
![Naming l To write the name write two words Prefix name -ide Exception - Naming l To write the name write two words Prefix name -ide Exception -](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-61.jpg)
![Name These N 2 O l NO 2 l Cl 2 O 7 l Name These N 2 O l NO 2 l Cl 2 O 7 l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-62.jpg)
![Write formulas for these diphosphorus pentoxide l tetraiodine nonoxide l sulfur hexaflouride l nitrogen Write formulas for these diphosphorus pentoxide l tetraiodine nonoxide l sulfur hexaflouride l nitrogen](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-63.jpg)
![Name 1 Name 2 Yes No No Does Name 2 have a prefix? Yes Name 1 Name 2 Yes No No Does Name 2 have a prefix? Yes](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-64.jpg)
![Prefix Nm Nm Prefix Nm Nm](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-65.jpg)
![Xx. Yy Yes No Yes Is X a metal? No Xx. Yy Yes No Yes Is X a metal? No](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-66.jpg)
![Prefix+name (no mono) Prefix+name+ide Molecular Prefix+name (no mono) Prefix+name+ide Molecular](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-67.jpg)
![Acids Writing names and Formulas Acids Writing names and Formulas](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-68.jpg)
![Acids Compounds that give off hydrogen ions when dissolved in water. l Must have Acids Compounds that give off hydrogen ions when dissolved in water. l Must have](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-69.jpg)
![Naming acids If the anion attached to hydrogen is ends in -ide, put the Naming acids If the anion attached to hydrogen is ends in -ide, put the](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-70.jpg)
![Naming Acids If the anion has oxygen in it l it ends in -ate Naming Acids If the anion has oxygen in it l it ends in -ate](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-71.jpg)
![Name these HF l H 3 P l H 2 SO 4 l H Name these HF l H 3 P l H 2 SO 4 l H](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-72.jpg)
![Writing Formulas Hydrogen will always be first l name will tell you the anion Writing Formulas Hydrogen will always be first l name will tell you the anion](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-73.jpg)
![Write formulas for these hydroiodic acid l acetic acid l carbonic acid l phosphorous Write formulas for these hydroiodic acid l acetic acid l carbonic acid l phosphorous](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-74.jpg)
![Name 1 Name 2 Is Name 2 acid? No Yes No Does Name 2 Name 1 Name 2 Is Name 2 acid? No Yes No Does Name 2](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-75.jpg)
![No Hydro- ? No Yes Charge from table -ic acid? Yes -ate Nm-Y HYNm No Hydro- ? No Yes Charge from table -ic acid? Yes -ate Nm-Y HYNm](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-76.jpg)
![Xx. Yy Is X hydrogen? Yes No Yes Is X a metal? No Xx. Yy Is X hydrogen? Yes No Yes Is X a metal? No](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-77.jpg)
![Oxygen? Yes -ate? No No Yes ____ ic acid ____ ous acid Acid Hydro____ Oxygen? Yes -ate? No No Yes ____ ic acid ____ ous acid Acid Hydro____](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-78.jpg)
![38. Name these acids a) H 2 C 2 O 4 b) HF c) 38. Name these acids a) H 2 C 2 O 4 b) HF c)](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-79.jpg)
![43. Name these compounds a) Al. F 3 b) Sn. O 2 c) Fe(C 43. Name these compounds a) Al. F 3 b) Sn. O 2 c) Fe(C](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-80.jpg)
![Summary Periodic table – Grouped by properties l Metals- make cations – 2 types Summary Periodic table – Grouped by properties l Metals- make cations – 2 types](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-81.jpg)
![Summary l l l l l Make all the decisions. First determine type of Summary l l l l l Make all the decisions. First determine type of](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-82.jpg)
- Slides: 82
![Naming Compounds Writing Formulas Chapter 5 Naming Compounds Writing Formulas Chapter 5](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-1.jpg)
Naming Compounds Writing Formulas Chapter 5
![Systematic Naming There are too many compounds to remember the names of them all Systematic Naming There are too many compounds to remember the names of them all.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-2.jpg)
Systematic Naming There are too many compounds to remember the names of them all. l Compound is made of two or more elements. l Put together atoms. l Name should tell us how many and what type of atoms. l
![Periodic Table More than a list of elements l Put in columns because of Periodic Table More than a list of elements. l Put in columns because of](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-3.jpg)
