THE s- BLOCK ELEMENTS General electronic configuration- [ noble gas] ns 1-2
|
|
- Anna Wright
- 6 years ago
- Views:
Transcription
1 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 Ionic Radii- Largest in a particular period Monovalent ions ( M + ) are smaller than the parent atom. On moving down the group, it increases.( increase in no. of shells) Ionisation Enthalpy- Low ( loss of one electron gives stable configuration) On moving down the group, it decreases ( effect of increasing size outweighs the increasing nuclear charge) Hydration Enthalpy- Li + > Na + > K + > Rb + > Cs + It decreases with increase in ionic sizes because as the size increases, charge density decreases. So, Lithium salts are mostly hydrated. E.g. LiCl.2H 2 O PHYSICAL PROPERTIES- Due to large size, they have low density which increases down the group. Low melting and boiling points due to weak metallic bonding ( presence of single valence electron)
2 Alkali metals and their salts impart characteristic colour in the flame ( Heat from the flame excites the outermost electron to a higher energy level. When the excited electron comes back to the ground state, it emits radiation in the visible range) Li - Crimson red, Na- Yellow, K- Violet, Rb Red violet,cs- Blue CHEMICAL PROPERTIES- Highly reactive due to large size and low Ionisation Enthalpy Reactivity Towards Air- They burn in oxygen forming oxides. Li forms monoxide, Na forms peroxide, the other metals form superoxides. ( Superoxide ion is stable with large cations only such as K, Rb, Cs. It is so because large anions are stabilized by large cations through lattice energy effects.) 4Li + O 2 2Li 2 O 2Na + O 2 Na 2 O 2 K + O 2 KO 2 Reactivity Towards Water- Except Li, other members of the group react explosively with water. 2M + 2H 2 O 2M + + 2OH - + H 2 Although Li has most negative E 0 value, its reaction with water is less vigorous than Na ( due to small size and high hydration enthalpy of Li) Reactivity Towards Dihydrogen- 2M + H 2 2MH Metal hydrides are ionic solids.
3 Reactivity Towards Halogens- 2M + X 2 2MX Alkali metal halides are ionic in nature except LiX ( due to small size, charge density is high and so have high polarization capability. LiI is most covalent alkali metal halide) Reducing Nature- Strong reducing agents. The standard electrode potential depends on sublimation enthalpy, ionization enthalpy and hydration enthalpy. M (s) M (g) sublimation enthalpy M (g) M + (g) +e - ionization enthalpy M + (g) + H 2 O M + (aq) hydration enthalpy On moving down the group, E o value becomes more and more negative from Na to Cs. Li has most negative E 0 value and hence most powerful reducing agent. (Due to small size, Li has the highest hydration enthalpy which overcomes the high ionization enthalpy and so has high negative E o.) Solutions in liquid ammonia- The alkali metals dissolve in liquid ammonia giving deep blue conducting solutions. M + (x+y)nh 3 [M(NH 3 )x] + + [e(nh 3 )y] - The blue colour of the solution is due to the ammoniated electron which absorbs energy in the visible region. ( absorbs from red region, so transmitted light is blue in colour)
4 The solutions are paramagnetic and on standing slowly liberate H 2 and so amide is formed. M + (am) + e - + NH 3 (l) MNH 2(am) + ½ H 2 (g) In conc. Solution, the blue colour changes to bronze colour and becomes diamagnetic. GENERAL CHARACTERISTICS OF THE COMPOUNDS OF THE ALKALI METALS I OXIDES AND HYDROXIDES They burn in oxygen forming oxides. Li forms monoxide, Na forms peroxide, the other metals form superoxides. ( Superoxide ion is stable with large cations only such as K, Rb, Cs. It is so because large anions are stabilized by large cations through lattice energy effects.) 4Li + O 2 2Li 2 O [M 2 O] 2Na + O 2 Na 2 O 2 [M 2 O 2 ] K + O 2 KO 2 [MO 2 ] Superoxides are paramagnetic. ( O 2 - is paramagnetic because of one unpaired electron in π* 2p molecular orbital.) Oxides are hydrolysed by water to form hydroxides( white crystalline solids) M 2 O + H 2 O 2M + + 2OH - M 2 O 2 + 2H 2 O 2M + + 2OH - + H 2 O 2 2MO 2 + 2H 2 O 2M + + 2OH - + H 2 O 2 + O 2 The alkali metal hydroxides are the strongest of all bases and dissolve freely in water with evolution of heat.
