Question

question 24 (1 point)
in which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?
○ a f, 19 protons, 19 electrons
○ b in, 49 protons, 49 electrons
○ c zn, 30 protons, 60 electrons
○ d cs, 55 protons, 132.9 electrons

question 25 (1 point)
which of the following is true about the electron configurations of the noble gases?
○ a the highest occupied s and p sublevels are partially filled.
○ b the electrons with the highest energy are in an f sublevel.
○ c the highest occupied s and p sublevels are completely filled.
○ d the electrons with the highest energy are in a d sublevel.

question 26 (1 point)
elements that are characterized by the filling of p orbitals are classified as ——
○ a groups 3a through 8a
○ b groups 1a and 2a
○ c transition metals
○ d inner transition metals

Explanation:

Question 24

• Option a: Fluorine (\(F\)) has 9 protons (atomic number = number of protons). For a neutral atom, number of electrons = number of protons. So, it should have 9 electrons, not 19.
• Option b: Indium (\(In\)) has an atomic number of 49. For a neutral \(In\) atom, number of protons = number of electrons = 49.
• Option c: Zinc (\(Zn\)) has 30 protons. For a neutral \(Zn\) atom, number of electrons = 30, not 60.
• Option d: Cesium (\(Cs\)) has 55 protons. Number of electrons in a neutral atom is an integer (55), not 132.9 (132.9 is the atomic mass of \(Cs\)).

• Noble gases have a full valence shell. The highest - occupied \(s\) and \(p\) sublevels are completely filled. For example, helium (\(He:1s^{2}\)), neon (\(Ne: [He]2s^{2}2p^{6}\)) etc.
• Option a: If the highest - occupied \(s\) and \(p\) sublevels were partially filled, the atoms would be reactive (like in halogens or alkali metals), but noble gases are inert.
• Option b: The highest energy electrons in noble gases (except for some heavier ones which are not the general case) are not in \(f\) - sublevels. For example, \(He\) has electrons in \(s\) - sublevel, \(Ne\) in \(s\) and \(p\) sublevels.
• Option d: The highest energy electrons in noble gases (except for some heavier ones which are not the general case) are not in \(d\) - sublevels.

• Option a: Groups \(3A - 8A\) (or \(13 - 18\) in the modern numbering) have their valence electrons filling \(p\) orbitals. For example, group \(3A: ns^{2}np^{1}\), group \(4A:ns^{2}np^{2}\) up to group \(8A:ns^{2}np^{6}\) (noble gases).
• Option b: Groups \(1A\) and \(2A\) have their valence electrons filling \(s\) orbitals (\(1A: ns^{1}\), \(2A:ns^{2}\)).
• Option c: Transition metals have their valence electrons filling \(d\) orbitals (\((n - 1)d^{1 - 10}ns^{0 - 2}\)).
• Option d: Inner - transition metals have their valence electrons filling \(f\) orbitals (\((n - 2)f^{1 - 14}(n - 1)d^{0 - 1}ns^{2}\)).

Answer:

B. In, 49 protons, 49 electrons

Question 25