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A short class with Sarah and her students. The other ways are under More.
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Let's talk about covalent compounds. What do you think distinguishes them from ionic compounds?
I think it's about how they form bonds, right? Sharing electrons instead of transferring them!
Exactly! Covalent compounds form by sharing electron pairs. Now, what about their melting and boiling points?
I remember they have lower melting and boiling points compared to ionic compounds.
Correct! We could say they are like a loose cluster compared to ionic compounds, which have strong attractions. Why do you think that affects their states of matter?
Because they can be gases or liquids, not just hard solids? Like water and oxygen?
Right again! They can exist as gases, liquids, or solids. Let's summarize: covalent compounds tend to have low melting and boiling points and can exist in various forms.
Now, we need to explore how covalent compounds behave in water. Any ideas on their solubility?
I think many of them are not very soluble in water.
That's right! In contrast to ionic compounds that generally dissolve in water, many covalent compounds remain insoluble. Can you think of an example of a covalent compound that is insoluble?
Like oil in water?
Perfect example! Oil is a covalent compound. Now, let’s move on to conductivity. Why do covalent compounds not conduct electricity?
Because they don’t have free ions to move around?
Exactly! Unlike ionic compounds that have dissociated ions, covalent compounds lack free ions, so they do not conduct electricity. Summarize what we discussed about solubility and conductivity for covalent compounds, please.
They are usually insoluble in water and do not conduct electricity.
Formed by sharing electron pairs.
Compared to ionic compounds due to weaker forces.
Can exist as gases, liquids, or solids.
Often insoluble in water.
Do not conduct electricity because they lack free ions.
Covalent bonds share, they seldom break air, lower points they declare.
Imagine two friends, Hydrogen and Oxygen, sharing an umbrella (electrons) to keep dry, creating water. They don't need to be solid to stick together!
To remember properties: M-S-E-C: Melting points low, States could vary, Electricity none, Conductivity is zero.
COVALENT: C - Can be various states, O - Often low melting points, V - Very low solubility, A - Always no conduction of electricity, L - Lighter than ionic, E - Easily recognized by shared pairs, N - Never dissolved like ionic, T - Typically less dense.
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What are covalent compounds?
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Why do covalent compounds have lower melting points?
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Do covalent compounds conduct electricity?
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A chemical compound formed by the sharing of electron pairs between atoms.
The temperature at which a solid becomes a liquid.
The temperature at which a liquid becomes a gas.
The ability of a substance to dissolve in a solvent.
The ability of a substance to conduct electricity.
This section describes the properties of covalent compounds, which differ significantly from those of ionic compounds.
Covalent compounds typically have lower melting and boiling points compared to ionic compounds, and they may exist as gases, liquids, or solids. These compounds are usually less soluble in water and do not conduct electricity due to the absence of free ions.
Covalent compounds are defined by the way they form bonds, specifically through the sharing of electron pairs between atoms. Here are the key characteristics:
Understanding these characteristics is crucial for predicting the behavior of covalent compounds in chemical reactions and their applications in real-world scenarios.