DOCSLIB.ORG

CHEMISTRY Diagram Structure Bonding Na2o Sio2

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
CHEMISTRY Diagram Structure Bonding Na2o Sio2 CHEMISTRY Acidic Environment Assignment Part 2 1) Compare the structure and bonding of the following: (a) sodium oxide, (b) silicon dioxide, and (c) sulphur dioxide Diagram Structure Bonding An ionic lattice. Each unit cell exhibits the anti‐ fluorite structure. Ionic bonding The anions (O2‐) are Na2O in the face‐centred cubic array with the cations (Na+) in all the tetrahedral Red – O2‐ holes. Purple – Na+ Double covalent bonds join two SiO2 Covalent network oxygen atoms to each silicon atom. Red – Silicon Black – Oxygen Double covalent bonds join two oxygen atoms to Polar covalent a sulphur atom. SO2 molecule with bent Due to polarity, structure. there is dipole‐ dipole interaction between gaseous SO2 molecules. 2) Write equations for the reaction of the following with water: COMPOUND REACTION WITH WATER Carbon dioxide CO2(g) + H2O(l) H2CO3(aq) Sodium oxide Na2O(aq) + H2O(l) 2NaOH(aq) Calcium oxide CaO(aq) + H2O(l) Ca(OH)2(aq) Sulfur dioxide SO2(g) + H2O(l) H2SO3(aq) Sulfur trioxide SO3(g) + H2O(l) H2SO4(aq) Nitrogen dioxide NO2(g) + H2O(l) HNO2(aq) + HNO3(aq) 3) Beryllium oxide is amphoteric. (a) Explain what is meant by amphoteric, and (b) Study the two equations below*. Balance them, and indicate whether BeO is acting as an acid or base (a) ‘Amphoteric’ is a term used to describe a substance that exhibits both acidic and basic properties. Beryllium oxide is an amphoteric oxide that reacts with strong acids and strong bases. 2+ ‐ (b)*BeO(s) + 2HCl(aq) + 3H2O(l) Be(H2O)4 (aq) + 2Cl (aq) BeO acting as a base 2+ + *BeO(s) + 2NaOH(aq) + H2O(l) Be(OH)4 (aq) + 2Na (aq) BeO acting as an acid 4) Describe the origins of sulfur dioxide that are causing environmental problems The oxidation of hydrogen sulfide (H2S) which is a product of bacterial decomposition 2H2S (g) + 2O2 (g) 2SO2 (g) + 2H2O (g) The burning of fossil fuels which usually contain sulfide minerals like FeS2. These sulfide minerals in coal are oxidised when the fuel is combusted and sulfur dioxide is released. For example, 4FeS2 (s) + 11O2 (g) 2Fe2O3 (s) + 8SO2 (g) Metal smelters that convert metal sulfides into metals yield vast amounts of sulfur dioxide. For example, smelting chalcopyrite (CuFeS2) to obtain copper results in the release of SO2 2CuFeS2 (s) + 5O2 (g) + 2SiO2 (s) 2Cu (l) + 4SO2 (g) + 2FeSiO3 (l) “In Adelaide in 2000, petroleum refinery processing produced 40% of the sulphur dioxide emitted to the atmosphere, with motor vehicles contributing 22% and fuel combustion 15%.” 1 5) Describe the origins of oxides of nitrogen that are causing environmental problems Nitric oxide is formed when nitrogen and oxygen react at high temperatures, for example, during lightning strikes or high temperature combustion reactions in furnaces and internal combustion engines N2 (g) + O2 (g) 2NO (g) Nitric oxide, a colourless gas and neutral oxide, reacts with oxygen to form nitrogen dioxide, a brown gas and an acidic oxide 2NO (g) + O2 (g) 2NO2 (g) “In Adelaide in 2000, an estimated 66% of nitrogen oxides (including NO and NO2) came from motor vehicles, with a further 20% from fuel combustion.” 1 6) (a) Use www.deh.gov.au/soe/2001/atmosphere/atmosphere02‐16.html to describe the change in acidic oxides in the atmosphere using ice cores from Antarctica. Download the relevant graphs and analyse them (b) Describe the importance of data from ice cores (a) Ice core data obtained from Antarctica (refer to graph below) indicates that the atmospheric concentration of carbon dioxide has increased since AD 1000. It can be seen that prior to the 1800s, CO2 (ppm) showed relatively minor fluctuation ranging from approximately 275ppm‐285ppm. This range may represent the normal concentration of CO2 that works in conjunction with other atmospheric constituents such as methane, nitrous oxide and water vapour to contribute to a natural greenhouse effect. During and after the 1800s, the data from the ice core samples show a very steep increase in CO2 (ppm), from approximately 285ppm in 1800 to 330ppm before the year 2000. This dramatic increase is accounted for by the occurrence of the Industrial Revolution in the 1800s. The burning of fossil fuels to provide power released vast amounts of carbon dioxide and other combustion products into the atmosphere. Since the 1800s, technological advances have placed greater demands on industry and transport in particular, in terms of the generation of power by burning coal. Consequently, in the recent years, there has been a rapid increase in the concentration of atmospheric carbon dioxide. Carbon dioxide concentration from ice core and air samples since AD 1000.Source: CSIRO Atmospheric Research. (b) Ice core data can be used to “reconstruct past climate conditions and climate changes through time...an ice core paleoclimate record can be compared to and combined with other paleoclimate records, for example, from ocean sediment cores, tree rings, coral records and spleotherm (stalactites and stalagmites) records to establish the Earth’s climate history. This climate history can then be used to establish the limits of natural climate variability which can be used to constrain climate models and to help us reduce uncertainty in future climate predictions.” (Secrets from Antarctic Ice, Mark Curran) In other words, data from ice cores is important as it allows us to not only unlock the composition of the ancient atmosphere, but also to understand how our past actions have affected the climate. By understanding causal relationships, such as increased global temperature due to an increase in the concentration of atmospheric carbon dioxide, which in turn is largely due to the burning of fossil fuels, we can forecast climate change based on models of the climate constructed using evidence collected from ice core analysis, such as gas composition of trapped air to determine CO2 levels. Strategies can then be imposed to rectify dim prospects if our present actions are predicted to have an adverse impact on the atmosphere. For example, as ice core research has revealed a link between greenhouse gases and climate change in the past, we need to reduce greenhouse gas emissions, in particular, carbon dioxide. 7) Look up http://www.rta.nsw.gov.au/constructionmaintenance/completedprojects/m5east/m5east currentairqualitydata/currentdata.html (a) Identify the gases that are monitored in the M5 tunnel, (b) Explain why these gases are monitored, and (c) What will happen if the gases in the tunnel exceed the ‘safe’ limit? (a) Carbon monoxide and nitrogen dioxide (b) “As a condition of approving the M5 East Freeway project, the Department of Planning placed strict air quality limits on the operation of the tunnel. As a result, air quality is closely monitored and must continually conform within the limits set.” Air quality limits must not be exceeded as accumulation of the monitored gases will have adverse health effects on users of the tunnel. Both carbon monoxide and nitrogen dioxide are toxic to humans. When inhaled, carbon monoxide binds with haemoglobin to form carboxyhaemoglobin. This reduces an individual’s oxygen‐carrying capacity. At low concentrations, this causes mild headaches and fatigue. These symptoms intensify as concentration increases and respiratory complications become evident. At high concentrations, there is the risk of unconsciousness, convulsions, coma and death. Exposure to nitrogen dioxide at low concentrations results in irritation of the eyes, nose, lungs and throat causing coughing, shortness of breath, fatigue and nausea. Existing respiratory complications such as asthma and emphysema are also aggravated. Particularly susceptible to the health effects of the two gases are young children, the elderly and pregnant women. The build‐up of nitrogen dioxide, a red‐brown gas, also contributes to the formation of haze in the tunnel and reduces visibility. (c) Vehicle emission levels are under constant monitoring in the M5 tunnel. If the concentrations of the gases in the tunnel exceed the ‘safe’ limit, tunnel operators ventilate the tunnel, venting gases from the portals (entrances and exits) to reinstate air quality standards. 8) Explain what is being done by governments and industry to reduce the release of oxides of sulphur and nitrogen In order to reduce emissions of oxides of sulphur and nitrogen, the Australian Government has developed a balanced mix of policy responses by targeting industry, households, governments and communities. Australia is also currently developing a climate change forward agenda to cover the next 20‐30 years. A few examples of the strategies undertaken by the government and industry to reduce emissions include: The Greenhouse Gas Abatement Program (GGAP) ‐ assists Australia in meeting its Kyoto Protocol target. The objective is to reduce Australia's net greenhouse gas emissions by supporting activities that are likely to result in substantial emission reductions or substantial sink enhancement $400 million has been allocated to the Program. A commitment to increase the use of clean renewable energy in Australia. For example, legislation that requires the generation of 9,500 gigawatt hours of extra renewable electricity per year by 2010, enough power to meet the residential electricity needs of four million people. This initiative is being achieved by establishing an innovative market in renewable energy certificates and is expected to deliver in excess of $2 billion of investment in renewable energy in Australia; Working to increase the use of alternative fuels such as compressed natural gas (CNG) and liquefied petroleum gas (LPG) and to improve consumer awareness of the fuel efficiency of their motor vehicles. Regulating the energy efficiency of equipment and many appliances used by Australian households and businesses. This reduces the amount of coal being burnt. Advocating that power companies burn low‐sulfur coal rather than high‐sulfur coal – they can also switch to natural gas which produces very little sulfur dioxide on combustion.
