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NAMING AND WRITING CHEMICAL COMPOUNDS

NAMING AND WRITING CHEMICAL COMPOUNDS. OUTLINE. IUPAC BOHR DIAGRAMS FOR ATOMS TYPES OF CHEMICAL BONDS MOLECULAR COMPOUNDS TYPES SIMPLE COVALENT COMMON NAME IONIC COMPOUNDS SIMPLE IONIC MULTIVALENT POLYATOMIC/COMPLEX HYDRATED IONIC ACIDS. IUPAC.

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NAMING AND WRITING CHEMICAL COMPOUNDS

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  1. NAMING AND WRITING CHEMICAL COMPOUNDS

  2. OUTLINE • IUPAC • BOHR DIAGRAMS FOR ATOMS • TYPES OF CHEMICAL BONDS • MOLECULAR COMPOUNDS • TYPES • SIMPLE COVALENT • COMMON NAME • IONIC COMPOUNDS • SIMPLE IONIC • MULTIVALENT • POLYATOMIC/COMPLEX • HYDRATED IONIC • ACIDS

  3. IUPAC • International Union of Pure and Applied Chemists • This is a global organization that sets the standards in chemistry. • One job of the IUPAC is to give compounds SYSTEMIC NAMES.

  4. BOHR DIAGRAMS FOR ATOMS • Bohr diagrams, also called ENERGY LEVEL DIAGRAMS, are a means of drawing atoms in a 2-D manner. • Keep in mind that atoms are actually 3-D, and there are more complex representations of atoms. • Bohr models always include the NUCLEUS and the ELECTRON ENERGY LEVELSof an atom. • LINK

  5. BOHR DIAGRAMS . . . • There are 3 types of SUBATOMIC PARTICLES found in the atom: • PROTONS (p+) • Positively charged particles with a significant mass • Atomic Number = Number of Protons • ELECTRONS (e-) • Negatively charged particles with an insignificant mass • Number of Electrons = Number of Protons • NEUTRONS (no) • Neutral particles with a significant mass • Number of neutrons = Atomic Mass – Atomic Number

  6. BOHR DIAGRAMS . . . • NUCLEUS • Center of the atom, contains protons and neutrons • The atomic mass is concentrated here • ELECTRON ENERGY LEVELS • Particular areas around the nucleus where electrons are likely to be found • Electrons DO NOT exist BETWEEN energy levels • 3 LEVELS: • FIRST LEVEL (Closest to Nucleus) 2 e- • SECOND LEVEL 8 e- • THIRD LEVEL (Outermost) 8 e-

  7. BOHR DIAGRAMS . . . • VALENCE LEVEL • DEFINITION: Outermost energy level of an atom • Electrons in this level are called VALENCE ELECTRONS • Atoms with FULL valence shells are STABLE, meaning they will not bond with other atoms in normal conditions. • The atoms of Group 18, the Noble Gases, have full valence levels. • Atoms that do not have full electron energy levels are unstable and must GAIN, LOSE, or SHARE electrons to become stable.

  8. BOHR DIAGRAMS . . . • ATOMIC NUMBER • Located in the top of each element box on the periodic table. • ATOMIC NUMBER = # OF PROTONS • ATOMIC MASS (MOLAR MASS) • Located in the bottom of each element box on the periodic table. • Round it off for calculations. • ATOMIC MASS = # OF PROTONS + # OF NEUTRONS

  9. BOHR DIAGRAMS . . . • EXAMPLE: DRAW BOHR DIAGRAMS FOR: • Li – lithium atom • ATOMIC # = _____________ • ATOMIC MASS = _____________ • # p+ = ________________________ • # e- = ________________________ • # no = ________________________

  10. BOHR DIAGRAMS . . . • EXAMPLE: DRAW BOHR DIAGRAMS FOR: • Ne – neon atom • ATOMIC # = _____________ • ATOMIC MASS = _____________ • # p+ = ________________________ • # e- = ________________________ • # no = ________________________

