Chapter3
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This document provides information about the periodic table and periodic properties of elements. It discusses the contributions of Dobereiner, Newlands and Mendeleev towards developing the periodic table. It explains that elements are arranged in the modern periodic table according to increasing atomic number. Properties like atomic radius, ionization energy and electronegativity repeat periodically with this arrangement. The document also answers multiple choice and short answer questions about periodic trends, periodic law, and classification of elements in periods and groups.
Chapter3
- 1. Chapter 3 periodic table and periodicity of properties ADNAN SOHAIL M. Phil Chemistry 1. What was the contribution of Dobereiner towards classification of elements? Ans. A German chemist Dobereiner observed relationship between atomic masses of several groups of three elements called triads. In these groups, the central or middle element had atomic mass average of the other two elements. One triad group example is that of calcium (40), strontium(88) and barium (137). 2. How Newlands arranged the elements? Ans. In 1864 British chemist Newlands put forward his observations in the form of ‘law of octaves’. He noted that there was a repetition in chemical properties of every eighth element if they were arranged by their increasing atomic masses. 3. Who introduced the name Periodic Table ? Ans. Russian chemist, Mendeleev introduced the name Periodic table. 4. Why the improvement in Mendeleev’s periodic table was made? Ans. In Mendeleev’s periodic table elements were arranged according to their atomic masses. It was found that Atomic number is a more fundamental property than atomic mass because atomic number of every element is fixed and it increases regularly by 1 from element to element. No two elements can have the same atomic number. So elements are arranged according to their atomic numbers. 5. State Mendeleev’s periodic law? Ans. According to Mendeleev’s periodic law, properties of the elements are periodic functions of their atomic masses. 6. Why and how elements are arranged in a period? Ans. The elements are arranged according to their atomic numbers. It was found that Atomic number is a more fundamental property than atomic mass because atomic number of every element is fixed and it increases regularly by 1 from element to element. No two elements can have the same atomic number. 1. How the properties of elements repeat after regular intervals? Ans. When the elements are arranged according to increasing atomic number from left to right in a horizontal row, properties of elements were found repeating after regular intervals such that elements of similar properties and similar configuration are placed in the same group. 2. In which pattern modern periodic table was arranged? Ans. The modern periodic table is based upon the arrangement of elements according to increasing atomic number. 1
- 2. Chapter 3 periodic table and periodicity of properties ADNAN SOHAIL M. Phil Chemistry 3. How many elements are in first period and what are their names and symbols? Ans. There are two elements in first period their names are hydrogen and helium. 4. How many elements are placed in 4th period? Ans. Fourth period consists of 18 elements. 5. From which element lanthanide series starts? Ans. Lanthanide series starts from Lanthanide. 6. From which period actinides series starts? Ans. Actinides series starts from Actinide. 7. How many elements are in 3rd period, write their names and symbols? Ans. Third period consist of 8 elements. 11 Sodium Na 12 Magnesium Mg 13 Aluminium Al 14 Silicon Si 15 Phosphorus P 16 Sulphur S 17 Chlorine Cl 18 Argon Ar 8. How many periods are considered normal periods? Ans. Two periods (2nd and 3rd ) are considered normal. 9. What do you mean by a group in a periodic table? Ans. The vertical columns in the periodic table are called groups. 10. What is the reason of arranging elements in a group? Ans. The elements of a group have similar electronic configuration i.e. same number of electrons are present in their valence shells. The elements of a group show similar chemical properties. 11. What do you mean by periodic function? Ans. Periodic function means repetition of properties of elements after regular intervals in periodic table. 12. Why the elements are called s or p block elements? Ans. Elements of group 1 and 2 have valence electrons in ‘s’ subshell. Therefore, they are called s-block elements Elements of group 13 to 18 have their valence electrons in ‘p’ subshell. Therefore, they are referred as p-block elements. 13. Write down the names of elements of group 1 with their symbols? Ans. Group 1 consists of hydrogen (H), lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs) and francium (Fr). 14. How many members are in group 17, is there any liquid, what is its name ? Ans. There are five elements that make Group 17 of the periodic table and consist of: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). Bromine (Br) is found in liquid state at room temperature. 2
