Today you need:
12/7
‐pencil
‐journal
Infographic
‐paper
‐G/O you made from 2.3
DUE!!
Warm up:
Describe the difference between a sodium atom and a sodium ion.
Today we will:
‐Explore Ionic Bonding‐ questions due end of period
Group‐columns each element in a group has = number of electrons on the outer energy level
Period‐
Rows
add 1 proton
as you meve
to the right‐
changes the
type of atom
Atomic Number
valence electron number
symbol
name of element
atomic mass
Atomic Number
‐number of protons
‐number of electrons
‐identity of the Atom
‐allows for the
calculation of mass
Atomic Mass
‐number of protons +
number of neutrons
(# of Neutrons= At. Mass ‐ At. number)
18
8
8
2
electron
proton
neutron
�
 We used the Bohr model to count
electrons ‐ number of electrons in a atom equals
the number of protons.
 Each circle represents a energy level a
certain distance from the nucleus
 We talked about the "Octet Rule" as a
model for filling the outer energy level to 8
electrons
 In this example, Oxygen "wants" 2 more
electrons to be "happy" (stable)
 The electrons in the outer shell are
generally called the VALENCE electrons
 Valence Electrons are involved in
bonding!
Lewis dot structures:
A useful model for bonding.
In 1916 a chemist named G. N. Lewis discovered the
mechanics of the covalent bond. Shortly after he came up
with a model for figuring out ionic and covalent bonds.
He came up with the concept of the octet rule. While not
completely accurate by today's standards, it is still a good
model for beginning chemistry. (We know a lot more about
things now than he knew then!)
Na
11+
Bohr Model
 Lewis Structure
only shows valence
electrons.
Na
Lewis Dot Structure
1
2
3
Cl
Cl
Cl
"dots" are used to
represent valence
electrons ‐places in 4
regions around the
symbol
Cl has 7 valence
electrons
one dot is placed
in each of the 4
regions before a
second dot is
placed.
Cl has 7 valence
electrons
‐continue placing
dots in the
regions around
the symbol until
all valence
electrons have
been used
Cl
You can see that
there is room for
one more
electron to
complete the
"Octet Rule"
Name
__ pd
_ Date
Lewis Structure Worksheet:
Use your notes and your Periodic Ta ble to help you complete the table and answer t he
questions below.
Symbol
-
#of Protons
#Electrons
# Valence
Electrons
1
H
Hydrogen
1.008
-
.,;;,,.....-
2
He
Helium
4.003
-,3
Li
I
•
Lithium
6.941
9
F
Fluorine
18.998
8
0
o ygen
15.999
>-- :
11
Na
Sodium
22.990
12
Mg
Magnesium
24.305
13
Al
Aluminum
26.982
15
p
Phosphorus
30.974
I
Lewis Dot
Structure
_
Symbol
#of Protons
#Electrons
# Valence
Electrons
I
17
Cl
Chlori
ne
35.453
18
-
-
Ar
Argon
39.948
19
K
Potassiu m
39.098
20
Ca
Calcium
40.078
35
Br
Bromine
79.904
What types of electrical charges are there?
What is an atom made of?
How do you tell what atom it is?
Do atoms have an electrical charge?
How do you know how many protons an atom has?
How do you know how many electrons an atom has?
How do you know how many neutrons an atom has?
Do neutrons contribute to the electrical cha rge of an atom?
What effect does gaining an electron have on the charge of an atom?
What effect does losing an electron have on the charge of an atom?
Lewis Dot
Structure
Forming an Naming Ionic Compounds
Forming Ions
Some Common Ions
Ion Name
Lithium
Charge
l
+
symbol
u·
Sodium
l+
Na+
Potassium
l+
K+
Ammonium
l
+
Ca L+
2+
Magnesium
2+
Mg2+
Aluminum
3+
Fluoride
1-
3
Al +
F1-
Chloride
1-
Cl 1-
Iodide
1-
Bicarbonate
1-
Nitrate
1-
Ox ide
2-
Sulfide
2-
Carbonate
2-
C03 2 -
Sulfate
2-
so.2 -
Phosphate
3-
PO/
t
HC03 1
NO/ 02 -
•
•
•
•
52 -
Naming Ionic Compounds
•
•
NH/
Calcium
•
•
•
Today you need:
‐work from yesterday
‐pencil
‐notes on ionic bonds
‐periodic table
12/9
Warm up: Write the formula for sodium sulfide. Which is the cation?
Which is the anion?
Today we will:
‐practice with ionic compounds
‐Due tomorrow: Notes/graphic organizer for 2.4
Covalent Bonds
Name --------------------- pd
Date
_
POSITIVE and NEGATIVE IONS
The tables below list some common positive and negative ions. Refer to the table as you answer the questions.
Table 2 : Negative Ions
Table 1: Positive Ions
Ion Name
Symbol
Symbol
Ion Name
aluminum
Al3+
x
bromide
Br-
barium
Ba2 +
cadmium
Cd2+
ClF1-
calcium
Ca 2 +
cesium
cs•
x chloride
x fluoride
x iodide
x nitride
x oxide
x phosphide
x sulfide
x
x
x
x
copper (I)
cu•
copper (II)
Cu2+
iron (II)
Fe2+
iron (Ill)
Fe3+
lithium
u•
potassium
K+
sodium
Na+
1 1N 3-
ozp352 -
1. How many electrons does sodium lose when making a chemical
bond?
2. How many electrons does phosphorus gain when making a chemical bond?
3.
_
Name 2 metals that do not always lose the same number of electrons. How can you tell?
4. Name 4 nonmetals that could take the electron that lithium loses when forming
bonds.
5. In a chemical compound, would you expect an oxide ion to be joined with one atom of calcium or
one atom of lithium
atomof potassium? Why?
6. A molecule of sodium nitride would contain how many sodium ions?
Why?
7. Predict the number of each atom needed to form an molecule of Potassium Sulfide.
)
Name
pd
NAMES AND FORMULAS WORKSHEET #1
Write the correct formula for each of the following compounds .
1. lithium iodide -------------
2. calcium oxide
_
3. sodium sulfide
_
4. aluminum oxide -------------5.
barium sulfide
6.
aluminum chloride
7.
lithium fluoride -----------
8.
cesium nitride
9.
beryllium fluoride ------------
_
_
10. potassium phosphide -----------Give the correct name for each of the following ionic compounds.
11. Lil
_
12. Na2S
13. MgBr
14. AIF 3
15. BaO
16. Bah
17. KCI
18. CaO
19. LiCI
20. Bes
_
Date
_
Name ----pd
Date
Formula Worksheet 2
1. strontium iodide
2. rubidium nitride
3. manganese(IV) chloride
4. zinc fluoride
5. chromium {Ill) oxide
6. iron {II) phosphide
7. cobalt {II) sulfide
8. silver oxide
9. mercury {I) chloride
11. Sc02
12. K20.
-------------------
13.NaCl
14.Zn S
17. FeP
_
Name
pd
Date
NAMES AND FORMULAS WORKSHEET #3
Write the correct formula for each of the following c ompounds.
1. mercury (II) sulfide
2.
zinc oxide
3. sodium sulfide
4.
copper (l)oxide
5.
iron(l l
)bromide
6. tin (IV) oxide
7. aluminum oxide
8.
manganese (I) sulfide
9.
cobalt (II) phosphide
10. silver iodide
Give the correct name for each of the following ionic compounds.
11.Cr2O3
12. MnBr
13. PbO
14. FeS
15. FeF2
16. Hgl
17. CuO
18. AgI
_
Today you need:
journal
‐Notes or G/O of 2.4 on Covalent Bonds
‐paper
Formula worksheets
12/10
Warm up: What force holds IONIC COMPOUNDS together?
Today we will:
‐Compare ionic bonds to COVALENT BONDS
In IONIC BONDS the metal (like
sodium) actually LOSES
electrons!...they are NOT
orbiting that atom anymore!
The non‐metal (like Chlorine)
GAINS electrons.
The one that left the metal now
completely orbits the non‐
metal
Octet Rule is satisfied for BOTH
atoms
Today you need:
‐journal
‐paper
Formula worksheets
12/11
Warm up: Describe the main difference between Covalent and Ionic
Bonds
Today we will:
‐Learn COVALENT BOND naming protocols
Naming worksheet due end of period!
Forming Covalent Bonds:
 Covalent Bonds form when 2 elements
SHARE electrons on the outer shell (valence
electrons)
 Both atoms sharing the electrons attract the
electrons equally
 Can form more than one bond‐ can make
double or triple bonds!
