THE PERIODIC TABLE

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THE PERIODIC TABLE
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The families (groups) are described by...

• PHYSICAL PROPERTIES - Density- Boiling Point-
  Melting Point- Conductivity- Heat Capacity

• CHEMICAL PROPERTIES - Valence electrons-
  Reactivity- Radioactivity

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• Families (groups) on the periodic table are
  similar in that they have the same numbers of
  valence electrons and want to bond with similar
  elements.

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• Periods are the rows of the table.
• Families/group are the columns.

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Metals

• Metals have LOW melting points and have luster.
• Conduction Metals are good at conducting
  electricity.
• Reactivity Metals are very reactive,most form
  compounds with other elements quite easily.
  Sodium (Na) and potassium (K) are some of the
  most reactive metals

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Transition metals

• These elements in the center of the periodic
  table are able to have more than one oxidation
  number and tend to not follow a similar pattern
  like the other families.
• Also includes the lanthanide and actinide series
  which are located below the bottom of the chart.

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Non metals

• These elements do not conduct electricity or heat
  well, lack luster and generally are not
  malleable.
• These elements want to gain electrons when
  bonding.

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Halogens

• When a halogen combines with another element, the
  resulting compound is called a halide. These
  elements are NOT very reactive.

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Noble gases

• These are sometimes called the inert gases.
• Dont bond with other elements because they have
  a full outer electron shell.

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Major scientists

• John Dalton developed the theory of atomic
  theory. Within theories he described matter as
  having small particles called atoms and that each
  of these particles are identical.

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• Democritus- 1st to identify that all matter is
  made of atoms.
• Plucker, Crooks and Thomas- 1st to use chemicals
  to conduct current.

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• Ernest Rutherford- used a gold foil and alpha
  particle experiment to theorize that in the most
  empty space of the atom existed a positive
  center.

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THE ATOM

• The atom is the smallest part of an element.
• In 1913, Neil Bohr created a model of the atom
  that contained the proton, neutron, and the
  electron

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• Protons The POSITIVELY charged particle in the
  nucleus.
• Neutrons The NEUTRALLY charged particle in the
  nucleus.
• Electrons The NEGATIVELY charged particle
  orbiting the nucleus in energy levels.

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Chemistry Vocab

• Atomic The of protons in the nucleus. This
  can NEVER change for a particular element.
• Atomic mass The of protons the of neutrons
  in the nucleus.

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ISOTOPES

• An isotope occurs when the of neutrons in an
  atom changes thus changing the atomic mass of the
  atom. Remember that the protons can NEVER change
  in an atom.

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Electron pattern

• Electrons follow a pattern when orbiting the
  nucleus. For this class we will use the 2, 8,
  8, scheme.

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Bohr model

• Put the PROTONS and NEUTRONS in the NUCLEUS
• ELECTRONS should be placed in energy rings around
  the nucleus.

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Draw a Bohr model for

• Oxygen
• Sodium
• Circle with a P in it for Proton circle with an
  N in it for Neutron circle with E for electron

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OXYGEN

• 8 PROTONS
• 8 NEUTRONS
• 8 ELECTRONS

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SODIUM

• 11 PROTONS
• 12 NEUTRONS
• 11 ELECTRONS

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Lewis dot diagrams

• Lewis dot diagrams show the valence electrons of
  elements in a standard shorthand. Write the
  elements symbol. Then through first 4,
  right-left-top-bottom then counter-clockwise
  beginning at the top for 5-8.
• Ex. Ge Se

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Quiz

1. Atomic
2. In an electrically neutral atom, the of protons
   is equal to the ________
3. _____ are aligned vertically
4. Rows in the PT of E are called ________
5. Abbreviation of element
6. Protons neutrons location
7. Maximum of energy levels is to ______________

1. Groups (families)
2. Nucleus
3. Periods
4. of protons in the nucleus
5. of periods
6. Symbol
7. Electrons