![]() ![]() Rubidium is used in the making of optical glasses, and also in laser cooling.Ĭaesium is used in night-vision equipment. Potassium is also used to make detergents Potassium is a vital component of fertilisers, and has a major role in the daily functioning of the human body. Sodium is used to make soaps, and is also used in street lamps. Lithium batteries power all modern electronics, electric vehicles, and most things that need electric power. ![]() Let us have a look at some common applications of group 1 alkali metals. When aluminium is alloyed with lithium, the alloy formed has better tensile strength, and it can be used in aircraft parts. Aluminium is a lightweight metal that is ideal for manufacturing aircraft parts, but aluminium alone cannot be used because of its low tensile strength. Alloys of alkali metals have several applications- for example, Li-Al alloy is used to manufacture aircraft parts. Group 1 elements have plenty of uses in not only industrial, but also biomedical and academic applications.Īlkali metals can be alloyed with different other metals, including transition metals, to improve their physical and chemical properties. Now let us visualise how a carbonate compound of a group 1 element looks like. ![]() Oxygen is marked in red to indicate that the negative charge is more likely to be found on those atoms. The negative charge in a carbonate ion is not focussed on any one or two oxygen atoms, but is delocalised over the entire ion (although more concentrated over the oxygen atoms than the carbon atom). 7: Carbonate Ion | StudySmarter Originals Now let us visualise the carbonate ion (CO 3 2-).įig. The c harge density of metal cations decreases as we go down group 1. A cation of the same charge but of a larger atom has lesser charge density, as the charge is spread out in a larger volume. This can be explained in terms of size and charge of the cations involved.Ī cation of a small atom packs a lot of charge in a smaller volume. Nitrates and carbonates of group 1 elements tend to have a trend in their thermal stability such that it increases as we go down the group. This makes it easier for the alkali metal atoms to lose 1 electron as the nucleus is not watching, making it easy to participate in reactions. As we go down the group, the atomic radius increases, and the outermost electron is more loosely held by the nucleus. Reactivity of alkali metals increases as we go down group 1. Hence, their tendency to attract an electron pair is very less. Therefore, alkali metals prefer to lose one electron to attain the nearest noble gas configurations. To attain stability, sodium has to lose electrons. Its nearest noble gas is neon (10 electrons). Notice that, alkali metals are one electron more than their respective nearest noble gases. Electronegativity decreases as we go down the group, which means that the elements get worse at attracting an electron pair. Judging from this, you can see that all elements in group 1 have very low electronegativity. The most electronegative element (fluorine) has the electronegativity value of 4.0 on the Pauling scale. 6: Electronegativity of Group 1 Elements | Chemguide Electronegativity is measured on the Pauling scale.įig. It is very stable, having a fully filled outer shell of electrons, and removing the second electron takes a humungous amount of energy.Įlectronegativityis the tendency of an atom to attract an electron pair. It is because the sodium atom loses an electron and attains the stable noble gas configuration of neon. Notice the huge difference between the first and second Ionisation energies. The second Ionisation energy of sodium is as high as 4563 k J mol -1. Finally, we'll look at some uses and applications of group 1 elements.We'll then find out how you can identify group 1 metals using flame tests and learn the colours that they produce.We'll also look into the thermal stabilities of group 1 nitrates and carbonates.After that, we'll explore the properties of group 1 elements and the trends found as you go down the group.We'll find out about their position in the periodic table.In particular, we'll focus on the alkali metals.In this article, we will see what elements make up group 1 in chemistry.Read on to know more about the Lithium family. On the contrary, do you know that some metals are very soft like a rubber? Lithium is one such metal which is so soft that it can be cut with a knife! Lithium's home is Group 1 of the periodic table. Iron stays in the d-block of the periodic table. What is the first thing that comes to your mind when you think of Iron? It is hard, shiny and a very good conductor of electricity. Yes, it is the most commonly used and one of the most abundant metals found in the universe. Can you think of a metal that we most frequently use in everyday life? ![]()
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