Melting and boiling points show no definite trends in the three transition series.
|
|
|
- Ashlie Watts
- 6 years ago
- Views:
Transcription
1 Physicochemical Properties a. Melting and Boiling Points: Melting and boiling points show no definite trends in the three transition series. The metals having the highest melting and boiling points are towards the middle of each transition series. b. Atomic (Covalent) and Ionic Radii: Atomic and ionic radii values decrease generally, on moving from left to right in the period.
2 The atomic radii for the elements from Cr to Cu are very close to one another. Radii of 5d series elements are virtually the same as those of corresponding members of 4d series due to lanthanoid contraction. c. Ionisation Potentials: First Ionization Potentials: I1 values for the first four 3d block elements (Sc, Ti, V and Cr) differ only slightly from one another. The value of II for Zn is considerably higher. This is due to the extra-stability of 3d 10 level which is completely filled in Zn-atom. Second ionisation potentials: The value of III for Cr and Cu are higher than those of their neighbours. This is due to the fact that the electronic configurations of Cr + and Cu + ions have extra stable 3d 5 and 3d 10 levels.there is a sudden fall in the values of ionisation potentials in going from II B (Zn-group elements) to IIIA sub-group. d. Oxidation States: The higher oxidation state of 4d and 5d series elements are generally more stable than those of the elements of 3d series, In short it may be said that in going down a sub-group the stability of the higher oxidation states increases while that of lower oxidation states decreases. Transition elements cannot form ionic compounds in higher oxidation states because the loss of more than three electrons is prevented by the higher attractive force exerted (on the electrons) by the nucleus e. Colour: Transition elements with partially filled d orbitals form coloured compounds. f. Complex Formation: Transition elements show tendency to form complex compounds due to. Small size and high effective nuclear charge Availability of low lying vacant d orbitals which can accept lone pair of electrons donated by a ligand. g. Catalytic properties: Transition metals and their compounds are known to act as good catalyst due tovariable oxidation state, they form unstable intermediate compounds and provide a new path with lower activation energy for the reaction (Intermediate compound formation theory)
3 In some cases the finely divided metals or their compounds provide a large surface area for adsorption and the adsorbed reactants react faster due to the closer contact(adsorption theory) h. Magnetic Properties: Magnetic moment is which is related to the number of unpaired electrons as follows n = number of unpaired electrons B.M. = Bohr Magneton, unit of magnetic moment More the magnetic moment more is the paramagnetic behaviour i. Formation of Alloys: As the transition elements have similar atomic sizes hence in the crystal lattice, one metal can be readily replaced by another metal giving solid solution and smooth alloys. The alloys so formed are hard and have often high melting point. j. Interstitial Compounds: Transition metals form no. of interstitial compounds, in which they take up atoms of small size e.g. H, C and N in the vacant spaces in the their lattices. The presence of these atoms results in decrease in malleability and ductility of the metals but increases their tensile strength. Potassium Dichromate (K2Cr2O7) a. Preparation It is prepared from the ore called chromate or ferrochrome or chrome iron, FeO.Cr2O3. Steps: 1, Preparation of sodium chromate 4FeO.Cr2O3 + O2 Fe2O3 + 4Cr2O3 4Na2CO3 + 2Cr2O3 + 3O2 4Na2CrO4 + 4CO2 Step: 2, Conversion of sodium chromate into sodium dichromate. 2Na2CrO4 + H2SO4 Na2Cr2O7 + Na2SO4 + H2O
