Highly reactive metal

Learning Objectives • To understand the basic properties separating Metals, from Nonmentals and Metalloids An element is the simplest form of matter that cannot be split into simpler substances or built from simpler substances by any ordinary chemical or physical method. There are 110 elements known to us, out of which 92 are naturally occurring, while the rest have been prepared artificially. Elements are further classified into metals, non-metals, and metalloids. Table 2.11.1: Characteristic properties of metallic and non-metallic elements: Metallic Elements Nonmetallic elements Distinguishing luster (shine) Non-lustrous, various colors Malleable and ductile (flexible) as solids Brittle, hard or soft Conduct heat and electricity Poor conductors Metallic oxides are basic, ionic Nonmetallic oxides are acidic, compounds Cations in aqueous solution Anions, oxyanions in aqueous solution Metals All elements except hydrogen, which form positive ions by losing electrons during chemical reactions are called metals. Thus metals are electropositive elements. They are characterized by bright luster, hardness, ability to resonate sound and are excellent conductors of heat and electricity. Metals are solids under normal conditions except for Mercury. Physical Properties of Metals Metals are lustrous, malleable, ductile, good conductors of heat and electricity. Other properties include: • State: Metals are solids at room temperature with the exception of mercury, which is liquid at roo...

Metals generally react with acids. We know this, but we often miss out the key word: generally. This sweeping statement is a gross generalisation. Metals have varying tendency to react. Some react explosively, some moderately, and others not at all. The reactivity series arranges metals from the most reactive to the least. 2. How to memorise the reactivity series without memorising: the Periodic Table The reactivity series is written into the Periodic Table! Highly Reactive Group I and II Metals Group I alkali metals and Group II alkaline earth metals are the most reactive. They have the greatest tendency to lose electrons to form cations. For the four metals we need to know, those from Group I are more reactive than those from Group II. Within each group, the metal lower down the group is more reactive. Moderatively Reactive Metals Transition metals are generally less reactive than the main group metals. Lead in Group IV is also moderately reactive. The Trio of Unreactive Metals And the least reactive metals we need to know are copper, silver, and gold. The trio sit in the same column within the transition metal hood. 3. The reactivity series tells us if a reaction will happen and under what conditions Metal Reacts with Potassium Sodium Calcium Magnesium Cold water Hot steam Hydrochloric acid Zinc Iron Hot steam Hydrochloric acid Lead Copper Silver Gold No reaction reactive metal + water ⟶ metal hydroxide + hydrogen reactive metal + steam ⟶ metal oxide + hydrogen reactive...

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Alkali metals are so-called because when they react with water, they create highly alkaline substances. Every element has a nucleus, made up of protons and neutrons, and alkali metals are no different. Surrounding the nucleus of atoms are electrons, which are particles with a negative charge. These electrons exist in All atoms naturally want to have a completely full outermost shell of electrons. However, elements in that first column of the periodic table all have one electron in their outermost shell. This outermost shell is also called the valence shell, and the electrons that reside there are called valence electrons. Having only one electron in the outermost shell makes it very easy for the atoms of alkali metals to reach points of stability – they just need to lose one electron! This willingness and ease of losing an electron to reach a state of equilibrium is known as high reactivity. In fact, reactivity in chemistry is defined by the number of electrons in the outermost shell. Noble gases (elements like neon and helium) are very unreactive because their outermost electron shells are full. "Since the alkali metals only have one valence electron, they typically achieve this state by giving up that electron. In this process, the alkali metal is said to be oxidized, and whatever takes the electron from the alkali metal is reduced. All of the alkali metals like to give up their single valence electron," says Since alkali metals are so reactive, they are usually found in...

