The greater the electronegativity difference between the atoms in a molecule, the greater the dipole moment is
953238
It is true for individual bonds, but not for molecules.\nThe dipole moment of the molecule will depend on the geometry of the polar covalent bonds. E.g. CF4 has 4 polar bonds but they arranged so that the sum of their dipole moments is zero and the molecule has actually no dipole moment.
980772
A negative ion will be larger than the atom; a positive ion will be smaller than the atom.
78348
The answer has to do with symmetry of the molecule and hydrogen bonding.  That should get you going in the right direction
858630
Ionic bonds are created by attraction of separated charges or differences in electronegativity.  This results in a dipole moment, which is a vector property, hence it is directional.
770852
The bigger the atom,\nthe taller the radius,\nthe taller the distance of the outer electron to the center of the ion,\nthe weaker the electric bond between the outer electron and the ion,\nthe lesser the first ionization energy.\n\nTh
833384
as the number of electrons increases, the atom will form a new cloud after a certain number in each previous cloud. The inner electrons shield the outer electrons from the pull of the posetively charged nucleus (because the electrons are negative) so the electrons are more easily stolen. Thats why as you go down the periodic table, electronegativity decreases
161637
ionic,the diference in electronegativity values is greater then 1.6.  the metal bonded to a non metal method is also correct
932777
ok. To tell which elements are more metallic then others, It depends on the left over valence electrons that are attracted to the positively charged cations in a metal. To tell which elements are more active then others it is towards the right of the periodic table. Noble gases are non-reactive. To tell which atoms are bigger then others remember going from top to bottom in a group, atomic size increases, going from left to right across a period, atomic size decreases.(there is a pattern to this). \nI think if there are more valence electrons, the stronger the metallic bond is.
151202
All molecules are experience London Dispersion, or induced dipole-induced dipole forces.\n\nConsider He.  When both electons in the electron cloud are spontaneously bear one another, this causes a partial negative charge on one side of the atom and a partial positive charge on the other side.  This 'dipole' can then induce a dipole moment on another He atom.  London dispersion forces are relatively weak and exponentially dependent on the distance between atoms- so they must be relatively close to one another.
863219
Electronegativity is a measure of the ability of an atom or molecule to attract electrons in the context of a chemical bond. The type of bond formed is largely determined by the difference in electronegativity between the atoms involved. Atoms with similar electronegativities will share an electron with each other and form a covalent bond. However, if the difference is too great, the electron will be permanently transferred to one atom and an ionic bond will form. Furthermore, in a covalent bond if one atom pulls slightly harder than the other a polar covalent bond will form.\n\nThe Pauling scale was devised in 1932 by Linus Pauling. On this scale, the most electronegative chemical element (fluorine) is given an electronegativity value of 3.98 (textbooks often state this value to be 4.0); the least electronegative element (francium) has a value of 0.7, and the remaining elements have values in between. On the Pauling scale, hydrogen is arbitrarily assigned a value of 2.1 or 2.2.\n\n'ΔEN' is the difference in electronegativity between two atoms or elements. Bonds between atoms with a large electronegativity difference (greater than or equal to 1.7) are usually considered to be ionic, while values between 1.7 and 0.4 are considered polar covalent. Values below 0.4 are considered non-polar covalent bonds, and electronegativity differences of 0 indicate a completely non-polar covalent bond.\n\nHope I helped!...\n
786962
If the molecule has O,N,F,or Cl then most likely it is polar.  Look at the periodic chart and remember that the elements in the upper right are the most electronegative, so they want electrons.  When these elements are in a compound with other atoms such as C and H they will pull electrons closer making a dipole moment.  \n\nThe only real trick is looking at the geometry of the molecule, if there is more than one electronegative atom pulling in opposite directions then the dipole is canceld.  Such as O=C=O which is liniar.\n\nLook at an electronegativity chart you will see what I mean
879729
Please see my answer to your previous question for more details.\n\nThe more unshared pairs of e-, the more distortion in the geometry of the molecule.
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
992740
Higher the charge greater the tendency to accept electrons, hence more acidic\n\nLower the radius, higher concentration of charge, hence more acidic.\n\nIn3+ is larger than Al3+ hence a weaker acid.
963808
The ligand will accomodate electrons from the ligands, forming dative bonds.\n\nThe sub-shell also ceases into two groups of orbitals.  One group will be at a higher energy level as compared with the other.  The difference in energy level is acounted by the strength of the ligand, in other words, by its polarising power.  The stronger the ligand, the greater is the energy difference between the two groups of orbitals.
7601
The strength of C-O pi-bond is greater than that of C-C pi bond.(~ 364kJ/mol vs ~ 250 kJ/mol). Greater strength means greater stability. Thus the keto form is much favoured.
839080
(D) is the right answer because O is more electronegative than N and N is more electronegative than S. So H-O bond is more polar than H-N bond and H-N bond is more polar than H-S bond.