- Which member of each of the following pairs of compounds would most likely contain covalent bonds? a. BaO or CO b. ClF or NaF c. FeCl3 or NCl3 d. CH4 or CaCl2
- Which member of each of the following pairs of compounds would most likely contain covalent bonds? a. Na2O or H2O b. SnO2 or CO2 c. BrCl or AlCl d. NH3 or Mg2N
The Correct Answer and Explanation is :
Answer:
- a. CO
- Explanation: In BaO (Barium oxide), Ba is a metal, and O is a non-metal, so the bond between them would be ionic, with the metal giving up electrons to the non-metal. However, in CO (Carbon monoxide), both carbon and oxygen are non-metals, meaning they are likely to form a covalent bond by sharing electrons. Hence, CO is more likely to contain covalent bonds. b. ClF
- Explanation: In ClF (Chlorine fluoride), both chlorine and fluorine are non-metals, so they will form a covalent bond through electron sharing. On the other hand, NaF (Sodium fluoride) consists of a metal (Na) and a non-metal (F), which would form an ionic bond. Therefore, ClF is more likely to contain covalent bonds. c. NCl3
- Explanation: In NCl3 (Nitrogen trichloride), both nitrogen and chlorine are non-metals, and they will form covalent bonds. In contrast, FeCl3 (Iron chloride) consists of a metal (Fe) and a non-metal (Cl), so it will have ionic bonds. Thus, NCl3 is more likely to contain covalent bonds. d. CH4
- Explanation: In CH4 (Methane), carbon and hydrogen are both non-metals, so they will form covalent bonds by sharing electrons. On the other hand, CaCl2 (Calcium chloride) involves a metal (Ca) and a non-metal (Cl), leading to an ionic bond. Therefore, CH4 is more likely to contain covalent bonds.
- a. H2O
- Explanation: In H2O (Water), both hydrogen and oxygen are non-metals, and they form covalent bonds by sharing electrons. Na2O (Sodium oxide), however, involves a metal (Na) and a non-metal (O), so it will form ionic bonds. Hence, H2O is more likely to contain covalent bonds. b. CO2
- Explanation: In CO2 (Carbon dioxide), both carbon and oxygen are non-metals, so the bond between them will be covalent. On the other hand, SnO2 (Tin dioxide) involves a metal (Sn) and a non-metal (O), leading to an ionic bond. Therefore, CO2 is more likely to contain covalent bonds. c. BrCl
- Explanation: In BrCl (Bromine chloride), both bromine and chlorine are non-metals, so the bond is covalent. In contrast, AlCl (Aluminum chloride) consists of a metal (Al) and a non-metal (Cl), leading to ionic bonding. Hence, BrCl is more likely to contain covalent bonds. d. NH3
- Explanation: In NH3 (Ammonia), both nitrogen and hydrogen are non-metals, so they will form covalent bonds. Mg2N (Magnesium nitride), however, involves a metal (Mg) and a non-metal (N), so it will form ionic bonds. Therefore, NH3 is more likely to contain covalent bonds.
Summary:
- Covalent bonds tend to form between non-metals, as they share electrons.
- Ionic bonds tend to form between metals and non-metals, with electron transfer occurring from the metal to the non-metal.
I’ll generate an image to visualize these concepts now.
Here’s a diagram comparing ionic and covalent bonds to help visualize the differences between them. It highlights how ionic bonds involve the transfer of electrons between a metal and a non-metal, while covalent bonds involve the sharing of electrons between two non-metals.