5 II HALIDES They are prepared by reaction of HX with oxides, hydroxides or carbonates of alkali metals. M 2 O + 2HX MOH + HX M 2 CO 3 + 2HX 2MX + H 2 O MX + H 2 O 2MX + CO 2 +H 2 O They have high negative values of Δ f H o. On moving down the group, Δ f H o value for fluorides become less negative. On moving down the group, Δ f H o value for chlorides, bromides and iodides become more negative. For a given metal, Δ f H o value always become less negative from fluoride to iodide. Trend of m.p. : For the same alkali metal ( due to decrease in lattice enthalpy) the order is : F - > Cl - > Br - > I - For the same halide ion, m.p. decreases from Na to Cs. But m.p. of Lithium halides is low because they are covalent in nature. Solubility in water- Low solubility of LiF due to high lattice enthalpy Low solubility of CsI due to smaller hydration enthalpy of ions. III SALTS OF OXOACIDS- Oxoacids are those in which the acidic proton is on a hydroxyl group with an oxo group attached to the same atom e.g. H 2 CO 3, H 2 SO 4. The alkali metals form salts with all the oxoacids.
6 Carbonates- ( M 2 CO 3 ) They are stable to heat but Li 2 CO 3 is not so stable to heat. Li 2 CO 3 Li 2 O + CO 2 Hydrogen carbonates ( MHCO 3 ) They are also stable to heat. Li does not form solid MHCO 3. Solubility in water- All carbonates and hydrogencarbonates are soluble in water which increases down the group. POINTS OF DIFFERENCE BETWEEN Lithium and other Alkali Metals- 1. Lithium salts are mostly hydrated. E.g. LiCl.2H 2 O whereas other metal chlorides do not form hydrates. 2. Li does not form solid MHCO 3 whereas other alkali metals form. 3. Li does not form ethynide on reaction with ethyne whereas other alkali metals form. 4. Li is least reactive but the strongest reducing agents among all the alkali metals. Points of Similarities between Lithium and Magnesium 1. They react slowly with water. 2. They form nitrides by direct combination with nitrogen. 3. Their carbonates decompose easily on heating. 4. They do not form solid hydrogencarbonates. 5. Their chlorides are deliquescent. LiCl.2H 2 O, MgCl 2.8H 2 O
7 GROUP 2 ELEMENTS : ALKALINE EARTH METALS General electronic configuration- [ noble gas] ns 2 Members- Be 4, Mg 12, Ca 20, Sr 38, Ba 56, Ra 88 Atomic and Ionic Radii- On moving down the group, it increases.( increase in no. of shells) Ionisation Enthalpy- Low ( due to large size of atoms) IE 1 of alkaline earth metals are higher than IE 1 of alkali metals. IE 2 of alkaline earth metals are smaller than IE 2 alkali metals. On moving down the group, it decreases ( effect of increasing size outweighs the increasing nuclear charge) Hydration Enthalpy- Be +2 > Mg +2 > Ca +2 > Sr +2 > Ba +2 It decreases with increase in ionic sizes because as the size increases, charge density decreases. The hydration enthalpies of Gp 2 metal ions are larger than those of Gp.1 ions. So, they are hydrated. E.g. MgCl 2.8H 2 O, CaCl 2.6H 2 O, SrCl 2.6H 2 O, BaCl 2.2H 2 O PHYSICAL PROPERTIES- On moving down the group electropositive character increases. Higher melting and boiling points than the corresponding alkali metals due to smaller sizes.( but not systematic trend) Ca, Sr, Ba metals and their salts impart characteristic colour in the flame.
