Transcript Naming Chemical Compounds

Naming
Chemical
Compounds
and
Writing
Chemical
Formulas
w/e 1/30
Warm-ups
112
1/26 – 1/29
Fat Man Little Boy – Questions and Notes
113
1/30
Writing Formulas and Naming Compounds
Notes
114
1/30
Compounds Quiz
115
Ionic vs. Covalent Compounds
REVIEW
 Ionic Compounds
– contain a metal and a nonmetal (example: sodium chloride (salt) –
sodium is a metal /chlorine is a nonmetal)
 Covalent
– contains only nonmetals (example:
hydrogen peroxide – hydrogen is a nonmetal /
oxygen is a nonmetal)
More REVIEW
 Electrons
in the same group have similar
chemical properties because they have the
same number of electrons in their valence
shell
 Chemical
bonds form between 2 atoms
when electrons in the outer shell of each
atom form a stable arrangement together
 Any atom or group of
atoms that carry an
electric charge is called an ion
CATIONS – Positively Charged
 When a neutral
atoms gives up an electron, the
positively charged ion is called a CATION
 All
alkali metals (Group 1) form cations very
easily
 They require little energy to remove that valence electron
ANIONS – Negatively Charged
 Non-metals gain electrons to obtain a
noble gas arrangement – ANIONS
 Halogens (group 17)
must gain an electron to do so
 Halogens gain an electron easily and
release a great deal of energy – therefore,
they too are very reactive
 Chemical
reactivity decreases as you
move down the group
 Substances
that are composed of anions and cations
are called IONIC COMPOUNDS
 Ionic Bond
– the attraction between oppositely
charged ions

Bond between a metal and a non-metal
 Covalent Bond – atoms that share a pair of
 Bond between 2 or more non-metals
electrons
Ionic Compound Names
EXAMPLE : Al2O3
1. The subscript for this compound indicates that
there are two atoms of aluminum and three
atoms of oxygen. These numbers do NOT
affect the name.
2. The first part of the name would be aluminum
(the metal).
3. The second part of the name, we drop the
ending on oxygen (non-metal) and add – ide,
thus it becomes oxide
Ionic Compound Name – aluminum oxide
Ionic Compound Names
 The first part of
the name is the name of the
metal element.
 The second
part of the name is the name of the
nonmetal element with the ending changed to
the suffix – ide
Ionic Compound Naming Practice
 NaCl
 KF
 MgF2
 CsCl
 BaCl2
 NaI
 Mg3N
Ionic Compound Naming Practice
NaCl
KF
MgF2
CsCl
BaCl2
NaI
Mg3N
Sodium Chloride
Potassium Fluoride
Magnesium Fluoride
Cesium Chloride
Barium Chloride
Sodium Iodide
Magnesium Nitride
CROSS-OVER RULE
Sodium chloride
Metal
Non-metal
Na
-
Cl
Identify the chemicals as either a metal,
transitional metal or non-metal
Write out the chemical symbols of each
metal
non-metal
sodium chloride
Na
+1
-1
NaCl
Cl
-1
+1
Identify the metal and
non-metal
i.) Write the symbols
ii.) Write the charges
iii.) Cross-over the
charges from top to
bottom
iv.) Remove the charge
v.) Simplify the numbers
and remove the 1’s
Opposites Attract
+1
Na
Cl
-1
*REMEMBER, that metals lose electrons and nonmetals gain electrons
metal
non-metal
Calcium oxide
Ca
+2
-2
CaO
O
-2
+2
Identify the metal and
non-metal
i.) Write the symbols
ii.) Write the charges
iii.) Cross-over the
charges from top to
bottom
iv.) Remove the charge
v.) Simplify the
numbers and remove
the 1’s
Opposites Attract
Ca
+2
O
-2
*REMEMBER, that metals lose electrons and nonmetals gain electrons
metal
non-metal
magnesium chloride
Mg
+2
-1
MgCl2
Cl
-1
+2
Identify the metal and
non-metal
i.) Write the symbols
ii.) Write the charges
iii.) Cross-over the
charges from top to
bottom
iv.) Remove the charge
v.) Simplify the numbers
and remove the 1’s
-1
Cl Mg
+2
MgCl2
Cl
-1
metal
non-metal
calcium phosphide
Ca
+2
-3
Ca3P2
P
-3
+2
Identify the metal and
non-metal
i.) Write the symbols
ii.) Write the charges
iii.) Cross-over the
charges from top to
bottom
iv.) Remove the charge
v.) Simplify the numbers
and remove the 1’s
PRACTICE QUESTIONS
Beryllium fluoride
Sodium nitride
Calcium sulfide
Aluminum chloride
Lithium phosphide
BeF2
Na3N
CaS
AlCl3
Li3P
Barium bromide
Gallium sulfide
Zinc bromide
Cesium phosphide
Germanium oxide
BaBr2
Ga2S3
ZnBr2
Cs3P
GeO2
More Rules
for Ionic Compounds
 If
the compound has more than 2 elements
(polyatomic), the second name is one of the following:
Oxidation #
NO2
NO3
OH
PO4
CO3
SO4
nitrite
nitrate
hydroxide
phosphate
carbonate
sulfate
111322-
Practice!!
 Sodium
Nitrate
 Sodium Hydroxide
 Sodium Phosphate
 Calcium Carbonate
Naming Compounds that use a COVALENT BOND
to join two atoms together (nonmetal and
nonmetal)
 BINARY
Molecular Formulas – Binary molecules will only
have TWO elements in their formula.
 The names of
the compounds will include a prefix to
indicate the number of atoms of each element.
CORRECTION ABOVE! – The number one is MONO!
Have you seen any of these prefixes before? The prefixes are
very similar to the prefixes of geometric shapes. You know
what a triangle is. Right? Well the prefix tri- means three. So
when you have three chlorine (Cl) atoms, you would name it
trichloride.
 Just like when you are
naming an ionic compound the
second elements name is changed to end in -ide.
 EXCEPTION
- An exception to using prefixes is when the
first element has only one atom. The prefix (mono) is not
used in this instance.

Example: CO2 - Carbon Dioxide
Naming Practice – Binary Covalent
Compounds Naming Practice
 CCl4
 S4N2
 CO
 CO3
 OF2
Naming Practice – Binary
Covalent Compounds
 CCl4
Carbon tetrachloride
 S4N2
Tetrasulfur dinitride
 CO
Carbon monoxide
 CO3
Carbon trioxide
 OF2
Oxygen difluoride