(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-MOD.MASTERINGCHEM.
- Using your knowledge of the trends in element sizes on going across the periodic table, explain briefly why the density of the elements increases from K through V.arrow_forwardWrite the electron configurations far each of the following elements: (a) Sc. (b) Ti. (c) Cr. (d) Fe. (e) Ruarrow_forwardName 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_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_forwardWrite 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_forwardWhat neutral atoms are isoelectronic with the following ions? (a) Pb4+ (b) Br (c) S2 (d) Ni3+arrow_forward
- Match 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_forwardArrange the following in order of increasing radius and increasing ionization energy. a. N+, N, N b. Se, Se, Cl, Cl+ c. Br, Rb+, Sr2+arrow_forwardAnswer the questions below concerning ground state electron configurations. (a) What element has the electron configuration [Ar]3d64s2? (b) What element has a 2+ ion with the configuration [Ar]3d5? Is the ion paramagnetic or diamagnetic? (c) Mow many unpaired electrons are in a Ni2+ ion? (d) The configuration for an element is given here. What is the identity of the element? Is a sample of the element paramagnetic or diamagnetic? How many unpaired electrons does a 3 ion of this element have? (e) What element has the following electron configuration? Write a complete set of quantum numbers for electrons 1-3.arrow_forward
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