8 Ca- Brick red, Sr - Crimson red, Ba- Grassy green or Apple green Be and Mg do not impart any colour their electrons are too strongly bound to get excited by flame) CHEMICAL PROPERTIES- Less reactive than alkali metals Reactivity Towards Air- Be and Mg are kinetically inert to oxygen. Powdered Be gives BeO and Be 3 N 2, when burnt in air. Mg, Ca, Sr and Ba give oxides and nitrides. E.g. MgO and Mg 3 N 2. Reactivity Towards Water- Be and Mg are kinetically inert to water. Ca, Sr and Ba react with wate rand form hydroxides. Reactivity Towards Dihydrogen- All the elements except Be form hydrides on heating. M + H 2 MH 2 Reactivity Towards Halogens- M + X 2 MX 2 Reducing Nature- Strong reducing agents. Their reducing power is less than the corresponding alkali meatls. Solutions in liquid ammonia-
9 The alkali metals dissolve in liquid ammonia giving deep blue black solutions. M + (x+y)nh 3 [M(NH 3 )x] [e(NH 3 )y] - The blue blackcolour of the solution is due to the ammoniated electron which absorbs energy in the visible region GENERAL CHARACTERISTICS OF THE COMPOUNDS OF THE ALKALINE EARTH METALS I OXIDES AND HYDROXIDES They burn in oxygen forming monoxides. BeO is covalent and amphoteric. All other oxides are ionic and basic. Oxides react with water to form basic hydroxides except Be which forms amphoteric hydroxide. MO + H 2 O M(OH) 2 These hydroxides are sparingly soluble in water. II HALIDES Be halides are covalent while other halides are ionic in nature. In the vapour phase BeCl2 forms dimer which dissociates at higher temperature. The tendency to form hydrates gradually decreases on going down the group e.g. MgCl 2.8H 2 O, CaCl 2.6H 2 O, SrCl 2.6H 2 O, BaCl 2.2H 2 O
10 III SALTS OF OXOACIDS- Oxoacids are those in which the acidic proton is on a hydroxyl group with an oxo group attached to the same atom e.g. H 2 CO 3, H 2 SO 4. The alkaline earth metals form salts of oxoacids. Carbonates- ( MCO 3 ) They decompose on heating to give oxide and CO 2. MCO 3 MO + CO 2 They are insoluble in water. Sulphates : MSO 4 White solids Stable to heat BeSO 4 and MgSO 4 are readily soluble in water ; The solubility decreases from CaSO 4 to BaSO 4.( high hydration enthalpies of Be 2+ and Mg 2+ overcomes the lattice enthalpy) Nitrates : M(NO 3 ) 2 On moving down the group, tendency to form hydrates decreases with increasing size and decreasing hydration enthalpy. E.g. Mg(NO 3 ) 2 crystallises with 6 H 2 O molecules whereas Ba(NO 3 ) 2 is anhydrous. They decompose on heating 2 M(NO 3 ) 2 2MO + 4NO 2 + O 2 ANOMALOUS BEHAVIOUR OF BERYLLIUM 1. Due to small size and high electronegativity it forms compounds which are covalent and get easily hydrolysed. 2. Max. covalency is 4 due to absence of d orbitals.
11 3.Oxide and hydroxide of Be are amphoteric in nature. DIAGONAL RELATIONSHIP BETWEEN BERYLLIUM AND ALUMINIUM 1. Their chlorides form dimer. 2. Their chlorides are strong Lewis acids and are used as Friedel Craft catalysts. 3. They are not readily attacked by acids because their oxide form a protective film on the surface. 4. They have strong tendency to form complexes. BeF 4 2-, AlF 6 3-
Unit 10 THE s -BLCK ELEMENTS I. Multiple Choice Questions (Type-I) 1. The alkali metals are low melting. Which of the following alkali metal is expected to melt if the room temperature rises to 30 C? Na
More informationClass XI Chapter 10 The s-block Elements Chemistry
Question 10.1: What are the common physical and chemical features of alkali metals? Physical properties of alkali metals are as follows. (1) They are quite soft and can be cut easily. Sodium metal can
More information(4) The metallic bonding present in alkali metals is quite weak. Therefore, they have low melting and boiling points.
