Single line.
The Lewis structure of CHBr3 can be drawn with carbon as the central atom bonded to three hydrogen atoms and one bromine atom. The carbon-bromine bond is represented by a single bond with three lone pairs on bromine, making the bromine atom negatively charged.
A single covalent bond between atoms can be represented using a single line (-) in a Lewis structure or a structural formula. For example, in the molecule H2O, the single bond between one hydrogen atom and the oxygen atom can be depicted as H-O-H.
In the Lewis dot structure for a fluorine atom, there should be 1 bond displayed, as fluorine has 1 unpaired electron that can form a single bond with another atom.
The correct Lewis dot structure for H2 has two hydrogen atoms sharing a single pair of electrons between them, represented by a single bond. Each hydrogen atom contributes one electron to the bond, leading to a stable diatomic molecule.
The Lewis structure of HOCl shows oxygen bonded to hydrogen and chlorine, with oxygen having two lone pairs of electrons and forming a single bond with hydrogen and a single bond with chlorine.
The Lewis structure of CHBr3 can be drawn with carbon as the central atom bonded to three hydrogen atoms and one bromine atom. The carbon-bromine bond is represented by a single bond with three lone pairs on bromine, making the bromine atom negatively charged.
A single covalent bond between atoms can be represented using a single line (-) in a Lewis structure or a structural formula. For example, in the molecule H2O, the single bond between one hydrogen atom and the oxygen atom can be depicted as H-O-H.
In the Lewis dot structure for a fluorine atom, there should be 1 bond displayed, as fluorine has 1 unpaired electron that can form a single bond with another atom.
The Lewis structure of CH2F2 is represented as H-C-H with a double bond to C and a single bond to F on each side of the C atom. This arrangement allows each atom to have a full valence shell and minimizes formal charges.
Three bonds should be drawn in the Lewis dot structure for SO3. Sulfur forms a double bond with one oxygen atom and single bonds with the other two oxygen atoms to complete its octet.
The Lewis dot structure for hydrogen bromide (HBr) consists of a single covalent bond between the hydrogen atom and the bromine atom. So, there is one single covalent bond in the Lewis dot structure of HBr.
In the Lewis dot structure for BH3, there should be 3 bonds drawn. Each hydrogen atom forms a single covalent bond with the boron atom. Boron has three valence electrons, so it can form three bonds with the hydrogen atoms.
The correct Lewis dot structure for H2 has two hydrogen atoms sharing a single pair of electrons between them, represented by a single bond. Each hydrogen atom contributes one electron to the bond, leading to a stable diatomic molecule.
The Lewis structure of HOCl shows oxygen bonded to hydrogen and chlorine, with oxygen having two lone pairs of electrons and forming a single bond with hydrogen and a single bond with chlorine.
The electron dot formula or Lewis structure for hydrogen gas (H2) consists of two hydrogen atoms sharing a pair of electrons between them. Each hydrogen atom contributes one electron to the shared pair, forming a single covalent bond. The structure is represented as H:H or H-H, with a single bond between the hydrogen atoms.
The Lewis structure for CH2CHCH3 (propene) includes one carbon-carbon double bond and one carbon-carbon single bond. Each carbon atom is surrounded by four total bonds (either C-H or C-C). The structure can be represented as H3C-CH=CH2.
Resonance structures demonstrate one of the weaknesses of the Lewis structure. Molecules represented by a the Lewis structure either have single bonds, double bonds, or triple bonds. The multiple bonds can sometimes be drawn in more than one place. In reality, the multiple bond is averaged out over the molecule, so that all of the atoms may have a 1 1/2 bond or a 1 1/3 bond rather than a single or a double bond.