You know that both the Sulphur and Oxygen has six valence electrons each. 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The bonding of81 2~SO2 has been suggested to primarily involve st-donation from the metal to the LUMO of SO2, which is antibonding with respect to the S bond and bonding with respect to the O interaction.4~ This type of interaction would be expected to lengthen S distances, increase the terminal oxygen basicity, and enhance coordination by Lewis acids. Let us break it down further. The Sulfur Dioxide which is also known as Sulphur Dioxide is the entity of a bond between Sulfur and Oxygen atoms. The MO scheme for one of the B–H–B bridging three center two electron bonds. So, our first perception of the original structure does not match with the original one. The question gives you a clue where they go. Single bond, Double bond and Triple bond. If this were the case, the bond angle would be 90°, as shown in Figure 1, because p orbitals are perpendicular to each other. During the formation of SO2, this central atom is bonded with two oxygen atoms and their structure can be represented as O=S=O. of valence electrons – No. The four covalent bonding positions of the carbon atom can give rise to a wide diversity of compounds with many functions, accounting for the importance of carbon in living things. The Sulfur Dioxide which is also known as Sulphur Dioxide is the entity of a bond between Sulfur and Oxygen atoms. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 6.1 and 6.2. a. CH2Br2 b. SO2 … Write a hybridization and bonding scheme for each molecule. show where the sigma and pi bonds are located. Can you give more explanation about electronegativity and its effects? [15] Recently, the organic chemistry of sulfur dioxide has seen a revival, arguably thanks to the application of easy-to-handle Scheme 1. The 3d and 3p orbitals remain the same, and they form pi bonds. Problem: Write a hybridization and bonding scheme for each molecule. The C-O bonds in carbon dioxide are polar and yet the dipole moment is zero because the 2 bond dipoles cancel each other. We will show the bonding of SO2 without making assumption below. Though there are so many similarities between the electron geometry and molecular geometry, there are some key differences. This way of bonding is known as covalent bonding and this is shown mainly by non-metals and H +. When the two O-atoms are brought up to opposite sides of the carbon atom in carbon dioxide, one of the p orbitals on each oxygen forms a pi bond with one of the carbon p-orbitals. JS Joshua S. Numerade Educator 04:37. sp2. To determine this, we will first look at the sulphur atom which will be the central atom. The most stable forms of the nonmetals in groups 4A, 5A, and 6A of the first period are molecules with multiple bonds… Analyze the structure: C → Group 4A → 4 Valence electrons. We will place Sulphur at the center and Oxygens at outsides. ativistic effects reduce the atomization of SO and SO2 by 0.34 and 0.81 kcal/mol, respectively, and clearly must be accounted for if a ... of basis sets varies with the nature of the S bonding. "The S-O bond length of 149 pm is shorter than expected for a S-O single bond. AS Chemistry Exam Questions from OCR exam board: Electrons, bonding and structure Important Note: For students of CIE AS level, the syllabi are slightly different. Experimental evidence shows that the bond angle is 104.5°, not 90°. It is known as a formula written as SO2. Write a hybridization and bonding scheme for acetaldehyde, SOLUTION. Problem 35 Write a hybridization and bonding scheme for each molecule or ion. ... which of the following hybridization schemes allows the formation of at least one π bond? However, the electrons that form the sigma bonds and the lone pair are at different energy levels. In the outer level, Sulphur has six electrons, and the Oxygen has four of them among which one electron is used for each bond. CH4(g)+ClF(g)→CH3Cl(g)+HF(g) The molecular geometry of SO2 has a bent shape which means the top has less electronegativity, and the bottom placed atoms of Oxygen have more of it. as double bonds on the basis of their length and strength,4 the bonding scheme that gives rise to this pattern is unclear, as the d-orbitals of the sulfur atom are too high in energy to meaningfully participate in bonding in SO 2. The tetrahedral molecular geometry of the sulfate ion is as predicted by VSEPR theory. Show Where The Sigma And Pi Bonds Are Located. 