4 Step: 3, Conversion of sodium dichromate into potassium dichromate. Na2Cr2O7 + 2KCl K2Cr2O7 + 2NaCl b. Properties 1. Action of heat: When heated, it decomposed to its chromate 4K2Cr2O7 +Δ 4K2CrO4 + 2Cr2O3 + 3O2 2. Action of alkalis K2Cr2O7 + 2KOH 2K2CrO4 + H2O 2K2Cr2O7 + H2SO4 K2Cr2O7 + K2SO4 + H2O 3. Action of conc. H2SO4 solution (a) In cold conditions K2Cr2O7 + 2H2SO4 2CrO3 + 2KHSO4 + H2O (b) In hot conditions 2K2Cr2O7 + 8H2SO4 2K2SO4 + 2Cr2(SO4)3 + 8H2O + 3O2 4. Oxidising propertiesit is a powerful oxidising agent. In the presence of dil. H2SO4 it furnishes 3 atoms of available oxygen. K2Cr2O7 + 4H2SO4 K2SO4 + Cr2(SO4)3 + 4H2O + 3O Some of the oxidizing properties of K2Cr2O7 are It liberates I2 from KI K2Cr2O7 + 7H2SO4 + 6Kl 4K2SO4 + Cr2(SO4)3 + 3l2 + 7H2O It oxidises ferrous salts to ferric salts K2Cr2O7 + 7H2SO4 + 6FeSO4 K2SO4 + Cr2(SO4)3 + 3Fe2(SO4)3 + 2H2O It oxidises S -2 to S K2Cr2O7 + 4H2SO4 + 3H2S K2SO4 + Cr2(SO4)3 + 7H2O + 3S
5 It oxidises nitrites to nitrates K2Cr2O7 + 4H2SO4 + 3NaNO2 K2SO4 + Cr2(SO4)3 + 3NaNO3 + 4H2O It oxidises SO2 to SO4 2 K2Cr2O7 + H2SO4 + 3SO2 K2SO4 + Cr2(SO4)3 + 3H2O It oxidises ethyl alcohol to acetaldehyde and acetic acid. 5. Chromyl chloride test When heated with conc. HCl or with a chloride in the presence of sulphuric acid, reddish brown vapours of chromyl chloride are obtained. K2Cr2O7 + 4KCl + 6H2SO4 2CrO2Cl2 + 6KHSO4 + 3H2O Thus reaction is used in the detection of chloride ions in qualitative analysis. c. Uses In volumetric analysis for the estimation of Fe 2+ and I -. In chrome tanning in leather industry. In photography and in hardening gelatin film. Potassium Permanganate a. Preparation: It is prepared from the mineral pyrolusite, MnO2. Step:1, Conversion of MnO2 into potassium manganate. 2MnO2 + 4KOH + O2 2K2MnO4 + 2H2O Step:2, Oxidation of potassium manganate into permanganate Chemical oxidation K2MnO4 is oxidised to KMnO4 by bubbling CO2 or Cl2 or ozone into the former. 3K2MnO4 + 2CO2 2KMnO4 + MnO2 + 2K2CO3 Electrolytic oxidation
6 2K2MnO2 + H2O + O 2K2MnO4 + 2KOH b. Properties KMnO4 exists as deep purple prisms. It is moderately soluble in water at room temperature and its solubility in water increases with temperature. (i) Action of heat When heated it decomposes to K2MnO4. 2KMnO4 K2MnO4 + MnO2 + O2 (ii) Action of conc. H2SO4 With cold conc. H2SO4 it gives Mn2O7 which on warming decomposes to MnO2. 2MnO2 + 2H2SO4 Mn2O7 + 2KHSO4 + 2H2O 2Mn2O7 + Δ 4MnO2 + 3O2 With hot Conc. H2SO4 O2 is evolved 4KMnO4 + 6H2SO4 2K2SO4 + 4MnSO4 + 6H2O + 5O2 (iii) Oxidising properties KMnO4 is a powerful oxidizing agent. The actual oxidizing action depends upon themedium i.e. acidic, basic or neutral. (a) In neutral solution, it acts as moderate oxidizing agent. 2KMnO4 + H2O 2KOH + 2MnO2 + 3O Some oxidizing properties of KMnO4 in neutral medium are 2KMnO4 + 3Na2S2O3 + H2O 3K2SO4 + 8MnO2 + 3Na2SO4 + 2KOH 2KMnO4 + 4H2S 2MnS + S + K2SO4 + 4H2O (b) In strong alkaline solution, it is converted into 2KMnO4 + 2KOH 2K2MnO4 + H2O + O Some reaction in alkaline medium are 2KMnO4 + H2O + Kl 2MnO2 + 2KOH + KlO3
7 (c) In acidic medium, Mn +7 is converted into Mn +2 2KMnO4 + 3H2SO4 K2SO4 + 2MnSO4 + 3H2O + 5O Some other reactions are (i) 2KMnO4 + 3H2SO4 + 5H2S K2SO4 + 2MnSO4 + 3H2O + 5S (ii) 2KMnO4 + 5SO2 + 2H2O K2SO4 + 2MnSO4 + 2H2SO4 (iii) 2KMnO4 + 3H2SO4 + 5KNO2 K2SO4 + 2MnSO4 + 3H2O + 5KNO3 (iv) 2KMnO4 + 3H2SO4 + 5C2H2O4 K2SO4 + 2MnSO4 + 8H2O + 10CO2 (v) 2KMnO4 + 8H2SO4 + 10FeSO4 K2SO4 + 2MnSO4 + 5Fe2(SO4)3 + 8H2O (vi) 2KMnO4 + 3H2SO4 + 10Kl K2SO4 + 2MnSO4 + 8H2O + 5l2 c. Uses (i)used in volumetric analysis for estimation of ferrous salts, oxalates, iodides & H2O2. (ii) Used as oxidizing agent in the laboratory as well as in industry. (iii) Used as disinfectant and germicide. Inner Transition Elements The f-block elements are known as inner transition elements because they involve the filling for inner sub-shells (4f or 5f) a. Lanthanides: It consists of elements that follows lanthanum and involve the filling of 4 subshell Electronic Configuration : [Xe] 4f n+1 5d 6s 2 or [Xe] 4f n 5d 1 6s 2 Oxidation State: +3, +2 and +4. Colouration: Many of the lanthanides ions are coloured in solid state as well as in solutions. The colour is due to the f-f transition since they have partly filled f-orbitals. Lanthanide Contraction: The steady decrease in the size of lanthanide ions (M 3+ ) with the increase in atomic no. is called lanthanide contraction.
