(a)
Interpretation:
To analyze whether the given statement- A covalent bond is formed between two atoms whose difference in electronegativity is less than 1.9, is true or not.
Concept Introduction:
The octet rule states that atoms of various elements enter chemical combination so as to attain a configuration of eight electrons in their outermost shell. They do so by either transference of electrons or by mutual sharing of electrons.
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
Answer to Problem 3.55P
A covalent bond is formed between two atoms whose difference in electronegativity is less than 1.9. Thus, the statement is true.
Explanation of Solution
The electronegativity difference between the atoms determine that whether the bond formed will be covalent or ionic.
If the atoms have equal electronegativity value, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale, if exceeded, the bond becomes ionic in nature.
For example: For hydrogen gas: The electronegativity of both the hydrogen is 2.2, therefore a non-polar covalent bond is formed.
For hydrogen chloride:
Electronegativity of Hydrogen = 2.2.
Electronegativity of Chlorine = 3.1.
Electronegativity difference = 0.9.
Therefore, a polar covalent bond is formed.
For sodium chloride:
Electronegativity of Sodium = 1.0.
Electronegativity of Chlorine = 3.1.
Electronegativity difference = 2.1.
Therefore, an ionic bond is formed.
Thus, a covalent bond is formed between two atoms whose difference in electronegativity is less than 1.9.
(b)
Interpretation:
To analyze whether the given statement- If the difference in electronegativity between two atoms is zero (they have identical electronegativities), then the two atoms will not form a covalent bond, is true or not.
Concept Introduction:
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
If the difference in electronegativity between two atoms is zero (they have identical electronegativities), then the two atoms will form a covalent bond. Thus, the statement is false.
The electronegativity difference between the atoms determine that whether the bond formed will be covalent or ionic.
If the atoms have equal electronegativity value, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale, if exceeded, the bond becomes ionic in nature.
For example: For hydrogen gas: The electronegativity of both the hydrogen is 2.2, therefore a non-polar covalent bond is formed.
(c)
Interpretation:
To analyze whether the given statement- A covalent bond is formed by sharing two electrons is called a double bond, is true or not.
Concept Introduction:
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
A covalent bond is formed by sharing two electrons is called a double bond. Thus, the statement is true.
Atoms taking part in covalent bond formation may share one, two or three electron pairs thus, forming single, double and triple bond respectively.
An oxygen atom is formed when an atom of oxygen shares a pair of atoms each.
(d)
Interpretation:
To analyze whether the given statement - In the hydrogen molecule
Concept Introduction:
The octet rule states that atoms of various elements enter into chemical combination so as to attain a configuration of eight electrons in their outermost shell. They do so by either transference of electrons or by mutual sharing of electrons.
In the hydrogen molecule
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively. Hydrogen has only one electron in their valence shell, it shares it with another electron of the other Hydrogen atom to form a single covalent bond.
Sharing of 1 pair of electrons forms a single bond.
(e)
Interpretation:
To analyze whether the given statement in the molecule
Concept Introduction:
The octet rule states that atoms of various elements enter chemical combination so as to attain a configuration of eight electrons in their outermost shell. They do so by either transference of electrons or by mutual sharing of electrons. The logic of 8 electrons is that the noble gases have 8 electrons in their outermost shell and are stable. So, to attain stability noble gas configuration is acquired either by sharing, donating or accepting electrons.
In the molecule
The electronic configuration of the elements is according to the distribution of the electrons in the shells of the atoms.
These shells are K, L, M, n and so on.
K can accommodate a maximum of 2 electrons.
L can accommodate a maximum of 8 electrons.
M can accommodate a maximum of 18 electrons.
N can accommodate a maximum of 32 electrons.
The element with electronic configuration 2 is Helium, therefore each hydrogen attains electronic configuration of Helium.
The element with electronic configuration 2,8 is Neon, therefore each Carbon attains electronic configuration of Neon.
(f)
Interpretation:
To analyze whether the given statement, in a polar covalent bond, the more electronegative atom has a partial negative charge
Concept Introduction:
If the atoms have same electronegativity or they are of same atom, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
In a polar covalent bond, the more electronegative atom has a partial negative charge
The electronegativity difference between the atoms determine that whether the bond formed will be covalent or ionic.
