Periodic Table

C (carbon)

The nitro group (NO2) is a substitution for one of the hydrogen atoms in methane, creating nitromethane (CH3NO2).

As they exist in nature, elements usually have no charge.

However, there are certain tendencies of elements to become anions (ions with negative charges) or cations (ions with positive charges) based upon their individual compositions.

Imagine the periodic table and it's groups. The transition metals in the middle of the table form various cations that are not easy to predict. Therefore, we can't represent all transition metals as their own group with one specific charge. But, we CAN do that for some other groups:

Group 1 elements (Li, Na, K etc.) have similar chemical properties that make them "want" to have a charge of +1.

Group 2 elements form 2+ ions, and

Group 3 elements form 3+ ions.

Group 4 elements may have a charge of either 4+ or 4- and need to be memorized.

The elements that form negative ions are in Group 6 (2- charge) and Group 7 (1- charge).

Noble gases have their outermost energy levels full of electrons and are "balanced" and thus have a very low tendency to become ions.

In order to reasonably assume the charge of an element in an equation, you have to consider the other elements it will be reacting with and take into consideration their properties as well.

For example, when Hydrogen and Oxygen combine to form water, two Hydrogen atoms bond with one Oxygen atom. Say you remember that Oxygen is in Group 6 on the periodic table and Group 6 elements have a 2- charge. Say you also remember that Hydrogen is a noble gas without a charge listed. Since the Oxygen atom has a 2- charge, each Hydrogen atom will have to have a +1 charge to attract to the oxygen and bond with it (this is because molecules like to be neutral and form a net charge of zero).

Beryllium (Be) has a smaller ionization energy than magnesium (Mg) because beryllium has a smaller atomic size and therefore the electrons are held less tightly, making it easier to remove an electron from a beryllium atom compared to a magnesium atom.

The horizontal rows on the periodic table are called periods.

Fluorine is the smallest halogen on the periodic table.

The number of shells increases. Moving down the periodic table leads an investigator to heavier elements, that is, elements with bigger atomic numbers. That means larger nuclei and more electrons, which will have to make themselves homes out in the electron cloud. More shells will be set up to provide places for those electrons to hang out.

As you move from left to right across period 3 on the periodic table, the atomic radius, metallic character, and reactivity generally decrease. This is because the increasing number of protons in the nucleus leads to stronger attraction for the electrons, resulting in a smaller atomic size and less metallic behavior.

There are 5 elements that have for letters: 10 Ne neon, 26 Fe iron, 30 Zn zinc, 79 Au gold and 82 PB lead. Neon is the only one, that is NOT a solid at room temperature here on planet earth. It also makes neat beer signs and vacancy indications.

The main similarity among elements in group 2 of the periodic table is that they all have two valence electrons in their outermost energy level. This gives them similar chemical properties, such as forming 2+ cations when they react with other elements.

Tungsten has a melting point of 3422 degrees Celsius.

It depends on the maker of the table, but generally if there's any designation at all it will be with background color or a thick black zigzag line drawn through the middle of the table, with the elements above and to the right being the nonmetals (and the elements that actually border the line being called "semimetals" or "metalloids").

Lutetium is a chemical element with the symbol Lu and atomic number of 71. It has a period of 6 and belongs in the Lanthanide group.

Elements vary in their ability to conduct electricity. From most conductive to least conductive in relative terms are (all figures are measured in cm ohm) silver at 0.63 10^6, copper at 0.596 10^6, and gold at 0.452 10^6.

To determine the energy level of the f-orbital in a particular period, consider the principal quantum number (n) of the period. The energy level of the f-orbital follows the pattern 4n, where n is the principal quantum number. This means that for each period, the energy level of the f-orbital will be 4 times the principal quantum number of that period.

Albert Ghiorso, Stanley G. Thompson, Gary H. Higgins, Glenn T. Seaborg, Martin H. Studier, P.R. Fields, Sherman M. Fried, H. Diamond, J.F. Mech, G.L. Pyle, John R. Huizenga, A. Hirsch, W.M. Manning, C.I. Browne, H. Louise Smith, R.W. Spence - 1952

They're called the alkali metals, and are comprised of lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and Francium (Fr). Group 1A also includes hydrogen (H), though that isn't an alkali metal.

Americium can change into neptunium through a process called alpha decay. During alpha decay, an alpha particle (helium nucleus) is emitted from the nucleus of the americium atom, resulting in the transformation of the americium atom into a neptunium atom.

The most active metals are located in Group 1 of the periodic table, known as the alkali metals. These metals include lithium, sodium, and potassium, which readily react with water and air. They are highly reactive due to their tendency to lose their outermost electron to achieve stability.

The atomic number of the element Si is 14.

Elements in the same group on the periodic table have similar chemical properties because they have the same number of valence electrons. Elements in the same family have similar physical properties because they have the same number of electron shells.

well, female has her "period" and a person called it period because it was the end of a females child life and you know a period at the end of a sentence and that's how period got its name lol

The equation for the alpha decay of plutonium-244 is:

[ ^{244}{94}Pu \rightarrow ^{240}{92}U + ^4_2He ]

Group 1 is known as the 'Alkali Metals'

They are in descending order of the group ; lithium, sodium, potassium rubidium, caesium, and francium.

They become increasing reactive with water on descending the group , to the point of explosion. Francium is not found in the lab, because it is also radio-active.

The Group 2 are known as the 'Alkali Earth Metals'. Because they are frequently found in rocks e.g. Calcium and magnesium as Calcium Carbonayte and magnesium carbonate.

The melting point decreases down the group for alkali metals because the metallic bonding weakens as the atomic size increases, resulting in weaker intermolecular forces. For halogens, the melting point increases down the group due to stronger van der Waals forces between larger molecules with increased electron cloud size, resulting in higher melting points.