Arrange these elements in order of increasing electronegativity:?
968327
The more at the top of the table, the more electronegative the element is.  So it's I Br Cl F
27684
Protons, neutrons, and electrons.
452453
No, we don't use the electronegativity chart; instead we draw the full structure of the molecule and then see which 'pulling of bonds' cancel each other. \nIn the molecule AsF3, since As has 5 outer most electrons(in group 5), each F is bonded to As with a single covalent bond. Hence, the shape of the molecule becomes trigonal pyramidal, with 3 bond pairs (with 3 F atoms) and 1 lone pair. The 3 bond pairs pull the electrons towards themselves in the lower plane, while the 1 lone pair pulls at the top. The pulling effect of the 2 F atoms at the 2 sides cancel out  because the pulling effect is the same for both F atoms; however, the pulling effect of the lone pair at the top and the 1 F bond pair at the bottom will not cancel, because it is not from the same atom/species. Hence the overall dipole moment( dipole moment = charge x distance) does not cancel out, so the molecule is polar, with some charge distribution remaining due to the unequal pulling effect.\n\nIn CF3Cl, the shape is tetrahedral, with the 3 Cl atoms and 1 F atom bonded by single covalent bonds to the central C atom. The bond pairs spread out with the 3 Cl atoms pulling at the bottom and the 1 F atom pulling at the top. The pulling effect of the 2 Cl atoms at the sides cancels out, but that of the F atom at the top and the Cl atom at the bottom does not, as the pullin effect of 2 different atoms is different. Hence, as before, overall dipole does not cancel and the molecule is hence polar.
697038
This is kinda hard to draw on here...\n......_\nK--Br|\n......_\n\nThe lines around Br represent 2 electrons, and the -- represents a bond...ignore the periods
191934
Two in the first shell. 10 in the second shell. 10 in the third shell. 5 in the 4th shell for neutral Manganese. Mn 2+ is missing 2 electrons, so it would only have 3 in the outer shell. The rest will stay the same.\n\nHere's a cool interactive periodic table that may help you with your homework. \n\nhttp://www.webelements.com/\n\nYou can click on the the element you are interested in, then in the column on the left you can go to electronic properties and it will show you how the electrons are distributed. You can add or remove electrons to configure the electron arrangement of various ions of the substance you are interested in.
765496
first of all write the molecular orbital configuration.then count the number of electrons with sigma bonds i.e., no. of bonding orbital electrons and then count the number of electrons with pi bonds i.e., no. of antibonding orbital electrons .Then\n\n bond order = 1/2[(No. of  bonding orbital  electrons) -(No.of antibonding orbital electrons)]
719199
You are supposed to use symmetry and electronegativities to answer this. Draw the three dimensional structure and identify which atoms have the highest electronegativity. That will give you your dipole moment.\n\nIn this case, Br has a higher electronegativity than C and H, so the positive charge will be directed towards the C and the negative between the two Br atoms.
284634
3K4Fe(CN)6 + 4FeCl3 -> 12KCl + Fe4[Fe(CN)6]3
253611
Li+\nBe2+\nB3+\nN3-\nO2-\nF-
791300
Use the FOIL method; First, Outer, Inner, Last.\n\nFirst, n * n\n\nOuter, n * 5\n\nInner, n * 7\n\nLast 7 * 5.\n\nThen add them all together.\n\n22 NOV 06, 0420 hrs, GMT.
933205
electron affinity\n\nas you are changing Cl2 ->2Cl-
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
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.
87280
MBrO3-9H2O where M can be Na,K,Li, other +1 cations\n\nIf M is other than these you have to adjust subscripts
367163
F has more electronegativity. That means that F doesn't share electrons nicely.  It holds the electron closer and doesn't let H have it much.  This makes F more negative and H more positive.
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
873114
→ Atomic radius decreases → Ionization energy increases → Electronegativity increases →\n\nIn general, the degree of electronegativity decreases down each group and increases across the periods, as shown below. Across a period, non-metals tend to gain electrons and metals tend to lose them due to the atom striving to achieve a stable octet. Down a group, the nuclear charge has less effect on the outermost shells. Therefore, the most electronegative atoms can be found in the upper, right hand side of the periodic table, and the least electronegative elements can be found at the bottom left. \n\nGenerally speaking, atomic ionization energies decrease down a group of the periodic table, and increase left-to-right across a period. Ionization energy exhibits a strong negative correlation with atomic radius.