8 Causes: As we move down the group from left to right in a lanthanide series, the atomic no. increases and for every proton in the nucleus the extra electron goes to 4f orbital. The 4f orbital is too diffused to shield the nucleus effectively, thus there is a gradual increase in the effective nuclear charge experienced by the outer electrons. Consequently, the attraction of the nucleus for the electrons in the outermost shell increases with the increase of atomic number, thus size decreases. Consequence of Lanthanide Contraction: Separation of Lanthanides: Due to the similar sizes of the lanthanides, it is difficult to separate them but due to lanthanide contraction their properties slightly vary (such as ability to form complexes). The variation in the properties is utilized to separate them. Basic Strength of Hydroxide: Due to the lanthanide contraction, size of M 3+ ions decreases and there is increase in covalent character in M OH and hence basic character decreases. Similarity of second and third transition series: The atomic radii of second row transition elements are almost similar to those of the third row transition elements because the increase in size on moving down the group from second to third transition elements is cancelled by the decrease in size due to the lanthanide contraction b. Actinides: It consists of elements that follow Actinium and involve the filling of 5f subshell. These are radioactive substances. 7s 2 is stable configuration for actinides. Show +3,+4,+5,+6 & +7 oxidation state. Lower ionization enthalpies than lanthinoids.
Chemistry STD-XII-Science-Top concepts and Notes on d and f block elements. The d and f-block Elements Top 15 Concepts
The d and f-block Elements Top 15 Concepts 1. d -Block elements: The elements lying in the middle of periodic table belonging to groups 3 to 12 are known as d block elements. Their general electronic configuration
UNIT VIII d & f Block Elements ( 5 : MARKS)
TEACHER RIENTED UNIT VIII d & f Block Elements ( 5 : MARKS) 1) Electronic configuration ) ccurrence and General characteristics of transition elements ) General trends in properties ) Preparation and properties
Electronic Configuration General characteristics of transition elements 1. Atomic and ionic radii 2. Melting and boiling points
The d and f Block Elements Elements from 3 rd group to 12 th group in the Modern Periodic table are called d-block elements. In these elements their last electron enters in the penultimate d- sub shell.
Transition Elements. Electronic Configuration- (n-1)d 1-10 ns 1-2 Physical Properties-
Transition Elements Electronic Configuration- (n-1)d 1-10 ns 1-2 Physical Properties- 1. Shows typical metallic character like high tensile strength, ductility, malleability, high thermal and electrical
DAV CENTENARY PUBLIC SCHOOL, PASCHIM ENCLAVE, NEW DELHI-87
Topic Name : General introduction d- & f- Block Elements (Class-12 Chemistry) The elements, which are placed between s and p block elements in the long fm of periodic table, are called transition elements.
Class XII Chapter 8 The d and f Block Elements Chemistry
Question 8.1: Write down the electronic configuration of: (i) Cr 3+ + (iii) Cu + (v) Co 2 + (vii) Mn 2+ (ii) Pm 3+ (iv) Ce 4+ (vi) Lu 2+ (viii) Th 4+ (i) Cr 3+ : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 3 Or, [Ar]
d and f block elements in Nutshell
d and f block elements in Nutshell 1. The elements lying in the middle of periodic table belong to group 3 to 12 are known as d-block element. d block elements are also called as transition elements 2.General
3. Explain briefly how +2 state becomes more and more stable in the first half of the first row transition elements with increasing atomic number.
