Covalent Bonding Overview
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Questions and Answers

What is formed as a result of covalent bonding between non-metals?

  • Ionic Compounds
  • Molecules (correct)
  • Salts
  • Metals

    • Which type of covalent bond involves the sharing of 3 pairs of valence electrons?

  • Single Bond
  • Quadruple Bond
  • Triple Bond (correct)
  • Double Bond

    • Which type of bond is formed by the head-to-head overlapping of atomic orbitals?

  • Pi Bond
  • Delta Bond
  • Variational Bond
  • Sigma Bond (correct)

    • What increases in strength in the order of Single bond, Double bond, Triple bond?

    <p>Bond strength</p> Signup and view all the answers

    Which of the following statements about sigma bonds is correct?

    <p>Sigma bonds involve direct overlapping of orbitals.</p> Signup and view all the answers

    Which type of overlapping occurs in an s-s sigma bond?

    <p>Head-on overlap</p> Signup and view all the answers

    Which parameter does NOT influence the formation of sigma and pi bonds?

    <p>Molecular weight</p> Signup and view all the answers

    What type of bond is typically the strongest among the types of covalent bonds?

    <p>Sigma Bond</p> Signup and view all the answers

    What is the first step in drawing Lewis structures for covalent substances?

    <p>Write the electronic configuration of your atoms.</p> Signup and view all the answers

    During the process of drawing Lewis structures, what determines the central atom?

    <p>The largest atom, which is the least electronegative.</p> Signup and view all the answers

    If both carbon and nitrogen are in a covalent bond, which should be placed as the central atom?

    <p>Carbon, as it takes precedence over nitrogen.</p> Signup and view all the answers

    What should be done if a molecule cannot be stabilized with a single bond?

    <p>Try using a double or triple bond.</p> Signup and view all the answers

    What key information is needed before drawing the Lewis structure?

    <p>The total number of valence electrons for all atoms.</p> Signup and view all the answers

    Which of the following compounds exhibits an expanded octet?

    <p>PF5</p> Signup and view all the answers

    In which scenario should the more electronegative atom be placed at the center of the structure?

    <p>In the case of water molecules.</p> Signup and view all the answers

    What step should be taken after drawing the structure of your atom?

    <p>Write the chemical formula and name of the substance.</p> Signup and view all the answers

    What is the purpose of calculating formal charge in a Lewis structure?

    <p>To assess the stability and resonance structures</p> Signup and view all the answers

    Which of the following correctly defines a covalent compound?

    <p>A molecule with atoms sharing electrons</p> Signup and view all the answers

    What happens if there are multiple carbon atoms in a molecule during the construction of a Lewis structure?

    <p>They should be joined side by side in a chain.</p> Signup and view all the answers

    Which molecule contains an odd number of valence electrons?

    <p>NO</p> Signup and view all the answers

    Which of the following represents the correct calculation of formal charge for an atom?

    <p>Total valence electrons - (non-bonding + 1/2(bonding electrons))</p> Signup and view all the answers

    Which of the following is not a characteristic of a covalent bond?

    <p>High melting and boiling points</p> Signup and view all the answers

    In the compound SF2, how many lone pairs are on the sulfur atom?

    <p>1</p> Signup and view all the answers

    What is the primary reason for the formation of expanded octets in certain molecules?

    <p>Availability of d orbitals</p> Signup and view all the answers

    What does a molecular formula indicate about a covalent compound?

    <p>The exact number of atoms of each element in one molecule of the compound</p> Signup and view all the answers

    Which prefix is used to denote 5 atoms of an element in a molecular compound's name?

    <p>Penta</p> Signup and view all the answers

    What is the correct name for the compound with the formula SO3?

    <p>Sulfur trioxide</p> Signup and view all the answers

    How many atoms of sulfur are present in the compound SO2?

    <p>One</p> Signup and view all the answers

    What is the main purpose of prefixes in naming binary molecular compounds?

    <p>To specify the number of atoms of each element</p> Signup and view all the answers

    What formula represents a compound containing one carbon atom and two oxygen atoms?

    <p>CO2</p> Signup and view all the answers

    Which of the following compounds contains 4 atoms of chlorine?

