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Dating online > Russian > Find the odd one out copper iron mercury brass

Find the odd one out copper iron mercury brass

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Justification: Here, all except Brass are metals, while brass is an alloy. Hence, the answer is c. Analogy Complete Analogous Pair. Simple Analogy.

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SEE VIDEO BY TOPIC: MERCURY vs LEAD - Rare experiment from 1952

Find the odd one out: copper, iron, Mercury ,brass,

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It is a heavy metal that is denser than most common materials. Lead is soft and malleable , and also has a relatively low melting point. When freshly cut, lead is silvery with a hint of blue; it tarnishes to a dull gray color when exposed to air.

Lead has the highest atomic number of any stable element and three of its isotopes are endpoints of major nuclear decay chains of heavier elements. Lead is a relatively unreactive post-transition metal. Its weak metallic character is illustrated by its amphoteric nature; lead and lead oxides react with acids and bases , and it tends to form covalent bonds.

Exceptions are mostly limited to organolead compounds. Like the lighter members of the group, lead tends to bond with itself ; it can form chains and polyhedral structures. Lead is easily extracted from its ores ; prehistoric people in Western Asia knew of it. Galena , a principal ore of lead, often bears silver , interest in which helped initiate widespread extraction and use of lead in ancient Rome.

Lead production declined after the fall of Rome and did not reach comparable levels until the Industrial Revolution. In , the annual global production of lead was about ten million tonnes, over half of which was from recycling.

Lead's high density, low melting point, ductility and relative inertness to oxidation make it useful. These properties, combined with its relative abundance and low cost, resulted in its extensive use in construction, plumbing , batteries , bullets and shot , weights, solders , pewters , fusible alloys , white paints , leaded gasoline , and radiation shielding.

In the late 19th century, lead's toxicity was recognized, and its use has since been phased out of many applications. However, many countries still allow the sale of products that expose humans to lead, including some types of paints and bullets. Lead is a neurotoxin that accumulates in soft tissues and bones; it damages the nervous system and interferes with the function of biological enzymes, causing neurological disorders, such as brain damage and behavioral problems.

A lead atom has 82 electrons , arranged in an electron configuration of [ Xe ]4f 14 5d 10 6s 2 6p 2. The sum of lead's first and second ionization energies —the total energy required to remove the two 6p electrons—is close to that of tin , lead's upper neighbor in the carbon group.

This is unusual; ionization energies generally fall going down a group, as an element's outer electrons become more distant from the nucleus , and more shielded by smaller orbitals. The similarity of ionization energies is caused by the lanthanide contraction —the decrease in element radii from lanthanum atomic number 57 to lutetium 71 , and the relatively small radii of the elements from hafnium 72 onwards. This is due to poor shielding of the nucleus by the lanthanide 4f electrons.

The sum of the first four ionization energies of lead exceeds that of tin, [3] contrary to what periodic trends would predict. Relativistic effects , which become significant in heavier atoms, contribute to this behavior. Lead's lighter carbon group congeners form stable or metastable allotropes with the tetrahedrally coordinated and covalently bonded diamond cubic structure. The energy levels of their outer s- and p-orbitals are close enough to allow mixing into four hybrid sp 3 orbitals.

In lead, the inert pair effect increases the separation between its s- and p-orbitals, and the gap cannot be overcome by the energy that would be released by extra bonds following hybridization. Lead consequently has a face-centered cubic structure [7] like the similarly sized [8] divalent metals calcium and strontium. Pure lead has a bright, silvery appearance with a hint of blue.

Characteristic properties of lead include high density , malleability, ductility, and high resistance to corrosion due to passivation. Lead's close-packed face-centered cubic structure and high atomic weight result in a density [16] of Lead is a very soft metal with a Mohs hardness of 1.

In comparison, that of aluminium is The melting point of lead—at Natural lead consists of four stable isotopes with mass numbers of , , , and , [30] and traces of five short-lived radioisotopes. With its high atomic number, lead is the heaviest element whose natural isotopes are regarded as stable; lead is the heaviest stable nucleus. This distinction formerly fell to bismuth , with an atomic number of 83, until its only primordial isotope , bismuth, was found in to decay very slowly. Three of the stable isotopes are found in three of the four major decay chains : lead, lead, and lead are the final decay products of uranium, uranium, and thorium, respectively.

As uranium decays into lead, their relative amounts change; this is the basis for uranium—lead dating. Apart from the stable isotopes, which make up almost all lead that exists naturally, there are trace quantities of a few radioactive isotopes. One of them is lead; although it has a half-life of only Lead, , and are present in the decay chains of uranium, thorium, and uranium, respectively, so traces of all three of these lead isotopes are found naturally.

