Interpretation: Find out and explain the type of bonding expected to be present in the compound Lithium Niobate (
Concept Introduction:
There are two types of bonds that can be formed between the atoms:
- Ionic Bond
- Covalent Bond
The ionic bond is formed due to the electrostatic attraction between the ions of opposite charge. An ionic bond is generally formed between a non-metal and a metal that has a very high difference in their properties. An ionic bond is formed when one or more valence shell electrons of an atom are transferred entirely to the valence shell of another atom.
The covalent bond is formed by the mutual sharing of electrons between the atoms. In case of a covalent bond, one electron from each atom is shared between them to form a bond. A covalent bond is generally formed between the atoms that have similar properties.
When one electron is shared between the atoms, the bond is referred to as a single covalent bond. When two electron and three electrons are shared between the combining atoms, the bond is referred to as double covalent bond and triple covalent bond respectively.
Want to see the full answer?
Check out a sample textbook solutionChapter 7 Solutions
Chemistry for Engineering Students
- The bond length in HI(1.62) is close to the sum of the atomic radii of H (0.37 Å) and I (1.33 Å). What does this fact indicate about the polarity of the bond?arrow_forwardQ.3 a) Write the chemical name and chemical formula of a compound formed between X (atomic number of X=56) and nitrate ion. (1 mark) b) Name and explain the type of chemical reaction that occurs in between two ionic compounds with the help of examples. (2 marks) c) Explain the bond formation with Lewis structure in a gas molecule that belongs to group 6A and exists as a diatomic molecule. (Mention the type of chemical bond) (2 marks)arrow_forwardFor the next compounds/ions, draw two (2) appropriate Lewis structures. One structure must obey the octet rule and the other structure must be a non-octet obeying structure (octet deficient or octet expansion). Be sure to indicate which structure is the “best” structure and explain your choice formal charge arguments and any other points you deem important. (a) BeCl2 (b) POF3 (c) SO42−arrow_forward
- Part A) Out of the following, the species with a single covalent bond is: (a) CO (b) CN- (c) Cl2 (d) N2 Part B) Which of the following compounds has ionic bonds only? (a) NH4ClO4 (b) Mg3N2 (c) Mg3(PO4)2 (c) CHCl3 Part C) The molecular shape and polarity of xenon tetrafluoride are: (a) Tetrahedral & non-polar (b) square planar & non-polar (c) Square pyramidal & polar (d) square planar & polararrow_forward(c) Draw the orbital diagrams and Lewis symbols to depict the formation of Na* and CI ions from the atoms. Give the formula of the compound formed. (d) The predicted bond length for HF is 109 pm (the sum of the covalent radii of H, 37 pm and F. 72 pm), however the actual bond length for HF is shorter (92 pm). It was observed that the difference between predicted and actual bond lengths becomes smalleor going down the halogen group from HF to HI Describe these observationsarrow_forward8.18 Specify which compound in each of the following pairsof ionic compounds should have the higher latticeenergy: (a) AlN or CaO, (b) NaF or CsF, (c) MgCl2 orMgF2. Explain your choice.arrow_forward
- 3.a. Explain the following observations: (i). The bond dissociation energy of the hydrogen molecule (H2) is greater than that of the hydrogen molecule ion (H2). (ii). Both carbon and aluminium are solids and aluminium forms sheets whereas carbon breaks into pieces when hammered. (iii). Ammonia boils at -33.3°C while phosphine boils at -87.7°C. WA b. (i). State and briefly explain the shapes of the following substances: Substances NH3 Shape Explanation BF3 (ii). Draw the electron density map for the hydrogen chloride molecule. c.(i). What is the difference between a simple covalent bond and a dative covalent bo (ii). Draw the dot and cross diagram as well as the shape of NI; molecule. Give the angle. and account for the bonding in sodium bromide (NaBr).arrow_forward• draw and label an atomic/molecular level depiction that explains the observedproperties below.• Then use the drawing to explain how the type of bonding in the element leads to itsobserved properties. 1) Bromine: Br2, mp 266 K, brown liquid, easily vaporized (bp 332 K). At temperatures above 1000K, Br2 dissociates.arrow_forwardThe structure of sodium hyaluronate, a sodium salt of hyaluronic acid used in skincare products for its hydrating properties, is shown below. What is the shape of the bonds at (ii) ? Hint: atom (iii) has been completed for you as an example. (iii) bond angle: 109.5°, geometry of the electron pairs: tetrahedral, shape of the bonds: tetrahedral ОН, OH ·•·•·||||| N O H H Ol.. OH |||| iv + Naarrow_forward
- 3. Which of the following compounds would you predict to be ionic and which would be covalent? (Hint: calculate the electronegativity difference between two bonded atoms) (d) BaCl2 (e) CO2 (a) MgO (b) HCI (c) PCI3 htolloWina' 4.0rawarrow_forwardAn important starting material for the manufacture ofpolyphosphazenes is the cyclic molecule (NPCl₂)₃. The mol-ecule has a symmetrical six-membered ring of alternating N and P atoms, with the Cl atoms bonded to the P atoms. The nitrogen-phosphorus bond length is significantly less than that expectedfor an N−P single bond.(a) Draw a likely Lewis structure for the molecule.(b) How many lone pairs of electrons do the ring atoms have?(c) What is the order of the nitrogen-phosphorus bond?arrow_forwardIn developing the concept of electronegativity, Pauling used the term excess bond energy for the difference between the actual bond energy of X¬Y and the average bond energies of X¬X and Y¬Y (see text discussion for the case of HF). Based on the values as shown, which of the following substances contains bonds with no excess bond energy?(a) PH3 (b) CS2 (c) BrCl (d) BH3 (e) Se8arrow_forward
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning