Sovi.AI - AI Math Tutor

Scan to solve math questions
ENFRDEESJAZH-CNZH-TW

QUESTION IMAGE

for each of the following grouping of elements, circle the element with…

Question

for each of the following grouping of elements, circle the element with the largest first ionization energy

  1. iron (fe), germanium (ge)
  2. fluorine (f), astatine (at)
  3. rubidium (rb), chlorine (cl)
  4. helium (he), radon (rn)

for each of the following groupings of elements, order them in order of increasing first ionization energy (smallest to largest)

  1. hydrogen (h), lithium (li), beryllium (be)
  2. boron (b), iodine (i), indium (in)
  3. strontium (sr), gold (au), tin (sn)
  4. seaborgium (sg), magnesium (mg), palladium (pd)
  5. krypton (kr), sodium (na), oxygen (o)
  6. carbon (c), cobalt (co), titanium (ti)
  7. neon (ne), rutherfordium (rf), selenium (se)

Explanation:

Brief Explanations

The first ionization energy is the energy required to remove the outermost (loosest) electron from a neutral atom in the gas phase. Generally, ionization energy increases across a period (from left to right) and decreases down a group in the periodic table. Noble gases have very high ionization energies as they have a full valence shell.

  1. Iron (Fe) is a transition metal and Germanium (Ge) is a metalloid. Ge is further to the right in the periodic table than Fe (Fe: period 4, group 8; Ge: period 4, group 14). As we move from left to right across a period, ionization energy increases (due to increased nuclear charge and same - electron shell shielding). So Ge has a higher first ionization energy.
  2. Rubidium (Rb) is an alkali metal (group 1, very low ionization energy as it readily loses an electron to get a noble - gas configuration). Chlorine (Cl) is a non - metal (group 17). Non - metals have higher ionization energies than metals in the same period (Cl is in period 3, group 17; Rb is in period 5, group 1. But even considering the period difference, the group trend (metals vs non - metals) is more significant here. Cl has a higher first ionization energy.
  3. Fluorine (F) and Astatine (At) are in the same group (group 17 - halogens). As we move down a group, ionization energy decreases (because the outermost electrons are further from the nucleus and more shielded). F is higher up in the group, so F has a higher first ionization energy.
  4. Helium (He) and Radon (Rn) are noble gases. He is in period 1, group 18; Rn is in period 6, group 18. Since ionization energy decreases down a group, He has a higher first ionization energy.
  5. Hydrogen (H: period 1, group 1), Lithium (Li: period 2, group 1), Beryllium (Be: period 2, group 2). Li has a lower ionization energy than H because the electron in Li is in a higher energy level (n = 2). As we move from left to right in period 2 (from Li to Be), ionization energy increases. So the order is Li < H < Be.
  6. Boron (B: period 2, group 13), Iodine (I: period 5, group 17), Indium (In: period 5, group 13). In (a metal) has a lower ionization energy than I (a non - metal). B (period 2) has a higher ionization energy than In (period 5) because of the period trend. So the order is In < B < I.
  7. Strontium (Sr: period 5, group 2 - alkaline earth metal), Gold (Au: period 6, transition metal), Tin (Sn: period 5, group 14 - metalloid). Sr (metal) has a lower ionization energy than Sn (metalloid). Au (transition metal) has a higher ionization energy than Sr (due to its position in the periodic table, but lower than Sn as Sn is a metalloid closer to non - metals). So the order is Sr < Au < Sn.
  8. Seaborgium (Sg: period 7, transition metal), Magnesium (Mg: period 3, group 2 - alkaline earth metal), Palladium (Pd: period 5, transition metal). Sg (very large atom, lower ionization energy) < Mg (but Mg is a group 2 element, which has a higher ionization energy than some transition metals in higher periods) < Pd (Pd has a relatively higher ionization energy due to its electron configuration and position). So the order is Sg < Mg < Pd.
  9. Krypton (Kr: period 4, group 18 - noble gas), Sodium (Na: period 3, group 1 - alkali metal), Oxygen (O: period 2, group 16 - non - metal). Na (metal) has the lowest ionization energy. O (period 2) has a higher ionization energy than Na (period 3). Kr (noble gas) has the highest. So the order is Na < O < Kr.
  10. Carbon (C: period 2, group 14 - non - metal), Cobalt (Co: period 4, transition metal), Titanium (Ti: period 4, transition metal). Ti and Co (metals) have lower ioniza…

Answer:

  1. Ge
  2. Cl
  3. F
  4. He
  5. Li < H < Be
  6. In < B < I
  7. Sr < Au < Sn
  8. Sg < Mg < Pd
  9. Na < O < Kr
  10. Ti < Co < C
  11. Rf < Se < Ne