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38 Cards in this Set
- Front
- Back
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Are a group of atoms bond together by covalent bonds |
Molecules |
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It exists between nonmetal atoms, which have small electronic activity difference |
Covalent bonds |
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Compounds that result from covalent bonding are called |
Molecular compounds |
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Sharing of one electron pair forms |
Single covalent bond |
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Sharing two pairs of electrons |
Double covalent bond |
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Two atoms sharing 6 valence electrons form |
Triple covalent bond |
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It forms between a metal and a nonmetal through an exchange of electrons |
Ionic bond |
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CO2, colorless and reactive gas, natural component of the atmosphere, by product of animal and human respiration, needed by plants for photosynthesis |
Carbon dioxide |
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CO, colorless highly toxic gas major air pollutants component of cigarette smoke and automobile exhaust gases |
Carbon monoxide |
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H2O2 Colorless unstable liquid in pure form used as a rocket fuel, beach and antiseptic 3% solution |
Hydrogen peroxide |
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SO2 Product of combustion of petroleum products and coal major air pollutant |
Sulfur dioxide |
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NO2 Dark brown gas major air pollutants product of combustion of fossil fuels |
Nitrogen dioxide |
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N2O colorless colorless sweet-smelling gas used as anesthetic laughing gas |
Nitrous oxide |
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HCl Colorless gas with a pungent odor readily dissolves in water to give hydrochloric acid an ingredient of cleaning products |
Hydrogen chloride |
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An atom that is covalently bonded to more than one |
Central atom |
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An atom that is man that only one other atom |
Terminal atom |
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It compares the number of electrons owned by an atom in a molecule or ion with those possessed by the same atom in a free state |
Formal charge |
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Formula for formal charge |
(no. of valence electrons) - (no. of unpaired electrons) - 1/2 (no. of shared electrons) |
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Describes the three-dimensional arrangement of atoms within a molecule or polyatomic ion |
Molecular geometry |
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VSEPR |
Valence shell electron pair repulsion |
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Suggests that electron pairs around an atom assume an arrangement in that reduces repulsion between them |
Valence shell electron pair repulsion theory |
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For two electron pairs in an atom to be as far apart as possible they should be at 180° angle from each other |
Linear arrangement |
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Three electron pairs in an atom are widely separated at 120 degree angle to one another forming an equilateral triangle |
Trigonal planar |
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Reduces repulsion among four sets of electron pairs. The angle between any two electron pairs is 109.5 degrees |
Tetrahedral arrangement |
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Represents a bond on the plane of the paper |
Single line |
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Suggest a bond protruding out of the paper and towards the reader |
Solid wedge |
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Means the bond protrudes to the back of the paper |
Dashed wedge |
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Considers the effect of the nonbonding domains to the shape of the molecule or ion |
Electron domain geometry |
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The higher electronegativity value of an element means |
That it has greater attraction for shared electrons in a chemical bond |
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With electronegativity value of 4.0 is the most electronegative of all elements |
Fluorine |
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Are the least electronegative elements with 0.7 electronegativity |
Cesium and francium |
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The larger the electronegativity difference between the atoms |
The more polar the bond will be |
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It has the highest electronegativity difference and are therefore the most polar of the chemical bonds |
Ionic bonds |
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Ionic bond electronegativity difference |
△EN ≥ 1.7 |
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Polar covalent bond electronegativity difference |
1.7 > △EN > 0.4 |
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Nonpolar covalent bond electronegativity difference |
△EN ≤ 0.4 |
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Results from the electron distribution (electron density) between atoms and consequence of their electronegativity |
Bond polarity |
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The charge separation resulting from the unequal sharing of the electrons |
Bond dipole |
