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Chemistry Chapter 6
Vocabulary
| Term | Definition |
|---|---|
| chemical bond | the attractive forces that holds atoms or ions together |
| ionic bonding | a force that attracts electrons from one atom to another, which transforms a neutral atom into an ion; metal and nonmetal |
| covalent bonding | a bond formed when atoms share one of more pairs of electrons; metal and metal |
| nonpolar covalent bond | a covalent bond in which the bonding electrons are equally attracted to both bonded atoms |
| polar | describes a molecule in which the positive and negative charges are separated |
| polar covalent bond | a covalent bond in which a pair of electrons shared by two atoms is held more closely by one atom |
| molecule | the smallest particle of a substance that has all of the chemical properties of that substance; is made up of one atom or two or more atoms bonded together |
| molecular comound | a chemical compound whose simplest units are molecules |
| chemical formula | a combination of chemical symbols and numbers to represent a substance. |
| molecular formula | a chemical formula that shows the number and kinds of atoms in molecule, but not the arrangement of atoms |
| bond energy | the energy required to the break the bonds in 1 mol of a chemical comound |
| electron-dot notation | and 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 |
| lewis structure | a structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds |
| structural formula | a formula that indicates the location of the atoms, groups, or ions relative to one another in a molecule and that indicates the number and location of chemical bonds |
| single bond | a covalent bond in which two atoms share one pair of electrons |
| multiple bond | a bond in which the atoms share more than one pair of electrons, such as a double bond or a triple bond |
| resonance | the bonding in molecules or ions that cannot be correctly represented by a single Lewis structure |
| ionic compound | a compound composed of ions bound together by electrostatic attraction |
| formula unit | the collection of atoms corresponding to an ionic compound's formula such that the molar mass of the compound is the same as the mass of 1 mol of the formula units |
| lattice energy | the energy associated with constructing crystal lattice relative to the energy of all constituent atoms separated by infinite distances |
| polyatomic ion | and ion made of two or more atoms |
| metallic bonding | a bond formed by the attraction between positively charged metal ions and the electrons around them |
| malleability | the ability of a substance to be hammered or beaten into a sheet |
| ductility | the ability of a substance to be hammered thin or drawn out into a wire |
| VSEPR theory | predicts some molecular shapes based on the idea that pairs of valence electrons surrounding an atom repel each other |
| hybridization | the mixing of two or more atomic orbitals of the same atom to produce new orbitals; represents the mixing of higher and lower energy orbitals to form orbitals of intermediate energy |
| hybrid orbitals | orbitals that have the properties to explain the geometry of chemical bonds between atoms |
| dipole | a pair of equal and oppositely charged or magnetized poles separated by a distance |
| hydrogen bonding | the intermolecular force occurring when a hydrogen atom that is bonded to a highly electronegative atom of one molecule is attracted to two unshared electrons of another molecule |
| london dispersion forces | in the intermolecular attraction from the uneven distribution of the electrons and the creation of temporary dipoles |
| AB2 | linear |
| AB3 | triangular planar |
| AB4 | tetrahedral |
| AB2E/AB2E2 | bent |
| AB3E | triagonal pyramidal |
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