Atomic Mass

* Atomic Radius: 0.79Å * Atomic Volume: 14.4cm3/mol * Covalent Radius: 0.32Å * Ionic Radius: 0.012Å * Atomic Radius: 0.79Å * Atomic Volume: 14.4cm3/mol * Covalent Radius: 0.32Å * Ionic Radius: 0.012Å

For compounds, it's called "molar mass" instead of atomic. You take each individual element (one C, four H) and add each atomic mass: e.g. 12.0 + 4(1.01) = 16.04 g/mol
30.06904 g/mol

Silver (Ag) has an Atomic Mass of 107.87 g/mol.

Periodic Table here: http://fermat.csci.unt.edu/~mikler/Courses/biocomputing/resources/periodic_table.gif

The atomic mass unit of an atom is the sum of the protons and neutrons in its nucleus. In this case, with 8 protons and 9 neutrons, the total atomic mass unit of the atom would be 17. The number of electrons does not significantly affect the atomic mass unit of an atom.

An atom's mass is located entirely in the nucleus. In the nucleus, there are protons and neutrons. Electrons are located outside of the nucleus, but because the mass of an electron is so insignificantly small, it's not counted when determining the total mass.

The atomic mass of palladium is approximately 106.42 atomic mass units.

Atomic mass is the total mass of an atom, which includes the mass of protons, neutrons, and electrons. Average atomic mass, on the other hand, is the weighted average of the masses of the isotopes of an element, taking into account the abundance of each isotope in a sample of the element.

The atomic mass of a sulfate ion (SO4) is calculated by adding up the atomic masses of its constituent atoms. This includes one sulfur atom (S) with an atomic mass of approximately 32.06 and four oxygen atoms (O) with an atomic mass of around 16.00 each. Therefore, the total atomic mass of a sulfate ion is around 96.06.

The unified atomic mass unit (u) is equal to 1/12 of the mass of a carbon-12 atom. This corresponds to a mass of approximately 1.66 x 10^-27 kg. The unified atomic mass unit is commonly used in chemistry and physics to express atomic and molecular weights on a scale relative to the mass of a carbon-12 atom.

The standard on which the atomic mass unit is based is the carbon-12 isotope. It is defined as 1/12th of the mass of a carbon-12 atom. This allows for a consistent reference point for measuring the masses of other atoms.

The atomic mass of sucrose is 342.30 grams per mole.

start by getting its isotpic mass. you can do this by taking the mass of an atom and dividing it by 12.01, which is kinown as the carbon standard and is used in the calculation for any element. this will give you a ratio. multiply this number by 12 amu and it will give you the isotopic mass. Next, multiply this number by the percentage in abundance as a fraction (ex. 92.12% = .09212)..... the resulting number will be your atomic mass ONLY for that isotope. To calculate the ATOMIC MASS of an element, you must repeat the previous steps for ALL isotopes. When this is finished, add the atomic masses for the isotopes together the get the atomic mass for that element. For a visual, we'll use Si (28)

(mass of Si atom)/ (mass of C standard) = 2.331411 that's your ratio

2.331411 x 12 amu = 27.97693 amu .... that's your isotopic mass for that specific isotope

27.97693 x .9223 (or 92.23%) = 25.8031..... that's your atomic mass for that isotope

Now the similar calculations done with the other isotopes of silicon give us..

Si(29) as (28.976495x.0467=1.3532) and Si(30) as (29.973770x.0310=.9292)

Lastly, add those together to get...

25.8031 + 1.3532+ .9292 = 28.09 amu which is the atomic mass for the element Silicon.

Good luck, chemistry sucks.

It's the electrons that throw it off.

What do you mean? Atomic mass of an atom is the weighted average mass of all the naturally occurring isotopes of that element, measured in amu (=atomic mass unit). I do not know how do you want to call it, it is just atomic mass, average atomic mass, mass of an atom, atom's mass...

Yes, that is correct. A proton and neutron each have a mass of approximately 1 atomic mass unit (amu). This unit is commonly used to express the mass of subatomic particles in relation to the standard carbon-12 atom.

the bigger the mass of an element, the higher its atomic number.

The average atomic mass of an element is the weighted average of the masses of its naturally occurring isotopes, taking into account their relative abundance. It is usually listed on the periodic table below the element's symbol.

Those elements do not exist on the periodic table as they are not real chemical elements. "Alien" elements are likely part of a fictional scenario or game. In reality, noble gases are a group of elements located in Group 18 of the periodic table, with helium having the least atomic mass and radon having the greatest. "Logon" is not a recognized element or term in chemistry.

The number of neutrons in an atom can be calculated by subtracting the atomic number from the atomic mass. In this case, an atomic mass of 16 and atomic number of 8 for oxygen means there are 8 neutrons (16 - 8 = 8).

87.62

Wrong, that is the Atomic Mass, not the Mass Number.

The Mass Number is the whole number of protons plus neutrons for the specific isotope.

For example, Sr-88 is a stable isotope, with 88-the atomic Number 38 being the number of neutrons.

Complicating the matter, Sr 86 and Sr 87 are also stable but would have mass numbers of 48 and 49.

The average weight of an element is expressed in atomic mass units (amu) and is calculated based on the relative atomic masses of the isotopes of that element weighted by their abundance in nature. This value can be found on the periodic table for each element. For example, the average atomic mass of carbon is 12.011 amu.

The atomic mass unit of oxygen is approximately 16.0 u.

The atomic mass of an element is based on the sum of the number of protons and neutrons in the nucleus of an atom. This value is typically given in atomic mass units (amu) and is an average of the isotopes of the element weighted by their abundances.

Most elements have isotopes---atoms that have the same number of protons (and hence they are still that element) but different numbers of neutrons. For instance, sulfur found in nature has four stable isotopes: S-32 16 protons 16 neutrons S-33 16 protons 17 neutrons S-34 16 protons 18 neutrons S-36 16 protons 20 neutrons Each of these isotopes has a different mass, but all are sulfur because they have 16 protons.