[Fe(H 2. ] 3+ [Cr(H 2 O) 6 ]3+ [Al(H 2
|
|
- Silvia Allison
- 5 years ago
- Views:
Transcription
1 Reactions of Inorganic Compounds in Aqueous Solution Metal-aqua ions Metal aqua ions are formed in aqueous solution. Each complex has six water ligands arranged in a octahedral shape. The complex has the same charge as the metal ion as water is a neutral ligand 2 O 2 O O 2 2+ Cu O 2 O 2 O 2 [Cu blue [Co [Fe pink green [Fe [Cr ]3+ [Al Ruby Violet colourless (appears (appears green) Yellow) In solution Cr(III) often appears green and Fe(III) appears yellow/brown due to hydrolysis reactions. The ruby and violet colour is only really seen in solid hydrated salts that contain these complexes. Cr (ruby) Fe (violet) [Zn colourless [Mn Very pale pink [Ni green N Goalby chemrevise.org 1
2 Acidity or hydrolysis reactions The following equilibria happen in aqueous solutions of metal ions. [M + 2 O [M O) 5 (O)] [M + 2 O [M O) 5 (O) + 3 For example, [Cu + 2 O [Cu O) 5 (O)] The equilibria lead to generation of acidic solutions with M 3+ ions, and very weakly acidic solutions with M 2+ ions. The 3 + ions are noticeably more acidic O O 2O O 2O Al + + Al 2O 2O The acidity of [M is greater than that of [M in terms of the greater polarising power (charge/size ratio) of the 3+ metal ion. The greater the polarising power, the more strongly it attracts the water molecule. This weakens the O- bond so it breaks more easily. Lewis acids and bases Definitions: Lewis acid: electron pair acceptor Lewis base: electron pair donator In the formation of complex ions the ligand is the Lewis base because it is donating a pair of electrons in the dative covalent bond and the metal ion is the Lewis acid. Metal aqua ions can also do acidity type reactions with the bases (sodium hydroxide) O -, (ammonia) N 3 and (sodium carbonate) CO 3. Reaction with limited O - and limited N 3 Aqueous complex ions react with limited amounts of sodium hydroxide and ammonia to form coloured precipitates. The colours of the precipitates formed can be used to identify the metal ion Examples Cu blue ppt Co blue Fe Ni Green ppt Mn pale Zn White ppt N Goalby chemrevise.org 2
3 Al (O) 3 (s) white ppt Cr(O) 3 (s). Fe (O) 3 (s) The bases O - and ammonia when in limited amounts form the same hydroxide precipitates. They form in deprotonation acid base reactions [Cu (aq) + 2O - (aq) Cu [Co (aq) + 2N 3 (aq) Co + 2N 4 + (aq) [Ni (aq) + 2O - (aq) Ni [Zn (aq) + 2N 3 (aq) Zn + 2N 4 + (aq) [Cr (aq) + 3O - (aq) Cr (O) 3 (s) [Fe (aq) + 3N 3 (aq) Fe (O) 3 (s) + 3N 4 + (aq) ere the N 3 and O - ions are acting as Bronsted-Lowry bases accepting a proton This process can happen step wise removing one proton at a time. One proton is removed at each step until the hydroxide precipitate is formed. e.g. [Cr (aq) + O - (aq) [Cr O) 5 (O) (aq) + 2 [Cr O) 5 (O) (aq) + O - (aq) [Cr ( ] + (aq) + 2 [Cr ( ] + (aq) + O - (aq) Cr (O) 3 (s) + 2 In some cases if sodium hydroxide is continued to be added until in excess then further deprotonation takes place, and the hydroxide precipitate dissolves. Reaction with excess O - With excess NaO, the Cr, Zn and Al hydroxides dissolve. Cr becomes [Cr(O) 6 ] 3- (aq) ution. Al becomes [Al(O ] - (aq) colourless solution. Zn becomes [Zn(O ] (aq) colourless solution Cr (O) 3 (s) + 3O - (aq ) [Cr(O) 6 ] 3- (aq) Al (O) 3 (s) + O - (aq ) [Al(O ] - (aq) Zn + 2O - (aq ) [Zn(O ] (aq) The hydroxides are classed as amphoteric because they react and dissolve in both acids and bases. + O - [Al(O) 3 ](s) [Al(O ] [Al( - 2 acidic neutral alkaline Cr (O) 3 (s) (aq ) [Cr (aq) Al (O) 3 (s) (aq ) [Al (aq) N Goalby chemrevise.org 3
4 Reaction with excess N 3 With excess N 3 ligand substitution reactions occur with some of the hydroxides and their precipitates dissolve Cu, Co, Zn, Ni and Cr hydroxides all dissolve in excess ammonia Cr becomes [Cr(N 3 ) 6 purple solution Zn becomes [Zn(N 3 colourless solution Ni becomes [Ni(N 3 ) 6 blue solution Co becomes [Co(N 3 ) 6 pale yellow solution Cu becomes [Cu(N 3 deep blue solution [Cu(N 3 [Co(N 3 ) 6 [Ni(N 3 ) 6 The ligands N 3 and 2 O are similar in size and are uncharged. Ligand exchange occurs without a change of co-ordination number for Co, Ni and Cr. Cr(O) 3 (s) + 6N 3 (aq) [Cr(N 3 ) 6 (aq) O - (aq) Co( (s) + 6N 3 (aq) [Co(N 3 ) 6 (aq) O - (aq) This substitution may, however, be incomplete as in the case with Cu. Cu( (s) + 4N 3 (aq) [Cu(N 3 (aq) O - (aq) In these reactions N 3 is acting as a Lewis base donating an electron pair. Reactions with Chloride Ions Addition of a high concentration of chloride ions (from conc Cl or saturated NaCl) to an aqueous ion leads to a ligand substitution reaction. The Cl - ligand is larger than the uncharged 2 O and N 3 ligands so therefore ligand exchange can involve a change of co-ordination number. Addition of conc Cl to aqueous ions of Cu, Co and Ni lead to a change in coordination number from 6 to 4. [CuCl 4 ] yellow/ution [CoCl 4 ] blue solution These are tetrahedral in shape [NiCl 4 ] [Cu + 4Cl - [CuCl 4 ] O [Co + 4Cl - [CoCl 4 ] O N Goalby chemrevise.org 4
5 Reactions with Carbonate solution The 2+ ions react differently to the 3+ ions with carbonate solutions. If + ions are added in sufficient concentrations to carbonate ions the following equilibria are pushed to towards products and CO 2 is produced + + CO 3 CO CO 3-2 CO 2 The metal aqua 2+ ions are acidic but not sufficiently acidic to bring about the changes mentioned above as the following equilibrium does not produce enough + ions [M + 2 O [M O) 5 (O)] So when 2+ metal aqua ions are added to carbonate ions they form coloured carbonate precipitates The 2+ ions with carbonate solution results in MCO 3 ppt being formed Cu = blue/, Co = pink ppt, Fe(II)=, Zn = white ppt, Mn= pink ppt, Ni= Mn 2+ (aq) + CO 3 (aq) MnCO 3 (s) Cu 2+ (aq) + CO 3 (aq) CuCO 3 (s) Fe 2+ (aq) + CO 3 (aq) FeCO 3 (s) Co 2+ (aq) + CO 3 (aq) CoCO 3 (s) [Cu + CO 3 CuCO O [Fe + CO 3 FeCO O [Co + CO 3 CoCO O These are precipitation reactions CoCO 3 CuCO 3 The 3+ ions with carbonate solution form a M(O) 3 ppt and CO 2 gas is evolved. MCO 3 is formed with 2+ ions but M 2 (CO 3 ) 3 is not formed with 3+ ions. The difference is explained by the greater polarising power of the 3+ ion due to its higher charge density. The greater the polarising power, the more strongly it attracts the water molecule. This weakens the O- bond so it breaks more easily, producing a high concentration of + ions. The metal aqua ion reacts releasing + ions and forms the hydroxide precipitate M(O) 3 This acidity decomposes the CO 3 ions CO CO 2 Al forms white ppt of Al(O) 3 + CO 2 Cr (III) forms of Cr(O) 3 + CO 2 Fe(III) forms of Fe(O) 3 + CO 2 2[Cr (aq) + 3CO 3 (aq) 2Cr(O) 3 (s) +3CO [Fe (aq) + 3CO 3 (aq) 2Fe(O) 3 (s) +3CO [Al (aq) + 3CO 3 (aq) 2Al(O) 3 (s) +3CO These are classed as acidity reactions. N Goalby chemrevise.org 5
6 2+ Ion Summary [MCl 4 ] [CuCl 4 ] [CoCl 4 ] blue sol [Zn(O ] colourless sol water Conc Cl - excess O - [M [Cu [Co [Fe [Ni [Mn [Zn Few drops O - or N 3 M( excess N 3 [Cu(N 3 + blue sol pink sol very pale pink sol colourless sol Cu( blue ppt Co( blue ppt Fe( Ni( Mn( light Zn( white ppt deep blue solution [Co(N 3 ) 6 yellow/light brown solution [Ni(N 3 ) 6 blue sol [Zn(N 3 colourless sol Air or 2 O 2 CO 3 Air or 2 O 2 [Co(N 3 ) 6 brown sol MCO 3 CuCO 3 blue/ FeCO 3 CoCO 3 pink ppt ZnCO 3 = white ppt MnCO 3 = pink ppt NiCO 3 = M(O) 3 Fe(O) 3 Co(O) 3 Mn(O) 3 dark Cr 2 O 7 orange sol 3+ Ion Summary + O - [Cr(O) 6 ] 3- [Al(O ] - colourless sol 2 O 2 CrO 4 yellow sol excess O - Few drops [M O - or N 3 excess N M(O) 3 3 [Cr(N3 ) 6 violet sol [Cr [Fe [Al yellow sol colourless sol + Cr(O) 3 Fe(O) 3 Al(O) 3 white ppt CO 3 (+ CO 2 ) N Goalby chemrevise.org 6
Topic 5.5 REACTIONS OF INORGANIC COMPOUNDS IN SOLUTION. Lewis Acids and Bases Hydrated Metal Cations Reactions of Complex Ions
Topic 5.5 REACTINS F INRGANIC CMPUNDS IN SLUTIN Lewis Acids and Bases ydrated Metal Cations Reactions of Complex Ions LEWIS ACIDS AND BASES A Lewis acid is a species which can bond by accepting a lone