The s-block Elements What are the common physical and chemical features of alkali metals? Ans. Physical properties of alkali metalsare as follows. (1) They are quite soft and can be cut easily. Sodium
More informationS-BLOCK ELEMENT (Test-36)
S-BLOCK ELEMENT (Test-36) READ THE INSTRUCTIONS CAREFULLY 1. The test is of 2 hours duration. 2. The maximum marks are 236. 3. This test consists of 70 questions. 4. Keep your mobiles switched off during
More informationDownloaded from
Subject: Chemistry Class: XI Chapter: The s-block Elements Top concepts. The s-block elements of the periodic table are those in which the last electron enters the outermost s-orbital. Elements of group
More informationCHEM 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
More informationChemistry of period II elements
digitalteachers.co.ug Chemistry of period II elements Period 2 consists of the following elements as shown in table 7.1 below. Table 7.1 Period 2 elements Element: Li Be B C N O F Ne Electron Configuration
More informationSummary Term 2 Chemistry STPM Prepared by Crystal Goh AI Tuition Centre
Summary Term Chemistry STPM Prepared by Crystal Goh AI Tuition Centre 017713136 Period 3 elements property Na Mg Al Si P (P 4 ) Type of element Metal Metalloid Non-metal Structure Giant metallic lattice
More informationDAV CENTENARY PUBLIC SCHOOL, PASCHIM ENCLAVE, NEW DELHI - 87
S BLOCK AND P BLOCK ELEMENTS REASONING 1. Explain why is sodium less reactive than potassium? Ionization energy of K < Na i.e. the outermost electron in potassium can be lost easily as compared to sodium
More informationNEET Chemistry Study Material 10. The s-block Elements
NEET Chemistry Study Material 10. The s-block Elements 1. Alkali metals are not found in free state due to their highly reactive nature. This is due to their large size and low ionization enthalpy their
More informationChapter 7. Periodic Properties of the Elements
Chapter 7 Periodic Properties of the Elements periodic table the most significant tool that chemist use for organizing and remembering chemical facts 7.1 Development of the periodic table discovery of
More informationS-BLOCK ELEMENTS. Question 1. What are the common physical and chemical features of alkali metals? Answer: Physical properties of alkali metals:
11 th Chemistry Study Material S-BLOCK ELEMENTS Question 1. What are the common physical and chemical features of alkali metals? Physical properties of alkali metals: Alkali metals have low ionization
More information2. 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.
More information10. 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
More information2.3 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).
More informationFor the element X in the ionic compound MX, explain the meaning of the term oxidation state.
1. (a) By referring to electrons, explain the meaning of the term oxidising agent.... For the element X in the ionic compound MX, explain the meaning of the term oxidation state.... (c) Complete the table
More informationGroup 13 Elements ( Boron Family)
Unit -11 The p- Block Elements Total no. of groups- 6 ( Group 13-18) General electronic configuration- ns 2 np 1-6 ( except for He) The first member of p-block differs from remaining members of their corresponding
More informationCHAPTER-3 CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES OF ELEMENTS
CHAPTER-3 CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES OF ELEMENTS Mandeleev s Periodic Law:- The properties of the elements are the periodic function of their atomic masses. Moseley, the English
More informationPart 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
More informationCHAPTER-9 NCERT SOLUTIONS
CHAPTER-9 NCERT SOLUTIONS Question 9.1: Justify the position of hydrogen in the periodic table on the basis of its electronic configuration. Hydrogen is the first element of the periodic table. Its electronic
More information5.1 The Periodic Table: chemical periodicity
5.1 The eriodic Table: chemical periodicity assification of elements in s, p, d blocks Elements are classified as s, p or d block, according to which orbitals the highest energy electrons are in. eriod
More informationTypes of bonding: OVERVIEW
1 of 43 Boardworks Ltd 2009 Types of bonding: OVERVIEW 2 of 43 Boardworks Ltd 2009 There are three types of bond that can occur between atoms: an ionic bond occurs between a metal and non-metal atom (e.g.