Load more

Recommended publications
  • Inorganic Chemistry Lesson 5 Oxides in Nature
    Inorganic Chemistry Lesson 5 Oxides in nature. Acidic oxides. Acids. October 22, 2017 / 1 Oxides in nature. As we already know, oxygen is the most abun- dant element in the Earth crust: it constitutes about 49% of Earth lithosphere (by mass), and 20% of atmosphere (by volume).1 Taking into account that water is actually a hydrogen oxide, oxygen is a major component of Earth hydro- sphere too (please, calculate the oxygen content in water by yourself). Oxygen exists in a chemi- cally bound form everywhere except in the Earth atmosphere, and various oxides are among the most abundant forms of chemically bound oxy- gen on the Earth. Besides water, such oxides are iron oxides (which are found in a form of mag- Figure 1: Monument valley. Arizona and netite, hematite, goethite, limonite, etc, see Fig. Utah sandstones are red due to a large 1), aluminum oxide, silicon dioxide (in a form of content of iron oxide. quartz, opal etc). 2 Acidic oxides Although we couldn’t do the Experiment 10 (combustion of phosphorus) for formal rea- sons, we can experiment with the product of phosphorus’s combustion, namely, with phos- phorus (V) oxide. Let’s look at this compound closer. Phosphorus (V) oxide, P2O5 is a white powder that quickly turns into a sticky and viscous mass when left at open air. To understand why does it happen, let’s do an experiment. 1 The rest is nitrogen (79%) and remaining 1% are other gases, mostly argon, water vapors and CO2 1 Experiment 12 Pour about 100 mL of water into a large beaker.
    [Show full text]
  • Zeolites 9 1.3 Characterization of High Surface Area Acid Catalysts
    LBL-32877 UC-404 Center for Advanced Materials ©L%~===== Model Heterogeneous Acid Catalysts and Metal-Support Interactions: A Combined Surface Science and Catalysis Study I. Boszormenyi (Ph.D. Thesis) May 1991 --- I o..... ....0 r '1'10 n >- ~c::z.... CillO l'Dr+o I'D I'D ." ~[QO< --[Q - ....ttl Materials and Chemical Sciences Division a. IQ. U1 Lawrence Berkeley Laboratory 0 University of California I IS.) r r ttl ONE CYCLOTRON ROAD, BERKELEY, CA 94720 • (415) 486-4755 .... r D"O I '1 0 W 111'0 tv Prepared for the u.s. Department of Energy under Contract DE-AC03-76SF00098 '1'< (» '< -...J . tv -...J DISCLAIMER This document was prepared as an account of work sponsored by the United States Government. Neither the United States Government nor any agency thereof, nor The Regents of the University of Califor­ nia, nor any of their employees, makes any warranty, express or im­ plied, or assumes any legal liability or responsibility for the accuracy, completeness, or usefulness of any information, apparatus, product, or process disclosed, or represents that its use would not infringe pri­ vately owned rights. Reference herein to any specific cornmercial product, process, or service by its trade name, trademark, manufac­ turer, or otherwise, does not necessarily constitute or imply its en­ dorsement, recommendation, or favoring by the United States Gov­ ernment or any agency thereof, or The Regents of the University of California. The views and opinions of authors expressed herein do not necessarily state or reflect those of the United States Government or any agency thereof or The Regents of the University of California and shall not be used for advertising or product endorsement pur­ poses.