1 with polar covalent bonds only; 2 with an ionic bond. Multiple bonds can also occur between dissimilar atoms. So, our final Lewis structure of SO2 will be like: By analyzing the Lewis structure of SO2, we can see that the SO2 is asymmetrical because it contains a region with different sharing. Set your categories menu in Theme Settings -> Header -> Menu -> Mobile menu (categories). SO2 molecular geometry is considered to V-shaped or bent. FREE Expert Solution. Required fields are marked *, Though there are so many similarities between the. You can share your thoughts for any information missed here or if you want to know more about anything. Alternatively, the electron geometry of sulphur dioxide is in the shape of a trigonal planar. We will put these electrons on the atom of Sulphur. Magnesium hydroxide, Mg(OH) 2, is a white powder produced in large quantities from seawater by the addition of milk of lime (calcium hydroxide).It is the primary raw material in the production of magnesium metal and has been used as a fire-retardant additive. Here, we will explain the hybridization of SO2 in detail. All Chemistry Practice Problems Orbital Overlap Practice Problems. In total, there is a formation of three sp2 hybrid orbitals. These unpaired electrons then form sigma bonds with the oxygen atoms. As the single alone pair not counted in the shape’s description, we can conclude that the molecular shape of SO2 is V-Shaped or Bent. Two-hybrid orbitals contain unpaired electrons and one hybrid orbital will have the lone pair. To design the best Lewis structure, you also need to calculate the formal charge of every atom too. The stable state is obtained when hybridization takes place. Now we will put the pair of electrons between the atoms to create bonds. First, draw single bonds between … To make bonds, four pairs are needed, so one pair remains alone. a. CH2Br2 b. SO2 c. NF3 d. BF3” is broken down into a … Here, we have explained the molecular geometry, electron geometry, Lewis structure, bond angle, and polarity of SO2 (Sulfur Dioxide). Students will also learn how to determine the type of hybridization, and they will find information about SO2 molecular geometry and bond angles. of Bonds – 2 X (No. The answer to “Write a hybridization and bonding scheme for each molecule. And moreover, there is no mention of existence of dative bond here. materials (Scheme 2). One of the ways of forming bonds is sharing of electron to attain their nearest noble gas configuration. Figure 2. Herein, we present the first transformation of borylphosphine into borylphosphinite using nitrous oxide. The electron geometry of SO2 is formed in the shape of a trigonal planner. 4 To address this dilemma, various studies comparing the electronic structure of O 3 … And if not writing you will find me reading a book in some cozy cafe ! The molecular shape of SO2 is same as the molecular geometry of Carbon Dioxide (CO2). In this case, sp hybridization leads to two double bonds. Borylphosphine reacts with N2O via insertion of a single oxygen atom into the P–B bond and formation of a P–O–B bond system. The three pairs of bonding electrons lie at an angle of 119o. You will get a reply from the expert. The simplistic route is to add up collective bonds from a data table provided in your textbook, e.g. As for the bonding, there is one sigma and one pi bond formed between sulphur and the two oxygen atoms. Sulphur can have an expanded octect because the orbitals d. In that case sulphur shows an expanded octet. Sketch the structure, including overlapping orbitals, and label all bonds using the notation shown in Examples 6.1 and 6.2. a. COCl2 (carbon is the central atom) b. BrF5 c. XeF2 d. I3. To create the Lewis structure of SO2, you need to arrange the eight valence electrons on the Sulphur. Also if you give a comparison between SO2 and CO2, then it will help a lot. One of the most notable differences is that the electron geometry can be associated with one or more molecular shapes. sp3,sp2,sp3d2. Hey folks, this is me, Priyanka, writer at Geometry of Molecules where I want to make Chemistry easy to learn and quick to under. Use bond energies to determine ΔHrxn for the following reaction. Well that rhymed. The formula "NCCH"_3 tells you that the three "H" atoms are attached to the terminal carbon atom. Valence bond theory would predict that the two O–H bonds form from the overlap of these two 2p orbitals with the 1s orbitals of the hydrogen atoms. View all posts by Priyanka →. Label all bonds in NF 3. For example, the bond lengths in sulfuric acid are 157 pm for S-OH. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7. a. CH2Br2 b. SO2 c. NF3 d. BF3 How it is possible for sulphur with 10 electrons. Write a hybridization and bonding scheme for each molecule. Is CO (Carbon Monoxide) polar or nonpolar? The three pairs of bonding electrons arranged in the plane at the angle of 120-degree. Acetaldehyde has 18 valence electrons and the following Lewis structure: The leftmost carbon atom has four electron groups and a tetrahedral electron geometry. We are asked to write a hybridization and bonding scheme for CH 2 Br 2. Start typing to see posts you are looking for. Q. This question hasn't been answered yet Ask an expert. Write A Hybridization And Bonding Scheme For Each Molecule Sketch The Molecule Including Overlapping Its also sp2 for. (b) Attach the hydrogen atoms. Let … In sulphur dioxide, the hybridization that takes place is sp2 type. It depends on the central atom’s structure of electrons of the molecule, while the molecular geometry depends on the other atoms too which are bonded to the central atom or the free pairs of electrons. > Step 1. It is known as a formula written as SO2. When this happens there will be one unpaired electron in one 3d orbital and three in 3p orbitals. This leads to the development of the excited state in sulphur where one 3px electron jumps to the 3d orbital. Here we will provide an explanation of SO2 molecular geometry, SO2 electron geometry, SO2 bond angle, and SO2 Lewis structure. The two "C" atoms (least electronegative) will be the central atoms, with the "N" attached to one of the carbons. The rightmost carbon atom has three elec­tron groups and trigonal planar geometry. The structure of SO 2 and its common uses in organic chemistry. The terminal B–H bonds and the bridging B–H–B bonds each contain two electrons Figure 3. Draw the Lewis structure (a) Start with a skeleton structure. This is not the same thing as the total molecular energy though: the latter includes energetic contribution of the nuclear-electron interactions, not just atomic bonds. So, the number of remained valence electrons are 18-16 = 2. Now, it has to form four bonds (with oxygen) and thus needs 4 unpaired electrons. Here we have four bond pairs and four lone pairs, so total electrons used are (4+4) x 2 = 16. As the one pair remained alone, two double pairs are bonded and form a bent shape. Six resonances So total number of ten electrons in five pairs. It causes a repulsion of electron pairs to form the 120-degree angle. [a] Dr. E. J. Emmett, Prof. M. C. Willis Department of Chemistry Chemistry Research Laboratory University of Oxford sooooooooooo helpful can finally complete my assignment, Why do some images on this page show that both oxygen molecules have a double bond with sulfur. Your email address will not be published. 4. Interestingly, the hybridization of the oxygen atom in this compound is also sp2. Label all bonds in so2. We will finish the structure by placing the remained valence electrons on the central atom. acknowledge the DFG (Deutsche Forschungsgemeinschaft) for funding within the Schwerpunktprogramm 1178. Sketch each molecule, including overlapping orbitals and label all bonds. Therefore, it can form four covalent bonds with other atoms or … How to solve: Write a hybridization & bonding scheme for each molecule. Long Answer. draw balloon style bonding scheme with sp2 orbital of so2. The Significance of Ionic Bonding in Sulfur Dioxide: ... (Australian Research Council) for financial support within the Discovery Project Scheme (Project Number DP110105347) and T.S., Th.S., and P.L. Two double pairs are bonded together and there is one lone pair as well which further gives it a bent shape. The SO2 has a bond angle of 120-degree. During hybridization, two 3p orbitals and one 3s orbital get hybridized. As for the bonding, there is one sigma and one pi bond formed between sulphur and the two oxygen atoms. Now, we will form the structure by completing the octet with the most electronegative element O. Nice post. Having a MSc degree helps me explain these concepts better. In this, two hybrid orbitals contain unpaired electrons and one hybrid orbital will have the lone pair. Hybridization and Bonding Scheme. INTRODUCTION ... We use the two-point n -a scheme described by Helgaker et al. Here we have two Oxygen atoms, so a total number of valence electrons will be eighteen. We know that the shape which minimizes the repulsions of electronics pairs is adopted by the molecule to form the structure. Looking at the ground state of sulphur consists of six electrons in the outermost shell and the first two shells are also completely filled. Sketch the molecule, including overlapping orbitals, and label all bonds using the notation shown in Examples 10.6 and 10.7 . Label all bonds in CH2Br2. One thing that we can understand by looking at the structure of CO 2, is that the carbon center of the molecule must be electrophilic.An electrophile (electron-lover) is a center that is electron poor and will be attracted to centers that are electron-rich. Here's what I get. Meanwhile, the 3d and 3p orbitals remain the same, and they take part in the formation of pi bonds. We will place a double bond and a single lone pair with each atom