Periodic Table More than a list of elements. l Put in columns because of similar properties. l Each column is called a group. l
![1 A Representative elements The group A 2 A elements l The tall columns 1 A Representative elements The group A 2 A elements l The tall columns](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-4.jpg)
1 A Representative elements The group A 2 A elements l The tall columns l 5 A 7 A 3 A 4 A 6 A 0
![Metals Metals](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-5.jpg)
Metals
![Transition metals l The Group B elements Transition metals l The Group B elements](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-6.jpg)
Transition metals l The Group B elements
![Dull l Brittle l Nonconductorsinsulators l Nonmetals Dull l Brittle l Nonconductorsinsulators l Non-metals](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-7.jpg)
Dull l Brittle l Nonconductorsinsulators l Non-metals
![Metalloids or Semimetals Properties of both l Semiconductors l Metalloids or Semimetals Properties of both l Semiconductors l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-8.jpg)
Metalloids or Semimetals Properties of both l Semiconductors l
![Atoms and ions Atoms are electrically neutral l Same number of protons and electrons Atoms and ions Atoms are electrically neutral. l Same number of protons and electrons.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-9.jpg)
Atoms and ions Atoms are electrically neutral. l Same number of protons and electrons. l Ions are atoms, or groups of atoms, with a charge. l Different numbers of protons and electrons. l Only electrons can move. l Gain or lose electrons. l
![Anion A negative ion l Has gained electrons l Non metals can gain electrons Anion A negative ion. l Has gained electrons. l Non metals can gain electrons.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-10.jpg)
Anion A negative ion. l Has gained electrons. l Non metals can gain electrons. l Charge is written as a superscript on the right. l 1 F 2 O Has gained one electron Has gained two electrons
![Cations Positive ions l Formed by losing electrons l More protons than electrons l Cations Positive ions. l Formed by losing electrons. l More protons than electrons. l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-11.jpg)
Cations Positive ions. l Formed by losing electrons. l More protons than electrons. l Metals form cations. l 1+ K Has lost one electron 2+ Ca Has lost two electrons
![Two Types of Compounds 1 Molecular compounds Made of molecules l Made by joining Two Types of Compounds 1 Molecular compounds Made of molecules. l Made by joining](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-12.jpg)
Two Types of Compounds 1 Molecular compounds Made of molecules. l Made by joining nonmetal atoms together into molecules. l
![Two Types of Compounds 2 Ionic Compounds Made of cations and anions l Metals Two Types of Compounds 2 Ionic Compounds Made of cations and anions. l Metals](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-13.jpg)
Two Types of Compounds 2 Ionic Compounds Made of cations and anions. l Metals and nonmetals. l The electrons lost by the cation are gained by the anion. l The cation and anions surround each other. l Smallest piece is a FORMULA UNIT. l
![Two Types of Compounds Smallest piece Types of elements State Melting Point Ionic Molecular Two Types of Compounds Smallest piece Types of elements State Melting Point Ionic Molecular](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-14.jpg)
Two Types of Compounds Smallest piece Types of elements State Melting Point Ionic Molecular Formula Unit Molecule Metal and Nonmetals solid Solid, liquid or gas High >300ºC Low <300ºC
![Chemical Formulas Shows the kind and number of atoms in the smallest piece of Chemical Formulas Shows the kind and number of atoms in the smallest piece of](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-15.jpg)
Chemical Formulas Shows the kind and number of atoms in the smallest piece of a substance. l Molecular formula- number and kinds of atoms in a molecule. l CO 2 l C 6 H 12 O 6 l
![Formula Unit l The smallest whole number ratio of atoms in an ionic compound Formula Unit l The smallest whole number ratio of atoms in an ionic compound.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-16.jpg)
Formula Unit l The smallest whole number ratio of atoms in an ionic compound. l Ions surround each other so you can’t say which is hooked to which.
![Charges on ions l For most of Group A elements location on the Periodic Charges on ions l For most of Group A elements, location on the Periodic](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-17.jpg)
Charges on ions l For most of Group A elements, location on the Periodic Table can tell what kind of ion they form l Elements in the same group have similar properties. l Including the charge when they are ions.