  11. BOHR DIAGRAMS . . . • EXAMPLE: DRAW BOHR DIAGRAMS FOR: • S – sulfur atom • ATOMIC # = _____________ • ATOMIC MASS = _____________ • # p+ = ________________________ • # e- = ________________________ • # no = ________________________

  12. TYPES OF CHEMICAL BONDS • CHEMICAL BONDS • DEFINITION: • A force of attraction between atoms. • There are 2 TYPES of Chemical bonds • Covalent • Ionic

  13. TYPES OF CHEMICAL BONDS • COVALENT BONDS • AKA: molecular bonds • “co” – together/sharing , “valent” – outer shell • DEFINITION: • A SHARING of ELECTRONS between 2 atoms • BETWEEN a two or more NONMETALS • Solutions of covalently bonded substances are NON-ELECTROLYTIC.

  14. TYPES OF CHEMICAL BONDS • IONIC BOND • DEFINITION: • A TRANSFER of ELECTRONS between two atoms • BETWEEN a METAL and a NONMETAL • Solutions of ionic bonded substances are ELECTROLYTIC. • COMPOUNDS consist of atoms or ions of two or more elements bonded together.

  15. MOLECULAR COMPOUNDS • Forms when 2 or more NONMETALS share electrons in COVALENT BONDS. • 2 TYPES: • BINARY Molecular Compounds • TRIVIAL NAME Molecular Compounds

  16. BINARY MOLECULAR COMPOUNDS • Also called SIMPLE molecular compounds. • Binary Molecular Compounds use IUPAC prefixes: • We will write these prefixes in the following table.

  17. Given Molecular Formula, Write Name • RULES: • Write NAMES of elements, with the 2nd element ending in “-ide”. • Add PREFIXES to indicate HOW MANY ATOMS of each element. • Do NOT use the prefix “mono” for the 1st element, only with the 2nd element.

  18. Given Formula, Write Name EXAMPLE • N2O4 ________________________ • P2O5 ________________________ • CCl4 ________________________

  19. GIVEN MOLECULAR NAME, WRITE FORMULA • RULES: • Write ELEMENT SYMBOLS for each element in the compound. • Use the PREFIX in the name to determine NUMBER OF ATOMS, and write that number as a SUBSCRIPT next to the symbol (no subscript for 1 atom).

  20. Given Name, Write Formula EXAMPLE • carbon monoxide ____________ • triphosphoruspentabromide ____________ • sulfur hexafluoride ____________

  21. TRIVIAL NAME Molecular Compounds • Also called COMMON NAME molecular compounds. • There are SOME molecular compounds that go by their COMMON NAMES, and we must memorize these names.

  22. IONS • RECALL: • AS mentioned earlier, atoms other than the NOBLE GASES are unstable, and need to GAIN, LOSE, or SHARE ELECTRONS to become more stable. • If they SHARE electrons, this forms a COVALENT BOND to another atom. • If they LOSE or GAIN electrons, atoms become IONS and form IONIC BONDS with other atoms. • OCTET RULE • Atoms that have an octet of valence electrons are STABLE and UNREACTIVE.

  23. WHAT IS AN ION? • Ions are charged atoms that have lost or gained electrons to achieve the valence configurations of a noble gas. • TWO TYPES: • CATIONS: • POSITIVE ions that are formed from a LOSS of electrons. • It has more PROTONS than ELECTRONS and therefore has a net POSITIVE charge. • METALS form cations. • MEMORY TOOL: t in “cation” resembles a “+” sign • EXAMPLE: lithium ionLi+ 1+ charge

  24. ANIONS: • NEGATIVE ions that are formed from a GAIN of electrons. • It has more ELECTRONS than PROTONS and therefore has a net NEGATIVE charge. • change the ending of the name of anions to -ide • NONMETALS form anions. • MEMORY TOOL: A Negative ION • EXAMPLE: fluoride ionF- 1- charge • LINK