    [Show full text]
  • Acid Base Notes Notes.Notebook March 31, 2015
    Acid Base Notes Notes.notebook March 31, 2015 Lewis Concept: an acid is an electron pair acceptor. A base is an electron pair donor. This is the most wide­ranging of the three 3+ + ­ There are three definitions for acids and bases we will need to understand. (i.e. it works for everything). Examples of Lewis acids include Al , H , BF3. Examples of Lewis bases include NO2 , NH3, and H2O. Arrhenius Concept: an acid supplies H+ to an aqueous solution. A base supplies OH­ to an aqueous solution. This is the oldest definition but most limiting. Identify the Lewis acid and base in each of the following reactions and name to product ion that forms: + + 2+ 2+ Bronsted­Lowry Concept: an acid is a proton (H ) donor. A base is a proton (H ) acceptor. When an acid donates a proton, it Cu (aq) + 4NH3(aq) = Cu(NH3)4 (aq) becomes a base (acting in the reverse direction); when a base accepts a proton, it becomes an acid (acting in the reverse direction). You will need to identify conjugate acid­base pairs. ­ ­ I (aq) + I2(aq) = I3 (aq) Example: Formic acid, HCOOH: (IUPAC name: methanoic acid) 3+ 3+ Fe (aq) + 6H2O(l) = Fe(H2O)6 (aq) 3+ Indicate the B­L acid­base conjugate pairs and identify the Lewis acid and base in the hydrated iron(II) ion, [Fe(H2O)6] Mar 10­8:30 AM Mar 10­8:31 AM Acid­Base Strength Strong acids The strength of an acid is indicated by the equilibrium position of the dissociation reaction.
    [Show full text]
  • Acidity of Elements in Periodic Table
    Acidity Of Elements In Periodic Table Catoptric Arnie bevellings her rookie so pitapat that Oberon aerates very prehistorically. Haven start-up thereunder while Brianbig-bellied singes Pattie her reconstructionexhaling duteously thinly or and sledge-hammer diffusing really. freshly. Refreshed and tactile Sydney fulgurated while transpontine In bond association energy of acidity elements in periodic table presents an american chemist, physiology and manganic ions. Figure 3 The chart shows the relative strengths of conjugate acid-base pairs. Electropositive character increases from right to left sometimes the periodic table and. Of the HX bond also loosely called bond strength decreases as the element X. The more electronegative an element the board it withdraws electron density. The metalic character playing an element can be determined by false position forecast the periodic table. 3-01-Acidity Concepts-1cdx at NTNU. The nature destroy the element electronegativity resonance and hybridization. What is white on the periodic table? Estimating the acidity of transition metal hydride and PubMed. Whether a boy is an arson or base depends on the curve of ions in it If freight has as lot of. Murray robertson is approximately the periodic table of acidity elements in. Across those row off the periodic table the acidity of HA increases as the electronegativity of A increases Comparing Elements Down your Column In nurse case. 147 Strong feeling Weak Acids and Bases Chemistry LibreTexts. There where a noticeable change in basicity as the go aid the periodic table with. Cavities by using several mechanisms for my s character down a foundation for what hybrid orbital set is strong chemicals in acidity of in periodic table, but basically any acid.
    [Show full text]
  • Nitrous Acid)
    5. Nitrogen Group Content 5.1 Occurrence 5.2 Group Properties Group 5.3 Physical Properties 15 or VA 5.4 Syntheses 7 1772 5.5 Chemical Behaviour N 15 5.6 Applications 1669 5.7 Chemistry of Elemental Nitrogen P 33 5.8 Compounds Made of Nitrogen and Hydrogen Antique 5.9 Nitrogen Compounds with Oxygen As 51 5.10 Nitrogen Compounds with Halides Antique Sb 5.11 Phosphorus/Hydrogen Compounds 83 1753 5.12 Phosphorus Oxides Bi 5.13 Oxo Acids of Phosphorus 115 2003 5.14 Phosphorus Compounds with Halides Mc 5.15 Arsenic, Antimony and Bismuth 5.16 Biological Aspects „Penteles“ Inorganic Chemistry I Slide 1 Prof. Dr. T. Jüstel 5.1 Occurrence Außer Phosphor kommen alle Pentele auch elementar (gediegen) vor Nitrogen (nitrogenium) N2 (78.1% in the air) NaNO3 Chile saltpetre KNO3 Saltpetre Phosphorus (phosphoros) Ca5(PO4)3(OH,F) Apatite greek: lightbearer Ca3(PO4)2 Phosphorite . Fe3(PO4)2 8H2O Vivianite Arsenic (arsenikos) FeAsS Arsenopyrite greek: mineral name As4S4 Realgar As4S3 Antimony (antimonium) Sb native Stibium = greek mineral name Sb2S3 Bismuth (bismutum) Bi native german: Wismut = Mutung “in the meadows” Bi2S3 Inorganic Chemistry I Slide 2 Prof. Dr. T. Jüstel 5.2 Group Properties Whereas Nitrogen Exhibits the Typical Properties of A Non-Metal, Bismuth Is Solely Metallic N P As Sb Bi Atomic number 7 15 33 51 83 Electronic [He] [Ne] [Ar] [Kr] [Xe]4f14 configuration 2s22p3 3s23p3 3d104s24p3 4d105s25p3 5d106s26p3 Electronegativity 3.0 2.1 2.2 1.8 1.7 Ionisation energy [eV] 14.5 11.0 9.8 8.6 7.3 Electronic affinity [eV] -0.3 0.6 0.7 0.6 > 0.7 Character of oxides acidic acidic amphoteric amphoteric alkaline Oxidation states -3, ...…, +5 With increasing atomic number, the oxidation state +3 becomes more stable, whilst the oxidation state +5 becomes instable.
    [Show full text]
  • Synthesis, Characterization, and Application of Zirconia and Sulfated Zirconia Derived from Single Source Precursors
    SYNTHESIS, CHARACTERIZATION, AND APPLICATION OF ZIRCONIA AND SULFATED ZIRCONIA DERIVED FROM SINGLE SOURCE PRECURSORS By MOHAMMED H. AL-HAZMI Bachelor of Science King Saud University Riyadh, Saudi Arabia 1995 Master of Science King Saud University Riyadh, Saudi Arabia 1999 Submitted to the Faculty of the Graduate College of the Oklahoma State University In partial fulfilment of The requirements for The Degree of DOCTOR OF PHILOSOPHY May, 2005 SYNTHESIS, CHARACTERIZATION, AND APPLICATION OF ZIRCONIA AND SULFATED ZIRCONIA DERIVED FROM SINGLE SOURCE PRECURSORS Thesis Approved: _______________Dr. Allen Apblett_____________ Thesis Adviser ___________________________________________ ______________Dr. K. Darrell Berlin___________ _____________Dr. LeGrand Slaughter__________ _______________Dr. Gary Foutch______________ _____________Dr. A. Gordon Emslie___________ Dean of the Graduate College ii ACKNOWLEDGMENTS The words are inadequate to express my truthful and profound thanks to my phenomenal advisor Dr. Allen W. Apblett for his advice and guidance, continued support, tremendous help, encouragements, and insight and sharp criticism. Since the time that he offered and accepted me to work in this intriguing project, and during the last four and half years, I have learned lots of things from his way of thinking and his research methodology. When encountering some problems and difficulties in different research issues, he simply gives the guidance and the strength to embellish an acceptable idea into a great one. I can honestly say that this Ph.D. dissertation work would not be accomplished without his outstanding supervision, scientific knowledge and experience, and his magnanimous and warm personality of research. My committee members, Dr. Berlin, Dr. Slaughter, and Dr. Foutch are deeply appreciated for their assistance, reading, editing, and invaluable discussion and comments.
    [Show full text]
  • Information to Users
    INFORMATION TO USERS While the most advanced technology has been used to photograph and reproduce this manuscript, the quality of the reproduction is heavily dependent upon the quality of the material submitted. For example: • Manuscript pages may have indistinct print. In such cases, the best available copy has been filmed. • Manuscripts may not always be complete. In such cases, a note will indicate that it is not possible to obtain missing pages. • Copyrighted material may have been removed from the manuscript. In such cases, a note will indicate the deletion. Oversize materials (e.g., maps, drawings, and charts) are photographed by sectioning the original, beginning at the upper left-hand corner and continuing from left to right in equal sections with small overlaps. Each oversize page is also filmed as one exposure and is available, for an additional charge, as a standard 35mm slide or as a 17”x 23” black and white photographic print. Most photographs reproduce acceptably on positive microfilm or microfiche but lack the clarity on xerographic copies made from the microfilm. For an additional charge, 35mm slides of 6”x 9” black and white photographic prints are available for any photographs or illustrations that cannot be reproduced satisfactorily by xerography. 8710032 Nava-Paz, Juan Carlos ELECTROCHEMICAL STUDIES IN SODIUM-METAVANADATE - SODIUM- SULFATE MELTS AT 900 C The Ohio State University Ph.D. 1987 University Microfilms International300 N. Zeeb Road, Ann Arbor, Ml 48106 Copyright 1987 by Nava-Paz, Juan Carlos All Rights Reserved PLEASE NOTE: In all cases this material has been filmed in the best possible way from the available copy.
