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26 Cards in this Set
- Front
- Back
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Bond Energy
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the energy required to break a chemical bond and form neutral isolated atoms
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Chemical Bond
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the mutual attraction between the nuclei and valance electrons of different atoms that bond the atoms together
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Chemical Formula
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tells the kinds of atoms and the number of each kinda in a chemical compound
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Covalent Bonding
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results from the sharing of electron pairs between two atoms
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Double Bond
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a bond in which 2 pairs of electrons is shared between two atoms
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Ductility
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the ability of a substance to be pulled into thin wire
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Electron-Dot Notation
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an electron configuration notation in which only valance electrons of an atom of a particular element are shown
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Electronegativity
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shows how strongly atoms of each element attract electrons
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Forming Unit
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the simplest collection of atoms from which an ionic compound's formula can be established
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Hydrogen Bond
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an intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of electronegative atom in a nearby atom
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Ionic Compound
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composed of positive and negative ions that are combined so that the positive and negative numbers of ions are equal
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Lattice Energy
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the energy released when 1 mole of an ionic crystalline compound is formed from gaseous ions
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Lewis Structures
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formulas in which atomic symbols represent nuclei and inner shell electrons, dot-pairs or dashes between atomic symbols represent electron represent electron pairs in covalent bonds, and dots adjacent to only 1 atomic symbol represent unshared electrons
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Malleability
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the ability of a substance to be hammered into thin sheets
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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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Molecular Compound
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a chemical compound whose simplest units are molecules
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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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Nonpolar-Covalent Bond
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a covalent bond in which electrons are shared equally and results in a balanced electrical distribution
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Octet Rule
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states that a chemical compound tends to form so that each atom by gaining, losing, or sharing has 8 electrons in its highest energy level
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Polar
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means that atoms in a compound have an uneven distribution of charge
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Polar-Covalent Bond
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a covalent bond in which the bonded atoms have an unequal attraction for the shared electrons
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Polyatomic Ion
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a charged group of covalently bonded atoms
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Resonance
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refers to bonding in molecules or ions that cannot be correctly represented by only 1 lewis structure
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Single bond
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bond in which 1 pair of electrons is shared between 2 atoms
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Structural Formula
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indicates the kind, number, arrangement, and bonds but not the unshared pairs, of atoms in a molecule
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Triple Bond
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a bond in which 3 pairs of electrons are shared between 2 atoms
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