Minute traces of lead arise from the very rare cluster decay of radium, one of the daughter products of natural uranium, and the decay chain of neptunium, traces of which are produced by neutron capture in uranium ores. Lead is particularly useful for helping to identify the ages of samples by measuring its ratio to lead both isotopes are present in a single decay chain. In total, 43 lead isotopes have been synthesized, with mass numbers — Bulk lead exposed to moist air forms a protective layer of varying composition.

Lead II carbonate is a common constituent; [46] [47] [48] the sulfate or chloride may also be present in urban or maritime settings. Fluorine reacts with lead at room temperature, forming lead II fluoride. The reaction with chlorine is similar but requires heating, as the resulting chloride layer diminishes the reactivity of the elements.

Lead metal resists sulfuric and phosphoric acid but not hydrochloric or nitric acid ; the outcome depends on insolubility and subsequent passivation of the product salt. The tetravalent state is common for the carbon group. The divalent state is rare for carbon and silicon , minor for germanium, important but not prevailing for tin, and is the more important of the two oxidation states for lead. The result is a stronger contraction of the lead 6s orbital than is the case for the 6p orbital, making it rather inert in ionic compounds.

The inert pair effect is less applicable to compounds in which lead forms covalent bonds with elements of similar electronegativity, such as carbon in organolead compounds. In these, the 6s and 6p orbitals remain similarly sized and sp 3 hybridization is still energetically favorable. Lead, like carbon, is predominantly tetravalent in such compounds.

There is a relatively large difference in the electronegativity of lead II at 1. Lead II compounds are characteristic of the inorganic chemistry of lead. Even strong oxidizing agents like fluorine and chlorine react with lead to give only PbF 2 and PbCl 2. As the chloride salt is sparingly soluble in water, in very dilute solutions the precipitation of lead II sulfide is achieved by bubbling hydrogen sulfide through the solution. Litharge is the most commonly used inorganic compound of lead.

Lead sulfide is a semiconductor , a photoconductor , and an extremely sensitive infrared radiation detector. The other two chalcogenides, lead selenide and lead telluride , are likewise photoconducting. They are unusual in that their color becomes lighter going down the group. Lead dihalides are well-characterized; this includes the diastatide [64] and mixed halides, such as PbFCl.

The relative insolubility of the latter forms a useful basis for the gravimetric determination of fluorine. The difluoride was the first solid ionically conducting compound to be discovered in , by Michael Faraday.

Lead II sulfate is insoluble in water, like the sulfates of other heavy divalent cations. Lead II nitrate and lead II acetate are very soluble, and this is exploited in the synthesis of other lead compounds. Few inorganic lead IV compounds are known. They are only formed in highly oxidizing solutions and do not normally exist under standard conditions.

Lead dioxide is a strong oxidizing agent, capable of oxidizing hydrochloric acid to chlorine gas. Lead disulfide [72] and lead diselenide [73] are only stable at high pressures. Lead tetrafluoride , a yellow crystalline powder, is stable, but less so than the difluoride. Lead tetrachloride a yellow oil decomposes at room temperature, lead tetrabromide is less stable still, and the existence of lead tetraiodide is questionable.

Lead III may be obtained, as an intermediate between lead II and lead IV , in larger organolead complexes; this oxidation state is not stable, as both the lead III ion and the larger complexes containing it are radicals. Numerous mixed lead II,IV oxides are known. A further sesquioxide , Pb 2 O 3 , can be obtained at high pressure, along with several non-stoichiometric phases. Many of them show defective fluorite structures in which some oxygen atoms are replaced by vacancies: PbO can be considered as having such a structure, with every alternate layer of oxygen atoms absent.

Lead can form multiply-bonded chains , a property it shares with its lighter homologs in the carbon group. Its capacity to do so is much less because the Pb—Pb bond energy is over three and a half times lower than that of the C—C bond. The lead analog of the simplest organic compound , methane , is plumbane. Plumbane may be obtained in a reaction between metallic lead and atomic hydrogen. These compounds are relatively stable: tetraethyllead only starts to decompose if heated [88] or if exposed to sunlight or ultraviolet light.

Tetraethyllead, once added to gasoline, was produced in larger quantities than any other organometallic compound. Lead's per-particle abundance in the Solar System is 0. Primordial lead—which comprises the isotopes lead, lead, lead, and lead—was mostly created as a result of repetitive neutron capture processes occurring in stars. The two main modes of capture are the s- and r-processes. In the s-process s is for "slow" , captures are separated by years or decades, allowing less stable nuclei to undergo beta decay.

