2. Compounds

3. Know Your Periodic Table Transition Metals Metals

4. Bonding  Bonding:  When two or more atoms come together to form a molecule or compound  In order for bonding to occur, atoms must:  Gain an electron (s) or  Lose an electron (s) or  Share an electron (s)  Bonding:  When two or more atoms come together to form a molecule or compound  In order for bonding to occur, atoms must:  Gain an electron (s) or  Lose an electron (s) or  Share an electron (s)

5. Basic Bonding Concepts  Atoms react in such a way as to achieve a STABLE ELECTRON CONFIGURATION (SEC)  A SEC is the result of a full valence shell  A full valence shell contains a total of 8 electrons  It can be referred to as a STABLE OCTET  The Noble Gases represent a stable octet or SEC because they have a full valence shell  - i.e.: HeArXe  Atoms react in such a way as to achieve a STABLE ELECTRON CONFIGURATION (SEC)  A SEC is the result of a full valence shell  A full valence shell contains a total of 8 electrons  It can be referred to as a STABLE OCTET  The Noble Gases represent a stable octet or SEC because they have a full valence shell  - i.e.: HeArXe

6. Bonding Types  There are two (2) main types of bonds:  1) Ionic  Electrons are transferred between atoms  Electrons are lost and gained by atoms  2) Covalent  Electrons are shared between atoms  There are two (2) main types of bonds:  1) Ionic  Electrons are transferred between atoms  Electrons are lost and gained by atoms  2) Covalent  Electrons are shared between atoms

7. Bonding Type 1 – Ionic Bonds  Ionic bonds are the result of the transfer of electrons  Electrons are lost or gained to achieve a SEC  Form ionic compounds  IONIC compounds form from the attraction between cations and anions.  The resulting compound is electrically neutral, so the charges must balance out.  Ionic bonds are the result of the transfer of electrons  Electrons are lost or gained to achieve a SEC  Form ionic compounds  IONIC compounds form from the attraction between cations and anions.  The resulting compound is electrically neutral, so the charges must balance out.

8. Bonding Type 1 – Ionic Bonds  Composed of two (2) parts:  1) Cations  Positive ions  “Cats have paws (POS)…”  Lose electrons when they bond to achieve a SEC  Metals  2) Anions  Negative ions  “A-Negative-ION…”  Gain electrons when they bond to achieve a SEC  non-metals  Composed of two (2) parts:  1) Cations  Positive ions  “Cats have paws (POS)…”  Lose electrons when they bond to achieve a SEC  Metals  2) Anions  Negative ions  “A-Negative-ION…”  Gain electrons when they bond to achieve a SEC  non-metals

9. Examples of Ions  Polyatomic Ions  Consist of more than one atom with an overall charge  Act as a single unit  Examples:  Carbonate – CO 3 2-  Sulphate – SO 4 2-  Located on the backside of your periodic table  Polyatomic Ions  Consist of more than one atom with an overall charge  Act as a single unit  Examples:  Carbonate – CO 3 2-  Sulphate – SO 4 2-  Located on the backside of your periodic table

10. Naming Ionic Compounds  Binary Ionic Compounds  Consist of two elements: metal cation and a non-metal anion  Metal is named first and says its own name  Non-metal is named second and changes its suffix to “ide”  For transition metals with more than one ionic charge  Use the anions to determine their charge  Indicate their charge with roman numerals  Only Ag +, Zn 2+, and Cd 2+ have 1 charge. You do not need Roman numerals for these  Binary Ionic Compounds  Consist of two elements: metal cation and a non-metal anion  Metal is named first and says its own name  Non-metal is named second and changes its suffix to “ide”  For transition metals with more than one ionic charge  Use the anions to determine their charge  Indicate their charge with roman numerals  Only Ag +, Zn 2+, and Cd 2+ have 1 charge. You do not need Roman numerals for these

11. Examples Ions Compound Name Sodium & chlorine Sodium chloride Aluminum & chlorine Aluminum chloride Aluminum & oxygen Aluminum oxide Sodium & sulphur Sodium sulphide Iron (2 +) & Oxygen iron (II) oxide Iron (3+) & Oxygen iron (III) oxide

