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Sodium and potassium have similar chemical and physical properties. This is best explained by the fact that both elements

have the same ground-state valence-electron configuration.

have low relative atomic masses.

are in Period 1 of the periodic table.

have relatively low first ionization energies.

are active metals.

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Related questions

1.

Sodium and potassium have similar chemical and physical properties. This is best explained by the fact that both elements

A.have low relative atomic masses.

B.are in Period 1 of the periodic table.

C.have relatively low first ionization energies.

D.have the same ground-state valence-electron configuration.

E.are active metals.

2.

Which of the following statements is true concerning the electron configuration [Ne]3s13p1?

A.It may represent a ground-state electron configuration of a Al+ cation.

B.It may represent an excited-state electron configuration of a Mg atom.

C.It may represent an excited-state electron configuration of a Ne– anion.

D.It may represent a ground-state electron configuration of a Na+ cation.

E.It may represent a ground-state electron configuration of a Mg+ cation.

3.

Which of the following subshells does not exist?

A.3p

B.3f

C.6g

D.4d

E.2s

4.

Sodium oxide reacts with water to produce sodium hydroxide. Suppose 10.2 g of sodium oxide is combined with 34.6 g of water. When the reaction is complete, all the sodium oxide has been consumed. According to the law of conservation of mass, which is a true statement?

A.The mass of sodium hydroxide produced plus the mass of unreacted water must equal 44.8 g.

B.The mass of sodium hydroxide produced must equal 10.2 g.

C.The mass of water consumed must equal 10.2 g.

D.The mass of sodium hydroxide produced must equal 44.8 g.

E.The mass of unreacted water must equal 24.4 g.

Which of the following statements about the periodic table is false?

(a) Elements in the same column have similar reactivities because their valence electrons tend to be located in the same type of orbitals.

(b) A series of ions that are isoelectronic (contain the same number of electrons) in their ground states must have the same electron configuration.

(c) The atomic size of the elements increases going across a period from left to right because the number of electrons increases, so the electrons are located further from the nucleus.

(d) It takes more energy to remove an electron from lithium than cesium because the valence electrons in lithium are located closer to the nucleus.

 

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