1 / 33

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.

vevay
Télécharger la présentation

Atoms want 8ve- to be stable “happy”

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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

More Related