Answer to Question #51139 in Inorganic Chemistry for vizzy




 How many types of sulphides are formed when alkali metals react with sulphur?  

2  

3  

4  

5  

4 The attractive force which binds a hydrogen atom of one molecule with an electronegative atom of another molecule of the same compound is called \_\_\_\_\_\_\_\_\_\_.  

nuclear bond  

electromagnetic force  

hydrogen bond  

covalent bond  

5 Ionization energy \_\_\_\_\_\_\_\_\_\_\_\_\_ down the group within the alkali metals.  

increases  

has no fixed pattern  

remains const
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recall that there are several types of intermolecular forces:1. ion-dipole interaction – occurs between an ion and a polar covalent compound2. hydrogen bonding – occurs in compounds where hydrogen is directly connected to an electronegative element such as n, o, or f3. dipole-dipole interaction – occurs between two polar covalent compounds4. induced-dipole interaction – occurs when a nonpolar compound interacts with a polar compound5. dispersion forces – occurs in all compounds. this is the primary intermolecular force exhibited by nonpolar compounds.[readmore]although hcl is a polar molecule, it still exhibits dispersion forces because it occurs in all compounds there are 3 types of hybridisation for carbon in organic compounds, sp, sp2 and sp3 depending on the number of sigma and pi bonds between the carbon atoms. more the ‘s’ character more is the electronegativity of the carbon as ‘s’ orbitals are closer to the nucleus, hence electrons held more closely. a) van der waals (present, all molecule/atoms contain it)[readmore](b) dipole-dipole (present, c=o creates a partial charge on c and o)(c) hydrogen bonding (not present, h-bonds are only present in compounds with h attached on o, n or f)(d) ion-ion (not present, only appears on compound with full charges) a) he helium (he) is an element by itself. he atom can only exhibit dispersion forces.b) hclh          1a                   1 × 1 e– = 1 e–cl         7a                   1 × 7 e– = 7 e–   total: 8 valence e–[readmore]cl is more electronegative than h, so hcl is a polar covalent compound. hcl exhibits dipole-dipole interaction.c) h2oh          1a                   1 × 2 e– = 2 e–o          6a                   1 × 6 e– = 6 e–   total: 8 valence e– since hydrogen is bonded directly to oxygen.h2o exhibits hydrogen bonding.d) cl2cl         7a                   1 × 7 e– = 14 valence e–composed of the same atom. there's no electronegativity difference.cl2 can only exhibit dispersion forces. (i) adsorption is a surface phenomenon that causes the accumulation of molecules of a substance at the surface of a solid or liquid rather than in the bulk. in adsorption, the substance gets concentrated at the surface only. it does not penetrate through the surface to the bulk of the solid or liquid. for example, when a chalk stick is dipped into an ink solution, only its surface becomes coloured.


on the other hand, the process of absorption is a bulk phenomenon. in absorption, the absorbed substance gets uniformly distributed throughout the bulk of the solid or liquid. for example, when a sponge is dipped in water the whole sponge gets wets.


(ii)according to the schulze-hardy rule, the effectiveness of the salt causing flocculation depends on the charge on the ion of opposite sign to the charge on the sol particles. the greater the magnitude of the opposite charge, the higher the ability of a salt to coagulate the sol.  
thus, trivalent salt alcl3 is more effective in causing the coagulation of a negatively charged sol than divalent salt mgcl2.


(iii)out of sulphur sol and proteins, sulphur sol forms multimolecular colloids. sulphur sol consists of particles containing a thousand or more s8 molecules. on the other hand, proteins form macromolecular colloids. chapter 5 key: electron: e                         number: # ­                 valence electron: ve   three­dimensional: 3d molecular: molec               with: w/ chemical: chem                 different: diff positive: pos negative: neg i. bonding theories ­ a. valence shell e pair repulsion (vsepr)  valence shell e pair repulsion: model predicting the arrangements of ve  ­ pairs around a central atom that minimizes their mutual repulsion  electron pair geometry: 3d arrangements of bonding pairs andn lone pairs  of e about a central atom  molecular geometry: 3d arrang hydrogen gas in its natural state consists of molecules of h2, where two hydrogen atoms are bound together by a 100% covalent bond.

the h2 molecules are attracted to each other by london dispersion forces. london dispersion forces result from the formation of temporary dipoles. magnesium atom loses 2 electrons to attain a stable electronic configuration and becomes a cation. example: a non-metallic atom like chlorine gains 1 electron to attain a stable electronic configuration and becomes an anion. example: cations and anions are oppositely charged particles which attract one another to form an electrovalent bond leading to the formation of an electrovalent compound here magnesium donates one electron each with two chlorine atoms resulting in the formation of magnesium chloride. we’re being asked which of the given compounds is a lewis acid and lewis base. let’s first define a lewis acid and a lewis base.based on the lewis definition:lewis acid is an electron pair acceptor.some characteristics of a lewis acid:• when hydrogen is connected to an electronegative element such as p, o, n, s or halogens▪ hydrogen gains a partially positive charge → makes hydrogen act as a lewis acid• positively charged metal ions[readmore]▪ can accept negative electron pairs → can act as lewis acids• central element that has less than 8 valence electrons around it▪ more likely to accept an electron pair to follow the octet rule▪ can accept electron pair → can act as lewis acidlewis base is an electron pair donor.some characteristics of a lewis base:• compounds that have lone pair(s) on a central element can act as lewis bases. • compounds that possess a negative charge can act as lewis bases. let’s draw the lewis structure of each given compound and check which of them can act as a lewis acid and lewis base.step 1: determine the central atom in this molecule.step 2: calculate the total number of valence electrons present.   step 3: draw the lewis structure for the molecule.a) cs2step 1: determine the central atom in this molecule.c is less electronegative than s → c will be the central atomstep 2: calculate the total number of valence electrons present.                group             valence electronsc         4a                   1 x 4 e‑ = 4 e-s         6a                   2 x 6 e‑ = 12 e-              total: 16 valence e- step 3: draw the lewis structure for the molecule• c has a total of 8 e- electrons around it and has a lone pair→ complete octet▪ can act as a lewis acidb) sh−step 1: determine the central atom in this molecule.only two atom → no central atomstep 2: calculate the total number of valence electrons present.                group             valence electronss         6a                   1 x 6 e‑ = 6 e-h        1a                   1 x 1 e‑ = 1 e-from -1 charge:                     +1 e-              total: 8 valence e- step 3: draw the lewis structure for the molecule▪ has a negative charge▪ can act as a lewis baseanswer: sh- is the lewis base and its lewis structure is cs2 is the lewis acid and its lewis structure is The physical and chemical properties of elements depend on the number of valence electrons. Elements present in the same group have the same number of valence electrons. Therefore, elements present in the same group have similar physical and chemical properties.