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Outline Chapter 10a The Periodic Law

Outline Chapter 10a The Periodic Law. 10-1. Chemical Change 10-2. Two Classes of Matter 10-3. The Atomic Theory 10-4. Metals and Nonmetals 10-5. Chemical Activity 10-6. Families of Elements 10-7. The Periodic Table . Alchemists.

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Outline Chapter 10a The Periodic Law

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  1. Outline Chapter 10a The Periodic Law 10-1. Chemical Change 10-2. Two Classes of Matter 10-3. The Atomic Theory 10-4. Metals and Nonmetals 10-5. Chemical Activity 10-6. Families of Elements 10-7. The Periodic Table

  2. Alchemists Alchemist tried to make lead into gold. They studies many materials and used mysterious symbols to represent these materials.

  3. 10-1. Chemical Change A chemical reaction results in the formation of a new substance whose properties are different from those of the individual substances that participate in the reaction.

  4. 10-2. Two Classes of Matter Two classes of matter are Pure Substances, and mixtures. Chemical Process/Properties Physical Process/ Properties

  5. 10-2. Two Classes of Matter The difference between a mixture and pure substance.

  6. Elements

  7. Compounds

  8. Homogeneous Mixtures (Solutions) Apple Juice Cranberry Juice Orange Juice

  9. Heterogeneous Mixtures

  10. 10-2. Two Classes of Matter Examples of Chemical and Physical Processes. Chemical Process Physical Process burning Filtering fermentation distillation rusting reverse osmosis Chemical Property Physical Property combustible hardness reactive color Edible texture

  11. 10-2. Two Classes of Matter In a compound, the elements are present in a specific ratio by mass according to the law of definite proportions. In a mixture, the components are not present in a specific ratio by mass.

  12. 10-3. Atomic Theory The English schoolteacher John Dalton (1766-1844) proposed an atomic theory, an old idea from Democritus. Some atoms form molecules. Not all compounds are molecules.

  13. 10-4. Metals and Nonmetals

  14. 10-4. Metals and Nonmetals Metals Nonmetals • All metals, except mercury, are solid at room temperature. • Metals have a characteristic metallic luster. • All metals are opaque. • Metals can be shaped by bending or hammering. • Metals are good conductors of heat and electricity. • Most elements are metals. • Nonmetals may be solid, liquid, or gaseous. • Nonmetals do not have a luster. • Most nonmetals are transparent in thin sheets. • Solid nonmetals are brittle. • Nonmetals are insulators.

  15. 10-5. Chemical Activity • Active elements combine readily to form compounds. • Inactive elements have little tendency to react chemically. • Active elements liberate more heat when they react than do inactive elements. • Active elements usually form stable compounds.

  16. 10-6. Families of Elements • The halogens, or "salt formers," are active nonmetals. They are in group 7. • The alkali metals are active metals and have low melting points.They are in group 1. • The alkaline earth metals are less active than the alkali metals. They are in group 2. • The inert gases are inactive nonmetals. They are in group 8 http://www.youtube.com/watch?v=m55kgyApYrY

  17. 10-7. The Periodic Table The Russian chemist Dmitri Mendeleev formulated the periodic law about 1869 which states that when elements are listed in order of atomic number, elements with similar chemical and physical properties appear at regular intervals. The periodic table is a listing of the elements according to atomic number in a series of rows such that elements with similar properties form vertical columns.

  18. 10-8. Groups and Periods The periodic table arranges chemical families of elements in vertical columns called groups. The horizontal rows of elements of the periodic table are called periods. The transition elements are placed between groups 2 and 3 and include: the rare-earth metals (atomic numbers 57-71), the actinides (atomic numbers 89-105).

  19. Outline Chapter 10b The Periodic Law 10-9. Shells and Subshells 10-10. Explaining the Periodic Table 10-11. Types of Bonding 10-12. Covalent Bonding 10-13. Ionic Bonding 10-14. Ionic Compounds 10-15. Atom Groups 10-16. Naming Compounds 10-17. Chemical Equations

  20. 10-9. Shells and Subshells The electrons in an atom that have the same principal quantum number n occupy the same shell. The electrons in an atom that have the same orbital quantum number l occupy the same subshell. The larger the value of l, the more electrons the subshell can hold. A shell or subshell that contains its full quota of electrons is said to be closed.

  21. 10-10. Explaining the Periodic Table The Grand Secret of Chemistry-All atoms want to become like the noble gases with filled shells or electronic orbitals. They do this by gaining or losing electrons to become ions.

