Consider that each of the following species is in its lowest energy state. Which

Question

Consider that each of the following species is in its lowest energy state. Which set contains species that all have the same electronic configuration?

a. Na+, K+, Rb+, Cs+

b. Mg2+, Ca2+, Sr2+, Ba2+

c. N, O, F, Ne

d. F?, Cl?, Br?, I?

e. N3?, O2?, Mg2+, Al3+

Which two species are isoelectronic (identical electron configurations)?

a. Na+ and K+

b. Cl? and F?

c. Ca2+ and Mg2+

d. Al3+ and Ne

e. P? and Ca+

The Lewis structure for phosphine, PH3, has…

a. four bonds

b. two bonds and one lone pair

c. three bonds and one lone pair

d. one bond and three lone pairs

e. three bonds

In the Lewis structure for the NF2? ion, there are __ lone pairs around the central nitrogen atom.

a.0

b.1

c.2

d.3

e.4

Which of the following species has more than one lone pair on the central atom?

a. NF3

b. SO2

c. NH2-

d. H3O+

e. CCl4

Which diatomic element contains a multiple bond?

a.F2

b.H2

c.Cl2

d.O2

e.I2

Explanation / Answer

Ans : e) N3- , O2- , Mg2+ , Al3+

The electronic configuration of the elements depend on the number of electrons present in their atoms.

Nitrogen typically has seven electrons but gains 3 to make 10. Likewise O has 8 , gains two to make 10. Mg has 12 , it loses 2 to make 10 and Al has 13 electrons , it loses three to make 10 electrons.

So the electron configuration of all these ions is given as : 1s2 2s2 2p6.

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