5.3.1 Transition Elements
5.3.1 Transition Elements General properties of transition metals transition metal characteristics of elements Ti u arise from an incomplete d sub-level in ions these characteristics include formation
15. Transition Metals General properties of transition metals
15. Transition Metals General properties of transition metals transition metal characteristics of elements Sc u arise from an incomplete d sub-level in ions these characteristics include complex formation,
Transition Metals General properties of transition metals
opyright N Goalby Bancroft's School Transition Metals General properties of transition metals transition metal characteristics of elements Ti u arise from an incomplete d sub-level in atoms or ions these
2. Transition Metals General properties of transition metals
2. Transition Metals General properties of transition metals transition metal characteristics of elements Sc u arise from an incomplete d sub-level in ions these characteristics include complex formation,
17. Transition Metals General properties of transition metals
17. Transition Metals General properties of transition metals transition metal characteristics of elements Sc u arise from an incomplete d sub-level in ions these characteristics include complex formation,
15 THE TRANSITION METALS
15 THE TRANSITION METALS What is the difference between a d-block element and a transition element? Clue: Sc and Zn are not transition elements (see next slide) Write the electronic configurations of the
Q.1 Predict what will happen when SiCl 4 is added to water.
Transition etals F325 1 The aqueous chemistry of cations Hydrolysis when salts dissolve in water the ions are stabilised by polar water molecules hydrolysis can occur and the resulting solution can become
Acids. Lewis Acids and Bases. Lewis Acids. Lewis acids: H + Cu 2+ Al 3+ E5 Lewis Acids and Bases (Session 1) March 19-24
E5 Lewis Acids and Bases (Session 1) March 19-24 Session one Pre-lab (p.151) due 1st hour discussion of E4 Lab (Parts 1and 2A) Session two Lab: Parts 2B, 3 and 4 Acids Bronsted: Acids are proton donors.
Topic 5 Transition Elements Revision Notes
Topic 5 Transition Elements Revision Notes 1) Introduction The d-block is the ten short columns in the middle of the Periodic Table. All of the elements in the d-block have their highest energy (outermost)
(a) Give the formula of the complex responsible for the pink colour in aqueous CoCl 2 and name its shape. Formula...
Q1. This question is about some reactions of cobalt compounds. (a) Give the formula of the complex responsible for the pink colour in aqueous CoCl 2 and name its shape. Formula... Name of shape... (b)
The d -Block Elements
The d-block Elements Introduction d-block elements locate between the s-block and p-block known as transition elements occur in the fourth and subsequent periods of the Periodic Table 2 d-block elements
M1. (a) Yellow (solution) 1. Orange solution 1 SO 4. Yellow / purple (solution) Allow orange / brown (solution) 1. Brown precipitate / solid 1 + 3H 2
M. (a) Yellow (solution) range solution Cr + H + Cr 7 + H Allow equation with H S (b) Yellow / purple (solution) Allow orange / brown (solution) Brown precipitate / solid [Fe(H ) 6 ] + + H Fe(H ) (H) +
Bronsted: Acids are proton donors. Session one Pre-lab (p.151) due 1st hour discussion of E4 Lab (Parts 1and 2A)
E5 Lewis Acids and Bases (Session 1) November 5-11 Acids Bronsted: Acids are proton donors. Session one Pre-lab (p.151) due 1st hour discussion of E4 Lab (Parts 1and 2A) Problem Compounds containing cations
What is the difference between a d-block element and a transition element? Clue: Sc and Zn are not transition elements.
TRANSITION METALS What is the difference between a d-block element and a transition element? Clue: Sc and Zn are not transition elements. Write the electronic configurations of the transition elements
Q.1 Predict what will happen when SiCl 4 is added to water.
