9.4.2 Practice: Bonding N_Cruz
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Practice Assignment
Physical Science (S1744040)
Nestor Cruz
Points possible: 50
Date: 12/19/12
1.Bonds are attractive forces that hold compounds together. What role do valence electrons play in the formation of bonds? (3 points)
The electrons in the outershell are the valence electrons. They can either be lost or gained in a chemical reaction
2.How do ionic bonds differ from covalent bonds? (3 points)
An ionic bond is the transfer of electrons and a covalent bond is the sharing of electrons.
3.What is the difference between the electronegativity values of carbon and sulfur? What type of bond do they form? How do you know? (4 points)
Sulfer and carbon are close to each other on the periodic table, so they have similar electronegativities.
Carbon=2.55
Sulfer=2.58
4.What is the difference between the electronegativity values of sodium and bromine? What type of bond do they form? How do you know? (4 points)
Sodium=Covalent
Bromine=Hydrogen
5.What does it mean when a covalent bond is polar? How can you tell if a bond is polar or nonpolar? (4 points)
The atoms that they share help you tell if it is polar or nonpolar. When a covalent bond is polar, it is a bond that shares a pair of electrons, but one is held more closely than the other.
6.How does the octet rule influence Lewis dot structures? (4 points)
Octet means 8, so this effects the amount of dots in the Lewis dot structure.
7.Answer the following questions based on the Lewis dot structure for water on the right. (4 points)
a. How many bonding pairs are present? How many lone pairs?
2 lone pairs & 2 bonding pairs.
b.The electron-group geometry of the water molecule is a tetrahedron, but the molecular geometry is bent. How can this be explained?
It can be explained because of the tetrahedral arrangement around the oxygen and the presence of lone pairs electrons.
c.Is the water molecule polar? Why, or why not?
Yes, because it is a tetrahedron.
8.Answer the following questions based on the Lewis dot structure for carbon dioxide on the right. (4 points)
a.Why does carbon dioxide have a higher bond order than water?
Carbon and Oxygen form a larger force and bond over water.
b.What does this bond-order difference mean, in terms of bond energy?
Bond order is the number of chemical bonds between a pair of atoms. The bond-order difference is the amount of extras.
9.Compare exothermic reactions and endothermic reactions. Give at least one similarity and one difference. (4 points)
Exothermic and Endothermic can both have very dangerous reactions. Exothermic-heat given off & Endothermic-heat added.
10. Why does hydrogen bonding help ice cubes float? (4 points)
The lattice structure makes it less dense than water.
11. Table salt, NaCl, is a classic binary ionic compound. (4 points)
a. What is the oxidation number of Na? Of Cl?
Na=+1
Cl=-1
b. What characteristics make NaCl a salt?
NaCl is an ionic compound.
12. Water is the most common covalent compound on the planet. (4 points)
a. Write the molecular formula for water. What would be the correct name for this molecule, if nomenclature (chemical-naming) guidelines were followed?
Dihydrogen Monoxide, H20
b. What evidence do you have that water is a covalent compound?
Hydrogen and oxygen are both nonmetals.
13. Iron is a transition metal with multiple oxidation numbers. (4 points)
a. What is the iron (II) ion? How does it differ from the iron (III) ion?
Theres a +2 charge.
b.If iron were to bond with oxygen, predict the formula for each oxidation number of iron.
Fe0^2, Fe0^3, Fe064
c.How would each formula be named?
By the data that is found in relation to each formula.
Williams, Sue
9.4.2 Practice: Bonding
Practice Assignment
Physical Science (S1744040)
Nestor Cruz
Points possible: 50
Date: 12/19/12
1.Bonds are attractive forces that hold compounds together. What role do valence electrons play in the formation of bonds? (3 points)
The electrons in the outershell are the valence electrons. They can either be lost or gained in a chemical reaction
3 points
2.How do ionic bonds differ from covalent bonds? (3 points)
An ionic bond is the transfer of electrons and a covalent bond is the sharing of electrons.
3 points
3.What is the difference between the electronegativity values of carbon and sulfur? What type of bond do they form? How do you know? (4 points)
Sulfer and carbon are close to each other on the periodic table, so they have similar electronegativities.
Carbon=2.55
Sulfer=2.58
0 points
4.What is the difference between the electronegativity values of sodium and bromine? What type of bond do they form? How do you know? (4 points)
Sodium=Covalent
Bromine=Hydrogen
4 points
5.What does it mean when a covalent bond is polar? How can you tell if a bond is polar or nonpolar? (4 points)
The atoms that they share help you tell if it is polar or nonpolar. When a covalent bond is polar, it is a bond that shares a pair of electrons, but one is held more closely than the other.
2 points
6.How does the octet rule influence Lewis dot structures? (4 points)
Octet means 8, so this effects the amount of dots in the Lewis dot structure.
1 point
7.Answer the following questions based on the Lewis dot structure for water on the right. (4 points)
a. How many bonding pairs are present? How many lone pairs?
2 lone pairs & 2 bonding pairs.
4 points
b.The electron-group geometry of the water molecule is a tetrahedron, but the molecular geometry is bent. How can this be explained?
It can be explained because of the tetrahedral arrangement around the oxygen and the presence of lone pairs electrons.
2 points
c.Is the water molecule polar? Why, or why not?
Yes, because it is a tetrahedron.
1 point
8.Answer the following questions based on the Lewis dot structure for carbon dioxide on the right. (4 points)
a.Why does carbon dioxide have a higher bond order than water?
Carbon and Oxygen form a larger force and bond over water.
0 points
b.What does this bond-order difference mean, in terms of bond energy?
Bond order is the number of chemical bonds between a pair of atoms. The bond-order difference is the amount of extras.
0 points
9.Compare exothermic reactions and endothermic reactions. Give at least one similarity and one difference. (4 points)
Exothermic and Endothermic can both have very dangerous reactions. Exothermic-heat given off & Endothermic-heat added.
2 points
10. Why does hydrogen bonding help ice cubes float? (4 points)
The lattice structure makes it less dense than water.
2 points
11. Table salt, NaCl, is a classic binary ionic compound. (4 points)
a. What is the oxidation number of Na? Of Cl?
Na=+1
Cl=-1
2 poinrs
b. What characteristics make NaCl a salt?
NaCl is an ionic compound.
1 point
12. Water is the most common covalent compound on the planet. (4 points)
a. Write the molecular formula for water. What would be the correct name for this molecule, if nomenclature (chemical-naming) guidelines were followed?
Dihydrogen Monoxide, H20
4 points
b. What evidence do you have that water is a covalent compound?
Hydrogen and oxygen are both nonmetals.
13. Iron is a transition metal with multiple oxidation numbers. (4 points)
a. What is the iron (II) ion? How does it differ from the iron (III) ion?
Theres a +2 charge.
0 points
b.If iron were to bond with oxygen, predict the formula for each oxidation number of iron.
Fe0^2, Fe0^3, Fe064
0 points
c.How would each formula be named?
By the data that is found in relation to each formula.
-- 0 points