Chemistry Section 8

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• Compounds with added water molecules are called hydrates.
• A solution of Na2SO4 will be neutral.
• A 1 molar solution of glucose in water contains a weight of 180g/dm3 of glucose.
• Water of crystallization can be removed by heating.
• Na2SO4 is a salt that does not hydrolyze.
• Molality is the concentration unit independent of temperature.
• The molal boiling point constant is the ratio of the elevation of boiling point to molality.
• One molal CaCI2 solution has the minimum freezing point.
• Na2SO4 * 10H2O doesn’t show a continuous solubility curve.
• A phase is a sample of matter with uniform properties and fixed composition.
• The component of a solution in smaller amount is the solute.
• 10ml of alcohol dissolves in 90ml of water using % v/v concentration.
• A solution with 58.5g of NaCl per 1 dm3 is a 1M solution of NaCl.
• A solution where the volume equals the sum of component volumes is an ideal solution.
• A zeotropic solution distills over with a change in composition.
• Solubility is the concentration of solute molecules in equilibrium with a solid substance.
• Correct molecular weight determination from Raoult’s law applies to non-volatile solutes in dilute solutions.
• Beckmann’s apparatus measures depression in freezing point.
• Hydration involves surrounding molecules or ions with solvent molecules.
• ppm means parts of solute in one million parts of solution.
• Relative lowering of vapor pressure is directly proportional to molality in a dilute solution.
• Passing electricity through CuSO4 solution using Pt electrode causes the solution’s color to fade.
• Mn has the maximum oxidation number among N, Cr, S, and Mn.
• In a galvanic cell, chemical energy is converted into electricity.
• Molten NaCl conducts electricity due to the presence of free ions.
• Electricity in a voltaic cell is produced through oxidation and reduction reactions.
• In an electrolytic cell, electricity drives a non-spontaneous reaction.
• In an electrolytic cell, electricity carries out non-spontaneous reactions.
• Electricity flows from anode to cathode through the external electric circuit in a voltaic cell.
• The standard electrode potential of Zn is measured using a 1 M ZnSO4 solution.
• [Ni(CO)4] is represented in a voltaic cell with Cu+2(aq) as the cathode.
• A voltaic cell can be recharged by replacing the external circuit with an external source of electricity.
• H2 gas in the standard hydrogen electrode (SHE) is filled at a pressure of 760mm of Hg.
• The chemical used in a salt bridge is KCI.
• The electrochemical series lists elements based on their hydrogen scale.
• In a galvanic cell, the standard reduction potential of Zn is greater than that of the coupled electrode.
• A greater value of standard reduction potential indicates a greater tendency to form positive ions.
• Lead accumulators are rechargeable secondary cells used in batteries.
• The capacity of one lead accumulator cell is 2 volts.
• The strength of sulfuric acid in a lead accumulator is 30%.
• A Voltaic cell is a device that converts chemical energy into electricity.
• In the production of wrought iron, Mg, Si, and P are removed in the form of slag.
• Half cells are interconnected through a salt bridge.
• Pt is used as an inert electrode in many electrochemical reactions.
• The stronger the oxidizing agent, the greater its reduction potential.
• Silver oxide cells are non-rechargeable.
• In a Zn-Cu cell, zinc acts as an anode, and copper acts as a cathode.
• The degree of dissociation of a weak electrolyte increases with dilution.
• In an electrolytic solution, conductance of electricity is due to ions.
• Oxidation is the reaction that occurs at the anode in an electrochemical cell.
• Reduction is the process that involves a decrease in the oxidation number of an element.
• In a Zn-Cu cell, the right half-cell contains the Cu electrode.
• A salt bridge transfers ions between the two half-cells in an electrochemical cell.
• E0red of an element can be calculated by comparing it with the standard hydrogen electrode (SHE).
• The potential of the standard hydrogen electrode (SHE) is considered to be zero.
• Electrode potential of Zn is a reduction process.
• A greater value of standard reduction potential indicates a greater tendency to get reduced.
• Non-rechargeable cells cannot be recharged and are used once.
• One lead accumulator cell has a capacity of 2 volts.
• The density of H2SO4 in a lead accumulator is 1.25g/cm3.
• In an alkaline battery, the anode is made up of Zn.