  22. Chemical Bond 8 10.11 Types of Bonds • Covalent Bonds (share electrons) • Ionic Bonds (transfer electrons) • Held together by electrostatic attractions (+ and – ions attract) • Metallic Bonds (sea of electrons)

  23. 10-12. The Covalent Bond Covalent compounds are substances whose atoms are joined by one or more pairs of electrons in a covalent bond.

  24. 10-12. The Covalent Bond Polar covalent compounds are those in which the shared electron pairs are closer to one atom than to the other, making one part of the molecule relatively negative and another part relatively positive. Hδ+-Clδ- Oδ- Hδ+ Hδ+

  25. 10-13. Ionic Bond An ionic bond is formed when electrons are transferred between two or more atoms and the resulting ions of opposite charge attract each other.

  26. 10-14. Ionic Compounds When a metal atom combines with a nonmetal atom to form an ionic compound, the chemical formula of the ionic compound formed can be determined by knowing how many electrons the metal atom loses and how many electrons the nonmetal atom gains.

  27. 10-14. Ionic Compounds What ionic compounds can you make from the following? Na K Ca Mg Al Cl Br O S N NaCl KBr CaCl2 MgBr2 sodium chloride potassium bromide calcium chloride magnesium bromide CaO AlCl3 K3N MgS calcium oxide magnesium sulfide aluminum chloride potassium nitride Al2O3 Aluminum oxide

  28. 10-15. Atom Groups Atom groups appear as units in many compounds and remain together during chemical reactions. The sulfate group SO4 is an example of an atom group. A precipitate is an insoluble solid that results from a chemical reaction in solution. When two or more atom groups of the same kind are present in the formula of a compound, parentheses are placed around the group. Example: Ca(NO3)2

  29. Ammonium……………... Nitrate…………………… Permanganate…………… Chlorate…………………. Hydroxide………………. Cyanide…………………. Sulfate…………………... Carbonate……………….. Chromate……………….. Silicate………………….. Phosphate……………..… NH4+ NO3- MnO4- ClO3- OH- CN- SO4 2 - CO32- CrO42- SiO32- PO43- Ions of Common Atom Groups Or Polyatomic Ions

  30. 10-16. Naming Compounds • A compound ending in -ide usually is composed of only two elements. Hydroxides which contain the OH- ion are an exception. Sodium Chloride=NaCl • A compound ending in -ate contains oxygen and two or more other elements. Calcium Sulfate=CaSO4 • When the same pair of elements occurs in two or more compounds, a prefix (mono = 1, di = 2, tri = 3, tetra = 4, penta = 5, hexa =6, and so on) may be used to indicate the number of one or both kinds of atoms in the molecule. Carbon Dioxide = CO2 • When one of the elements in a compound is a metal that can form different ions, the ionic charge of the metal is given by a roman numeral. Copper(II) Chloride= CuCl2

  31. Lets Practice! Na2CO3 Sodium carbonate KMnO4 Potassium permanganate NaOH Sodium hydroxide CuSO4 Copper (II) sulfate or Cupric sulfate SnF2 Tin (II) Flouride or Stannous Flouride SnF4 Tin (IV) Flouride or Stannic Flouride PbCrO4 Lead (II) chromate or Plubous chromate H2O Hydrogen oxide (no……just water) NH3 Nitrogen trihydride (no..just ammonia)

  32. Taking 20 kids to the zoo? What if you came home with only 18 kids? What if you came home with 22 kids? At who’s house would you drop them off? Parents are funny that way!

  33. 10-17. Chemical Reactions In a chemical equation the formulas of the reacting substances (reactants) appear on the left-hand side and the formulas of the products appear on the right-hand side. CH4 + O2 H2O + CO2 Chemical equations must be balanced, meaning that the number of atoms of each kind of element must be the same on both sides of the equation. Unbalanced chemical equations have unequal numbers of at least one kind of atom on both sides of the equation. Is the reaction below balanced? K2CrO7+ SO2 K2SO4 + CrO2

  34. Balancing using the underlinemethod. Na2O(s) + H2O(l)  NaOH(aq) 2 CH4(g) + O2(g)  CO2(g) + H2O(g) 2 2 4 2 Fe(s) + O2(g)  Fe2O3(s) 2 3 LiOH(s) + CO2(g)  LiHCO3(s) D KClO3(s)  KCl(s) + O2(g) 2 2 3 MnO2

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