 Lewis DOT structures help!‐ shared pairs of
electrons count for each atom that is sharing
them
Properties:
 MUCH lower melting and boiling point than Ionic
Compounds‐ Forces holding covalent bonds together
are much weaker than ionic bonds so...
.... Less heat required to separate the
particles than in an ionic solid.
 Very poor conductors of electricity‐ no charged
particles move around in covalent solids and so...
... no charged particles to help electricity move
***That is why molecular solids like plastic are used
as electrical insulators!!***
http://www.slideshare.net/gueste5efd8/atomic-structure-student-copy
Unequal Sharing of Electrons:
 Some atoms pull on shared electrons harder than other atoms so...
... the shared electrons move a little closer to toward one atom
than another
RESULT: one part of the molecule has a slight + charge another part has
a slight ‐ charge called a POLAR molecule‐ not as strong as an ion, but definitely
different charges in different parts of the molecule.
Two Atoms that pull on shared electrons equally‐ neither atom is charged and the
NON‐POLAR
molecule is referred to as
Example: Carbon Dioxide (CO 2)
POLAR MOLECULE:
Water is polar. Oxygen pulls harder on the shared electrons and so the shared electron
spend more time around the oxygen end than the hydrogen end. RESULT: The oxygen
side is slightly negative, the hydrogen side is slightly positive
Naming Covalent Compounds
Several methods or systems for naming chemicals have been developed
over the years.
Simple names are used for ionic compounds (and some covalent compounds) where only one
compound is made from those elements.
Latin names are used for ionic compounds (and some covalent compounds) where more than
one compound is made from those elements.
Stock names are used for ionic compounds and covalent compounds where more than one
compound is made from those elements.
Prefix names are used for covalent compounds.
Using Prefixes to name Covalent Compounds
Covalent compounds are named in different ways than ionic compounds (although
there is some overlap).
Many of these compounds have common names such as "methane", "ammonia" and
"water".
However, simple covalent compounds are generally named by using prefixes to
indicate how many atoms of each element are shown in the formula. Also, the ending
of the last (most negative) element is changed to ‐ide.
The prefixes used are mono‐, di‐, tri‐, tetra‐, penta‐, hexa‐, and so
forth.
The mono‐ prefix is usually not used for the first element in the formula. The "o" and
"a" endings of these prefixes commonly are dropped when they are attached to
"oxide." You should memorize the prefixes from 1‐10
1
2
3
4
5
6
7
8
9
10
mono‐
di‐
tri‐
tetra‐
penta‐
hexa‐
Hepta‐
octa‐
nona‐
deca‐
You also need to know which element to put first in the formulas!
Generally, they are in the same left‐to‐right order that they are on the periodic table,
except that you would have to squeeze hydrogen in between nitrogen and oxygen.
Name the following compounds.
PH3
N2O3
CO
SO2
HI
SCl6
CH4
NH3
H2O
HCl
phosphorus trihydride
dinitrogen trioxide
carbon monoxide
sulfur dioxide
hydrogen monoiodide*
sulfur hexachloride
methane carbon tetrahydride
ammonia nitrogen trihydride
water
dihydrogen monoxide
Hydrogen monochloride
Naming Covalent Compounds Worksheet
Write the formulas for the following covalent compounds:
1)
antimony tribromide
2)
hexaboron silicide
3)
chlorine dioxide
4)
hydrogen iodide
5)
iodine pentafluoride
6)
dinitrogen trioxide
7)
ammonia
8)
phosphorus triiodide
Write the names for the following covalent compounds:
9)
P4S5
10)
O2
11)
SeF6
12)
SbBr6
13)
SCl4
14)
CH4
15)
B2Si
16)
NF3
For those who want a real Challenge!
1) NaBr
2)
Ca(C2H3O2)2
3)
P 2 O5
4)
Ti(SO4)2
5)
FePO4
6)
K3N
7)
SO2
8) CuOH
9)
Zn(NO2)2
10) V2S3
Write the formulas for the following chemical compounds:
11)
silicon dioxide
12)
nickel (Ill) sulfide
13)
manganese (II) phosphate
14)
silver acetate
15)
diboron tetrabromide
16)
magnesium sulfate heptahydrate
17)
potassium carbonate
18)
ammonium oxide
19)
tin (IV) selenide
20)
carbon tetrachloride