Which type of bond and how many bonds would occur as carbon dioxide (CO2) is formed from carbon in Group IVA and oxygen in Group VIA?(1 point)Responsesone covalent bondone covalent bondthree metallic bondsthree metallic bondstwo ionic bondstwo ionic bondsfour covalent bondsfour covalent bonds
Carbon dioxide (CO2) is formed through the sharing of electrons between carbon and oxygen atoms. This type of bond is known as a covalent bond. Since there are two oxygen atoms in CO2, there would be a total of four covalent bonds in carbon dioxide. Therefore, the correct answer is four covalent bonds.
To determine the type and number of bonds formed when carbon dioxide (CO2) is formed, we need to consider the electron configurations of carbon and oxygen.
Carbon in Group IVA has 4 valence electrons, while oxygen in Group VIA has 6 valence electrons.
Both carbon and oxygen need 8 electrons in their outermost energy level to achieve a stable configuration.
Carbon can achieve a stable configuration by sharing electrons with two oxygen atoms, forming two covalent bonds. Each covalent bond involves the sharing of 2 electrons.
Therefore, when carbon dioxide (CO2) is formed, it involves two covalent bonds.
To determine the type of bond and the number of bonds in carbon dioxide (CO2), we need to consider the valence electron configuration of carbon (Group IVA) and oxygen (Group VIA) in the periodic table.
Carbon, in Group IVA, has four valence electrons, and oxygen, in Group VIA, has six valence electrons. Both carbon and oxygen tend to follow the octet rule, which means they want to have eight electrons in their outermost energy level for stability.
Since carbon needs four more electrons to complete its octet, and oxygen needs two more electrons to complete its octet, they will share electrons in a covalent bond.
In the case of carbon dioxide, each oxygen atom will share two electrons with the carbon atom. This leads to a double bond between the carbon atom and each oxygen atom.
Therefore, the correct answer is: two covalent bonds.