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Questions and Answers
What type of bond is formed between sodium (Na) and chlorine (Cl) in sodium chloride (NaCl)?
What type of bond is formed between sodium (Na) and chlorine (Cl) in sodium chloride (NaCl)?
- Covalent bond
- Metallic bond
- Ionic bond (correct)
- Hydrogen bond
Covalent bonds are typically formed between metals.
Covalent bonds are typically formed between metals.
False (B)
What allows nonmetals to become more stable when forming covalent bonds?
What allows nonmetals to become more stable when forming covalent bonds?
Obeying the octet rule
In a polar covalent bond, the electrons are ________ attracted to the two atoms.
In a polar covalent bond, the electrons are ________ attracted to the two atoms.
Match the following types of bonds with their descriptions:
Match the following types of bonds with their descriptions:
Which of the following correctly describes covalent bonds?
Which of the following correctly describes covalent bonds?
A fluorine atom can form a covalent bond by sharing one electron with a carbon atom.
A fluorine atom can form a covalent bond by sharing one electron with a carbon atom.
What happens to electron density in a polar covalent bond?
What happens to electron density in a polar covalent bond?
What type of bond is formed when two electrons are shared between two atoms?
What type of bond is formed when two electrons are shared between two atoms?
A pi bond can exist without a sigma bond being present.
A pi bond can exist without a sigma bond being present.
How many single bonds does carbon need to form with fluorine to fill its octet?
How many single bonds does carbon need to form with fluorine to fill its octet?
A covalent bond formed between two atoms that share four electrons is called a ______ bond.
A covalent bond formed between two atoms that share four electrons is called a ______ bond.
Which of the following overlap types results in a sigma bond?
Which of the following overlap types results in a sigma bond?
Covalent bonds can only be single or double bonds, but not triple bonds.
Covalent bonds can only be single or double bonds, but not triple bonds.
What is the primary characteristic of a coordinate bond?
What is the primary characteristic of a coordinate bond?
Match the type of bond with its characteristics:
Match the type of bond with its characteristics:
Which type of bond involves the sharing of electrons between two non-metals?
Which type of bond involves the sharing of electrons between two non-metals?
Ionic bonds typically form between two non-metals.
Ionic bonds typically form between two non-metals.
What is the main difference between intramolecular and intermolecular forces?
What is the main difference between intramolecular and intermolecular forces?
In a __________ bond, electrons are transferred from one atom to another, resulting in the formation of ions.
In a __________ bond, electrons are transferred from one atom to another, resulting in the formation of ions.
Which of the following is NOT a type of chemical bond?
Which of the following is NOT a type of chemical bond?
Match the type of chemical bond with its description:
Match the type of chemical bond with its description:
What effect does hybridization have on bond length?
What effect does hybridization have on bond length?
Strong intramolecular forces are related to weaker intermolecular forces.
Strong intramolecular forces are related to weaker intermolecular forces.
What type of bond is formed due to electrostatic attraction between δ+ and δ-?
What type of bond is formed due to electrostatic attraction between δ+ and δ-?
Intramolecular hydrogen bonds do not influence boiling points.
Intramolecular hydrogen bonds do not influence boiling points.
What is the hybridization state of carbon in methane (CH4)?
What is the hybridization state of carbon in methane (CH4)?
In methane (CH4), the bond angles are approximately _____ degrees.
In methane (CH4), the bond angles are approximately _____ degrees.
Which hybridization involves mixing one s orbital and two p orbitals?
Which hybridization involves mixing one s orbital and two p orbitals?
Valency refers to the total number of electrons present in the outermost shell of an atom.
Valency refers to the total number of electrons present in the outermost shell of an atom.
Match the following chemical compounds with their hybridization types:
Match the following chemical compounds with their hybridization types:
What is the combined percentage of s character in sp3 hybridized molecules?
What is the combined percentage of s character in sp3 hybridized molecules?
What type of effect describes the tendency of an atom or group to attract or release electrons?
What type of effect describes the tendency of an atom or group to attract or release electrons?
Heterolytic fission results in the formation of free radicals.
Heterolytic fission results in the formation of free radicals.
Name one example of an electron withdrawing group.
Name one example of an electron withdrawing group.
The _______ effect involves the delocalization of π electrons in a planar system.
The _______ effect involves the delocalization of π electrons in a planar system.
Which of the following properties is NOT associated with homolytic fission?
Which of the following properties is NOT associated with homolytic fission?
Match the types of bond fission to their descriptions:
Match the types of bond fission to their descriptions:
What kind of systems do resonance effects occur in?
What kind of systems do resonance effects occur in?
Electron donating groups are typically ______ groups.
Electron donating groups are typically ______ groups.
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Study Notes
Chemical Bonds
- Chemical bonds hold atoms together in chemical compounds
- Covalent bonds are formed when atoms share electrons
- Ionic bonds are formed when atoms transfer electrons to form ions
- The attraction between ions is called an ionic bond
Types of Chemical Bonds
- Ionic bond: Formed between a metal and a nonmetal.
- Covalent bond: Formed between two nonmetals, where electrons are shared to achieve a stable octet.
- Coordinate bond (dative covalent bond): A covalent bond where both electrons come from the same atom.
- Hydrogen bond: An electrostatic attraction between a hydrogen atom covalently linked to a highly electronegative atom (like oxygen or nitrogen) and an electron pair in the adjacent molecule.
Covalent Bonds
- Sigma bonds (σ): Formed by the overlap of atomic orbitals along the orbital axis.
- Pi bonds (Ï€): Formed by the overlap of two lobes of the interacting atomic orbitals above and below the orbital axis.
Hybridization
- The concept of atomic orbitals fusing to form hybridized orbitals influences molecular geometry and bonding properties.
- sp3 Hybridization: In methane (CH4), one s and three p orbitals combine creating 4 sp3 hybridized orbitals that are tetrahedral, resulting in bond angles of 109.5°.
- sp2 Hybridization: In ethylene, one s and two p orbitals combine forming three sp3 orbitals and leaves one p orbital. The sp2 orbitals are trigonal planar, with bond angles around 120°.
Factors Affecting Electron Availability at an Atom
- Inductive Effect: Electron-withdrawing groups (I-) pull electron density away from a carbon atom while electron-donating groups (+I) push electron density towards a carbon atom.
- Resonance: The delocalization of pi electrons or lone pairs in a planar system with parallel p orbitals.
- Hyperconjugation: The interaction of electrons in a σ bond with an adjacent empty p orbital.
Breaking of Covalent Bonds
- Homolytic fission: A bond breaks, and one electron goes to each atom, resulting in radicals.
- Heterolytic fission: A bond breaks, and one atom gets both electrons, resulting in ions.
Valence
- The number of unpaired electrons present in the outermost shell of an atom, determining its bonding capacity.
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