Finishing
Ionic Naming,
Starting
Covalent
Properties
GT Chemistry
12/3/14
Drill
Write the formula:
1. Copper (II) chlorate
2. Calcium nitride
3. Aluminum carbonate
4. Potassium bromide
5. Barium fluoride
6. Cesium hydroxide
HW: pg. 7 – Naming compounds
Objectives
• IWBAT
–
–
–
–
–
Identify the “conservative” and “liberal” metal ions
Identify polyatomic ions
Name and write a formula for any ionic compound
Describe the properties of covalent compounds.
Write the abstract for my STEM fair project.
• NOTE:
– Tomorrow—Ionic and Covalent Compounds Lab –
closed toe shoes!!
– Polyatomic Ion Quiz—Thurs, Fri, or Mon! Spelling
counts
– December 12 – Due date for abstract
Agenda
•
•
•
•
Drill
Discuss Abstract
Covalent Properties & Naming
Lewis Structures with Covalent
compounds
• Closure
What is an abstract?
• A VERY brief summary of your research
• No more than 250 words!
• In 250 words (or less) you need to:
– Identify the problem and hypothesis
– Summarize the experiment, with a brief
overview of the results (yes, SOME data!)
– Identify the application and relevance of the
results
More on the abstract
• Write it and then edit it! Edit it! Edit it!
• Cut out all the “fluff” and excess words
• Make sure it’s in
– Past tense
– Passive voice (no “I” “me” “you” “we”)
• Remember that this is probably ALL of
the project that your judge will read, so
make it GOOD and SHORT
Not this. 
Covalent Bonding
• Sharing of valence
electrons
• Formed by two (or more)
non-metals
– ex. CO2, sugar (C12H22O11)
• The smallest unit of the
compound is a molecule.
More about Covalent
Compounds
• May or may not be water-soluble.
• Covalent compounds do not
conduct electricity, as solids,
liquids, or in solution.
– One exception – Graphite (pure C)
conducts electricity and is a solid
• Low melting point
Naming Covalent
Compounds
CO2 Carbon dioxide
CH4 methane
BCl3
boron trichloride
All are
formed from
two or more
nonmetals.
Ionic
compounds
generally
involve a metal
and nonmetal
(NaCl)
Common Names
• A lot of chemicals have common
names as well as the proper
IUPAC name.
• Chemicals that should always be
named by common name and
never named by the IUPAC
method are:
– H2O water, not dihydrogen
monoxide
– NH3 ammonia, not nitrogen
trihydride
Covalent (Molecular) Nomenclature
for two nonmetals
• Prefix System (binary compounds)
1. Less electronegative atom
comes first.
2. Add prefixes to indicate # of atoms.
Omit mono- prefix on the FIRST
element.
3. Change the ending of the
second element to -ide.
Molecular Nomenclature Prefixes
PREFIX
monoditritetrapentahexaheptaoctanonadeca-
NUMBER
1
2
3
4
5
6
7
8
9
10
Molecular Nomenclature:
Examples
 CCl4
 carbon
tetrachloride
 N 2O
 dinitrogen
monoxide
 SF6
 sulfur
hexafluoride
More Molecular Examples
 arsenic
trichloride
 AsCl3
 dinitrogen
pentoxide
 N2O5
 tetraphosphorus
 P4O10
decoxide
Learning Check
Fill in the blanks to complete the following
names of covalent compounds.
CO
carbon ______oxide
CO2
carbon _______________
PCl3
_______chloride
phosphorus
CCl4
carbon ________chloride
N2O
_____nitrogen _____oxide
Learning Check
1.
P2O5
a) phosphorus oxide
b) phosphorus pentoxide
c) diphosphorus pentoxide
2.
Cl2O7
a) dichlorine heptoxide
b) dichlorine oxide
c) chlorine heptoxide
3.
Cl2
a) chlorine
b) dichlorine
c) dichloride
Practice
• Practice naming covalent (molecular)
compounds
• Take a look at your Periodic Table Exam
Lewis Structures with Covalent
Compounds
• RULES for making covalent bonds:
• Add up the valence electrons of each
contributing element
• Place the electrons around the bonding
elements so that the octet rule is obeyed
(remember that H's "octet" is 2 electrons) - you
may have single, double, or triple bonds
• Examples: F2, O2, N2, CO2, HCN
Practice
• Back of pg. 2
• Please do NOT circle the valence (like in
their example)
– Show the shared electrons as a dash
– H—H, instead of H:H
Closure
• Without looking at a pink or white sheet,
what is…?
– Chlorate
– Nitrate
– Nitrite
– Acetate
– Ammonium