Transition etals 1 The aqueous chemistry of cations Hydrolysis when salts dissolve in water the ions are stabilised by polar water molecules hydrolysis can occur and the resulting solution can become acidic
Date: Names: Section: To investigate various chemical equilibria and explain them using Le Chatelier s Principle. Equilibrium I
Chem 1105 EQUILIBRIUM Date: Names: Section: OBJECTIVE: PROCEDURE: To investigate various chemical equilibria and explain them using Le Chatelier s Principle. As in Chem. 1105 lab manual, pp. Equilibrium
THEORIES OF ACIDS AND BASES
THEORIES OF ACIDS AND BASES These notes describe the Arrhenius, and Bronsted-Lowry, theories of acids and bases, and explains the relationships between them. It also explains the concept of a conjugate
Q.1 Predict what will happen when SiCl 4 is added to water.
Transition etals 2815 1 The aqueous chemistry of cations ydrolysis when salts dissolve in water the ions are stabilised by polar water molecules hydrolysis can occur and the resulting solution can become
E5 Lewis Acids and Bases. Acids. Acids. Session one. Session two Lab: Parts 2B, 3 and 4
E5 Lewis Acids and Bases Session one Pre-lab (p.141) due at start of lab. First hour: Discussion of E4 Lab: Parts 1and 2A Session two Lab: Parts 2B, 3 and 4 Acids Bronsted: Acids are proton donors and
Lecture 21 Cations, Anions and Hydrolysis in Water:
2P32 Principles of Inorganic Chemistry Dr. M. Pilkington Lecture 21 Cations, Anions and ydrolysis in Water: 1. ydration.energy 2. ydrolysis of metal cations 3. Categories of acidity and observable behavior
Acid, Bases and Salts (IGCSE Chemistry Syllabus )
Acid, Bases and Salts (IGCSE Chemistry Syllabus 2016-2018) Acid o A compound when dissolved in water produces hydrogen ions (H + ) ; proton (H + ) donor o It turns blue damp litmus paper to red o ph 1
Page 2. Q1. Consider the reaction scheme below and answer the questions which follow.
Q1. Consider the reaction scheme below and answer the questions which follow. (a) A redox reaction occurs when Cu(NO 3) 2 is decomposed by heat. Deduce the oxidation state of nitrogen in Cu(NO 3) 2 and
Inorganic Chemistry Standard answers
Inorganic Chemistry Standard answers 2.1 Periodicity Atomic radius a) Across a Period, atomic radius decreases: Shells: Same number of electron shells Shielding: Similar amount of shielding Protons: Number
1. Electronic configuration of a transition element X in +3 oxidation state is [Ar]3d 5. What is its atomic number? (i) 25 (ii) 26 (iii) 27 (iv) 24
Unit 8 The d- and f- Block Elements I. Multiple Choice Questions (Type-I) 1. Electronic configuration of a transition element X in +3 oxidation state is [Ar]3d 5. What is its atomic number? 25 26 27 24
H H O - : O O. Complex formation. N Goalby chemrevise.org H 2 O OH 2
omplex formation complex :is a central metal ion surrounded by ligands. ligand.: An atom, ion or molecule which can donate a lone electron pair. H 2 H 2 H 2 u H 2 H 2 H 2 o-ordinate bonding is involved
QUESTIONSHEETS INORGANIC CHEMISTRY REACTIONS OF PERIOD 3 ELEMENTS WITH WATER REACTIONS OF PERIOD 3 ELEMENTS WITH OXYGEN
CHEMISTRY QUESTIONSHEETS A2 Level A2 TOPIC 21 INORGANIC CHEMISTRY Questionsheet 1 Questionsheet 2 Questionsheet 3 Questionsheet 4 Questionsheet 5 Questionsheet 6 Questionsheet 7 Questionsheet 8 Questionsheet
Transition metals. This means that Scandium and Zinc are not Transition elements. It also explains why compounds of these are white and not coloured.
Transition metals A d - block element is found between Group 2 and Group 3 on the Periodic table. A Transition element is a d - block element that forms at least one ion with an incomplete d - sub shell.
1 Must be dot-and-cross circles for outer shells NOT needed IGNORE inner shells Non-bonding electrons of N do not need to be shown as a pair.
Question Expected Answers Marks Additional Guidance 1 a i a shared pair of electrons 1 ALLOW any response that communicates electron pair ALLOW shared pairs ii N iii Shape: pyramidal (trigonal) pyramid
Downloaded from
I.I.T.Foundation - XI Chemistry MCQ #10 Time: 45 min Student's Name: Roll No.: Full Marks: 90 Solutions I. MCQ - Choose Appropriate Alternative 1. Molarity is the number of moles of a solute dissolved
100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals.
2.21 Ionic Bonding 100% ionic compounds do not exist but predominantly ionic compounds are formed when metals combine with non-metals. Forming ions Metal atoms lose electrons to form +ve ions. Non-metal
SOLVED PROBLEMS. Problem 1: The chemical reactivity of lanthanides resemble to which other elements of the periodic table?
SOLVED PROBLEMS Board Level Questions Problem 1: The chemical reactivity of lanthanides resemble to which other elements of the periodic table? The chemical reactivity of the starting lanthanides resemble
Part of the practical procedure is given below.
