(a)
Interpretation:
Which element is a metal should be determined.
Concept introduction:
Most of the elements found in the periodic table are metals. All elements in group 1 and 2 are metals except hydrogen. All elements in d block are metals. They are called
(b)
Interpretation:
Which element has the greater ionization energy should be determined.
Concept introduction:
Ionization energy is amount of energy must be absorbed by a gaseous atom in ground state to remove an electron. Further away the electron from the nucleus; it’s easy to remove the electron from the atom/ion. Hence, ionization energy will be less.
(c)
Interpretation:
Which element has the larger atomic radius should be determined.
Concept introduction:
Atomic radius is the distance between the nucleus and the valence electron shell of the atom.
(d)
Interpretation:
Which element has the greater
Concept introduction:
Electron affinity is the change in energy when an electron is added to an atom to form a negative ion.
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General Chemistry: Principles and Modern Applications (11th Edition)
- Write electron configurations for the following elements. a. The Group III A element in the same period as 4Be b. The Period 3 element in the same group as 5B c. The lowest-atomic-numbered metal in Group IIA d. The two Period 3 elements that have no unpaired electronsarrow_forwardWrite the electron configurations far each of the following elements: (a) Sc. (b) Ti. (c) Cr. (d) Fe. (e) Ruarrow_forwardWrite the symbol of each element described below. (a) largest atomic radius in Group 1 (b) smallest atomic radius in period 3 (c) largest first ionization energy in Group 2 (d) most electronegative in Group 16 (e) element(s) in period 2 with no unpaired p electron (f) abbreviated electron configuration is [Ar] 4s23d3 (g) A +2 ion with abbreviated electron configuration [Ar]3d5 (h) A transition metal in period 4 forming a +2 ion with no unpaired electronsarrow_forward
- Name and give the symbol of the element that has the characteristic given below. (a) Its electron configuration in the excited state can be 1s22s22p63s1 3p3. (b) It is the least electronegative element in period 3. (c) Its +3 ion has the configuration [36Kr]. (d) It is the halogen with the largest atomic radius. (e) It has the largest ionization energy in Group 16.arrow_forwardWhich main group atom would be expected to have the lowest second ionization energy?arrow_forwardMatch each element on the right with a set of characteristics on the left. a A reactive, pale yellow gas; the atom has a large electron affinity b A soft metal that reacts with water to produce hydrogen c A metal that forms an oxide of formula R2O3 d A colorless gas; the atom has a moderately large negative electron affinity Oxygen (O2) Gallium (Ga) Barium (Ba) Fluorine (F2)arrow_forward
- Fluoride ion, F, has no unpaired electrons. Vanadium forms four binary fluoridesVF2, VF3, VF4, and VF5. Assume that all four are ionic compounds. (a) Which fluoride is diamagnetic? (b) Which fluoride has the greatest attraction to a magnetic field? (c) Which fluoride has two unpaired electrons per vanadium?arrow_forwardWhich of the following statements is(are) true? a. F has a larger first ionization energy than does Li. b. Cations are larger than their parent atoms. c. The removal of the first electron from a lithium atom (electron configuration is ls2 2s1 ) is exothermic-that is, removing this electorn gives off energy. d. The He atom is larger than the H+ ion. e. The Al atorn is smaller than the Li atom.arrow_forwardWrite the orbital diagram for (a) Li(b) P(c) F(d) Fearrow_forward
- Describe the major trends that emerge when atomic radii are plotted against atomic number. Describe the trends observed when first ionization energies are plotted against atomic number.arrow_forwardWhat neutral atoms are isoelectronic with the following ions? (a) Pb4+ (b) Br (c) S2 (d) Ni3+arrow_forward6.82 A particular element has the following values for its first four ionization energies: 900, 1760, 14, 850, and 21,000 kJ/mol. Without consulting a list of ionization energy values, determine what group in the periodic table this element belongs in.arrow_forward
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