Atomic Mass

The standard atomic weight of darmstadtium is considered 281.

Interestingly, nickel has a lower atomic mass (58.693) than cobalt (58.933), even though cobalt has a lower atomic number (27) than nickel (28).

The atomic mass of an atom can be calculated by adding the number of protons and neutrons together. In this case, an atom with 8 protons and 9 neutrons would have an atomic mass of 17 atomic mass units (amu).

The atomic mass of germanium is approximately 72.63 atomic mass units.

this is because the atomic number is the number of protons in an atom, and this never changes. However, the recorded atomic mass is a weighted average of all of the isotopes of the atom, because atomic mass is the number protons plus the number of neutrons, and the number of neutrons in an atom differs, causing different atomic masses.

The average atomic mass can be calculated by taking the weighted average of the atomic masses of the isotopes based on their abundance. For this case, the average atomic mass would be: (0.50 * 197) + (0.50 * 198) = 197.5.

Well, that depends on what substance it is. There's a way to figure it out, though, for every substance. On the periodic table, the atomic mass number for every element is the number of grams in 1 mole of that substance. 1 mole of every substance contains a constant number of representative particles, 6.02x1023. That's called Avogadro's number, and it's the most important constant in chemistry. Given a mass of a substance, it's a simple matter of finding out the number of atoms. For example, let's say you have 80 grams of calcium (Ca). Calcium's atomic mass is 40, and that means 40 grams per mole. You have 80 grams, so that's 2 moles. 1 mole of anything contains 6.02x1023 particles, so that number times your 2 moles get you 1.2x1024 atoms of calcium.

No. Atoms of the same element can have different masses as the number of neutrons can vary.

Atoms of the same element but with different masses are called isotopes.

The atomic mass of uranium is approximately 238.02891 atomic mass units.

The atomic mass number generally increases as you move across the periodic table from left to right. This is because the number of protons in the nucleus increases as you move to elements with higher atomic numbers.

The atomic mass is the sum of the number of protons and neutrons in the nucleus because protons and neutrons have a mass of approximately 1 atomic mass unit each. Electrons are much lighter and do not significantly contribute to the overall mass of the atom.

Fluorine has a greater atomic mass than carbon. Carbon has an atomic mass of approximately 12 atomic mass units (amu) while fluorine has an atomic mass of approximately 19 amu.

Atomic mass includes the total mass of protons, neutrons, and electrons in an atom. Since protons and neutrons contribute significantly to the mass of an atom, atomic mass is generally greater than atomic number, which represents the number of protons in the nucleus. Electrons have a much smaller mass compared to protons and neutrons, so they have less impact on the overall atomic mass.

The average atomic mass is a weighted average of the masses of all isotopes of an element, taking into account their abundance. The atomic mass listed on the periodic table is the weighted average of all naturally occurring isotopes of the element. So, they are essentially the same thing, with the average atomic mass being a more specific term.

Copper (Cu) has a relative atomic mass because it is an average value that considers the different isotopes of copper and their abundance in nature. The relative atomic mass provides a more accurate representation of the average mass of an atom of copper compared to using just the mass number of the most abundant isotope.

Because copper has isotopes. All Copper atoms have exactly the same number of protons, but not all of them have the same number of neutrons. The ones with different numbers of neutrons are known as isotopes. A given sample of Copper will contain various amounts of each of its isotopes. The atomic mass (weight) is an average weight, based on the percentages of the isotopes

The atomic mass number, which is always an integer, is the sum of the numbers of protons and neutrons in the nucleus. This is approximately equal to the mass of in atomic mass units of an atom of a particular isotope, because the only other constituents of an atom are electrons, of which there are the same number as protons but which have only about 0.005 times the mass of either protons or neutrons. There are also small variations in actual atomic masses because of the fact that nuclei have varying degrees of stability to radioactive decay, and this is reflected in their masses because of the equivalence between mass and energy first postulated by Einstein and later proved by many others.

The atomic mass of a pepper can vary depending on the type of pepper. For example, the atomic mass of a bell pepper is approximately 18.02 g/mol, while the atomic mass of a chili pepper is around 16.04 g/mol.

Before I begin, you must understand that atomic number means the number of protons in the atom, and that the number of protons determines what element an atom is, i.e. an atom with 13 protons will always be aluminum, and one with 16 protons will always be sulfur. So, if you could somehow take away 3 protons from a sulfur atom, it would become aluminum. When the atomic mass of an element is shown with decimal places, this is an average of all the possible atomic masses that that element could have. Each element may have more than one atomic mass due to things called isotopes. These are not complicated - an isotope is just a version of an atom with a different number of neutrons in the nucleus than another version (isotope).

Remember that if the number of neutrons changes, the element will not change, as it is the number of protons that determines the element. Therefore, there can be multiple versions (isotopes) of the same element, with the same amount of protons, but with different numbers of neutrons. So, for example, the sodium atom, which will always have 11 protons in an atom (this is what makes it sodium), has 20 possible different isotopes (versions) ranging from 7 to 26 neutrons in each.

Therefore, you cannot work out a single atomic mass. It could be anywhere between 18 (11+7) and 37 (11+26) (here I am adding the constant proton (atomic) number of sodium to the highest and lowest possible neutron numbers to make two possible atomic masses). However, there will be many other possibilities for each neutron number in between 7 and 26. So, because of all these possibilities, the mean (average) is taken of all the possible atomic masses, which is often a decimal. This gives the best result which supports the many different isotopes available for a single element.

Chlorine is the non metal halogen family atomic mass.... 35

The atomic number refers to the number of protons in the atom. Since the proton cannot be an in-between number, the atomic number will have to be a whole number.

On the other hand, the atomic mass does not have to be a whole number because it is the mass of an atom and is roughly equivalent to the number of protons plus the average number of neutrons in that particular element.

Atomic mass = weight in gram / moles = 10 / 2.5 = 4 amu

Polonium is a metal element. Atomic mass of it is 209.

Atomic number is a unique number for each element. No two elements have the same atomic number. Atomic number is also the number of protons in the nuclei of the atoms of any given atom. Atomic mass, however, is the number of protons, neutrons and electrons. The number of neutrons can vary with different isotopes of the same element, this means that atomic mass can vary with different isotopes. So atomic number does not vary, but atomic mass does, so it is more logical to use atomic number to organize the elements. In addition, when the elements are arranged according to atomic number into seven rows and 18 columns, it becomes evident that there are certain trends that occur across the periods, and that elements in the same group have similar properties.