Further captures result in lead, lead, and lead On capturing another neutron, lead becomes lead, which quickly decays into bismuth On capturing another neutron, bismuth becomes bismuth, and this beta decays to polonium, which alpha decays to lead The cycle hence ends at lead, lead, lead, and bismuth In the r-process r is for "rapid" , captures happen faster than nuclei can decay.

The neutron flux involved may be on the order of 10 22 neutrons per square centimeter per second. Lead is classified as a chalcophile under the Goldschmidt classification , meaning it is generally found combined with sulfur. This accounts for lead's relatively high crustal abundance of 14 ppm; it is the 38th most abundant element in the crust. The main lead-bearing mineral is galena PbS , which is mostly found with zinc ores. Arsenic , tin, antimony, silver , gold, copper, and bismuth are common impurities in lead minerals.

Metal Alloys From A to Z

An alloy is a material made by melting one or more metals together with other elements. This is an alphabetical list of alloys grouped according to base metal. Some alloys are listed under more than one element, since the composition of the alloy may vary such that one element is present in a higher concentration than the others. Share Flipboard Email.

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Oil and water. Cellphones and swimming pools. Toothpaste and orange juice. Combining silver, gold, brass, or iron just to name a few , is a great strategy for adding visual interest and depth to a space.

Mixing Metals at Home: The Do’s and The Don’ts to Know

All Rights Reserved. The material on this site can not be reproduced, distributed, transmitted, cached or otherwise used, except with prior written permission of Multiply. Metal and Alloys. Wiki User Iron is odd man out. Related Questions Asked in Plumbing Is brass an alloy of copper and iron? Asked in Elements and Compounds, Metal and Alloys What is difference between brass and copper alloys? Brass IS an alloy of copper and zinc Copper and zinc are pure metals elements. Asked in Percentages, Fractions, and Decimal Values What metal contains 60 percent copper and 40 percent zinc?

MBA CET – Solved Questions – Set 1

These solutions for Composition Of Matter are extremely popular among Class 8 students for Science Composition Of Matter Solutions come handy for quickly completing your homework and preparing for exams. Choose the appropriate option and rewrite the following statements. Solids retain their voume even when external pressure is applied. Water, mercury and bromine are similar o each other, because three are i.

The questions posted on the site are solely user generated, Doubtnut has no ownership or control over the nature and content of those questions. Doubtnut is not responsible for any discrepancies concerning the duplicity of content over those questions.

Pustak Mahal Amazon. Pustak Mahal Editorial Group. Pustak Mahal , 5. It is a common sentiment expressed by many students from time to time.

Find odd man out of copper iron mercury and brass

Carrot is a root. Answer: Root. Four of the following five are alike in a certain way and so form a group.

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With frame. Critical Museum Guide. General Remarks to Literature and Sources. Books and Other Major Sources. History of Carbon.

Find the Odd Word : 1.Aluminium 2.Iron 3. Copper. 4. Brass

Doc Brown's Chemistry. Actually 1 scandium and 10 zinc are not really proper transition metals, they are not very 'colourful' in their chemistry! The physical properties of Transition Metals like density, melting points, boiling points, strength are described and discussed along with a description of the important transition metal chemical properties of e. There are also sections on how transition metals can be improved to increase their usefulness e. Some Reminders about the Periodic Table by way of an introduction. The basic structure of the Periodic Table and note where the 'Transition Metals' are. A note about 'TRUE' transition metals it can be confusing! There are three important characteristics of transition metals and their compounds you should know about:.

Magnesium + = magnesium oxide 3 What is the missing word? 18 Which is the "odd man out"? copper iron lead mercury potassium. platinum 19 What is the  Pustak Mahal Editorial Group -

The transition elements or transition metals occupy the short columns in the center of the periodic table, between Group 2A and Group 3A. They are sometimes called the d -block elements , since in this region the d -orbitals are being filled in, and are also referred to as B-group elements since in most numbering systems of the columns on the periodic table the numerals of these groups are followed by the letter B. The period 7 transition metals are the naturally-occurring actinium Ac , and the artificially produced elements rutherfordium Rf , dubnium Db , seaborgium Sg , bohrium Bh , hassium Hs , meitnerium Mt , darmstadtium Ds , roentgenium Rg , and the as-yet unnamed ununbiium Uub. In the transition metals, the five d orbitals are being filled in, and the elements in general have electron configurations of n -1 d ns 2 , although there are some exceptions when electrons are shuffled around to produce half-filled or filled d subshells. All of the transition metals in their elemental forms are malleable and ductile except for mercury, which is a liquid at room temperature , and are good conductors of heat and electricity.

It is a heavy metal that is denser than most common materials. Lead is soft and malleable , and also has a relatively low melting point. When freshly cut, lead is silvery with a hint of blue; it tarnishes to a dull gray color when exposed to air.






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