Question

1. the ionic radius compared to the atomic radius of the parent atom is: (a) generally larger for all ions (b) generally smaller for all ions (c) larger for positive ions and smaller for negative ions (d) larger for negative ions and smaller for positive ions. 45. in the same group of elements, the ionization energy tends to decrease with increasing atomic number. this is due partially to the: (a) decreasing size of the atom itself (b) increasing forces of attraction (c) outer electrons being closer to the nucleus (d) outer electrons being farther form the nucleus. 46. an element with the electron configuration of 1s² 2s² 2p⁶ 3s² would belong in which group? (a) nitrogen group (b) alkaline earth metals (c) noble gases (d) halogens. 47. the characteristic properties of metals are associated with: (a) strongly held valence electrons (b) completely filled energy levels (c) partially filled orbitals (d) loosely held valence electrons. fill in the blank: 48. how many valence electrons does silver have? 49. what is the valence shell of tungsten (w)? 50. which element (y, tc, cd) has the least electronegativity? 51. which element (na, k, fr, o) has the greater ionization energy? 52. which element (fe, zn, ru, ta, fr) is the most metallic? 53. what do you call a vertical column on the periodic table? 54. what do you call a horizontal row on the periodic table? 55. which scientist is responsible for the periodic table that we are using today? 56. within a group of elements in the periodic table, as the atomic number increases, the atomic radius (increases, decreases, remains the same)? 57. which family contains the most active (reactive) group of nonmetals? 58. where are the most metallic elements found on the periodic table? (upper right, lower left, upper left, or lower right) 59. as you go from left to right on the periodic table, does the ionization energy increase or decrease? 60. as you go from left to right on the periodic table, does the electronegativity increase or decrease? 61. as you go down the periodic table, does the ionization energy increase or decrease? 62. what term means that an element can be hammered into flat sheets?

Explanation:

• 44: When an atom loses electrons to form a positive ion (cation), the remaining electrons are more strongly attracted to the nucleus, so the ionic radius is smaller than the atomic radius. When an atom gains electrons to form a negative ion (anion), the electron - electron repulsion increases, and the ionic radius is larger than the atomic radius.
• 45: In a group, as the atomic number increases, the number of electron shells increases. Outer electrons are farther from the nucleus. The ionization energy is the energy required to remove an electron. Electrons farther from the nucleus are easier to remove (lower ionization energy).
• 46: The electron configuration \(1s^{2}2s^{2}2p^{6}3s^{2}\) has 2 valence electrons (\(3s^{2}\)). Alkaline earth metals (Group 2) have 2 valence electrons.
• 47: Metals have loosely held valence electrons. These delocalized electrons are responsible for properties like electrical conductivity, thermal conductivity, and malleability.
• 48: Silver (\(Ag\)) has an electron configuration of \([Kr]4d^{10}5s^{1}\), so it has 1 valence electron.
• 49: Tungsten (\(W\)) has an electron configuration of \([Xe]4f^{14}5d^{4}6s^{2}\), and its valence shell is the 6th shell (\(n = 6\)).
• 50: Electronegativity generally decreases down a group and increases across a period. Yttrium (\(Y\)) is in Group 3, Technetium (\(Tc\)) in Group 7, and Cadmium (\(Cd\)) in Group 12. Yttrium has the least electronegativity among them.
• 51: Ionization energy generally decreases down a group. Oxygen (\(O\)) is a non - metal, and among the metals \(Na\), \(K\), \(Fr\), oxygen has a higher ionization energy as non - metals have relatively higher ionization energies compared to metals in the same period (for \(O\) and \(Na\)) and it is not in the same group as \(K\) and \(Fr\) but based on general trends (non - metal vs metal).
• 52: Metallic character increases down a group and decreases across a period. Francium (\(Fr\)) is the most metallic among the given elements as it is the lowest in the group (Group 1) among them.
• 53: A vertical column on the periodic table is called a group.
• 54: A horizontal row on the periodic table is called a period.
• 55: Dmitri Mendeleev is responsible for the periodic table that we are using today (with some modern refinements).
• 56: Within a group, as the atomic number increases (more electron shells), the atomic radius increases.
• 57: The halogens (Group 17) are the most active (reactive) group of nonmetals as they only need one electron to complete their octet.
• 58: The most metallic elements are found in the lower left of the periodic table.
• 59: As you go from left to right on the periodic table, the ionization energy generally increases (due to increased nuclear charge and decreased atomic radius).
• 60: As you go from left to right on the periodic table, the electronegativity generally increases (due to increased nuclear charge and smaller atomic size, making it easier to attract electrons).
• 61: As you go down the periodic table, the ionization energy generally decreases (as electrons are farther from the nucleus).
• 62: The term that means an element can be hammered into flat sheets is malleability.

Answer:

• 44. (d) larger for negative ions and smaller for positive ions
• 45. (d) outer electrons being farther form the nucleus
• 46. (b) alkaline earth metals
• 47. (d) loosely held valence electrons
• 48. 1
• 49. 6th shell
• 50. Y
• 51. O
• 52. Fr
• 53. Group
• 54. Period
• 55. Dmitri Mendeleev
• 56. increases
• 57. Halogens
• 58. lower left
• 59. increase
• 60. increase
• 61. decrease
• 62. Malleability