Periodic Table & Ions

Neon is an example of a noble gas because it belongs to Group 18 of the periodic table, which is also known as the noble gases. Noble gases are characterized by their full outer electron shells, making them stable and unreactive. Neon specifically has a full outer shell of electrons, making it highly stable and commonly used in neon lights due to its ability to emit a bright orange-red light when an electric current passes through it.

Magnesium (Mg) is in the alkaline earth metal family because it belongs to Group 2 of the periodic table. Alkaline earth metals are characterized by having two valence electrons and are located in the second column of the periodic table. They are less reactive than alkali metals but more reactive than transition metals. Magnesium exhibits similar properties to other alkaline earth metals such as beryllium, calcium, strontium, and barium.

The alkali metals family has 1 valence electron.

Halogens are highly reactive because they have 7 valence electrons and want to gain 1 more electron to achieve a stable octet configuration. This makes them highly electronegative and eager to form bonds with other elements in order to gain the missing electron and achieve a stable electron configuration.

Bromine, with atomic number 35, has an electron configuration of [Ar] 3d10 4s2 4p5. By gaining 1 electron, it will complete its outermost energy level and achieve a stable electron configuration similar to that of krypton (Kr), which is [Ar] 3d10 4s2 4p6. This process allows bromine to attain a full octet, making it more stable.

Noble gases are the least reactive family because they have a full outer electron shell, making them stable and unlikely to react with other elements. Their outer shell is already complete, so they do not need to gain or lose electrons to achieve stability. This lack of reactivity is due to their full valence electron configuration, making them chemically inert.

Polonium, Po, has the largest atomic radius among the elements in group 16. Atomic radius generally increases as you move down a group in the periodic table due to the addition of more energy levels. Since Polonium is located at the bottom of group 16, it has more energy levels compared to Oxygen, Sulfur, Selenium, and Tellurium, resulting in a larger atomic radius.

Fluorine is the most electronegative element on the periodic table. Electronegativity is a measure of an atom's ability to attract electrons towards itself in a chemical bond. Fluorine has the highest electronegativity value because it has a small atomic size and a high effective nuclear charge, which results in a strong attraction for electrons. This strong attraction makes fluorine highly reactive, and it readily forms bonds with other elements to achieve a stable electron configuration.

Rubidium (Rb) is an alkali metal located in Group 1 of the periodic table. Alkali metals tend to lose one electron to achieve a stable electron configuration, forming a positive ion with a charge of +1. Therefore, the correct answer is Rb+1.

Lithium, Li, is the correct answer because it is an alkali metal. Alkali metals are found in Group 1 of the periodic table and have similar properties, including being highly reactive and having a single valence electron. Hydrogen, H, is not an alkali metal as it is a nonmetal. Beryllium, Be, is not an alkali metal either as it is an alkaline earth metal. Vanadium, V, is a transition metal and not an alkali metal.

Fluorine is the most electronegative element on the periodic table because it has the highest electronegativity value. Electronegativity refers to an atom's ability to attract electrons towards itself in a chemical bond. Fluorine has a high electronegativity due to its small atomic size and high effective nuclear charge, which results in a strong attraction for electrons. This makes fluorine highly reactive and capable of forming strong bonds with other elements.

Transition metals have 2 valence electrons. This is because transition metals are located in the d-block of the periodic table, and the d sublevel can hold a maximum of 10 electrons. However, in transition metals, the outermost s sublevel is usually partially filled, with 1 or 2 electrons. Therefore, transition metals typically have 2 valence electrons.

Rubidium, Rb, has the largest atomic radii among the given elements. Atomic radius refers to the size of an atom, which is determined by the distance between the nucleus and the outermost electron shell. As you move down a group or period in the periodic table, the atomic radius generally increases. Since Rubidium is located in period 5, it has more energy levels and a larger atomic radius compared to Xenon, Vanadium, and Duborium which are located in period 5 as well. Therefore, Rubidium has the largest atomic radius among the given elements.