• The oxidation number of the central metal atom in K2Cr2O7 is 6.
• Group VIB of transition elements includes Cr, Mo, and W.
• The melting points and boiling points in the middle of the 3d-series elements generally increase.
• Compounds that are attracted by an applied strong magnetic field are paramagnetic.
• When light is exposed to transition elements, electrons jump from lower to higher energy orbitals.
• A compound of a transition element dissolved in a solution of salt produces complex ions.
• Transition elements have variable oxidation states.
• Transition elements are located between the lanthanides & actinides and the s and p block elements.
• Pure metals do not corrode easily.
• The electronic configuration of Cr is [Ar]4s13d5.
• The oxidation state of the central metal atom in [Ni(CO)4] is 4.
• Hydration is a process in which molecules and ions are surrounded by water molecules.
• A ligand that donates two electron pairs in a coordination compound is a bi-dentate ligand.
• The species that donate two electron pairs in a coordination compound is a bi-dentate ligand.
• The geometry of complex compounds depends on the hybridization of the central metal atom.
• The oxidation number of a transition element is usually variable.
• In the production of wrought iron, MnO is reduced to Mn.
• The inner d orbitals of a metal are shielded from the nuclear charge by the outer d orbitals.
• The elements at the bottom of the groups in the periodic table tend to have higher electron affinities.
• Coordination compounds have distinctive colors due to their electronic transitions.
• A ligand can be an atom, ion, or molecule that donates a pair of electrons to the central metal atom.
• The central metal atom in a coordination compound is often a Lewis acid.
• The catalytic activity of transition metals is due to their variable oxidation states.
• Transition elements have high melting and boiling points.
• Transition elements exhibit catalytic activity due to their variable oxidation states.
• The d orbitals of transition metals fill in a specific manner.
• The magnetic properties of transition metal complexes arise due to the presence of unpaired electrons.
• The elements in the d-block of the periodic table are often referred to as transition elements.
• The formation of complex compounds involves coordination bonds.
• The variable oxidation states of transition elements are due to the presence of unpaired electrons.
• Transition elements often form colored compounds due to electronic transitions.
• Transition elements show catalytic activity due to their ability to adopt multiple oxidation states.
• Ligands in coordination compounds can be classified as monodentate or polydentate.
• Transition elements exhibit magnetic properties due to the presence of unpaired electrons.
• In coordination compounds, ligands are attached to the central metal ion through coordination bonds.
• The d orbitals of transition metals play a key role in their chemistry.
• Transition elements form complex compounds when they react with ligands.
• The variable oxidation states of transition metals are important for their ability to act as catalysts.
• The magnetic properties of transition metal complexes are due to the presence of unpaired electrons.
• The electronic configuration of Cu is [Ar]4s23d9.
• The coordination number of a complex compound is the number of donor atoms attached to the central metal ion.
• The formation of coordinate bonds involves the sharing of electrons between the central metal atom and the ligand.
• Transition elements often exhibit different oxidation states in their compounds.
• The presence of partially filled d orbitals in transition elements contributes to their reactivity.
• Coordination compounds are substances in which central metal atoms are surrounded by ions or molecules.
• The color of coordination compounds is due to the absorption of specific wavelengths of light.
• Transition elements are characterized by the filling of 3d orbitals.
• The variable oxidation states of transition elements allow them to form a wide range of compounds.
• The catalytic activity of transition elements is due to their ability to change oxidation states during reactions.
• In coordination compounds, ligands donate electron pairs to the central metal ion to form coordinate bonds.
• Transition elements often have higher melting and boiling points compared to s-block elements.
• The electronic configuration of Fe is [Ar]4s23d6.
• Ligands in coordination compounds can be classified as monodentate, bi-dentate, or polydentate.
• Transition elements are good conductors of heat and electricity due to their metallic properties.
• The magnetic properties of coordination compounds arise due to the presence of unpaired electrons in metal d orbitals.
• Coordination compounds are often used as catalysts in various industrial processes.
• The variable oxidation states of transition elements are a consequence of their electronic configuration.
• The formation of complex compounds is a result of the coordination bonds formed between the central metal ion and ligands.
• Transition elements often form colored compounds due to the splitting of d orbitals in a ligand field.