Name____________________
Date___________________
Advanced Chemical Bonds Worksheet
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Ionic Bonding
How create the Lewis Structure (Dot Diagram) of an
atom. (Problems 1-8)
Example: Draw the Lewis Structure of a Magnesium Atom.
1.
Find the atomic number of that element by locating that element using the
periodic table. The atomic number tells us the number of total protons,
electrons, and neutrons in the atom.
Mg has an atomic number of 12.
Mg has 12 TOTAL electrons
2.
Find the number of valence electrons. Remember that atomic numbers tell
us the number of electrons, but NOT the number of VALENCE electrons.
Valence electrons are the electrons in the outermost energy level, that
determine if the element forms a chemical bond or not.
There can be 2 electrons in the innermost energy level of the atom
There can be 8 electrons in each of the energy levels after the 1 st one.
Magnesium
Atomic
Number
Atomic
Mass
Number of
Protons,
electrons,
and
neutrons
Column in
the periodic
table
Number of
valence
electrons
12
24.305
amus
12
2
2
Mg has 2 valence electrons because it has 12 total electrons. 2 of those occupy the 1st energy
level, and 8 of them occupy the 2nd energy level. Therefore there are 2 electrons left over in the 3 rd
energy level.
Shortcut- Mg has 2 valence electrons because it is in the 2 nd column.
3.
Draw the Lewis structure, by writing down the atomic symbol. Then place each valence electron
around the symbol as a dot. Place one at each of the 4 sides of the symbol, then double them up.
The most valence electrons that an element can have would be 8 and the least would be 1 valence
electron.
BAD
GOOD
Lewis Structures of Atoms: Draw Lewis Structures for the following elements.
1. Cl
5. S
2. H
6. Ca
3. O
4. Ar
7. F
8. Na
How to Convert an atom into an ION. (Problems 9-16)
Example: What does a Chlorine Ion look like?
1.
2.
Draw the lewis structure of a chlorine atom.
Follow the octet rule. Atoms are unstable until they have a full
outer shell of electrons. For H and He, this means that they have 2
electrons. For all other elements, this means that they have 8.
For this reason, Noble Gases do NOT form ions.
Atom
Ion
F
-
Ca
2+
S
2-
Ne
Does not
form an
ion
If chlorine gains just 1 electron, it will have 8 electrons in its outer shell. So add 1 electron to the
chlorine atom.
3.
Remember that the charge of an electron is negative. So if we gain 1 electron our atom gets a
negative charge. All negatively charged ions are called anions. Write the ion’s charge in the
upper right hand side of the lewis structure.
4.
If an ion loses electrons to have 8 electrons in its outer shell, it loses negative charges. This makes
the atom positively charged. Positively charged ion are called cations. See the steps below for
making a sodium cation.
Lewis Structures of Ions: Draw Lewis Structures for the following IONS. (one of them doesn’t form an
ion)
9. Cl
10. H
11. O
12. Ar
13. S
14. Ca
15. Cu(I)
16. Na
How to draw Lewis Structures of Ionic Compounds (Page
201-203. Problems 17-21)
Example: What molecule would form from Sodium ions and chlorine ions?
1.
Draw the lewis structure of a chlorine atom and a sodium atom.
2.
Convert the atoms to ions. But…
Electrons can’t just come from nowhere (that would violate the 1 st law of Thermodynamics!). So
when sodium loses an ion it must be transferred to the chlorine.
Draw the process of moving electrons from one atom to the other.
3.
Re-draw the lewis structure of the combined molecule. Include the charge of each ion.
4.
Sometimes this can be a little more difficult. Think of bonding aluminum to oxygen. Aluminum
wants to get rid of 3 electrons, but oxygen can only take 2.
Therefore, the last remaining electron must go to another oxygen atom. But this atom is still short
1 electron.
In order to make the oxygen have a full octet lets take an electron away from a second Aluminum
atom.
In order to make the aluminum have a full octet, it would have to lose another 2 electrons, so lets
add another oxygen atom
Now all 3 oxygen atoms have full octets and both aluminum atoms have full octets. Redraw the
ionic compound to make everything look neat. Add in charges.
