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46 Cards in this Set
- Front
- Back
a mutual electrical attraction between the nuclei and valence electrons of different atoms that bind the atoms together
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Chemical Bond
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chemical bonding that results from the electrical attraction between large numbers of cations (main group metals) and anions (nonmetals)
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Ionic Bond
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results from the sharing of electron pairs between two atoms
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Covalent Bond
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The degree to which bonding between atoms of two elements is ionic or covalent can be estimated by
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calculating the difference in electronegativity
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0-0.3
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NON-POLAR
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0.3-1.7
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POLAR
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1.7<
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IONIC
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- covalent bond in which the bonded electrons are shared equally by the bonded atoms, resulting in a balanced distribution of electrical charge
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Non-polar covalent Bond
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uneven distribution of charge
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Polar
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covalent bond in which the bonded atoms have an unequal attraction for the shared electrons (0.3-1.7)
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Polar covalent bond
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a neutral group of atoms hat are held together by covalent bonds
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Molecule
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a chemical compound whose simplest units are molecules
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molecular compound
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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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Chemical Formula
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shows the types and numbers of atoms combined in a single molecule of a molecular bond
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molecular formula
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a molecule containing only two atoms
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diatomic molecule
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- the distance between two bonded atoms at their minimum potential energy (average distance between two bonded atoms)
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bond length
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the energy required to break a chemical bond and form neutral isolated atoms
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bond energy
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Octet Rule
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chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level
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an electron configuration notation in which only the valence electrons of an atom of a particular element are shown, indicated by dots placed around the element’s symbol
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Electron Dot Notation
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pair of electrons that is not involved in bonding and that belongs exclusively to one atom
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lone pair (unshared pair)
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formulas in which atomic symbols represent nuclei and inner-shell electrons, dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds, and dots adjacent to only one atomic symbol represent unshared electrons
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Lewis structures
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indicates the kind, number, arrangement and bonds but not the unshared pairs of the atoms in a molecule
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Strucural Formula
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covalent bond produced by the sharing of one pair of electrons between two atoms
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single bond
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a covalent bond produced by the sharing of two pairs of electrons between two atoms
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double bond
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covalent bond produced by the sharing of three pairs of electrons between two atoms
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triple bond
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double and triple bonds
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multiple bonds
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Double bonds are shorter and have _ bond energy
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higher
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triple bonds are stronger and higher than ___
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double bonds
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bonding in molecules or ions that cannot be correctly represented by a single Lewis structure
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Resonance
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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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ionic compound
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the simplest collection of atoms from which an ionic compound’s formula can be established
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formula unit
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NATURE FAVORS ARRANGEMENTS IN WHICH POTENTIAL ENERGY IS
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minimized
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the energy released when one mole of an ionic crystalline compound is formed from gaseous ions
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lattice energy
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Molecular compounds melt at low temperature because
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the forces of attraction between molecules is weak
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Ionic are higher __ and __ Ionic compounds are hard but brittle
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melting and boiling points
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charged group of covalently bonded atoms
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polyatomic ion
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the chemical bonding that result form the attraction between metal atoms and the surrounding sea of electrons
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metallic bonding
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the ability of a substance to be pounded into thin sheets
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malleability
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ability of a substance to be drawn into wire
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ductility
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uneven distribution of molecular charge
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molecular polarty
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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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VSEPR theory
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VESPR
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Valence-Shell Electron-Pair Repulsion
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the forces of attraction between molecules
The higher boiling point, the stronger forces between particles |
intermolecular forces
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created by equal but opposite charges that are separated by a short distance
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dipole
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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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hydrogen bonding
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the intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
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London dispersion forces
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