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Atoms: The Building Blocks of Matter

Learn about atoms, the smallest particles that make up elements. Discover their structure, including the nucleus and subatomic particles. Understand atomic charge, mass, and symbols. Explore isotopes and their significance.

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Atoms: The Building Blocks of Matter

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  1. Chapter 4 Atoms

  2. Atoms • The smallest particle that has the properties of an element.

  3. Dalton’s Atomic Theory • Every element is made of tiny, unique, particles called atoms that cannot be subdivided. • Atoms of the same element are exactly alike. • Atoms of different elements can join to form molecules or compunds

  4. Parts of an Atom • Nucleus – small, dense center of an atom made up of 2 subatomic particles that are identical in size and mass. • Protons – have a positive charge • Neutrons – have no charge

  5. Parts of an Atom cont. • Electrons – are tiny subatomic particles that have very little mass that moves around the outside of the nucleus. These particles are negatively charged and form a “cloud” around the nucleus.

  6. The number of protons and electrons an atom has is unique for each element.

  7. Atomic Charge • Atoms have no overall charge because the protons (+) cancel out the electrons (-). Helium 2 protons - +2 2 neutrons - 0 2 electrons --2 total charge 0

  8. Protons • positive (+) charge • Found in the nucleus • # of protons = atomic # • The number of protons identify the element (atomic #)

  9. Neutrons • no charge • Found in the nucleus • Along with protons makes up atomic mass • Atomic Mass – atomic number = # of neutrons (rounded to whole #)

  10. Electrons • negative (–) charge • travel in orbitals (or energy levels) around the nucleus. (electron cloud) • Equals atomic number in neutral atoms • valence electrons - the # of electrons in the outer shell and relates to the oxidation #

  11. Unit of measure for atomic particles is Atomic mass unit (amu) protons and neutrons = about 1 amu (electrons are about 1/2000 of the size of protons and neutrons))

  12. Chemical symbols • The one or two letter abbreviation of the element name. • Some are based on Latin name • ALL 1st letter is upper case • ALL 2nd letter is lower case

  13. Mass Number or Atomic Mass • the sum of the number of protons and the number of neutrons in the nucleus of an atom. • # of neutrons = mass # - atomic # Neutrons Protons +

  14. Atom Summary • Atomic Number = protons = electrons • Atomic Mass = Protons + Neutrons • Neutrons = atomic mass – atomic number • Atomic symbols • First letter is ALWAYS upper case • Second letter is ALWAYS lower case • Example: Oxygen element 6 with mass 16 P = 8 E = 8 N = 16-8 = 8

  15. Isotopes • Atoms of the same element that have a different # of neutrons and a different atomic mass. (identified by the element name followed by the mass # ) • ex. C-12, C-14, B-10, B-11) Carbon 14 = 8 neutrons 6 protons 6 electrons 6 electrons 6 protons Carbon 12 = 6 neutrons

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