Atomic Mass

I assume you mean the atomic mass. Its atomic mass is 98.91g/mol

Bromine is a non meta element. Atomic mass of it is 80.

Electron

Tricky bit that, but it's part of the definition of the molar mass. Basically, if you were to collect 6.022×1023 atoms of a substance of a particular atomic mass (lets say 6 for arguments sake), then the resultant pile of atoms would have a mass of 6 grams.

Isotopes. They differ in the number of neutrons in the nucleus.

The weighted average mass of a mixture of isotopes is calculated by multiplying the mass of each isotope by its natural abundance, and then summing these values together. This gives a more accurate representation of the overall mass of the isotopes in the mixture, taking into account their relative abundances.

The atomic mass of H2O is 18.01528amu. Each hydrogen atom has a mass of 1.00794amu and the oxygen atom has a mass of 15.9994amu. There is not atomic number for H2O, as it is a compound, not an element.

H: 2 x 1.00794amu = 2.01588amu

O: 1 x 15.9994amu = 15.9994amu

Total = 18.01528amu

Proton: 1,007 276 466 77(10) atomic units of mass (u)

Neutron: 1,008 664 915 6 (6) atomic units of mass (u)

Electron: 5,485 799 094 3(23).10-4 atomic units of mass (u)

don't know

The mass number of an atom is the average of all it's isotopes in ratio to how often an isotope occurs naturally (abundance). An isotope is a variant of an element that has a different number of neutrons, therefore causing the atom to have a different mass. The percent abundance of an isotope is converted to a fraction, and multiplied by the mass of the isotope. Then all the factional masses of different isotopes are added together.

Atomic mass = (mass isotope 1)x(fractional natural abundance of isotope 1) + (mass isotope 2)x(fractional natural abundance of isotope 2) + (mass isotope 3)x(fractional natural abundance of isotope 3)

For example:

Hydrogen has 3 naturally occurring isotopes:

Protium - Abundance - 99.985% (.99985) Mass - 1.0078

Deuterium - Abundance - .015% (.00015) Mass - 2.014

Tritium - Abundance - 0% (.000) Mass - 3.016

Atomic mass number of Hyrdogen = (.99985)(1.0078) + (.00015)(2.014) + (.000)(3.016) = 1.00795

Go look up the mass number of Hydrogen on the periodic table and it says 1.008

An element's atomic mass is actually a weighted average of all the masses of all the isotopes of that element. Every element has a certain number of isotopes, which are different versions of that element. Different, because they have varying numbers of neutrons. Neutrons have mass, so non-standard numbers of neutrons makes isotope atoms weigh differently than the normal version of that atom. For example, carbon typically has 6 protons and 6 neutrons. So you would think that carbon's atomic mass would be 12. However, there is a small amount of carbon out there that has either 7 or 8 neutrons, which makes these atoms weigh more. This is why carbon's atomic mass on the perioidic table is slightly more than 12. In the case of most elements, isotopes make up a relatively small percentage of the total, which is why many atomic masses are very close to a whole number, but not quite.

Titanium is a metal element. Atomic number of it is 22.

Neutrons is the heaviest particle, because it contain both electron and proton . We know mass of the proton is (1.672623 X 10-27 kg) 1840 times heavier than that of electron mass (9.109390 X 10-31 kg). On comparing proton and electron we get a new idea that neutron (the neutral particle) have both electron and proton so mass of neutron is 1.674929 X 10-27 kg .

By A.V. NARENDARA KUMAR (CHENNAI)

The atomic mass unit (amu), or Dalton (Da) or, sometimes, universal mass unit, is a unit of mass used to express atomic and molecular masses. It is the approximate mass of a hydrogen atom, a proton, or a neutron.

. 1 u = 1/NA gram = 1/ (1000 NA) kg (where NA is Avogadro's number) 1 u = 1.660538782(83)×10−27 kg = 931.494027(23) MeV/c2

It is a unit of mass used to express atomic and molecular weights, equal to one-twelfth of the mass of an atom of carbon-12. It is equal to approximately 1.66 x 10^-27 kg.

The most important isotope of neptunium (237Np) has the atomic mass

237,048 173 4(20).

the elements in the substance are mixtures of their isotopes

Iodine is a non meta element. Atomic mass of it is 127.6.

they increase by one going from left to right

totally a guess

36 The answer of this question is there are 30 protons and 35 neutrons

There is no element called 'flouorine', however there is one called fluorine. What is it's atomic mass? It depends how accurate you want the answer, for most of us 19.0 is accurate enough.

Mike Slater

19.0 is inappropriate, given that .0 is a significant figure and will be assumed to be correct. 19 would be more appropriate, and 18.998 would be more accurate.

The Atomic Mass of an element is the numerical average of all the masses of the naturally occurring isotopes of that element proportionately. Man made elements do not count in supposedly.

IE: If we have an element with atomic weight 100 and we have an isotope of that element with atomic weight 102 and if they occurred equally in nature then the Atomic Mass would be 101.

If the atomic mass of water is 18 and the atomic mass of hydrogen is 1 then the atomic mass of oxygen is 16