12. Formulas for Ionic Compounds  Binary Ionic Compounds  Write down the symbols for each individual ion side by side – cation first, anion second  Balance the charges by crossing them  (Swap & Drop)  *Charges become subscripts*  Write the formula  Note:  You do not need to write the subscript 1 in the formula  You should reduce the subscripts if possible  Binary Ionic Compounds  Write down the symbols for each individual ion side by side – cation first, anion second  Balance the charges by crossing them  (Swap & Drop)  *Charges become subscripts*  Write the formula  Note:  You do not need to write the subscript 1 in the formula  You should reduce the subscripts if possible

13. Examples Compound Name IonsFormula Sodium chloride Na + & Cl - NaCl Aluminum oxide Al 3+ & O 2- Al 2 O 3 iron (III) oxide Fe 3+ & O 2- Fe 2 O 3 iron (II) oxide Fe 2+ & O 2- Fe 2 O 2  FeO

14. Naming Ionic Compounds  Ternary Ionic Compounds  Ionic compounds that contain polyatomic ions  Polyatomic ions act as a single unit (subscripts included)  Monatomic cations say their own name; monatomic anions end in the suffix “ide”  Polyatomic ions always say their own name  When more than one polyatomic ion is used in a formula, it will be placed in brackets  Ternary Ionic Compounds  Ionic compounds that contain polyatomic ions  Polyatomic ions act as a single unit (subscripts included)  Monatomic cations say their own name; monatomic anions end in the suffix “ide”  Polyatomic ions always say their own name  When more than one polyatomic ion is used in a formula, it will be placed in brackets

15. Examples Ions Compound Name Ammonium & chlorine Ammonium chloride Potassium & sulfate Potassium sulfate Lead (2+) & phosphate Lead (II) phosphate Ammonium & oxalate Ammonium oxalate

16. Formulas for Ionic Compounds  Ternary Ionic Compounds  Same as binary ionic compounds  Make sure that when you balance the charges that the subscript for a polyatomic ion is OUTSIDE of the brackets  This is because polyatomic ions act as a single unit and the subscript applies to the entire unit  Remember, numbers WITHIN the brackets of a polyatomic ion CANNOT be reduced  Ternary Ionic Compounds  Same as binary ionic compounds  Make sure that when you balance the charges that the subscript for a polyatomic ion is OUTSIDE of the brackets  This is because polyatomic ions act as a single unit and the subscript applies to the entire unit  Remember, numbers WITHIN the brackets of a polyatomic ion CANNOT be reduced

17. Examples Compound Name IonsFormula Ammonium sulphide NH 4+ & S 2- (NH 4 ) 2 S Potassium carbonate K + & CO 3 2- K 2 CO 3 Iron (II) nitrate Fe 2+ & NO 3 - Fe(NO 3 ) 2 Sodium sulfate Na + & SO 4 2- Na 2 (SO 4 )

18. Acid Structure Have a characteristic formula structure: “HX”  Where “H” is a hydrogen cation  Where “X” is an anion  So generally, if you see a formula for an ionic compound that starts with an “H” it is likely an acid Have a characteristic formula structure: “HX”  Where “H” is a hydrogen cation  Where “X” is an anion  So generally, if you see a formula for an ionic compound that starts with an “H” it is likely an acid

19. Naming Acids  Scenario 1 – The anion ends in the suffix “ide”  Add the prefix “hydro” to the anion  Change the suffix to “ic”  Add the word “acid” to the end  i.e. HF  hydrogen & fluoride   hydrofluoric acid  i.e. HCN  hydrogen & cyanide   hydrocyanic acid  Scenario 1 – The anion ends in the suffix “ide”  Add the prefix “hydro” to the anion  Change the suffix to “ic”  Add the word “acid” to the end  i.e. HF  hydrogen & fluoride   hydrofluoric acid  i.e. HCN  hydrogen & cyanide   hydrocyanic acid

