Q.7 The trends, in melting points of the elements of 3rd period, are depicted in figure below.
The sharp decrease observed from ‘Si’ to ‘P’ is due to
A) Decrease in atomic radius from ‘Si’ to ‘P’ C) Different universities of two elements
B) Change in bonding and structure of two elements D) Increase in electron density from ‘Si’ to ‘P’
Q.8 Arrange the following elements according to the trend of ionization energies. (C, N, Ne, B)
A) Ne < N < C < B C) B < C < N < Na
B) B < N < C < Na D) Ne < B < C < N
The sharp decrease observed from ‘Si’ to ‘P’ is due to
A) Decrease in atomic radius from ‘Si’ to ‘P’ C) Different universities of two elements
B) Change in bonding and structure of two elements D) Increase in electron density from ‘Si’ to ‘P’
Q.8 Arrange the following elements according to the trend of ionization energies. (C, N, Ne, B)
A) Ne < N < C < B C) B < C < N < Na
B) B < N < C < Na D) Ne < B < C < N
Q.9 Which one of the following will have the smallest radius?
A) Al+3 C) Mg+2
B) Si+4 D) Na+1
Q.10 Keeping in view the size of atoms, which order is correct?
A) N > C C) Ar > Cl
B) P > Si D) Li > Be
A) Al+3 C) Mg+2
B) Si+4 D) Na+1
Q.10 Keeping in view the size of atoms, which order is correct?
A) N > C C) Ar > Cl
B) P > Si D) Li > Be
Q.11 Melting points of group II-A elements are higher than those of group I-A because:
A) Atoms of II-A elements have smaller size C) Atoms of II-A elements provide two binding electrons
B) II-A elements are more reactive D) I-A elements have smaller atomic radius
Q.12 The ionic radius of fluoride ion is:
A) 72 pm C) 136 pm
B) 95 pm D) 157 pm
A) Atoms of II-A elements have smaller size C) Atoms of II-A elements provide two binding electrons
B) II-A elements are more reactive D) I-A elements have smaller atomic radius
Q.12 The ionic radius of fluoride ion is:
A) 72 pm C) 136 pm
B) 95 pm D) 157 pm