What is the difference in ionic and covalent bonding?
157312
To put it very simply,\nin a covalent bond, the atoms share electrons,\nin an ionic bond, electrons from one atoms are totally removed and added to the other atom, forming ions.\n\nBut in all bonds, there is some degree of sharing, even ionic.  Atoms of different elements "pull" on electrons with different strengths, the stronger the pull (larger electron negativity), the more time the electron will be found around that atom as opposed to the other.\n\nHydrogen gas (H2) is a good example of a covalent bond between two of the same elements, in this case, they share the electrons perfectly since they both have the same electron negativity.\n\nHF, or Hydrogen Floride is an example of a very ionic bond, with an electronegativity difference of 2.0 (4.1 - 2.1).  In this case, the electrons being shared spend almost all of thier time around the Floride ion, making that side develop a negative charge whereas the Hydrogen develops a positive charge.
916600
Ionic compounds try to achieve the same thing...only instead of atoms sharing electrons with other atoms (co-valent) in a chemical bond, Ionic compounds achieve lowest energy configurations by receiving, or giving up, electrons.  For example, the sodium atom has one electron in it's valence "shell" and will give it up (becoming positively charged in the process) in order to have the same electronic configuration as the previous noble gas (neon) and becomes the sodium cation.\nFluorine, having seven electrons in it's valence shell would rather accept and electron (to have the neon electron configuration) and becomes the negatively charged fluoride anion.
979578
An ion is formed when one electron completely transfers over from one atom to another atom.  The one losing the electron acquires a positive charge and the one losing the electron acquires a negative charge.  But then these two ions are attracted to each other forming an ionic compound.  After coming together, the bonding electrons spend most of the time around the atom with the negative charge, that is, the more electronegative ion.  However, there are also moments when the electrons get closer to the electropositive atom.  Though it's rare to find the bonding electrons near the electropositive atom (since it's orbitals are higher in energy), calculations find that ~5% of the time the electrons are closer to the electropositive atom than to the electronegative atom.  (Don't trust me on the ~5%... this is based on only a few examples from my Inorganic Chemistry chapter I read a few weeks ago).  A popular example is that of HF.  If you use molecular orbital diagrams, you see that the 2s orbital is so low in energy (around -40eV) that it doesn't share it's electrons.  The 2p(z) orbital bonds with the hydrogen's 1s orbital but you'll see that the resulting bonding orbital is so close to the 2p(z) orbital in energy that you can sort of consider it somewhat nonbonding.  The point is that there is little influence from the H 1s orbital, but there is still a small amount of influence.  This means the bonding electrons spend a fraction of the time around the H atom, meaning that the original electron in question has no completely transferred over to the F atom.
953050
If the difference in the electronegativity between the two elements is less than 1.67, the bond will be covalent.\n\nNote: As to the statement that electronegative atoms don't form covalent bonds, that's nonsense.  ALL atoms are electronegative to some extent.  Just go look up the electronegativity series in any general chem. text.  Or check out this:\nhttp://dbhs.wvusd.k12.ca.us/webdocs/Bonding/Electroneg-Bond-Polarity.html
126671
Molecules always refer to atoms that have covalent bonds (like a water molecule). Stuff with ionic bonds are just ionic compounds.\n\nMore info: http://misterguch.brinkster.net/covalentcompounds.html
347735
1)ionic and covalent depend on the situation and are considered generally equal \n2)network bonds are a type of covalent bond\n3)metallic bonds are weaker (this one's kinda fuzzy)\n4)intermolecular are the weakest
59794
i dunno the first one...but sharing electrons is a covalent bond, and charged atoms are ions and they form ionic bonds
1075073
well it depends, but generally they don't stay that way for long. They react with other atoms that are charged opposite of whatever they are. This is how chemical bonds are formed. It can either be a covalent bond in which they atoms are "sharing" electrons in order for both to be neutrally charged or they form an Ionic bond.
233865
Generally, the elements that form ionic bonds tend to have either very high or very low electronegativity. This means the Alkali metals, Alkaline Earth metals, and the Halogens, especially when reacting with each other.
695062
ok listen if u have a compound formed by 2 atoms u take the electronegativity of the second atom and u substract the electronegativity of the first one if the number that u get is between 0 and 0.3 its non polar covalent if its 0.4-1.7 then its polar covalent and if its 1.7 or more than it is ionic
953247
the previous answer is deficient on the following points...\nelemental C has the atoms held together by covalent bonding\nNa, being a metal, has metallic bonding, not ionic. Ionic bonds occure BETWEEN a metal and a non metal such as Na with Cl.\nMetallic character decreases as you cross the periodic table, and increases as you go down the periodic table, so Na is more metallic than Fe\nnon metallic character does the opposite..\nSo from the list above, metallic character would be Na > Fe >C  > S > O\nNa is a metallic lattice while O2 exists as discrete molecules\nHope that helps
741551
Covalent.\nMetallic bond (do research on the Band Theory)\nIonic.\nCovalent.\nCovalent.\nIonic.
879105
Atoms may fill their valence shells by chemical bonding. This can be achieved one of two ways: \n1. an atom can either share electrons with other atoms (a covalent bond), \n2. or it can remove electrons from (or donate electrons to) other atoms (an ionic bond). The formation of a bond causes a strong attraction between two atoms, creating molecules or ionic compounds.
459909
If you're referring to Lewis structures, dashes represent pairs of electrons being shared between 2 atoms and dots represent one electron (see link below).  When there is more than one line connecting atoms, that means they are sharing more than one pair of electrons.  Ionic bonds aren't usually represented this way. But to do this, each atom is surrounded by dots representing the electrons present after they are transferred to bond, surrounded by brackets individually (brackets can be left off if there are no electrons after bonding), and the charge is marked in the upper right corner.  The second link shows an example with salt (NaCl).
960999
Well, obviously the donation of electrons from + to - atoms. Also, ionic compounds are soluble in water. Since ionic interactions are weak, they are weakly bound together.
740938
If a bond has ionic nature, the electrons have a tendency to hang out by one of the atoms in the bond more than the other... On the other hand if the bond is completely covalent in nature, the electrons are shared equally by both bonded atoms.
986449
The lead compounds would be much more covalent in character, with a very high bond strength (aka lattice enthalpy). Where a compound is insoluble, this energy is too high for hydration enthalpies (the energy released when water surrounds an ion of either charge) to compensate for.