Chemistry Objective. Warm-Up What do the following atoms have to do to become stable? a. barium b. nitrogen c. fluorine
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1 Chemistry Objective Students will: 1. describe how a covalent bond is formed. 2. describe properties of a covalently bonded substance. 3. describe the difference between a polar covalent and nonpolar covalent bond. Warm-Up What do the following atoms have to do to become stable? a. barium b. nitrogen c. fluorine
2 Types of Chemical Bonds Last chapter we discussed one type of chemical bond,
3 Types of Chemical Bonds Last chapter we discussed one type of chemical bond, the Ionic Bond.
4 Types of Chemical Bonds Last chapter we discussed one type of chemical bond, the Ionic Bond. An Ionic Bond is formed one atom transfers one or more electrons to another.
5 Types of Chemical Bonds Last chapter we discussed one type of chemical bond, the Ionic Bond. An Ionic Bond is formed one atom transfers one or more electrons to another. That transfer produces two oppositely charged ions which are then attracted to each other.
6 Types of Chemical Bonds Last chapter we discussed one type of chemical bond, the Ionic Bond. An Ionic Bond is formed one atom transfers one or more electrons to another. That transfer produces two oppositely charged ions which are then attracted to each other. metal gives its electron away Na Cl Na + Cl - nonmetal accepts the electron Ca Cl Ca 2+ Cl2 - Cl ionic compound made up a cation and an anion.
7 Types of Chemical Bonds Last chapter we discussed one type of chemical bond, the Ionic Bond. An Ionic Bond is formed one atom transfers one or more electrons to another. That transfer produces two oppositely charged ions which are then attracted to each other. metal gives its electron away Na Cl Na + Cl - nonmetal accepts the electron ionic compound made up a cation and an anion. Since metals have such a low electronegativity, they will not attract electrons from another atom to become negative ions. In fact they will gladly give up their own electrons to become stable. Nonmetals on the other hand have a high electronegativty and will gladly accept any electrons to themselves. This means that the difference in electronegativity between the two atoms will be GREAT!
8 Types of Chemical Bonds But take for example water, H2O. Water is not bonded ionically. How do we know? Let s look at some data: Substance Table salt (NaCl) Water (H2O) Physical state (@ room temp) solid liquid Melting Point 801 C 0 C Boiling Point 1413 C 100 C Lower melting and boiling points for water suggest that the attractions among particles are weaker than those in salt.
9 Types of Chemical Bonds But take for example water, H2O. Water is not bonded ionically. How do we know? Let s look at some data: Substance Table salt (NaCl) Water (H2O) Physical state (@ room temp) solid liquid Melting Point 801 C 0 C Boiling Point 1413 C 100 C Remember in a salt crystal each ion is bonded to six adjacent ions. Each of those bonds must be broken to get the particle to melt.
10 Types of Chemical Bonds But take for example water, H2O. Water is not bonded ionically. How do we know? Let s look at some data: Substance Table salt (NaCl) Water (H2O) Physical state (@ room temp) solid liquid Melting Point 801 C 0 C Boiling Point 1413 C 100 C However in a water molecule the atoms are bonded only to each other, not between molecules.
11 Types of Chemical Bonds But take for example water, H2O. Water is not bonded ionically. How do we know? Let s look at some data: Substance Table salt (NaCl) Water (H2O) Physical state (@ room temp) solid liquid Melting Point 801 C 0 C Boiling Point 1413 C 100 C However in a water molecule the atoms are bonded only to each other, not between molecules. And because of that water has a much lower melting and boiling point.
12 Types of Chemical Bonds Being that there are NO attractions between molecules, then that means there are no charges as well. But how do the atoms achieve a stable octet?
13 Types of Chemical Bonds Being that there are NO attractions between molecules, then that means there are no charges as well. But how do the atoms achieve a stable octet? The atoms within a water molecule achieve a stable octet by SHARING electrons with one another. Let s look at a simple molecule of fluorine, F2.
14 Types of Chemical Bonds Being that there are NO attractions between molecules, then that means there are no charges as well. But how do the atoms achieve a stable octet? The atoms within a water molecule achieve a stable octet by SHARING electrons with one another. Let s look at a simple molecule of fluorine, F2. F F Each fluorine atom has 7 valence electrons. So both are not stable by themselves.
15 Types of Chemical Bonds Being that there are NO attractions between molecules, then that means there are no charges as well. But how do the atoms achieve a stable octet? The atoms within a water molecule achieve a stable octet by SHARING electrons with one another. Let s look at a simple molecule of fluorine, F2. F F Inside of this yellow oval there are now 8 electrons, or a stable octet.
16 Types of Chemical Bonds Being that there are NO attractions between molecules, then that means there are no charges as well. But how do the atoms achieve a stable octet? The atoms within a water molecule achieve a stable octet by SHARING electrons with one another. Let s look at a simple molecule of fluorine, F2. F F And inside of this blue oval there are now 8 electrons, or a stable octet.
17 Types of Chemical Bonds Being that there are NO attractions between molecules, then that means there are no charges as well. But how do the atoms achieve a stable octet? The atoms within a water molecule achieve a stable octet by SHARING electrons with one another. Let s look at a simple molecule of fluorine, F2. F F F2 Now both fluorine atoms have a stable octet if they share an electron each.
