Section 6.1-6.4
By forming _____ with eachother most atoms______ there potential energy and become more stable This is a ___ change
bonds; reduce; chemical
metal is a
cation (give up electrons)
The fact that metals are malleable and ionic crystals are brittle is best explained in terms of their
chemical bonds
nonmetal& nonmetal
covalent bond either polar or non polar
10
deca
electrons that are free to move in metals
delocalized electrons
How is the strength of metallic bonds measured?
determined by the enthalpy vaporization
2
di
When a metal is drawn into a wire, the metallic bonds
do not break
The property of _____________, which is the measure of the atoms ability to attract electrons, can be used to predict the degree to which the bonding between atoms of two elements is ionic or covalent.
electronegativity
the measure of an atom's ability to attract electrons
electronegativity
All chemical changes involve what?
energy
non polar
even
non-polar
evenly shared bonds between 2 atoms
In metallic bonding valence electrons move ____ in a _____ of metal atoms. The network of metal atoms is called _______.
freely, network, crystal lattice
the greater the electronegativity the ______ the ionic bond
greater
7
hepta
6
hexa
metal&nonmetal
ionic
> 1.7
ionic bond
What happens between bonds as you move left to right?
left to right bonds increase
Mobile electrons in the metallic bond are responsible for
luster, thermal conductivity, electrical conductivity
chemical bonding that results from the attraction between metal atoms and the sea of electrons
metallic bonding
3 types of bonds are
metallic, ionic, and covalent
How does the behavior of electron in metals contribute to metals ability to conduct electricity and heat?
mobile
1
mono
Chemical bond
mutual electrical attraction between the nuclei and valence electrons of different atoms that bind the atoms together
0, .3
non-polar covalent
9
nona
8
octa
In a metal, the vacant orbitals in the atoms' outer energy levels _____, which allows the outer electrons of the atoms to roam ______ throughout the entire metal.
overlap; freely
5
penta
>.3,<1.7
polar covalent bond
First element does not need a ____ while second element always needs it
prefix
Rarely is bonding between atoms_____ ionic or purely covalent.
purely
valence electrons around metal atoms which are packed around of a crystal lattice
sea of electrons
ionic has ______ electron clouds
separate
ionic
separate electron clouds
In valence electrons, the valence electrons are considered to be
shared by all surrounding atoms
Covalent bonding
sharing electrons between 2 or more atoms
Why don't the noble gases form chemical bonds?
stable octet (or 2 if helium)
4
tetra
malleability
the ability of a substance to be hammered or beaten into thin sheets
Relationship between the enthalpy of vaporization of a metal and the strength of the bonds that hold the metal together?
the greater the enthalpy if vaporization the greater the metallic bond direct relationship
conductivity electrical
ability to conduct electricity
conductivity thermal
ability to conduct heat
As light strikes the surface of a metal, the electrons in the electron sea
absorb amd re emit the light
nonmetals
anion (get electrons)
ductility
Ability to be drawn or pulled.
Why are atoms lacking eight electrons in the outermost s and p orbitals said to be more reactive?
Atoms that don't have a stable octet or more reactive
What 2 electrons could have less than 8 electrons to be a stable octet
Be and He
properties of covalent compounds
Covalent compounds generally have much lower melting and boiling points than ionic compounds. soft not usually hard flammable
In general, the strength of the metallic bond ________ moving from left to right on any row of the periodic table
Increases
What 2 electrons could have more than 8 valence electrons
S and P
luster
Shiny appearance; absorbed a wide range of light frequencies many separated by small energy differences
Ionic bonding
bonds that result from electrical attractions between cations and anions; 1 atom losses electrons 1 atom gains electrons
Instead, it usually falls somewhere between the two extremes. Why?
The extent of ionic or covalent bonding between two atoms can be estimated by calculating the difference in each elements' electronegativity.
electrical conductivity thermal conductivity malleability ductility shiny appearance (luster - absorb a wide range of light frequencies )
The unique characteristics of metallic bonding
3
tri
polar
uneven
polar has ____ bonds
uneven