1. 1. Write down the electronic configuration of: (i) Cr 3+ (iii) Cu + (v) Co 2+ (vii) Mn 2+ (ii) Pm 3+ (iv) Ce 4+ (vi) Lu 2+ (viii) Th 4+ (a) Cr 3+ 1S 2 2S 2 2P 6 3S 2 3P 6 3d 3 (b) Cu + 1S 2 2S 2 2P
Class XII Chapter 8 The d and f Block Elements Chemistry
Question 8.1: Write down the electronic configuration of: (i) Cr 3+ + (iii) Cu + (v) Co 2 + (vii) Mn 2+ (ii) Pm 3+ (iv) Ce 4+ (vi) Lu 2+ (viii) Th 4+ (i) Cr 3+ : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 3 Or, [Ar]
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
![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](/thumbs/84/89512424.jpg "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
Downloaded from 2. The general electronic configuration of these elements is [Xe] f, d, s.
![Downloaded from 2. The general electronic configuration of these elements is [Xe] f, d, s.](/thumbs/94/119630972.jpg "Downloaded from 2. The general electronic configuration of these elements is [Xe] f, d, s.")
POINTS TO BE REMEMBERED: Chapter: 8 The d and f Block Elements 1. The elements of periodic table belonging to group to are known as d Block elements. 2. The general electronic configuration of these elements
Chapter: 8 The d and f Block Elements
POINTS TO BE REMEMBERED: Chapter: 8 The d and f Block Elements 1. The elements of periodic table belonging to group 3 to 12 are known as d Block elements. 2. The general electronic configuration of these
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
7-OXIDATION, REDUCTION, RED-OX REACTIONS, TYPES
7-OXIDATION, REDUCTION, RED-OX REACTIONS, TYPES 1) In the reaction CuO + NH Cu + N + HO, the oxidation number of N changes from 1) to 0 ) 0 to + ) to + 4) to 0 ) In the reaction MnO 4 MnO, the number of
ICSE Board Class IX Chemistry Paper 5 Solution
ICSE Board Class IX Chemistry Paper 5 Solution SECTION I Answer 1 i. Dalton used the symbol for oxygen and the symbol for hydrogen. Symbol represents gram atom(s) of an element. i Symbolic expression for
d AND f BLOCK ELEMENTS
d AND f BLOCK ELEMENTS Electronic Configuration of Transition Metal/Ions The d-block element is called transition metal if it has partly filled d-orbitals in the ground state as well as in its oxidised
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
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
CHEMISTRY. SCIENCE Paper 2
CHEMISTRY SCIENCE Paper 2 (Two hours) Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading
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
Atoms and Bonding. Chapter 18 Physical Science
Atoms and Bonding Chapter 18 Physical Science 2017-2018 Atoms and Bonding: Chemical Bonding The combining of atoms of elements to form new substances. Bonding of atoms determine a compound s properties.
Question Bank Organic Chemistry II
Question Bank Organic Chemistry II 1. What are saturated and unsaturated hydrocarbons. Classify the following as saturated and unsaturated hydrocarbons. CH 4, C 2 H 2, C 2 H 6, C 3 H 6, C 3 H 4 Ans. Compounds
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.
Question 1: Solution 1:
Book Name: Selina Concise Question 1: Comment, sulphuric acid is referred to as: (a) King of chemicals (b) Oil of vitriol Solution 1: (a) Sulphuric acid is called King of Chemicals because there is no
Patterns in the Chemical World
Topic12 Patterns in the Chemical World Unit 41 Periodic trends in elements and their compounds Unit 42 The transition metals Key C o ncepts Periodic trends in elements and their compounds Periodic variations
CHEMISTRY. SCIENCE Paper 2
CHEMISTRY SCIENCE Paper 2 (Two hours) Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading
Stoichiometry Practice Problems
Name Period CRHS Academic Chemistry Stoichiometry Practice Problems Due Date Assignment On-Time (100) Late (70) 9.1 9.2 9.3 9.4 9.5 Warm-Up EC Notes, Homework, Exam Reviews and Their KEYS located on CRHS
STIOCHIOMETRY Single answer type questions: 21. SO -2
STIOCHIOMETRY Single answer type questions: 1. SO - + S - + I (Calculated amount) X + I -1. Then X in this reaction is a) SO - b) IO -1 c) SO - d) IO -1. A certain quantity of Ammonium chloride is boiled
Chemical Bonding. Comparison of Properties Ionic Compounds Covalent Compounds Metals
Chemical Bonding Comparison of Properties Ionic Compounds Covalent Compounds Metals Essential Questions Why/How do atoms combine with one another to form the vast array of chemical substances that exist?
