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

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

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

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

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

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

<p>Sigma Bond (A)</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. (A)</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. (C)</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. (C)</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. (A)</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. (A)</p> Signup and view all the answers

Which of the following compounds exhibits an expanded octet?

<p>PF5 (C)</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. (D)</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. (C)</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 (C)</p> Signup and view all the answers

Which of the following correctly defines a covalent compound?

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

Which molecule contains an odd number of valence electrons?

<p>NO (C)</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)) (A)</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 (B)</p> Signup and view all the answers

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

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

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

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

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

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

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

<p>CO2 (C)</p> Signup and view all the answers

Which of the following compounds contains 4 atoms of chlorine?

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

What is the correct naming convention for the compound N2O3?

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

Which of the following correctly represents the compound carbon disulfide?

<p>CS2 (D)</p> Signup and view all the answers

What is the correct application of prefixes when naming CO?

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

What is the name of the compound SF6?

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

What is the correct formula for silicon trioxide?

<p>SiO2 (A)</p> Signup and view all the answers

Which of the following compounds is incorrectly named?

<p>CH4 - methanium (C)</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. (C)</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 (C)</p> Signup and view all the answers

What characterizes a polar molecule?

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

Which of the following examples is a polar covalent molecule?

<p>NH3 (C)</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. (D)</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. (C)</p> Signup and view all the answers

Flashcards

Covalent Bonding

A chemical bond formed when two or more nonmetals share valence electrons.

Molecule

The substance formed by covalent bonding. It only consists of nonmetals.

Single Bond

A covalent bond where 1 pair of valence electrons is shared (2 electrons total).

Double Bond

A covalent bond where 2 pairs of valence electrons are shared (4 electrons total).

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Triple Bond

A covalent bond where 3 pairs of valence electrons are shared (6 electrons total).

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Bond Strength (Covalent)

Bond strength increases from single to double to triple bonds.

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Sigma (σ) Bond

A covalent bond formed by head-to-head overlapping of atomic orbitals along the internuclear axis.

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Pi (π) Bond

A covalent bond formed by lateral (sideways) overlapping of atomic orbitals, above and below the internuclear axis.

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s-s Overlapping

A type of sigma bond formed by the head-on overlap of two 's' orbitals.

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Lewis Structure Steps

A step-by-step guide to drawing the Lewis structures of covalent molecules.

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Valence Electrons

Electrons in the outermost shell of an atom that participate in bonding.

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Central Atom

Atom in the center of a molecule's Lewis structure, usually the least electronegative.

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Octet Rule

Atoms tend to gain, lose, or share electrons to achieve a full outer electron shell (8 electrons).

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Covalent Bond

A bond formed when two non-metal atoms share one or more pairs of electrons.

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Electronegativity

A measure of how strongly an atom attracts bonding electrons.

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Single, Double, Triple Bonds

Different ways atoms share electrons (1, 2, or 3 pairs of electrons), affecting bonding.

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Stability

The tendency of atoms to arrange in ways that minimize energy and maximize electron sharing for full outer shells.

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Naming Covalent Compounds

Covalent compounds are formed by sharing electrons between nonmetal atoms. Naming them involves using prefixes (mono, di, tri, etc.) to indicate the number of each atom in the molecule, followed by an -ide suffix for the second element.

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Prefixes in Naming

Prefixes are used to indicate the number of atoms of each element in a covalent compound. Examples: mono (1), di (2), tri (3), tetra (4), penta (5), hexa (6).

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Naming the Second Element

The second element in a covalent compound is named by changing the ending to -ide.

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Diselenium Dibromide

Example of covalent compound naming convention. Di- means two, and the second element's ending transformed to -ide.

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Special Cases (Naming)

Some covalent compounds have unique names, like water (H2O), ammonia (NH3), methane (CH4), and hydrogen sulfide (H2S).

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Diatomic Molecules

Certain elements (e.g., oxygen, nitrogen, hydrogen) exist naturally as molecules with two atoms bonded together (diatomic).

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Converting word to formula

Given the name of a covalent compound, you write the chemical formula using correct prefixes and subscripts.

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Covalent Bonding (Ordinary)

A chemical bond where atoms share a pair of electrons.

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Lewis Structure

A diagram that shows the arrangement of atoms and electrons in a molecule.

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Valence Electrons

Outermost electrons involved in bonding.

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Dative Covalent Bonding

A type of covalent bonding where one atom provides both electrons in the shared pair.

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Covalent Bond

Bond formed by sharing electrons between nonmetals.

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Polar Molecule

A molecule with uneven distribution of charge, one end slightly positive and the other slightly negative.

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Octet Rule

Atoms tend to gain, lose, or share electrons to achieve a full outer shell (8 electrons).

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Non-Polar Molecule

A molecule with even distribution of charge.

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Expanded Octet

Some elements exceed 8 valence electrons in their structures

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Electronegativity

An atom's ability to attract electrons in a bond.

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Formal Charge

Difference between valence electrons of free atom & electrons assigned to it in a Lewis structure.

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Like Dissolves Like

Polar substances dissolve polar substances, and non-polar substances dissolve non-polar substances.

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IUPAC Nomenclature

Standard systematic method for naming organic compounds.

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Polar Covalent Substance

A covalent substance where electrons are unequally shared, due to differences in electronegativity between the bonded atoms. It exhibits a dipole moment.

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Single Bond

Two atoms share one pair of valence electrons.

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Double Bond

Two atoms share two pairs of valence electrons.

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Coordination Compounds

Compounds with metals bonded to multiple ligands.

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Period 3 Elements

Elements in the third row of the periodic table

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Period 2 Elements

Elements in the second row of the periodic table.

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Binary Molecular Compound

A substance composed of exactly two different elements that cannot be simplified further by chemical means.

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Molecular Formulas

The representation of the exact number of atoms of each element in a molecule of the compound

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Prefixes (Naming Compounds)

Used to indicate the number of atoms of each element in a molecular compound.

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Mono (Prefix)

Indicates 1 atom of a specific element in a molecule

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Di (Prefix)

Indicates 2 atoms of a specific element in a molecule

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Tri (Prefix)

Indicates 3 atoms of a specific element in a molecule.

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Tetra (Prefix)

Indicates 4 atoms of a specific element in a molecule.

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Penta (Prefix)

Indicates 5 atoms of a specific element in a molecule.

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Hexa (Prefix)

Indicates 6 atoms of a specific element in a molecule.

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Hepta (Prefix)

Indicates 7 atoms of a specific element in a molecule.

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Octa (Prefix)

Indicates 8 atoms of a specific type of element in a molecule.

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Nona (Prefix)

Indicates 9 atoms of a specific type of element in a molecule.

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Deca (Prefix)

Indicates 10 atoms of a specific element in a molecule.

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Formula Writing (Covalent Compounds)

Write the central atom symbol first, then the other atom symbol(s),using subscripts to identify element quantity.

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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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