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Compounds

Compounds. Molecular and Ionic. Molecular Compounds. Molecular compounds have relatively melting points and boiling points do not conduct electricity when may or may not conduct electricity when. Molecular Compounds. Molecular compounds

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Compounds

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  1. Compounds Molecular and Ionic

  2. Molecular Compounds • Molecular compounds • have relativelymelting points and boiling points • do not conduct electricity when • may or may not conduct electricity when

  3. Molecular Compounds • Molecular compounds • exist as with definite composition • have individual molecules that are held together by relatively that are generally proportional to the size of the molecule • for the binary compound AB, the A is attracted than to other B’s

  4. Molecular Compounds B A • Imagine that these are binary molecular compounds where the red end represents element A and the white end represents element B. A is attracted to all B’s but to one B more than the others

  5. Molecular Compounds • Law of Definite Proportions: In a given compound, the elements are combined in a • This means that for something like water, H2O, there are always 2 H’s for every 1 O. There can never be water with 3 H’s for every 1 O or 2 H’s for every 3 O’s.

  6. Molecular Compounds • Law of Multiple Proportions: When elements form more than one compound, the mass ratio of one element to the other in a compound is an of the ratio in another • Mass O : Mass C in carbon monoxide is 1.33:1 • Mass O : Mass C in carbon dioxide is 2.67:1 • This makes sense, since there is in CO2 as in CO

  7. Binary Molecular Compounds • A binary molecular compound is composed of two • To name a binary molecular compound, it is necessary to use

  8. Binary Molecular Compounds • Naming the first element: • Only use a prefix if there is atom of the first element • of the element’s name • Naming the second element: • use a prefix • of the element’s name

  9. The prefixes are: 1-mono 2-di 3-tri 5-penta 6-hexa 7-hepta 9-nona 10-deca Binary Molecular Compounds

  10. Binary Molecular Compounds • Name these compounds: • CCl4 • P2O5 • Give the formula for these compounds: • dinitrogen monoxide • oxygen difluoride

  11. Ionic Compounds • Ionic compounds • have melting points and boiling points • conduct electric current when • conduct electric current when in

  12. Ionic Compounds • Ionic compounds • have a basic unit that is a of oppositely charged particles called • have empirical formulas giving the simplest integer ratio of the ions in a • NaCl is not a molecule but a series of Na+ ions surrounded by Cl- ions • Each Na+ ion is attracted equally byCl- ions • Each Cl- ion is attracted equally by Na+ ions

  13. Ionic Compounds • This is a crystal lattice of NaCl, a common ionic compound • Every Na+ ion (green) is surrounded by 6 Cl- (blue) ions

  14. Ionic Compounds • This website will show how a NaCl unit cell repeats to form a crystal lattice. http://departments.kings.edu/chemlab/animation/nacl.html • Are there individual molecules in an ionic compound?

  15. Ions • Ions are neutral atoms that have gained or lost electrons to develop a charge • Metals to form positive ions called • Nonmetals to form negative ions called

  16. Ionic Charges • Representative elements have predictable charges

  17. Ionic Charges • The transition metals may have multiple charges

  18. Ionic Charges • Transition metals and those representative metals that are under the stair-step line may have possible charge • To differentiate between them, you must use a • Example: Cu1+ is copper (I) and Cu2+ is copper (II)

  19. Binary Ionic Compounds • Binary ionic compounds consist of ions—a cation which is a metal and an anion which is a nonmetal. • Binary ionic compounds only contain • The ions’ charges must cancel in order to create a formula unit

  20. Binary Ionic Compounds • Let’s say that you wanted to combine the metal Sr with the nonmetal I. • First, you would have to on Sr and the charge on I • Sr is in Group 2 and has a charge of • I is in Group 17 and has a charge of • Then, you would have to make sure the charges • It would take two I1-’s to cancel one Sr2+:

  21. Naming Binary Ionic Compounds • Name the cation/metal first • NEVER use prefixees • the ending • If there are multiple charges, use a • Name the anion/nonmetal second • NEVER use prefixes • Change the ending to

  22. Naming Binary Ionic Compounds • Name the following compounds: • LiF • MgCl2 • Cu3N • Give the formulas for the following compounds: • calcium sulfide • iron (III) oxide

  23. Naming Ternary Ionic Compounds • Name the cation first • Is it a polyatomic ion? If so, name it. • Is it a monatomic ion? If so, check to see if it needs a and then name it. • Remember, metal’s endings do not change! • Name the cation second • Is it a polyatomic ion? If so, name it. • Is it a monatomic ion? If so, change the ending to .

  24. Naming Ternary Ionic Compounds • Name the following compounds • Na2SO4 • NH4CO3 • Al(NO3)3 • Give the formula of the following compounds • lead (II) acetate • calcium carbonate

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