A peptide is hydrolysed to form a solution containing a mixture of amino acids. This mixture is then analysed by silica gel thin-layer chromatography (TLC) using a toxic solvent. The individual amino acids
Required Reading Material.
JF Chemistry 1101 2010 Introduction to Physical Chemistry: Acid Base and Solution Equilibria. Dr Mike Lyons School of Chemistry melyons@tcd.ie Required Reading Material. Silberberg, Chemistry, 4th edition.
CHEM N-3 November Transition metals are often found in coordination complexes such as [NiCl 4 ] 2. What is a complex?
CHEM100 014-N-3 November 014 Transition s are often found in coordination complexes such as [NiCl 4 ]. What is a complex? 8 A complex contains a cation surrounded by ligands which bond to the cation using
What is an acid? What is a base?
What is an acid? What is a base? Properties of an acid Sour taste Turns litmus paper red Conducts electric current Some acids are strong and some are weak Properties of a base Bitter taste Slippery to
Topic 12 Transition Metals Revision Notes
Topic 12 Transition Metals Revision Notes 1) Introduction Transition metals have 4 characteristic properties: they form complexes, they form coloured compounds, they have more than one oxidation state
8.1 Theories of acids and bases
8. Acids and bases 8.1 Theories of acids and bases Sour-tasting substances (acids) have been known for thousands of years. Lavoisiers early theory: Acid= a compound of oxygen and a nonmetal. Arrhenius
voltmeter salt bridge
2012 H2 Chemistry Preliminary Examination Paper 3 Solutions 1 1 (a) (i) 4FeCr 2 O 4 + 8Na 2 CO 3 + 7O 2 2Fe 2 O 3 + 8Na 2 CrO 4 + 8CO 2 a = 8, b = 7, c = 2, d = 8, e = 8 Any dilute acid e.g. dilute H 2
ICSE QUESTION PAPER Class X Chemistry (2016) Solution
ICSE QUESTION PAPER Class X Chemistry (016) Solution Section I 1. Metals are good reducing agents because they are electron donors. Electrovalent compounds have high melting points. (iii) Higher the ph
Chemical Equilibrium: Le Chatelier s Principle Examples of Chemical Equilibria
E6 Chemical Equilibrium: Le Chatelier s Principle Examples of Chemical Equilibria Objective! Observe several interesting and colorful chemical reactions that are examples of chemical systems at equilibrium.!
Solubility Equilibria
Solubility Equilibria Heretofore, we have investigated gas pressure, solution, acidbase equilibriums. Another important equilibrium that is used in the chemistry lab is that of solubility equilibrium.
Final. Mark Scheme. Chemistry CHEM5. (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry
Version General Certificate of Education (A-level) January 20 Chemistry CHEM5 (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry Final Mark Scheme Mark schemes are prepared by the Principal
Acids, Bases and ph Preliminary Course. Steffi Thomas 14/09/2017
Acids, Bases and ph Preliminary Course Steffi Thomas ssthomas@tcd.ie 14/09/2017 Outline What are acids and bases? Can we provide a general definition of acid and base? How can we quantify acidity and basicity?
Concentration Units. Solute CONCENTRATION. Solvent. g L -1. (M, molarity) concentration in. mol / litre of solution. mol L -1. molality. molality.
CHAPTER 4 REACTIONS IN AQUEOUS SOLUTION CONCENTRATION Solute Solvent Concentration Units mass NaCl / unit volume of solution g L -1 (M, molarity) concentration in moles per litre of solution c NaCl c B
E5 Lewis Acids and Bases: Complexation
chem.125/126 review E5 F08 Hourly II page 1 /5 E5 Lewis Acids and Bases: Complexation 1. ACIDITY OF CATIONS (Part 1) Cations are Lewis acids and exist as aquo complex ions in aqueous solution. Example:
1.12 Acid Base Equilibria
.2 Acid Base Equilibria BronstedLowry Definition of acid Base behaviour A BronstedLowry acid is defined as a substance that can donate a proton. A BronstedLowry base is defined as a substance that can
(a) (i) Explain what is meant by the terms transition element, complex ion and ligand,
1. This question looks at the chemistry of transition elements. (a) Explain what is meant by the terms transition element, complex ion and ligand, Discuss, with examples, equations and observations, the
E5 Lewis Acids and Bases: Complexation
chem.125/126 review E5 W09 Hourly II page 1 /5 E5 Lewis Acids and Bases: Complexation 1. ACIDITY OF CATIONS (Part 1) Cations are Lewis acids and exist as aquo complex ions in aqueous solution. Example:
(08) WMP/Jun10/CHEM5
Transition Metals 8 3 Transition metal ions can act as homogeneous catalysts in redox reactions. For example, iron(ii) ions catalyse the reaction between peroxodisulfate (S 2 O 8 2 ) ions and iodide ions.
