Periodic Table

In the periodic table, 'd' refers to the blocks of elements in the d-block, which includes transition metals. These elements have partially filled d orbitals in their electron configurations.

There is no difference between "period table" and "periodic table" - they refer to the same thing. The periodic table is a tabular display of the chemical elements organized by atomic number, electron configuration, and recurring chemical properties.

The main group metals in the 6th period are cesium, barium, and radium. They belong to Group 1 (alkali metals) and Group 2 (alkaline earth metals) of the periodic table.

Some elements that have 3 valence electrons include aluminum, boron, and thallium. These elements can form compounds by either losing the 3 valence electrons to achieve a full outer shell, or by sharing electrons to complete their valence shell.

Metalloids, such as silicon and germanium, are used in computers because they have properties of both metals and nonmetals. They can conduct electricity like metals, but also have some properties of nonmetals, making them ideal for use in semiconductors and other electronic components.

The general trend in atomic radius across a row of elements decreases from left to right due to increasing effective nuclear charge, which attracts the electrons closer to the nucleus. As you move across a period, the number of protons in the nucleus increases, resulting in a stronger pull on the electrons and a decrease in atomic radius. Additionally, the shielding effect of inner electrons remains relatively constant, further contributing to the trend.

Non-metals and metals from opposite sides of the periodic table tend to undergo ionic bonding. The non-metal typically gains electrons to form negatively charged ions (anions), while the metal loses electrons to form positively charged ions (cations). These oppositely charged ions attract each other and form an ionic compound.

As of our current knowledge, there are 118 known elements on the periodic table, each with a specific number of electrons. The electron is a fundamental particle, and there are trillions upon trillions of electrons present in the universe, making it impossible to provide an exact count.

n-Hexene is considered a polar molecule due to the presence of the carbon-carbon double bond. The asymmetric distribution of electrons around the double bond creates a small dipole moment, making the molecule polar.

Rn is radon, a radioactive gas, atomic number 86. It is the product of radium decay.

The most reactive metal is francium. Francium is a highly unstable alkali metal and is usually found in trace amounts in uranium and thorium ores. It readily reacts with air and water, making it one of the most reactive elements known.

Element 7 on the periodic table is Nitrogen (N). It is a non-metal element with an atomic number of 7 and is found in the atmosphere as a diatomic gas.

The ionization energy generally increases across a period from left to right. This is because as you move across a period, the effective nuclear charge increases, making it more difficult to remove an electron. Additionally, the increasing number of protons in the nucleus leads to stronger attraction between the nucleus and the electrons.

The numbers on a gold bar typically indicate its weight in troy ounces or grams, its purity level, and the serial number of the bar for tracking and authentication purposes. These markings help identify the gold bar's value and ensure its authenticity in the market.

Yes, the periodic table organizes the 109 known elements based on their atomic number, electron configuration, and chemical properties. It helps scientists predict the behavior of elements and identify patterns in their characteristics.

Lithium is the lightest element metal with a relative atomic mass of 7 (3 protons, 4 neutrons).

A group in the periodic table is a column of elements with similar chemical properties, while a period is a row of elements with increasing atomic number. Elements in the same group have the same number of valence electrons, which contributes to their similar properties. On the other hand, elements in the same period have the same number of electron shells.

The Russian, Dmitri Mendeleev's periodic table became available to the scientific community vi publication in 1869 and he is generally credited with its "creation"

Carbon. it is the standard to which every other element is measured against (In terms of atomic mass)

E.G. Each atomic mass unit is 1/12 of a Carbon-12 atom, so an atom of lead is 82 x (1/12) atoms of carbon 12

Hence, Carbon-12 must be the perfect element...

Helium, as it has full 1S orbital, does not form compounds, and has a symmetrical nucleolus.

Electronegativity increases when atoms have a stronger attraction for electrons due to factors like having a higher nuclear charge, being smaller in size, or having more effective nuclear charge. This results in a greater ability to attract and hold onto electrons in a chemical bond.

Silicon belongs to the Group 14 elements in the periodic table, meaning it has 4 valence electrons as carbon does. However, silicon's larger atomic size allows it to accommodate additional electrons in its outer shell, resulting in a co-valency of 6. Carbon, on the other hand, is smaller in size and can only effectively bond with a maximum of 4 other atoms.

The reactivity of an element depends on how easy it can gain to to lose electrons in its outer most shell (which results in a reaction).

In metals, the reactivity increases down the group. This is because as we move down the groups of metals, there are more shells of electrons, which results in the increased distance between the nucleus (which has the protons) and the valence electrons. The increased distance means that the protons can only exert a weaker attractive force on the valence electrons, which ultimately makes it easier for the atom of the element to lose electrons to form ions in order to react because less energy is now required to overcome the force acting on the valence electron.

In non-metals, reactivity decreases down the group. Using the same principle as above, we know that as we go down the group, the element gains more shells and electrons are held by a weaker attractive force to the protons. As we know, non-metals usually form negatively charged ions. As such, they need to attract electrons in a reaction. As a result of the protons decreased strength of attraction to the valence electrons as we progress down the group, elements generally are less capable of reacting down a group of non-metals because it is less likely for elements down the group to form ions.

In metals, reactivity decreases across the group. Across the group, the number of shielding electrons (total electron number minus the valence electrons) remains the same but the number of protons increases. This causes an increase in effective nuclear charge. An increase in the effective nuclear charge means that the protons will be exert a greater force on the electrons, which means that it would be harder for the valence electrons to be liberated. Hence, metals are less capable of forming ions across the group.

Using the same idea, non-metals will definitely be more reactive across the group. With the higher effective nuclear charge, they will possess more electrostatic attractive power to hold the electrons together. Hence, it is easier for them to attract and hold on to an electron to become an ion.

Do note that Group 0 (a.k.a Group VIII) consist of noble gases, which generally do not react. They are inert gases. They do not tend to react because they have achieved octet structure (8 electrons) in their valence shell, with the exception of helium. However, some of these elements do go through reactions in extreme conditions (e.g. argon).

To calculate the atomic volume occupied by Pt, you can use the formula for the volume of a sphere, which is V = 4/3 * π * r^3. Given the atomic radius of Pt as 91.1 Å, you can substitute this value into the formula to find the atomic volume occupied by Pt.