Chemistry Notes Review

Flashcards summarizing key concepts related to chemical bonding, electronegativity, and molecular geometry.

Electronegativity

Ability of an atom in a bond to attract shared electrons to itself.

Bond Formation

Process of atoms becoming bonded together through the sharing or transferring of electrons.

Ionic Bonds

Bonds formed between metal cations and nonmetal anions, stabilized by achieving Noble Gas configuration.

Covalent Bonds

Bonds formed when nonmetals share pairs of electrons.

Lewis Dot Structure

A representation of the arrangement of electrons around atoms in a molecule.

Resonance Structures

Different valid Lewis structures for the same molecule that illustrate delocalization of electrons.

Formal Charge

A theoretical charge assigned to atoms in a molecule that helps identify the most stable structure.

Octet Rule

Atoms tend to form bonds so that each atom has eight electrons in its valence shell.

VSEPR Theory

Valence Shell Electron Pair Repulsion; predicts molecular shapes based on electron pairs repelling each other.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals suitable for pairing of electrons to form chemical bonds.

Electronegativity

Ability of an atom in a bond to attract shared electrons to itself.

Bond Formation

Process of atoms becoming bonded together through the sharing or transferring of electrons.

Ionic Bonds

Bonds formed between metal cations and nonmetal anions, stabilized by achieving Noble Gas configuration.

Covalent Bonds

Bonds formed when nonmetals share pairs of electrons.

Lewis Dot Structure

A representation of the arrangement of electrons around atoms in a molecule.

Resonance Structures

Different valid Lewis structures for the same molecule that illustrate delocalization of electrons.

Formal Charge

A theoretical charge assigned to atoms in a molecule that helps identify the most stable structure.

Octet Rule

Atoms tend to form bonds so that each atom has eight electrons in its valence shell.

VSEPR Theory

Valence Shell Electron Pair Repulsion; predicts molecular shapes based on electron pairs repelling each other.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals suitable for pairing of electrons to form chemical bonds.

Polar Covalent Bond

A covalent bond between two atoms where the electrons are unequally shared due to a difference in electronegativity.

Nonpolar Covalent Bond

A covalent bond between two atoms where the electrons are equally shared due to similar electronegativity.

Molecular Polarity

A property of a molecule determined by the polarity of its bonds and its molecular geometry.

Sigma Bond (\sigma bond)

A type of covalent bond formed by the direct, 'head-on' overlap of atomic orbitals, occurring in single, double, and triple bonds.

Pi Bond (\pi bond)

A type of covalent bond formed by the sideways overlap of p orbitals, occurring in double and triple bonds alongside a sigma bond.

Electronegativity

Ability of an atom in a bond to attract shared electrons to itself.

Bond Formation

Process of atoms becoming bonded together through the sharing or transferring of electrons.

Ionic Bonds

Bonds formed between metal cations and nonmetal anions, stabilized by achieving Noble Gas configuration.

Covalent Bonds

Bonds formed when nonmetals share pairs of electrons.

Lewis Dot Structure

A representation of the arrangement of electrons around atoms in a molecule.

Resonance Structures

Different valid Lewis structures for the same molecule that illustrate delocalization of electrons.

Formal Charge

A theoretical charge assigned to atoms in a molecule that helps identify the most stable structure.

Octet Rule

Atoms tend to form bonds so that each atom has eight electrons in its valence shell.

VSEPR Theory

Valence Shell Electron Pair Repulsion; predicts molecular shapes based on electron pairs repelling each other.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals suitable for pairing of electrons to form chemical bonds.

Polar Covalent Bond

A covalent bond between two atoms where the electrons are unequally shared due to a difference in electronegativity.

Nonpolar Covalent Bond

A covalent bond between two atoms where the electrons are equally shared due to similar electronegativity.

Molecular Polarity

A property of a molecule determined by the polarity of its bonds and its molecular geometry.

Sigma Bond (\sigma bond)

A type of covalent bond formed by the direct, 'head-on' overlap of atomic orbitals, occurring in single, double, and triple bonds.

Pi Bond (\pi bond)

A type of covalent bond formed by the sideways overlap of p orbitals, occurring in double and triple bonds alongside a sigma bond.

Electron Geometry vs. Molecular Geometry

Electron geometry describes the arrangement of electron domains (bonding and non-bonding) around central atom, while molecular geometry describes the arrangement of only the atoms in a molecule.

Linear Geometry

Characterized by two electron domains around the central atom, resulting in a bond angle of 180^ ext{o}. Example: CO_2.

Trigonal Planar Geometry

Characterized by three electron domains around the central atom, resulting in ideal bond angles of 120^ ext{o}. Example: BF_3.

Tetrahedral Geometry

Characterized by four electron domains around the central atom, resulting in ideal bond angles of 109.5^ ext{o}. Example: CH_4.

Trigonal Pyramidal Geometry

A molecular geometry derived from a tetrahedral electron geometry with one lone pair and three bonding pairs, resulting in bond angles less than 109.5^ ext{o} (e.g., NH_3).

Bent Geometry

A molecular geometry that can arise from trigonal planar (one lone pair) or tetrahedral (two lone pairs) electron geometries, characterized by bond angles less than the ideal (e.g., SO2, H2O).

Trigonal Bipyramidal Geometry

Characterized by five electron domains around the central atom, with 90^ ext{o} and 120^ ext{o} bond angles. Example: PCl_5.

Octahedral Geometry

Characterized by six electron domains around the central atom, with all bond angles being 90^ ext{o}. Example: SF_6.