There are many different types of people in the world. Some are very calm and not much bothers them. Others can get agitated on occasion, and some get very animated and upset about pretty much anything. This is an analogy for metallic elements. Some are highly reactive with many compounds, some only react with certain compounds and others hardly react at all. Let's go through the different types of metal reactions. There are a few highly reactive metals, which react with dilute acids, water, and oxygen, and include potassium, sodium, lithium, and calcium, to name a few. These metals are part of the alkali metal and alkaline earth metals, which are the two columns on the far left side of the periodic table. Let's look at the reaction of sodium with a dilute acid, water, and oxygen. Sodium reacts with dilute hydrochloric acid according to the following equation: 2Na (s) + 2HCl (aq) → 2NaCl (aq) + H 2 (g) If we saw this reaction take place we would see hydrogen bubbles forming in the solution. Let's break this reaction down to see what's happening in terms of electrons transferring between the reactants: 2Na (s) + 2H +1 (aq) + 2Cl -1 (aq) → 2Na +1 (aq) + 2Cl -1 (aq) + H 2 (g) Less reactive metals react with acids and oxygen, but not water, and include several transition metals such as zinc, iron, and tin. Let's look at how zinc reacts with a dilute acid, water, and oxygen. Zinc reacts with dilute acids and we'll see the same electron transfer in this reaction as we did wh...

All metals are reactive by definition, but two groups are considered to be much more highly reactive than the rest. The Alkali Metals group consists of the first row on the left side of the periodic table - lithium, sodium, potassium, rubidium, cesium,and francium. These metals have just one electron in the outermost orbital, called a valence electron. They lose this electron very readily in reaction with other elements, becoming a +1 ion and releasing energy in the process; that's where the reaction comes from. A classic lab demonstration consists of putting a chunk of sodium into water, where it explodes violently. See the youtube link below for a demonstration of this - it's quite amazing! The next column to the right, the Alkaline Earth Metals, consists of beryllium, magnesium, calcium, strontium, barium, and radium. These metals are not quite as reactive as the first group, but will still react- for instance, magnesium burns very readily. They have 2 valence electrons and will produce a +2 ion when reacting. See eNotes Ad-Free

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Metalloids or Semimetals • Electronegativity and ionization energy intermediate between that of metals and nonmetals • May possess a metallic luster • Variable density, hardness, conductivity, and other properties • Often make good semiconductors • Reactivity depends on the nature of other elements in the reaction 1 IA 1A 18 VIIIA 8A 1 H 1.008 2 IIA 2A 13 IIIA 3A 14 IVA 4A 15 VA 5A 16 VIA 6A 17 VIIA 7A 2 He 4.003 3 6.941 4 9.012 5 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00 10 20.18 11 22.99 12 24.31 3 IIIB 3B 4 IVB 4B 5 VB 5B 6 VIB 6B 7 VIIB 7B 8 ← ← 9 VIII 8 10 → → 11 IB 1B 12 IIB 2B 13 Al 26.98 14 Si 28.09 15 P 30.97 16 S 32.07 17 Cl 35.45 18 39.95 19 39.10 20 40.08 21 44.96 22 Ti 47.88 23 50.94 24 52.00 25 Mn 54.94 26 Fe 55.85 27 Co 58.47 28 Ni 58.69 29 Cu 63.55 30 Zn 65.39 31 Ga 69.72 32 Ge 72.59 33 As 74.92 34 Se 78.96 35 Br 79.90 36 83.80 37 85.47 38 87.62 39 Y 88.91 40 Zr 91.22 41 Nb 92.91 42 Mo 95.94 43 Tc (98) 44 Ru 101.1 45 Rh 102.9 46 Pd 106.4 47 Ag 107.9 48 Cd 112.4 49 In 114.8 50 Sn 118.7 51 Sb 121.8 52 Te 127.6 53 I 126.9 54 131.3 55 132.9 56 137.3 * 72 Hf 178.5 73 Ta 180.9 74 W 183.9 75 Re 186.2 76 Os 190.2 77 Ir 190.2 78 Pt 195.1 79 Au 197.0 80 Hg 200.5 81 Tl 204.4 82 Pb 207.2 83 Bi 209.0 84 Po (210) 85 At (210) 86 (222) 87 (223) 88 (226) ** 104 Rf (257) 105 Db (260) 106 Sg (263) 107 Bh (265) 108 (265) 109 Mt (266) 110 Ds (271) 111 Rg (272) 112 Cn (277) 113 Uut -- 114 Fl (296) 115 Uup -- 116 Lv (298) 117 -- 118 -- * Lanthanide Series 57 La 138.9 58 Ce 14...