The following table represents the first three periods of the modern periodic table. Study the table and answer the questions that follow:
(i) Write the formula of the sulphate of the element with atomic number 13.
(ii) What type of bonding will be present in the oxide of the element with atomic number 1?
(iii) Which feature of the atomic structure accounts for the similarities in the chemical properties of the elements in group VIIA of the periodic table?
(iv) Name the element which has the highest ionization potential.
(v) How many electrons are present in the valence shell of the element with atomic number 18?
Figure
(vi) What is the name given to the energy released, when an atom in its isolated gaseous state accepts an electron to form an anion?
(vii) What is the electronic configuration of the element in the third period which gains one electron to become an anion?
(viii) Fill in the blanks:
The atomic size ________ as we move from left to right across the period, because the ________ increases, but the ________ remains the same.
(i) Write the formula of the sulphate of the element with atomic number 13.
(ii) What type of bonding will be present in the oxide of the element with atomic number 1?
(iii) Which feature of the atomic structure accounts for the similarities in the chemical properties of the elements in group VIIA of the periodic table?
(iv) Name the element which has the highest ionization potential.
(v) How many electrons are present in the valence shell of the element with atomic number 18?
Figure
(vi) What is the name given to the energy released, when an atom in its isolated gaseous state accepts an electron to form an anion?
(vii) What is the electronic configuration of the element in the third period which gains one electron to become an anion?
(viii) Fill in the blanks:
The atomic size ________ as we move from left to right across the period, because the ________ increases, but the ________ remains the same.
(i) Aluminium has atomic number 13. It will lose its three valence electrons and sulphate ion will gain two electrons. So, the chemical formula of aluminium sulphate is Al2(SO4)3.
(ii) Polar covalent bonding will be present in the oxide of hydrogen (atomic number 1). Oxygen is more electronegative than hydrogen; therefore, a polar bond is formed between them.
(iii) Same number of valence electrons in the outermost shell of the elements of group VIIA is responsible for similarities in their chemical properties.
(iv) Helium has the highest ionisation potential because of its small size and completely filled valence shell.
(v) Argon (atomic number 18) has completely filled outermost shell with eight valence electrons.
(vi) Electron affinity is the name given to the energy released when an atom in its isolated gaseous state accepts an electron to form an anion.
(vii) Chlorine is the element in the third period that has an electronic configuration of 2, 8, 7. This causes chlorine to gain one electron to become an anion.
(viii) The atomic size decreases as we move from left to right across the period, because the nuclear charge increases, but the number of shells remains the same.
(i) Aluminium has atomic number 13. It will lose its three valence electrons and sulphate ion will gain two electrons. So, the chemical formula of aluminium sulphate is Al2(SO4)3.
(ii) Polar covalent bonding will be present in the oxide of hydrogen (atomic number 1). Oxygen is more electronegative than hydrogen; therefore, a polar bond is formed between them.
(iii) Same number of valence electrons in the outermost shell of the elements of group VIIA is responsible for similarities in their chemical properties.
(iv) Helium has the highest ionisation potential because of its small size and completely filled valence shell.
(v) Argon (atomic number 18) has completely filled outermost shell with eight valence electrons.
(vi) Electron affinity is the name given to the energy released when an atom in its isolated gaseous state accepts an electron to form an anion.
(vii) Chlorine is the element in the third period that has an electronic configuration of 2, 8, 7. This causes chlorine to gain one electron to become an anion.
(viii) The atomic size decreases as we move from left to right across the period, because the nuclear charge increases, but the number of shells remains the same.