  25. BOHR DIAGRAMS FOR IONS • METALS • ATOMS of METALS will LOSE electrons to become CATIONS. • ATOMS with 1, 2, or 3 VALENCE electrons will LOSE these electrons to form 1+, 2+, or 3+ ions respectively. • GROUP 1 ATOMS – ALKALI • 1valence electrons(s) (will lose 1 to become stable) • 1 + ion • GROUP 2 ATOMS – ALKALINE EARTH • 2valence electrons(s) (will lose 2 to become stable) • 2 + ion • GROUP 13 ATOMS • 3valence electrons(s) (will lose 3 to become stable) • 3 + ion

  26. BOHR DIAGRAMS FOR IONS • NONMETALS • ATOMS of NONMETALS will GAIN electrons to become ANIONS. • ATOMS with 5,6, or 7 VALENCE electrons will GAIN these electrons to form 3-, 2-, or 1- ions respectively. • GROUP 15 ATOMS • 5valence electrons(s) (will gain 3 to become stable) • 3 - ion • GROUP 16 ATOMS • 6valence electrons(s) (will gain 2 to become stable) • 2 - ion • GROUP 17 ATOMS - HALOGENS • 7valence electrons(s) (will gain 1 to become stable) • 1 - ion • GROUP 18 ATOMS - NOBLE GASES • FULL outer valence levels

  27. TO DRAW: • Note that in BOHR DIAGRAMS for IONS, electron numbers have changed. • Here is a quick equation for calculating the number of electrons: • # e- = #p+ - charge

  28. DRAW A BOHR DIAGRAM FOR: • A sodium ATOM and a sodium ION

  29. DRAW A BOHR DIAGRAM FOR: • A chlorine ATOM and a chloride ION

  30. IONIC COMPOUNDS • Form when at least 1 METAL AND 1 NONMETAL transfer electrons in an IONIC BOND. • Metals will become CATIONS and LOSE electrons and nonmetals will become ANIONS and GAIN electrons. • These ions, with opposite charges, attract and form IONIC BONDS. • Unlike covalent bonds, these bonds are not “ACTUAL BONDS,” but forces of attraction between oppositely charged ions. • They stay together in a CRYSTAL LATTICE.

  31. IONIC COMPOUNDS • Example: NaCl (Draw on your sheet) Cl- Cl- Cl- Cl- Na+ Na+ Na+ Cl- Cl- Na+ Na+ Cl- Na+ Na+ Cations are surrounded by anions and vice versa Also refer to Figure 4, p. 189

  32. IONIC COMPOUNDS • Example: NaCl

  33. IONIC COMPOUNDS • 3 TYPES: • Binary Ionic Compounds • SIMPLE • MULTIVALENT • Polyatomic Ionic Compounds • Hydrated Ionic Compounds

  34. BINARY IONIC COMPOUNDS • “Binary” • Only 2 types of ions involved. • SIMPLE IONIC COMPOUNDS • Simple ionic compounds are composed of a metal ion (+) and a nonmetal ion(-). • GIVEN FORMULA, WRITE NAME • RULES: • Write the name of the CATION before the ANION (Be positive before being negative  ) • Change the ending of the ANION name to “-ide” • Do not use CAPITALS, Do not use PREFIXES!

  35. SIMPLE IONIC COMPOUNDS • EXAMPLE: • MgBr2 _________________________________ • KCl _________________________________ • Na2S _________________________________ • Mg3P2 _________________________________ • Ba3N2 _________________________________ • WHAT’S WRONG WITH THE FOLLOWING NAMES FOR BaS? • barium sulfur ____________________________ • Barium Sulfide ____________________________ • barium sulfuride ____________________________

  36. SIMPLE IONIC COMPOUNDS • GIVEN NAME, WRITE FORMULA • RULES: • Write element symbols. • Look up the ION CHARGE on the periodic table. • Use the “crossover” method to determine the numbers of each ion in the compound. • Ion ratios are always in the lowest common multiple. • Ion charges must add up to “zero” overall.

  37. SIMPLE IONIC COMPOUNDS EXAMPLE: • sodium bromide _____________________ • barium iodide ___________________

  38. SIMPLE IONIC COMPOUNDS EXAMPLE: • magnesium oxide _____________________ • aluminum oxide ___________________

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