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Stability and Ionic Bonding. Section 20.1 & 20.2. SC Standards Covered. Standard PS-4.1 Explain the role of bonding in achieving chemical stability. Standard PS-2.5

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Stability and Ionic Bonding

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Stability and ionic bonding

Stability and Ionic Bonding

Section 20.1 & 20.2

Sc standards covered

SC Standards Covered

  • Standard PS-4.1

  • Explain the role of bonding in achieving chemical stability.

  • Standard PS-2.5

  • Predict the charge that a representative element will acquire according to the arrangement of electrons in its outer energy level.

  • Standard PS-4.6

  • Predict the ratio by which the representative elements combine to form binary ionic compounds, and represent that ratio in a chemical formula.

  • Standard PS-4.4

  • Classify compounds as crystalline (containing ionic bonds) or molecular (containing covalent bonds) based on whether their outer electrons are transferred or shared.

Combined elements

Combined Elements

  • Most elements are not found by themselves in nature

  • Usually they are found combined with other elements

  • Two or more elements chemically combined is called a compound

  • The properties of a compound are very different from the properties of the elements that make up the compound

Consider table salt

Consider Table Salt…

Chemical formulas

Chemical Formulas

  • Chemical formula – tells what elements and how many of each element are in a unit of that compound

  • H2O – water; contains two atoms of hydrogen and one atom of oxygen

  • NH3 – ammonia; contains one atom of nitrogen and 3 atoms of hydrogen








Stability and ionic bonding

  • Mg(OH)2 – milk of magnesia – contains one atom of magnesium, two atoms of oxygen, and two atoms of hydrogen






Atomic stability

Atomic Stability

Why do Elements Form Compounds?

- the noble gases are extremely stable atoms that do not combine with other elements.

- it is the eight valence electrons that make the noble gas atoms stable

Stability and ionic bonding

  • An atom is chemically stable when its outermost energy level is complete

    • 1st level – 2 electrons

    • All other levels – 8 electrons

  • All elements combine with other elements by losing, gaining or sharing electrons so that they will have eight valence electrons!!

Stability and ionic bonding

- When atoms begin to lose, share, or gain electrons they begin to get attracted to other atoms and form chemical bonds - a force that holds atoms together in a substance.


Ionic bonding

Ionic Bonding

  • Atoms that gain or lose electrons become charged forming an ion.

What ion will Sodium form?

Since sodium has 1 valence electron it can lose that electron and then have eight valence elect.

1 e-

8 e-

11 p+


2 e-

Stability and ionic bonding

  • This will give the sodium atom a +1 charge

  • 11p+ + 10e- = +1Na+1

Superscript – written above line; gives the charge of ion

Group 1 → 1 valence e- → +1

Group 2 → 2 valence e- → +2

Group 13 → 3 valence e- → +3

Stability and ionic bonding

What ion will fluorine form?


Fluorine needs to gain 1e- in order to become stable




- This will give fluorine a -1 charge


Group 17 → 7 valence e-→ -1

Group 16 → 6 valence e- → -2

Group 15 → 5 valence e- → -3


Using electron dot structure to show ionic bonds

Using electron dot structure to show ionic bonds

Explain the formation of the ionic bond between sodium and chlorine



Na+[ Cl ]-1


Electron dot struct.

Formula unit

Stability and ionic bonding

Steps to draw electron dot structures for ionic compounds

  • Draw the electron dot structures of the elements

  • transfer electrons from the metal to the nonmetal

  • add elements as needed

  • continue transferring until all atoms are stable

Stability and ionic bonding

5. Write out the chemical formula using subscripts to show how many of each element it took

Stability and ionic bonding

Lets try aluminum and oxygen!!





[ O ]-2






Your turn

Your Turn!!

Use electron dot structures to write chemical formulas for the following combination of elements:

  • potassium and fluorine

  • Magnesium and fluorine

  • Aluminum and nitrogen

  • Magnesium and phosphorous

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