Periodic Table - Trends & Families

Magneiusm is in the alkaline earth metal family because it belongs to Group 2 of the periodic table, which includes elements such as beryllium, magnesium, calcium, strontium, barium, and radium. These elements have two valence electrons and are generally shiny, silvery-white, and relatively reactive. They are also known for their high melting points and low electronegativity.

Noble gases are the least reactive family because they have a full outer electron shell, making them stable and less likely to form chemical bonds with other elements. This stability is due to their complete electron configuration, which does not require them to gain or lose electrons to achieve a stable state. As a result, noble gases have little tendency to react with other elements, making them the least reactive family on the periodic table.

The alkali metals family has 1 valence electron.

Lithium is an alkali metal because it belongs to Group 1 of the periodic table. Alkali metals are highly reactive metals that are soft, have low melting points, and readily lose their outermost electron to form a positive ion. Lithium exhibits these characteristics, making it an alkali metal. Hydrogen is not an alkali metal as it is a nonmetal, beryllium is an alkaline earth metal, and vanadium is a transition metal.

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 reactive and likely to form compounds with other elements in order to gain that additional electron.

Ionization energy refers to the energy needed to remove an electron from an atom or molecule. This energy is required to overcome the attractive force 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 hold of the electron by the nucleus.

Electronegativity refers to the energy needed to attract an electron. It is a measure of an atom's ability to attract and hold onto electrons when it is bonded to another atom. The higher the electronegativity of an atom, the stronger its attraction for electrons. This property is important in determining the type of bond that will form between atoms, as atoms with higher electronegativity values will tend to attract electrons more strongly and form polar covalent or ionic bonds.

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

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 of 3.98 on the Pauling scale, indicating its strong ability to attract electrons. This is due to its small atomic size and high effective nuclear charge. Therefore, fluorine has a strong tendency to gain electrons and form negative ions, making it the most electronegative element.

Selenium is an example of a chalcogen. Chalcogens are a group of elements in the periodic table that includes oxygen, sulfur, selenium, tellurium, and polonium. These elements have similar chemical properties and are located in Group 16 of the periodic table. Selenium, with atomic number 34, is a nonmetal and is commonly used in various industries, including electronics, glass production, and medical applications.

The correct answer is the number of orbits/shells. Within a period, the elements have the same number of orbits or shells in their atomic structure. This is because elements in the same period have the same number of energy levels or electron shells. The number of valence electrons, reactivity characteristics, and physical properties may vary within a period depending on the specific element.

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 towards itself in a chemical bond. As you move down a column, the number of energy levels or shells increases, causing the outermost electrons to be farther from the nucleus. This decrease in attraction between the nucleus and the outermost electrons results in a decrease in electronegativity.

Helium (He) has 2 valence electrons. Valence electrons are the electrons in the outermost energy level of an atom. Helium is in the second period of the periodic table, so it has 2 energy levels. The first energy level is filled with 2 electrons, so the 2 remaining electrons in the second energy level are the valence electrons.

Rubidium, Rb, has the largest atomic radii among the given elements in period 5. Atomic radii generally increase from top to bottom within a group or period. Since Rubidium is located towards the bottom of period 5, it has more energy levels and electron shielding, causing its atomic radius to be larger compared to the other elements in the same period.

Francium, Fr, has the lowest ionization energy among the given elements. Ionization energy refers to the energy required to remove an electron from an atom. The trend of ionization energy in the periodic table is that it generally decreases from top to bottom and increases from left to right. Since Francium is located at the bottom and leftmost position in the periodic table, it has the lowest ionization energy. This means that Francium is the easiest to remove an electron from, making it the element with the lowest ionization energy.

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 filled with 2 electrons, giving them a total of 2 valence electrons.

Iron, Fe, is smaller than Hassium, Hs, primarily because iron has fewer orbits. The size of an atom is determined by the number of electrons and the energy levels or orbits in which they are located. Iron has fewer orbits compared to Hassium, which means that the electrons in iron are closer to the nucleus and the atomic radius is smaller. This results in a smaller atom size for iron compared to Hassium.

As you go across a period, the atomic radius decreases because the nucleus pulls more on the electrons. This is due to the increase in the number of protons in the nucleus, which increases the positive charge. The increased positive charge attracts the negatively charged electrons more strongly, causing them to be pulled closer to the nucleus and resulting in a smaller atomic radius.

The actinides family consists primarily of large, radioactive, man-made elements. These elements are located in the bottom row of the periodic table and have atomic numbers ranging from 89 to 103. They are all radioactive and are primarily produced through nuclear reactions. Examples of actinides include uranium, plutonium, and americium.

Ununhexium, also known as element 116, has the largest atomic radius among the elements in group 16. This is because as you move down a group in the periodic table, the atomic radius generally increases. Ununhexium is located at the bottom of group 16, so it has the largest atomic radius compared to Oxygen, Sulfur, Selenium, Tellurium, and Polonium.