1st Year Chemistry ch # 1 _ Important Shorts ( Periodic Table and Periodic Properties) Click Here To Download Imp. Longs Imp. MCQs Exercise Solution 📌 Topics for Short Questions – Chapter 1 (Periodic Table & Periodicity) Short questions in board exams usually come from these topics: 1. What is the periodic table? Define the periodic table and explain how elements are arranged in it. 2. What are periods and groups? Explain the difference between periods (horizontal rows) and groups (vertical columns) in the periodic table. 3. What are metals, non-metals, and metalloids? Define each and give their positions in the periodic table. 4. What are the four blocks of the periodic table? Name the four blocks (s, p, d, f) and explain what they represent. 5. What is the period number (n)? Recognize that the period number (n) represents the outer energy level occupied by electrons. 6. How can you find electron configuration from the periodic table? Explain how the position of an element on the periodic table helps you deduce its electron configuration. 7. What is atomic radius and how does it trend? Define atomic radius. Explain how it changes across a period and down a group. 8. What is ionization energy? Define ionization energy and explain the trend in ionization energy across a period and down a group. 9. What is electron affinity? Define electron affinity and explain the trend in electron affinity. 10. What is electronegativity? Define electronegativity and explain how it varies in the periodic table. 11. Why do metallic properties decrease across a period? Explain the reason for the decrease in metallic character across a period. 12. Why do non-metallic properties increase across a period? Explain the reason for the increase in non-metallic character across a period. 13. What are acidic and basic oxides? Give examples of acidic oxides (e.g., CO₂, SO₂) and basic oxides (e.g., Na₂O, MgO). 14. What is an amphoteric oxide? Define amphoteric oxide and give an example (e.g., Al₂O₃). 15. What happens when oxides react with water? Write the general reaction of acidic and basic oxides with water. Give the pH of the resulting solution. 16. What are the reactions of Na and Mg with oxygen? Write simple equations for Na reacting with O₂ and Mg reacting with O₂. 17. How do chlorides react with water? Explain the reaction of chlorides with water and the resulting pH. 18. What is the oxidation number trend in oxides and chlorides? Explain the variation of oxidation numbers in oxides and chlorides using valence electrons. 19. Why are trends in metallic and non-metallic behavior due to valence electrons? Explain the relationship between valence electrons and metallic/non-metallic behavior. 20. What is the shielding effect and how does it affect trends? Define the shielding effect and explain how it influences atomic radius and ionization energy. Leave a Reply Cancel reply Logged in as mubasharaliraza121@gmail.com. Edit your profile. Log out? Required fields are marked * Message*

1st Year Chemistry ch # 1 _ Important MCQs ( Periodic Table and Periodic Properties) Click Here To Download Imp. Shorts Imp. Longs Exercise Solution 📌 Topics for MCQs – Chapter 1 (Periodic Table & Periodicity) MCQs in board exams are mostly based on these topics: 1. Basic Concepts Who proposed the periodic table? (Mendeleev) What is the modern periodic table based on? (Atomic number) How many periods and groups are in the periodic table? What are periods and groups? 2. Blocks of the Periodic Table Which block are alkali metals in? (s-block) Which block are halogens in? (p-block) Which block are transition metals in? (d-block) Which block are lanthanides and actinides in? (f-block) 3. Electron Configuration What is the electron configuration of Na? (1s² 2s² 2p⁶ 3s¹) What is the electron configuration of Cl? (1s² 2s² 2p⁶ 3s² 3p⁵) How many valence electrons does Group 1 elements have? (1) How many valence electrons does Group 17 elements have? (7) 4. Periodic Trends Which element has the largest atomic radius in a period? (Alkali metal) Which element has the smallest atomic radius in a period? (Halogen) Ionization energy increases across a period: True or False? Electronegativity decreases down a group: True or False? 5. Metals, Non-Metals, Metalloids Which elements are metals? (Left side of periodic table) Which elements are non-metals? (Right side of periodic table) What is an example of a metalloid? (Silicon, Germanium) Where are metalloids located? (Between metals and non-metals) 6. Properties of Groups Group 1 elements are called: (Alkali metals) Group 17 elements are called: (Halogens) Group 18 elements are called: (Noble gases) Which group is most reactive? (Group 1 and Group 17) 7. Oxides and Hydroxides Na₂O is a basic oxide: True or False? CO₂ is an acidic oxide: True or False? What is the pH of the solution formed when basic oxide reacts with water? (pH > 7) What is the pH of the solution formed when acidic oxide reacts with water? (pH < 7) Al₂O₃ is an example of: (Amphoteric oxide) 8. Ionization Energy and Electron Affinity Which element has the highest ionization energy in a period? (Noble gas) Which element has the lowest ionization energy in a period? (Alkali metal) Which group has the highest electron affinity? (Group 17 / Halogens) 9. Reactions of Elements Na reacts with water to form: (NaOH + H₂) Mg reacts with oxygen to form: (MgO) Na reacts with chlorine to form: (NaCl) Mg reacts with chlorine to form: (MgCl₂) 10. Oxidation States What is the oxidation state of Na in NaCl? (+1) What is the oxidation state of Mg in MgCl₂? (+2) What is the oxidation state of O in Na₂O? (-2) What is the oxidation state of Cl in NaCl? (-1) Leave a Reply Cancel reply Logged in as mubasharaliraza121@gmail.com. Edit your profile. Log out? Required fields are marked * Message*

1st Year Chemistry ch # 1 : Exercise Solution ( Periodic Table and Periodic Properties) Click Here To Download Imp. Shorts Imp. MCQs Imp. Longs 📌 Topics Covered in Exercise – Chapter 1 (Periodic Table & Periodicity) The exercise questions in this chapter are based on these topics: 1. Electron Configuration Practice Write the electron configuration of given elements. Identify the block, period, and group from the electron configuration. 2. Periodic Trends Compare and explain the trends in atomic radius, ionization energy, electron affinity, and electronegativity. Justify why certain elements have larger or smaller atomic radii. 3. Classification of Elements Identify metals, non-metals, and metalloids from given properties. Classify elements into s-block, p-block, d-block, or f-block. 4. Reactions of Elements Write balanced equations for the reactions of Na and Mg with oxygen, chlorine, and water. Predict the products and type of bonding. 5. Oxides and Hydroxides Predict whether an oxide is acidic, basic, or amphoteric. Write equations for the reactions of oxides with water. Write equations for the acid/base behavior of NaOH and Mg(OH)₂. 6. Chemical Properties and pH Predict the pH of solutions formed when oxides or chlorides react with water. Explain the acid/base behavior of oxides. 7. Oxidation Numbers Determine the oxidation numbers of elements in oxides and chlorides. Explain the variation based on valence electrons. 8. Trends in Reactivity Explain the reactivity trend in Group 1 and Group 17 elements. Justify trends in metallic and non-metallic behavior. 9. Application of Periodic Trends Predict the position of unknown elements based on given properties. Predict the characteristic properties of an element using knowledge of chemical periodicity. 10. Bonding and Electronegativity Suggest the type of bonding present in chlorides and oxides based on observations of physical and chemical properties. Explain variations and trends in terms of bonding and electronegativity. Leave a Reply Cancel reply Logged in as mubasharaliraza121@gmail.com. Edit your profile. Log out? Required fields are marked * Message*

1st Year Chemistry ch # 1 : Long Questions ( Periodic Table and Periodic Properties) Click Here To Download Imp. Shorts Imp. MCQs Exercise Solution 📌 Topics for Long Questions – Chapter 1 (Periodic Table & Periodicity) In this chapter, the following topics are important for long questions in board exams: 1. Arrangement of Elements in the Periodic Table Explain how elements are arranged in the periodic table. Describe the modern periodic table, periods, groups, and the significance of atomic number. Also explain the position of metals, non-metals, and metalloids. 2. Blocks of the Periodic Table (s, p, d, f) Explain that the periodic table is divided into four blocks based on the subshell (s, p, d, f) that receives the last electron. Describe the location and characteristics of each block. 3. Electron Configuration from Periodic Table Position Explain how to deduce the electron configuration of an atom from its position in the periodic table. Also show how to find the position of an element from its electron configuration (based on s, p, d, f subshells). 4. Periodic Trends – Atomic Radius, Ionic Radius, Ionization Energy, Electron Affinity, Electronegativity Explain the trends in atomic radius, ionic radius, ionization energy, electron affinity, and electronegativity across a period and down a group. Explain why these trends exist (nuclear charge, shielding effect, etc.). 5. Trends in Group 1 and Group 17 Explain the trends in ionization energy and electron affinity for Group 1 (alkali metals) and Group 17 (halogens). Compare the reactivity and trends within each group. 6. Metallic and Non-Metallic Behavior Explain how metallic and non-metallic behavior changes across a period and down a group. Relate these trends to valence electrons and ionization energy. 7. Reactions of Oxides and Chlorides with Water Describe the reactions of oxides (acidic and basic) with water, including the pH of the resulting solutions. Also explain the reactions of chlorides with water and the pH of the solutions obtained. 8. Amphoteric Behavior (NaOH and Mg(OH)₂) Explain the acid/base behavior of oxides and hydroxides, with special focus on amphoteric behavior (reactions with both acids and bases). Include equations for NaOH and Mg(OH)₂. 9. Oxidation Numbers of Oxides and Chlorides Explain the variation in oxidation numbers of oxides and chlorides (e.g., NaCl, MgCl₂, Na₂O, MgO) in terms of outer shell (valence shell) electrons. 10. Reactions of Na and Mg with Oxygen, Chlorine, and Water Write balanced equations for the reactions of sodium (Na) and magnesium (Mg) with oxygen, chlorine, and water. Explain the trends in bonding and electronegativity. Leave a Reply Cancel reply Logged in as mubasharaliraza121@gmail.com. Edit your profile. Log out? Required fields are marked * Message*