The sodium chloride is an ionic compound. The chloride ions crystallize in a fcc and the sodium ion occupies half of the octahedral holes. Describe the arrangement of the ions in the crystalline structure.
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- Which of these are examples of hydrogen bonding?Describe the fourteen Bravais latticesSodium hydride, NaH, is available commercially as a gray-white powder. It melts at 800°C with decomposition. It reacts explosively with water and ignites spontaneously upon standing in moist air. Q) Write a Lewis structure for the hydride ion and for sodium hydride. Is your Lewis structure consistent with the fact that this compound is a high-melting solid? Explain.
- How is the chemical bonding within a molecule of carbon dioxide different from chemical bonding within a crystal of iron?Define valency by taking examples of silicon and sulphur?Quartz crystals are made of silicon dioxide. What is the molecular geometry of silicon dioxide? (*hint* sketch the molecule before answering) O Linear O Bent O Trigonal Pyramidal O Tetrahedral
- A new element was discovered that fits into group 16 of the 8th period. This element, apocalyptium (symbol Ap), forms compounds with the formula ApBr4 Determine the electron geometry and the molecular geometry of this compound. The electron geometry is trigonal bipyramidal and the molecular geometry is the see-saw shape. O The electron geometry is tetrahedral and the molecular geometry is square planar. O The electron geometry is tetrahedral and the molecular geometry is tetrahedral. The electron geometry is trigonal bipyramidal and the molecular geometry is tetrahedral.Dispersion forces are produced when an electronegative atom pulls on the electron of a hydrogen atom so much that the proton of the hydrogen can closely interact with the electronegative atom of another molecule electronegative atoms pull electrons toward one area of the molecule, creating regions of partial positive and partial negative charge that are attracted to regions of other molecules with the opposite charge electrons are transferred from one atom to another to produce anions and cations that are then held together in a rigid lattice electrons in molecular compounds are constantly moving and produce short-term regions of positive and negative charge that are attracted to regions of other molecules with the opposite chargeIn a hydrogen molecule, the two hydrogen atoms are held together by a single bond with a bond energy of 436 kJ/mol of hydrogen. In other words, to break the H-H bonds in one mole of molecular hydrogen requires the expenditure of 436 kJ of energy. Using the balanced chemical equation for the formation of water from oxygen and hydrogen (shown above), and interpreting the stoichiometric coefficients as mole amounts, how much energy must be expended in breaking the H-H bonds? kJ
- What is the general formula for a compound if anions occupy the hcp lattice points and cations occupy half of the tetrahedral holes? AB O O A3B AB₂ A₂BExplain how the stoichiometry between cation-to-anion (or vice-versa) affects whether a given ionic compound is going to adopt one of the structure of binary compounds or notAnswer the questions in the table below about the shape of the xenon tetrafluoride (XeF4) molecule. How many electron groups are around the central xenon atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central xenon atom? (You may need to use the scrollbar to see all the choices.) 0 (choose one) (choose one) linear bent T-shaped trigonal planar trigonal pyramidal square planar square pyramidal tetrahedral sawhorse trigonal bipyramidal octahedral