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The Atom The Periodic Table

Learn about atoms, their subatomic particles, atomic numbers, mass numbers, isotopes, electron arrangements, and how the periodic table organizes elements. Explore the properties and classifications of metals, nonmetals, metalloids, alkali metals, alkali earth metals, halogens, and noble gases.

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The Atom The Periodic Table

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  1. The Atom The Periodic Table

  2. Comparing Atoms

  3. The Atom • Atoms are the smallest part of all matter. • All atoms contain three smaller particles called subatomic particles: • Protons: positive particle • Neutrons: neutral particle • Protons and neutrons have the same mass • Electrons: negative particle with very little mass

  4. Atoms • Atoms are neutral; they have the same number of electrons as protons. • Example: An atom of 42He has an atomic number of 2 and a mass of 4. Therefore, it has 2 protons and 2 neutrons in its nucleus. Since it has 2 positive protons (neutrons are neutral) it must have 2 negative electrons to make the total charge neutral.

  5. How does one kind of atom differ from another? • Number of protons determines an element. • Even if atoms bond or break apart, number of protons will always be the same.

  6. Protons and neutrons cluster together in the atom’s center called the nucleus. • Electrons orbit the nucleus. • An atom is only about 0.0000000001 meters big. It would take 10 BILLIONS atoms lying side by side to equal 1 meter!

  7. What is the atomicnumber? • Atomicnumber is number of protons an atom contains. • Atomic numbers start at one, with hydrogen, and go up by ones until element 111, unununium.

  8. MASS NUMBER • The massnumber is equal to the total number of protonsplusneutrons.

  9. AVERAGE ATOMIC MASS • Atomicmass is the average of all the known isotopes of an element.

  10. Atomic Mass/Mass Number • The mass number can be written as a superscript above the symbol and the atomic number as a subscript below the symbol.

  11. Isotopes • Atoms of the same element can have different numbers of neutrons. • These different forms of the same element are called isotopes. • The atomic mass is the average mass of all the known isotopes of the element.

  12. How are electrons arranged? • Electrons are located in different energy levels. • The farther away from the nucleus the electron is found, the higher the energy. • As electrons move from a lower level to a higher level energy is absorbed. • As electrons move from a higher level to a lower level energy is release in the form of light.

  13. Group Periodic Table • The elements are listed in order of increasing atomic number. • By looking at the row (period) number you can determined how many energy levels are filled. • By looking at the column (group) number you can determine how many electrons are in the outermost level. Period

  14. Group 1 (blue) – Alkali metal; note Hydrogen is a gas, not a metal • Group 2 (red) – Alkali Earth Metals • Group 7 (pink)– Halogens • Group 8 (brown) – Nobel Gases – do not react with anything • Metalloids – (purple, staircase) acts like both metal and nonmetal • Metal – (yellow, red, blue) – left of metalloids • Nonmetal – (green, pink, brown) – right of metalloids

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