40 Questions
How many covalent bonds does carbon typically form to achieve an octet of valence electrons?
Four
What is the purpose of sharing electrons through covalent bonding for elements like nitrogen, oxygen, and the halogens?
To achieve an octet of valence electrons
What is the typical number of covalent bonds formed by nitrogen through sharing its valence electrons?
Three
How many valence electrons do hydrogen and helium have in common?
Two
What is the purpose of the octet rule in covalent bonding?
To achieve an octet of valence electrons
What is the typical number of valence electrons left unshared as electron pairs for oxygen?
Two
How many nonbonding pairs of electrons are assigned to the fluorine atom in the Lewis structure of CH3F?
Three
What is the total number of valence electrons represented by the bonding pairs in the Lewis structure of CH3F?
8
What is the main difference between dash structural formulas and condensed structural formulas?
Dash structural formulas show bonding electron pairs, while condensed structural formulas show hydrogen atoms attached to carbon.
What is the purpose of writing resonance structures?
To describe molecules and ions for which a single Lewis structure is inadequate.
What is a characteristic of resonance structures?
They exist only on paper and are used to describe molecules and ions.
What is the rule for writing resonance structures?
The positions of the nuclei of the atoms must remain the same in all of the structures.
What is the symbol used to connect resonance structures?
←→
What is the advantage of using condensed structural formulas?
They can be written in multiple ways for the same molecule.
What is a characteristic of condensed structural formulas?
Hydrogen atoms are written immediately after the carbon they are attached to.
Why are resonance structures drawn?
To describe the bonding in molecules and ions for which a single Lewis structure is inadequate.
What is the first step in writing a Lewis structure for a molecule?
Find the total number of valence electrons on all of the atoms.
What is the purpose of using unshared electron pairs in a Lewis structure?
To fill the valence shell of an atom.
What is the total number of valence electrons used so far in the given example?
6 valence electrons
Which of the following statements is true about the valence shells of the atoms in the given example?
The valence shell is full only for the hydrogen atoms.
What is the purpose of the octet rule in writing Lewis structures?
To ensure that each atom has a full valence shell.
How many electrons are left to use after forming the bonds between the hydrogen atom and the carbon atom, and the carbon atom and the nitrogen atom?
4 electrons
What is the electronic structure of the hydrogen atom in the Lewis structure of hydrogen cyanide (HCN)?
Like helium with 2 electrons.
What is the bond between the carbon atom and the nitrogen atom in the Lewis structure of hydrogen cyanide (HCN)?
Triple bond
What is the formal charge of an atom in a molecule calculated as?
Number of valence electrons - 1/2 number of shared electrons - number of unshared electrons
What is the arithmetic sum of all the formal charges in a molecule or ion equal to?
The overall charge on the molecule or ion
What is the symbol used to represent the formal charge?
F
What does the number of unshared electrons represent in the formal charge equation?
The number of electrons not shared with other atoms
What is the purpose of calculating formal charges?
To keep track of the electrons in a molecule
What is the relationship between the number of shared electrons and the formal charge?
The number of shared electrons is inversely proportional to the formal charge
What is the purpose of the equation F = Z - (1/2)S - U?
To calculate the formal charge
What does the symbol Z represent in the formal charge equation?
The group number of the element
What is the first step in writing a Lewis structure for a molecule?
Find the total number of valence electrons for all the atoms
What is the purpose of using multiple bonds in Lewis structures?
To satisfy the octet rule and give atoms a noble gas configuration
How many electron pairs are used to form single bonds between the carbon and hydrogen atoms in the Lewis structure of methylamine (CH3NH2)?
Three pairs
What is the final step in writing the Lewis structure of methylamine (CH3NH2)?
Use the remaining electron pair as a lone pair on the nitrogen atom
How many valence electrons are used to form single bonds between the nitrogen atom and hydrogen atoms in the Lewis structure of methylamine (CH3NH2)?
Two pairs
What is the purpose of finding the total number of valence electrons in a molecule?
To determine the total number of electron pairs available for bonding
In writing the Lewis structure of a molecule, what should be done if necessary?
Use multiple bonds to satisfy the octet rule
What is the correct order of steps in writing a Lewis structure?
Find the total number of valence electrons, use pairs to form single bonds, use multiple bonds to satisfy the octet rule
Study Notes
How to Write and Interpret Structural Formulas
- Dash structural formulas show bonding electron pairs and include elemental symbols for all atoms in a molecule.
- Condensed structural formulas write all hydrogen atoms attached to a particular carbon immediately after the carbon.
- The condensed formula for isopropyl alcohol can be written in four different ways.
Rules for Writing Resonance Structures
- Resonance structures exist only on paper and are used to describe molecules and ions for which a single Lewis structure is inadequate.
- Resonance structures are connected by double-headed arrows (←→) and the real molecule or ion is a hybrid of all of them.
- Only electrons can be moved in writing resonance structures, not the positions of the nuclei of the atoms.
- Hydrogen forms one covalent bond by sharing its electron with an electron of another atom.
- Carbon forms four covalent bonds by sharing its four valence electrons with four valence electrons from other atoms.
- Nitrogen, oxygen, and the halogens typically share only some of their valence electrons through covalent bonding, leaving others as unshared electron pairs.
Writing Lewis Structures
- To write a Lewis structure, find the total number of valence electrons of all the atoms.
- Use pairs of electrons to form bonds between all atoms that are bonded to each other.
- Add the remaining electrons in pairs to give each hydrogen 2 electrons (a duet) and every other atom 8 electrons (an octet).
Exercises
- Write a Lewis structure for CH3F:
- Find the total number of valence electrons of all the atoms.
- Use pairs of electrons to form bonds between all atoms that are bonded to each other.
- Add the remaining electrons in pairs to give each hydrogen 2 electrons and every other atom 8 electrons.
- Write a Lewis structure for methylamine (CH3NH2):
- Find the total number of valence electrons for all the atoms.
- Use one electron pair to join the carbon and nitrogen.
- Use three pairs to form single bonds between the carbon and three hydrogen atoms.
- Use two pairs to form single bonds between the nitrogen atom and two hydrogen atoms.
- Leave one electron pair as a lone pair on the nitrogen atom.
- Write a Lewis structure for CH3OH:
- Use multiple bonds to satisfy the octet rule (i.e., give atoms the noble gas configuration).
- Write a Lewis structure for CH2O (formaldehyde):
- Find the total number of valence electrons of all the atoms.
- Use pairs of electrons to form single bonds.
- Determine which atoms already have a full valence shell and which ones do not.
- Use the remaining electrons as bonds or unshared electron pairs to fill the valence shell of any atoms whose valence shell is not yet full.
Formal Charges
- The formal charge is the number of valence electrons minus 1/2 the number of shared electrons minus the number of unshared electrons.
- The arithmetic sum of all the formal charges in a molecule or ion will equal the overall charge on the molecule or ion.
- Calculate the formal charge using the formula: F = Z - (1/2)S - U.
- Exercises:
- Calculate the formal charge of the ammonium ion.
- Calculate the formal charge of the nitrate ion.
- Calculate the formal charge of water.
- Calculate the formal charge of ammonia.
A Summary of Formal Charges
- Formal charges are used to determine the overall charge of a molecule or ion.
- The formal charge is calculated using the formula: F = Z - (1/2)S - U.
Learn about structural formulas in molecular and cellular medical sciences. Understand how to write and interpret dash structural formulas, including bonding electron pairs and elemental symbols.
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