It isn't clear from the syllabus that you need this explanation, but look at it anyway. As elements get bigger, they have a higher level of reactivity. For similar reasons the electronegativity decreases. 2, why does the reactivity of elements in group 7 (florine,chorine) decrease as you continue down the group? Reactivity increases down the group. - The atomic radius increases as you move down a group. As you go down the Group, the carbonates have to be heated more strongly before they will decompose. One to one online tution can be a great way to brush up on your Chemistry knowledge. Mg(s) + H2O(g) → MgO(s) + H2(g) b) Calcium is more reactive. Generally the melting point of the alkali metals decreases down the group. Show the electron shell including the s, p, and d orbitals together. The electrons in the outer shell move further away from the nucleus as we go down the group and the attraction force between the electrons and the nucleus become weaker and weaker. This is clearly seen if we observe the reactions of magnesium and calcium in water. Now on moving down the group , the size of atom increases due to addition of atomic shells due to this , the tendency of an atom to gain electron decreases down the group due to decrease in nuclear charge . Chemical reactivity of group 17 elements decreases down group 17 from top to bottom. On the reaction profile below, label the activation energy and the energy given out ((delta)H) - 2 marks. Explaining trends in reactivity. We have evidence for the stability of the electronic configuration of the group 1 cations based on inspection of the values for the second ionisation for this group. The reactivity increases as you go down a group.This is because the number of shells increases and so the effective nuclear charge on the valence electrons decreases.the valence electrons are in the outermost shell so they can be lost easily. The solubilities of the sulphates of the elements decreases down the group. 2) There are more inner electrons which repel the outer shell electron. As you go down group 1 (the alkali metals) in the periodic table, the elements get more reactive. The reactivity of group 1 metals increases as you go down the group because: 1) The atomic radius increases. An atom is made in such a way that the nucleus with the positive charges (protons) is in the centre and the negative charge (electrons) are arranged in shells around it. Why do the reactivity of the group 1 atoms increase as you go down the group, but the reactivity of group 7 decreases as you go down the group. As you go down the group, there are more inner electrons. When a halogen atom reacts, it gains one electron into their highest occupied energy level (outer shell) to form a singly negative charged ion. Group 1 elements are known as Alkali Metals. Reactions compared The table shows the main observations when lithium, sodium and potassium are added to water. The hydroxides all react with acids to make salts. As you go down the group, the outer shell electron is further away from the positive nucleus. Because solubility increases down the group, the pH of a saturated solution increases down the group. Hydrogen - Hydrogen - Reactivity of hydrogen: One molecule of hydrogen dissociates into two atoms (H2 → 2H) when an energy equal to or greater than the dissociation energy (i.e., the amount of energy required to break the bond that holds together the atoms in the molecule) is supplied. The answer lies in understanding what the atoms are trying to do. As you go up group 7 (the halogens), again the elements get more reactive. We have evidence for the stability of the electronic configuration of the group 1 cations based on inspection of the values for the second ionisation for this group. When they react they form positive metal ions by losing this electron. I know why group 1 reactivity increases as you go down the group but I am confused on group 7 and why it is different? Atoms get bigger so electrons are not held as tightly and are lost more easily. F is more reactive than Cl etc. The reactions proceed faster as the energy needed to form positive ions falls. The atom is held together by strong electrostatic forces of attraction between the positive protons in the nucleus and negative electrons. The reactivity of Group 7 elements decreases down the group. Since there is only one electron to lose, group 1 metals are all extrememely reactive. As the atomic structure of the halogens becomes more complex with increasing atomic weight there is a gradiation in physical properties. Magnesium chloride is an ionic compound and has a high melting point. The carbonates become more stable to heat as you go down the Group. Non-metal atoms gain electrons when they react with metals. The distance "c" is greater than "a" and the force of attraction between the nucleus and … I get why it does in group 1, but I don't get why it does in group 7?? Electrons present in the outermost shell of an atom are called valence electrons … due to ionization energy decreases . It reacts with cold water to produce an alkaline solution of calcium hydroxide and hydrogen gas is released. Progressing down group 1, the atomic radius increases due to the extra shell of electrons for each element. However, in a reaction with steam it forms magnesium oxide and hydrogen. These repel the outer shell electron (like charges repel) therefore pushing it away. The solubilities of the hydroxides of the elements increase going down the group. The reactivity of these metals increases going down the group. The reactions become easier as the energy needed to form positive ions falls. This is in part due to a decrease in ionization energy down the group, and in part to a decrease in atomization energy reflecting weaker metallic bonds … Example - potassium(K) in the 4th period is more reactive than lithium(Li) in the 2nd period in group 1 The reactivity of group 1 metals increases as you go down the group because: 1) The atomic radius increases. The Group II elements are powerful reducing agents. Group 1 elements increase in chemical reactivity as you go down the group from top to bottom. Chemical Reactivity  decrease as you go down  the For Non-Metals, the farther right-up in the table you go, the higher the electronegativity. Nitrogen reacts with hydrogen to produce ammonia. All group 1 metals have one electron in its outer shell. Ionisation is a reaction so ionisation energy decreases as reactivity increases. Group 1 & 7 elements are missing 1 electron from their valance shell making them highly votile and reactive. Valence Electrons. Melting point and boiling point increase down Group 17 from top to bottom. Less precipitate is formed down the group with increasing solubility. It helps to think about the size of an atom with the location of the electrons and nucleus in mind. Reactivity increases down the group. As I said earlier, they are powerful reducing agen… Thermodynamic Properties of the Reactions The effect of heat on the Group 2 nitrates. As you go down the group, the outer shell electron is further away from the positive nucleus. Describe the structure and bonding of sodium chloride. I'll try not to make this confusing: 1. When they do react they produce hydroxides and hydrogen. a gp the removal of electron require less energy .therefore reactivity increases. Explain why the reactivity of elements in group 1 increases down the group but decrease in group 7 down the group, Electron affinity trend;why does it decrease down a group, Electronegativity and ionnisation energy trend in the periodic table, Periodic Trend Explanation about atomic radius. This attraction helps stabilize the atom. Electronegativity: This property determines how much the element attracts electrons. Not sure if I would put H in group 1. Look at this page again, and this time read the explanation for the increase in reactivity as you go down the group. N'T clear from the positive nucleus trends?????????????! It helps to think about the size of an atom is held together by strong electrostatic forces of attraction nucleus. One to one online tution can be a great way to brush up on Chemistry! Atom with the location of the distance is inversely proportional to the extra shell of electrons each. Nitrogen dioxide and oxygen ( florine, chorine ) decrease as you go down group. 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