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67 Cards in this Set
- Front
- Back
a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together
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Chemical Bond
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different _____ may be of the same element or different elements
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atoms
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Atoms bond to be in a more ______ _____. They are less stable when they are __ __________. The potential energy _________ when the atoms bond.
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stable state; by themselves; decreases
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When atoms bond their _______ _________ are redistributed in ways that make the atoms more stable
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valence electrons
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The way in which the electrons are _____________ determines the type of bond
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redistributed
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chemical bonding that results from the electrical attraction between large numbers of anions and cations
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Ionic bonding
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results from the sharing of valence electron pairs between 2 atoms
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Covalent bonding
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In purely covalent bonds, the electrons are ______ _______ between the atoms
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shared equally
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Bonding between atoms of different elements is rarely ______ _____ or ______ ________
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purely ionic or purely covalent
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The bonding falls between the 2 extremes depending upon how strongly the _____ of each element attract electrons
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atoms
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(high electronegativity - low electronegativity) / * 100
high electronegativity |
% ionic character
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if % ionic character is > 50%, then an _____ bond exists
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ionic
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--if % ionic character is < 50%, then a _______ bond exists
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covalent
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a _____ ________ bond falls between 5% and 50% including 50%
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polar covalent
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a ________ ________ bond falls between 0%-5% including 5%
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nonpolar covalent
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Use the electronegativity for ___ ____ of each element to determine the % ionic character even if the compound contains more than 1 atom of an element.
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one atom
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electron configuration in which only the valence electrons are shown as dots around the element's symbol
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Electron dot Notation
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the _____ _____ _________ are not shown
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inner shell electrons
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to write electron dot notation for _______, draw the symbol with the charge on the cation
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cations
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To write the electron dot for ______, draw the symbol surrounded by 8 dots with the charge on the anion
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anions
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Chemical compounds tend to form so that each atom, by gaining, losing or sharing electrons, has an octet or 8 electrons in its highest energy level
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Octet Rule
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________ ________ _____ are covalent bonds where the electrons are shared equally by the bonded atoms resulting in a balanced distribution of electrical charge
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Nonpolar covalent bonds
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there is a ____ _____ __________ in electronegativities between the atoms
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very small difference
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_____ ________ _____ are covalent bonds with an uneven distribution of electrical charges because the bonded atoms have an unequal attraction for the shared electrons
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Polar covalent bonds
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the difference between the electronegativities is ___________
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significant
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the electrons are attracted to the more _______________ ____
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electronegative atom
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a neutral group of atoms that are held together by covalent bonds
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molecule
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molecules containing 2 atoms
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Diatomic molecules
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_ elements occur in nature as diatomic molecules
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7
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formulas for the 7 diatomic molecules are:
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H2, N2, O2, F2, Cl2, Br2, I2
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A ________ _______ indicates the relative numbers of atoms of each kind of element in a chemical compound by using atomic symbols and numerical subscripts
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chemical formula
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_________ ________ show the types and numbers of atoms combined in a single molecule of a molecular compound
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Molecular formulas
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Lewis structures are formulas in which:
- ______ _______ represent the nuclei and inner shell electrons - dot pairs between 2 atomic symbols represent ________ ____ in covalent bonds, dots adjacent to only one atomic symbol represent unshared electrons |
atomic symbols
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__________ _______ indicates the kind, number, arrangement and bonds but not the unshared pairs of electrons in the atoms in a molecule
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structural formula
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covalent bonds produced by the sharing of one pair of electrons between 2 atoms
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single bonds
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covalent bonds produced by the sharing of 2 pairs of electrons between 2 atoms.
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double bonds
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covalent bonds produced by the sharing of 3 pairs of electrons between 2 atoms
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triple bonds
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Compounds made of positive and negative ions combined so that the numbers of positive and negative charges are equal
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Ionic compounds
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The simplest collection of atoms from which an ionic compound's formula can be established
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Formula units
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_______ _____ are not independent neutral units that can be separated and examined like a molecule can be
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formula units
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_____ _________ are networks of positive and negative ions mutually attracted to each other
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ionic compounds
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_______ ____ represents the lowest ratio of the compound's combined ions that give electrical neutrality
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formula unit
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ionic compounds usually exist as ___________ _____
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crystalline solid
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_______ _______ is the orderly arrangement of ions in an ionic compound
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crystal lattice
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In naming ______, the ending of the element's name is replaced with "ide"
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anions
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It creates the ability for metals to be ____ __________ __ ___________ in the solid state
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good conductors of electricity
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within a metal, there are usually 1 or 2 electrons in the outer s-sublevel with no electrons in the _____ _-________
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outer p-sublevel
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the vacant sublevels overlap providing a path for the _______ _________ to move throughout the metal
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valence electrons
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the attraction between the metal's atoms and the surrounding sea of electrons
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metallic bonding
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good conductors of heat and electricity because the sea of electrons carries the ____ or ___________ throughout the atoms
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heat or electricity
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_____ because metals absorb light at different frequencies resulting in electron transition
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Shiny
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The shine is the light given off as the electrons return to the ______ _____
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ground state
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_________ and _______ because metallic bonding is the same in all directions
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Malleable and ductile
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forces that hold the different molecules in a substance together
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Intermolecular forces
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Three types of intermolecular forces:
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- dipole-dipole
- hydrogen bonding - London dipersion forces |
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forces of attraction between polar molecules
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Dipole-dipole
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negative region in one polar molecule attracts the ________ ______ in an adjacent molecule throughout the substance
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positive region
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short range forces acting on nearby _________
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molecules
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important in determining ________ __________ such as the boiling point of a substance or its solubility
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physical properties
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special type of dipole-dipole force that is very strong
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Hydrogen bonding
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occurs in compounds containing _-_ bonds, _-_ bonds and _-_ bonds
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H-F; H-O; H-N
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hydrogen atoms that are bonded to a highly electronegative atom are attracted to an ________ ____ __ _________ of a highly electronegative atom in a nearby molecule
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unshared pair of electrons
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temporary dipoles that occur in any polar or nonpolar molecule
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London dispersion forces
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occur because the electrons are __________ ______
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constantly moving
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at any moment the electron distribution in the electron cloud becomes ______, thus creating a dipole
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uneven
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these temporary _______ induce dipoles in adjacent molecules and cause a weak attraction that holds the molecules together
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dipoles
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these are the only intermolecular forces acting between _____ _____ and _____ ________ _________
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noble gases and other nonpolar molecules
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