    <p>Carbon tetrachloride (CCl4)</p> Signup and view all the answers

    In writing the formula for a covalent compound, which atom is typically written first?

    <p>The central atom or atoms</p> Signup and view all the answers

    What is the correct naming convention for the compound N2O3?

    <p>Dinitrogen trioxide</p> Signup and view all the answers

    Which of the following correctly represents the compound carbon disulfide?

    <p>CS2</p> Signup and view all the answers

    What is the correct application of prefixes when naming CO?

    <p>Carbon monoxide</p> Signup and view all the answers

    What is the name of the compound SF6?

    <p>Sulfur hexafluoride</p> Signup and view all the answers

    What is the correct formula for silicon trioxide?

    <p>SiO2</p> Signup and view all the answers

    Which of the following compounds is incorrectly named?

    <p>CH4 - methanium</p> Signup and view all the answers

    What is the primary identifying characteristic of diatomic molecules?

    <p>They contain two atoms of the same type.</p> Signup and view all the answers

    Which of the following is an example of a compound with a special naming exception?

    <p>NH3 - ammonia</p> Signup and view all the answers

    What characterizes a polar molecule?

    <p>One atom attracts electrons more strongly than the other.</p> Signup and view all the answers

    Which statement accurately describes the process of dissolving substances?

    <p>Like dissolves Like applies to polar and non-polar substances.</p> Signup and view all the answers

    Which of the following examples is a polar covalent molecule?

    <p>NH3</p> Signup and view all the answers

    How is a non-polar molecule typically formed?

    <p>By the equal sharing of electrons between atoms with similar electronegativity.</p> Signup and view all the answers

    What defines ionic substances in terms of polarity?

    <p>They consist of cations and anions, giving them a charge difference.</p> Signup and view all the answers

    Study Notes

    Covalent Bonding

    • Covalent bonding is a chemical bond between two or more nonmetals in a fixed ratio.
    • The covalent bond consists of two or more nonmetal atoms sharing their valence electrons with each other.
    • The substance formed after a covalent bond forms is called a molecule.
    • Covalent compounds are also called molecules.

    Types of Covalent Bonds

    • Single bond: Sharing of one pair of valence electrons (2 electrons).
    • Double bond: Sharing of two pairs of valence electrons (4 electrons).
    • Triple bond: Sharing of three pairs of valence electrons (6 electrons).
    • Bond strength increases in the order: single bond < double bond < triple bond.

    Sigma and Pi Bonds

    • Sigma and pi bonds are types of covalent bonds that differ in the overlapping of atomic orbitals.
    • Covalent bonds form by overlapping atomic orbitals.
    • Sigma bonds result from head-to-head overlapping of atomic orbitals.
    • Pi bonds result from lateral overlapping of atomic orbitals.
    • Sigma bonds are stronger than pi bonds due to direct overlapping.

    Types of Sigma Bonds

    • s-s overlap: One 's' orbital from each participating atom undergoes head-on overlapping along the internuclear axis. An s orbital must be half-filled before it overlaps with another. This type of overlapping is observed in H₂ molecules.
    • s-p overlap: One half-filled s orbital overlaps with one half-filled p orbital along the internuclear axis, forming a covalent bond. This type of overlapping is observed in ammonia (NH₃).
    • p-p overlap: One half-filled p orbital from each participating atom undergoes head-on overlapping along the internuclear axis. This type of overlapping is observed in chlorine (Cl₂).
    • P to P overlap: A Cl₂ molecule features a p-p overlap of the 3p orbitals of two chlorine atoms. The head-to-head overlapping of two p orbitals gives a sigma bond, and lateral overlap gives pi bonds.

    Pi (π) Bond

    • Pi bonds form by the lateral (sidewise) overlap of atomic orbitals along a direction perpendicular to the internuclear axis.
    • The axes of atomic orbitals are parallel to each other in pi bonds.
    • Pi bonds are weaker than sigma bonds.

    Amount of Sigma and Pi Bonds

    • A triple bond consists of two pi bonds and one sigma bond.
    • A double bond consists of one pi bond and one sigma bond.
    • A single bond consists of one sigma bond..

