A certain ionic compound is made entirely of aluminum and oxygen.What is the formula for this compound?
Q. A certain ionic compound is made entirely of aluminum and oxygen What is the formula for this compound? THANKS! ALSO What is the mass percentage of each element in this compound? (% of Al and % of O)
Asked by kayyy - Wed Oct 28 01:06:27 2009 - - 2 Answers - 0 Comments
A. Aluminium Oxide: Al2O3 The ions: Al3+ ... O2- When they bond: It is ionic as it takes place by the transfer of electrons from Aluminium(metal) to Oxygen(Non-metal). Hence, the bond is: Al2O3, Aluminium Oxide or alumina.
Answered by Cool lovable Math Genius LOL - Wed Oct 28 01:17:35 2009
Q. A certain ionic compound is made entirely of aluminum and oxygen What is the formula for this compound? THANKS! ALSO What is the mass percentage of each element in this compound? (% of Al and % of O)
Asked by kayyy - Wed Oct 28 01:06:27 2009 - - 2 Answers - 0 Comments
A. Aluminium Oxide: Al2O3 The ions: Al3+ ... O2- When they bond: It is ionic as it takes place by the transfer of electrons from Aluminium(metal) to Oxygen(Non-metal). Hence, the bond is: Al2O3, Aluminium Oxide or alumina.
Answered by Cool lovable Math Genius LOL - Wed Oct 28 01:17:35 2009
What is the difference between a covalent compound and an Ionic compound?
Q. What is the difference between a covalent compound and an Ionic compound? Give specific examples to support your response.
Asked by PeejayButta - Fri Jul 11 20:20:01 2008 - - 3 Answers - 0 Comments
A. Covalent bonds = shared elctrons Ionic bonds = transfer of electrons First, you must know that a driving force for bonding is for an atom to fill its outermost shell with 8 valence electrons (except hydrogen, which only wants 2). Covalent bond = O2 (2 oxygens bonded together) Oxygen has 6 valence electrons, so that means 2 oxygen atoms will have a total of 12 valence electrons. However, most atoms (except hydrogen) need 8 valence electrons to fill their outermost orbital. So in order for 2 bonded oxygen atoms to have a full orbital of 8 electrons each, then they must need a total of 16 valence electrons right? (8 + 8 = 16). No. Not with covalent bonding. In covalent bonding, valence electrons are shared. So if each oxygen atom has… [cont.]
Answered by Vocal Guru - Fri Jul 11 20:46:34 2008
Q. What is the difference between a covalent compound and an Ionic compound? Give specific examples to support your response.
Asked by PeejayButta - Fri Jul 11 20:20:01 2008 - - 3 Answers - 0 Comments
A. Covalent bonds = shared elctrons Ionic bonds = transfer of electrons First, you must know that a driving force for bonding is for an atom to fill its outermost shell with 8 valence electrons (except hydrogen, which only wants 2). Covalent bond = O2 (2 oxygens bonded together) Oxygen has 6 valence electrons, so that means 2 oxygen atoms will have a total of 12 valence electrons. However, most atoms (except hydrogen) need 8 valence electrons to fill their outermost orbital. So in order for 2 bonded oxygen atoms to have a full orbital of 8 electrons each, then they must need a total of 16 valence electrons right? (8 + 8 = 16). No. Not with covalent bonding. In covalent bonding, valence electrons are shared. So if each oxygen atom has… [cont.]
Answered by Vocal Guru - Fri Jul 11 20:46:34 2008
How do you determine the chemical formula of an ionic compound?
Q. Im studying chemistry right now and i am having trouble determining what the chemical formulas are to ionic and covalent compounds. Here is a sample question: Calcium (Ca) combines with chlorine (Cl) to form calcium chloride, an ionic compound. Calcium has two electrons in its outer energy level and chlorine has seven electrons in its outer energy level. Determine the formula for calcium chloride and EXPLAIN your answer. I researched calcium chloride and found the formula is CaCl2, but on a test i wont be able to research the answer. Are there easy ways to determining chemical formulas? Thank you for helping, Ryan C.