Electronegativity of Hydrogen = 2.2.
Electronegativity of Chlorine = 3.1.
Electronegativity difference = 0.9.
Therefore, a polar covalent bond is formed, the shared paired of electrons are more towards the electronegative chlorine atom and it will get a partial negative charge and hydrogen being electropositive in nature get a partial negative charge.
(g)
Interpretation:
To analyze whether the given statement - These bonds are arranged in order of increasing polarity.
Concept Introduction:
If the atoms have same electronegativity or they are of same atom, then a non polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
The bonds are arranged in order of increasing polarity as follows:
Thus, the statement is true.
If the atoms have same electronegativity or they are of same atom, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
More the electronegativity difference, more polar is the bond. Since, the order of electronegativity is as follows:
Therefore, bonds in order of increasing polarity.
(h)
Interpretation:
To analyze whether the given statement- These bonds are arranged in order of increasing polarity.
Concept Introduction:
If the atoms have same electronegativity or they are of same atom, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
These bonds are arranged in order of increasing polarity.
Thus, the statement is false.
Electronegativity of hydrogen -2.2.
Electronegativity of Fluorine- 3.9.
Electronegativity of Chlorine-3.1.
Electronegativity of Bromine-2.9.
More the electronegativity difference, more polar is the bond.
Therefore, bonds in order of increasing polarity is as follows:
(i)
Interpretation:
To analyze whether the given statement, a polar bond has a dipole with the negative end located at the more electronegative atom., is true or not.
Concept Introduction:
If the atoms have same electronegativity or they are of same atom, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
A polar bond has a dipole with the negative end located at the more electronegative atom. Thus, the statement is true.
Electronegativity of Hydrogen = 2.2.
Electronegativity of Chlorine = 3.1.
Electronegativity difference = 0.9.
Therefore, a polar covalent bond is formed, and dipole is shown as follows:
A polar bond has a dipole with the negative end located at the more electronegative atom which is shown by the arrow.
(j)
Interpretation:
To analyze whether the given statement, in a single bond, two atoms share one pair of electrons; in a double bond, they share two pairs of electrons; and in a triple bond, they share three pair of electrons., is true or not.
Concept Introduction:
The octet rule states that atoms of various elements enter chemical combination so as to attain a configuration of eight electrons in their outermost shell. They do so by either transference of electrons or by mutual sharing of electrons.
In a single bond, two atoms share one pair of electrons; in a double bond, they share two pairs of electrons; and in a triple bond, they share three pair of electrons. Thus, the statement is true.
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
(k)
Interpretation:
To analyze whether the given statement- The Lewis structure for ethane,
Concept Introduction:
Lewis concept states that atoms of various elements enter chemical combination so as to attain the configuration of eight electrons in their outermost shell. They do so either by transference of electrons or by mutual sharing of electrons.
The Lewis structure for ethane,
From the structure of ethane.
Total single bonds= 7.
Non-bonding electrons left with carbon = 0.
Non-bonding electrons left with Hydrogen= 0.
Therefore, total electron counts in valence shell-
The Lewis structure for ethane,
(l)
Interpretation:
To analyze whether the given statement -
The Lewis structure for formaldehyde,
Concept Introduction:
Lewis concept states that atoms of various elements enter chemical combination so as to attain the configuration of eight electrons in their outermost shell. They do so either by transference of electrons or by mutual sharing of electrons.
The Lewis structure for formaldehyde,
From the structure of Formaldehyde-
Total single bonds= 2.
Total double bonds=1.
Non-bonding electrons left with carbon = 0.
Non-bonding electrons left with Hydrogen= 0.
Non-bonding electrons left with Oxygen= 4.
Therefore, total electron counts in valence shell-
(m)
Interpretation:
To analyze whether the given statement -
The Lewis structure for ammonium ion,
Concept Introduction:
Lewis concept states that atoms of various elements enter chemical combination so as to attain the configuration of eight electrons in their outermost shell. They do so either by transference of electrons or by mutual sharing of electrons.
The Lewis structure for ammonium ion,
From the structure of Ammonium ion-
Total single bonds= 4.
Total double bonds=0.
Charge =+1.
Non-bonding electrons left with Nitrogen = 1.
