Chapter 5 - Periodic Table

The s block of elements consists of two groups.

The element with the electron configuration [Ar] 4s2 3d10 4p1 belongs to period 4 because the highest energy level (valence shell) is the fourth energy level. It belongs to group 13 because it has one valence electron in the p orbital, which corresponds to group 13 on the periodic table.

The noble gases are actually located in the p block of elements, specifically in group 18 of the periodic table. The d block of elements is known as the transition metals. Therefore, the statement that the noble gases are located in the d block of elements is incorrect.

The division of the periodic table labeled with the number 14 refers to the group 14 elements, which include carbon, silicon, germanium, tin, and lead. These elements have similar chemical properties and are often referred to as a family or group. Therefore, the statement that this section can be called a family is true.

The statement is false because the lanthanides and actinides are not in group 3 of the periodic table. They are actually located in the f-block, which is below the main body of the periodic table. The f-block consists of two series of elements, the lanthanide series and the actinide series, which are placed separately at the bottom of the periodic table.

Atomic radii is not measured in the unit "am". The correct unit for measuring atomic radii is picometers (pm). The term "am" is not a recognized unit for measuring atomic radii.

Period 6 elements have a lower ionization energy than period 2 elements because as you move down a periodic table, the atomic radius increases. This means that the outermost electrons in period 6 elements are further away from the nucleus and experience less attraction, making it easier to remove them. In contrast, period 2 elements have smaller atomic radii, resulting in stronger attraction between the nucleus and outermost electrons, requiring more energy to remove them. Therefore, period 6 elements have lower ionization energies compared to period 2 elements.

It should be [Ar] 4s²3d¹ because when you move from the s to d sublevel you drop one main energy level.

The correct answer for the question is "series" or "Series" or "SERIES". The question is asking for another name for a period, which refers to a sequence or set of events or actions that occur in a particular order. Therefore, "series" is an appropriate term to describe a period.

Doberiner's quartets did not state that elements 2 and 3 have properties halfway between elements 1 and 4. Instead, it proposed that elements 1 and 4 have similar properties, while elements 2 and 3 have properties that are different from both 1 and 4. This concept was later refined and expanded upon by Mendeleev in the development of the periodic table.

Newlands did not leave spaces in his periodic table and predict the properties of the elements that belonged there. This statement is false.

The main group elements in the periodic table are located in the s and p blocks. These blocks consist of the elements in the first two columns (Group 1 and 2) and the last six columns (Group 13 to 18). The s block contains elements with their outermost electron in the s orbital, while the p block contains elements with their outermost electron in the p orbital. Therefore, the correct answer is p and s.

Germanium does not have a higher metallic character than sodium. Metallic character refers to the ability of an element to exhibit metallic properties such as being malleable, ductile, and having a high electrical conductivity. Sodium is a highly reactive metal with a low melting point and is commonly found in its metallic form. Germanium, on the other hand, is a metalloid that exhibits both metallic and non-metallic properties. While it can conduct electricity, it is brittle and has a higher melting point compared to sodium. Therefore, the statement is false.

The atomic radii refers to the size of an atom. As you move down a group in the periodic table, the number of energy levels or shells increases. This results in an increase in atomic size because there are more electrons and a greater distance between the nucleus and the outermost energy level. Therefore, the statement "It increases as you go down a group" is true.

Ramsey is the correct answer because he was the scientist who discovered the group 18 elements, also known as the noble gases.

The statement is false because the most common ion for aluminum (Al) has a smaller ionic radii than the most common ion for bromide. Aluminum typically forms a +3 ion (Al3+), which has a smaller ionic radius compared to the bromide ion (Br-).

Electron affinity refers to the energy change that occurs when an atom gains an electron to form an ion. It quantifies the attraction between an atom and an additional electron. When an atom gains an electron, energy is released, resulting in a negative electron affinity value. This process is important in understanding the reactivity and chemical behavior of elements, as it helps determine the likelihood of an atom gaining an electron to form an ion.

Mosley used X-Rays to determine the atomic number of the elements. X-rays have the ability to penetrate materials and interact with the electrons in an atom. By studying the X-ray spectra produced by different elements, Mosley was able to identify patterns and correlations between the spectra and the atomic number. This led to the discovery of the relationship between the atomic number and the number of protons in the nucleus, which is now known as the basis of the modern periodic table.

Mendeleev knowingly based the order of his periodic table on chemical properties. He arranged the elements according to their similar chemical properties, which allowed him to group elements with similar behaviors together. This arrangement was unique and different from any previous attempts at organizing the elements. Mendeleev's periodic table became the foundation for the modern periodic table we use today.