Draw Lewis structures for each of the following molecules....

Draw Lewis structures for each of the following molecules. (Hint: See Sample Problem D.) a. contains one $\mathrm{C}$ and four $\mathrm{F}$ atoms b. contains two$\mathrm{H}$ and one $\mathrm{Se}$ atom c. contains one $\mathrm{N}$ and three $\mathrm{I}$ atoms d. contains one $\mathrm{Si}$ and four $\mathrm{Br}$ atoms e. contains one $\mathrm{C},$ one $\mathrm{C} 1,$ and three $\mathrm{H}$ atoms

Draw Lewis structures for each of the following molecules. (Hint: See Sample Problem D.)
a. contains one $\mathrm{C}$ and four $\mathrm{F}$ atoms
b. contains two$\mathrm{H}$ and one $\mathrm{Se}$ atom
c. contains one $\mathrm{N}$ and three $\mathrm{I}$ atoms
d. contains one $\mathrm{Si}$ and four $\mathrm{Br}$ atoms
e. contains one $\mathrm{C},$ one $\mathrm{C} 1,$ and three $\mathrm{H}$ atoms

Key Concepts

Formal Charge

Formal charge is a bookkeeping tool used in Lewis structures to determine the most stable arrangement of electrons among atoms. By calculating the formal charge on each atom, one can assess which resonance structure is most appropriate, ensuring that the overall charge distribution is minimized and the structure is as stable as possible.

Octet Rule

The octet rule states that atoms tend to form bonds until they are surrounded by eight valence electrons, achieving a stable electronic configuration similar to a noble gas. This rule guides the placement of electrons in Lewis structures and helps in predicting the most stable structure for a given molecule.

Covalent Bonding

Covalent bonding involves the sharing of electron pairs between atoms, allowing each atom to achieve a full valence shell. When drawing Lewis structures, recognizing the formation of single, double, or triple bonds is important to correctly represent how electrons are shared between the atoms.

Lewis Structures

Lewis structures are diagrams that represent the distribution of valence electrons among the atoms in a molecule. They are used to visualize the arrangement of atoms, bonding between atoms, and any lone pairs of electrons. This concept is essential in understanding molecular structure and predicting reactivity and properties.

Valence Electrons

Valence electrons are the electrons in the outermost shell of an atom that partake in chemical bonding. Knowing the number of valence electrons for each atom is crucial for constructing Lewis structures because it determines the number of bonds that can be formed and how electrons are distributed among the atoms in a molecule.

Transcript

00:01 In this video, i will be showing how to draw basic lewis structures with covalent bonds.

00:07 The first example we have is a lewis structure with one carbon atom and four fluorine atoms.

00:15 So first we can start by drawing out each individual atom with its valence electrons.

00:22 So we know that carbon has four valence electrons and fluorine has seven.

00:29 So we know that a covalent bond is forming between these two atoms, meaning that they will share their electrons.

00:41 So in order for their octets to be fulfilled, carbon needs to share four more electrons in these positions, and fluorine needs to share one more electron in this position.

00:57 So we can see that a bond will form between two atoms in these areas where the electrons need to be shared.

01:06 And since we have four fluorine atoms, they will each go to one of these positions.

01:18 So when that happens, the bonds will form between the atoms leaving us with this overall structure.

01:31 And fluorines would have three loan pairs each.

01:42 Our second example is a structure with two hydrogen atoms and one selenium atom.

01:54 So hydrogen has one valence electron and selenium has six.

02:03 So for their octets to be fulfilled, the additional electrons need to be shared in these positions.

02:12 So we know the bond will form between areas where the electrons need to be shared and since we have two hydrogens, they will each go to one of these positions on selenium.

02:28 So our overall structure will have two bonds between hydrogen and selenium with two lone pairs on selenium...

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