Lesson Outline

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Lesson Outline

• Lesson 1 - The Atom
• Lesson 2 The Periodic Table
• Lesson 3 Groups of The Periodic Table

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Lesson 1

• The Atom

Back to the Lesson Outline
3
Bell Ringer Answer the following questions

• Does this cube of sugar contain atoms?
• Does a grain of sugar contain an atom?
• If you mix sugar with water, does the sugar now
  contain atoms?

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Answer

• The cube of sugar is made up of many grains of
  sugar, which contain atoms. Even the smallest
  grain of sugar contains an atom.
• When you add sugar to water, it may seem like the
  sugar completely dissolves. In all actuality, the
  sugar is still present and still contains atoms.

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Why do we need to know this?

• Everything around us is made up of matter, and
  the simplest form of matter is an atom.
• An atom is the smallest component of an element
  having the chemical properties of that element.
• An atom can exist either alone or in combination
  with other atoms.

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Objective

• Students will be able to
• Identify the parts of an atom, and explain each
  part, which includes the protons, neutrons, and
  electrons.
• Will apply this knowledge to the introduction of
  the periodic table.
• PA Standards
• 3.1.12E 3.4.10A

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So what makes up an atom?
Electrons
Nucleus
Protons
Neutrons
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The Structure of the Atom

• At the center of every atom there is a nucleus
  which holds the positively charged protons and
  the neutrally charged neutrons.
• Surrounding the center of the atom is the
  electron cloud that holds the moving negatively
  charged electrons.

Click here to see where these three parts of an
atom are located
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Electrons

• Orbit the nucleus
• Each atom contains orbitals, which is a 3-D
  region around the nucleus in which the electrons
  are located.
• Click to see the number of orbitals and the max
  electrons in each orbital.

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Protons and Neutrons

• Both of which are located in the nucleus of an
  atom.
• Protons- subatomic particles that have a positive
  charge equal in magnitude to the negative charge
  of an electron.
• Neutrons- subatomic particles that have a neutral
  charge.
• All atoms have neutrons except for the simplest
  type of Hydrogen.

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Closure

• What is an atom?
• What particles make up an atom?
• Where are these particles located?

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Interactive Activities

• Click here to identify the particles of an atom
• Click to see an electron orbit the nucleus.
• Click here for an Atom Builder activity.
• Click here for an example of an interactive atom.
• Want to know more about the atom? Click here!

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Lesson 2

• The Periodic Table

Back to the Lesson Outline
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Bell Ringer What do these 2 pictures have in
common?
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Importance of the Periodic Table

• The Periodic Table is the most important tool to
  chemists.
• It lists every known element and their
  arrangement based upon similar number of
  electrons and protons.

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Objective

• Students will be able to
• Recall prior knowledge about the atom.
• Learn about the development of the Periodic Table
• Classify atoms in the periodic table based on the
  number of protons, neutrons, and electrons.
• PA Standards
• 3.1.10C 3.4.10A 3.1.12E

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Pre-Periodic Table

• A big mess
• The elements were not organized.
• Imagine going to a library that was not organized
• It would be difficult to find information

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How did the Periodic Table become organized?

• Dmitri Mendeleev Father of the Table
• How it worked
• Put elements in rows by increasing atomic weight.
• Put elements in columns by reactivity
• Click here to view the Mendeleevs periodic table

• Some problems
• Blank spaces were left for elements that were
  said to have not been discovered yet.
• His pattern of increasing atomic weight was
  broke-now organized by reactivity.

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The Current Periodic Table

• Mendeleev was on the right track
• Nowthe elements are put into rows by increasing
  Atomic Number!
• The horizontal rows are called periods, which are
  labeled from 1 through 7.
• The vertical columns are called groups, which are
  labeled from 1 to 18.

• Click here to see the difference between the 2.

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What information can we get from the Periodic
Table?

• Periodic Table provides us with an elements
  symbol,atomic number,and atomic mass
• Where can we find these on the Periodic Table?

Symbol
Atomic Mass
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What is Atomic Number and Mass?

• Atomic number- the number of protons in the
  nucleus of each atom of that element.
• Atomic mass- the total number of protons and
  neutrons in the nucleus of an isotope.
• The of protons the of electrons.
• To find the number of neutrons subtract the
  atomic number from the atomic mass.
• Click here for an example

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Closure

• Who is the Father of the Periodic Table?
• How can one identify an element?
• What information does the periodic table provide
  us with?

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Interactive Lessons

• Click here to complete the worksheet on the last
  2 lessons.
• For students with visual impairments, click here
• For students with physical disabilities, click
  here
• Click here for flashcard review
• Chemistry Jeopardy Game
• Click to move onto Lesson 3

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Lesson 3

• Groups of The Periodic Table

Back to the Lesson Outline
25
Bell Ringer

• Recall the information about an element from
  Lesson 2
• Identify the Atomic and Atomic Mass of
  Magnesium.
• How many protons, neutrons, and electrons does
  Magnesium have?

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Answer

• Atomic 12
• Atomic mass 24
• of protons 12
• of electrons 12
• of neutrons 12

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Students will be able to

• Examine the location of each elements in its
  group on the periodic table.
• Identify the names of certain groups in the
  periodic table.
• PA Standards
• 3.4.10A 3.4.12A 3.5.10A 3.6.10C

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Groups are also known as families

• Why are the elements organized in groups?
• Elements in the same group have similar chemical
  and physical properties.

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Group 1 Alkali Metals

• 1st column of the Periodic Table (except for
  Hydrogen)
• Li, Na, K, Rb, Cs, and Fr
• Combine vigorously w/many nonmetals.
• Extremely reactive, therefore they are not found
  in nature as free elements.
• Soft enough to cut w/a knife

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Group 2 Alkaline Earth Metals

• 2nd column of the Periodic Table
• Be, Mg, Ca, Sr, Ba, and Ra
• Harder, denser, and stronger metals with a higher
  MP than alkali metals
• Less reactive than alkali metals
• Always combined with nonmetals

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Groups 3-12 Transition Metals

• Least reactive metals
• Hardest of the metals
• Mostly used in construction or jewelry

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Groups 13-18

• These groups are known as the metals
• They are located to the right of the staircase
• Click here to locate the metals and nonmetals

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Halogens

• Group 17
• Very reactive,volatile,nonmetals
• Always combined with another element in nature
• Halogens are used in bleaches, water
  purification, insecticides.

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Noble Gases

• Group 18
• Least reactive gases
• Harder and denser than alkaline earth metals
• Have a full valence shell of electrons(contain 8
  electrons in their outer shell)
• Used in neon lights

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Other Families

• Group 13 Boron Family
• Group 14 Carbon Family
• Group 15 Nitrogen Family
• Group 16 Oxygen Family

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Closure

• Based on the information discussed, see if you
  can complete this review.Click here!
• Elemental FlashcardsTry this!
• Arrangement of elements challenge.
• Mystery Element game!

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Location of the parts of an atom
Return to Lesson 1
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Energy Levels
Return to Lesson 1
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Electron
Proton
Neutron
Click here to return to Lesson 1
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Periods 1-7

• Click here to view the groups

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Groups 1-18

• Click to go back to Lesson 2

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Metals and Nonmetals
Click to return to Lesson 3
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Example Atomic Mass and Atomic Number of the
following

• Mass 23
• Atomic 11
• of protons 11
• of neutrons 12
• (23-11)
• of electrons 11

Click to return to Lesson 2