Non-bonding electrons left with Hydrogen= 0.
Therefore, total electron counts I valence shell-
(n)
Interpretation:
To analyze whether the given statement-Atoms of third-period elements can hold more than eight electrons in their valence shells, is true or not.
Concept Introduction:.
Atoms of third-period elements can hold more than eight electrons in their valence shells.
According to the Lewis model of bonding, atoms bond together in such a way that each atom participating in the bond acquires an outer-shell electron configuration matching that of the noble gas nearest to it in atomic number.
The electronic configuration of the elements is according to the distribution of the electrons in the shells of the atoms.
These shells are K, L, M, n and so on.
K can accommodate a maximum of 2 electrons.
L can accommodate a maximum of 8 electrons.
M can accommodate a maximum of 18 electrons.
N can accommodate a maximum of 32 electrons.
The element with electronic configuration 2 is Helium.
The element with electronic configuration 2,8 is Neon.
The element with electronic configuration 2,8,18 is Argon and so on.
Since, these configurations corresponds to noble gas configurations on attaining these configurations an atom of an element becomes stable.
Atoms of elements upto 2nd period have can have only 8 electrons in their valence shell due to the presence of only s and p orbitals, whereas atoms of higher periods have d, f orbitals also which can occupy more electrons.
Answer to Problem 3.55P
If the difference in electronegativity between two atoms is zero (they have identical electronegativities), then the two atoms will form a covalent bond. Thus, the statement is false.
Explanation of Solution
The electronegativity difference between the atoms determine that whether the bond formed will be covalent or ionic.
If the atoms have equal electronegativity value, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale, if exceeded, the bond becomes ionic in nature.
For example: For hydrogen gas: The electronegativity of both the hydrogen is 2.2, therefore a non-polar covalent bond is formed.
(c)
Interpretation:
To analyze whether the given statement- A covalent bond is formed by sharing two electrons is called a double bond, is true or not.
Concept Introduction:
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
Answer to Problem 3.55P
A covalent bond is formed by sharing two electrons is called a double bond. Thus, the statement is true.
Explanation of Solution
Atoms taking part in covalent bond formation may share one, two or three electron pairs thus, forming single, double and triple bond respectively.
An oxygen atom is formed when an atom of oxygen shares a pair of atoms each.
(d)
Interpretation:
To analyze whether the given statement - In the hydrogen molecule
Concept Introduction:
The octet rule states that atoms of various elements enter into chemical combination so as to attain a configuration of eight electrons in their outermost shell. They do so by either transference of electrons or by mutual sharing of electrons.
Answer to Problem 3.55P
In the hydrogen molecule
Explanation of Solution
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively. Hydrogen has only one electron in their valence shell, it shares it with another electron of the other Hydrogen atom to form a single covalent bond.
Sharing of 1 pair of electrons forms a single bond.
(e)
Interpretation:
To analyze whether the given statement in the molecule
Concept Introduction:
The octet rule states that atoms of various elements enter chemical combination so as to attain a configuration of eight electrons in their outermost shell. They do so by either transference of electrons or by mutual sharing of electrons. The logic of 8 electrons is that the noble gases have 8 electrons in their outermost shell and are stable. So, to attain stability noble gas configuration is acquired either by sharing, donating or accepting electrons.
Answer to Problem 3.55P
In the molecule
Explanation of Solution
The electronic configuration of the elements is according to the distribution of the electrons in the shells of the atoms.
These shells are K, L, M, n and so on.
K can accommodate a maximum of 2 electrons.
L can accommodate a maximum of 8 electrons.
M can accommodate a maximum of 18 electrons.
N can accommodate a maximum of 32 electrons.
The element with electronic configuration 2 is Helium, therefore each hydrogen attains electronic configuration of Helium.
The element with electronic configuration 2,8 is Neon, therefore each Carbon attains electronic configuration of Neon.
(f)
Interpretation:
To analyze whether the given statement, in a polar covalent bond, the more electronegative atom has a partial negative charge
Concept Introduction:
If the atoms have same electronegativity or they are of same atom, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
Answer to Problem 3.55P
In a polar covalent bond, the more electronegative atom has a partial negative charge
Explanation of Solution
The electronegativity difference between the atoms determine that whether the bond formed will be covalent or ionic.