- 3. Chapter 3 periodic table and periodicity of properties ADNAN SOHAIL M. Phil Chemistry 1. Define atomic radius? Ans. Half of the distance between the nuclei of the two bonded atoms is referred as the atomic radius of the atom. 2. What are SI units of atomic radius? Ans. Picometer (pm) is the SI units of atomic radius. 3. Why the size of atoms decreases in a period? Ans. There is gradual increase of effective nuclear charge which increases due to addition of protons. This force contracts the outermost shell towards the nucleus. Due to this atomic size decreases in s period. 4. Define ionization energy? Ans. The ionization energy is the amount of energy required to remove the most loosely bound electron from the valence shell of an isolated gaseous atom. 5. Why the 2nd ionization energy of elements is higher than first one? Ans. With the removal of first electron, force of attraction between nucleus and remaining outer most electrons increases. So to remove 2nd electron more amount of energy is required. 6. What is the trend of ionization energy in a group? Ans. As we move down the group more and more shells lie between the valence shell and the nucleus of the atom, these additional shells reduce the electrostatic force felt by the electrons present in the outermost shell. Resultantly the valence shell electrons can be taken away easily. Therefore, ionization energy of elements decreases from top to bottom in a group. 7. Why the ionization energy of sodium is less than that of magnesium? Ans. Magnesium has 12 protons its nucleus. It attracts its outer most electrons more tightly than sodium which has 11 protons in its nucleus. Due to this, ionization energy of sodium is less than that of magnesium 8. Why is it difficult to remove an electron from halogens? Ans. It is difficult to remove an electron from halogens because halogens being non metals have high electronegativity values. 9. What is shielding effect? Ans. The electrons present in the inner shells screen or shield the force of attraction of nucleus felt by the valence shell electrons. This is called shielding effect. 10. How does shielding effect decrease the forces of electrostatic attractions between nucleus and outer most electrons? Ans. The attractions of outer electrons towards nucleus is partially reduced because of presence of inner electrons. As a result valence electron experiences less nuclear charge than that of the actual charge. 3
- 4. Chapter 3 periodic table and periodicity of properties ADNAN SOHAIL M. Phil Chemistry 11. Why does the bigger size atoms have more shielding effect? Ans. Bigger size atoms have more inner electrons to screen nuclear charge so they have more shielding effect. 12. Why does the trend of electron affinity and electronegativity is same in a period? Ans. These have same trend because the value of both electron affinity and electronegativity depend upon same factor i.e. force of attraction of nucleus for electrons. 13. Which element has the highest electronegativity? Ans. Fluorine has highest electronegativity value equal to 4.0 . SHORT ANSWER QUESTIONS 1. Why are noble gases not reactive? Ans. Noble gases are not reactive because their valence shells are complete. 2. Why Cesium (at. no.55) requires little energy to release its one electron present in the outermost shell? Ans. Cesium is present at the bottom of first group. Due to its bigger size it has strong shielding effect and requires little energy to remove its one electron present in the outermost shell. 3. How is periodicity of properties dependent upon number of protons in an atom? Ans. The arrangement of elements according to increasing atomic number shows the periodicity (repetition of properties after regular intervals) in the electronic configuration of the elements that leads to periodicity in their properties. 4. Why shielding effect of electrons makes cation formation easy? Ans. Bigger size atoms have strong shielding effect. Their valence electrons are loosely bound. This makes removal of valence electrons and cation formation easy. 5. What is the difference between Mendeleev’s periodic law and modern periodic law? Ans. Mendeleev periodic law: properties of the elements are periodic function of their atomic masses. Modern periodic law: properties of the elements are periodic function of their atomic numbers. 6. What do you mean by groups and periods in the Periodic Table? Ans: The vertical columns in the periodic table are called groups. The horizontal rows of elements in the periodic table are called periods. 7. Why and how are elements arranged in 4th period? Ans. 4th period consist of 18 elements from potassium (K-19) to krypton (Kr-36). The elements in this period are arranged in order of their increasing atomic number. 8. Why the size of atom does not decrease regularly in a period? Ans. With the increase in a proton in nucleus there is also addition of an electron in outermost shell of atom from left to right in a period. Due to this, size of atom does not decrease regularly in a period. 9. Give the trend of ionization energy in a period? Ans. If we move from left to right in a period, the value of ionization energy increases. It is because the size of atoms reduces and valence electrons are held strongly by the electrostatic force of nucleus. Therefore, elements on left side of the periodic table have low ionization energies as compared to those on right side of the periodic table. 4 4