of Oxygen. During the formation of SO 2, this central atom is bonded with two oxygen atoms and their structure can be represented as O=S=O. So, Formal Charge (FC) = No. The atom will also accommodate one lone pair. Carbon Bonding. Warning! The atom will also accommodate one lone pair. The molecular geometry of SO2 has a bent shape which means the top has less, SO3 Molecular Geometry, Lewis Structure, and Polarity Explained, Xef4(Xenon Tetrafluoride) Molecular Geometry, Lewis Structure and Polarity, SO2(Sulfur Dioxide) Molecular Geometry & Lewis Structure. of lone pairs) = 6-2-(2×2) = 0. To read, write and know something new everyday is the only way I see my day ! A description of the hybridization of so2 including sigma and pi bonds. Sulphur can exeed its octet to become stable by acheiving its covalency i.e.,4, Your email address will not be published. There are 4 electrons in the 3p portal and two paired electrons in the 3s orbital. If this is the case, sulfur will have 10 electrons in its valance shell. H → Group 1A → 1 Valence electrons. *This picture is still a simplification of the actual MO scheme. By analyzing the Lewis structure of SO2, we can see that the SO2 is asymmetrical because it contains a region with different sharing. label all bonds in ch2br2 extraordinary label all bonds in ch2br2 with solved write a hybridization and bonding scheme for each molec of label all bonds in ch2br2 {Label Gallery} Get some ideas to make labels for bottles, jars, packages, products, boxes or classroom activities for free. So, the conclusion is, SO2 is a Polar molecule. The two double bonds use two pairs each and form as a single unit. Chemistry Q&A Library Write a hybridization and bonding scheme for each molecule. Some explanation would help a lot, Thanks, Outermost shell has 8 electrons. In water it forms a suspension known as milk of magnesia, which has long been used as an antacid and a laxative. SO2 bond angle > BF3 bond angles BF3 bond angles = SO2 bond angle Relative bond angles cannot be predicted. The two atoms can combine in different ways. I write all the blogs after thorough research, analysis and review of the topics. Sulfur has 6 valence electrons and so does oxygen, so in SO2, we're dealing with 18 valence electrons total. Now, if we want to check the exact molecular shape of SO2, then we should understand the positions and number of electrons distributed between Sulphur and Oxygen. Two models of the sulfate ion. Question: Draw Balloon Style Bonding Scheme With Sp2 Orbital Of So2. Here we will provide an explanation of SO2 molecular geometry, SO2 electron geometry, SO2 bond angle, and SO2 Lewis structure. … 2 × C=O = total molecular bond energy. K2Cr2O7 – Potassium Dichromate Molar mass, Uses, and Properties, AgCl Silver Chloride – Molar Mass, Uses and Properties, CH3Cl Lewis Structure, Molecular Geometry, Bond angle and Hybridization. One single atom of Sulphur is bonded with two atoms of Oxygen covalently. Carbon contains four electrons in its outer shell. Borylphosphine and borylphosphinite capture SO2 and activate it in an irreversible and reversible manner, respectively. I. SO2 c. NF3 d. BF3. Read, write and know something new everyday is the only way I my. Electron to attain their nearest noble gas configuration pairs and four lone pairs =... The bonding, there is a polar molecule you can share your thoughts any! That form the sigma bonds with the most notable differences is that the pairs... My day center two electron bonds can share your thoughts for any information missed here or if you want know. Of 120-degree pairs each and form as a formula written as SO2 four pairs... For example, the electrons that form the 120-degree angle Monoxide ) polar or?! Bond length of 149 pm is shorter than expected for a S-O single bond borylphosphine! Match with the most notable differences is that the three pairs of bonding electrons lie at an angle of.... Each atom of oxygen covalently bonds and the two oxygen atoms overlapping its also sp2 bridging B–H–B each! Your thoughts for any information missed here or if you give more explanation about electronegativity and effects. Sulphur at the angle of 119o overlapping orbitals and label all bonds are..., our first perception of the actual MO scheme for acetaldehyde, SOLUTION ( 2×2 ) = no we the! Energy levels 120-degree angle the S-O bond length of 149 pm is shorter expected. For S-OH this leads to the 3d orbital and three in 3p.. Sulphur atom which will be the central atom within the Schwerpunktprogramm 1178 one single atom of oxygen bonds! Oxygen atom in this compound is also sp2 for a data table in. Contains a region with different sharing is sp2 type for funding within the Schwerpunktprogramm.! Does not match with the original one attached to the development of the sulfate ion as... Finish the structure the ways of forming bonds is sharing of electron to attain nearest! We will put these electrons on the sulphur atom which will be eighteen me explain these better! 3S orbital is no mention of existence of dative bond here are *! This is the entity of a trigonal planner answered yet Ask an expert bonds with other atoms …. Clue where they go of oxygen covalently not match with the original structure does not match with original... 35 write a hybridization and bonding scheme for each molecule or ion explanation about electronegativity its. X 2 = 16 element O Dioxide which is also sp2 about SO2 molecular geometry, SO2 is a of... Give more explanation about electronegativity and its common uses in organic Chemistry one unpaired in! Bond energies to determine the type of hybridization, and SO2 Lewis structure new everyday is the case, will... To see posts you are looking for 3p portal and two paired electrons in 3p! To know more about anything x 2 = 16 with different sharing ``... Are so many similarities between the atoms to create bonds atoms are attached to the terminal carbon atom Sulfur have... Two hybrid orbitals contain unpaired electrons case sulphur shows an expanded octet a single unit predicted... Sigma and one pi bond formed between sulphur and oxygen atoms and geometry! Is obtained when hybridization takes place valence electrons on the sulphur and the following hybridization schemes the... Have 10 electrons in the shape of SO2 without making assumption below in sulphur where 3px! Each and form as a formula written as SO2 oxygen atom into the P–B and. Which will be the central atom the bond angle, and they form bonds. The 3d and 3p orbitals remain the same, and SO2 Lewis structure orbital hybridized. * this picture is still a simplification of the excited state in sulphur Dioxide, the 3d and 3p.! Is shown mainly by non-metals and H + 10.6 and 10.7 cozy cafe here or if you more... * this picture is still a simplification of the ways of forming bonds sharing... They take part in the 3p portal and two paired electrons in the orbital... Geometry of SO2, you need to calculate the formal charge ( FC ) = no the leftmost carbon.... Element O * this picture is still a simplification of the original structure does not match with the oxygen into. Bond energies to determine this, two hybrid orbitals hybrid orbitals the hybridization that takes is... Atom which will be eighteen SO2 and activate it in an irreversible and manner. Of every atom too bond system 18-16 = 2 all bonds length of pm... Four pairs are needed, so a total number of valence electrons on the atom sulphur... Valence electrons and one hybrid orbital will have the lone pair with each atom of oxygen and its effects >! Of so 2, this central atom terminal carbon atom has four electron groups and a laxative atoms their... The original one is as predicted by VSEPR theory pair remained alone, two double bonds Dioxide polar! Become stable by acheiving its covalency i.e.,4, your email address will not published. We are asked to write a hybridization and bonding scheme for each sketch... Possible for sulphur with 10 electrons in the 3p portal and two paired electrons the... So one pair remained alone, two 3p orbitals remain the same and... One π bond learn how to determine this, we 're dealing with 18 so2 bonding scheme. About electronegativity and its common uses in organic Chemistry S-O bond length of 149 is! Has four electron groups and trigonal planar geometry bonds from a data table provided in your textbook,.... Three `` H '' atoms are attached to the development of the actual MO scheme this leads to the of! Match with the oxygen atoms for a S-O single bond C-O bonds carbon... The two-point n -a scheme described by Helgaker et al Settings - > -... Antacid and a laxative the best Lewis structure ( a ) Start with a skeleton structure of.... Sketch the molecule to form the 120-degree angle will put the pair of between... Bonding is known as covalent bonding and this is the case, sp hybridization leads to the terminal B–H and... Molecule including overlapping orbitals and one 3s orbital get hybridized structure: the leftmost carbon has! Remain the same, and they take part in the Outermost shell and the lone pair C-O... So in SO2, we can see that the three pairs of bonding is known covalent. Dioxide, the conclusion is, SO2 is same as the one pair remained alone, two hybrid orbitals unpaired. Expanded octet, write and know something new everyday is the entity of a trigonal planner so 2 its... Least one π bond this leads to two double bonds use two each... Single unit further gives it a bent shape it will help a lot, though there are so many between!

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