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Atoms want 8ve- to be stable “happy”

Atoms want 8ve- to be stable “happy”. Chemical Bonds / Formulas. Atoms bond to become stable or “happy” – octet rule (full valence shell) When they bond they form compounds. Each compound has a special formula Subscripts show how many of each element is in the compound. FORMULAS.

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Atoms want 8ve- to be stable “happy”

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  1. Atoms want 8ve- to be stable “happy”

  2. Chemical Bonds / Formulas • Atoms bond to become stable or “happy” – octet rule (full valence shell) • When they bond they form compounds. • Each compound has a special formula • Subscripts show how many of each element is in the compound

  3. FORMULAS MgCl2 • The subscript is the number at the bottom of a formula. • There is 1- Mg & 2 – Cl • Never use 1 as a subscript!

  4. IONIC BONDbond formed between two ions by the transferof electrons

  5. Ions • Atom that gains or loses electrons to become stable “happy” • Cation: loses e- to form (+) charged ion • Anion: gains e- to form (-) charged ion

  6. Formation of Ions from Metals • Ionic compounds result when metals react with nonmetals • Metalslose electrons to form a positive charge • Nonmetalsgain electrons to form a negative charge • Metals:Nonmetals: Na+ N -3 Ca+2 S -2 Al+3 Br -

  7. IONIC BONDS • Bonds form from the (+) & (-) charges. • Form a network of ions. – very strong bonds. • Conduct electricity when melted or dissolved in water.

  8. Writing Ionic Formulas – binaryRepresentative metals Calcium & oxygen Write the metal ion Ca +2 Write the nonmetal ion O -2 If charges cancel – ratio is 1:1 ( 1 of each) CaO Magnesium & chlorine Write the metal ion Mg +2 Write the nonmetal ion Cl- If charges DO NOT cancel – drop & swap MgCl2

  9. Writing Ionic Formulas – binaryTransition metals • Ion charges change – an element can have more than one ion charge • The charge is given as a ROMAN NUMERAL • Ex: Iron (II) Fe+2 / Iron (III) Fe+3 • Gold (I) Au + / Gold (III) Au+3 • You will never have to memorize all the charges each transition metal forms – the charges will be given to you !!!!!

  10. Practice • Magnesium & iodine • Strontium & bromine • Barium & nitrogen • Aluminum & phosphorus

  11. Naming Ionic Formula - binary • Representative Metals • Name the metal • Change the ending of the nonmetal to – ide MgCl2 - magnesium chloride AlP - aluminum phosphide Cl – chloride C - carbide F – flouride Se - selenide I – iodide N – nitride P – phosphide S – sulfide Br – bromide O – oxide • Transition Metals • Name the metal & Include the charge using a Roman Numeral Ex: Iron (II) Fe+2 / Iron (III) Fe+3 Gold (I) Au + / Gold (III) Au+3 • Change the ending of the nonmetal ending to –ide Fe +2 Cl- iron (II) chloride Au + O -2 gold (I) oxide

  12. Practice • CaBr2 • Na3N • BCl3 • MgO • FeCl3 • Ni3N • ZnO • FeS

  13. Ternary Ionic Bonds – contain Polyatomic Ions • Polyatomic ion : a group of (covalently) bonded nonmetals that form a charge. • Act as a single ion in an ionic bond • Have special names that DO NOT CHANGE • You need to write down the polyatomic ions and their names on a sheet of paper and DO NOT LOSE IT!!! • You will use your list on all quizzes and tests!

  14. Carbonate CO3-2 Chromate CrO4-2 Dichromate Cr2O7-2 Oxalate C2O4-2 Sulfate SO4-2 Sulfite SO3-2 PhosphitePO3-3 Phosphate PO4-3 Permanganate MnO4- Peroxide O2-2 • Ammonium NH4+ • Acetate C2H3O2- • Hypochlorite ClO- • Chlorite ClO2- • Chlorate ClO3- • PerchlorateClO4- • Cyanide CN- • Hydroxide OH- • Nitrite NO2- • Nitrate NO3- • Bicarbonate/Hydrogen Carbonate HCO3-

  15. Writing Ionic Formulas - ternary • Write the cation – all metals (only polyatomic cation is ammonium: NH4+ ) • Write the anion – all nonmetals and polyatomic ions • If charges cancel – 1:1 ratio • If charges DO NOT cancel – drop & swap • You must use parenthesis if more than one polyatomic ion is present

  16. Practice • cesium nitrate • barium sulfite • aluminum hydroxide • strontium phosphate • ammonium sulfide • Iron(III) chlorite • Zinc(II) nitrite • Gold(III) carbonate • Silver(I) phosphite • Copper(I) acetate

  17. Naming ionic formulas - ternary Representative metal • Name the cation • Use the same name for the polyatomic ion • If the anion is a nonmetal – change the ending to -ide Transition metal • Name the metal and include a ROMAN NUMERAL for the charge of the metal • Use the same name for the polyatomic ion • If the anion is a nonmetal – change the ending to -ide

  18. Group 1 - Alkali Metals • reacts violently with water • VERY reactive, one valence e- to lose; • +1 cation

  19. Alkali metals • http://www.youtube.com/watch?v=m55kgyApYrY&safety_mode=true&persist_safety_mode=1

  20. Group 2 - Alkaline Earth Metals • 2 valence e-; • +2 cation • reactive

  21. http://www.youtube.com/watch?v=m55kgyApYrY&safety_mode=true&persist_safety_mode=1http://www.youtube.com/watch?v=m55kgyApYrY&safety_mode=true&persist_safety_mode=1

  22. Transition Metals • Groups 3-12 • Ions charges change – changes properties • NOT REPRESENTATIVE!

  23. Halogens • -Group 17 • -1 ions, highly reactive • 7 valence e-

  24. Noble Gases • Group 18 • unreactive, 8 valence e- • do not form ions • exist as single atoms, don’t bond - inert

  25. COVALENT BONDbond formed by the sharingof electrons

  26. Covalent Compounds • Covalent compounds result when nonmetals react with nonmetals • Both nonmetalsshare their valence electrons to be happy – Octet Rule • Examples: • CO2 SCl2 • H2O CH4

  27. Naming Covalent formulas • Use prefixes to show the # of atoms of each element in a covalent compound • 1 – mono 6 - hexa • 2 – di 7 - hepta • 3 – tri 8- octa • 4 – tetra 9 - nona • 5 – penta 10 – deca • 1st element – use prefixes only of the # of atoms is greater than 1 • 2nd element – use prefixes; change ending to – ide

  28. Practice carbon dioxide • CO2 • N3F8 • Se4Br9 • S7O trinitrogenoctaflouride tetraseleniumnonabromide heptasulfur monoxide

  29. Writing Covalent formulas • Use the prefix to identify how many of each nonmetal atoms are in each molecule • The prefix becomes the subscript. • Carbon TetrahydrideDisulfurHexachloride • CH4 S2Cl6

  30. 1) Name the following covalent compounds: a) SiF4 b) N2S3 c) H3Br7 d) S5Br9 e) H2O • Write the formulas for the following covalent • compounds: a) diboronhexahydride b) nitrogen tribromide c) sulfur hexachloride d) diphosphoruspentoxide

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