Using only the elements P, Cl, and Ca, give a formula for an ionic compound?
CaCl2
Using only the elements Ca, Cl, Si, give formulas for an ionic compound.?
CaCl2 and SICl4
Using only the elements P, Cl, and Ca, give a formula for a molecular compound with polar covalent bonds that?
That? ... that what? rest of question appears missing! Didn't you check what you posted?
Using only the elements P, Cl, and Ca, give a formula for an ionic compound.?
I doubt there is any such compound. There is such a thing as CaClO3P, but it requires oxygen too.
What are some compounds that contain both ionic and covalent bonds?
Electron sharing involves the sharing of electrons between two atoms and the creation of covalent bonds. Covalently bonded compounds typically have very different properties from ionic compounds, and they also involve combinations of different types of elements.KNC: Potassium cyanide.NH4Cl ( ammonium chloride).N2O4: Dinitrogen tetroxide, commonly referred to as nitrogen tetroxide.NaNO3 - sodium nitrate(NH4)S - ammonium sulfide Ba(CN)2 Barium cyanide. CaCO3 : Calcium sulfite, or calcium sulphite.CaSO4: Calcium sulfate (or calcium sulphate).Also remember also polyatomic ions (relating to a molecule made up of more than two atoms.) are held together by covalent bonds, so this compound contains both ionic and covalent bonds.
How do I find if a compound is ionic or covalent by just looking at its chemical formula?
If you are very familiar with the periodic table of elements, you will notice that elements are grouped in vertical column called groups and horizontal rows called period.The first three columns to the left (ie groups 1, 2 and 3) are classified as metals due to their very low electronegative values, while columns far right with exception to the very last column (ie groups 5,6 and 7) are classified as non metals due to their high electronegative values.Now to go straight to your question on how to easily identify if a compound is ionic or covalent just by inspection. What you have to do is to look at the compound this way:if the compound is made of just two elements, if one is a metal (ie belongs to any of groups 1, 2 or 3) and the other element a non metal, (ie belongs to group 5, 6 or 7) then the compound is most likely to be an ionic compound. For example NaCl, MgOIf the compound is made of identical non metalic elements as in O2, Cl2 then the compound is covalentIf the compoud is made of just two elements that are both non metals such as in SO2, CO, NO, CCl4, the compound is covalentIf the compound is made up of more than two elements, such as in HNO3, Na2CO3, CuSO4.5H2O, you may need to break the compound into dissociating parts. You will see that, the compounds are ionic.Hydrocarbons, compounds containing only hydrogen and carbon of varying molecular size are all covalent. Examples are C2H6, C2H4, C2H2,Note that there could be some little exceptions to the examples given. Mostly with first members of every group because of their small size which make them show substantial deviations from group behavior. For example HCl is covalent not ionic.I hope this help
Use only the elements Ca, Cl, Si, give formulas for a compound with polar covalent bonds that obeys the octet rule and has no formal charges?
SiCl4; Si is in the center, each Cl is bonded to the Si
Why is hydrogen chloride (HCl) a covalent compound? Why can't it be an ionic compound?
HCl is polar (covalent), because the electron from the H only spends most of its time around the Cl nuclei, (H-es need an electron too,) whereas the Na in NaCl - an ionic compound - would prefer to lose its valence electron and become a positive ion. hydrogen is weird and an exception, because when neutral it only uses its innermost shell and would not be stable as just a (positive) proton and (neutral) neutron with no (negative) electrons whatsoever. Na does use its other shells, so can just fall back on their electrons to remain stable and balanced. now that we've established that a complete electron transfer is not going on in the case of HCl, we know that the H will sustain a slight positive charge, and Cl will sustain a slight negative one, making the compound polar. (we also know that it is not nonpolar because the electronegativity difference is greater than 1.6- data that will be on any complete and up to date periodic table)
Is NaF a covalent or ionic compound? What are the differences between covalent and ionic?
Once again you have found yourself on a lower rung of Wittgenstein's ladder, lies for children. These are prototypes, ie at the opposite poles of a spectrum of variation, so it is valid to talk about degree of ionic character or degree of covalent character, depending on your preference.You could say that chemists invented fuzzy logic before the mathematicians formalised it as partial set membership.Objectively it quantifies the electron density distribution between atoms, and in particular the appearance and use of molecular orbitals in the covalent case. In ions an electron is fully donated, in covalency two electrons form a bonding pair and set up and occupy a molecular orbital between the atoms. The single polar bond can also be viewed this way, as a mixrure, and the polar charge will start to nfluence its physical properties as well as how it reacts. At the fully ionic end, ions have lattkce energy in condensed phases where there is a significant long range contribution from other ions. Which then means crystal structure is important. In this respect an ionic solid is an extreme case of charge separation. Less extensive charge separations gjve rise to dielectric materials, and layered materials or clays may present more opportunities for ions to coexist with covalent structures.The archetypal ionic solid would be common salt, and ionic solution chemistry in water is often the starting point of inorganic chemistry courses. The archetypal covalent material depends on its own sructure, but we could choose an alkane as an archetype for organic chemistry say. So we get the typical low melting point non-polar iquids or gases of organic chemistry,
How can I differentiate between Ionic compounds, molecular compounds, and acids given only the formula?
This is a difficult question. First of all, acids invariably contain hydrogen atoms, and the hydrogen atom will be bound to an electronegative atom. For example: HF, HCl, HBr, HI. 99% of the time it will either be bound to a halogen or to an oxygen atom. Hydrogen bound to other atoms usually shows negligible acidity. As for differentiating between ionic and molecular compounds, this turns out to be difficult. In general, there is no sharp dividing line: for example, aluminium chloride is on the borderline between covalent and ionic. Generally, the compound's ionic character will be increased if the cation is large, the anion small, and the charges on the cation and anion are small. The charge on a cation does not exceed +3 in ionic compounds, with the possible exception that some metals of high atomic number may form +4 ions. For example, OsO4 is obviously covalent, since Os8+ cannot exist. UF4 may be ionic since uranium is such a heavy metal (I don't mean density-wise), or it may be borderline. Alkali metals form almost exclusively ionic compounds, except for organometallics. Beryllium forms no compounds which are unequivocally ionic - BeF2 and BeO, which we would expect to be the most ionic of beryllium compounds, are on the borderline. Magnesium forms mostly ionic compounds, with the major exceptions of the hydride and organometallics. The heavier alkaline earths form mostly ionic compounds, again with the possible exception of the organometallics. Transition metal compounds are usually considered ionic if the oxidation state of the metal is +3 or less, covalent otherwise. Nonmetals cannot form positive ions, with the exception of polyatomic ions - compounds of NH4+ are usually ionic; other polyatomic cations are rare. The atoms C, N, O, F, P, S, Cl, Se, Br, Te, and I are known to form anions with electropositive metals. The metalloids form mostly covalent compounds - the fluorides and oxides are usually borderline (with the exception of boron, which forms almost no ionic compounds - Na3B may be ionic.) The post-transition metals often form borderline compounds as well, although the fluorides and oxides in low oxidation states are usually considered ionic.