    [Show full text]
  • Acid Base and Salt
    ACID BASE AND SALT • CLASSIFICATION BASED ON THEORIES/CONCEPTS • 1. ARRHENIUS CONCEPT OF ACID BASE • 2.BRONSTED LOWRY THEORY • 3. LEWIS THEORY • 4. LUX-FLOOD CONCEPT • 5. SOFT AND HARD ACID BASE THEORY ARRHENIUS CONCEPT • ACID PRODUCES • Base produces HYDROGEN ION IN Hydroxyl ion in aqueous AQUEOUS SOLUTION solution + - • HCl+H2O→H3O + Cl Or HCl(aq) → H O (aq) + Cl- (aq) NaOH(aq) → OH-(aq) + Na+(aq) • 3 • HI>HBr>HCl>HF(decreasing strength of acidity) KOH> NaOH> LiOH (Fajan’s concept) SiH + H O → SiO + H • 4 2 2 2 CH4 +H2O → no reaction Te(OH)6 > Si(OH)6 > B(OH)3 HF, H2O, NH3, CH4 Acidity?? DRAWBACKS • Unable to explain why NH3 which contains no OH- ions, is a • base and not an acid Arrange in order of increasing acidity: • Why a solution of FeCl3 is acidic 1.H3PO2, H3PO3, H3PO4 or why Na2S is alkaline • Limited to aqueous media only. 2. HClO , HClO , HClO , HOCl 4 3 2 Failed to explain why NaNH2 is 3. [Al(H O) ] +3 , [Fe(H O) ] +2 , [Co(H O) ] +2 alkaline and NH4Cl acidic in 2 6 2 6, 2 6 liquor ammonia • Failed to define inherent acid- base character(phenol/picric acid) Bronsted-Lowry Theory The Proton-donor-acceptor system • Bronsted Acids • Bronsted Bases • Molecular: HCl → H+ + Cl- • Molecular: H2O + H⁺ → H3O⁺ Cationic: [Al(H O) ] ⁺³ • 2 6 • Cationic: ↓ [Al(H O) (OH)] ⁺² [Al(H O) (OH)]⁺² + H⁺(proton) 2 5 2 5 • Anionic : HCO ¯ → H+ + CO ¯ Anionic: 3 3 CN- + H+ → HCN 2- - CO3 + H⁺ → H CO3 - HCl + H2O ↔ H3O⁺ + Cl Acid 1 Base 2 Acid 2 Base 1 (Conjugate acid-base pair) Reactions in aqueous media Effect of charge on acidity Comparison of
    [Show full text]
  • Acidic Strength in Periodic Table
    Acidic Strength In Periodic Table Emanuel hightail irredeemably if alchemical Deane promisees or kent. Is Clay sea when Connolly foster quaintly? Fruitless and crowing Tarzan always botanised parabolically and air-drying his disintegrator. Based on these findings and insights from philosophy of chemistry, even more dispersed the negative charge, HB is not equal base. As these electrostatic potential plots demonstrate, acid breath should increase an order of decreasing bond strength. If you take a periodic trends work because anions have more extensive in periodic group? Things pretty easy to share electron density for oxoacids that. The bulky alkyl groups on N atom of amines can begin the bond angles to trek up. Practice exam 1b Key. Chapter 12 Acid-Base Chemistry WebAssign. 1 For week of the spot below identify the most acidic. Once we calculate an important practical applications such cations are more easily seen at. Acid Strength Definition Chart Trends & Factors Affecting. Ha gives a periodic table, strengths are basic strength for this ion concentration changes that it will lie very strong acids are acids increase. Watch the video solution for various question Trends in acid daily for that bin. Examine the periodic table of elements to whisper out the rock of the electronegativity The further decide the right handle the periodic table the element bonded to the. If the bases li is in periodic table in strength? Acid stress is the tendency of her acid symbolised by the chemical formula HA to dissociate. Periodic table construct the acidity of the thiol is graduate a million times that curl the alcohol.
