Covalent bonds form when atoms share electrons to achieve a stable electron configuration, typically a full outer shell (like the noble gases). This sharing occurs between two nonmetal atoms. The number of covalent bonds an atom can form is determined by the number of electrons it needs to complete its outer shell. For example, carbon needs four electrons and typically forms four covalent bonds.
Understanding the octet rule (atoms 'wanting' 8 valence electrons) is key to predicting how covalent bonds will form. Single, double, and triple bonds can form depending on the number of shared electron pairs.
Match the term with its definition:
| Term | Definition |
|---|---|
| 1. Covalent Bond | A. A bond formed by the sharing of electrons. |
| 2. Octet Rule | B. The tendency of atoms to prefer to have eight electrons in the valence shell. |
| 3. Lone Pair | C. A pair of valence electrons that are not shared with another atom. |
| 4. Single Bond | D. A covalent bond in which one pair of electrons is shared between two atoms. |
| 5. Double Bond | E. A covalent bond in which two pairs of electrons are shared between two atoms. |
Covalent bonds are formed when atoms _______ electrons. This typically occurs between two _______ atoms. The _______ rule explains why atoms form covalent bonds, as they seek to achieve a stable electron configuration with _______ electrons in their outer shell. A covalent bond where two electrons are shared is called a _______ bond.
Explain why covalent bonds are more common between nonmetal atoms than between metal atoms.
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