Chemistry Chapter on Bonding

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Questions and Answers

Which element's octet rule is considered most important when drawing Lewis structures?

  • Chlorine
  • Carbon (correct)
  • Potassium
  • Helium

What is the main consideration when determining the appropriate Lewis structure for molecules with elements outside the first two periods?

  • Minimizing formal charges (correct)
  • Using only single bonds
  • Maximizing the number of lone pairs
  • Satisfying only the octet rule

How does electronegativity influence Lewis structures?

  • It affects the arrangement of electrons but not bond types.
  • It has no impact on Lewis structure representation.
  • It influences which atom will carry a formal charge. (correct)
  • It determines the bond strength in single bonds only.

In Lewis structures, an expanded octet typically involves which of the following elements?

<p>Phosphorus (D)</p> Signup and view all the answers

What type of bonding is primarily represented by Lewis structures?

<p>Covalent bonds only (C)</p> Signup and view all the answers

What is the primary characteristic of ionic bonding?

<p>Transfer of electrons between atoms (B)</p> Signup and view all the answers

Which statement correctly defines a polar covalent bond?

<p>Unequal sharing of electrons resulting in partial charges (B)</p> Signup and view all the answers

What does the concept of electronegativity refer to?

<p>An atom's ability to attract electrons in a bond (B)</p> Signup and view all the answers

Which element has the highest electronegativity according to the Pauling scale?

<p>Fluorine (F) (A)</p> Signup and view all the answers

When drawing a Lewis structure, which conditions must be satisfied for a complete octet?

<p>All main group elements must have 8 electrons around them (D)</p> Signup and view all the answers

Under which condition can elements in periods 3 and beyond have expanded octets?

<p>When they are involved as the central atom (D)</p> Signup and view all the answers

Which of the following statements about formal charges is inaccurate?

<p>Formal charges are the actual charges on atoms (C)</p> Signup and view all the answers

In a Lewis structure for chlorine gas (Cl2), how many total valence electrons are present?

<p>4 (A)</p> Signup and view all the answers

What is the typical difference in electronegativity (ΔEN) for a polar covalent bond?

<p>0.5 ≤ ΔEN &lt; 1.9 (D)</p> Signup and view all the answers

Which type of bonding is exhibited by sodium chloride (NaCl)?

<p>Ionic bonding (A)</p> Signup and view all the answers

What is the average formal charge on an oxygen atom in the PO43- ion?

<p>-1 (B)</p> Signup and view all the answers

What is the average bond order for the P-O bonds in PO43-?

<p>1 (D)</p> Signup and view all the answers

Which molecule has the highest average terminal C-O bond order among HCO3−, CO2, and CO32−?

<p>2 (B)</p> Signup and view all the answers

As bond order increases, what happens to bond length?

<p>It decreases. (B)</p> Signup and view all the answers

What is the relationship between bond length and bond dissociation energy?

<p>As bond length decreases, bond energy increases. (A)</p> Signup and view all the answers

How many equivalent resonance structures exist for the PO43- ion?

<p>4 (A)</p> Signup and view all the answers

In terms of formal charge, rank HCO3−, CO2, and CO32− from the least negative to the most negative average charge on terminal oxygens.

<p>HCO3− &lt; CO32− &lt; CO2 (C)</p> Signup and view all the answers

What do resonance structures allow for in a molecule?

<p>The molecule to be a hybrid of all equivalent structures. (B)</p> Signup and view all the answers

What theory helps predict molecular shape based on electron pair repulsion?

<p>Valence Shell Electrons Pair Repulsion Theory (C)</p> Signup and view all the answers

What happens to the bond energy as the bond order increases?

<p>It increases. (D)</p> Signup and view all the answers

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Study Notes

Bonding

  • Involves either the sharing or transfer of outer electrons
  • Goal is for atoms to achieve a stable configuration
  • Usually accomplished by following the octet rule, which states that atoms strive to have eight valence electrons

Ionic Bonding

  • Involves the transfer of electrons
  • Usually between a metal and a non-metal
  • Example: Sodium Chloride (NaCl)
    • Sodium ([Ne]3s1) becomes Na+ ([Ne]) by losing an electron
    • Chlorine ([Ne]3s23p5) becomes Cl- ([Ar]) by gaining an electron

Covalent Bonding

  • Involves the sharing of electrons
  • Usually between two non-metals
  • Often used to gain an octet of electrons
  • Lewis structures show all electrons as equivalent
  • Bonds are often depicted as lines

Electronegativity (EN)

  • An atom's ability to attract electrons in a bond
  • Trend:EN increases across a period and up a group
  • Pauling scale: Fluorine has the highest electronegativity at 4.0

Bond Polarity

  • Polar covalent bonds are characterized by unequal sharing of electrons
  • Dipole moment: The difference in electronegativity between atoms dictates the polarity of a covalent bond
    • Large difference (>1.9): Ionic bond
    • Intermediate difference (0.5 - 1.9): Polar Covalent Bond
    • Small difference (< 0.5): Nonpolar covalent bond

Electrostatic Potential Maps

  • Visual representations of electron density within a molecule
  • Red regions indicate high electron density (negative)
  • Blue regions indicate low electron density (positive)

Lewis Structures

  • Show all bonding and non-bonding electrons
  • Formal charges are also indicated
  • Complete shells are usually achieved by combining bonding and non-bonding electrons
    • Hydrogen is content with 1 electron pair
    • Beryllium is content with 2 electron pairs
    • Boron and Aluminum are content with 3 electron pairs
    • Elements in periods 3 and beyond can have expanded octets if they are the central atom
  • Bonding electrons can participate in single, double, or triple bonds

Drawing Lewis Structures

  1. Count the total number of valence electrons
  2. Choose the central atom: The least electronegative atom becomes the central atom
  3. Arrange surrounding atoms
  4. Fill in the outer atoms with electrons to achieve octets
  5. Fill in the central atom with electrons to achieve an octet
  6. If you run out of electrons, make double or triple bonds

Resonance Structures

  • Resonance Structures represent alternative Lewis structures for a molecule that share the same connectivity but have different electron distributions.
  • These structures are connected by double headed arrows
  • The resonance hybrid is an average of all possible resonance structures
  • They help explain the delocalization of electrons within a molecule
  • Bond lengths, orders, and charges are averages of all resonance structures
  • Most polyatomic anions have resonance structures

Bond Order, Length & Energy

  • Covalent bond length: The approximate distance between two nuclei involved in a covalent bond
  • Bond dissociation energy (homolysis): The energy required to break 1 mole of bonds in the gas phase
  • Bond order, length, and energy are related:
    • As bond order increases, bond length decreases
    • As bond length decreases, bond energy increases

Molecular Shape

  • VSEPR Theory/Gillespie-Nyholm theory proposes: Electron pairs around a central atom repel each other and try to maximize their separation

Special Cases

  • The octet rule is more important for C, N, O, F
  • Minimizing formal charges is more important for other elements on the periodic table

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