Tucson, AZ Plumbing
In & Out Plumbing, LLCIn & Out Plumbing, LLC provides complete commercial and residential plumbing services to the Tucson, AZ area.When price and time matter - call us first for solutions to all your Plumbing needs. Our technicians are troubleshooting experts and always provide prompt and professional service. We offer the quality service that you can count on with honest prices - no hidden charges. We provide free estimates.
No. Two atoms of similar or identical electronegativity would form a nonpolar covalent bond.
They form both. For example, the standard alkyls, alcohols, acids, amines, aminos, etc. form covalent bonds, but organometallic compounds, salts of acids and amines, and similar compounds form ionic (although still using covalent bonding for part of thir structure).
The bond in Si normally described as covalent. Its structure is similar to that of diamond.
Buckminsterfullerene, has a lower melting point than diamond and graphite because it has a simple molecular structure. This means that unlike graphite and diamond the strong covalent bonds do not extend throughout the structure. The intermolecular bonds between molecules of C60 are easier to break and therefore it is much easier to separate C60 into it's individual molecules through the input of energy. However the covalent bonds between each atom of C60 is just as strong as the covalent bonds holding both diamond and graphite together, and similar amounts of energy would be required to split the three into it's individual atoms.
In giant molecules such as diamond, silon dioxide, the atoms are all regularly positioned and form a lattice. In this respect they are similar to ionic compounds.
No. Two atoms of similar or identical electronegativity would form a nonpolar covalent bond.
They form both. For example, the standard alkyls, alcohols, acids, amines, aminos, etc. form covalent bonds, but organometallic compounds, salts of acids and amines, and similar compounds form ionic (although still using covalent bonding for part of thir structure).
The bond in Si normally described as covalent. Its structure is similar to that of diamond.
Four. they are arranged tetrahedrally. The structure is similar to diamond.
Germanium, metalloid with a similar structure to silicon- 4 covalent bonds per germanium atomPhosphorus, the most familiar form is white phosphorus which is molecular, consisting of P4 units, each P atom has 3 covalent bonds, other allotropes are not discrete molecules but all have 3 covalent bonds per P atomSelenium This is molecular in Se8 rings each Se atom has two covalent bondsChlorine this is a diatomic gas with a single covalent bond
Buckminsterfullerene, has a lower melting point than diamond and graphite because it has a simple molecular structure. This means that unlike graphite and diamond the strong covalent bonds do not extend throughout the structure. The intermolecular bonds between molecules of C60 are easier to break and therefore it is much easier to separate C60 into it's individual molecules through the input of energy. However the covalent bonds between each atom of C60 is just as strong as the covalent bonds holding both diamond and graphite together, and similar amounts of energy would be required to split the three into it's individual atoms.
Covalent molecules which contain only bonds between elements of similar electronegativity. For example: Carbon and hydrogen. They must not contain polar bonds like Oxygen and hydrogen.
In giant molecules such as diamond, silon dioxide, the atoms are all regularly positioned and form a lattice. In this respect they are similar to ionic compounds.
When atoms have a similar electronegativity, (Tendency to take electrons) they can't form ionic compounds where one becomes positive (gives an electron or some of them) and the other negative (takes that electrons). Instead they share it with other atoms in covalent bonds (both are neutral). Most organic compounds are covalent-bonded, like methane, ethane, propane, butane, isobutane, ethanol. Other non organic molecules that are covalent are diatomic molecules (O2, H2, Cl2), ammonia...
Both molecules have a hydrophobic hydrocarbon-chain and ibuprofen has a hydrocarbon ring structure. This makes them very similar along with the polarity and structure in this case "like dissolves like".
Compounds are made of molecules
Electronegativity dif. - dEN 0 > dEN > 0.6 ----> covalent (I think this is what you mean by "similar") 0.7 > dEN > 1.6 -----> polar covalent 1.7 > dEN > 4.0 ------> ionic