Unit-8 Equilibrium. Rate of reaction: Consider the following chemical reactions:
Unit-8 Equilibrium Rate of reaction: Consider the following chemical reactions: 1. The solution of sodium chloride and silver nitrate when mixed, there is an instantaneous formation of a precipitate of
Colours in common redox reactions
Colours in common redox reactions Fe 3+ Cr 2 O 7 MnO 4 - Cl 2 Br 2 I 2 Fe 2+ Cr 3+ Mn 2+ Cl - Br - I - Oxidation of metals Cu Fe Zn Mg Na Cu 2+ Fe 2+ Zn 2+ Mg 2+ Na + CHEM 2.7 Assessment For A: link one
ICSE Board Class IX Chemistry Paper 3 Solution
ICSE Board Class IX Chemistry Paper 3 Solution SECTION I Answer 1 i. The number of electrons, that atom can lose, gain or share during a chemical reaction is called its valency. ii. Solute: A solute is
CHEMISTRY PAPER 1999
CHEMISTRY PAPER 1999 (One and a half hours) Answers to this paper must be written on the paper provided separately. You will NOT be allowed to write during the first 15 minutes. This time is to be spent
CHEMICAL BONDING. Dear Reader
CHEMICAL BONDING Dear Reader As you have already studied that the substances exist as discrete units called molecules. These molecules are formed by the combination of atoms. When these atoms combine,
OXIDATION AND REDUCTION
OXIDATION AND REDUCTION IMPORTANT FACTS: IMPORTANT DEFINATIONS Many chemical reactions involve the addition of oxygen or hydrogen to the reactants. The reaction in which oxygen is added is called oxidation
Periodicity SL (answers) IB CHEMISTRY SL
(answers) IB CHEMISTRY SL Syllabus objectives 3.1 Periodic table Understandings: The periodic table is arranged into four blocks associated with the four sublevels s, p, d, and f. The periodic table consists
Redox Worksheet 1: Numbers & Balancing Reactions
Name: Date: Per: Redox Worksheet 1: Numbers & Balancing Reactions Assigning Oxidation Number rules: Elements and Compounds have an oxidation number/total of 0 Group I and II In addition to the elemental
Chemistry 101 Chapter 4 STOICHIOMETRY
STOICHIOMETRY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant is necessary
SUBJECTIVE. O Thus, evaluation of ox. no. of S should be made as a + 3 ( 2) + 2 ( 1) = 0 a = +6
Solved Problems Chemistry: Oxidation and Reduction-1 SUBJECTIVE Problem 1: Determine the oxidation no. of following elements underlined: a) K Cr O 7 b) H SO 5 c) H S O 8 d) NH NO e) Fe O f) KI g) Na S
AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry:
AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry: Water as a solvent Strong and Weak Electrolytes Solution Concentrations How to Make up a solution Types of Reactions Introduction
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
Student Instructions. 1. Ensure that you have blank paper and a Data Booket.. 2. Record all aswers on a separate piece of paper.
Student Instructions 1. Ensure that you have blank paper and a Data Booket.. 2. Record all aswers on a separate piece of paper. 3. Answer keys are provided at the beginning of each section. 4. When you
AP Chemistry Review Packet #3
AP Chemistry Review Packet #3 Warmup Given the reaction N 2 O 3(g) NO (g) + NO 2(g) H = +39.7 kj, predict the effect that each of the following changes will have on the given values N 2 O 3 NO NO 2 Keq
Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary
Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen s electronegativity is high (3.5) and hydrogen s is low (2.1)
Oxidation, Reduction, Red-ox reactions, Types
Oxidation, Reduction, Red-ox reactions, Types 1) Oxidation number is the charge which an atom appears to acquire in a molecule, when all the bonding electrons are counted to more electro negative element.
ICSE Chemistry Model Paper-9
ICSE Chemistry Model Paper-9 Answers to this Paper must be written on the paper provided separately. You will not be allowed to write during the first 15 minutes. This time is to be spent in reading the
Chemistry I: Midterm Review 2014
Chemistry I: Midterm Review 2014 General Stuff 1. Density and formula: density is mass per unit volume The units usually are g/cm 3 or g/l or g/ml m D = V 2. Define Accuracy and precision: Accuracy refers
2.3 Group 7 The Halogens
2.3 Group 7 The Halogens Physical properties of the Halogens: The melting and boiling point of the halogens increases with atomic number due to increased van der Waals (from increased number of electrons).
Hydrated nickel(ii) salts are green in colour. Give the electron configuration of a nickel(ii) ion and hence state why the ion is coloured.
1. This question is about nickel compounds. (a) Hydrated nickel(ii) salts are green in colour. Give the electron configuration of a nickel(ii) ion and hence state why the ion is coloured.......... (b)
CHAPTER 10 ELECTROCHEMISTRY TEXT BOOK EXERCISE Q1. Multiple choice questions. (i) The cathode reaction in the electrolysis of dill. H2SO4 with Pt electrode is (a) Reduction (b) Oxidation (c) Both oxidation
INDIAN SCHOOL MUSCAT THIRD PRELIMINARY EXAMINATION CHEMISTRY ANSWER KEY
Roll Number Code Number 4 / INDIAN SCHOOL MUSCAT THIRD PRELIMINARY EXAMINATION CHEMISTRY ANSWER KEY CLASS: XII Sub. Code: 04 08.0.018 1. P type semiconductor 1. 1. (C H 5 ) N > (C H 5 ) NH > C H 5 NH >
MAHESH TUTORIALS I.C.S.E.
MAHESH TUTORIALS I.C.S.E. GRADE - X (2017-2018) Exam No. : MT/ICSE/SEMI PRELIM - I-SET -A 008 Sulphuric acid, Ammonia, Analytical Chemistry, Organic Chemistry HCl, Nitric acid, Metallurgy Chemistry SCIENCE
Honors Unit 4 Homework Packet
1 Honors Homework Packet Reactions in Aqueous Solutions Part I: Aqueous Solns. Part II: Acid/Base Chemistry Part III: Redox Reactions Name: 2 Molarity of Solutions (pg. 2 & 3) Directions: Solve each of
d- Block Elements
d- Block Elements Short Answer Questions: **1. Explain Werner s theory of coordination compounds with suitable examples A: The important postulates of Werner s theory are: i) In coordination compounds
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
Transition Metals. Thursday 09/10/15. Thursday, September 10, 15
Transition Metals Thursday 09/10/15 Agenda Review assigning oxidation numbers and practice with partners Start topic 13.1 First row d-block elements - Transition Metals Rules for assigning oxidation numbers
ICSE Board Class X Chemistry Board Paper Time: 1½ hrs Total Marks: 80
ICSE Board Class X Chemistry Board Paper 2011 Time: 1½ hrs Total Marks: 80 General Instructions: 1. Answers to this paper must be written on the paper provided separately. 2. You will NOT be allowed to
MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements)
MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements) 1 PERIODS: Period number = Number of basic energy levels = The principal quantum number The horizontal lines in the periodic system
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
YEAR 10 CHEMISTRY TIME: 1h 30min
YEAR 10 CHEMISTRY TIME: 1h 30min NAME: CLASS: Useful data: Q = It. Faraday Constant = 96,500 C mol -1. Use the Periodic table, given below, where necessary. Marks Grid [For Examiners use only] Question
Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material
Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is
Regents review Electrochemistry(redox)
2011-2012 1. Chlorine has an oxidation state of +3 in the compound A) HClO B) HClO2 C) HClO3 D) HClO4 2. What is the oxidation number of iodine in KIO4? A) +1 B) 1 C) +7 D) 7 3. What is the oxidation number
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.
2011 CHEM 120: CHEMICAL REACTIVITY
2011 CHEM 120: CHEMICAL REACTIVITY INORGANIC CHEMISTRY SECTION Lecturer: Dr. M.D. Bala Textbook by Petrucci, Harwood, Herring and Madura 15 Lectures (4/10-29/10) 3 Tutorials 1 Quiz 1 Take-home test https://chemintra.ukzn.ac.za/
d & f BLOCK ELEMENTS
d & f BLOCK ELEMENTS Q1. Cu(I) ion is not stable in an aqueous solution. Why? Ans. Cu + (aq) Cu(s) + Cu 2+ (aq) Thus Cu(I) ion undergoes disproportionation in aqueous medium because Cu 2+ is more stable
MC 17 C - 6 SECTION - I
SECTION - I (40 marks) Compulsory : Attempt all questions from this section. Question 1. (a) Name the gas in each of the following : An alkaline gas which gives dense white fumes with hydrogen chloride.
