Lewis structure PBr3

AlCl3.Structure 2 can be classified as both a Brønsted–Lowry and a Lewis base. Explanation: Let us recall that a Lewis acid is a lone pair acceptor while a Lewis base is a lone pair donors. A Brownstead-Lowry acid is a proton donor while a Brownstead-Lowry base is a lone pair acceptor. NH3 functions as a Lewis base because it can donate it’s lone pairs in coordinate covalent bonding. It can also accept a proton thereby acting as a Brownstead-Lowry base in the formation of the NH4+ ion.

Each oxygen atom is connected to the central O atom with 2 covalent bonds.
Explanation:
Oxygen atoms are connected by two covalent bonds in the oxygen molecule from the Lewis structure, we see that the bond order for O2 is 2 (a double bond) this is clearly seen in the image attached. There are no resonance structures for the oxygen molecule since there are no partial bonds in the molecule, only the two covalent bonds present.
This structure of oxygen shown in the image is its only structure, showing the covalent bonds formed and other non bonding electrons present in the molecule. The octet rule is followed in drawing the structure. Each oxygen atom possesses an octet of electrons on its outermost shell.

Another explanation A Lewis structure is also called a dot electron structure. A Lewis structure represents all the valence electrons on atoms in a molecule as dots. Lewis structures can be used to represent molecules in which the central atom obeys the octet rule as well as molecules whose central atom does not obey the octet rule.
Sometimes, one Lewis structure does not suffice in explaining the observed properties of a given chemical specie. In this case, we evoke the idea that the actual structure of the chemical specie lies somewhere between a limited number of bonding extremes called resonance or canonical structures.
The canonical structure of the carbonate ion as well as the lewis structure of phosphine is shown in the image attached to this answer. Explanation:

Each oxygen atom is connected to the central O atom with 2 covalent bonds. Explanation: Oxygen atoms are connected by two covalent bonds in the oxygen molecule from the Lewis structure, we see that the bond order for O2 is 2 (a double bond) this is clearly seen in the image attached. There are no resonance structures for the oxygen molecule since there are no partial bonds in the molecule, only the two covalent bonds present. This structure of oxygen shown in the image is its only structure, showing the covalent bonds formed and other non bonding electrons present in the molecule. The octet rule is followed in drawing the structure. Each oxygen atom possesses an octet of electrons on its outermost shell.

here is the answer! Explanation: Lewis Structure is a very simplified representation of the valence shell electrons in a molecule. It is used to show how the electrons are arranged around individual atoms in a molecule. Electrons are shown as “dots” or for bonding electrons as a line between the two atoms. The goal is to obtain the “best” electron configuration. the octet rule and formal charges need to be satisfied. 1)First determine the total number of valence electrons in the molecule. This will be the sum of the group number a of all atoms plus the charge. 2)Draw a skeletal structure for the molecule which connects all atoms using only single bonds. The central atom will be the one that can form the greatest number of bonds and/or expand its octet. This usually means the atom lower and/or to the right in the Periodic Table 3)Now we need to add lone pairs of electrons. Of the 24 valence electrons available in NO3-, 6 were used to make the skeletal structure. Add lone pairs of electrons on the terminal atoms until their octet is complete or you run out of electrons.
4)If there are remaining electrons they can be used to complete the octet of the central atom. If you have run out of electrons you are required to use lone pairs of electrons from a terminal atom to complete the octet on the central atom by forming multiple bond(s). In this case the N is short 2 electrons so we can use a lone pair from the left most O atom to form a double bond and complete the octet on the N atom.
5) Now you need to determine the FORMAL CHARGES for all of the atoms. The formal charge is calculated by: (group number of atom) – (½ number of bonding electrons) – (number of lone pair electrons)

I didn’t understand sorry

Answer 6

See explanation Explanation: A Lewis structure is also called a dot electron structure. A Lewis structure represents all the valence electrons on atoms in a molecule as dots. Lewis structures can be used to represent molecules in which the central atom obeys the octet rule as well as molecules whose central atom does not obey the octet rule. Sometimes, one Lewis structure does not suffice in explaining the observed properties of a given chemical specie. In this case, we evoke the idea that the actual structure of the chemical specie lies somewhere between a limited number of bonding extremes called resonance or canonical structures. The canonical structure of the carbonate ion as well as the lewis structure of phosphine is shown in the image attached to this answer.

Answer 7

You have to give all atoms their right charge

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