Ch.7 - Periodic Properties of the Elements

Brown - Chemistry: The Central Science 14th Edition

Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경

Brown 14th Edition

Ch.7 - Periodic Properties of the Elements

문제 25

7장, 문제 25

Using only the periodic table, arrange each set of atoms in order from largest to smallest: (a) Ar, As, Kr (b) Cd, Rb, Te (c) F, O, N.

검증된 단계별 안내

Identify the position of each element (F, O, N) on the periodic table. Note that they are located in the second period.

Understand that atomic size decreases across a period from left to right due to the increase in the number of protons in the nucleus, which pulls the electrons closer.

Locate the elements in the periodic table: Nitrogen (N) is in Group 15, Oxygen (O) is in Group 16, and Fluorine (F) is in Group 17.

Since atomic size decreases from left to right across a period, the order from largest to smallest atomic size in the second period for these elements is N > O > F.

Arrange the atoms accordingly based on their atomic size: Nitrogen (N) is the largest, followed by Oxygen (O), and Fluorine (F) is the smallest.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Atomic Radius

The atomic radius is a measure of the size of an atom, typically defined as the distance from the nucleus to the outermost electron shell. Atomic radius generally decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus. Conversely, it increases down a group as additional electron shells are added, resulting in larger atomic sizes.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. Key trends include atomic radius, ionization energy, and electronegativity. Understanding these trends helps in predicting the behavior of elements, such as their size, reactivity, and bonding characteristics.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. While it primarily influences bonding behavior, it is also related to atomic size; smaller atoms with higher electronegativity tend to have stronger attractions for electrons. This concept is important for understanding how elements interact and form compounds.

관련 실천

교과서 질문

Using only the periodic table, arrange each set of atoms in order of increasing radius: (a) Cs, Se, Te (b) S, Si, Sr (c) P, Po, Pb.

515

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교과서 질문

Identify each statement as true or false: (b) Li⁺ is smaller than Li.

371

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교과서 질문

The experimental Pb¬Cl bond length in lead(II)chloride, PbCl2, is 244 pm. Based on this value and data in Figure 7.7, predict the atomic radius of Pb.

955

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교과서 질문

Identify each statement as true or false: (a) Cations are larger than their corresponding neutral atoms.

540

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교과서 질문

Which of the following statements about the bonding atomic radii in Figure 7.7 is incorrect? (i) For a given period, the radii of the representative elements generally decrease from left to right across a period. (ii) The radii of the representative elements for the n = 3 period are all larger than those of the corresponding elements in the n = 2 period. (iii) For most of the representative elements, the change in radius from the n = 2 to the n = 3 period is greater than the change in radius from n = 3 to n = 4. (iv) The radii of the transition elements generally increase moving from left to right within a period. (v) The large radii of the Group 1 elements are due to their relatively small effective nuclear charges.

1124

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교과서 질문

Estimate the As¬I bond length from the data in Figure 7.7 and compare your value to the experimental As ¬I bond length in arsenic triiodide, AsI₃, 2.55 Å.

589

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