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ldv1452
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For inorganic molecules, is ionic or covalent bonding more common?
Borek said:This answer is about as vague as the question was.
Sodium sulfate - does it contain ionic, or covalent bonds?
samblohm said:I was thinking in the earth, ionic is far more common. Silicon dioxide- ionic. Iron, aluminum, carbon, magnesium, calcium, oxide (dioxide). And I have a quick question- in a hydroxide, are the O and the H ionic or covalently bonded to each other?
The main difference between ionic and covalent bonding is the way in which atoms are bonded together. In ionic bonding, one atom gives up an electron to another atom, creating positively and negatively charged ions that are attracted to each other. In covalent bonding, atoms share electrons to form a stable outer electron shell.
Ionic bonds are generally stronger than covalent bonds. This is because ionic bonds involve the transfer of electrons, creating strong attractions between oppositely charged ions. Covalent bonds, on the other hand, involve the sharing of electrons, which may not be as strong as the attraction between ions.
You can determine if a compound has ionic or covalent bonding by looking at the elements involved. Ionic bonding usually occurs between a metal and a nonmetal, while covalent bonding typically occurs between two nonmetals. You can also look at the electronegativity difference between the atoms; a larger electronegativity difference indicates ionic bonding, while a smaller difference indicates covalent bonding.
Yes, compounds can have both ionic and covalent bonding. This is known as polar covalent bonding, where the electrons are shared unequally between atoms, creating partial charges. An example of this is water, which has both ionic and covalent bonding between the oxygen and hydrogen atoms.
The type of bonding in a compound can greatly affect its properties. Ionic compounds tend to have high melting and boiling points, are usually soluble in water, and conduct electricity when dissolved in water. Covalent compounds, on the other hand, have lower melting and boiling points, are not usually soluble in water, and do not conduct electricity. The strength of the bonds also affects the hardness and brittleness of the compound.