Oxidation numbers. and. balancing equations
Oxidation numbers and balancing equations Oxidation was originally named for dealing with processes where oxygen was transferred during reactions Oxidation was originally named for dealing with processes
Chemical Bonding: Chemical Formulas HL
Name: Chemical Bonding 5. Chemical Bonding: Chemical Formulas Ionic Bonding Covalent Bonding Electronegativity Shapes of Molecules and Intermolecular Forces Objectives -understand that compounds can be
CHEMISTRY
CHEMISTRY PAPER 1 (THEY) (Maximum marks: 70) (Time allowed: Three hours) (Candidates are allowed additional 15 minutes for only reading the paper. They must NOT start writing during this time.) All questions
Questions Booklet. UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION. Level 3 Applied Science. Name:.. Teacher:..
Level 3 Applied Science UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION Questions Booklet Name:.. Teacher:.. Level 3 Applied Science 2017-2018 Unit 1 (Chemistry) 1 1. State the relative
Ionic Bonding (Ch.7) Covalent Bonding (Ch.8) Metallic Bonding
Unit 3: Chemical Bonding Outline Ionic Bonding (Ch.7) Valence electrons Positive and negative ions and transition metal ions Ionic bonding: Charge on compounds Ionic compounds characteristics Writing ionic
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
(c) Na is deposited at the cathode (d) Na appears at the anode
year chemiry n0tes new CHAPTER 10 ELECTROCHEMISTRY MCQS Q.1 Electrolysis is the process in which a chemical reaction takes place at the expense of (a) chemical energy (b) electrical energy (c) heat energy
Part A Unit-based exercise
Topic 2 Microscopic World I / Microscopic World (Combined Science) Part A Unit-based exercise Unit 5 Atomic structure Fill in the blanks 1 atoms 2 solids; liquids; gases 3 metals; metalloids; non-metals
ELECTRON CONFIGURATION AND THE PERIODIC TABLE
ELECTRON CONFIGURATION AND THE PERIODIC TABLE The electrons in an atom fill from the lowest to the highest orbitals. The knowledge of the location of the orbitals on the periodic table can greatly help
CHEMISTRY REVIEW REVIEW WORKSHEET
The student should be able to:. Describe the classification of matter. 2. Describe the conservation of mass. 3. Identify products and reactions in a chemical equation. 4. Describe the structure of an atom
- Chapter 7 - Periodic Properties of the Elements
- Chapter 7 - Periodic Properties of the Elements Summary 7.1 Development of the periodic table 7.2 Effective nuclear charge 7.3 Size of atoms and ions 7.4 Ionization energy 7.5 Electron affinities 7.6
CLASS 12th. d&f-block Elements
CLASS 12th d&f-block Elements 01. Introduction All transition elements belong to d-block. Zn, Cd, and Hg are not transition elements and are called non-typical transition elements or pseudo transition
9.1.2 AQUEOUS SOLUTIONS AND CHEMICAL REACTIONS
9.1.2 AQUEOUS SOLUTIONS AND CHEMICAL REACTIONS Work directly from Zumdahl (Chapter 4). Work through exercises as required, then summarise the essentials of the section when complete. To understand the
Nihal İKİZOĞLU. MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements) kimyaakademi.com 1
MOSELEY and MODERN PERIODIC TABLE (designed by atomic numbers of elements) kimyaakademi.com 1 PERIODS: Period number = Number of basic energy levels = The principal quantum number The horizontal lines
PERIODIC PROPERTIES OF THE ELEMENTS
PERIODIC PROPERTIES OF THE ELEMENTS DEVELOPMENT OF PERIODIC TABLE Elements in the same group generally have similar chemical properties. Properties are not identical, however. DEVELOPMENT OF PERIODIC TABLE
Reactions in Aqueous Solution
Reactions in Aqueous Solution Chapter 4 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A solution is a homogenous mixture of 2 or more substances The solute
THE s- BLOCK ELEMENTS General electronic configuration- [ noble gas] ns 1-2
![THE s- BLOCK ELEMENTS General electronic configuration- [ noble gas] ns 1-2](/thumbs/75/71696980.jpg "THE s- BLOCK ELEMENTS General electronic configuration- [ noble gas] ns 1-2")
THE s- BLOCK ELEMENTS General electronic configuration- [ noble gas] ns 1-2 GROUP 1 ELEMENTS : ALKALI METALS General electronic configuration- [ noble gas] ns 1 Members- Li, Na, K, Rb, Cs, Fr Atomic and