More informationCHAPTER THE S-BLOCK ELEMENTS
90 CHAPTER THE S-BLOCK ELEMENTS 1. Which one of the following properties of alkali metals increases in magnitude as the atomic number rises? [1989] (a) Ionic radius (b) Melting point (c) Electronegativity
More informationChapter 3 Classification of Elements and Periodicity in Properties
Question 3.1: What is the basic theme of organisation in the periodic table? The basic theme of organisation of elements in the periodic table is to classify the elements in periods and groups according
More informationChapter 3 Classification of Elements and Periodicity in Properties
Question 3.1: What is the basic theme of organisation in the periodic table? The basic theme of organisation of elements in the periodic table is to classify the elements in periods and groups according
More informationThe Periodic Table consists of blocks of elements
The Periodic Table consists of blocks of elements s block d block p block There is a clear link between the Periodic Table and the electronic configuration of an element 1s 2s 2p 3s 3p 4s 3d 4p 1s ATOMIC
More information4 Inorganic chemistry and the periodic table Answers to Exam practice questions
Pages 116 118 Exam practice questions 1 a) Atomic radius increases down the group [1] because of the increasing number of inner full shells of electrons. [1] The more full shells the larger the atom. [1]
More information5.1 The Periodic Table: chemical periodicity
5.1 The eriodic Table: chemical periodicity assification of elements in s, p, d blocks Elements are classified as s, p or d block, according to which orbitals the highest energy electrons are in. eriod
More informationGroup 2: The Alkaline Earth Metals
Group 2: The Alkaline Earth Metals Atomic radius Atomic Radii nm Atomic radius increases down Group 2. As one goes down the group, the atoms have more shells of electrons making the atom bigger and there
More informationCHEMICAL COMPOUNDS AND THEIR CHARACTERISTIC PROPERTIES
Seminar_2 1. Chemical compounds and their characteristic properties. 2. Types of chemical bonds (theses). 3. Basic types of complex compounds (theses). 4. Stability of complex compounds. TEST 2_ Chemical
More informationChemistry (www.tiwariacademy.com)
() Question 3.1: What is the basic theme of organisation in the periodic table? Answer 1.1: The basic theme of organisation of elements in the periodic table is to classify the elements in periods and
More informationF321: Atoms, Bonds and Groups Structure & Bonding
F321: Atoms, Bonds and Groups Structure & Bonding 1. This question is about different models of bonding and molecular shapes. Magnesium sulfide shows ionic bonding. What is meant by the term ionic bonding?
More information2.7 The periodic table groups 2 and 7
2.7 The periodic table groups 2 and 7 Students will be assessed on their ability to: 1 Properties down group 2 a. explain the trend in the first ionization energy down group 2 b. recall the reaction of
More informationQuestion 3.2: Which important property did Mendeleev use to classify the elements in his periodic table and did he stick to that?
Question 3.1: What is the basic theme of organisation in the periodic table? The basic theme of organisation of elements in the periodic table is to classify the elements in periods and groups according
More informationPeriodicity 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
More informationChapter 6: Chemical Bonding
Chapter 6: Chemical Bonding Learning Objectives Describe the formation of ions by electron loss/gain to obtain the electronic configuration of a noble gas. Describe the formation of ionic bonds between
More informationWRITING CHEMICAL FORMULAS & NAMING COMPOUNDS
WRITING CHEMICAL FORMULAS & NAMING COMPOUNDS Electrons in the same group have similar chemical properties because they have the same number of electrons in their valence shell Chemical bonds form between
More informationMass number of isotope Number of neutrons Number of electrons. Element J K L M N P O Q Atomic
NAME SCHOOL INDEX NUMBER DATE STRUCTURE OF THE ATOM, PERIODIC TABLES AND CHEMICAL FAMILIES 1. 1989 Q1a (i) An element X has atomic number 3, relative atomic mass 6.94 and consist of two isotopes of mass
More informationGroup 2: The Alkaline Earth Metals
Group 2: The Alkaline Earth Metals Atomic radius Atomic Radii nm Atomic radius increases down Group 2. As one goes down the group, the atoms have more shells of electrons making the atom bigger and there
More informationChemistry 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
More informationTHE ST. MICHAEL SCHOOL THIRD FORM CHEMISTRY MANUAL 3 SYMBOLS AND FORMULAE, CHEMICAL BONDING AND CHEMICAL EQUATIONS
1 THE ST. MICHAEL SCHOOL THIRD FORM CHEMISTRY MANUAL 3 SYMBOLS AND FORMULAE, CHEMICAL BONDING AND CHEMICAL EQUATIONS COMPILED BY G.WALKER, L.WORRELL, T. HARDING REFERENCE BOOKS Anne Tindale Chemistry A
More informationHYDROGEN AND s-block ELEMENTS
MDULE - 6 Chemistry 19 YDRGEN AND s-blck ELEMENTS ydrogen, alkali metals (like sodium and potassium) and alkaline earth metals (like magnesium and calcium) are the essential parts of the world we live
More informationInorganic 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
More informationCAREER POINT. PRE FOUNDATON DIVISION FACULTY SELECTION TEST CHEMISTRY [Time : 2 Hr.] [Max. Marks : 60]
CAREER POINT PRE FOUNDATON DIVISION FACULTY SELECTION TEST CHEMISTRY [Time : 2 Hr.] [Max. Marks : 60] INSTRUCTIONS : 1. Attempt all questions. 2. Indicate your answer on the question paper itself. 3. Each
More informationSCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions
SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions [Exam ID:25FPCV 1 When a strontium atom loses its valence electrons, it has the same electron configuration as which element?
