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63 Cards in this Set
- Front
- Back
What are the diatomic seven?
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Hydrogen, Nitrogen, Oxygen, Iodine, Bromine, Flourine, Chlorine
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Cation
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positive charge
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anion
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negative charge
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where can you find valence electrons
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top of the periodic table
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ionic bond
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metal + non metal
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characteristics of ionic bonds
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-lost/gained
-transferred -ionizes -conductor |
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covalent bond
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non metal +non metal
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covalent bond characteristics
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-shared
-poor conductor |
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metallic bond
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metal + metal
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metallic bond characteristics
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-delocalized
-shiny/luster -flow -conductor |
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hydrogen bond
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polar covalent molecules
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electronegativity
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a scale which measure the attraction that an element has for valence electrons
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Active metals have _____ electronegativities.
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lower
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The most active non metals have ______ electronegativities.
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higher
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Nonpolar
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covalent bond with equal sharing of electrons
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Polar
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covalent bond with unequal sharing of electrons
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stable element
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full octet of electrons
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alkali metals
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located in the first column of the periodic table
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alkali earth metals
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located in the second column of the periodic table
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transition metals
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located in the 3-12 columns of the periodic table
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halogens
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second to last column
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nobel gasses
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last column
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atomic mass
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a.m.u. smallest unit of mass in chemistry. protons and neutrons weigh one a.m.u.
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molar mass
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the mass of one mole of particles
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Lewis Dot Notation
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A structural formula that shows all of the atoms and valence electrons in a molecule.
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Synthesis
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single product
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decomposition
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single reactant
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single replacement
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element + compound
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double replacement
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compound + compound
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combustion
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hydrocarbon + oxygen
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Atoms combine in order to become more ______.
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stable
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the group of elements that "give up" electrons is?
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metals
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an electronegativity difference of 2.60 indicates a ____ bond.
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ionic
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a _____ molecule is an example of a polar covalent bond.
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H20
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An atom of sodium could reach noble gas configuration by ______ an electron.
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losing
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charged particles are held together by _____ bonds.
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ionic
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many covalent (molecular) compunds are composed of a _____ combined with a _____.
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nonmetal + nonmetal
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bond and lattice energy is measured in ___ per mole
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kilojoules
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the group of elements with lowest electronegativity is ______.
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metals
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when electrons are "lost" and "gained" you will find a _____ bond.
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ionic
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noble gas configuration is an _____ of outer level electrons.
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octet
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molecules are held together by _______ bonds.
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covalent
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outer level electrons are called ______ electrons.
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valence
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when electrons are shared you have ____ bonds.
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covalent
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the group of elements with highest electronegativity is?
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non metals
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the group of elements that "take on" electrons are _______.
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non metals
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a scale of ______ measures an elements attraction for electrons.
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electronegativity
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an example of a non polar covalent bond is _____
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diatomic hydrogen
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most ionic compunds consist of a ____ combined with a _____.
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metal
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bromine would reach noble as configuration by ____ one electron.
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gaining
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electronegattivity difference indictates the ______ of bond character.
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degree
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molecular compounds possess ____ bonds.
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covalent
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an electronegativity difference of 0.95 would indicate that the bond is ____.
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covalent
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ionic bonds generally have (higher/lower) boilinf points than covalent bonds.
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higher
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electrons in metallic bonds are (fluid/not fluid)
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fluid
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covalent bonds generally have (weaker/ stronger) bond strength that ionic bonds
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weaker
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the surface appearance of metallic bonds is (shiny/dull)
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shiny
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ionic bonds generally have (lower, higher) melting points than covalent bonds.
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higher
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metallic bonds (allow/do not allow) for ductility
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allow
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covalent bonds generally have (poorer/ better) electrical conductivity than ionic bonds
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poorer
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ionic bonds generally have a (crystalline/noncrystalline) structure
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crystalline
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transition metals tend to be (soft/hard)
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hard
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the electrons in metallic bonds are described as (localized/delocalized)
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delocalized
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