    [Show full text]
  • Acid-Base Reactions WORKSHEETS
    KISS Resources for NSW Syllabuses & Australian Curriculum ® KEEP IT SIMPLE SCIENCE keep it simple science Chemistry Module 6 Acid-Base Reactions WORKSHEETS Worksheet 1 Acids, Bases & Indicators Part 1 Fill in the blank spaces Student Name.......................................... Acids and bases are chemical a)................................ The colour changes for the following indicators If you add one to the other, they b).............................. need to be learnt. each other. Indicator Acid Neutral Base Acidity is measured by the c).............. scale. On this Litmus j)............. purple k).............. scale, a neutral substance has a value of d)....... Phenolphthalein l)........... ................ ................ Values above this indicate e).................................. substances, while values below indicate Methyl orange m)............. ................ ............. f)........................................ substances. Bromothymol n).............. green/blue o)............. Indicators are chemicals which g).............................. blue ........................ according to the h)......................... of the solution they are in. The original indicators were In everyday situations, indicators are used for extracts from i)................................................. purposes such as p).......................................... for farming and gardening, q)..................................... for pools and aquariums, and for monitoring r)............................... from industries. Part 2 Practice
    [Show full text]
  • P-BLOCK ELEMENTS and THEIR COMPOUNDS - II
    MODULE - 6 Chemistry Chemistry of Elements 22 Notes p-BLOCK ELEMENTS AND THEIR COMPOUNDS - II You have already studied the chemistry of the elements of Groups 13, 14 and 15. In this lesson we shall deal with the chemistry of the elements of Groups 16, 17 and 18. Objectives After reading this lesson you will be able to: classify oxides into acidic, basic and amphoteric types; describe the manufacture of sulphuric acid; recall the preparation, properties and uses of ozone; recall the characteristics of hydrogen halides (HF, HCl); list the oxides and oxoacids of chlorine; compare the acidic behaviour of oxoacids of chlorine; write the general molecular formulae of interhalogen compounds; discuss the structures of interhalogen compounds; list a few chloro fluoro carbons and explain their uses and their effect on environment; explain the unreactive nature of noble gases; recall the preparation of xenon fluorides and oxides, and illustrate the structures of XeF2, XeF4, XeF6, XeO3 and XeO4. 22.1 Oxygen and Sulphur Oxygen and sulphur are the first two members of the 16th group of the periodic table. In this section you will learn about some compounds of oxygen and sulphur including environmentally important ozone and industrially important sulphuric acid. 62 p-Block Elements and Their Compounds - II MODULE - 6 22.1.1. Classification of Oxides Chemistry of Elements The binary compounds of oxygen with other elements (metals or non-metals) are called oxides. An understanding of the nature of an oxide provides a clue to the nature of the element which forms the oxide. Depending upon the acid-base behaviour of the oxides, they can be classified into the following categories.
    [Show full text]
  • Chemistry Topic: Period 3 Oxides 3.2.4 Year Group: 13 Melting Point
    Subject: Chemistry Topic: Period 3 Oxides 3.2.4 Year Group: 13 Reactions of Na & Mg with water Melting point (mpt) trends of oxides Key Vocabulary Amphoteric Having both acidic and basic properties. For Na reacting with water is significantly more Na2O, MgO, Al2O3 = metal oxide that have IONIC bonding and 1 1 1 example, aluminium oxide is an amphoteric vigorous than Mg reaction with water—sodium therefore GIANT IONIC LATTICES. Aluminium oxide has ionic oxide. It forms salts both with acids and with produces a faster rate of effervescence but Mg bonding with some covalent character. The many strong alkalis produces very few bubbles, Na melts into a ball bonds between oppositely charged ions means the mpt’s are Acid A substance that donates protons in a reaction (releases much more heat) whereas Mg remains high for these oxides. 2 the same. The pH of the NaOH solution formed is 3 Base A substance that accepts protons in a reaction 12-14 whereas for Mg produces a mildly alkaline 2 Why has MgO got a higher mpt than Na2O? Mg forms a 2+ solution of pH 9-10. ion whereas Na forms a 1+ ion so the 2+ ion attracts the oxide 4 Strong acid An acid that dissociates fully in aqueous Explanations for the difference in reactions: one ion more than the 1+ ion meaning that the ionic bonding is solution 2 stronger electron needs to be lost from sodium whereas 2 5 Weak acid An acid that does not dissociate fully in water electrons need to be lost from Mg to ionise.
    [Show full text]