More informationMAHESH 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
More informationPeriodicity 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
More information85 Q.1 A substance X melts at 1600 o C. Its does not conduct electricity in the solid or in the molten state. X probably has
Element and atomic structure / Section 1 / Sect1pp.doc / S. W. Tse / P.1 85 Q.1 A substance X melts at 1600 o C. Its does not conduct electricity in the solid or in the molten state. X probably has A.
More informationTest 5: Periodic Table, Ionic, and Molecular Compounds
Name: - Grade/Group: Subject: Chemistry-7 Teacher: Mrs. Raj Date: Test 5: Periodic Table, Ionic, and Molecular Compounds Directions: Identify the letter of the choice that best completes the statement
More informationHL 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
More informationElements in the Periodic Table show a periodic trend in atomic radius. In your answer you should use appropriate technical terms, spelled correctly.
1 The Periodic Table is arranged in periods and groups (a) Elements in the Periodic Table show a periodic trend in atomic radius State and explain the trend in atomic radius from Li to F In your answer
More informationQuestions 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
More informationChapter 7. Periodic Properties of the Elements. Lecture Outline
Chapter 7. Periodic Properties of the Elements Periodic Properties of the Elements 1 Lecture Outline 7.1 Development of the Periodic Table The periodic table is the most significant tool that chemists
More informationUnit 1 Review: Matter and Chemical Bonding
Unit 1 Review: Matter and Chemical Bonding 1. Do you think DHMO should be banned? Justify your answer. Write the formula for dihydrogen monoxide. H 2 O 2. Name these groups on the periodic table: 1, 2,
More informationClassification of o. f Elements ties. Unit. I. Multiple Choice Questions (Type-I)
Unit 3 Classification of o f Elements and Periodicit P eriodicity y in Proper P operties ties I. Multiple Choice Questions (Type-I) 1. Consider the isoelectronic species, Na +, Mg 2+, F and O 2. The correct
More information(b) electrovalent and covalent (c) electrovalent and co-ordinate (d) covalent and co-ordinate 10. Which pair is different from others (a) Li Mg (b)
1. Following triads have approximately equal size (a) Na+, Mg 2+, Al 3+ (iso-electronic) (b) F, Ne, O 2 (iso-electronic) (c) Fe, Co, Ni (d) Mn+, Fe 2+, Cr (iso-electronic) 2. Which of the following halides
More information1. Ham radio operators often broadcast on the 6 meter band. The frequency of this electromagnetic radiation is MHz. a. 500 b. 200 c. 50 d. 20 e. 2.
Name: Score: 0 / 60 points (0%) [1 open ended question not graded] Chapters 6&7 Practice Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Ham radio
More information2011 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/
More information9.3 Group VII. Content
9.3 Group VII Content 9.3.1 The similarities and trends in the physical and chemical properties of chlorine, bromine and iodine (i) Characteristic physical properties (ii) The relative reactivity of the
More information4.4. 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
More informationDAV CENTENARY PUBLIC SCHOOL PASCHIM ENCLAVE
DAV CENTENARY PUBLIC SCL PASCIM ENCLAVE GRUP 17 ELEMENTS Q1. With what neutral molecule is - isoelectronic? Ans. F Q2. Give the formula of the noble gas species that is isostructrural with (a) I4 - (b)
More informationICSE Board. Class X Chemistry. Board Paper Time: 1½ hrs Total Marks: 80
ICSE Board Class X Chemistry Board Paper 2013 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
More informationBonding Mrs. Pugliese. Name March 02, 2011
Bonding Mrs. Pugliese Name March 02, 2011 1. Atoms of which element have the greatest tendency to gain electrons? 1. bromine 3. fluorine 2. chlorine 4. iodine 2. Which polyatomic ion contains the greatest
More informationElements and the Periodic Table
CHAPTER 6 Elements and the Periodic Table 6.2 Properties of Groups of Elements There are millions and millions of different kinds of matter (compounds) composed of the same 92 elements. These elements
More informationChapter : 14) S-block elements (Alkali and Alkaline earth metals)
Chapter : 14) S-block elements (Alkali and Alkaline earth metals) Question ID: 1657 Q 1.Alkali metals are characterized by (A) good conductivity (B) high oxidation potentials (C) high melting point (D)
More informationProperties of Compounds
Chapter 6. Properties of Compounds Comparing properties of elements and compounds Compounds are formed when elements combine together in fixed proportions. The compound formed will often have properties
More informationSodium, Na. Gallium, Ga CHEMISTRY Topic #2: The Chemical Alphabet Fall 2017 Dr. Susan Findlay See Exercises 6.1 to 6.5 and 7.1.