    Free Rotation

    • Sigma bonds have electron density along the bond axis, allowing for free rotation.
    • Pi bonds have electron density above and below the bond axis, restricting rotation.

    Rotation, Length, and Strength Differences

    Feature Single Bond Double Bond Triple Bond
    Composition σ σ + π σ + 2π
    Free Rotation Yes No No
    Length Longest Middle Shortest
    Strength Weakest Middle Strongest

    Differences Between Sigma and Pi Bonds

    Feature Sigma Bond Pi Bond
    Overlapping orbitals Can be pure or hybrid Must be unhybridized
    Bond energy High Relatively low
    Existence Can exist independently Must exist along with a sigma bond
    Influence on molecular shape Has an impact Has no role

    Questions

    • Possible combinations of orbitals in covalent sigma bonds
      • s-s overlap
      • s-p overlap
      • p-p overlap
    • Number of sigma and pi bonds in a benzene molecule
      • 12 sigma bonds
      • 3 pi bonds

    Lone Pairs

    • Lone pairs are regions of valence electrons that do not participate in covalent bonds.
    • Lone pairs become essential to participate in chemical reactions if the molecule reacts with another substance.

    Lewis Structures of Atoms

    • Lewis structures represent the valence shell with valence electrons and the element symbol.
    • Understand how to draw Lewis structures.

    Lewis Structures of Molecules

    • A Lewis structure is a representation of simple molecules.
    • 1 line = single bond = 2 electrons
    • 2 lines = double bond = 4 electrons
    • 3 lines = triple bond = 6 electrons -Electron pairs that are not used in bonding are called lone pairs.

    Lewis Structures for molecules

    • Understand conversion of dot-and-cross diagrams to Lewis structures.
    • Understand how to determine the structure of molecules such as SF₆ and CO₂ to draw a Lewis structure.

    Conversion from Word Formulas to Chemical Formulas

    • Understand how to write chemical formulas from covalent substance names(Example: selenium trioxide, carbon disulphide, carbon tetrabromide).

    Special Names and Exceptions

    • Some covalent substances have special names (e.g., water (H₂O), ammonia (NH₃), methane (CH₄)).
    • Many acids have special names (e.g., hydrochloric acid (HCl), sulfuric acid (H₂SO₄)).

    Diatomic Molecules

    • Diatomic molecules consist of two atoms of the same element.
    • Examples include hydrogen (H₂), oxygen (O₂), nitrogen (N₂), fluorine (F₂), chlorine (Cl₂), bromine (Br₂), and iodine (I₂).
    • Memorize names and formulas of common acids.

    Drawing Lewis Structures for Ions

    • Methods for drawing Lewis structures for ions

    Coordinate (Dative) Bond

    • In a coordinate bond, both electrons in the shared pair come from the same atom.
    • The second atom does not contribute electrons.

    The Ammonium Cation

    • Ammonium ion formation from ammonia and hydrogen ion.

    The Hydronium Ion

    • Formation of the hydronium ion (H₃O⁺) from water and a hydrogen ion (H⁺).

    Polarity

    • Polar substances have positive and negative charges.
    • Nonpolar substances do not have significant charge differences.
    • Like dissolves like (polar dissolves polar, nonpolar dissolves nonpolar).

    Electronegativity

    • Electronegativity differences dictate bond types (polar covalent, nonpolar covalent, or ionic).
    • Larger electronegativity differences indicate a more ionic bond.

    Nonpolar Covalent Bonds

    • In nonpolar covalent bonds, electrons are shared equally between atoms.
    • Electronegativity values of atoms are similar.

    Polar Covalent Bonds

    • In polar covalent bonds, electrons are shared unequally between atoms.
    • Atoms have different electronegativities.

    Other examples of Polar Covalent molecules

    • HF (Hydrogen flouride)
    • HCl (Hydrogen chloride)
    • NH3 (Ammonia)

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    Lewis Structures & Covalent Bonding PDF

    Description

    Explore the fundamentals of covalent bonding, including the types of bonds and the concept of molecules formed through electron sharing. Understand the differences between single, double, and triple bonds, as well as sigma and pi bonds. This quiz will enhance your knowledge of chemical bonding.

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