Question 1

How many electrons are in the most likely ion formed from an atom located in group 2A and period 5?  Paired item 1)

Accepted Answer

Atoms in group 2A typically lose two electrons to form a +2 ion. An atom in group 2A and period 5 is strontium (Sr), which has 38 electrons in its neutral state. When it forms a +2 ion, it loses 2 electrons, resulting in 36 electrons.

Question 2

UV-Visible spectroscopy can be used to study chromophores such as C=C-C=C which absorb in the UV region of the electromagnetic spectrum ranging from _____.

Accepted Answer

Chromophores like C=C-C=C absorb in the UV region, typically within the range of 100 - 300 nm, as they have electronic transitions that require the energy provided by UV light.

Question 3

In what block, group, and period on the periodic table can the atom with a 1s²2s²2p⁶3s¹ ground-state electron configuration be found? Paired item 1)

Accepted Answer

The given electron configuration corresponds to sodium (Na), which is in the s-block, group 1A (alkali metals), and period 3 of the periodic table.

Question 4

Which of the following sources of radiation is higher in energy?

Accepted Answer

Ultra violet light has a higher energy compared to visible and infrared light because it has a shorter wavelength and higher frequency.

Question 5

In which orbital does an electron add to in chlorine to form an octet?

Accepted Answer

An electron adds to the 3p orbital in chlorine to form an octet, as chlorine needs to fill its 3p orbital to achieve a stable electronic configuration.

Question 6

What is the ground-state electron configuration of carbon?

Accepted Answer

The correct electron configuration for carbon in its ground state is 1s^2 2s^2 2p^2, which corresponds to the notation given in option B. This notation indicates that carbon has two electrons in the 1s orbital, two electrons in the 2s orbital, and two electrons in the 2p orbital.

Question 7

What is the electron configuration of a copper II) ion?

Accepted Answer

Copper(II) ion (Cu²⁺) is formed by removing two electrons from a neutral copper atom, which has the configuration [Ar]4s¹3d¹⁰. Removing two electrons results in [Ar]3d⁹.

Question 8

According to periodic trends, which metal has the lowest ionization energy?

Accepted Answer

Cs (Cesium) has the lowest ionization energy among the options given. This is because ionization energy decreases down a group in the periodic table, and Cs is located below Li and Rb in Group 1, making it the easiest to remove an electron from.

Question 9

Identify the transition metal ion and the number of electrons with the following electron configuration, [Ar]4s⁰3d⁷.

Accepted Answer

The electron configuration [Ar]4s^03d^7 corresponds to a cobalt ion with a +2 charge, meaning it has lost 2 electrons from its neutral state, resulting in 25 electrons.

Question 10

According to periodic trends, which metal has the highest ionization energy?  Paired item 1)

Accepted Answer

Lithium (Li) has the highest ionization energy among the options given. Ionization energy generally increases across a period from left to right and decreases down a group in the periodic table. Since lithium is located in the first group and is the lightest and topmost among the options, it has the highest ionization energy.

Question 11

Which nonradioactive group I metal would be the most reactive in water and why?

Accepted Answer

Cesium is the most reactive group I metal in water because its one valence electron is the farthest from the nucleus compared to the other metals, making it easier to lose that electron in reactions.

Question 12

In what block, group, and period on the periodic table can the atom with a 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁵ ground-state electron configuration be found?

Accepted Answer

The given electron configuration corresponds to an element with 35 electrons, which is bromine (Br). Bromine is in the p-block, group 7A (or 17 using IUPAC numbering), and period 4 of the periodic table.

Question 13

How many electrons are in the most likely ion formed from an atom located in group 6A and period 3?

Accepted Answer

Atoms in group 6A (or 16 using the IUPAC system) have 6 valence electrons and tend to gain 2 electrons to achieve a stable electron configuration, resembling the nearest noble gas. An atom in period 3 of this group is sulfur (S), which has 16 electrons in its neutral state. Gaining 2 electrons to form an ion, it would have 18 electrons.

Question 14

Which of the following elements have a tendency to gain electrons?

Accepted Answer

Elements like Cl, O, and F are nonmetals with high electronegativities, meaning they have a strong tendency to gain electrons to achieve a stable electronic configuration.

Question 15

What is the m_s value for an electron added to bromine to form an octet?

Accepted Answer

The m_s value for an electron added to bromine to form an octet is -1/2, indicating the spin of the electron.

Question 16

What is the electron configuration of a copper atom?

Accepted Answer

The correct electron configuration for a copper atom is [Ar] 3d^10 4s^1, which is a simplified way to represent the actual electron configuration. The given options seem to be incorrectly formatted or use a non-standard notation. However, option B appears to attempt to convey [Ar] 3d^10 4s^1, despite the unconventional notation. Copper is known for its exception to the expected electron configuration due to electron correlation effects and stability reasons, preferring to have a full d-subshell.

Quiz 6: Electronic Structure and Periodic Properties of Elements

How many electrons are in the most likely ion formed from an atom located in group 2A and period 5? Paired item 1)