Question

uration b) 4s24p4 ser, write the elec- alence electrons of Group 6A/16 Charles D. Winters 59. Using n for the principal quantum number, write the tron configuration for the valence electrons of Grou atoms. 60. In what group and period do you find elements with the valence electron configurations given? a) 2s22p2 svold b) 4s24p ellicho R svold s ruldu Section 6.6: Trends in the Periodic Table 61. Identify an atom of a main-group element in Period 4 that is (a) larger than an atom of arsenic (Z = 33) and (b) smaller than an atom of arsenic. 62. Using only the periodic table, arrange the following ele- v ments in order of increasing atomic radius: aluminum, boron, indium (Z = 49), gallium (Z = 31). del 63. Why does atomic size decrease as you go left to right across a row in the periodic table? 64. Using only the periodic table, arrange the following ele- ments in order of increasing atomic radius: sulfur, magne- sium, sodium, chlorine. 65. Even though an atom of germanium (Z = 32) has more than twice the nuclear charge of an atom of silicon (Z = 14), the germanium atom is larger. Explain. Solqienia no sto niworld Phil Degginger / Alamy

Answer 1

Ans :

60) a) In period 2 and group 14.( Carbon- 1s²2s²2p²)

b) In period 4 and group 17(Bromine-[Ar]4s²4p5)

61) a) Zn

b) Selenium ( Se )

62) All the elements are group 13 elements. As we go from top to bottom of a group atomic size generally increases. So, the increasing orderr will be -

Boron(B)<Aluminium (Al)<Galium(Ga)<Indium(In)

63) As we go from left to right across a period, more protons are added to the nucleus whereas electrons are added to the same energy level. The concentration of more protons in the nucleus creates a stronger forces of attraction ( effective nuclear charge) that will pull the electrons more closer to the nucleus resulting in smaller atomic radius.

64) The increasing order will be -

Cl < S < Mg < Na

65) Si and Ge are group 15 elements. As we move down a group from top to bottom, the no. of energy levels also increases with the increasing no. of electrons. Each subsequent energy levels are further apart than the last. Due to this, the nucleus can not pull the electrons closer which results in increasing atomic size.