![Charge in groups 1 A 2 A and 3 A is the group number Charge in groups 1 A, 2 A and 3 A is the group number](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-18.jpg)
Charge in groups 1 A, 2 A and 3 A is the group number 1+ 2+ in 5 A, 6 A and 7 A 3+ 3 - 2 - 1 are different.
![Can also use electron dots l If it has a few it loses them Can also use electron dots l If it has a few it loses them](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-19.jpg)
Can also use electron dots l If it has a few it loses them l If it has many, it gains enough for octet 3+ Al 3 - + K F N -
![What about the others l We have to figure those out some other way What about the others? l We have to figure those out some other way.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-20.jpg)
What about the others? l We have to figure those out some other way. l More on this later.
![Naming ions l Cation if the charge is always the same Group A just Naming ions l Cation- if the charge is always the same (Group A) just](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-21.jpg)
Naming ions l Cation- if the charge is always the same (Group A) just write the name of the metal. l Most transition metals can have more than one type of charge. l Indicate the charge with Roman numerals in parenthesis. l Co 2+ Cobalt(II) ion
![Naming ions l A few like silver zinc and cadmium only form one kind Naming ions l. A few, like silver, zinc and cadmium only form one kind](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-22.jpg)
Naming ions l. A few, like silver, zinc and cadmium only form one kind of ion l Don’t get roman numerals l Ag+ silver ion l Zn 2+ zinc ion l Cd 2+ cadmium ion
![l Na 1 2 l Ca 3 l Al l Fe 3 l Fe l. Na 1+ 2+ l. Ca 3+ l. Al l. Fe 3+ l. Fe](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-23.jpg)
l. Na 1+ 2+ l. Ca 3+ l. Al l. Fe 3+ l. Fe 2+ 2+ l. Pb 1+ l. Li Name these Sodium ion Calcium ion Aluminum ion Iron(III) ion Iron(II) ion Lead(II) ion Lithium ion
![Write Formulas for these l Potassium ion l Magnesium l CopperII ion K 1 Write Formulas for these l. Potassium ion l. Magnesium l. Copper(II) ion K 1+](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-24.jpg)
Write Formulas for these l. Potassium ion l. Magnesium l. Copper(II) ion K 1+ 2+ Mg 2+ Cu 6+ Cr l. Chromium(VI) ion 2+ Ba l. Barium ion l. Mercury(II) ion 2+ Hg
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same. l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-25.jpg)
Naming Anions l Anions are always the same. l Change the element ending to – ide 1 l F Fluorine
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same. l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-26.jpg)
Naming Anions l Anions are always the same. l Change the element ending to – ide 1 l F Fluorin
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-27.jpg)
Naming Anions l Anions are always the same l Change the element ending to – ide 1 l F Fluori
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-28.jpg)
Naming Anions l Anions are always the same l Change the element ending to – ide 1 l F Fluor
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-29.jpg)
Naming Anions l Anions are always the same l Change the element ending to – ide 1 l F Fluori
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-30.jpg)
Naming Anions l Anions are always the same l Change the element ending to – ide 1 l F Fluorid
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-31.jpg)
Naming Anions l Anions are always the same l Change the element ending to – ide 1 l F Fluoride
![Naming Anions l Anions are always the same l Change the element ending to Naming Anions l Anions are always the same l Change the element ending to](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-32.jpg)
Naming Anions l Anions are always the same l Change the element ending to – ide 1 l F Fluoride ion
![Name these l Cl 1 l N 3 l Br 1 l O 2 Name these l. Cl 1 l. N 3 l. Br 1 l. O 2](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-33.jpg)
Name these l. Cl 1 l. N 3 l. Br 1 l. O 2 l. Ga 3+ Chloride ion Nitride ion Bromide ion Oxide ion Gallium ion