18 F F That sharing of electrons is referred to as a COVALENT BOND.
19 F F That sharing of electrons is referred to as a COVALENT BOND. You will remember that we said that the smallest portion of a crystal structure is called the unit cell. And that unit cell is always written in the lowest terms, such as NaCl.
20 F F That sharing of electrons is referred to as a COVALENT BOND. You will remember that we said that the smallest portion of a crystal structure is called the unit cell. And that unit cell is always written in the lowest terms, such as NaCl. Well since substances that are bonded covalently are not attracted to each other, we can refer to them as molecular compounds because they exist as individual molecules.
21 F F That sharing of electrons is referred to as a COVALENT BOND. Also since the electrons are shared, there are no charges associated with the molecules which means that
22 F F That sharing of electrons is referred to as a COVALENT BOND. Also since the electrons are shared, there are no charges associated with the molecules which means that there is no way that covalently bonded substances will conduct electricity.
23 Well what kind of atoms will share electrons as opposed to transfer electrons to become stable? NONMETALS and some Metalloids!!
24 So molecular compounds are predominantly made up of TWO NONMETALS.
25 So molecular compounds are predominantly made up of TWO NONMETALS. This also means that the difference in their values for electronegativity will not be so great. In fact we will consider them to have a small difference in electronegativity.
26 You see the bond properties are directly related to the difference in electronegativities.
27 You see the bond properties are directly related to the difference in electronegativities. Let s look in more detail. Substance Formula Melting Point Boiling Point Water H2O 0 C 100 C Methane CH4-182 C -161 C If you look at it water remains a liquid for a larger temperature range. This can be explained by looking at how the electrons are being shared.
28 You see the bond properties are directly related to the difference in electronegativities. Let s look in more detail. Substance Formula Melting Point Boiling Point Water H2O 0 C 100 C Methane CH4-182 C -161 C If you look at it water remains a liquid for a larger temperature range. This can be explained by looking at how the electrons are being shared. This leads us to the thought that chemical bonds are not completely covalent. Or for that matter, bonds are not fully ionic as well.
29 This leads us to the thought that chemical bonds are not completely covalent. Or for that matter, bonds are not fully ionic as well.
30 This leads us to the thought that chemical bonds are not completely covalent. Or for that matter, bonds are not fully ionic as well. For example, even though electrons are shared between the hydrogen and oxygen atoms, they are not shared evenly.
31 This leads us to the thought that chemical bonds are not completely covalent. Or for that matter, bonds are not fully ionic as well. For example, even though electrons are shared between the hydrogen and oxygen atoms, they are not shared evenly. Remembering back to the trend for electronegativity, decreasing going down and increasing going across, rarely will two different atoms have identical electronegativities. decreasing increasing
32 This leads us to the thought that chemical bonds are not completely covalent. Or for that matter, bonds are not fully ionic as well. For example, even though electrons are shared between the hydrogen and oxygen atoms, they are not shared evenly. Remembering back to the trend for electronegativity, decreasing going down and increasing going across, rarely will two different atoms have identical electronegativities. decreasing If the two values for electronegativity don t match up, then the shared electrons will be pulled closer towards one atom than the other. increasing
33 F F So if you think about that original fluorine molecule, the pair of electrons that are being shared will be evenly distributed between the two atoms.
34 F F So if you think about that original fluorine molecule, the pair of electrons that are being shared will be evenly distributed between the two atoms. An even, or equal, sharing of electrons is called a Nonpolar Covalent Bond.
35 F F So if you think about that original fluorine molecule, the pair of electrons that are being shared will be evenly distributed between the two atoms. An even, or equal, sharing of electrons is called a Nonpolar Covalent Bond. But inside of the water molecule, oxygen has a higher electronegativity. That means that oxygen will pull the electrons being shared more towards itself, leading to an uneven sharing of electrons. H O H
36 F F So if you think about that original fluorine molecule, the pair of electrons that are being shared will be evenly distributed between the two atoms. An even, or equal, sharing of electrons is called a Nonpolar Covalent Bond. But inside of the water molecule, oxygen has a higher electronegativity. That means that oxygen will pull the electrons being shared more towards itself, leading to an uneven sharing of electrons. An uneven, or unequal, sharing of electrons is called a Polar Covalent Bond. H O H
37 H O H That means we draw a water molecule like so: H O H Remembering that the electrons are NOT transferred only pulled closer to the oxygen atom.
38 H O H That means we draw a water molecule like so: H O H Remembering that the electrons are NOT transferred only pulled closer to the oxygen atom. Now determining the type of bonds is easy given the electronegativity values for the atoms.
39 Remember that the difference in electronegativity will determine the type of bond formed POLAR COVALENT 2.0 IONIC 4.0 NONPOLAR COVALENT So for the following bonds: Cs & F C & O I & I
40 Remember that the difference in electronegativity will determine the type of bond formed POLAR COVALENT 2.0 IONIC 4.0 NONPOLAR COVALENT So for the following bonds: Cs & F C & O F = 4.0 Cs = = 3.3 IONIC C = = = 1.0 POLAR Covalent I & I I = = 0 NONPOLAR Covalent
41 Homework: Pg. 197 #1-5
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