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57 Cards in this Set
- Front
- Back
chemical bond
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a link between atoms that results from the mutual electrical attractions between the nuclei and valence electrons of both atoms
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ionic bond
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*a chemical bond resulting from the electrical attraction btwn. large numbers of + and - ions.
The TRANSFER of electrons *becomes larger when combined |
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covalent bond
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*a chemical bond resulting from the SHARING of electron pairs btwn two atoms
*remains the same size when share |
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impure bonds
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bonds that range in btwn ionic and covalent
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ionic bonds electronegativity
range |
1.7-4.0
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polar covalent electronegativity range
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1.7-0.3
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nonpolar covalent electronegativity range
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0.0-0.3
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polar covalent bond
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a covalent bond where the united atoms have an UNEQUAL attraction for the shared electrons
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nonpolar covalent bond
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a covalent bond in which the bonding electrons are shared EQUALLY by bonded atoms with a resulting balanced distribution of charge.
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metallic bonds
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metals give up electrons but unlike ionic bonds give up an e- and then share them equally
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ionic compound
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composed of positive and negative ions combined so that the positive and negative charges are equal
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formula unit
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simplest collection of atoms from which a compound's formula can be established
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lattice energy
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the energy released when one mole of of an ionic crystalline compound is formed from gaseous ions
*larger the energy released the STRONGER THE BOND |
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molecule
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the smallest unit quantity of matter which can exist by itself and retain all the properties of the original substance
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diatomic molecules
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a molecule made up of two atoms
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molecular compound
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a chemical compound whose simplest units are molecules
*made up of COVALENT bonds |
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chemical formula
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indicates the relative number of each kind of atom in a compound using symbols and subscripts
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molecular formula
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indicates the relative number of each kind of atom in a MOLECULAR COMPOUND using symbols and subscripts
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bond energy
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the energy required to break a chemical bond and form neutral atoms
*units are kj/mol |
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bond length
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the average distance btwn. two bonded atoms
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octet rule
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chemical compounds will form so that each atom by gaining, losing or sharing electrons, has an octet of electrons in its highest occupied level.
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expanded valence
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when elements have more than 8 in their outer shell
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unshared pair
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*also called lone pairs
*a pair of electrons that is not involved in bonding but instead belongs exclusively to one atom |
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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.
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isomers
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compounds that have the smae formula but a different structure
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single bond
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sharing a single pair of electrons
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double bond
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sharing two pairs of electrons
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triple bond
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sharing three pairs of electrons
*the strongest and hardest bond to break(as compared to single and double) |
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covalent networking bonds
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a continous 3-D network of several different atoms
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polyatomic ions
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a charged group of covalently bonded atoms
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resonance
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refers to the bonding in molecules that cannot be correctly represented by a single lewis structure
*occurs with double and triple bonds |
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central atom
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written first in the formulas
Ex. S=C=S Carbon is central atom Formula--CS2 |
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NM+NM=
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covalent bond
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M+M=
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metallic bond
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M+NM=
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ionic bond
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Electrons are delocalized?
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*electrons are free to move
*highly mobile |
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Metallic bond def.
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a chemical bond resulting from the attraction between metal atoms and surrounding mobile electrons
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heat of vaporization
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amount of heat needed to change a metal from a solid to a gas
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VSEPR theory
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describes where the bonded atoms are in realation to one another. used for predicting molecular geometry
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VSEPR stands for...
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Valence Shell Electron Pair Repulsion
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VSEPR theory states...
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repusion btwn the set of valence level electron pairs surrounding an atom causes these sets to be oriented as far apart as possible.
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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 orbitals of equal energy.
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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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AB2
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linear
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AB2E
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bent
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AB3
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trigonal planar
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AB4
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tetrahedral
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AB3E
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trigonal pyramidal
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AB2E2
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bent
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AB5
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trigonal bipyramidal
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AB6
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octahedral
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intermolecular forces
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the forces of attraction between molecules
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dipole
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equal but opposite charges separated by a short distance. always points toward the more electronegative
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dipole-dipole forces
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forces of attraction between polar molecules
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induction
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a polar molecule can induce a dipole in a non-polar molecule.
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hydrogen bonding
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an intermolecular attraction btwn a hydrogen atom and an unshared pair of electrons on a strongly electronegative atom in another molecule
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London Dispersion Forces
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intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles and induced dipoles
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