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63 Cards in this Set

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