Electronegativity Quiz

Oxygen is the more electronegative element compared to carbon. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Oxygen has a higher electronegativity value than carbon because it has a greater ability to attract electrons due to its higher effective nuclear charge and smaller atomic size. This means that oxygen has a stronger pull on shared electrons in a chemical bond, making it more electronegative than carbon.

The e-neg difference between carbon and oxygen is 1. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Oxygen has a higher electronegativity value than carbon, indicating that it has a greater ability to attract electrons. The electronegativity difference between carbon and oxygen is therefore 1.

Carbon has a higher electronegativity than silicon. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Carbon has a higher electronegativity because it has a smaller atomic radius and a higher effective nuclear charge compared to silicon. These factors result in a stronger attraction for electrons in carbon, making it more electronegative than silicon.

The bond that forms between oxygen and carbon is covalent because both elements have similar electronegativities. In a covalent bond, the electrons are shared between the atoms, resulting in a stable molecule. Ionic bonds, on the other hand, occur between elements with significantly different electronegativities, leading to the transfer of electrons from one atom to another. Since oxygen and carbon have similar electronegativities, they share electrons and form a covalent bond.

The bond that forms between radium and bromine is ionic because radium is a metal and bromine is a nonmetal. In ionic bonding, one atom donates electrons to another atom, resulting in the formation of positive and negative ions that are attracted to each other. Radium, as a metal, tends to lose electrons and form a positive ion, while bromine, as a nonmetal, tends to gain electrons and form a negative ion. This electrostatic attraction between the oppositely charged ions leads to the formation of an ionic bond.

Radium is more likely to give up an electron because it is an alkali metal located in Group 2 of the periodic table. Alkali metals have a tendency to lose electrons and become positively charged ions. Radium has a low ionization energy, which means it requires less energy to remove an electron from its outermost shell compared to other elements. This makes it more likely for radium to give up an electron and form a positive ion.