Sodium, Na Gallium, Ga CHEMISTRY 1000 Topic #2: The Chemical Alphabet Fall 2017 Dr. Susan Findlay See Exercises 6.1 to 6.5 and 7.1 Forms of Carbon What is an alkali metal? Any element in Group 1 except
More informationExam Style Questions
Calderglen High School Chemistry Department CfE Higher Chemistry Unit 1: Chemical Changes and Structure Exam Style Questions Page 2 1.1 Periodicity (25 marks) Page 6 1.2 Bonding and Structure part 1 (25
More informationChemical Families. Group 0 The Noble Gases
Chemical Families Elements in the same Group have the same number of outer shell electrons. The same number of outer shell electrons means similar chemical properties so each Group is a chemical family.
More informationUnit Review : Chemistry
SNC2DE_09-10 Unit Review : Chemistry 1. A gas can be proved to be oxygen by means of: (a) a burning splint, which causes a small explosion or "pop"; (b) a glowing splint, which bursts into flame; (c) a
More information*ac112* Chemistry. Assessment Unit AS 1 [AC112] WEDNESDAY 10 JUNE, AFTERNOON. assessing Basic Concepts in Physical and Inorganic Chemistry
Centre Number ADVANCED SUBSIDIARY (AS) General Certificate of Education 2015 Chemistry Candidate Number Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC112] WEDNESDAY
More informationExam Review Questions - Multiple Choice
Exam Review Questions - Multiple Choice The following questions are for review. They are in no particular order. 1. An atom of iron 56 26Fe has... a) 26 protons, 26 electrons, 30 neutrons b) 30 protons,
More informationUNIT F321: ATOMS, BONDS AND GROUPS REVISION CHECKLIST. Miscellaneous Questions
UNIT F321: ATOMS, BONDS AND GROUPS REVISION CHECKLIST Miscellaneous Questions 1.1 Module 1: Atoms and Reactions 1.1.1 Atoms Candidates should be able to: Atomic structure (a) describe protons, neutrons
More informationChem Selected Aspects of Main Group Chemistry
Selected Aspects of Main Group Chemistry For the rest of the course, we will look at some aspects of the chemistry of main group compounds. The basic principles that you have learned concerning atoms,
More informationModel Question Paper PART A ANSWER ALL QUESTIONS:
Std: XI Standard Subject: Chemistry ANSWER ALL QUESTIONS: Model Question Paper PART A Time: 2.30 hours Max Marks: 75 Marks (15X1=15) 1. Which one of the following is a standard for atomic mass? a) 6 C
More informationCh 7: Periodic Properties of the Elements
AP Chemistry: Periodic Properties of the Elements Lecture Outline 7.1 Development of the Periodic Table The majority of the elements were discovered between 1735 and 1843. Discovery of new elements in
More information4.4. 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
More informationa) State modern periodic law. Name the scientist who stated the law.
INTEXT - QUESTION - 1 Question 1: a) State modern periodic law. Name the scientist who stated the law. b) What is a periodic table? How many groups and periods does modern periodic table have? Solution
More informationTopic 3.2: Other Trends (Physical and Chemical)
Topic 3.2: Other Trends (Physical and Chemical) Essential Ideas: 3.2: Elements show trends in their physical and chemical properties across periods and down groups Physical/ Chemical Properties Chemical
More information1 P a g e h t t p s : / / w w w. c i e n o t e s. c o m / Chemistry (A-level)
1 P a g e h t t p s : / / w w w. c i e n o t e s. c o m / Lattice energy (Chapter 19 TB) Chemistry (A-level) Lattice energy is the enthalpy change when 1 mole of an ionic compound is formed from its gaseous
More information26 s-block chemistry
26 s-block chemistry Answers to worked examples WE 26.1 Estimating the enthalpy change of formation of lithium nitride (Li 3 N) (on p. 1178 in Chemistry 3 ) Estimate a value for the enthalpy change of
More information1. (i) Give an equation for the dissociation of propanoic acid and hence an expression for its dissociation constant, K a. ...
