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- Which of the four atoms Na, P, Cl, or K (a) has the largest atomic radius? (b) has the highest ionization energy? (c) is the most electronegative?Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?Arrange in order of increasing ionization energy (a) the Group 1A elements Na, Cs, and K(b) the Period 4 elements As, Ca, and Br
- Arrange in order of increasing nonmetallic character. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 4 elements V, Ge, and K (b) the Group 5A elements N, As, and Bi Arrange in order of increasing atomic size. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 3 elements Mg, Si, and Ar (b) the Group 2A elements Ca, Ba, and Sr(a) Would you expect scandium oxide to be a solid, liquid, or gas at room temperature?Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?
- choose three . What are the characteristerses of a metal like element? (a) they try to get additional electrons (b) they are melleable. (c) they are lightly to give away or share electrons. (d) they are good conductors of electricityWhich element would you expect to be more metallic?(a) Ca or Rb(b) Mg or Ra(c) Br or IThe sum of IE1through IE₄ for Group 4A(14) elements shows a decrease from C to Si, a slight increase from Si to Ge, adecrease from Ge to Sn, and an increase from Sn to Pb. (a) What is the expected trend for IEs down a group? (b) Suggest a reason for the deviations in Group 4A(14).(c) Which group might show even greater deviations?
- Which of the following ions has the smallest size? (a) Cl- (b) F- (c) Al3+ (d) Na+(a) Which ion is smaller, Co3+ or Co4+? (b) In a lithium-ionbattery that is discharging to power a device, for every Li+that inserts into the lithium cobalt oxide electrode, a Co4+ion must be reduced to a Co3+ ion to balance charge. Using the CRC Handbook of Chemistry and Physics or other standardreference, find the ionic radii of Li+, Co3+, and Co4+. Orderthese ions from smallest to largest. (c) Will the lithium cobaltoxide cathode expand or contract as lithium ions areinserted? (d) Lithium is not nearly as abundant as sodium.If sodium ion batteries were developed that function in thesame manner as lithium ion batteries, do you think “sodiumcobalt oxide” would still work as the electrode material?Explain. (e) If you don’t think cobalt would work as the redox-active partner ion in the sodium version of the electrode,suggest an alternative metal ion and explain your reasoning.34. According to general trends in the periodic table, predict which element in each of the following pairs has the greater metallic character. (b) Na or K (d) H or Fe (a) B or Al (c) Mg or Ba 1ist