Chapter 1: Atomic Structure and the Periodic Table 1.1 Atoms are the smallest form of elements.

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1 Chapter 1: Atomic Structure and the Periodic Table 1.1 Atoms are the smallest form of elements. All matter is made of atoms. About 100 different atoms, or elements, make up everything on Earth. Hydrogen is the most abundant element in the universe, it makes up 90% of all elements in the universe. Oxygen is the most abundant element in the human body and in Earth's crust. The structure of an atom

2 Nucleus: is at the center of the atom, and is a combination of protons and neutrons. Protons: are positively charged particles. Neutrons: are particles that have NO electrical charge. Protons and neutrons have approximately the same mass. Electrons: are tiny particles with a negative charge.

3 o They form a cloud, because at the same time that they repel each other, they are attracted to the positively charged protons in the nucleus. (2000 times smaller than protons and neutrons) What part of the atom has a positive charge, negative charge and no charge? What is the smallest sub-atomic particle? Atomic Number: is the number of protons in an atom s nucleus. Atomic mass number: is the combined number of protons and neutrons in a nucleus. Isotopes: are atoms of an element that have a different number of neutrons. For example, most carbon atoms contain 6 protons and 6 neutrons. Some carbon

4 atoms, however, have 6 protons and 8 neutrons. Chemists will often put the atomic mass number after the element's name, such as carbon-12 or carbon-14, to signify different isotopes. How would we write these isotopes? What is the difference between each isotope?

5 Atomic Mass: of an element is the average mass of all the element s isotopes. Ions are atoms that have lost or gained one or more electrons. They no longer contain equal numbers of protons and electrons, so they have an electric charge. Atoms that have lost electrons are positive ions; atoms that have gained electrons are negative ions.

6 An electron is lost The Na a because proton th Sodium atom (Na) 11 protons & 11 electrons Sodium ion (Na + ) 11 protons & 10 electrons An electron is gained Chlorine atom (Cl) 17 protons & 17 electrons Chlorine atom (Cl - ) 17 protons & 18 electrons 1.2 Elements make up the periodic table. Mendeleev s Periodic Table A Russian chemist, Dmitri Mendeleev, was the first to produce a periodic table of the elements. His periodic table was organized by increasing atomic mass and similarities in chemical properties.

7 The periodic table has a system of organization. The number at the top is the atomic number. The big bold letters are the chemical symbol The name of the element is below the chemical symbol. Under the name is the atomic mass number. The periodic table is organized into groups and periods. In a group (vertical column) of the periodic table, elements show similarities in their physical and chemical properties.

8 In a period (horizontal row) of the periodic table, the physical and chemical properties change in a predictable way from one to the next, and the atomic number increases by one across a period. How is the modern periodic table different then Mendeleev s? An element's position in the periodic table dictates what type of ion it will form. Atoms at the left of the table tend to lose an electron to form positive ions Atoms at the right of the table tend to gain electrons to form negative ions. Atoms in group 18 rarely form ions at all. Atoms in groups 3-12 all form positive ions.

9 Atomic size and density show patterns in the periodic table. Density generally increases from the top of a group to the bottom of a group. Elements to the left and right sides of the periodic table are less dense than the elements in the middle of the table.

10 Atomic size increases, or gets larger, from top to bottom. Atomic size decreases, or gets smaller, from left to right.

11 1.3 The periodic table is a map of elements. The periodic table has distinct regions Metals (Yellow) Nonmetals (Green) Metalloids (Purple) The element's position on the periodic table determines how reactive it is

12 Reactivity is a measure of how likely an element is to undergo a chemical change. Most elements are metals. Metals are elements that conduct electricity and heat well and have a shiny appearance. The most reactive metals in the periodic table. Alkali metals in Group 1 (most reactive) Alkaline earth metals in Group 2 (more reactive than most other metal elements, but not as reactive as those in group 1) Transition metals in the middle of the periodic table, like iron and copper, are less reactive and were among the first known elements.

13 Rare earth elements are the elements in period 6, the portion taken out of the body of the periodic table. Nonmetals Most nonmetals are gases at room temperature. In the solid state, nonmetals have dull surfaces and can be hammered into shape or drawn into a wire. Halogens in Group 17 are very reactive nonmetals. The noble gases in Group 18 almost never react with other elements. Metalloids Have properties of both metals and nonmetals. Metalloids make up the semiconductors in electronic devices.

14 The metalloid silicon is the second most abundant element in the Earth's crust.

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