Billy's Chemistry Chapter 7 Section 1 questions

10)Explain how an anion of nitrogen forms.

N gains three electrons, forming N3, which has the stable electron configuration of Ne.

4)The periodic table shown in Figure 14 contains elements labeled A-G. For each labeled element, state the number of valence electrons and identify the ion that will form.

A: three valence electrons Al3, B: two valence electrons Ba2, C: one valence electron Rb, D: five valence electrons N3, E: seven valence electrons I, F: eight valence electrons, no ion formed, G: six valence electrons, Se2 50

9)Discuss the formation of the barium ion.

Ba will lose two electrons and form Ba2, which has the stable electron configuration of Xe.

11)The more reactive an atom is, the higher its potential energy will be. Which atom has higher potential energy, neon or fluorine? Explain.

Fluorine, because it will easily gain one more electron to fill its outer energy level

3)Why are halogens and alkali metals likely to form ions? Explain your answer.

Halogens need to gain only one electron to have a noble gas electron configuration. Alkali metals need to lose one.

12)Explain how the iron atom can form both an iron 2+ ion and an iron 3+ ion.

Iron has the electron configuration [Ar]4s23d6. To form the 2 ion the iron atom loses the 4s2 electrons. When forming the 3 ion the iron atom loses the 4s2 electrons and one 3d electron.

1)How do positive ions and negative ions form?

Positive ions: forms when an atom loses one or more valence electrons in order to attain a noble gas configuration. Negative ions: forms when nonmetals gain electrons to attain a stable outer electron configuration.

14)Discuss the formation of a 3+ scandium ion using its orbital notation, shown in Figure 16

Scandium, [Ar]4s23d1, loses both the 4s2 electrons and the 3d1 electron to form the 3 ion in the stable [Ar] configuration.

6)The orbital notation of sulfur is shown in Figure 15. Explain how sulfur forms its ion.

Sulfur gains 2 electrons in the 3p sublevel, forming a complete octet.

8)Explain why noble gases are not likely to form chemical bonds.

They already have a full, stable outer energy level

13)Predict the reactivity of each atom based on its electron configuration. a. potassium b. fluorine c. neon

a) potassium: Potassium, [Ar]4s1, is reactive. It will tend to lose one outer electron and form a 1 ion. b) fluorin: Fluorine, [He]2s22p5, is reactive. It will tend to gain one more electron and form a 1 ion. c) neon: Neon, 1s22s22p6, will not react because it already has eight electrons in its outer energy level

7)Give the number of valence electrons in an atom of each element. a. cesium b. zinc c. rubidium d. strontium e. gallium

a. cesium: 1 b. zinc: 2 c. rubidium: 1 d. strontium: 2 e. gallium: 3

5)Discuss the importance of electron affinity and ionization energy in the formation of ions.

high electron affinity: atom easily gains an electron; low ionization energy: atom easily loses an electron

2)When do chemical bonds form?

when a positive nucleus attracts electrons of another atom, or oppositely charged ions attract