As you go across the elements in a period, each element has an increased effective nuclear charge, or Z eff attracting its outer shell electrons.Electrostatic theory explains the trend in electronegativity in the Periodic Table, in the Periodic Table both across a period and down a group:.It is measured using the Pauling scale fluorine is highest at 4.0 on the scale, the most electronegative element, whilst francium is the lowest at 0.7 and is the least electronegative element. Electronegativity is the ability of an atom (specifically the nucleus) to attract bonding electrons to its outer electron shell.#4: Repulsive forces between like-charged particles decrease with distance.#3: Attractive forces between oppositely charge particles decrease with distance.#2: The greater the charge difference of two particles, the greater their force of attraction (for example, the attractive force between a 2 + ion and a 2 - ion is stronger than the attractive force between a 1 + and a 1 - ion).#1: Oppositely charged particles attract each other, while particles of like charge repel each other.As seen in Periodic trends: Atomic radius, chemists have found, through experimenting, some principles of electrostatic forces forces that exist because charged particles attract or repel each other. How metallic and acid-base properties change across a period.To predict the electronegativity of elements compared to each other.To apply our understanding of electrostatic principles to the periodic trends in electronegativity.The definition of electronegativity and how it is measured.
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