We expect Ionic bond in the above compound but it is written in text books as covalent bond, if so how is the formation of the bond.
208730
The Be2+ cation is smaller in size (being above the rest of the group 2 elements) and hence has high charge density. This enables it to easily polarise the comparatively larger Cl- anion, which results in a covalent characteristic of the compound. As explained clearly in the previous answer, dative bonding occurs in the compound and BeCl2 usually occurs as a dimer i.e Be2Cl4 (polymeric type) based on the linear molecular structure of BeCl2.\n\nPolarisation occurs between a small cation with high charge density and a larger anion. Since the size of the cations of the group 2 elements increases down the group (more atomic radius), charge density around the cation decreases and hence their ability to polarise the Cl- also decreases, resulting in an ionic compound.
659596
No. Think about connections. CH3-CH2-O-S-O3H. The ethyl must bind to an oxygen, not the hydrogen. [CH3CH2]- [HSO4]+ would seem to be the right "ionic" form, but these aren't ions.\n\nYou need to show that the hydrogen is on one side of the sulphur and the ethyl is on the other side, and each of them are connected through oxygens.
546211
You should probably need your periodic table.\nGenerally chemical formulas are for ionic compounds, hence you need to know the charges of the ions formed.\nAll Group I metals form ions of +1 charge, Group II metals forms +2 charged ions, Group III (like Al) forms +3 charge, Group IV prefers to share, seldom will they form ions, hence we shall keep them out of the picture.\nGroup V non-metals form -3 charge, Group VI -2 and Group VII -1. Group O elements have full outermost shell, hence they seldom participate in bonding.\nSo if you are looking at magnesium oxide, the ionic compound is formed between magnesium ion (Group II, hence Mg2+) and the oxide ion (from oxygen, Group VI, hence O2-).\nYou will realise that to balance the charges, you need exactly 1 Mg2+ and 1 O2-. Hence the chemical formula of magnesium oxide is MgO.\nAnother example, for sodium chloride. Sodium ion (Na+) and chloride ion (Cl-). Hence 1 of each is needed to balance the charges and the formula is NaCl.\nAnother example, lead (IV) oxide. Lead is a transition metal and transition metals form ions of variable valencies. Lead (IV) means the charge of the lead ion here is Pb4+. Thus you need 1 Pb4+ and 2 O2- (so that the charges are cancelled) for lead (IV) oxide, PbO2.\nYou have also polyatomic ions, like hydroxide (OH-), sulphate [(SO4)2-], nitrate [(NO3)-] and carbonate [(CO3)2-]. Similarly, ionic compounds formed will require the balance of charges.\nExample, with sodium sulphate.\nYou have Na+ and sulphate [(SO4)2-].\nYou will need 2 sodium ions to balance the -2 charge of the sulphate ion. Hence the chemical formula is Na2SO4.\nHope this helps. :)
469907
Covalent bond: bond in which one or more pairs of electrons are shared by two atoms.\n\nIonic bond: bond in which one or more electrons from one atom are removed and attached to another atom, resulting in positive and negative ions which attract each other.
121334
1. electron\n2. ionic\n3. molecules of compounds\n4. decomposition (not sure)
445590
Generally Group I and Group II elements form ionic compounds with non-metals. Hence for all of the metals above, they should form ionic compounds with oxygen.\nSodium - Na+; oxide - O2-\nHence you need 2 sodium ions to calcen out the -2 charge on the oxide ion, and the formula of sodium oxide is Na2O.\nSimilarly for potassium oxide, K2O.\nCalcium - Ca2+, oxide - O2-\n1 of each is needed to cancel out the charges, hence the formula CaO.\nSimilarly for MgO.\nAns: Na2O, K2O, MgO and CaO\n\nHope this helps :)
515948
You get the first answered.\nCovalent bonds are strong and don't disassociate into ions, as ionic bonds do. Watch.\nNaCl common salt, sodium and chlorine, put in solution.\n\nNa+  and Cl- they disassociate and you can follow the path of electricity Electron jumps from sodium to be accepted by chlorine. That is electron flow; conduction of electricity.
191934
manesiun and fluorine....magnesium forms a positively charged ion, while fluorine forms a negatively charged ion, different charges attract, so they form ionic bond to each other forming a ionic compound.\n\nnitrogen and sulphur both form negative charged ions, so there is noway to make them react unless in a prescence of a catalyst.\n\nionic compounds generally fom using, metals and nonmetals. magnesium is a metal, and fluorine nitrogen and sulphur are all non metals
347740
KCl(aq) + AgNO3(aq)  --> KNO3(aq) + AgCl(s)\n\nNet ionic: Cl-(aq) + Ag+(aq)  --> AgCl(s)\n\nNa2SO4(aq) + Ba(NO3)2  --> 2NaNO3(aq) + BaSO4(s)\n\nnet ionic: SO4(-2)(aq) + Ba(+2)(aq)  --> BaSO4(s)
416403
Covalent bond: are those which one or more pairs of electrons are shared by two atoms.\nCovalent chemical bonds involve the sharing of a pair of valence electrons by two atoms, in contrast to the transfer of electrons in ionic bonds. These bonds lead to stable molecules if they share electrons in such a way as to create a noble gas configuration for each atom. \n\nHydrogen gas forms the simplest covalent bond in the diatomic hydrogen molecule. The halogens such as chlorine also exist as diatomic gases by forming covalent bonds. The nitrogen and oxygen which makes up the bulk of the atmosphere also exhibits covalent bonding in forming diatomic molecules. \n\n\n\nIonic Bonds\nIn chemical bonds, atoms can either transfer or share their valence electrons. In the extreme case where one or more atoms lose electrons and other atoms gain them in order to produce a noble gas electron configuration, the bond is called an ionic bond. \n\nTypical of ionic bonds are those in the alkali halides such as sodium chloride, NaCl\n\n\nThe below reference has some diagrams which are helpful as well.
528618
no boron as with berylium among others is an exception to the octet rule. when bonding, the boron need only to share 3 bonds with (an)other element/s translating to 6 electrons for it to become stable... an example of a compound following this setup is triflouride (BF3)\n\ni hope that helps...
363990
1)SO2, the sulfur, when it burns in air reacts with the O to form SO2. When Mg burns in air it reacts with the O and the N in the air and forms both MgO and Mg3O2. The product SO2 is a gas and MgO and Mg3O2 is a solid.\n\n2)It is ionic. Ionic bonds form between a + ion and a - ion. Na is + and F is -.\n\n3)P with O is covalent. Both elements are negative ions so they share. You need a + and a - to be ionic.\n\n4)No! Lots and lots of liquids. Some solids also.\n\n5)O and S are in the same groups because they both have 2 electrons in their outer shells. P and S are next to each other because they both have the same number of energy levels (3).\n\nGet an "A".
421776
i think an ion makes up a molecule. i am taking physical science and i went over it a few weeks ago.
401972
An element is ionic if it doesn't have a charge of zero. This would be if it was in a compound with any other element because the total charge of that compound would equal zero. If the element was by itself, it should have a charge of zero. I'm pretty sure there are some exceptions.
425294
No concrete way to work it out. Groups one and two take positive charges equal to their group number (Mg2+, Li1+ etc). Groups 3, 4, 5, 6 and 7 ionise to a negative charge of 8 minus their group number (Cl1-, O2- etc), though 3, 4, and 5 tend to resist ionisation and are much more commonly found bonded covalently. The Transition elements ion charges are virtually impossible to predict without an extensive knowledge of d orbitals etc..
421066
'A Person' gives a short, simple, and correct answer. \n\nIt is simply when two atoms (ions [thus the name]) join to form a compound. One ion is + the other -.\n\nGet an "A".
511580
1. NaCN\n2. NO2\n3. CuCl2\n4. NaC2H3O2 \n5. F2\n6. bonding involves transfer of electrons between atoms