Electronegativity of Hydrogen = 2.2.
Electronegativity of Chlorine = 3.1.
Electronegativity difference = 0.9.
Therefore, a polar covalent bond is formed, the shared paired of electrons are more towards the electronegative chlorine atom and it will get a partial negative charge and hydrogen being electropositive in nature get a partial negative charge.
(g)
Interpretation:
To analyze whether the given statement - These bonds are arranged in order of increasing polarity.
Concept Introduction:
If the atoms have same electronegativity or they are of same atom, then a non polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
Answer to Problem 3.55P
The bonds are arranged in order of increasing polarity as follows:
Thus, the statement is true.
Explanation of Solution
If the atoms have same electronegativity or they are of same atom, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
More the electronegativity difference, more polar is the bond. Since, the order of electronegativity is as follows:
Therefore, bonds in order of increasing polarity.
(h)
Interpretation:
To analyze whether the given statement- These bonds are arranged in order of increasing polarity.
Concept Introduction:
If the atoms have same electronegativity or they are of same atom, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
Answer to Problem 3.55P
These bonds are arranged in order of increasing polarity.
Thus, the statement is false.
Explanation of Solution
Electronegativity of hydrogen -2.2.
Electronegativity of Fluorine- 3.9.
Electronegativity of Chlorine-3.1.
Electronegativity of Bromine-2.9.
More the electronegativity difference, more polar is the bond.
Therefore, bonds in order of increasing polarity is as follows:
(i)
Interpretation:
To analyze whether the given statement, a polar bond has a dipole with the negative end located at the more electronegative atom., is true or not.
Concept Introduction:
If the atoms have same electronegativity or they are of same atom, then a non-polar covalent bond is formed.
But if there is an electronegativity difference between the atoms forming a bond, the bond formed is a polar bond. This difference should not exceed 1.9 on Pauling scale.
Answer to Problem 3.55P
A polar bond has a dipole with the negative end located at the more electronegative atom. Thus, the statement is true.
Explanation of Solution
Electronegativity of Hydrogen = 2.2.
Electronegativity of Chlorine = 3.1.
Electronegativity difference = 0.9.
Therefore, a polar covalent bond is formed, and dipole is shown as follows:
A polar bond has a dipole with the negative end located at the more electronegative atom which is shown by the arrow.
(j)
Interpretation:
To analyze whether the given statement, in a single bond, two atoms share one pair of electrons; in a double bond, they share two pairs of electrons; and in a triple bond, they share three pair of electrons., is true or not.
Concept Introduction:
The octet rule states that atoms of various elements enter chemical combination so as to attain a configuration of eight electrons in their outermost shell. They do so by either transference of electrons or by mutual sharing of electrons.
Answer to Problem 3.55P
In a single bond, two atoms share one pair of electrons; in a double bond, they share two pairs of electrons; and in a triple bond, they share three pair of electrons. Thus, the statement is true.
Explanation of Solution
A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.
(k)
Interpretation:
To analyze whether the given statement- The Lewis structure for ethane,
Concept Introduction:
Lewis concept states that atoms of various elements enter chemical combination so as to attain the configuration of eight electrons in their outermost shell. They do so either by transference of electrons or by mutual sharing of electrons.
Answer to Problem 3.55P
The Lewis structure for ethane,
Explanation of Solution
From the structure of ethane.
Total single bonds= 7.
Non-bonding electrons left with carbon = 0.
Non-bonding electrons left with Hydrogen= 0.
Therefore, total electron counts in valence shell-
The Lewis structure for ethane,
(l)
Interpretation:
To analyze whether the given statement -
The Lewis structure for formaldehyde,
Concept Introduction:
Lewis concept states that atoms of various elements enter chemical combination so as to attain the configuration of eight electrons in their outermost shell. They do so either by transference of electrons or by mutual sharing of electrons.
Answer to Problem 3.55P
The Lewis structure for formaldehyde,
Explanation of Solution
From the structure of Formaldehyde-
Total single bonds= 2.
Total double bonds=1.
Non-bonding electrons left with carbon = 0.
Non-bonding electrons left with Hydrogen= 0.
Non-bonding electrons left with Oxygen= 4.