QUESTIONS: Equilibria AS & AS
QUESTION (2012:2) Phosphorus pentachloride gas, PCl 5 (g), decomposes to form phosphorus trichloride gas, PCl 3 (g), and chlorine gas, Cl 2 (g). The equilibrium can be represented as: PCl 5 (g) Ý PCl 3
... [1] Catalyst:... [1] H 30 N 6. Ni 3+, exists as two optical isomers [2]
1 This question looks at properties of transition elements, ions and complexes. (a) What is the oxidation number of r in the complex ion [rl 5 ] 2?... [1] (b) Write the equation for a reaction catalysed
2. Which of the following salts form coloured solutions when dissolved in water? I. Atomic radius II. Melting point III.
1. Which pair of elements reacts most readily? A. Li + Br 2 B. Li + Cl 2 C. K + Br 2 D. K + Cl 2 2. Which of the following salts form coloured solutions when dissolved in water? I. ScCl 3 II. FeCl 3 III.
4.4. Revision Checklist: Chemical Changes
4.4. Revision Checklist: Chemical Changes Reactivity of metals When metals react with other substances the metal atoms form positive ions. The reactivity of a metal is related to its tendency to form positive
CHEMISTRY Topic #3: Colour in Chemistry Fall 2017 Dr. Susan Findlay See Exercises 12.1 to Fe 2 O 3 Cr 2 O 3 Co 2 O 3 TiO 2.
CdS Fe 2 3 Cr 2 3 Co 2 3 Ti 2 Mn 3 (P 4 ) 2 Fe 3+ Co 2+ Ni 2+ Cu 2+ Zn 2+ CHEMISTRY 1000 iron copper Topic #3: Colour in Chemistry Fall 2017 Dr. Susan Findlay See Exercises 12.1 to 12.3 Cr 2 3 Cu 2 Co
Homework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107
Homework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107 Chapter 15 Applications of Aqueous Equilibria (mainly acid/base & solubility)
Chem 1102 Semester 1, 2011
Chem 1102 Semester 1, 2011 1 Lecture 29-30: Calculations involving K sp and Q (sat solutions of sparingly soluble electrolytes) Common Ion, T, p, solvent effects Enthalpy-entropy interplay Solubility curves
Periodicity 4. Chlorides of the 3 rd period. d-block elements
Periodicity 4 Chlorides of the 3 rd period d-block elements Period 3 oxides Last class, we talked about the trends we see as we move across the period 3 oxides. We saw that the melting points decrease
MAHESH TUTORIALS I.C.S.E.
MAHESH TUTORIALS I.C.S.E. GRADE - X (2017-2018) Exam No. : MT/ICSE/SEMI PRELIM - II - SET -A 020 Periodic Table, Chemical bonding, Acid, Bases and Salts, Practical Work, Mole Concept, Electrolysis Chemistry
Solubility & Equilibrium Unit Review
Solubility & Equilibrium Unit Review This review is worth 3 marks of your total test marks. It must be completed on test day. 3 marks will be given to students who have fully completed this review with
Arrhenius base is one that dissociates in water to form hydroxide ions.
Chemistry Notes: Acids and Bases Arrhenius base is one that dissociates in water to form hydroxide ions. Arrhenius acid is on that dissociates in water to form hydrogen ions (protons). A Bronsted-Lowry
Acids and Bases. CHEM 102 T. Hughbanks. In following equilibrium, will reactants or products be favored? Strong acid (HCl) + Strong base (NaOH)
Acids and Bases According to the Brønsted Lowry theory, all acid base reactions can be written as equilibria involving the acid and base and their conjugates. CEM 102 T. ughbanks All proton transfer reactions
7/16/2012. Chapter Four: Like Dissolve Like. The Water Molecule. Ionic Compounds in Water. General Properties of Aqueous Solutions
General Properties of Aqueous Solutions Chapter Four: TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY A solution is a homogeneous mixture of two or more substances. A solution is made when one substance
4.4. Revision Checklist: Chemical Changes
4.4. Revision Checklist: Chemical Changes Reactivity of metals When metals react with other substances the metal atoms form positive ions. The reactivity of a metal is related to its tendency to form positive
Page 2. Q1. The complex cisplatin acts as an anticancer drug by changing the properties of DNA when it reacts with guanine, a component of DNA.