![Write these l Sulfide ion S 2 l Iodide ion I 1 l Phosphide Write these l. Sulfide ion S 2 l. Iodide ion I 1 l. Phosphide](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-34.jpg)
Write these l. Sulfide ion S 2 l. Iodide ion I 1 l. Phosphide ion P 3 l. Strontium ion Sr 2+
![Polyatomic ions l Groups of atoms that stay together and have a charge l Polyatomic ions l Groups of atoms that stay together and have a charge. l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-35.jpg)
Polyatomic ions l Groups of atoms that stay together and have a charge. l Covalently bonded l You must note these. (pg 178 Table 2)
![1 ions C 2 H 3 O 21 l Nitrate NO 31 l 1 - ions C 2 H 3 O 21 l Nitrate NO 31 l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-36.jpg)
1 - ions C 2 H 3 O 21 l Nitrate NO 31 l Nitrite NO 21 l Acetate l Hydroxide 1 OH l Permanganate l Cyanide CN 1 - Mn. O 4 1 -
![1 ions Cl O 41 l Chlorate Cl O 31 l Chlorite Cl 1 - ions Cl. O 41 l Chlorate Cl. O 31 l Chlorite Cl.](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-37.jpg)
1 - ions Cl. O 41 l Chlorate Cl. O 31 l Chlorite Cl. O 21 l Perchlorate 1 l Hypochlorite
![2 ions l Sulfate 2 SO 4 2 l Sulfite SO 3 2 - ions l Sulfate 2 - SO 4 2 l Sulfite SO 3](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-38.jpg)
2 - ions l Sulfate 2 - SO 4 2 l Sulfite SO 3 2 l Carbonate CO 3 2 l Chromate Cr. O 4 l Dichromate Cr 2 O 72 l Silicate Si. O 32 -
![3 ions l Phosphate 3 PO 4 3 l Phosphite PO 3 3 - ions l Phosphate 3 - PO 4 3 l Phosphite PO 3](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-39.jpg)
3 - ions l Phosphate 3 - PO 4 3 l Phosphite PO 3 1+ ion l Ammonium NH 41+
![Adding Hydrogen to Polyatomics l Hydrogen ions are 1 l Attach to other polyatomic Adding Hydrogen to Polyatomics l Hydrogen ions are 1+ l Attach to other polyatomic](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-40.jpg)
Adding Hydrogen to Polyatomics l Hydrogen ions are 1+ l Attach to other polyatomic ionschanges charge by one l Sulfate SO 42 l Hydrogen sulfate HSO 41 l Phosphate PO 43 l Hydrogen phosphate HPO 42 l Dihydrogen phosphate H 2 PO 41 -
![Ions in Ionic Compounds Ions in Ionic Compounds](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-41.jpg)
Ions in Ionic Compounds
![Naming Binary Ionic Compounds Binary Compounds 2 elements l Ionic a cation Naming Binary Ionic Compounds Binary Compounds - 2 elements. l Ionic - a cation](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-42.jpg)
Naming Binary Ionic Compounds Binary Compounds - 2 elements. l Ionic - a cation and an anion. l The name is just the names of the ions. l Cation first anion second l Easy with Group A elements. l Na. Cl = Na+ Cl- = sodium chloride l Mg. Br 2 = Mg 2+ Br- = magnesium bromide l Na 2 S l
![Naming Binary Ionic Compounds The problem comes with the transition metals l Cation name Naming Binary Ionic Compounds The problem comes with the transition metals. l Cation name](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-43.jpg)
Naming Binary Ionic Compounds The problem comes with the transition metals. l Cation name includes the charge. l The compound must be neutral. l same number of + and – charges. l Use the negative charge to find the charge on the positive ion. l
![Naming Binary Ionic Compounds Write the name of Cu O l Need the charge Naming Binary Ionic Compounds Write the name of Cu. O l Need the charge](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-44.jpg)
Naming Binary Ionic Compounds Write the name of Cu. O l Need the charge of Cu l O is 2 l copper must be 2+ l Copper(II) oxide l Name Co. Cl 3 l Cl is 1 - and there are three of them = 3 l Co must be 3+ l Cobalt(III) chloride l
![Naming Binary Ionic Compounds Write the name of Cu 2 S l Since S Naming Binary Ionic Compounds Write the name of Cu 2 S. l Since S](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-45.jpg)
Naming Binary Ionic Compounds Write the name of Cu 2 S. l Since S is 2 -, the Cu 2 must be 2+, so each one is 1+. l copper(I) sulfide l Fe 2 O 3 l Each O is 23 x 2 - = 6 l 2 Fe must = 6+, so each is 3+. l iron(III) oxide l
![Naming Binary Ionic Compounds Write the names of the following l KCl l Na Naming Binary Ionic Compounds Write the names of the following l KCl l Na](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-46.jpg)
