The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? c. O 2s²2p⁴

검증된 단계별 안내

Identify the number of valence electrons for oxygen. Oxygen is in group 16 of the periodic table, so it has 6 valence electrons.

Write the electron configuration for the valence shell of oxygen: 2s^2 2p^4.

Determine the number of unpaired electrons in the valence shell. In the 2p subshell, there are 4 electrons, which means there are 2 unpaired electrons.

Each unpaired electron can form a bond, so the number of bonds oxygen can form without hybridization is equal to the number of unpaired electrons.

Conclude that oxygen can form 2 bonds without hybridization, as it has 2 unpaired electrons in its 2p subshell.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

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

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how an atom can bond with others. The number of valence electrons influences the atom's ability to form bonds, as these electrons are involved in chemical reactions and bond formation.

Octet Rule

The octet rule states that atoms tend to form bonds in such a way that they have eight electrons in their valence shell, achieving a stable electron configuration similar to that of noble gases. This rule helps predict the bonding behavior of elements, particularly in covalent bonding.

Bonding Capacity

Bonding capacity refers to the maximum number of bonds an atom can form based on its valence electron configuration. For oxygen, which has six valence electrons (2s²2p⁴), it can typically form two bonds to achieve a full octet, allowing it to stabilize its electron configuration.

The valence electron configurations of several atoms are shown here. How many bonds can each atom make without hybridization? c. O 2s22p4