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Chemical Bonds template

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This set includes the following cards:
Chemical Bonda mutual electrical attraction between the nuclei and valence electrons or different atoms that binds the atoms together
Ionic Bondingthe chemical bond resulting from electrical attraction between large numbers of cations and anions
Covalent Bondinga chemical bond resulting from sharing of an electron pair between two atoms
Polarhaving an uneven distribution of charge
Polar-Covalent Bonda covalent bond in which the bonding electrons are shared equally by the bonded atoms resulting in a balanced distribution of electrical charge
Bond Energythe energy required to break a chemical bond and form neutral isolated atoms
Chemical Formulaa formula that indicated the relative numbers of atoms of each kind in a chemical compound by using atoms symbols and numerical subscriptions
Diatomic Moleculea molecule containing only two atoms
Double Bonda covalent bond produced by the sharing of two pairs of electrons between two atoms
Electron-Dot notationan EC notation in which the only valence electrons of an atom of a particular element are shown indicated by dots placed around the elements symbol
Lewis Structuresformula 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 unshaved electrons
Lone Paira pair of electrons that is not involve in bonding and that belong exclusively to one atom
Molecular Compounda chemical compound whose simplest units are molecules
Molecular Formulaa formula showing they types and numbers of atoms combines in a single molecule of a molecular compound
Moleculea neutral group of atoms that are held together by covalent bonds
Multiple Bonda double or triple bond
Octet Rulechemical compunds tend to form so that each atoms by gaining losing or sharing electrons has an octet of electrons in its highest occupied energy level
Resonancethe bonding in molecules orions that cannot be correctly represent by a single lewis structure
Single Bondcovalent bond produced by the sharing of one pair of electrons between two atoms
Structural Formulaa formula that indicates the number and typed of atoms present in a molecule and also shows the bonding arrangement if the atoms
Triple Bonda covalent bond produced by the sharing of three pairs of electrons between two atoms
Unshared Paira pair of electrons that is not involved in bonding and that belongs exclusively to one atom
Formula Unitthe simplest collection of atoms from which an ionic compounds formula can be established
Ionic Compounda compound imposed of positive and negatice ions that are combined so that the numbers of positive and negative charges are equal
Lattice Energythe energy released when one mole of an ionic crystalline compound is formed from gaseous ions
Polytomic Iona charge group of covalently bonded atoms
Ductilitythe ability of a substance to be drawn pulled or extruded through a small opening to produce a wire
Malleabilitythe ability of a substance to be hammered or beaten into thin sheets
Metallic Bondinga chemical bonding that results from the attraction between metal atoms and the surrounding sea of electrons
Dipoleequal but opposite charges that are separated by a short distance
Dipole-Dipole Forcesa force of attraction between polar molecules
Hybrid Orbitalsorbitals of equal energy produced by the combinations of two or more orbitals on the same atom
Hybridizationthe mixing of two or more atomic orbitals of similar energy on the same atoms to produce new orbitals on the same atom
Hydrogen Bondingintermolecular force in which a hydrogen atom that is bonding to a highly EN atom is attracted to an unshared pair of electrons of an EN atom nearby molecule
Intermolecular Forcesthe force of attraction between molecules
London Dispersion Forcedan IM attraction resulting from the constant motion of electrons and the creation of instantaneous dipoles
Molecular Polaritythe uneven distribution of molecular charges
VSEPR Theorythe repulsion between the sets of valence electron surrounding an atom causes these sets to be oriented as far apart as possible

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