Ionic Bonding: Draw the lewis structures of the following ionic compounds.
17.
Potassium and chlorine
18.
Bromine and Calcium
19.
Sulfur and Copper (I)
20. Oxygen and aluminum
21.
Lithium and Sulfur
How to write the chemical formula of an ionic
compound(Page 271-275. Problems 22-26)
Example:
Write the chemical formula of the compound made from fluorine and
magnesium
1. Draw the lewis structure of the compound that a fluorine atom and
a magnesium atom make.
Metal
Compound
Na
Nonmetal
Cl
Al
O
Al2O3
Mg
F
MgF2
NaCl
2.
Ionic compounds are made when metals and
non-metal bond together. Identify the metal
and a non-metal using the periodic table
3.
Write the atomic symbols of the two elements. The metal always goes first.
4.
Since there are 2 fluorine ions in one molecule of this compound, add a “2” subscript after the F.
Chemical formulae of ionic compounds: write the chemical formulae of the following ionic compounds
22.
Potassium and chlorine
Answer__________________
23.
Oxygen and aluminum
Answer__________________
24.
Sulfur and Copper (I)
Answer__________________
25.
Bromine and Calcium
Answer__________________
26.
Lithium and Sulfur
Answer__________________
How to name ionic compounds (Page 271-275. Problems 27-31)
Example: Name the compound made from chlorine and sodium.
1. Draw the lewis structure of the compound that a chlorine atom and a sodium atom make.
2.
Write the chemical formula of the compound that they make.
NaCl
3.
The first part of the name is just the metal.
Sodium
4.
The second part of the name is the nonmetal
Sodium chlorine
5.
Take away the last syllable of the non-metal and replace it with the “–ide” suffix.
Sodium chloride
Naming ionic compounds: name the following ionic compounds
27.
Potassium and chlorine
Answer__________________
28.
oxygen and aluminum
Answer__________________
29.
magnesium and fluorine
Answer__________________
30.
Bromine and Calcium
Answer__________________
31.
Copper(I) and Sulfur
Answer__________________
Covalent Bonding
How to draw Lewis Structures of
Covalent Compounds (Pages 226-229. Problems 32-37)
Example: What molecule would form from 1 Carbon atom and unlimited
hydrogen atoms?
1.
Draw the lewis structure of a Carbon atom and a hydrogen atom.
Atom
Calcium
Carbon
Aluminum
Hydrogen
Metal or
Nonmetal
Metal
NonMetal
Metal
NonMetal
2.
Create a covalent bond between the carbon atom and the hydrogen atom. All covalent bonds are
between 2 or more non-metals (no metals are needed). In a covalent bond, electrons are shared.
Therefore a single bond counts as 2 electrons for both the carbon and the hydrogen.
3.
Follow the octet rule. Atoms are unstable until they have a full outer shell of electrons. For H
and He, this means that they have 2 electrons. For all other elements, this means that they have 8.
For this reason, Noble Gases do NOT form covalent bonds.
Our Hydrogen now has 2 valence electrons and is “happy” according to the octet rule.
Our Carbon has 3 single electrons and a single bond for a total of 5 electrons. It is NOT “happy.”
4.
Bond more hydrogen atoms on to the carbon atom until all the hydrogen atoms have 2 valence
electrons and the carbon atom has 8 valence electrons.
5.
Rewrite the lewis structure of the molecule to make it look neat.
Simple Covalent Bonding: Draw the lewis structures of the following covalent compounds.
32.
2 carbon atoms and unlimited hydrogen atoms
33.
Bromine and Oxygen
34.
1 Nitrogen atoms and unlimited hydrogen atoms
35.
Oxygen and hydrogen
36.
1 sulfur atom, 4 oxygen atoms and unlimited hydrogen atoms (tricky)
37.
Phosphorus and hydrogen
How to draw Lewis Structures of
Covalent Compounds using Double and
Triple bonds (Page 230-231. Problems 38-43)
Example: What molecule would form from 1 Carbon atom and unlimited
oxygen atoms?
1.
Draw the lewis structure of a Carbon atom and an Oxygen atom.
Bond
Single
Number
of
electrons
it holds
2
Double
4
Triple
6
2.