Helium (He) has 2 valence electrons. In the periodic table, the number of valence electrons can be determined by looking at the group number of the element. Helium is in group 18, also known as the noble gases. Elements in group 18 have a full outer electron shell, which means they have 8 valence electrons except for helium, which has only 2.

As you go down a column, electronegativity decreases because the electrons are farther from the nucleus. Electronegativity is the measure of an atom's ability to attract electrons in a chemical bond. As you move down a column in the periodic table, the number of energy levels or shells increases, causing the outermost electrons to be farther from the nucleus. This increased distance weakens the attraction between the nucleus and the electrons, resulting in a decrease in electronegativity.

Ionization energy refers to the energy needed to remove an electron from an atom or ion. This energy is required to overcome the attraction between the negatively charged electron and the positively charged nucleus. The higher the ionization energy, the more difficult it is to remove an electron, indicating a stronger attraction between the electron and the nucleus. Ionization energy is an important property in understanding the behavior of atoms and their reactivity.

Electronegativity refers to the energy needed to attract an electron. This property is used to measure the ability of an atom to attract and hold onto electrons in a chemical bond. It is determined by factors such as the number of protons in the nucleus and the distance between the nucleus and the outermost electrons. Electronegativity values are used to predict the polarity of chemical bonds and the distribution of electron density in molecules.

When an atom loses an electron, it becomes positively charged because it now has more protons than electrons. This positively charged atom is called a cation. Cations are formed when atoms undergo oxidation, which involves the loss of electrons. Cations play an important role in chemical reactions and can easily form bonds with other atoms or molecules to achieve a stable electron configuration.

Francium, Fr, has the lowest ionization energy on the periodic table. Ionization energy is the energy required to remove an electron from an atom. Francium is located in the bottom left corner of the periodic table in Group 1, which is known as the alkali metals. Alkali metals have the lowest ionization energies because they have a single valence electron that is loosely held and easily removed. Francium, being the heaviest alkali metal, has the lowest ionization energy among all the elements on the periodic table.

Fluorine (F) is located in Group 17 of the periodic table, also known as the halogens. Halogens have seven valence electrons and need to gain one electron to achieve a stable electron configuration, similar to the noble gas configuration. When fluorine gains one electron, it will have a total of eight electrons, resulting in a negatively charged ion. This is because the added electron creates an excess negative charge, balancing out the positive charge of the protons in the nucleus.

Within a period, the number of orbits/shells remains the same. A period in the periodic table represents the number of energy levels or shells that an atom has. As you move across a period, the number of protons and electrons increases, but the number of shells remains constant. This is because each period represents a new energy level being filled with electrons. Therefore, the number of orbits/shells is the same within a period.

As you go across a period, the atomic radius decreases because the nucleus pulls more on the electrons. This is due to the increasing number of protons in the nucleus, which increases the positive charge and attraction for the negatively charged electrons. As a result, the electrons are pulled closer to the nucleus, leading to a decrease in atomic radius.

Iron (Fe) is smaller than Hassium (Hs) primarily because iron has fewer orbits. The size of an atom is determined by the arrangement and number of its electrons in their respective energy levels or orbitals. Iron has fewer orbits compared to Hassium, which means that its electrons are closer to the nucleus and experience a stronger attraction. This results in a smaller atomic size for iron compared to Hassium.

An ion of Aluminum (Al) will have 13 protons because the atomic number of Aluminum is 13, which represents the number of protons in its nucleus. However, it will have 10 electrons because ions are formed when atoms gain or lose electrons. Since the question does not specify whether the ion is positively or negatively charged, we cannot determine the exact number of electrons gained or lost. However, since Aluminum is in Group 13 of the periodic table, it tends to lose 3 electrons to achieve a stable configuration, resulting in 10 remaining electrons.

The family that consists primarily of large, radioactive, man-made elements is the actinides. Actinides are a series of elements that follow actinium in the periodic table and include elements such as uranium, plutonium, and americium. These elements are typically radioactive and are often produced artificially in nuclear reactors or particle accelerators.