C O, N O, N 2 O ).Īmphoteric oxides behave as acidic with bases and as basic with acids, whereas neutral oxides have no acidic or basic properties. Oxides of elements in the centre are amphoteric. The element on extreme right is the most acidic. The normal oxide formed by the element on extreme left is the most basic. (3) Reactivity with Oxygen : Elements on two extremes of a period easily combine with oxygen to from oxides. (2) Metallic and non-metallic Properties : We move left to right in a period metallic property decreases and non-metallic property increases. (1) Reactivity of Oxidation and Reduction : Extremely left elements of periodic table are reducing agent and extremely right elements of periodic table are oxidising agent. (Exception : Noble gas)Įlements are more reactive in both of the side and elements are less reactive in middle in periodic table.Įlements are situated very left side (Alkali metals) have tendency to lose one electron and elements are situated right side (Halogen) have tendency to gain one electron and becomes negative. The energy required in this process is called. So, we can say that in period ionisation enthalpy is very less in left side and electron gain enthalpy is very high and negative in right side. An atoms reactivity can be judged by the ease with which the electrons can be withdrawn from an atom. So, ionisation enthalpy increases in period and value of electron gain enthalpy becomes more negative. Gethin: So, the further down the table you go the more reactive they become.When we go left to right atomic radius and ionic radius decreases. So, the reason we didn't see the reactions of those last three metals is that they are so reactive the explosion would be far too big. Miss Armit: No, it's the second rarest element on Earth. That's not an element that you hear a lot of. We saw there lithium, then sodium and then potassium, but you didn't see rubidium, caesium and francium. As you can see the metal's get increasingly more reactive as you go down this group. Gethin: It's fair to say that you love the Group 1 metals, don't you. Well, sodium is below lithium in group one and the reactivity of the alkali metals increases as you go down the group, so potassium is even more reactive. So let's try it with another Group 1 metal - sodium.Īs you can see it reacts far more vigorously then lithium.

And can you see the little purple trail there? That universal indicator is showing us that the water now contains an alkali in this case - lithium hydroxide. Electronegativity: the atoms electron attracting power. 1 Periodic trends: Valency 2 Periodic trends: Atomic radius 3 Periodic trends: Metallic character 4 Periodic trends: Non metallic character 5 Periodic trends: Electronegativity 6 Periodic trends: Electron affinity 7 Periodic trends: Ionization energy What are Periodic trends You feel hot in summer and cold in winter. Ionisation Energy: energy required to remove an electron from a gaseous atom. This is due to the decreasing atomic radius and increasing nuclear charge meaning. It's transferring its energy to its surroundings by heating. PERIODIC TABLE TRENDS PROPERTIES OF ELEMENTS Atomic Radius: half the distance between 2 nuclei in a molecule. First ionisation energies follow a general increasing trend along Period 2. Well, you can see it's reacting with the water straight away - it's steadily fizzing away there.

And if I put some universal indicator in, like this, you'll see that it's green and that means it's neutral.īut let's see what happens when we put the lithium in. And do you see how quickly it tarnishes, how quickly it's changing colour? Here we've got some water. Here I've got some lithium and I'm just going to cut a little bit off. When a Group 1 element reacts with water it produces a metal hydroxides solution and hydrogen gas. They're soft and shiny when freshly cut, but they quickly tarnish as the metal reacts with oxygen in the air. Let's take a look at some Group 1 metals then - also known as alkaline metals.įran: Group 1 elements are called the alkali metals. Gethin: And today we're going to be looking at the periodic table.

Reactivity trend across periodic table