The higher the electronegativity of a metal the less likely it is to corrode. Metals that corrode easily have a low electronegativity.
Water
Electronegativity decreases across a period because the effective nuclear charge increases. This causes the attraction between the electrons and the nucleus to become stronger, making it harder for atoms to attract additional electrons and thus reducing electronegativity.
Pauling electronegativity 2.33 Sanderson electronegativity 2.29 Allred Rochow electronegativity 1.55 Mulliken-Jaffe electronegativity 2.41 (sp3 orbital) Allen electronegativity no data
You think probable to electronegativity.
It is a polar covalent bond. I was looking for this answer for chem hw and found just after coming to this page :P
Yes, the effective nuclear charge is directly related to electronegativity. Electronegativity increases as the effective nuclear charge on an atom increases.
When electronegativity decrease the first ionization energy also decrease.
Electronegativity and first ionization energy both increase going up the Periodic Table.
Electron affinity is related to the formation of anions; electronegativity is related to the formation of cations.
Water
Examples: chemical reactivity, flammability, electronegativity, polarization of a molecule, resistance to corrosion, solubility, iodine index, pH, etc.
No, the color of an element does not determine its electronegativity. Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond, which is determined by the atom's size, nuclear charge, and electron configuration. Color is a property of an element when it is in a specific form or compound and is not directly related to electronegativity.
Refer to the related link for a periodic table listing the electronegativities of the elements.
Examples: resistance to corrosion, valence, Pauling electronegativity.
Electronegativity is the ability of an atom to attract shared electrons in a covalent bond. The greater the electronegativity difference between two atoms, the more polar the covalent bond will be. In nonpolar covalent bonds, atoms have similar electronegativities, resulting in equal sharing of electrons.
Electronegativity decreases across a period because the effective nuclear charge increases. This causes the attraction between the electrons and the nucleus to become stronger, making it harder for atoms to attract additional electrons and thus reducing electronegativity.
Pauling electronegativity 2.33 Sanderson electronegativity 2.29 Allred Rochow electronegativity 1.55 Mulliken-Jaffe electronegativity 2.41 (sp3 orbital) Allen electronegativity no data