Ch.7 - Periodic Properties of the Elements

Problem 17

Chapter 7, Problem 17

Which will experience the greater effect nuclear charge,the electrons in the n = 2 shell in F or the n = 2 shell in B?Which will be closer to the nucleus?

Verified step by step guidance

Step 1: Understand the concept of nuclear charge. The nuclear charge is the total charge of all the protons in the nucleus of an atom. It is equal to the atomic number of the atom. The greater the nuclear charge, the stronger the force of attraction between the nucleus and the electrons.

Step 2: Compare the atomic numbers of Fluorine (F) and Boron (B). Fluorine has an atomic number of 9, meaning it has 9 protons, while Boron has an atomic number of 5, meaning it has 5 protons.

Step 3: Determine the effect of nuclear charge on the electrons in the n = 2 shell. The electrons in the n = 2 shell of Fluorine will experience a greater nuclear charge than the electrons in the n = 2 shell of Boron because Fluorine has more protons.

Step 4: Understand the concept of electron proximity to the nucleus. The greater the nuclear charge, the closer the electrons will be to the nucleus due to the stronger force of attraction.

Step 5: Determine which electrons will be closer to the nucleus. The electrons in the n = 2 shell of Fluorine will be closer to the nucleus than the electrons in the n = 2 shell of Boron because they experience a greater nuclear charge.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Effective Nuclear Charge (Z_eff)

Effective nuclear charge refers to the net positive charge experienced by an electron in an atom. It accounts for the actual nuclear charge (the number of protons) and the shielding effect of inner-shell electrons. In general, as the effective nuclear charge increases, electrons are pulled closer to the nucleus, affecting their energy levels and stability.

Electron Shells and Energy Levels

Electron shells are defined energy levels where electrons reside around the nucleus of an atom. The principal quantum number (n) indicates the shell's energy level, with lower numbers corresponding to shells closer to the nucleus. Electrons in lower energy levels experience a stronger attraction to the nucleus, influencing their stability and reactivity.

Comparison of Atomic Structure in Elements

When comparing elements like fluorine (F) and boron (B), it's essential to consider their atomic structure, including the number of protons and electron configurations. Fluorine has a higher atomic number than boron, resulting in a greater effective nuclear charge for its electrons. This difference affects the distance of the n = 2 electrons from the nucleus, with fluorine's electrons being closer due to the stronger nuclear attraction.

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Textbook Question

Detailed calculations show that the value of Zeff for the outermost electrons in Na and K atoms is 2.51+ and 3.49+, respectively. (e) Predict Zeff for the outermost electrons in the Rb atom based on the calculations for Na and K.

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Textbook Question

Detailed calculations show that the value of Zeff for the outermost electrons in Si and Cl atoms is 4.29+ and 6.12+, respectively. (a) What value do you estimate for Zeff experienced by the outermost electron in both Si and Cl by assuming core electrons contribute 1.00 and valence electrons contribute 0.00 to the screening constant?

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Textbook Question

Arrange the following atoms in order of increasing effectivenuclear charge experienced by the electrons in the n = 2shell: Be, Br, Na, P, Se.

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Textbook Question

Which quantity must be determined experimentally inorder to determine the bonding atomic radius of an atom?(a) The distance from the nucleus where the probability of finding an electron goes to zero.(b) The distance between the nuclei of two atoms that are bonded together.(c) The effective nuclear charge of an atom.

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Textbook Question

With the exception of helium, the noble gases condense to form solids when they are cooled sufficiently. At temperatures below 83 K, argon forms a close-packed solid whose structure is shown below. (b) Is this value larger or smaller than the bonding atomic radius estimated for argon in Figure 7.7?

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