The force of attraction between the nucleus and the electron is less than for smaller atoms, and the outer electron is lost more easily. The larger the atom, the further the outer electron is from the nucleus. These atoms are larger because they have more shells. Group 1 elements become more reactive as we move down the group. This can be represented by a half equation (higher tier): A sodium atom loses one electron to form a sodium ion Group 1 metals all react in the same way, because each of them loses an electron to form a positive ion with a stable electronic configuration – a full outer shell.įor example, sodium loses one electron to form a sodium ion, Na +, with a full outer shell. potassium will do this as well but it is hard to see as the reaction is so fast and also potassium burns with a lilac flame and crackles as it explodes at the end of the reaction.sodium also melts to form a silvery-grey ball on the surface of the water.the solution remaining at the end will be colourless.they will all release heat as they react as the reactions are exothermic and they will eventually disappear. ![]() the metals move about the surface of the water and fizz as hydrogen gas is produced. The simpler it is for electrons to be given or taken away the farther to the left and down the periodic chart you travel, the greater the reactivity.lithium, sodium and potassium are less dense than water so they float on the surface of the water.There are some common observations and some differences: ![]() Sodium + water → sodium hydroxide + hydrogenĪll Group 1 metal reacts with water. This is the equation for the reaction between sodium and water: They must be stored under oil to prevent them reacting with the air or water vapour.Īll Group 1 elements react with water to produce a metal hydroxide and hydrogen. The electrons on the outer most energy level (shells) are called.
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