Naming Binary Ionic Compounds Write the names of the following l KCl l Na 3 N l Cr. N l Sc 3 P 2 l Pb. O 2 l Na 2 Se l
![Ternary Ionic Compounds Will have polyatomic ions l At least three elements 3 capital Ternary Ionic Compounds Will have polyatomic ions l At least three elements (3 capital](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-47.jpg)
Ternary Ionic Compounds Will have polyatomic ions l At least three elements (3 capital letters) l Still just name the ions l l Na. NO 3 l Ca. SO 4 l Cu. SO 3
![Ternary Ionic Compounds l NH 42 O l FeOH3 l Li CN l NH Ternary Ionic Compounds l (NH 4)2 O l Fe(OH)3 l Li. CN l (NH](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-48.jpg)
Ternary Ionic Compounds l (NH 4)2 O l Fe(OH)3 l Li. CN l (NH 4)2 CO 3 l Ni. PO 4
![Writing Formulas The charges have to add up to zero l Get charges on Writing Formulas The charges have to add up to zero. l Get charges on](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-49.jpg)
Writing Formulas The charges have to add up to zero. l Get charges on pieces. l Cations from name or periodic table. l Anions from periodic table or polyatomic. l Balance the charges by adding subscripts. l Put polyatomics in parenthesis if there is more than one of them l
![Writing Formulas Write the formula for calcium chloride l Calcium is Ca 2 l Writing Formulas Write the formula for calcium chloride. l Calcium is Ca 2+ l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-50.jpg)
Writing Formulas Write the formula for calcium chloride. l Calcium is Ca 2+ l Chloride is Cl 1 l Ca 2+ Cl 1 - would have a 1+ charge. l Need another Cl 1 l Ca 2+ Cl 21 l
![Crisscross l Switch the numerical value of the charges 3 32 2 Ba N Crisscross l Switch the numerical value of the charges 3 32 2+ Ba N](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-51.jpg)
Crisscross l Switch the numerical value of the charges 3 32 2+ Ba N Ba 3 N 2 l Reduce ratio if possible
![Write the formulas for these Lithium sulfide l tin II oxide l tin IV Write the formulas for these Lithium sulfide l tin (II) oxide l tin (IV)](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-52.jpg)
Write the formulas for these Lithium sulfide l tin (II) oxide l tin (IV) oxide l Copper (II) sulfate l Iron (III) phosphide l gallium nitrate l Iron (III) sulfide l ammonium sulfide l
![Write the formulas for these Ammonium chloride l barium nitrate l Write the formulas for these Ammonium chloride l barium nitrate l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-53.jpg)
Write the formulas for these Ammonium chloride l barium nitrate l
![Polyatomic Roman Numeral Yes No Charge from name Charge from table Yes No Formula Polyatomic? Roman Numeral? Yes No Charge from name Charge from table Yes No Formula](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-54.jpg)
Polyatomic? Roman Numeral? Yes No Charge from name Charge from table Yes No Formula and charge from memory M+X Charge from table Nm-Y MYNm. X Ionic
![Yes Group 1 A 2 A or 3 A Poly atomic Yes No Yes Yes Group 1 A, 2 A or 3 A? Poly atomic? Yes No Yes](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-55.jpg)
Yes Group 1 A, 2 A or 3 A? Poly atomic? Yes No Yes Metal Name Metal (charge) Ionic No Name +ide
![Things to look for If cations have the number is their charge Not Things to look for If cations have (), the number is their charge. Not](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-56.jpg)
Things to look for If cations have (), the number is their charge. Not how many. l If anions end in -ide they are probably off the periodic table (Monoatomic) l If anion ends in -ate or -ite it is polyatomic l The positive piece always gets written first l Hydrogen- it depends on where it’s at – If it is second, it’s a nonmetal -hydride l
![Molecular Compounds Writing names and Formulas Molecular Compounds Writing names and Formulas](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-57.jpg)
Molecular Compounds Writing names and Formulas
![Molecular compounds made of just nonmetals l smallest piece is a molecule l cant Molecular compounds made of just nonmetals l smallest piece is a molecule l can’t](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-58.jpg)
