Parts Of The Periodic Table: Quiz! Test

The transitional metals are located in the middle of the periodic table. They are found between the alkali earth metals and the nonmetals. These elements have properties that are a combination of both metals and nonmetals. They are known for their ability to form multiple oxidation states and for their high melting and boiling points. Some examples of transition metals include iron, copper, and zinc.

The first energy level can hold a maximum of 2 electrons. This is because the first energy level consists of only one sublevel, which is the s sublevel. The s sublevel can hold a maximum of 2 electrons.

Metals are located on the left side of the periodic table. This is because metals tend to lose electrons and form positive ions. They have a shiny appearance, are good conductors of heat and electricity, and are generally malleable and ductile. On the other hand, nonmetals are located on the right side of the periodic table and have properties opposite to metals. The middle and top sections of the periodic table consist of metalloids and noble gases, respectively.

The left side of the periodic table contains the majority of the metallic elements. These elements are known as "metals." Metals are characterized by properties like high electrical and thermal conductivity, malleability, and ductility. Some of the most well-known metals found on the left side include:



Alkali Metals: These are found in the first column (Group 1) of the periodic table, including elements like lithium (Li), sodium (Na), and potassium (K).



Alkaline Earth Metals: These are in the second column (Group 2) and include elements like calcium (Ca) and magnesium (Mg).



Transition Metals: These are found in the middle of the periodic table, starting from Group 3 to Group 12. Examples include iron (Fe), copper (Cu), and gold (Au).

Metals are known for their ability to conduct electricity and heat, making this the characteristic that sets them apart from other materials. This property is due to the presence of free electrons in the metal's atomic structure, which can easily move and transfer energy. The other options, non-shiny and generally liquid at room temperature, and shiny and generally gas at room temperature, do not accurately describe the characteristics of metals.

Dmitri Mendeleev is credited with inventing the periodic table. He published the first version of the periodic table in 1869, arranging the elements based on their atomic mass and properties. Mendeleev's periodic table provided a systematic organization of the elements, allowing for the prediction of undiscovered elements and their properties. His work laid the foundation for the modern periodic table we use today, which is arranged based on atomic number.

The correct answer is Mg because it is the only element in the options that belongs to group 2 and period 3 on the periodic table. Be belongs to group 2 but is in period 2, B belongs to period 2 but is not in group 2, and None of these is not a valid element.

The correct answer is up/down because the question is asking about the direction in which the families are located. The options "up/down" and "left/right" indicate the two possible directions. Since the answer is "up/down," it means that the families are positioned vertically, either above or below each other.

The group of elements called the Alkali metals is Group 1 (IA). Alkali metals include elements such as lithium, sodium, potassium, and cesium. These elements are highly reactive and have only one valence electron, making them very reactive and easily losing that electron to form a positive ion. They are typically soft, shiny, and have low melting points.

The number 3 in this cell from the periodic table indicates the number of protons in the lithium atom. The atomic number of an element represents the number of protons in its nucleus, and since lithium is in the third row of the periodic table, it has 3 protons.

The number 3.91 in this cell from the periodic table indicates the average atomic mass of lithium, considering the naturally occurring isotopes.