Q1. The complex cisplatin acts as an anticancer drug by changing the properties of DNA when it reacts with guanine, a component of DNA. When cisplatin is absorbed into the human body, it undergoes a ligand
Acid Dissociation Constant
CE 131 Lecture 37 Lewis Acids and Bases Chapter 16: pp. 800-802. Acid Dissociation Constant C 2 3 2 + 2 3 + + C 2 3-2 [ 3 + ][C 2 3-2 ] K = [ 2 ][C 2 3 2 ] [ 3 + ][C 2 3-2 ] K a = K [ 2 ] = [C 2 3 2 ]
12. Acid Base Equilibria
2. Acid Base Equilibria BronstedLowry Definition of acid Base behaviour A BronstedLowry acid is defined as a substance that can donate a proton. A BronstedLowry base is defined as a substance that can
AP Chemistry. Slide 1 / 39. Slide 2 / 39. Slide 3 / 39. Equilibrium Part C : Solubility Equilibrium. Table of Contents
Slide 1 / 39 AP Chemistry Slide 2 / 39 Equilibrium Part C : Solubility Equilibrium 2014-10-29 www.njctl.org Table of Contents click on the topic to go to that section Slide 3 / 39 Molar Solubility Calculating
D. Ammonia can accept a proton. (Total 1 mark)
1. Which statement explains why ammonia can act as a Lewis base? A. Ammonia can donate a lone pair of electrons. B. Ammonia can accept a lone pair of electrons. C. Ammonia can donate a proton. D. Ammonia
REACTIONS OF PERIOD 3 ELEMENTS WITH WATER
QUESTINSHEET 1 REACTINS F PERID 3 ELEMENTS WITH WATER a) (i) Sodium melts into a ball / heat is given out Effervescence / gas evolved Sodium skates across the surface Ignition may occur Maximum 3 marks
Give the number of protons, neutrons and electrons in this atom of aluminium. Why is aluminium positioned in Group 3 of the periodic table? ...
Q1.An atom of aluminium has the symbol (a) Give the number of protons, neutrons and electrons in this atom of aluminium. Number of protons... Number of neutrons... Number of electrons... (3) (b) Why is
HL Topics 3 and 13 : Periodicity (2)
HL Topics 3 and 13 : Periodicity (2) For each question choose the answer you consider to be the best. 1. An element is in period 3 and group 5 of the periodic table. How many electrons are present in the
CHAPTER 7.0: IONIC EQUILIBRIA
Acids and Bases 1 CHAPTER 7.0: IONIC EQUILIBRIA 7.1: Acids and bases Learning outcomes: At the end of this lesson, students should be able to: Define acid and base according to Arrhenius, Bronsted- Lowry
AP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section
Slide 1 / 91 Slide 2 / 91 AP Chemistry Aqueous Equilibria II: Ksp & Solubility Products Table of Contents: K sp & Solubility Products Slide 3 / 91 Click on the topic to go to that section Introduction
F.Y.B.Sc BIOTECH TOPIC: ACID BASE
F.Y.B.Sc BIOTECH TOPIC: ACID BASE 2016-17 Q.1) Define the following terms: 1)Electrolyte: A substance which forms a conducting solution when dissolved in water is called an electrolyte. 2) Strong electrolyte:
CHAPTER 8 SALTS. NaCl. A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion.
CHAPTER 8 SALTS A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion. The salt consists of two parts, cation from base and anion from acid.
H 2 SO 4. HCl. HNO 3 nitric acid. TOPIC: Acids and Bases. e.g. HCl! H + + Cl - sulphuric acid. hydrochloric acid
TOPIC: Acids and Bases Learn these formulae! H 2 SO 4 sulphuric acid HCl hydrochloric acid Acids, especially concentrated acids, are corrosive: you need eye protection and gloves. HNO 3 nitric acid What
( 1 ) Concept of acid / base
Section 6.2 Ionic Equilibrium Unit 628 ( 1 ) Concept of acid / base The best definition of acids and bases is that proposed by T.M. Lowry and also, independently by J.N. Bronsted in 1923. BronstedLowry
Subject: Trends and Patterns Code: 2815/01 Session: January Year: 2004 Mark Scheme MAXIMUM MARK 45 Mark Scheme ADVICE TO EXAMINERS ON THE ANNOTATION OF SCRIPTS 1. Please ensure that you use the final version
Final. Mark Scheme. Chemistry CHEM5. (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry
Version.2 General Certificate of Education (A-level) January 202 Chemistry CHEM5 (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry Final Mark Scheme Mark schemes are prepared by the
JUNIOR COLLEGE CHEMISTRY DEPARTMENT EXPERIMENT 22 SECOND YEAR PRACTICAL. Name: Group: Date: Cr 3+ (aq)+ 3 OH (aq) Cr(OH) 3(s)
JUNIOR COLLEGE CHEMISTRY DEPARTMENT EXPERIMENT 22 SECOND YEAR PRACTICAL Name: Group: Date: THE CHEMISTRY OF CHROMIUM AND MANGANESE CHROMIUM 1. To a solution of Cr 3+ ions add aqueous sodium hydroxide until
Topic 9.4: Transition Elements Chemistry
Topic 9.4: Transition Elements Chemistry AJC 2009/P3/Q3c,d 1 167 CJC 2009/P2/Q3a-c 2 (a) Cr: 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 1 or [Ar] 3d 5 4s 1 Cr 3+ : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 3 or [Ar] 3d 3 (b)
