First of all, not all molecular bonds are covalent, any bond that involves a metal is an ionic bond. These bonds occurs because every element except the noble gases (the elements on the rightmost group: Helium, Neon, Argon, krypton, Xenon, and Radon) want to take or lose Valence electrons (the outermost electron shell) so that they have all full shells of electrons (the first shell holds 2, then 8,18 etc.), like the noble gases. To bond elements can give, take or share electrons with other elements, and they will arrange themselves into molecules with a certain number of each element, so every element has the number of electrons it "wants".
covalent bonds
A pure compound which contains covalent bonds is CO2 gas that you breathe out. Another example found in every day life is water.
Ionic bonds, covalent bonds, and probably hydrogen bonds
Covalent bonding is a type not found in metals (there mainly metal bonds or ionic bonds) In nonmetals more covalent bonding is common.
The substance not paired correctly isCl2 - polar covalent bonds.
covalent bonds
A pure compound which contains covalent bonds is CO2 gas that you breathe out. Another example found in every day life is water.
Ionic bonds, covalent bonds, and probably hydrogen bonds
Covalent bonding is a type not found in metals (there mainly metal bonds or ionic bonds) In nonmetals more covalent bonding is common.
The substance not paired correctly isCl2 - polar covalent bonds.
There are covalent bonds found in TTX and a covalent bond is a sharing of two electrons between two atoms in a molecule.
Covalent. I had this same question and then found the answer! Hope this helps!
There are four covalent bonds in Carbon Tetrachloride. The bonds sit between C and Cl.
collagen
Sodium chloride has an ionic bond.
Covalent bonds between carbon-carbon and carbon-hydrogen
Metallic bonds are similar to highly delocalised bonds found in giant covalent molecules, such as those found in graphite. Other substances with a metallic appearance such as galena lead sulfide, PbS and iron pyrites, FeS2 although usually considered at high school level to be ionic are in fact semiconductors implying covalency and delocalisation.