Therefore, total electron counts in valence shell-
(m)
Interpretation:
To analyze whether the given statement -
The Lewis structure for ammonium ion,
Concept Introduction:
Lewis concept states that atoms of various elements enter chemical combination so as to attain the configuration of eight electrons in their outermost shell. They do so either by transference of electrons or by mutual sharing of electrons.
Answer to Problem 3.55P
The Lewis structure for ammonium ion,
Explanation of Solution
From the structure of Ammonium ion-
Total single bonds= 4.
Total double bonds=0.
Charge =+1.
Non-bonding electrons left with Nitrogen = 1.
Non-bonding electrons left with Hydrogen= 0.
Therefore, total electron counts I valence shell-
(n)
Interpretation:
To analyze whether the given statement-Atoms of third-period elements can hold more than eight electrons in their valence shells, is true or not.
Concept Introduction:.
Answer to Problem 3.55P
Atoms of third-period elements can hold more than eight electrons in their valence shells.
Explanation of Solution
The electronic configuration of the elements is according to the distribution of the electrons in the shells of the atoms.
These shells are K, L, M, n and so on.
K can accommodate a maximum of 2 electrons.
L can accommodate a maximum of 8 electrons.
M can accommodate a maximum of 18 electrons.
N can accommodate a maximum of 32 electrons.
The element with electronic configuration 2 is Helium.
The element with electronic configuration 2,8 is Neon.
The element with electronic configuration 2,8,18 is Argon and so on.
Since, these configurations corresponds to noble gas configurations on attaining these configurations an atom of an element becomes stable.
Atoms of elements upto 2nd period have can have only 8 electrons in their valence shell due to the presence of only s and p orbitals, whereas atoms of higher periods have d, f orbitals also which can occupy more electrons.
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Chapter 3 Solutions
INTRO.TO GEN.,ORG.,+BIO.-HYBRID ED PKG.
- 3-41 Describe the structure of sodium chloride in the solid state.arrow_forward3-58 In Section 2-3B, we saw that there are seven diatomic elements. (a) Draw Lewis structures for each of these diatomic elements. (b) Which diatomic elements are gases at room temperature? Which are liquids? Which are solids?arrow_forward3-26 Table 3-2 shows the following ions of copper: Cu+ and Cu2+. Do these violate the octet rule? Explain.arrow_forward
- 3-106 Consider the structure of Penicillin G shown below, an antibiotic used to treat bacterial infections caused by gram-positive organisms, derived from Penicillium fungi: (a) Identify the various types of geometries present in each central atom using VSEPR theory. (b) Determine the various relative bond angles associated with each central atom using VSEPR theory (c) Which is the most poiar bond in Penicillin G? (d) Would you predict Penicillin G to be polar or nonpolar?arrow_forward3-31 Why does electronegativity generally increase going from left to right across a row of the Periodic Table?arrow_forward3-25 Why are carbon and silicon reluctant to form ionic bonds?arrow_forward
- 3-67 Why does nitrogen have three bonds and one unshared pair of electrons in covalent compounds?arrow_forward3-57 What is: (a) A single bond? (b) A double bond? (c) A triple bond?arrow_forward3-68 Draw a Lewis structure of a covalent compound in which nitrogen has: (a) Three single bonds and one unshared pair of electrons (b) One single bond, one double bond, and one unshared pair of electrons (c) One triple bond and one unshared pair of electronsarrow_forward
- 3-87 Consider the molecule boron trffluoride, BF3. (a) Write a Lewis structure for BF3. (b) Predict the FBF bond angles using the VSEPR model. (c) Does BF3 have polar bonds? Is it a polar molecule?arrow_forward3-70 Draw a Lewis structure of a covalent compound in which oxygen has: (a) Two single bonds and two unshared pairs of electrons (b) One double bond and two unshared pairs of electronsarrow_forward3-105 Consider the structure of Vitamin E shown below, which is found most abundantly in wheat germ oil, sunflower, and safflower oils: (a) Identify the various types of geometries present in each central atom using VSEPR theory. (b) Determine the various relative bond angles as sociated with each central atom using VSEPR theory. (c) Which is the most polar bond in Vitamin E? (d) Would you predict Vitamin E to be polar or nonpolar?arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning