Transcript Section 2.0
Section 2.0 An understanding of the nature of matter has developed through observations over time. Goals for this Section: 1. Describe ancient theories of matter and chemical change 2. Distinguish between observation and theory 3. Describe the different models of the structure of the atom 4. Identify patterns that are used to group elements 5. Describe the arrangement of atoms within the periodic table 6. Use the periodic table to describe the properties of individual atoms 7. Explain relationships within periods and groups within the periodic table 2.1 – Evolving Theories of Matter • We could consider stoneage people to be the very first chemists • They learned to use fire as a tool to produce chemical changes that made their lives easier http://www.mrdowling.com Early Interests in Metals & Liquids • Until about 1000 B.C., chemists only investigated materials that had high value to humans • Most of these materials were metals, such as gold, copper, and iron • Other substances of interests were liquids such as oils and plant juices http://www.shee-eire.com The Idea of the Atom • The first scientist to suggest an idea of an atom was Democritus, in about 400 B.C. • He suggested that all matter was made up of very small, indivisible particles known as atomos • However, another Greek philosopher had a more popular idea… Earth, Wind & Fire (… and Water) • Aristotle suggested that all materials contained different proportions of four elements – Earth, Wind, Fire, and Water • This idea was the preferred theory about the composition of matter for about 2000 years http://www.britannica.com Alchemy • Alchemy was a field of study where the “scientists” attempted to find elixirs that would extend life, or to develop a method of turning base metals into gold http://hem.fyristorg.com Alchemy and Chemistry • In fact, some of the most famous alchemists were in fact good con-men who managed to convince nobles to provide them with money in return for recipes for creating gold from base metals • However, these alchemists did contribute to what we now know as legitimate chemistry • Many of the chemical reactions that were used by alchemists are now used by chemists, and much of the specialized apparatus that is used in chemistry was developed by alchemists as well http://www.powerlabs.org The Modern Chemists • Early chemists like Robert Boyle and Antoine Lavoisier began to develop theories about matter and reactions based on observations and experiments • Eventually, by the 1800s, an atomic theory began to take shape Dalton’s Model http://192.107.108.56 http://turing.kingsu.ca J.J. Thomson’s Experiment http://www.lightandmatter.com Thomson’s Model Rutherford Scattering Rutherford’s Model http://www.osa.ceu.hu Bohr & Atomic Spectra http://outreach.atnf.csiro.au The Bohr Model http://education.jlab.org Modern Models http://static.howstuffworks.com 2.2 – Organizing the Elements • Rather than using names for chemicals early scientist used symbols for the elements that they knew • Scientists tried to organize elements by using their properties, however, this was difficult because different scientists used different properties • John Dalton first attempted to categorize and order the elements in the early 1800’s. He developed a new system of symbols Jöns Jacob Berzelius • In 1814 Berzelius suggested using letters rather than symbols • the first letter is capitalized • if two elements had the same first letter (like Hydrogen and Helium) then the second letter would be used • this system is still in use today The Evolution of Symbols Ordering the Elements • order for the elements was soon discovered by using the atomic mass as a means to list them • scientists could establish the average mass of an atom by comparing it to the mass of a carbon atom • in 1864 John Newlands recognized that there was a pattern of repeating properties within the elements when they were listed in increasing mass Dimitri Mendeleev • Dmitri Mendeleev arranged elements by their chemical properties • When he did this, a clear pattern emerged • There were holes in his pattern created by undiscovered elements • These holes were filled over time – showing that Mendeleev’s table was accurate 2.3 – The Periodic Table Divisions Within the Periodic Table • The table can be divided into horizontal rows (periods) or vertical columns (groups or families) • Each box within a periodic table contains important information Useful Information on Each Elements 8 2- O oxygen 16.0 Atomic Mass and Isotopes • The atomic mass of an element provides you with the total mass of the protons and neutrons in an atom • However, you will notice that not all atoms have atomic masses that are whole numbers • Because you cannot have fractions of protons and neutrons, what is happening here? • It turns out that the atomic mass is the average weighted mass of different isotopes of an atom • For example, there are three different isotopes of hydrogen: http://images.encarta.msn.com Protons + Neutrons = Atomic Mass Fun! • We can determine the number of protons and neutrons in the nucleus of an atom by using its atomic number and its atomic mass # of Protons (Atomic Number) + # of Neutrons _______________ Atomic Mass Example: Number of Protons & Neutrons in Uranium • Uranium has an atomic mass of 238.0. How many protons and neutrons are present in this element? Metals & Nonmetals • There are two major groups of elements in the periodic table – the metals and the nonmetals Metals http://www.britannica.com • Properties: Nonmetals • Properties: http://www.britannica.com Groups • There are 18 groups on the modern periodic table • The elements that make up a particular group typically have similar reactivity and often engage in the same reactions and form similar products Periods • Periods are repeating patterns of elements created by the separation of elements into their groups • The atomic mass of elements increases as you move from left to right along a period General Reactivity of Elements Group 1 – Alkali Metals • These are the most reactive metals • They will react when exposed to air or water • Typically will not be found in their elemental state in nature http://www.webelements.com Group 2 – Alkaline Earths • Reactive metals, although their reactivity is much lower than the alkali metals • React readily with air and water • Many are combustible http://upload.wikimedia.org Group 17 – The Halogens • These are the most reactive nonmetals • They are all diatomic, meaning that in their natural state, two atoms of the element are bonded together http://en.wikipedia.org Group 18 – The Noble Gases • These gases are all very stable – in fact, until 1962 it was believed that they would not react at all http://en.wikipedia.org