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Chapter 6 The Periodic Table

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1 Chapter 6 The Periodic Table
Stylish Shoes

2 What is in common with all the pictures below?

3 Which one does not belong?

4 Which one does not belong?

5 Which one does not belong?

6 Which one does not belong?

7

8 History of the Periodic Table
Mendeleev published a classification scheme of all the currently known elements Organized elements based on similar characteristics. Left blank spaces in table for undiscovered elements.

9 Mendeleev’s Periodic Table (1869)
Mendeleev arranged the elements on his table in order of increasing atomic mass.

10 Many scientist suggested other periodic tables.
Albert Tarantola’s Orbital Table                                                                            

11 Timothy Stowe – Table for Physicists
                                                     

12 Theodor Benfey                                                                            

13 Emil Zmaczynski                                                        

14 Vocational Exile Periodic Table

15 The Periodic Law In the modern periodic table, elements are arranged in order of increasing atomic number

16 Periodic Law – when elements are arranged in order of increasing atomic number, there is a trend in their physical and chemical properties

17 Metals, Metalloids and Nonmetals
Elements can be grouped into three broad classes based on their general properties Metals Nonmetals Metalloids

18 Metals: Generally solid at room temp. Ductile – drawn into wires. Malleable – hammered into sheets Shiny surface Conduct heat and electricity

19 Metals

20 Nonmetals: Varying properties, but are generally poor conductors of heat and electricity Brittle

21 Non-metals Nonconductors

22 Metalloids: some properties of metals and nonmetals Intermediate

23 Metalloids or Semimetals
Properties of both

24

25 Practice Tell me all you can about the following elements:
Titanium (Ti) Germanium (Ge) Calcium (Ca) Fluorine (F) 1- Ti – metal, 2 – Ge – metalloid, 3 – Ca – metal, 4 – F – nonmetal,

26 Section 6.2 - Classifying the Elements
The periodic table displays the symbols and names of the elements, along with information about the structure of their atoms (# of protons, neutrons, and electrons)

27 Black symbol = solid Green = gas Blue = liquid

28 Electron Configurations in Groups
Elements can be sorted into 4 different groupings based on their electron configurations: Noble gases Representative elements Transition metals Inner transition metals *

29 Transition Representative Inner Trans. Noble Gases

30 Electron Configurations in Groups
Noble gases elements in Group 8A Very stable = do not react Noble gases have an electron configuration that has the outer s and p sublevels completely full *

31 Ci Circle the Noble Gases

32 Electron Configurations in Groups
Representative Elements are in Groups 1A through 7A Display wide range of properties, thus a good “representative” Include metals, nonmetals, metalloids, solids, gases, or liquids Their outer s and p electron configurations are NOT filled *

33 Circle the Representative Elements

34 Electron Configurations in Groups
Transition metals are in the “B” columns of the periodic table Electron configuration has outer s sublevel full Elements in the “d” sublevel A “transition” between the metal area and the nonmetal area *

35 Circle the Transition Metals

36 Electron Configurations in Groups
Inner Transition Metals are located below the main body of the table, in two horizontal rows Electron configuration has the outer s sublevel full Elements in the f sublevel *

37 Circle the Inner Transition Metals

38 Elements in the 1A-7A groups are called the representative elements
outer s or p filling 1A 8A 2A 3A 4A 5A 6A 7A *

39 The group B are called the transition elements
These are called the inner transition elements, and they belong here *

40 Groups of elements - family names
Group 1A – alkali metals Forms a “base” (or alkali) when reacting with water Exception is Hydrogen Group 2A – alkaline earth metals Also form bases with water; do not dissolve well, hence “earth metals” Group 7A – halogens Means “salt-forming” *

41 Group 1A - alkali metals (but NOT H) Group 2A - alkaline earth metals
*

42 Group 8A are the noble gases Group 7A is called the halogens
*

43 The Groups of the Periodic Table
Representative Elements Noble Gases Transition Metals Inner Transition Metals Family names: Alkali metals Alkaline earth metals Halogens

44 Practice Tell me all you can about the following elements:
Titanium (Ti) Germanium (Ge) Calcium (Ca) Fluorine (F) 1- Ti – metal, inner trans. 2 – Ge – metalloid, representative 3 – Ca – metal, representative, alkaline earth metal 4 – F – nonmetal, rep, halogen

45

46 Section 6.3 – Periodic Trends
Properties of elements are related to their location on the periodic table We will be studying 3 periodic trends: Atomic Radius Ionization Energy Electronegativity

47 1. Atomic Radius or Atomic Size
One-half the distance from center to center of two atoms Atomic Radius

48 Atomic Radius or Atomic Size
What do you notice about the atomic radii of the elements on the periodic table? Atomic Radius increases towards the bottom left corner of the PT

49 Atomic Radius/Size Practice
Which element has a greater atomic radius? F or Cs Ga or K Kr or Rb Ba or Si Fr or W O or Ag

50 Ions Normally, atoms are neutral because they have the same number of protons and electrons When elements combine in compounds, they transfer electrons. Ions are atoms that have a positive or negative charge.

51 Transfer of an electron forms two ions: a cation and anion

52 Cations Circle the cation
Cation – an ion with a positive charge (lost electrons) Circle the cation Na+

53 Anions Circle the anion
Anion – an ion with a negative charge gained electrons) Circle the anion Na+

54

55 Ionic Size Cations are always smaller than the atoms from which they form Anions are always larger than the atoms from which they form

56 Before After

57 Does this make sense? Where are electrons located in the atom? Around the nucleus The more electrons around the nucleus, the larger the atom will be.

58 Practice Which of the following is larger? Na or Na+ Al or Al3+
I or I- Ca2+ or Ca S or S2- O2- or O

59 2. Ionization Energy The energy required to remove an electron from an atom

60 Ionization Energy What trend do you notice about the ionization energy of the elements on the periodic table? Ionization Energy increases towards the top right corner of the PT

61 Does this make sense? Which elements are the most stable? Elements with full orbitals The more stable the elements is, the harder it will be to remove an electron.

62 Ionization Energy Practice
Which of these elements has a greater ionization energy? Kr or Ar Al or Na S or Rb Si or Cs He or Ca P or O

63 3. Electronegativity (EN)
The ability of an atom to attract electrons to itself when in a compound

64 Electronegativity What trend do you notice about the electronegativity of the elements on the periodic table? Electronegativity increases towards the top right corner of the PT

65 Does this make sense? Which elements want electrons? Elements closest to filling their orbitals The closer the elements is to filling its orbital, the more it will attract electrons.

66 Electronegativity Practice
Which element has greater electronegativity? Na or F Ca or C Al or Mg Sr or Al Ca or K Cl or F

67

68 Draw a diagonal arrow showing increasing atomic size

69 Draw a diagonal arrow showing increasing ionization energy

70 Draw a diagonal arrow showing increasing electronegativity


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