Download presentation
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?
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
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
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+
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
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
Similar presentations
© 2024 SlidePlayer.com Inc.
All rights reserved.