Asked by Ryan C - Sun Sep 17 16:06:28 2006 - - 1 Answers - 1 Comments
A. In ionic compounds, you have the metals (on the left side of the periodic table) who tend to pass off electrons, and you have the non-metals (on the right side) who have "gaps" in their electron shells and tend to accept electrons. In the case of CaCl2: Chlorine has 7 electrons in its outer shell. A full shell for would require 8 electrons, so it is "looking" for 1 extra electron to fill its outer shell. Calcium has 2 electrons in its outer shell. It would like to give those extra two away, so it's looking for 2 takers. Soo... Chlorine (with the one gap) calls up another Chlorine (also with the one gap), and now you have a total of two gaps. Two extra electrons from Calcium and two gaps from the two Chlorine make a good fit, and… [cont.]
Answered by borscht - Sun Sep 17 23:02:08 2006
Q. Im studying chemistry right now and i am having trouble determining what the chemical formulas are to ionic and covalent compounds. Here is a sample question: Calcium (Ca) combines with chlorine (Cl) to form calcium chloride, an ionic compound. Calcium has two electrons in its outer energy level and chlorine has seven electrons in its outer energy level. Determine the formula for calcium chloride and EXPLAIN your answer. I researched calcium chloride and found the formula is CaCl2, but on a test i wont be able to research the answer. Are there easy ways to determining chemical formulas? Thank you for helping, Ryan C.
Asked by Ryan C - Sun Sep 17 16:06:28 2006 - - 1 Answers - 1 Comments
A. In ionic compounds, you have the metals (on the left side of the periodic table) who tend to pass off electrons, and you have the non-metals (on the right side) who have "gaps" in their electron shells and tend to accept electrons. In the case of CaCl2: Chlorine has 7 electrons in its outer shell. A full shell for would require 8 electrons, so it is "looking" for 1 extra electron to fill its outer shell. Calcium has 2 electrons in its outer shell. It would like to give those extra two away, so it's looking for 2 takers. Soo... Chlorine (with the one gap) calls up another Chlorine (also with the one gap), and now you have a total of two gaps. Two extra electrons from Calcium and two gaps from the two Chlorine make a good fit, and… [cont.]
Answered by borscht - Sun Sep 17 23:02:08 2006
How to calculate percentage of calcium in an ionic compound dissolved in water?
Q. What is the percentage of calcium in an ionic compound of unknown composition if a 2.141g sample of the compound is completely dissolved in water and produces 1.222g of CaCO3 upon addition of an excess Na2CO3 solution? --- All I can deduce from here is that CaCO3 is the limiting reagent. Other than that, I don't know how to proceed. Help? Thanks!
Asked by Pancha Pistolas - Mon Oct 8 01:14:13 2007 - - 1 Answers - 0 Comments
A. Formula weight of CaCO3=40+12+48=100. So Ca is 40/100 by weight of CaCO3. In your sample you had 1.222g of CaCO3 which would have .4*1.222g of Ca in it or .4888g of Ca. That is all you ended with so that is what you started with in a compound that weighed 2.141g .4888/2.141*100=22.83% Ca in the original sample
Answered by chasrmck - Mon Oct 8 04:34:35 2007
Q. What is the percentage of calcium in an ionic compound of unknown composition if a 2.141g sample of the compound is completely dissolved in water and produces 1.222g of CaCO3 upon addition of an excess Na2CO3 solution? --- All I can deduce from here is that CaCO3 is the limiting reagent. Other than that, I don't know how to proceed. Help? Thanks!
Asked by Pancha Pistolas - Mon Oct 8 01:14:13 2007 - - 1 Answers - 0 Comments
A. Formula weight of CaCO3=40+12+48=100. So Ca is 40/100 by weight of CaCO3. In your sample you had 1.222g of CaCO3 which would have .4*1.222g of Ca in it or .4888g of Ca. That is all you ended with so that is what you started with in a compound that weighed 2.141g .4888/2.141*100=22.83% Ca in the original sample
Answered by chasrmck - Mon Oct 8 04:34:35 2007
How can an ionic compound always be a strong electrolyte & not necessarily always completely soluble in water?
Q. How can an ionic compound always be a strong electrolyte (100% dissociation into ions) but not necessarily always completely soluble in water?
Asked by srvevh1 - Sun Feb 8 16:21:26 2009 - - 1 Answers - 0 Comments
A. Solubility and dissociation are two different things. There are lots of compounds which have relatively high solubilities which don't dissociate at all. Take sugar (sucrose) for example. On the other hand we have compounds which dissolve very little in water, but what does dissolve dissociates completely. That would be compounds like the alkaline earth strong bases, like Ca(OH)2, Sr(OH)2 and Ba(OH)2.
Answered by pisgahchemist - Sun Feb 8 16:27:35 2009
Q. How can an ionic compound always be a strong electrolyte (100% dissociation into ions) but not necessarily always completely soluble in water?
Asked by srvevh1 - Sun Feb 8 16:21:26 2009 - - 1 Answers - 0 Comments
A. Solubility and dissociation are two different things. There are lots of compounds which have relatively high solubilities which don't dissociate at all. Take sugar (sucrose) for example. On the other hand we have compounds which dissolve very little in water, but what does dissolve dissociates completely. That would be compounds like the alkaline earth strong bases, like Ca(OH)2, Sr(OH)2 and Ba(OH)2.
Answered by pisgahchemist - Sun Feb 8 16:27:35 2009
How do you work out the formula of an ionic compound?
Q. How do you work out the formula of an ionic compound?
Asked by Faith J - Wed Sep 24 13:53:07 2008 - - 2 Answers - 0 Comments
A. an ionic compound is made when a metal reacts with a non-metal, to balance out the equation you must see what charges they are, eg copper, Cu and bromine Br react Cu has to loose 2 electrons making the it a position ion Cu2+ Br can only gain one electron for a full outer shell Br1+ we need to balance this out, the end formula will be CuBr2 since the charges are all cancelled out, use your periodic table to help you with finding out the charges
Answered by [-Sathit-] - Wed Sep 24 14:03:13 2008
Q. How do you work out the formula of an ionic compound?
Asked by Faith J - Wed Sep 24 13:53:07 2008 - - 2 Answers - 0 Comments
A. an ionic compound is made when a metal reacts with a non-metal, to balance out the equation you must see what charges they are, eg copper, Cu and bromine Br react Cu has to loose 2 electrons making the it a position ion Cu2+ Br can only gain one electron for a full outer shell Br1+ we need to balance this out, the end formula will be CuBr2 since the charges are all cancelled out, use your periodic table to help you with finding out the charges
Answered by [-Sathit-] - Wed Sep 24 14:03:13 2008
How do water molecules affect a soluble ionic compound when it is mixed into water?
Q. A) They change ionic bonds to covalent B) They change covalent bonds to ionic C) they remove electrons from the compound d) add protons to ionic nuclei
Asked by SYED A J - Fri May 1 01:30:36 2009 - - 2 Answers - 0 Comments
A. It would depend on the compound. A would be possible if the ions actually reacted with the water to form new compounds. C is possible because electrons can move from one molecule to another. D is also possible if the water was dissociated into H+ and OH- and the H+ reacted with the starting compound. There is another possibility too. For something as simple as table salt, when it dissolves, the ionic Na+Cl- bond is broken and the ions are surrounded by clouds of water molecules. The Na+ is surrounded by water molecules with the oxygen closer to the Na+ than the hydrogen. The Cl- ion is surrounded by water molecules with their hydrogens closer to the Cl- than the oxygen. Because oxygen is more negative than hydrogen in a water molecule. [cont.]
Answered by unknown - Fri May 1 02:56:53 2009
Q. A) They change ionic bonds to covalent B) They change covalent bonds to ionic C) they remove electrons from the compound d) add protons to ionic nuclei
Asked by SYED A J - Fri May 1 01:30:36 2009 - - 2 Answers - 0 Comments
A. It would depend on the compound. A would be possible if the ions actually reacted with the water to form new compounds. C is possible because electrons can move from one molecule to another. D is also possible if the water was dissociated into H+ and OH- and the H+ reacted with the starting compound. There is another possibility too. For something as simple as table salt, when it dissolves, the ionic Na+Cl- bond is broken and the ions are surrounded by clouds of water molecules. The Na+ is surrounded by water molecules with the oxygen closer to the Na+ than the hydrogen. The Cl- ion is surrounded by water molecules with their hydrogens closer to the Cl- than the oxygen. Because oxygen is more negative than hydrogen in a water molecule. [cont.]
Answered by unknown - Fri May 1 02:56:53 2009
Compare the electrical conductivity of a metal with that of an ionic compound. How is it the same? How is it d?
Q. Compare the electrical conductivity of a metal with that of an ionic compound. How is it the same? How is it different?
Asked by Tinky W - Wed Oct 8 23:31:34 2008 - - 1 Answers - 0 Comments
A. Ionic compounds are compounds that do not share electrons. what is a metal, is it ionic covalent polar covalent... These are just hints.
Answered by HSSTUDY - Wed Oct 8 23:43:26 2008
Q. Compare the electrical conductivity of a metal with that of an ionic compound. How is it the same? How is it different?
Asked by Tinky W - Wed Oct 8 23:31:34 2008 - - 1 Answers - 0 Comments
A. Ionic compounds are compounds that do not share electrons. what is a metal, is it ionic covalent polar covalent... These are just hints.
Answered by HSSTUDY - Wed Oct 8 23:43:26 2008
Predict the chemical formula for the ionic compound formed by?
Q. Predict the chemical formula for the ionic compound formed by Hg 2 2+ and CO 3 2- (the first 2 is a subscript and the 2+ is a superscript) (the 3 is a subscript and the 2- is a superscript) OMG! does anyone ever explain? where the hell did the 2 in the Hg2 go?
Asked by jaddai29rb - Wed Jul 22 23:54:28 2009 - - 2 Answers - 0 Comments
A. HgCO3 - mercuric carbonate or mercury(II)carbonate
Answered by Doc89891 - Thu Jul 23 00:00:07 2009
Q. Predict the chemical formula for the ionic compound formed by Hg 2 2+ and CO 3 2- (the first 2 is a subscript and the 2+ is a superscript) (the 3 is a subscript and the 2- is a superscript) OMG! does anyone ever explain? where the hell did the 2 in the Hg2 go?
Asked by jaddai29rb - Wed Jul 22 23:54:28 2009 - - 2 Answers - 0 Comments
A. HgCO3 - mercuric carbonate or mercury(II)carbonate
Answered by Doc89891 - Thu Jul 23 00:00:07 2009
Which is the correct formula for the ionic compound?
Q. Which is the correct formula for the ionic compound formed by the transfer of electrons from Potassium to Oxygen? Would it be: A. KO B. K2O C.KO2 K2O2 Thanks for your help!
Asked by Amber - Sat Aug 30 20:21:12 2008 - - 4 Answers - 0 Comments
A. B. K2O Potassium(K) has a +1 charge, oxygen(O) has a -2 charge so you need 2 potassiums to get a total of +2 charge to cancel out the -2 charge of Oxygen.
Answered by Johnny D - Sat Aug 30 20:25:17 2008
Q. Which is the correct formula for the ionic compound formed by the transfer of electrons from Potassium to Oxygen? Would it be: A. KO B. K2O C.KO2 K2O2 Thanks for your help!
Asked by Amber - Sat Aug 30 20:21:12 2008 - - 4 Answers - 0 Comments
A. B. K2O Potassium(K) has a +1 charge, oxygen(O) has a -2 charge so you need 2 potassiums to get a total of +2 charge to cancel out the -2 charge of Oxygen.
Answered by Johnny D - Sat Aug 30 20:25:17 2008
What is the formula for ionic compound composed of the potassium,K+, and the oxide of ion O2-?
Q. What is the formula for ionic compound composed of the potassium,K+, and the oxide of ion O2-?
Asked by Candi - Mon Jul 27 11:56:51 2009 - - 2 Answers - 0 Comments
A. K2O Potassium Oxide
Answered by The Wonderful Man - Mon Jul 27 12:10:28 2009
Q. What is the formula for ionic compound composed of the potassium,K+, and the oxide of ion O2-?
Asked by Candi - Mon Jul 27 11:56:51 2009 - - 2 Answers - 0 Comments
A. K2O Potassium Oxide
Answered by The Wonderful Man - Mon Jul 27 12:10:28 2009
Why is it difficult to produce metal by the electrolysis of the aq solution of its ionic compound?
Q. Why is it sometimes difficult to produce a metal by the electrolysis of the aqueous solution of its ionic compound? a) The melting point is so low that liquid forms b) The boiling point is so low it vapourizes c) The metal quickly forms an oxide layer d) Water is a stronger oxidizing agent 1 hour ago - 3 days left to answer.
Asked by William S - Thu Jul 10 00:55:51 2008 - - 1 Answers - 0 Comments
A. d - if the metal is a very strong reducing agent (such as Na),, it would be immediately after being made react with the water (for example you are not able to make Na K but also Al by simple electrolysis - they have too negative potentials). Theoretically, all metals with potential below zero would have those problems, but no - due to the overpotential of water (H2 creates around -.7V instead of 0V)
Answered by Chloralhydrate - Thu Jul 10 04:49:43 2008
Q. Why is it sometimes difficult to produce a metal by the electrolysis of the aqueous solution of its ionic compound? a) The melting point is so low that liquid forms b) The boiling point is so low it vapourizes c) The metal quickly forms an oxide layer d) Water is a stronger oxidizing agent 1 hour ago - 3 days left to answer.
Asked by William S - Thu Jul 10 00:55:51 2008 - - 1 Answers - 0 Comments
A. d - if the metal is a very strong reducing agent (such as Na),, it would be immediately after being made react with the water (for example you are not able to make Na K but also Al by simple electrolysis - they have too negative potentials). Theoretically, all metals with potential below zero would have those problems, but no - due to the overpotential of water (H2 creates around -.7V instead of 0V)
Answered by Chloralhydrate - Thu Jul 10 04:49:43 2008
Crystals of the ionic compound calcium fluoride have a different structure from that of the ionic compound cal?
Q. Crystals of the ionic compound calcium fluoride have a different structure from that of the ionic compound calcium chloride. Suggest a reason for this difference.
Asked by beast6k - Wed Nov 4 23:01:07 2009 - - 1 Answers - 0 Comments
A. The size of a chloride ion is much larger than the size of a fluoride ion. CaF2 arranges in the fluorite crystal structure ( where the blue balls are the fluoride ions. The holes where these fluoride ions fit in between the closely packed calcium cations are a certain size, which aren't big enough for chloride ions to fit into. Therefore, CaCl2 has to form a different crystal structure that allows for the larger anion size (
Answered by L - Wed Nov 4 23:06:27 2009
Q. Crystals of the ionic compound calcium fluoride have a different structure from that of the ionic compound calcium chloride. Suggest a reason for this difference.
Asked by beast6k - Wed Nov 4 23:01:07 2009 - - 1 Answers - 0 Comments
A. The size of a chloride ion is much larger than the size of a fluoride ion. CaF2 arranges in the fluorite crystal structure ( where the blue balls are the fluoride ions. The holes where these fluoride ions fit in between the closely packed calcium cations are a certain size, which aren't big enough for chloride ions to fit into. Therefore, CaCl2 has to form a different crystal structure that allows for the larger anion size (
Answered by L - Wed Nov 4 23:06:27 2009
Which of the following best describes the formula unit of the ionic compound resulting from interations?
Q. Which of the following best describes the formula unit of the ionic compound resulting from interactions of ferrous (Fe (II)) ions and bromide ions? Fe3Br FeBr2 Fe2Br FeBr3 FeBr
Asked by Mizeny M - Sat Apr 12 02:13:43 2008 - - 2 Answers - 0 Comments
A. iron II bromide is FeBr2 bye
Answered by Dr R - Sat Apr 12 07:05:23 2008
Q. Which of the following best describes the formula unit of the ionic compound resulting from interactions of ferrous (Fe (II)) ions and bromide ions? Fe3Br FeBr2 Fe2Br FeBr3 FeBr
Asked by Mizeny M - Sat Apr 12 02:13:43 2008 - - 2 Answers - 0 Comments
A. iron II bromide is FeBr2 bye
Answered by Dr R - Sat Apr 12 07:05:23 2008
Which ionic compound is expected to form from the combination of the following pairs of elements? (Type your a
Q. Which ionic compound is expected to form from the combination of the following pairs of elements? (Type your answer using the format H2O for H2O.) (a) chlorine and magnesium (b) barium and oxygen (c) rubidium and oxygen (d) magnesium and nitrogen
Asked by hotatlboy0519 - Mon Nov 26 15:43:10 2007 - - 1 Answers - 0 Comments
A. (a) MgCl2 (b) BaO (c) Rb2O (d) Mg3N2
Answered by Luke C - Mon Nov 26 15:52:54 2007
Q. Which ionic compound is expected to form from the combination of the following pairs of elements? (Type your answer using the format H2O for H2O.) (a) chlorine and magnesium (b) barium and oxygen (c) rubidium and oxygen (d) magnesium and nitrogen
Asked by hotatlboy0519 - Mon Nov 26 15:43:10 2007 - - 1 Answers - 0 Comments
A. (a) MgCl2 (b) BaO (c) Rb2O (d) Mg3N2
Answered by Luke C - Mon Nov 26 15:52:54 2007
How do you decided in an ionic compound its boiling point?
Q. Is it the molecular forces, electronegativity. Because for hw i have a whole list of ionic compounds however im not sure how to figure out the rules for ionic compounds boiling point.
Asked by velvrevolver1 - Sun Nov 16 19:43:40 2008 - - 1 Answers - 0 Comments
A. There are no `hard rules`. Generally ionic compounds with smaller ions with larger charges have higher boiling temps. due to strong electrostatic attractions.
Answered by aaj - Sun Nov 16 22:25:03 2008
Q. Is it the molecular forces, electronegativity. Because for hw i have a whole list of ionic compounds however im not sure how to figure out the rules for ionic compounds boiling point.
Asked by velvrevolver1 - Sun Nov 16 19:43:40 2008 - - 1 Answers - 0 Comments
A. There are no `hard rules`. Generally ionic compounds with smaller ions with larger charges have higher boiling temps. due to strong electrostatic attractions.
Answered by aaj - Sun Nov 16 22:25:03 2008
How can you identify an ionic compound?
Q. What are some ionic compound examples?
Asked by fuzzysparkle182 - Wed Apr 2 19:55:00 2008 - - 1 Answers - 0 Comments
A. Generally, an ionic compund will be between a metal and a non-metal, with only a very few exceptions. Example: NaCl, KF, Mg(OH)2
Answered by brian_the_coelcanth - Wed Apr 2 20:02:13 2008
Q. What are some ionic compound examples?
Asked by fuzzysparkle182 - Wed Apr 2 19:55:00 2008 - - 1 Answers - 0 Comments
A. Generally, an ionic compund will be between a metal and a non-metal, with only a very few exceptions. Example: NaCl, KF, Mg(OH)2
Answered by brian_the_coelcanth - Wed Apr 2 20:02:13 2008
Why ionic compound could only be a pair?
Q. In these day, I did a experiment, to add some ionic compound(aq) into different ions. I am wondering that why ions can be only a pair of elements, but not 3 or more elements to form 1 compound.
Asked by Jack__EX - Mon Jan 28 10:00:52 2008 - - 3 Answers - 0 Comments
A. An ionic compound, by definition, contains two components, a cation and an anion. However, each of these can be a single atom (Na+, Cl-), a group of atoms (NH4+, SO4 2-), or even a very large organic or bio-organic grouping. It is also possible for a solid to contain more than two types of ion. As an example, consider the alums, salts of formula M(I)M(III)(SO4)2.12H2O such as KAl(SO4)2.12H2O, which are fairly easily persuaded to grow from aqueous solution as beautiful large optical crystals. A very complex example is provided by naturally occurring clays, which have polymeric anions and, usually, a mixture of different kinds of cation.
Answered by Paul B - Mon Jan 28 10:58:01 2008
Q. In these day, I did a experiment, to add some ionic compound(aq) into different ions. I am wondering that why ions can be only a pair of elements, but not 3 or more elements to form 1 compound.
Asked by Jack__EX - Mon Jan 28 10:00:52 2008 - - 3 Answers - 0 Comments
A. An ionic compound, by definition, contains two components, a cation and an anion. However, each of these can be a single atom (Na+, Cl-), a group of atoms (NH4+, SO4 2-), or even a very large organic or bio-organic grouping. It is also possible for a solid to contain more than two types of ion. As an example, consider the alums, salts of formula M(I)M(III)(SO4)2.12H2O such as KAl(SO4)2.12H2O, which are fairly easily persuaded to grow from aqueous solution as beautiful large optical crystals. A very complex example is provided by naturally occurring clays, which have polymeric anions and, usually, a mixture of different kinds of cation.
Answered by Paul B - Mon Jan 28 10:58:01 2008
how to know if the substances is an ionic compound?
Q. I do many question.I know Lead(II) bromide is an ionic compound.But how to determine?Please tell me.Thank you very much.Give me more example.
Asked by Wong - Thu Sep 24 23:32:29 2009 - - 2 Answers - 0 Comments
A. Well, to tell whether the compound is ionic or covalent just by looking at the formula, you need to know if the elements that make up the compoundd are metals or non-metals. As a general guide, metals and non-metals form ionic compounds while non-metals and non-metals form covalent compounds. HCl is actually a covalent compound with ionic character and thus acts somewhat much like an ionic compound sometimes. This kind of compounds form due to the difference in electronegativity. As chlorine has more protons compared to hydrogen, the pull of chlorine to its protons would be stronger compared to that of hydrogen. Thus, electrons would mostly be pulled to the chlorine atom. This results in chlorine being partially negative (due to the… [cont.]
Answered by ashish sinha - Sun Sep 27 09:39:37 2009
Q. I do many question.I know Lead(II) bromide is an ionic compound.But how to determine?Please tell me.Thank you very much.Give me more example.
Asked by Wong - Thu Sep 24 23:32:29 2009 - - 2 Answers - 0 Comments
A. Well, to tell whether the compound is ionic or covalent just by looking at the formula, you need to know if the elements that make up the compoundd are metals or non-metals. As a general guide, metals and non-metals form ionic compounds while non-metals and non-metals form covalent compounds. HCl is actually a covalent compound with ionic character and thus acts somewhat much like an ionic compound sometimes. This kind of compounds form due to the difference in electronegativity. As chlorine has more protons compared to hydrogen, the pull of chlorine to its protons would be stronger compared to that of hydrogen. Thus, electrons would mostly be pulled to the chlorine atom. This results in chlorine being partially negative (due to the… [cont.]
Answered by ashish sinha - Sun Sep 27 09:39:37 2009
What test can be performed to confirm an experimental product is an ionic compound?
Q. We did a lab in chemistry with Mg, O, and heat that crated a product that was supposedly ionized. One of the analysis questions was the following: "What test could be performed to confirm that the product(s) are ionic compounds?" Help? Please&Thanks. :)
Asked by amanda (: - Sun Aug 23 16:59:54 2009 - - 2 Answers - 0 Comments
A. Ionic compounds ionize in aqueous solution but some molecular compounds ionize in aqueous solution as well, such as HCl. Also not all ionic compounds are soluble in water. We can heat up the product to its melting point and if it has a very high melting point then that could tell you that it is an ionic compound. We can therefore conduct an electric current through its molten state, and if it conducts electricity then it is an ionic compound. Basically, the big hit on the head will be if the compound conducts electricity in its molten state.
Answered by Mauri - Sun Aug 23 17:08:12 2009
Q. We did a lab in chemistry with Mg, O, and heat that crated a product that was supposedly ionized. One of the analysis questions was the following: "What test could be performed to confirm that the product(s) are ionic compounds?" Help? Please&Thanks. :)
Asked by amanda (: - Sun Aug 23 16:59:54 2009 - - 2 Answers - 0 Comments
A. Ionic compounds ionize in aqueous solution but some molecular compounds ionize in aqueous solution as well, such as HCl. Also not all ionic compounds are soluble in water. We can heat up the product to its melting point and if it has a very high melting point then that could tell you that it is an ionic compound. We can therefore conduct an electric current through its molten state, and if it conducts electricity then it is an ionic compound. Basically, the big hit on the head will be if the compound conducts electricity in its molten state.
Answered by Mauri - Sun Aug 23 17:08:12 2009
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