What noble-gas configurations and charges are the following elements likely to attain in reactions in which they form ions? (a) I (b) O (c) Al (d) Ca

Name: Chemistry
Author: McMurry
ISBN: 9781292336145

검증된 단계별 안내

Identify the position of each element in the periodic table to determine how many electrons they need to gain or lose to achieve a noble-gas configuration.

For iodine (I), which is in Group 17, determine how many electrons it needs to gain to achieve the electron configuration of the nearest noble gas, xenon (Xe).

For oxygen (O), which is in Group 16, determine how many electrons it needs to gain to achieve the electron configuration of the nearest noble gas, neon (Ne).

For aluminum (Al), which is in Group 13, determine how many electrons it needs to lose to achieve the electron configuration of the nearest noble gas, neon (Ne).

For calcium (Ca), which is in Group 2, determine how many electrons it needs to lose to achieve the electron configuration of the nearest noble gas, argon (Ar).

주요 개념

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

Noble Gas Configuration

Noble gas configuration refers to the electron arrangement of noble gases, which have full outer electron shells, making them stable and unreactive. Elements tend to achieve this configuration by gaining, losing, or sharing electrons during chemical reactions. For example, sodium (Na) loses one electron to attain the same configuration as neon (Ne), resulting in a stable ion.

Ion Formation and Charges

Ion formation occurs when atoms gain or lose electrons, resulting in charged particles called ions. Metals typically lose electrons to form positively charged cations, while nonmetals gain electrons to form negatively charged anions. The charge of the ion reflects the number of electrons lost or gained; for instance, oxygen (O) usually gains two electrons to form an O²⁻ ion.

Periodic Trends in Reactivity

Periodic trends in reactivity refer to the predictable patterns in how elements behave based on their position in the periodic table. Elements in the same group often exhibit similar reactivity due to their valence electron configurations. For example, alkali metals are highly reactive because they have one electron in their outer shell, while noble gases are largely inert due to their full outer shells.