What is the underlying cause of periodic trends? Trends in atomic size, ionization energy, ionic size, and electronegativity can be explained by variations in atomic structure. The increase in nuclear charge within groups and across periods explains many trends.
Elements of the periodic table are arranged in order of increasing atomic number. The periodic law states “When elements are arranged in order of increasing atomic number, there is a periodic repetition of their chemical and physical properties.”
The Periodic Law states that the physical and chemical properties of the elements recur in a systematic and predictable way when the elements are arranged in order of increasing atomic number.
Mendeleev went even further. He corrected the known atomic masses of some elements and he used the patterns in his table to predict the properties of the elements he thought must exist but had yet to be discovered. The accuracy of those predictions led to the periodic table’s acceptance. Timeline of Mendeleev’s life.
Ionic size increases from top to bottom down a group of elements in the periodic table. From left to right across a period, the ionic size decreases as long as you are comparing all metals or all nonmetals. Between the metals and nonmetals, the ionic size increases as you switch from cations to anions.
|Atomic number (Z)||13|
|Group||group 13 (boron group)|
1) The periodic law states that similar properties recur periodically when elements are arranged according to increasing atomic number. similar properties recur periodically when elements are arranged according to increasing atomic weight.
The modern periodic table is based on Moseley’s Periodic Law (atomic numbers). He suggested that instead of arranging elements in the ascending order of their atomic masses, they should be arranged in the ascending order of their atomic numbers. The number of electrons in an atom is equal to the atomic number Z.
The modern periodic law states that the physical and chemical properties of the elements are the periodic functions of their atomic numbers. Scientists arranged elements in increasing order of their atomic numbers from left to right across each row.
The modern periodic law states that the properties of the elements are a periodic function of their atomic numbers. As the properties of the elements are dependent upon the atomic number we can say that these are dependent upon the electronic configuration of the elements.
Internet search giant Google has dedicated a Doodle to Russian chemist Dmitri Mendeleev on his 182nd birth anniversary. Born on February 8, 1834, Mendeleev is popularly known as the “Father of Periodic Table”.
In 1869 Russian chemist Dimitri Mendeleev started the development of the periodic table, arranging chemical elements by atomic mass. He predicted the discovery of other elements, and left spaces open in his periodic table for them. In 1886 French physicist Antoine Bequerel first discovered radioactivity.
Mendeleev’s periodic law states that the physical and chemical properties of elements are a periodic function of their atomic weights. When the elements are arranged in order of their increasing atomic weights, elements with similar properties are repeated after certain regular intervals.
They are Darmstadtium, or Ds, which has 110 protons in its nucleus and was named after the town in which it was discovered; Roentgenium, or Rg, with 111 protons, named after the discoverer of X-rays Wilhelm Conrad Roentgen; and Copernicium, or Cn, which has 112 protons and is named after the Polish astronomer
: a law in chemistry: the elements when arranged in the order of their atomic numbers show a periodic variation of atomic structure and of most of their properties.