0
What else can I help you with?
What is the most optimal Lewis structure for the cyanate ion, NCO- , based on formal charge?
The most optimal Lewis structure for the cyanate ion, NCO-, based on formal charge, is where the nitrogen atom has a formal charge of 1, the carbon atom has a formal charge of 0, and the oxygen atom has a formal charge of -1.
Lewis Structure of CS32-?
The Lewis structure of CS3^2- consists of a carbon atom bonded to three sulfur atoms. The carbon atom has a formal negative charge, and each sulfur atom has a formal negative charge to balance the charge of the ion. The carbon atom and sulfur atoms are connected by single bonds.
Is carbonate an anion or cation?
no ion can be form
What is the formal charge of the nitrogen atom in NCl3?
The formal charge of the nitrogen atom in NCl3 is 0.
What is the Lewis structure of sodium carbonate?
The Lewis structure of sodium carbonate (Na2CO3) consists of one sodium (Na) atom, one carbon (C) atom, and three oxygen (O) atoms arranged such that each oxygen is connected to the carbon. The sodium atoms are connected to the oxygens, completing the structure. Sodium has a +1 charge, while carbonate (CO3) has a -2 charge.
What formal charge does carbon have?
The formal charge on the carbon atom of carbon monoxide in its major resonance form (triple bonded with oxygen) is -1. However, the electronegativity difference cancels it out for the most part (oxygen in this case as a formal charge of +1). It would be more accurate to say that there is simply a small dipole moment between the two molecules with the negative end on carbon.
Is Carbonate a cation?
No carbonate has a negative charge so it is an anion.
What is the most optimal Lewis structure for the cyanate ion, NCO- , based on formal charge?
The most optimal Lewis structure for the cyanate ion, NCO-, based on formal charge, is where the nitrogen atom has a formal charge of 1, the carbon atom has a formal charge of 0, and the oxygen atom has a formal charge of -1.
What is the oxidation number for carbonate and barium?
The oxidation number for carbonate is -2, as it is composed of one carbon atom with a formal charge of +4 and three oxygen atoms each with a formal charge of -2. The oxidation number for barium is +2, as it is a group 2 element in the periodic table, meaning it typically forms 2+ cations.
What is the charge of a carbonate ion?
The charge of a carbonate ion (CO3^2-) is -2. It consists of one carbon atom and three oxygen atoms, giving it a total of 4+ charge carried by the carbon atom and 6- charge carried by the three oxygen atoms.
Lewis Structure of CS32-?
The Lewis structure of CS3^2- consists of a carbon atom bonded to three sulfur atoms. The carbon atom has a formal negative charge, and each sulfur atom has a formal negative charge to balance the charge of the ion. The carbon atom and sulfur atoms are connected by single bonds.
Is carbonate an anion or cation?
no ion can be form
What is the formal charge of c3h8?
To calculate the formal charge of a molecule like C3H8, we first need to determine the number of valence electrons each element brings. Carbon brings 4, and hydrogen brings 1. Then, we must assign the electrons to the atoms based on the molecular structure to determine the formal charge. For C3H8, each carbon atom will have a formal charge of 0, and each hydrogen atom will have a formal charge of +1.
What is the formal charge of the nitrogen atom in NCl3?
The formal charge of the nitrogen atom in NCl3 is 0.
What is the Lewis structure of sodium carbonate?
The Lewis structure of sodium carbonate (Na2CO3) consists of one sodium (Na) atom, one carbon (C) atom, and three oxygen (O) atoms arranged such that each oxygen is connected to the carbon. The sodium atoms are connected to the oxygens, completing the structure. Sodium has a +1 charge, while carbonate (CO3) has a -2 charge.
Is carbonate a polyatomic ion?
The covalent bond is like a molecule and the charge is like an ion.
What is the formal charge of the central atom in BeCl2?
The formal charge of the central beryllium atom in BeCl2 is zero.