Always start with the carbon atom (if there is one). Carbon often forms the “central atom” of
covalent compounds. Create a covalent bond between the carbon atom and the oxygen atom. In a
covalent bond, electrons are shared. Therefore the carbon is now surrounded by 5 electrons and
the oxygen is now surrounded by 7 electrons. According to the octet rule, neither atom is
“happy.”
3.
Create another covalent bond between the carbon atom and another oxygen atom. In a covalent
bond, electrons are shared. Therefore the carbon is now surrounded by 6 electrons and both
oxygens are now surrounded by 7 electrons. According to the octet rule, none of the atoms are
“happy.”
If we add two more oxygens the carbon will be “happy” but none of the oxygens will be. So this is not
possible
4.
There is a way that we can satisfy both the oxygens and the carbon. If we take the one of the extra
electrons on the carbon and share it with one of the extra electrons on one of the oxygens, we can
form a second bond. We now have a double bond.
5.
Take the last extra electron on the carbon and share it with the extra electron on one of the last
oxygen, we can form a second double bond. We now have 2 double bonds. Each double bond
counts as 4 electrons. All of our atoms now have 8 valence electrons.
6.
Rewrite the lewis structure of the molecule to make it look neat.
Advanced Covalent Bonding: Draw the lewis structures of the following covalent compounds.
38.
1 carbon atom, 2 oxygen atoms and unlimited hydrogen atoms
39.
1 sulfur atom, 1 nitrogen atom, 2 oxygen atoms, and 1 hydrogen atom
40.
1 Nitrogen atom, 1 hydrogen, and 1 carbon atom
41.
2 Carbon atoms and 2 hydrogen atoms
42.
Hydrogen, Oxygen, and Nitrogen
43.
2 Nitrogens
How to draw Lewis Structures of Covalent Compounds
using Coordinate Bonds (Pages 232-234, Problems 44-48)
Sometimes in a covalent compound, one atom will donate an electron pair so that it can bond to another
atom.
Example: What molecule would form from an N2 molecule and an oxygen atom?
1.
Draw the lewis structure of an N2 molecule and an Oxygen atom.
2.
The N2 molecule already has a stable configuration, but the oxygen does not.
3.
Therefore the entire system can become more stable when one of the nitrogen atoms donates its
lone pair of electrons to form a bond with the oxygen atom. To illustrate that BOTH of the
electrons are coming from the Nitrogen to the oxygen, we draw the bond as an arrow from the
Nitrogen to the Oxygen.
4.
Let look at the example of NH3 (ammonia, a neutral molecule). And a hydrogen ion. Draw the
lewis structure of both below.
5.
The Hydrogen ion can become more stable by bonding with nitrogen, but it does not have any
electrons to use. Fortunately, the Nitrogen has a lone pair to form a coordinate bond.
6.
How many protons and electrons do we now have in our ammonium molecule?
7.
Since our ammonium should have a +1 charge, we know it is a polyatomic ion (an ion made of
several atoms). Our ammonium ion must have the charge written and be placed in brackets.
Coordinate Covalent Bonding and Polyatomic ions: Draw the lewis structures of the following covalent
compounds.
44.
1 carbon atom and 1 oxygen atom
45.
1 sulfur atom, 3 oxygen atoms and 2 electrons
46.
1 oxygen atom, 1 hydrogen atom, and 1 electron
47.
1 water molecule and 1 hydrogen ion
48.
Nitric Acid (1 Hydrogen atom, 1 nitrogen atom, and 3 oxygen atoms)
49.
1 Carbon atom, 3 oxygen atoms, and 2 electrons
How to write the chemical formula of a covalent
compound (Page 280-286. Problems 50-55)
Example: Write the chemical formula of the compound made from
Nitrogen and Bromine.
1. Draw the lewis structure of the compound that a Nitrogen atom
and bromine atoms make.
Nonmetal
C
Nonmetal
F
Compound
H
O
H2O
C
O
CO2
CF4
2.
Write the atomic symbols of the two elements. The central atom usually goes first.
3.
Since there are 3 bromine atoms in one molecule of this compound, add a “3” subscript after the
Br.
