Anena Sheila
4 hours ago
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4 hours ago
1. Covalent compounds are formed by the sharing of electrons between atoms.
2. They have low melting and boiling points compared to ionic compounds.
3. Covalent compounds are typically insoluble in water.
4. They do not conduct electricity in their solid or liquid state.
5. Covalent compounds can be either molecular or network covalent structures.
6. They often have a lower density compared to ionic compounds.
7. Covalent compounds can exhibit a wide range of physical properties, depending on the specific atoms and bonds present in the molecule.
2. They have low melting and boiling points compared to ionic compounds.
3. Covalent compounds are typically insoluble in water.
4. They do not conduct electricity in their solid or liquid state.
5. Covalent compounds can be either molecular or network covalent structures.
6. They often have a lower density compared to ionic compounds.
7. Covalent compounds can exhibit a wide range of physical properties, depending on the specific atoms and bonds present in the molecule.
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Google Gemini AI
4 hours ago
Characteristics of Covalent Compounds:
- Formation:
- Formed by the sharing of electrons between atoms.
- Electrical Properties:
- Generally nonpolar or slightly polar (depending on electronegativity difference).
- Do not conduct electricity in the solid or liquid state.
- Solubility:
- Usually insoluble in water (polar solvents).
- Soluble in nonpolar solvents (e.g., gasoline, oil).
- Physical State:
- Range in physical state at room temperature from gases (e.g., methane) to liquids (e.g., water) to solids (e.g., diamond).
- Molecular Structure:
- Form discrete molecules that consist of two or more atoms.
- Have varying molecular shapes, depending on the number of bonding atoms and lone pairs.
- Chemical Properties:
- Generally react by forming new bonds or breaking existing ones.
- Can form hydrogen bonds with other molecules containing lone pairs (e.g., water).
- Bonding:
- Covalent bonds are directional and have specific geometries (e.g., tetrahedral, trigonal planar).
- Bond strength is determined by the number of electron pairs shared and the electronegativity of the atoms involved.
- Examples:
- Water (H2O)
- Methane (CH4)
- Carbon dioxide (CO2)
- Diamond (carbon network)
- Formation:
- Formed by the sharing of electrons between atoms.
- Electrical Properties:
- Generally nonpolar or slightly polar (depending on electronegativity difference).
- Do not conduct electricity in the solid or liquid state.
- Solubility:
- Usually insoluble in water (polar solvents).
- Soluble in nonpolar solvents (e.g., gasoline, oil).
- Physical State:
- Range in physical state at room temperature from gases (e.g., methane) to liquids (e.g., water) to solids (e.g., diamond).
- Molecular Structure:
- Form discrete molecules that consist of two or more atoms.
- Have varying molecular shapes, depending on the number of bonding atoms and lone pairs.
- Chemical Properties:
- Generally react by forming new bonds or breaking existing ones.
- Can form hydrogen bonds with other molecules containing lone pairs (e.g., water).
- Bonding:
- Covalent bonds are directional and have specific geometries (e.g., tetrahedral, trigonal planar).
- Bond strength is determined by the number of electron pairs shared and the electronegativity of the atoms involved.
- Examples:
- Water (H2O)
- Methane (CH4)
- Carbon dioxide (CO2)
- Diamond (carbon network)
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