Periodic table reactive metals3/24/2024 ![]() The valence electrons are held closer towards the nucleus of the atom. This means that the nucleus attracts the electrons more strongly, pulling the atom's shell closer to the nucleus. The effect of increasing proton number is greater than that of the increasing electron number therefore, there is a greater nuclear attraction. Chemistry The Periodic Table Periodic Trends in Atomic Size. The alkali metals provide the best example of group trends in properties in the periodic table, with elements exhibiting well-characterized homologous behaviour. ![]() Group - reactivity decreases as you go down the group. However, at the same time, protons are being added to the nucleus, making it more positively charged. Group - reactivity increases as you go down a group In Non-metals Period - reactivity increases as you go from the left to the right. This is because, within a period or family of elements, all electrons are added to the same shell. Atomic radius patterns are observed throughout the periodic table.Ītomic size gradually decreases from left to right across a period of elements. The covalent radii of these molecules are often referred to as atomic radii. Nevertheless, it is possible for a vast majority of elements to form covalent molecules in which two like atoms are held together by a single covalent bond. Some are bound by covalent bonds in molecules, some are attracted to each other in ionic crystals, and others are held in metallic crystals. From left to right in the periodic table, the nonmetals can be divided into the reactive nonmetals and the noble gases. However, this idea is complicated by the fact that not all atoms are normally bound together in the same way. They’re closely followed by the marginally less reactive group two metals. The atomic radius is one-half the distance between the nuclei of two atoms (just like a radius is half the diameter of a circle). Group 1 metals, the most reactive metals in the periodic table, head up the rankings. This is caused by the increase in atomic radius. ![]() Electron affinity decreases from top to bottom within a group.This is caused by the decrease in atomic radius. Electron affinity increases from left to right within a period.This causes the electron to move closer to the nucleus, thus increasing the electron affinity from left to right across a period. All the elements in Group 2 have two electrons in their valence shells, giving them. Although many characteristics are common throughout the group, the heavier metals such as Ca, Sr, Ba, and Ra are almost as reactive as the Group 1 Alkali Metals. Moving from left to right across a period, atoms become smaller as the forces of attraction become stronger. Group 2 contains soft, silver metals that are less metallic in character than the Group 1 elements. With a larger distance between the negatively-charged electron and the positively-charged nucleus, the force of attraction is relatively weaker. This means that an added electron is further away from the atom's nucleus compared with its position in the smaller atom. \( \newcommand\): Periodic Table showing Electron Affinity TrendĮlectron affinity generally decreases down a group of elements because each atom is larger than the atom above it (this is the atomic radius trend, discussed below). ![]()
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