Chemical formulae of covalent compounds: write the chemical formulae of the following covalent
compounds
50.
Phosphorus and chlorine
Answer__________________
51.
1 sulfur atom, 1 nitrogen atom, 2 oxygen atoms, and 1 hydrogen atom
Answer__________________
52.
Oxygen and fluorine
Answer__________________
53.
1 Carbon and 4 Hydrogens
Answer__________________
54.
2 Nitrogens
Answer__________________
55.
1 oxygen and 1 hydrogen and 1 electron
Answer__________________
How to name covalent compounds (Chapter 9 in the book. Problems 56-70)
Example: Name the compound made from nitrogen and bromine.
1. Draw the lewis structure of the compound that nitrogen and bromine make.
2.
Write the chemical formula of the compound that they make.
NBr3
3.
The first part of the name is just the central atom.
Nitrogen
4.
The second part of the name is the second element with the “ide” suffix.
Number
2
3
4
5
6
7
8
9
10
Prefix
Bi
Tri
Tetra
Penta
Hexa
Septa
Octa
Nona
Deca
Nitrogen bromide
5.
Add in the latin prefix to denote the number of atoms.
Nitrogen tribromide
Naming covalent compounds: name the following covalent compounds
56.
1 carbon and 2 oxygens
Answer__________________
57.
Hydrogen and Chlorine
Answer__________________
58.
Oxygen and fluorine
Answer__________________
59.
2 carbon atoms and 2 hydrogen atoms
Answer__________________
60.
2 carbon atoms and 6 chlorine atoms
Answer__________________
How to draw Lewis Structures of Covalent Compounds
using Polyatomic Ions (Pages 276-277, Problems 61-64)
Example: What molecule would form from magnesium ions and nitrate ions (NO3-)?
1.
Write the charges of the 2 ions
2.
3.
By looking at the charges, we can infer that we will need 2 nitrate ions for our 1 magnesium ion.
Write the lewis structures of the ions and draw the electrons leaving the metal and going to the
nonmetals.
4.
The polyatomic ions should be in brackets.
Polyatomic ionic Compounds: Draw the lewis structures of the following polyatomic compounds.
61.
1 calcium ion and 2 nitrate ions (NO3-)
62.
Hydronium ions (NH4+) and Oxygen ions.
63.
aluminum ions and carbonate ions (CO32-)
64.
Iron (II) and phosphate ions (PO43-)
How to write the chemical formula of a polyatomic
compound(Pages 276-277Problems 65-68)
Example: Write the chemical formula of the compound made from Magnesium and nitrate (NO3-).
1. Draw the lewis structure of the compound that would be formed.
2.
Write the atomic symbols of the two elements. The metal usually goes first.
3.
Since there are 2 nitrate ions in one molecule of this compound, add a “2” subscript after the
(NO3). The polyatomic ion must be in parentheses if there is more than one.
Polyatomic ionic Compounds: Write the chemical formulae of the following polyatomic compounds.
65.
1 calcium ion and 2 nitrate ions (NO3-)
Answer______________
66.
Hydronium ions (NH4+) and Oxygen ions.
Answer______________
67.
aluminum ions and carbonate ions (CO32-)
Answer______________
68.
Iron(II) ions and phosphate ions (PO43-)
Answer______________
How to name of a polyatomic compound (Pages 278. Problems 69-72)
Example: Write the name of the compound made from Magnesium and nitrate (NO3-).
1. Figure out the chemical formula of the compound.
2.
When naming, the metal usually goes first.
3.
There are 2 polyatomic NO ions, NO3- is nitrate and NO2- is nitrite. Usually, the polyatomic ion
with MORE Oxygens gets the –ATE suffix, and the one with LESS oxygens gets the –ITE suffix.
Polyatomic ionic Compounds: Write the chemical formulae of the following polyatomic compounds.
69.
Al2(NO3)3
Answer__________________
70.
Ammonium ions (NH4+) and Oxygen ions.
Answer__________________
71.
aluminum ions and carbonate ions (CO32-)
Answer__________________
72.
Iron(II) and phosphate ions (PO43-)
Answer__________________