Chemistry Chapter 7-9
Terms
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- Ionic bonds properties
-
-High melting point
-conduct electric current when melted or dissolved
-soluble in water
-usually crystallize
-held together by electrostatic force
-compounds are electrically neutral
-crystalline soids at room temperature - Ionic bonds-
- composed of formula, lowest whole number ratio of ions in an ionic compound
- molecule-
- smallest particle of a compound that retains all the properties of the compound (covalently bonded)
- oxidation energy-
- positive or negative number assigned to an atom
- Hydrogens oxidation energy is
- +1 except in hydrides where it is negative one
- Oxygen oxidation number is
- -2 except peroxides where it is -1
- free element=
- 0
- compounds
- oxidation numbers sum to zero
- polyatomic ions sum of oxidation numbers must
- equal ionic charge of the ion
- polyatomic-
- many atoms grouped together (bonds that have a covalent bond and have charge)
- Electronegativity determines
- bond character
- The greater the DiFferEnCE between electronegativity
- the more ionic the bond becomes
- The more electornegativity difference
- the StRonGer the bond strength
- Electronegativity trend
- all bonds have some ions and covelant characteristics execept when diatomic!
- If the change in electronegativity is less than 0.5
- the bond is non polar covelant (covelant bond where the electrons are shared equally)
- If the change in electronegativity is between 0.5 and 1.6
- the bond is considered polar covalent (covelant bond where the electrons arent equally distributed)
- If the change in electronegativity is greater than 1.6
- the bond is usually ionic
- Coordination number
- number of ions of oppostite charge that surrounds an ion in a crystal
- Bonding in Metals
- valence electrons known as a sea of electrons also called the delocalized electrons
- metalic bonds
- delocalized electrons attracted to positivley charged metal ions
- Properties of metalic bonds
- conductors, ductile and malleable (cations slide past one another due to the protection of "sea of electrons" ; reshape themselves
- Ionic compounds
- ions linked together by electrostatic force (opp. charges), dont have properties of ductility and malleablity (shatter on impact)
- the Law of Definite Proportions
- for any given compound, the masses of the element are always in the same proportion
- the Law of multiple proportions
- whenever the same 2 element form more than one compound, the different masses of one element that combine with a fixed mass (constant)of the other element are in the ratio of small to whole numbers
-
1-
2-
3
4
5
6
7
8
9
10 -
mono
di
tri
tetra
penta
hexa
hepta
octa
nona
deca - stannic
- (tin) +4
- stannous
- (tin) +2
- plumbic
- (iron) +4
- plumbous
- (iron) +2
- Mercuric
- Hg +2
- Mercurous
-
Hg +2
2 - Cobaltic
- +3
- Cobaltous
- +2
- Cupric
- +2
- Cuprous
- +1
- Ferric
- +3
- Ferrous
- +2
-
NO -
3 - nitrate
-
NO -
2 - nitrite
-
SO 2-
4 - sulfate
-
SO 2-
3 - sulfite
-
BO -3
3 - Borate
-
BO -3
2 - Borite
-
IO -
3 - Iodate
-
IO -
2 - Iodite
- perchlorate
-
ClO -
4 - chlorate
-
ClO -
3 -
ClO -
2 - chlorite
- ClO
- Hypochlorate
-
Acid:
Anion ends in -ide -
prefix= hydro-
suffix= -ic -
Acid:
Anion ends in -ate -
NO prefix
-ic ending -
Acid:
Anion ends in -ite
(polyatomic ion) -
NO prefix
-ous ending - CuS
- Copper II sulfide
-
Cu S
2 - Copper I oxide
- FeO
- Iron II oxide
-
Fe O
2 3 - Iron III oxide (rust)
- Abnormalities in oxidation
-
Zn +2
Ag +
Sn +2 or +4
Pb +2
Pb +4