Progressing down group 1, the atomic radius increases due to the extra shell of electrons for each element. 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. That is why as you go up a group Chemical Reactivity increases because it is easier for elements to gain electrons when they have high electronegativity. Group 1 elements are known as Alkali Metals. 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 up group 7 (the halogens), again the elements get more reactive. The atom is held together by strong electrostatic forces of attraction between the positive protons in the nucleus and negative electrons. However, in a reaction with steam it forms magnesium oxide and hydrogen. WHY? Less precipitate is formed down the group with increasing solubility. 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. The reactivity all increases as you go down the periodic table, for example rubidium is far more reactive than sodium. It's how resistant a molecule is to decomposition at higher temperatures. I'll try not to make this confusing: 1. Elements become darker in colour going down group … As you go down the group, there are more inner electrons. due to ionization energy decreases . 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. Explaining the increase in reactivity down the group. - The atomic radius increases as you move down a group. Electrons present in the outermost shell of an atom are called valence electrons … The reactivity of group 1 metals increases as you go down the group because: 1) The atomic radius increases. Valence Electrons. so the reactivity increases .as we go down in . Reactions compared The table shows the main observations when lithium, sodium and potassium are added to water. Since there is only one electron to lose, group 1 metals are all extrememely reactive. As you go down the group, the outer shell electron is further away from the positive nucleus. Chemical Reactivity  decrease as you go down  the For Non-Metals, the farther right-up in the table you go, the higher the electronegativity. Calcium hydroxide is mainly formed as a white precipitate (although some does dissolve). As we go down the group, an additional electron shell is added thereby increasing the atomic radii of the atom. We saw the reactions, now we discuss why they actually get more reactive down the group. Describe the structure and bonding of sodium chloride. Chemical Reactivity  decrease as you go down  the For Non-Metals, the farther right-up in the table you go, the higher the electronegativity. The distance "c" is greater than "a" and the force of attraction between the nucleus and … They react with water to produce an alkaline metal hydroxide solution and hydrogen. Atoms get bigger so electrons are not held as tightly and are lost more easily. Electronegativity: This property determines how much the element attracts electrons. The effect of heat on the Group 2 nitrates. The larger an atom is, the more reactive it will be. All you really need to know is that the reactivity increases because the activation energy for the reactions falls. So what is thermal stability? On the reaction profile below, label the activation energy and the energy given out ((delta)H) - 2 marks. © 2021 Yeah Chemistry, All rights reserved. therefore the reactivity decreases down the group. Hence the attraction between nucleus and electrons decreases down the group. Nitrogen reacts with hydrogen to produce ammonia. Group 1 metals all have one electron in their outer shell. it means it is easy to form an ion. 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 quote from your text: So the stability that you are referring to is thermal stability.This is an important detail. Thermodynamic Properties of the Reactions Summarising the reason for the increase in reactivity as you go down the Group. The reactions become easier as the energy needed to form positive ions falls. This is also a good measure of reactivity, because the more that an element attracts electrons, the more reactive it is. For similar reasons the electronegativity decreases. It isn't clear from the syllabus that you need this explanation, but look at it anyway. First ionization energy decreases down group 17 from top to bottom. Group 1 & 7 elements are missing 1 electron from their valance shell making them highly votile and reactive. Going down the group, the first ionisation energy decreases. When they do react they produce hydroxides and hydrogen. Could someone please help me understand trends????? You know that protons are positively charged and electrons are negatively charged, therefore there is a level of attraction between these two oppositely charged subatomic particles. The reactions of the elements with water become more vigorous down the group. Because solubility increases down the group, the pH of a saturated solution increases down the group. 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 … A reducing agent is the compound that gets oxidised in the reaction and, therefore, loses electrons. The hydroxides all react with acids to make salts. Generally the melting point of the alkali metals decreases down the group. Group 1 elements increase in chemical reactivity as you go down the group from top to bottom. 1,why does the reactivity of elements in group 1 (hydrogen,lithium,sodium,pottasium)increase as you continue down? Group 1 elements increase in chemical reactivity as you go down the group from top to bottom. The group 1 elements are all soft, reactive metals with low melting points. 1,why does the reactivity of elements in group 1 (hydrogen,lithium,sodium,pottasium)increase as you continue down? Ionisation is a reaction so ionisation energy decreases as reactivity increases. 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