1. (i) Give an equation for the dissociation of propanoic acid and hence an expression for its dissociation constant, K a.... At 5 C K a for propanoic acid is 1.30 10 5 mol dm 3. Find the ph of a solution
More informationUNIT 5.1. Types of bonds
UNIT 5.1 Types of bonds REVIEW OF VALENCE ELECTRONS Valence electrons are electrons in the outmost shell (energy level). They are the electrons available for bonding. Group 1 (alkali metals) have 1 valence
More informationLecture 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
More informationPatterns 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
More informationCHAPTER 10: Chemical Periodicity
CHAPTER 10: Chemical Periodicity 10.1 Periodicity in Physical Properties 10.2 Periodicity in Chemical Properties 10.3 Period 3 Oxides 10.4 Period 3 Chlorides Learning outcomes: (a) describe qualitatively
More informationYou have mastered this topic when you can:
CH 11 T17 IONIC COMPOUNDS IONIC BONDS 1 You have mastered this topic when you can: 1) define or describe these terms: IONIC BOND, CATION, ANION and FORMULA UNIT. 2) predict the formation of an IONIC BOND
More information7. How many unpaired electrons are there in an atom of tin in its ground state? 2
Name period AP chemistry Unit 2 worksheet 1. List in order of increasing energy: 4f, 6s, 3d,1s,2p 1s, 2p, 6s, 4f 2. Explain why the effective nuclear charge experienced by a 2s electron in boron is greater
More informationElements react to attain stable (doublet or octet) electronic configurations of the noble gases.
digitalteachers.co.ug Chemical bonding This chapter teaches the different types and names of bonds that exist in substances that keep their constituent particles together. We will understand how these
More information1 Two white powders, A and B, known to be Group 2 carbonates, are investigated.
1 Two white powders, A and B, known to be Group 2 carbonates, are investigated. (a) (i) The presence of the carbonate ion is usually confirmed using a simple test carried out in two stages at room temperature.
More informationPowerPoint to accompany. Chapter 6. Periodic Properties of the Elements
PowerPoint to accompany Chapter 6 Periodic Properties of the Elements Development of the Periodic Table Elements in the same group generally have similar chemical properties. Properties are not identical,
More information8.1 Early Periodic Tables CHAPTER 8. Modern Periodic Table. Mendeleev s 1871 Table
8.1 Early Periodic Tables CHAPTER 8 Periodic Relationships Among the Elements 1772: de Morveau table of chemically simple substances 1803: Dalton atomic theory, simple table of atomic masses 1817: Döbreiner's
More informationICSE Chemistry Board Paper 2016
2015 Time: 2 hours; Max. Marks: 80 General Instructions: Answers to this Paper must be written on the paper provided separately. You will not be allowed 10 write during the first 15 minutes. This time
More informationGHW#3. Chapter 3. Louisiana Tech University, Chemistry 481. POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3.
GHW#3. Chapter 3. Louisiana Tech University, Chemistry 481. POGIL(Process Oriented Guided Inquiry Learning) Exercise on Chapter 3. Energetics of Ionic Bonding. Why? What are the properties of ionic compounds?
More informationCHEM 115 EXAM #3 Practice Exam Fall 2013
Name CHEM 115 EXAM #3 Practice Exam Fall 2013 Circle the correct answer. (numbers 1-9, 3 points each) 1. Choose the correct statement about the compound SO 2. a. the S O bonds are ionic in character b.
More informationinsoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water
Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of
More informationMOSELEY 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
More informationSIR MICHELANGELO REFALO
SIR MICELANGELO REFALO SIXT FORM alf-yearly Exam 2014 Name: CEMISTRY ADV 1 ST 3 hrs ANSWER ANY 7 QUESTIONS. All questions carry equal marks. You are reminded of the importance of clear presentation in
More information(B) K2O potassium dioxide
PRACTICE CHEMISTRY EOC TEST 1. Which substance is a conductor of electricity? (A) NaCl(s) (B) NaCl(l) (C) C6H12O6(s) (D) C6H12O6(l) 2. Which formula is correctly paired with its name? (A) MgCl2 magnesium
More information2. Which important property did mendeleev use to classify the elements in his periodic table and did he stick to that?
1. What is the basic theme of organization in the periodic table? At the beginning of 18 th century, only a very few elements were known, it was quite easy to study and remember their individual properties.
More information