Molecular compounds made of just nonmetals l smallest piece is a molecule l can’t be held together because of opposite charges. l can’t use charges to figure out how many of each atom l
![Easier l Ionic compounds use charges to determine how many of each Have Easier l Ionic compounds use charges to determine how many of each. – Have](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-59.jpg)
Easier l Ionic compounds use charges to determine how many of each. – Have to figure out charges. – Have to figure out numbers. l Molecular compounds name tells you the number of atoms. l Uses prefixes to tell you the number
![Prefixes 1 monol 2 dil 3 tril 4 tetral 5 pental 6 hexal 7 Prefixes 1 monol 2 dil 3 tril 4 tetral 5 pental 6 hexal 7](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-60.jpg)
Prefixes 1 monol 2 dil 3 tril 4 tetral 5 pental 6 hexal 7 heptal 8 octal 9 nonal 10 decal
![Naming l To write the name write two words Prefix name ide Exception Naming l To write the name write two words Prefix name -ide Exception -](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-61.jpg)
Naming l To write the name write two words Prefix name -ide Exception - we don’t write mono- if there is only one of the first element. l No ao oo double vowels when writing name, io, oi, and ai are okay. l
![Name These N 2 O l NO 2 l Cl 2 O 7 l Name These N 2 O l NO 2 l Cl 2 O 7 l](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-62.jpg)
Name These N 2 O l NO 2 l Cl 2 O 7 l CBr 4 l CO 2 l Ba. Cl 2 l
![Write formulas for these diphosphorus pentoxide l tetraiodine nonoxide l sulfur hexaflouride l nitrogen Write formulas for these diphosphorus pentoxide l tetraiodine nonoxide l sulfur hexaflouride l nitrogen](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-63.jpg)
Write formulas for these diphosphorus pentoxide l tetraiodine nonoxide l sulfur hexaflouride l nitrogen trioxide l Carbon tetrahydride l phosphorus trifluoride l aluminum chloride l diagram l
![Name 1 Name 2 Yes No No Does Name 2 have a prefix Yes Name 1 Name 2 Yes No No Does Name 2 have a prefix? Yes](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-64.jpg)
Name 1 Name 2 Yes No No Does Name 2 have a prefix? Yes
![Prefix Nm Nm Prefix Nm Nm](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-65.jpg)
Prefix Nm Nm
![Xx Yy Yes No Yes Is X a metal No Xx. Yy Yes No Yes Is X a metal? No](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-66.jpg)
Xx. Yy Yes No Yes Is X a metal? No
![Prefixname no mono Prefixnameide Molecular Prefix+name (no mono) Prefix+name+ide Molecular](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-67.jpg)
Prefix+name (no mono) Prefix+name+ide Molecular
![Acids Writing names and Formulas Acids Writing names and Formulas](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-68.jpg)
Acids Writing names and Formulas
![Acids Compounds that give off hydrogen ions when dissolved in water l Must have Acids Compounds that give off hydrogen ions when dissolved in water. l Must have](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-69.jpg)
Acids Compounds that give off hydrogen ions when dissolved in water. l Must have H in them. l will always be some H next to an anion. l The anion determines the name. l
![Naming acids If the anion attached to hydrogen is ends in ide put the Naming acids If the anion attached to hydrogen is ends in -ide, put the](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-70.jpg)
Naming acids If the anion attached to hydrogen is ends in -ide, put the prefix hydro- and change -ide to -ic acid l HCl - hydrogen ion and chloride ion l hydrochloric acid l H 2 S hydrogen ion and sulfide ion l hydrosulfuric acid l
![Naming Acids If the anion has oxygen in it l it ends in ate Naming Acids If the anion has oxygen in it l it ends in -ate](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-71.jpg)
Naming Acids If the anion has oxygen in it l it ends in -ate or -ite l change the suffix -ate to -ic acid l HNO 3 Hydrogen and nitrate ions l Nitric acid l change the suffix -ite to -ous acid l HNO 2 Hydrogen and nitrite ions l Nitrous acid l
![Name these HF l H 3 P l H 2 SO 4 l H Name these HF l H 3 P l H 2 SO 4 l H](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-72.jpg)
