Chapter 6: The Periodic Table. Section 6.1: Organizing the elements
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1 Chapter 6: The Periodic Table Section 6.1: Organizing the elements
2 How do we know that we have found all of the elements? Some elements have been known to exist for thousands of years By 1700 only 13 elements had been discovered When scientists starting using the scientific method to analyze elements the rate of discovery significantly increased
3 How can you group elements together? In the 1820s, J.W. Dobereiner began grouping elements together into Triads A Triad is a set of three elements with similar properties - One example is Chlorine, Bromine and Iodine Grouped together because they all react easily with metals Did not work for all elements
4 Who is Dmitri Mendeleev? How did he change our understanding of chemistry? Dmitri Mendeleev was a Russian Chemist working in the mid 19th Century He was writing a textbook, and investigated how elements were related He wrote properties on cards, and arranged them until he found an organization which worked His table was based upon the atomic mass of an element He left gaps were he thought elements should go that had not been discovered, and was ultimately proved correct
5 How is Mendeleev s periodic table different to todays? For same elements, Mendeleev had to ignore atomic mass in order to group elements with similar properties together Instead, we no know that elements should be arranged in order of increasing atomic number rather than mass
6 The modern periodic table Period: Row Group: Column Periodic law: When elements are arranged in order of increasing atomic number; there is a periodic repitition of their properties
7 There are other ways to classify elements rather than simply groups There are three classes of elements; metals, nonmetals and metalloids
8 What are the key characteristics of metals? Metals make up 80% of the periodic table They are good conductors of heat and electric current They often have a high luster, and are shiny (reflect a lot of light) With the excpetion of mercury, all are solid at room temperature Many are ductile, meaning they can be drawn into wires Many are malleable, meaning they can be hammered into thin sheets
9 What are the key characteristics of nonmetals? Most are gasses at room temperature, some are solid and only one is liquid There is much more variation among nonmetals than metals Hard to give general properties, although most tend to be the opposite of metals There are exceptions - eg. carbon will conduct electricity
10 What about metalloids? A metalloid has some properties that are similar to metals and some that are similar to nonmetals At times it behave like a metal, at times it may behave like a non-metal Scientists can sometimes change the behavior of a metalloid For example - silicon is a poor conductor of electricity, but add a small amount of boron and it will become a great conductor of electric current This mixture is used to make computer chips
11 Classifying the elements Section 6.2
12 Why is the periodic table so useful? It contains so much information!
13 What information exactly? Individual elemental squares can contain: Atomic number and atomic mass, element symbol and name, AND number of electrons in each energy level The color of the Chemical symbol can be used to distinguish state of matter, or whether it is found in nature Background color of square links elements that have similar properties Example - Group 1A and Group 2A elements are orange, but different shades Same idea with halogens, group 7A
14 What is the connection between an element s electron configuration and many elemental properties? Elements can be sorted into four classes on the basis of the their electron configurations
15 What is special about the nobel gasses? These are the elements found in group 8A Often referred to as inert gasses, as they rarely take part in reactions; largely due to their electron configuration They are the only elements whose highest energy levels are completely filled.
16 What is a representative element? An element in group 1A through 7A There are a wide range of physical and chemical properties Characteristic is that the s and p sublevels of the highest occupied energy levels are not filled For any representative element, the group number is equal to the number of electrons in the highest occupied energy level
17 What are the transition elements? These are the B group elements found in the middle of the periodic table Transition metals: Group B elements in the main body of the table. They contain electrons in d orbitals Inner transition metals: They do not appear in the main periodic table Electron contained in a f orbital
18 Block view of periodic table Why didn t I just teach you electron configuration this way? What is the electron configuration of Nickel?
19 Periodic trends Section 6.3
20 What is atomic size, why is it important? Atoms have different sizes These can be calculated from looking at molecules, and measuring the distance between nuclei (half this distance is the atomic radius) This distance is very small It is often expressed in picometers (pm). There are one trillion (1012) picometers in a meter.
21 Group trend in Atomic radius
22 Group trends in atomic radius What changes across the periodic table? As atomic number increases the nucleus has a greater positive charges, drawing the electrons closer to the nucleus
23 Why do atoms get bigger then as you move down a group? Electron shielding The electrons in the lower energy levels acts as a shield between the charge of the nucleus and the electrons in the highest energy levels
24 Why does size decrease along a period?
25 Period trends explained The shielding effect remains the same as you move across the period, but the number of protons remains the same The increased positive charge in the nucleus draws the outer electrons in closer, decreasing atomic radii.
26 What is an ion? An ion is an atom or a group of atoms that has a positive or a negative charge. They form when electrons are transferred between atoms Ions with positive charge (more protons than electrons) are called cations Ions with a negative charge (more electrons than protons) are called anions
27 What is Ionization energy? Ionization energy is the energy required to remove an electron from an atom The first ionization energy is the energy required to remove the first electron from an atom
28 Trends in Ionization energy As you move down a group less energy is required to remove an electron from that level, so the ionization energy is smaller As move from left to right along a period, nuclear charge increase yet shielding remains the same, so more energy is required to remove an electron from an atom
29 Second and third ionization energies Sometimes more than one electron can be removed from an atom The energy needed to remove a second electron is the second ionization energy The energy needed to remove the third is the third ionization energy The energy level needed increases as you move to subsequent ionization energies Ionization energies allow you to predict the possible ions that an element can form
30 Are there any other trend you need to know about! Yes! Metals tend to lose electrons and form cations Nonmetals tend to gain electrons and form anions Cations are always smaller than the atom from which they formed Anions are always larger than the atom from which they formed
31 What is electronegativity? Electronegativity is the ability of an atom to attract electrons when the atom is in a compound Fluorine is the most electronegative element (value of 4) Caesium is the least electronegative element (value of 0.7)
32 Periodic trend summary
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