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Step 1:I'll solve this problem step by step:
Step 2:: Identify the key characteristics of semimetals
- Semimetals (metalloids) are elements that have properties between metals and nonmetals - They are located along the zigzag line on the periodic table - Common semimetals include boron, silicon, germanium, arsenic, antimony, and tellurium
Step 3:: Consider bonding capabilities
- The ability to form four single covalent bonds requires: * Having 4 valence electrons * Being able to form stable covalent bonds
Step 4:: Analyze the semimetal properties
- Silicon (Si) is the semimetal that perfectly matches these requirements - Silicon is located in Group 14 (IVA) of the periodic table - It has 4 valence electrons in its outer shell - Can readily form four single covalent bonds - Commonly used in semiconductor and electronics industries
Step 5:: Verify bonding characteristics
- Electronic configuration of silicon: $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{2}
- Can hybridize its orbitals to form 4 equivalent covalent bonds
Final Answer
Silicon (Si) is the semimetal that can form four single covalent bonds.
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