Fluorine Gas. Chlorine Gas. Bromine Liquid. Iodine Solid
Halogens Fluorine (F 2 ): very pale yellow gas. It is highly reactive Chlorine : ( ) greenish, reactive gas, poisonous in high concentrations Bromine ( ) : red liquid, that gives off dense brown/orange
Periodicity Unit 3 The Periodic Table Physical and Chemical Properties Periodic Trends (period 3) First Row d-block Elements
Periodicity Unit 3 The Periodic Table Physical and Chemical Properties Periodic Trends (period 3) First Row d-block Elements Do You know these terms/phrases? Distinguish between the terms group and period
2 Answer all the questions. 1 Born Haber cycles can be used to determine lattice enthalpies of ionic compounds
2 Answer all the questions. 1 Born Haber cycles can be used to determine lattice enthalpies of ionic compounds. (a) Define, in words, the term lattice enthalpy............. [2] (b) The Born Haber cycle
TRANSITION METALS
C H E M By @DaK_74 TRNSITION METLS CHEM 5 Part 1 Definitions LTEST: Define transition metal, ligand, complex ion, unidentate, bidentate, hexadentate, SUMMRY OF THE WEEK Lewis acid, Lewis base. State the
Chap 17 Additional Aspects of Aqueous Equilibria. Hsu Fu Yin
Chap 17 Additional Aspects of Aqueous Equilibria Hsu Fu Yin 1 17.1 The Common-Ion Effect Acetic acid is a weak acid: CH 3 COOH(aq) H + (aq) + CH 3 COO (aq) Sodium acetate is a strong electrolyte: NaCH
REACTIONS OF ACIDS. J:\Science\Chemistry\Stage 1 Notes\Acids & Bases\Reactionsofacids.doc
REACTIONS OF ACIDS 1. Acids taste sour We do not attempt to taste strong acids as they are too dangerous. They do taste sour, but then they proceed to destroy cells on your tongue and mouth. If you vomit,
Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride
Acids and Bases Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated
Since Q>Ksp, precipitation will occur!
198 Precipitation - also known as the reaction quotient To predict whether a salt at a given concentration will precipitate out, calculate the reaction quotient Q and compare it to the Ksp Example: IF...
Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.
Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when
M1.(a) Must be 1 decimal place 1
M.(a) 64.0 Must be decimal place 7.(%) (= 28.0 00 / Qa) Consequential on their (a) Ignore precision but must be to at least 2 sig fig. (i.e. accept 7 or 7.07) (c) (i) Absorption depends on (proportional
10. Group 2. N Goalby chemrevise.org. Group 2 reactions. Reactions with oxygen. Reactions with water.
10. Group 2 Atomic radius Atomic radius increases down the Group. As one goes down the group, the atoms have more shells of electrons making the atom bigger. Melting points Down the group the melting points
What is an acid? What is a base?
What is an acid? What is a base? Properties of an acid Sour taste Turns litmus paper red Conducts electric current Some acids are strong and some are weak Properties of a base Bitter taste Slippery to
1 Which of the following gives the electronic configurations for a chromium atom and a chromium(ii) ion? A [Ar]3d 4 4s 2 [Ar]3d 4
1 Which of the following gives the electronic configurations for a chromium atom and a chromium(ii) ion? r 2+ [r]3d 4 4s 2 [r]3d 4 [r]3d 5 4s 1 [r]3d 4 [r]3d 4 4s 2 [r]3d 2 4s 2 [r]3d 5 4s 1 [r]3d 3 4s
ICSE Board Class X Chemistry Board Paper 2013 Solution SECTION I
ICSE Board Class X Chemistry Board Paper 2013 Solution SECTION I 1) i. Hydronium ii. Hydroxide iii. Salt iv. Water v. Hydrogen 2) i. C 2 H 6 gas Reaction: ii. Sulphur dioxide gas is evolved. K 2 SO 3 +
Chapter 25 Transition Metals and Coordination Compounds Part 1
Chapter 25 Transition Metals and Coordination Compounds Part 1 Introduction The transition elements are defined as: those metallic elements that have a partially but incompletely filled d subshell or easily
Acids Bases and Salts Acid
Acids Bases and Salts Acid ph less than 7.0 Sour taste Electrolyte Names of Acids Binary acids Contain only 2 elements Begin with hydro; end with ic Ternary acids Ex: H 2 S = hydrosulfuric Contain a polyatomic
The Chemistry of Acids and Bases
The Chemistry of 1 Acids and Bases 2 Acid and Bases 3 Acid and Bases 4 Acid and Bases 5 Strong and Weak Acids/Bases Generally divide acids and bases into STRONG or WEAK ones. STRONG ACID: HNO 3 (aq) +
Oxidation-Reduction Reactions
Oxidation-Reduction Reactions What is an Oxidation-Reduction, or Redox, reaction? Oxidation-reduction reactions, or redox reactions, are technically defined as any chemical reaction in which the oxidation