Chapter 6 Chemical Bonding – Inorganic Chemistry – Flashcards
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chemical bond
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a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
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ionic bonding
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the chemical bonding that results from the electrical attraction between cations and anions
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covalent bonding
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results from the sharing of electron pairs between two atoms
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molecule
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a neutral group of atoms that are held together by covalent bonds
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chemical formula
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indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts
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molecular formula
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shows the types and numbers of atoms combined in a single molecule of a molecular compound Ex. H20 for water
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diatomic molecule
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a molecule containing only two atoms
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bond energy
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the amount of energy required to break a chemical bond and form neutral isolated atoms
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structural formula
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indicates the kind, number, arrangement, and bonds but not the unshared pairs of the atoms in a molecule Ex. F--F
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resonance
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refers to bonding in molecules or ions that cannot be correctly represented by a single Lewis structure (doubled headed arrows can be placed)
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ionic compound
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composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal
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most ionic compounds exist as...
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crystalline solids
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formula unit
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the simplest collection of atoms from which an ionic compound's formula can be established Ex. NaCl is one sodium cation plus one chloride anion
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ions minimize their potential energy by combining in an orderly arrangement known as...
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crystal lattice
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lattice energy
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the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
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the force that holds ions in ionic compounds together is...
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a very strong overall attraction between positive and negative charges
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many molecular compounds...
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melt/boil at lower temperatures; are completely gaseous at room temperature
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ionic compounds are hard but brittle...
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because of the ionic crystal structure
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in the solid state...
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ionic compounds are not electrical conductors, but they are in the molten state
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many ionic compounds can dissolve in...
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water
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polyatomic ions
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charged groups of covalently bonded atoms; combine w/ ions of opposite charged to form ionic compounds; their charges come from shortages (pos) / excesses (neg) of electrons
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metallic bonding
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results from the attraction between metal atoms and the surrounding sea of electrons
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metallic properties include...
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high electrical and thermal conductivity, strong absorbtion/ reflection of light, malleability, ductility
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enthalpy of vaporization
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the amount of energy absorbed as heat when a specified amount of a substance vaporizes at a constant pressure
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VSEPR theory
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states that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible
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linear
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2
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trigonal-planar
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3
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bent/angular
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2
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tetrahedral
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4
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trigonal-pyramidal
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3
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trigonal-bipyramidal
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5
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octahedral
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6
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hybridization
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the mixing of two or more atomic orbitals of similar energies on the same atom to produce new hybrid atomic orbitals of equal energies
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hybrid orbitals
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orbitals of equal energy produced by the combination of two or more orbitals on the same atom
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dipole
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created by equal but opposite charges that are seperated by a short distance
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dipole-dipole forces
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short-range forces, acting only between nearby molecules
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hydrogen bonding
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the intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
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London dispersion forces
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the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