20. Naming Acids  Scenario 2 – The anion ends with the suffix “ate”  Change the suffix of the anion to “ic”  Add the word “acid” to the end  Note: no need for the “hydro” prefix  Hint to remember – “If you ATE it, its Icky”  i.e. HNO 3  hydrogen & nitrate   nitric acid  i.e. H 2 SO 4  hydrogen & sulfate   Sulfuric acid  Scenario 2 – The anion ends with the suffix “ate”  Change the suffix of the anion to “ic”  Add the word “acid” to the end  Note: no need for the “hydro” prefix  Hint to remember – “If you ATE it, its Icky”  i.e. HNO 3  hydrogen & nitrate   nitric acid  i.e. H 2 SO 4  hydrogen & sulfate   Sulfuric acid

21. Naming Acids  Scenario 3 – The anion ends with the suffix “ite”  Change the suffix on the anion to “ous”  Add the word “acid” to the end  Note: no need for the “hydro” prefix  i.e. HNO 2  hydrogen & nitrite   nitrous acid  i.e. H 2 SO 3  hydrogen & sulfite   sulfurous acid  Scenario 3 – The anion ends with the suffix “ite”  Change the suffix on the anion to “ous”  Add the word “acid” to the end  Note: no need for the “hydro” prefix  i.e. HNO 2  hydrogen & nitrite   nitrous acid  i.e. H 2 SO 3  hydrogen & sulfite   sulfurous acid

22. Writing Acid Formulas  Use the prefix/suffix combinations to figure out the anion  Balance the charges with a H + cation (s)  Write the formula  i.e. – permanganic acid   permanganate anion  MnO 4 -   HMnO 4  Use the prefix/suffix combinations to figure out the anion  Balance the charges with a H + cation (s)  Write the formula  i.e. – permanganic acid   permanganate anion  MnO 4 -   HMnO 4

23. Covalent Bonds – The Basics  Covalent bonds result from the sharing of electrons between two non-metals to achieve a SEC  Since electrons are shared, charged ions are NOT formed  Also known as “molecular bonding”, since covalent bonds form molecules  We can create covalent bonds by having two atoms come together to share an electron pair.  Covalent bonds result from the sharing of electrons between two non-metals to achieve a SEC  Since electrons are shared, charged ions are NOT formed  Also known as “molecular bonding”, since covalent bonds form molecules  We can create covalent bonds by having two atoms come together to share an electron pair.

24. Example

25. Naming Covalent Compounds  Prefixes are used to indicate the number of atoms  The prefix “mono” is only used for the second atom; no mono prefix needed for the first atom  The second atom named ends with the suffix, “ide”  Prefixes are used to indicate the number of atoms  The prefix “mono” is only used for the second atom; no mono prefix needed for the first atom  The second atom named ends with the suffix, “ide”  Prefixes:  1 – “mono”  2 – “di”  3 – “tri”  4 – “tetra”  5 – “penta”  6 – “hexa”  7 – “hept”  8 – “oct”  9 – “non”  10 - “deca”

26. Examples of Naming Covalent Compounds  N 2 H 4 :  Dinitrogen tetrahydride  SO 3 :  Sulfur trioxide  CO 2 :  Carbon dioxide  P 2 O 5 :  Diphosphorus pentoxide  PCl 3:  Phosphorus trichloride N2H4:N2H4:  Dinitrogen tetrahydride  SO 3 :  Sulfur trioxide  CO 2 :  Carbon dioxide P2O5:P2O5:  Diphosphorus pentoxide  PCl 3:  Phosphorus trichloride

27. Formulas for Covalent Compounds  Read the prefixes to determine the amount of each atom  Examples:  carbon tetrachloride:  CCl 4  dinitrogen trioxide:  N 2 O 3  carbon disulfide:  CS 2  dihydrogen monosulfide:  H 2 S  sulfur hexafluoride:  SF 6  Read the prefixes to determine the amount of each atom  Examples:  carbon tetrachloride:  CCl 4  dinitrogen trioxide: N2O3N2O3  carbon disulfide:  CS 2  dihydrogen monosulfide: H2SH2S  sulfur hexafluoride:  SF 6