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Atomic Bonding

This chapter delves into atomic bonding, explaining how unstable elements combine to achieve stability by forming compounds. Compounds exhibit unique properties distinct from their parent elements. Key examples include sodium’s reaction with water and chlorine’s reactivity. The chapter also introduces chemical formulas that represent the composition of compounds, along with the concepts of covalent and ionic bonds. By examining electronegativity and the electron transfer, learners grasp how atoms form stable structures. Understanding these principles is fundamental to chemistry.

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Atomic Bonding

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  1. Atomic Bonding Ch 19 sects1 & 2

  2. Combining Elements • Elements that are unstable will combine with other elements to become stable • Unstable = Wants to change = ready to react • Stable = wants to stay the same • Elements that have combined to be stable are known as compounds • Compounds take on new properties • Properties-The way it looks and behaves

  3. Examples of Compounds andNew properties • Na in water is highly reactive (Metal) • Sodium and Water • Chlorine is highly reactive (gas) • Sodium and Chlorine are unstable elements that combine to become stable (table salt) • When Na and Cl combine to form NaCl the new chemical properties cause it to become stable and it only dissolves in water

  4. Chemical Formulas • Chemical formulas are used to show which elements are in a compound • Chemical formulas also tell you how much of each element is involved • C12H22O11 = Sucrose (cane sugar) • Which elements are part of sucrose? • How many of each element form sucrose?

  5. Atomic Stability • Atoms want a full outer valence so they can become stable • Atoms will gain, lose, or share electrons to become stable • The elements in column 8 (18) on the periodic table have full outer valences • These elements are known as noble gases • These elements are chemically stable

  6. Factors That Affect Bonding • How many electrons the atom needs • If an element only needs to gain/lose 1 electron it will usually form an ionic bond • The electronegativity of the elements involved • Electronegativity describes how bad an atom wants an electron/How strong is its pull

  7. Using Electronegativity • Find the electronegativity of the elements forming the bond • Larger electronegativity (minus) smaller electronegativity (should always be a positive number) • Find what type of bond it is (Listed above the chart)

  8. Types of Bonds • There are 2 major types of bonds • Covalent bonds-Elements share electrons to have a full outer valence • Covalent bonding will be broken down into two more categories • Ionic bonds-Elements give or take electrons • Remember when an element changes its number of electrons it also changes its overall charge

  9. Covalent Bonding • Covalent bonding is the sharing of electrons and it is broken into two different types • Non-polar Covalent Bonding-Equal sharing of electrons • Elements have a similar electronegativity • Because the electrons are shared evenly there is no change in the charges of the atoms

  10. Covalent Bonding • Polar Covalent Bonding-Atoms are shared unequally between atoms • One atom will have a greater electronegativity • The atom with the greater electronegativity will have a stronger pull on the electron • Since the electron spends more time around one of the elements that element will have a slight (-) charge

  11. Ionic Bonding • Ionic bonding forms when one atom gives up an electron and another atom takes that electron • Forms between an atom with a weak electronegativity and an atom with a strong electronegativity • Usually between a metal and non-metal • Usually between atoms from the right side of the periodic table and the left side of the periodic table

  12. Ionic Bond • forming an ionic bond

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