Atomic Mass

The atomic weight (not mass !) of thorium is 232,0381.

multiply by acceleration

It is amu or AMU.

After IUPAC tables (2oo9) the atomic weight of nobelium is [259].

The mass of a pear can vary depending on its size and variety, but on average, a medium-sized pear typically weighs around 166 grams. To determine the exact mass of a specific pear, you would need to use a scale to measure its weight in grams. This measurement is important for various purposes, such as tracking nutritional intake or calculating recipe ingredients accurately.

Atomic number. This gives the count of protons in the nucleus and therefore the posiitive charge of the nucleus.

For an uncharged atom it therefore gives the total number of electrons in all shells

Scientists determine the atomic mass of an atom by averaging the masses of all the isotopes of that element, weighted by their abundances. This information can be obtained from mass spectrometry data and is used to calculate the weighted average mass. The atomic mass is typically reported in atomic mass units (amu).

Developing the atomic mass unit allowed for a standardized method of measuring atomic masses, providing a more precise and consistent way to compare the masses of different atoms. This was crucial for advancements in chemistry and physics, leading to a better understanding of atomic structures and the development of the periodic table.

83.98 amu is the Atomic Mass, 36 is the atomic number.

The unit used to measure weighted average atomic mass is atomic mass unit (amu). This unit is a standard for atomic and molecular mass measurements in chemistry and is defined as one twelfth of the mass of an atom of carbon-12.

The atomic age was primarily caused by the development and use of nuclear weapons, starting with the atomic bombings of Hiroshima and Nagasaki in 1945. The Manhattan Project, a research and development program during World War II, led to the creation of the first atomic bombs, marking the beginning of the atomic age.

Krypton is a non meta element. Atomic mass of it is 35.

Atomic mass unit is a unit of mass for all chemical elements, not only for hydrogen.

The atomic weight of hydrogen is [1,00784; 1,00811]; the conventional atomic weight is 1,008.

1 atom is equal to 1 amu.

Both nitrogen gas and carbon monoxide have the same molecular weight, around 28 grams per mole. Therefore, 10 grams of each substance contain approximately one-third of a mole of molecules. Since Avogadro's number (6.022 x 10^23) represents the number of molecules in one mole of a substance, both 10 grams of nitrogen gas and 10 grams of carbon monoxide contain the same number of molecules, which is roughly 2 x 10^23.

The only element with a radioactively stable isotope with a mass number of 27 is aluminum.

Chlorine is a non meta element. Atomic mass of it is 35.

Mendeleev's periodic table was based on the atomic masses of elements. However, this was not effective when isotopes were discovered. An isotope of an element is defined as the element having the same atomic number but varying mass numbers. So, mass numbers weren't constant and hence, a better characteristic was chosen -atomic number. Atomic number of any element was a characteristic of a particular element. Hence atomic numbers were taken as the basis of classification instead of atomic masses.

The relative atomic mass of oxygen is determined by taking the weighted average of the isotopic masses of its naturally occurring isotopes (O-16, O-17, O-18) in respect to their abundance in nature. This calculation gives an average value close to 16, which is the standard atomic mass unit for oxygen.

They don't contain the same number of particles because some particles are more dense than others making one atom and another atom the same mass but not have the same number of particles.

Yes, that is what is used. Bromine is I think ~51:49 ratio of Br79 and Br81. Therefore it is somewhere in between (79.9g/mol)

Deuterium, which is an isotope of hydrogen, has an atomic mass of 3. It has one proton and two neutrons in its nucleus.

Isotopes. The isotope has the same number of protons and electrons as the regular atom, but has more (or sometimes less) neutrons, and therefore its atomic mass is more (or less, depending on whether the neutrons have increased or decreased).

As a first approximation it tells us simply the total number of protons and neutrons in the nucleus. The electrons and binding energy of the nucleus contribute a very much smaller amount to the mass.

Since the number of protons in a given element is constant (the atomic number), we can also tell the number of neutrons in an atom by subtracting the atomic number from the atomic mass (approximately).

Since different isotopes of each element have different numbers of neutrons (but the same number of protons), they will have different atomic masses. The given atomic weight for a particular element is usually based on the relative abundance of the isotopes as they occur in nature.

It is also true that elements with very high elemental weights tend to be unstable, that is, radioactive.

(Referring to the Wikipedia entry on "atomic mass" I see that what I have defined here may include some of the sense of "atomic weight", however the difference is subtle. See that entry for further clarification.)

Protons and neutrons make up an atom's atomic mass. Protons have a positive charge and are found in the nucleus along with neutrons, which have no charge. Electrons, which have a negative charge, contribute very little to the atomic mass of an atom.