Chemical Bonds I. Why Atoms Combine

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1 Chemical Bonds I. Why Atoms Combine Chemical Formula Chemical Bond Stability

2 What is a compound? What does the word compound mean in this sentence? I have a compound fracture in my leg.

3 What is a compound? Compounds involve more than one element/atom. Table salt is a compound made of two elements, sodium (Na) and chlorine (Cl).

4 What is a compound? A compound always has the same chemical formula. Remember that a chemical formula helped you to categorize a substance as a mixture or a compound a few chapters ago.

5 A. Chemical Formula Shows: 1) elements in the compound 2) ratio of their atoms H 2 O 1 oxygen atom 2 hydrogen atoms

6 Practice Silver chloride = one atom of silver + one atom of chlorine Hydrochloric acid = one atom of hydrogen + one atom of chlorine

7 Practice Hydrogen peroxide= two atoms of hydrogen + two atoms of oxygen Magnesium carbonate = one atom of magnesium + one atom of carbon + three atoms of oxygen

8 Practice Glucose = six atoms of carbon + twelve atoms of hydrogen + six atoms of oxygen sucrose, C 12 H 22 O 11 Show me the elements and atom amount

9 B. Chemical Bond Strong attractive force between atoms or ions in a molecule or compound. The higher the melting and boiling points of a substance, the stronger the attractive forces.

10 C. What is an ion? An ion is an atom with a net charge because it no longer has the same number of electrons and protons. An ion is formed when atoms need to give up or take electrons to fill their outer energy level.

11 Ions Going back to sodium (Na) and chlorine (Cl) forming table salt, sodium gave up an electron to chlorine. So sodium chloride is made of sodium and chlorine ions. Both elements now have a charge.

12 Chemical bonds Formed by either: transferring e - (losing or gaining) sharing e -

13 D. Stability Octet Rule most atoms form bonds in order to have 8 valence e - full outer energy level like the Noble Gases! Ne Stability is the driving force behind bond formation!

14 C. Stability Transferring e - Sharing e -

15 Chemical Bonds II. Kinds of Chemical Bonds Ionic Bond Covalent Bond Comparison Chart

16 A. Ionic Bond Attraction between 2 oppositely charged ions Ions - charged atoms formed by transferring e - from a metal to a nonmetal

17 A. Ionic Bond ions form a 3-D crystal lattice NaCl

18 A. Oxidation Number 1+ The charge on an ion. Indicates the # of e - gained/lost to become stable

19 Metallic Bonds Metals: can conduct electricity flexible can be hammered into thin sheets stretched into thin wire

20 Metallic Bonds Electrons move freely between metal atoms Metal atoms pack closely together so their outer orbitals (energy levels) overlap So electrons are free to move from atom to atom

21 Metallic Bonds Valence electrons of metals are not associated with a particular metal ion. This helps electricity to move fast along metal wires.

22 B. Covalent Bond Attraction between neutral atoms formed by sharing e - between two nonmetals

23 B. Covalent Bond covalent bonds result in discrete molecules Cl 2 NH 3 H 2 O

24 Covalent Bond sharing

25 B. Covalent Bond Nonpolar Covalent Bond e - are shared equally usually identical atoms

26 B. Covalent Bond Polar Covalent Bond e - are shared unequally between 2 different atoms results in partial opposite charges + -

27 B. Covalent Bond Nonpolar Polar Ionic View Bonding Animations.

28 C. Comparison Chart Electrons Melting Point Soluble in Water Conduct Electricity Other Properties IONIC transferred from metal to nonmetal high yes yes (solution or liquid) crystal lattice of ions, crystalline solids COVALENT shared between nonmetals low usually not no molecules, odorous liquids & gases

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30 Chemical Bonds III. Naming Molecular Compounds Molecular Names Molecular Formulas

31 A. Molecular Names Write the names of both elements. Change the final ending to -ide. Add prefixes to indicate subscripts. Only use mono- prefix with oxide.

32 A. Molecular Names PREFIX monoditritetrapenta- SUBSCRIPT

33 A. Molecular Names PREFIX hexaheptaoctanonadeca- SUBSCRIPT

34 A. Molecular Names CCl 4 carbon tetrachloride N 2 O dinitrogen monoxide SF 6 sulfur hexafluoride

35 B. Molecular Formulas Write the more metallic element first. Add subscripts according to prefixes.

36 B. Molecular Formulas phosphorus trichloride PCl 3 dinitrogen pentoxide N 2 O 5 dihydrogen monoxide H 2 O

37 B. Molecular Formulas The Seven Diatomic Elements Br 2 I 2 N 2 Cl 2 H 2 O 2 F 2

38 Chemical Bonds IV. Naming Ionic Compounds Oxidation Number Ionic Names Ionic Formulas

39 A. Oxidation Number 1+ The charge on an ion. Indicates the # of e - gained/lost to become stable

40 B. Ionic Names Write the names of both elements, cation first. (metal) Change the anion s ending to -ide. (nonmetal) For ions with variable oxidation # s, write the ox. # in parentheses using Roman numerals. Overall charge = 0. (Transition metals)

41 B. Ionic Names NaBr sodium bromide Be 3 P 2 Beryllium phosphide

42 C. Ionic Formulas Write each ion. Put the cation first. Overall charge must equal zero. If charges cancel, just write the symbols. If not, crisscross the charges to find subscripts.

43 C. Ionic Formulas potassium chloride K + Cl - KCl

44 C. Ionic Formulas calcium oxide Ca 2+ O 2- CaO Sodium oxide Na + + O > Na 2 O

45 Ionic Formulas Aluminum chloride Al 3+ + Cl - ---> AlCl 3

46 Covalent Bond Naming SiO 2 silicon dioxide NO nitrogen monoxide XeF 4 Xenon tetrafluoride

47 Covalent Bond Naming P 4 S 3 Tetraphosphorus trisulfide PBr 3 phosphorus tribromide CS 2 carbon disulfide

48 Covalent bond formula Nitrogen trifluoride NF 3 Dinitrogen pentoxide N 2 O 5

49 Covalent Bond formula Trisilicon tetranitride Si 3 N 4 Carbon dioxide CO 2

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