Electronic Structure and Reactivity of the Transition Metals
Ashley Robison My Preferences Site Tools Popular pages MindTouch User Guide FAQ Sign Out If you like us, please share us on social media. The latest UCD Hyperlibrary newsletter is now complete, check it
GCSE Additional Science
GCSE Additional Science Module C5 Chemicals of the Natural Environment: What you should know Name: Science Group: Teacher: each of the statements to help focus your revision: R = Red: I don t know this
Chemistry Study Guide
Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion
(c) dilute solution of glucose (d) chloroform 12 Which one of the following represents the same net reaction as the electrolysis of aqueous H2SO4
1 Electrolysis is the process in which a chemical reaction takes place at the expense of (a) chemical energy (b) electrical energy (c) heat energy (d) none of these 2 Standard hydrogen electrode has an
UNIT 3: The Octet Rule & Chemical Bonding
UNIT 3: The Octet Rule & Chemical Bonding Section 1: The Octet Rule Section 2: Ionic Bonding & Ionic Compounds Section 3: Covalent Bonding & Molecules Section 4: VESPR & Molecular Polarity Section 5: The
ICSE Board Class X Chemistry Board Paper 2014 Solution SECTION I
ICSE Board Class X Chemistry Board Paper 2014 Solution SECTION I Answer 1 1) D 2) B 3) C 4) A 5) C 6) A 7) D 8) C 9) A 10) D 11) 1 12) Sodium ethoxide 13) CaO is alkaline 14) Downward displacement of air
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)
CHEMISTRY HIGHER LEVEL
*P15* PRE-LEAVING CERTIFICATE EXAMINATION, 2009 CHEMISTRY HIGHER LEVEL TIME: 3 HOURS 400 MARKS Answer eight questions in all These must include at least two questions from Section A All questions carry
Chapter 23. Transition Metals and Coordination Chemistry
Chapter 23 Transition Metals and Coordination Chemistry The Transition Metals: Exact Definition Transition metal: An element whose atom has an incomplete d subshell or which can give rise to cations with
Chapter 4: Reactions in Aqueous Solutions
Chapter 4: Reactions in Aqueous Solutions Water 60 % of our bodies heat modulator solvent for reactions covers 70% of Earth Chapter 4 3 types of reactions that occur in H 2 O 1. precipitation 2. acid-base
Another substance, called a reducing agent, causes or promotes the reduction of a metal compound to an elemental compound.
Electrochemistry Oxidation and Reducation The technology of metalurrgy has allowed humanity to progress from the Stone Age, through the Bronze Age and the Iron Age to modern times. Very few metals exist
NOBLE GASES. 1. Oxygen and Xenon have similar. a. Atomic size b. Ionization energy c. Electron affinity d. Electronegativity
NOBLE GASES 1. Oxygen and Xenon have similar a. Atomic size b. Ionization energy c. Electron affinity d. Electronegativity 2. Which of the following is least soluble in water? a.neon c.krypton b. Argon
The Periodic Table. run vertically on the periodic table (up and down).
Lesson Objective: The Periodic Table Science 8.5B Interpret the arrangement of the Periodic Table, including groups and periods, to explain how properties are used to classify elements 8.2E Analyze data
CHEM 122 Unit 1 Introduction to Group Chemistry
DEPARTMENT OF CHEMISTRY FOURAH BAY COLLEGE UNIVERSITY OF SIERRA LEONE CHEM 122 Unit 1 Introduction to Group Chemistry CREDIT HOURS 2.0 MINIMUM REQUIREMENTS C6 in WASSCE Chemistry or equivalent Pass in
Ionic Compounds and Metals
Ionic Compounds and Metals Chapter 7 Ch. 7.1 Chemical bond Cation Anion Vocabulary Ch. 7.2 Ionic bond Ionic compound Binary compound Crystal lattice Electrolyte Lattice energy 2 Objectives Define a chemical
(g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (c) Chromium(III) sulfate: ; (h) Dinitrogen tetroxide:
1. Name each of the following compounds: (a) Ca(OCl) 2 : ; (b) (NH 4 ) 3 PO 4 : ; (c) K 2 Cr 2 O 7 : ; (d) HBrO 2 : ; (e) PF 5 : ; (f) B 2 O 3 : ; (g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (i) Na 2 C 2 O 4
Answers for UNIT ONE NAT 5 Flash Cards
Answers for UNIT ONE NAT 5 Flash Cards 1. (a) rate increases (b) rate increases (c) rate increases (d) rate increases 2. Average rate = change in property / change in time Where property = concentration,