Name these HF l H 3 P l H 2 SO 4 l H 2 SO 3 l HCN l H 2 Cr. O 4 l
![Writing Formulas Hydrogen will always be first l name will tell you the anion Writing Formulas Hydrogen will always be first l name will tell you the anion](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-73.jpg)
Writing Formulas Hydrogen will always be first l name will tell you the anion l make the charges cancel out. l Starts with hydro- no oxygen, -ide l no hydro, -ate comes from -ic, -ite comes from -ous l
![Write formulas for these hydroiodic acid l acetic acid l carbonic acid l phosphorous Write formulas for these hydroiodic acid l acetic acid l carbonic acid l phosphorous](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-74.jpg)
Write formulas for these hydroiodic acid l acetic acid l carbonic acid l phosphorous acid l hydrobromic acid l diagram l
![Name 1 Name 2 Is Name 2 acid No Yes No Does Name 2 Name 1 Name 2 Is Name 2 acid? No Yes No Does Name 2](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-75.jpg)
Name 1 Name 2 Is Name 2 acid? No Yes No Does Name 2 have a prefix? Yes
![No Hydro No Yes Charge from table ic acid Yes ate NmY HYNm No Hydro- ? No Yes Charge from table -ic acid? Yes -ate Nm-Y HYNm](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-76.jpg)
No Hydro- ? No Yes Charge from table -ic acid? Yes -ate Nm-Y HYNm No -ite
![Xx Yy Is X hydrogen Yes No Yes Is X a metal No Xx. Yy Is X hydrogen? Yes No Yes Is X a metal? No](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-77.jpg)
Xx. Yy Is X hydrogen? Yes No Yes Is X a metal? No
![Oxygen Yes ate No No Yes ic acid ous acid Acid Hydro Oxygen? Yes -ate? No No Yes ____ ic acid ____ ous acid Acid Hydro____](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-78.jpg)
Oxygen? Yes -ate? No No Yes ____ ic acid ____ ous acid Acid Hydro____ ic acid
![38 Name these acids a H 2 C 2 O 4 b HF c 38. Name these acids a) H 2 C 2 O 4 b) HF c)](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-79.jpg)
38. Name these acids a) H 2 C 2 O 4 b) HF c) HCl. O 2 d) H 2 CO 3 39. Write formulas for these compounds a) nitrous acid b) hydroselenic acid c) phosphoric acid d) acetic acid 43. Name these compounds a) Al. F 3 b) Sn. O 2 c) Fe(C 2 H 3 O 2)3 d) KHSO 4 e) Ca. H 2 f) HCl. O 3 g) Hg 2 Br 2 h) H 2 Cr. O 4 44. Write formulas for these a) Phosphorus pentabromide b) Carbon chloride c) potassium permanganate
![43 Name these compounds a Al F 3 b Sn O 2 c FeC 43. Name these compounds a) Al. F 3 b) Sn. O 2 c) Fe(C](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-80.jpg)
43. Name these compounds a) Al. F 3 b) Sn. O 2 c) Fe(C 2 H 3 O 2)3 d) KHSO 4 e) Ca. H 2 f) HCl. O 3 g) Hg 2 Br 2 h) H 2 Cr. O 4 44. Write formulas for these a) Phosphorus pentabromide b) Carbon chloride c) potassium permanganate d) Calcium hydrogen carbonate e) dichlorine heptoxide f) trisilicon tetrahydride g) sodium dihydrogen phosphate
![Summary Periodic table Grouped by properties l Metals make cations 2 types Summary Periodic table – Grouped by properties l Metals- make cations – 2 types](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-81.jpg)
Summary Periodic table – Grouped by properties l Metals- make cations – 2 types those with () and those without l Nonmetals make anions – Three types • Without O -ide • With O -ite and -ate l Only electrons can move to make ions l
![Summary l l l l l Make all the decisions First determine type of Summary l l l l l Make all the decisions. First determine type of](https://slidetodoc.com/presentation_image/733000d32db30b9222a29d0d80c8663f/image-82.jpg)
Summary l l l l l Make all the decisions. First determine type of compound Then figure out name or formula Acid = H to start Metal = Ionic No H, No metal = molecular Only molecular get prefixes Roman numeral is NOT how many Hydro means no O
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Section 3 writing formulas and naming compounds
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Writing formulas from names
In an ionic compound the chemical formula represents
Naming and writing formulas for acids and bases
Unit 7 test naming and formula writing
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